L-Cysteine Hydrochloride Monohydrate; Cys; L-Cysteinium Chloride Monohydrate; L-Cysteine Hydrochloride; Monohydrate; cas no: 06.04.7048

L-cystine; cystine; L-Cystin; L-Dicysteine Cas no :52-90-4

CAS no.: 142-91-6; Nom INCI : ISOPROPYL PALMITATE; Nom chimique : Isopropyl palmitate;Hexadecanoic acid, 1-methylethyl ester; Hexadecanoic acid, 1-methylethyl ester; Hexadecansäure-1-methylethylester; propan-2-yl hexadecanoate N° EINECS/ELINCS : 205-571-1. Isopropyl Palmitate est un ester d'acide palmitique et d'alcool isopropylique. L'acide palmitique est naturellement présent dans les plantes et les animaux. Sa structure possède une chaîne carbone-hydrogène-oxygène plus longue, ce qui la rend beaucoup plus lipophile et lui permet de pénétrer facilement dans la peau. C'est un liquide incolore et inodore. C'est un liquide huileux non polaire. Cette propriété physique en fait un antistatique. La fonction antistatique d'un agent antistatique est cruciale dans toute formulation, car une charge statique peut provoquer une instabilité dans n'importe quelle préparation et peut briser l'émulsion en deux phases différentes, l'huile et l'eau. L'agent antistatique peut neutraliser cette charge et améliorer la stabilité. C'est aussi un agent hydratant et revitalisant pour la peau. Ainsi, il forme un film à la surface de la peau ou des cheveux qui est résistant à l'eau et ne laisse pas l'humidité s'échapper. Ainsi, il permet d'économiser l'hydratation de la peau. Ce qui est utile en cas de peau sèche. De plus, il a une chaîne plus longue dans sa structure, ce qui lui donne une plus grande affinité avec la peau. Il fonctionne comme un lubrifiant ; il aide à la circulation des ingrédients secs. Il donne également un aspect doux et lisse à la peau. Il agit comme liant pour un mélange de poudre sèche. Il peut également être utilisé comme adhésif pour comprimer les comprimés et les gâteaux. On le retrouve dans les crèmes hydratantes, les revitalisants, les rouges à lèvres, les correcteurs, les fards à paupières et les produits anti-âge.IPP, Le Palmitate d’isopropyle est produit à partir d’acide palmitique dérivé d’huile végétale & d’isopropanol (ou alcool isopropylique) . C’est l’ester de l’acide palmitique et de l’isopropanol. Le Palmitate d’isopropyle (parfois abrégé PIP) est un liquide incolore et huileux. Il est très utilisé en cosmétique et en pharmacie (en émulsion avec l’eau, pour faciliter la pénétration des produits dans la peau).; La palmitate d'isoporpyle est utilisé dans les cosmétiques comme un lubrifiant de la peau. Il la rend plus douce et plus lisse. Il peut aussi être utilisé en tant que liant.Isopropyl palmitate;

LEAD(+2)BOROFLUORIDE LEAD(+2)TETRAFLUOROBORATE LEAD FLUOBORATE Lead fluoborate，solution(containing>28%) LEAD FLUOROBORATE LEAD(II) FLUOROBORATE LEAD(II) TETRAFLUOROBORATE Borate(1-),tetrafluoro-,lead(2+)(2:1) lead(ii)tetrafluoroboratesolution leadborofluoride leadboronfluoride leadfluoroborate(pb(bf4)2) leadfluoroboratesolution leadtetrafluoroborate leadtetrafluoroborate(pb(bf4)2) tetrafluoro-borate(1-lead(2+) tetrafluoro-borate(1-lead(2+)(2:1) tetrafluoro-borate(1-lead(2++)(2:1) lead bis(tetrafluoroborate) LEAD(II) TETRAFLUOROBORATE 50 WT. % & CAS :13814-96-5

PC;kelecin;LECITHIN;froM Egg;Alcolec-S;granulestin;L-α-Lecithin;Lecithin, NF;LIPOID(R)E80;Lecithin CAS No.8002-43-5

Lead Octoate PB-36 is one of the auxiliary driers also called as through drier.
Lead Octoate PB-36 is a pale yellow liquid and is used as an active top drier in paints and coatings.


CAS Number: 301-08-6; 64742-81-0
EC Number: 206-107-0; 265-184-9
MDL Number: MFCD00014003
Compound Formula: C16H30O4Pb



Lead 2-Ethylhexanoic acid, Lead Bis ( 2-Ethylhexanoate ), Kerosine (petroleum), hydrodesulfurized, Hydrodesulfurized kerosine (petroleum), HYDRODESULPHURIZEDKEROSINE, HYDRODESULFURIZEDKEROSENE, KEROSINE, STRAIGHTRUN,HYDROTREATED, hydrodesulfurized kerosin, hydrodesulphurized kerosene, kerosene (non-specific name), (40.5-42.5% PB), Leadethylhexanoate, Leadα-ethylcaproate, LeadethylhexanoatePb, LEAD 2-ETHYLHEXANOATE, lead 2-ethylhexanoate 95%, plumbous 2-ethylhexanoate, LEAD(II) 2-ETHYLHEXANOATE, lead bis(2-ethylhexanoate), lead(ii)2-ethylhexanoate95%, 2-ethyl-hexanoicacilead(2++)salt, (40.5-42.5% PB), Bis(2-ethylhexanoic acid)lead(II) salt, Hexanoicacid, 2-ethyl-,lead(II)salt, plumbous 2-ethylhexanoate, 2-Ethylhexanoic acid, lead(2+) salt, 2-ethyl-hexanoicacilead(II)salt, Hexanoicacid,2-ethyl-,lead(2+)salt



Lead Octoate PB-36 is the most effective polymerization catalyst.
Lead Octoate PB-36 is registered under the REACH Regulation and is manufactured in and / or imported to the European Economic Area, at ≥ 10 000 000 to < 100 000 000 tonnes per annum.


Lead Octoate PB-36 is a pale yellow liquid and is used as an active top drier in paints and coatings.
Lead Octoate PB-36 provides hard, through drying throughout the film and also provides flexibility.
Lead Octoate PB-36 is the most important auxiliary drier in applications where drying is required at low temperatures.


Lead Octoate PB-36 has a metal content of 36% (± 0.2) and a specific gravity of 1.33 at 300°C (± 0.03).
Lead Octoate PB-36 is lead octoate grade.
Lead Octoate PB-36 is designed to use with oily paint & grease as a drier.


Lead Octoate PB-36 is suitable to be used together with cobalt and calcium driers.
The recommended usage amount is between 0.08-0.6% based on solid content.
Lead Octoate PB-36 is used polymerization catalyst for drying oils and provides internal drying.


Lead Octoate PB-36 is the most effective polymerization catalyst.
Lead Octoate PB-36 is suitable to be used together with Cobalt, Calcium etc. driers.
Not recommended Lead Octoate PB-36 to use for Aluminum coatings.


Lead Octoate PB-36 is recommended usage amount is between
0,08% – 0,6% based on solid content.
Lead Octoate PB-36 is the most important auxiliary through drier.


Lead Octoate PB-36 is used with active driers like Cobalt and it promotes thorough drying by virtue of its polymerizing effect.
Lead Octoate PB-36 may not be used in aluminum paint where it interferes with leafing and has to be avoided in fume resistant paints as well.
The recommended dosage of Lead Octoate PB-36 is 0.3-1.0 w/w% lead metal on resin NV.



USES and APPLICATIONS of LEAD OCTOATE PB-36:
Films of Lead Octoate PB-36 can be cast on silicon solutions by spin coating.
Lead Octoate PB-36 is a common solvent in metal-organic deposition (MOD) process.
Intermetallic PtPb nanoparticles have been synthesized by the chemical reduction of dimethyl(1,5-cyclooctadiene)platinum and Lead Octoate PB-36 by sodium naphthalide in THF or diglyme.


The precursors used for the photochemical production of PZT or PLZT films were Lead Octoate PB-36, lanthanum(III) 2-ethylhexanoate, zirconyl(IV) 2-ethylhexa- noate, and titanium(IV) isopropoxide.
Lead Octoate PB-36 is used as active or top drier.


Lead Octoate PB-36 is used in polyurethane finishes as major auxiliary drier.
Lead Octoate PB-36 is used important auxiliary drier especially in applications where drying required at low temperatures.
Lead Octoate PB-36 is used mainly in industrial paint applications. Its use has been limited because of environmental effects.


Lead promotes an even through drying and in combination with Calcium and Barium it prevents precipitation of difficult to dissolve Lead compounds.
In conjunction with Butyltitanate Lead is used as an accelerator for the hardening of silicon resins.
Lead Octoate PB-36 is used by consumers, in articles, by professional workers (widespread uses), in formulation or re-packing, at industrial sites and in manufacturing.


Other release to the environment of Lead Octoate PB-36 is likely to occur from: indoor use as processing aid, outdoor use as processing aid, indoor use in close systems with minimal release (e.g. cooling liquids in refrigerators, oil-based electric heaters) and outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids).


Release to the environment of Lead Octoate PB-36 can occur from industrial use: in processing aids at industrial sites and of substances in closed systems with minimal release.
Lead Octoate PB-36 is used in the following products: lubricants and greases, adhesives and sealants, polishes and waxes, anti-freeze products, coating products and fuels.


Other release to the environment of Lead Octoate PB-36 is likely to occur from: outdoor use, indoor use as processing aid, indoor use in close systems with minimal release (e.g. cooling liquids in refrigerators, oil-based electric heaters) and outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids).


Lead Octoate PB-36 is used in the following products: lubricants and greases, adhesives and sealants, polishes and waxes, anti-freeze products, coating products and fuels.
Lead Octoate PB-36 is used in the following products: lubricants and greases, metal working fluids and fuels.


Lead Octoate PB-36 is used for the manufacture of: chemicals.
Other release to the environment of Lead Octoate PB-36 is likely to occur from: outdoor use, indoor use as processing aid, indoor use in close systems with minimal release (e.g. cooling liquids in refrigerators, oil-based electric heaters) and outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids).


Release to the environment of Lead Octoate PB-36 can occur from industrial use: formulation of mixtures, manufacturing of the substance, formulation in materials, in processing aids at industrial sites, in the production of articles, as an intermediate step in further manufacturing of another substance (use of intermediates), as processing aid, for thermoplastic manufacture, as processing aid and of substances in closed systems with minimal release.


Lead Octoate PB-36 is used in the following products: fuels and metal working fluids.
Lead Octoate PB-36 has an industrial use resulting in manufacture of another substance (use of intermediates).
Lead Octoate PB-36 is used in the following areas: formulation of mixtures and/or re-packaging.


Lead Octoate PB-36 is used for the manufacture of: chemicals.
Release to the environment of Lead Octoate PB-36 can occur from industrial use: in processing aids at industrial sites, of substances in closed systems with minimal release, as an intermediate step in further manufacturing of another substance (use of intermediates), formulation of mixtures, manufacturing of the substance and as processing aid.


Release to the environment of Lead Octoate PB-36 can occur from industrial use: manufacturing of the substance, in processing aids at industrial sites, formulation of mixtures, formulation in materials, in the production of articles, as an intermediate step in further manufacturing of another substance (use of intermediates), as processing aid, for thermoplastic manufacture, as processing aid and of substances in closed systems with minimal release.


Films of Lead Octoate PB-36 can be cast on silicon solutions by spin coating.
Lead Octoate PB-36 is a common solvent in metal-organic deposition (MOD) process.
Intermetallic PtPb nanoparticles have been synthesized by the chemical reduction of dimethyl(1,5-cyclooctadiene)platinum and Lead Octoate PB-36 by sodium naphthalide in THF or diglyme.


The precursors used for the photochemical production of PZT or PLZT films were Lead Octoate PB-36, lanthanum(III) 2-ethylhexanoate, zirconyl(IV) 2-ethylhexa- noate, and titanium(IV) isopropoxide.
Lead Octoate PB-36 is used as active or top drier.


Lead Octoate PB-36 promotes hard, through drying throughout the entire film and also promotes flexibility.
In alkyd finishes where fume proof finishes are not specified.
Lead Octoate PB-36 is used s oil drying agents.


Lead Octoate PB-36 acts as a wetting agent, dispersing agent and drier.
Lead Octoate PB-36 is a clean liquid without suspended matter.
Lead Octoate PB-36 promotes through-drying across the entire film depth.


In comparison to linoleate, phthalates and naphthenates, Lead Octoate PB-36 provides better color, odor, stability and viscosity.
Lead Octoate PB-36 shows lower price level in comparison to synthetic acids and metallic salts like those prepared with iso-acids as well as neo-acids.
Lead Octoate PB-36 enables high metal concentration with superior quality and reproducibility.


Lead Octoate PB-36 is one of numerous organo-metallic compounds (also known as metalorganic, organo-inorganic and metallo-organic compounds) sold by American Elements under the trade name AE Organo-Metallics for uses requiring non-aqueous solubility such as recent solar energy and water treatment applications.


The numerous commercial applications for Lead Octoate PB-36 include batteries, cable covering, plumbing, and ammunition.
Lead Octoate PB-36 is used alloys include solder, type metal, and various antifriction metals and compounds.
Lead Octoate PB-36 is suitable to use with oily paints as a drier and also suitable for using with grease.



FEATURES OF LEAD OCTOATE PB-36:
Polymerization catalyst for drying oils and provides internal drying.
Lead Octoate PB-36 is the most effective polymerization catalyst. Suitable to be used together with Cobalt, Calcium etc. driers.

Lead Octoate PB-36 is suitable for use with oily paints as a drier and also suitable for using with grease.
Not recommended to use for Aluminum coatings.
Lead Octoate PB-36 is recommended usage amount is between 0,08% – 0,6% based on solid content.



THROUGH DRIER IN ALKYD RESIN PAINTS USES OF LEAD OCTOATE PB-36:
Lead Octoate PB-36 is one of the auxiliary driers also called as through drier.
Lead Octoate PB-36 is used as active or top drier.
Lead Octoate PB-36 promotes hard, through drying throughout the entire film and also promotes flexibility.

In alkyd finishes where fume proof finishes are not specified.
Lead is used in combination with Cobalt and Calcium octoate, It is always advisable to use Lead Octoate PB-36 after the addition of Calcium octoate to eliminate the possibility of reaction of lead with unreacted phthalic anhydride in alkyd media, which could form lead phathlate.

In tong oil alkyd medium 0.05 to 2.00% of lead is the usual amount required in conjunction with Cobalt and Calcium soaps.
In outside paints and floorfinishes as well as in banking enamels Lead Octoate PB-36 is used with Manganese drier to produce a tough and hard film.
In tong oil phenolic resin, lead promotes drying.

Lead Octoate PB-36 is also used in Polyurethane finishes as major auxiliary drier.
Lead Octoate PB-36 is the most important auxiliary drier especially in applications where drying is required at low temperatures (less than 10 deg. centigrade.)
Different metal concentrations of lead drier such as 18,24,32,36 percentage are used by the paint industry.



FEATURES OF LEAD OCTOATE PB-36:
*Polymerization catalyst for drying oils and provides internal drying.
*Lead Octoate PB-36 is the most effective polymerization catalyst.
*Suitable to be used together with Cobalt, Calcium etc. driers.
*Suitable to use with oily paints as a drier and also suitable for using with grease.
*Not recommended to use for Aluminum coatings.
*Lead Octoate PB-36 is recommended usage amount is between 0,08% – 0,6% based on solid content.



PHYSICAL and CHEMICAL PROPERTIES of LEAD OCTOATE PB-36:
Compound Formula: C16H30O4Pb
Molecular Weight: 493.61
Appearance: Viscous liquid
Melting Point: N/A
Boiling Point: N/A
Density: 1.56 g/mL
Solubility in H2O: N/A
Exact Mass: 494.191062
Monoisotopic Mass: 494.191062
CAS Number: 301-08-6
EINECS Number: 206-107-0
Chemical Formula: [CH3(CH2)3CH(C2H5)COO]2Pb
Molecular Formula: (C8H15O2)2Pb
Molecular Weight: 493.61

Linear Formula: Pb[OOCCH(C2H5)C4H9]2
MDL Number: MFCD00014003
EC No.: 206-107-0
Beilstein/Reaxys No.: N/A
Pubchem CID: 160451
IUPAC Name: 2-ethylhexanoate; lead(2+)
SMILES: CCCCC(CC)C(=O)[O-].CCCCC(CC)C(=O)[O-].[Pb+2]
InchI Identifier: InChI=1S/2C8H16O2.Pb/c2*1-3-5-6-7(4-2)8(9)10;/h2*7H,3-6H2,1-2H3,(H,9,10);/q;;+2/p-2
InchI Key: RUCPTXWJYHGABR-UHFFFAOYSA-L

CAS: 301-08-6; 64742-81-0
EINECS/ELINCS: 206-107-0; 265-184-9
ACRONYM: PB
DILUENT: White Spirite
VISCOSITY:5 - 15(@20°C)
DENSITY: 1,09±0,01(@20°C)
APPEARANCE: Liquid
STORAGE TEMP.: (+5) / (+40)
SHELF LIFE: 1 Y

COLOR: Light Yellow
METAL CONTENT: 23,9 - 24,1 %
SOLİD CONTENT: 45 ± 2 %
CAS Number: 301-08-6
MDL Number: MFCD00014003
Molecular Formula: C16H30O4Pb
Formula Weight: 493.61
Chemical Formula: Pb[OOCCH(C2H5)C4H9]2
Color and Form: colorless to light brown viscous liq.
Physical Characteristics: flash point 324°F, density 1.56

Density: 1,56 g/cm3
Flash point: 162°C
form: liquid
Specific Gravity: 1.56
Water Solubility: Insoluble in water.
Hydrolytic Sensitivity 4: no reaction with water under neutral conditions
Exposure limits NIOSH: IDLH 100 mg/m3; TWA 0.050 mg/m3
CAS DataBase Reference: 301-08-6(CAS DataBase Reference)
EPA Substance Registry System: Lead(II) 2-ethylhexanoate (301-08-6)

density: 1,56 g/cm3
Fp: 162°C
form: liquid
Specific Gravity: 1.56
Water Solubility: Insoluble in water.
Hydrolytic Sensitivity 4: no reaction with water under neutral conditions
Exposure limits NIOSH: IDLH 100 mg/m3; TWA 0.050 mg/m3
CAS DataBase Reference: 301-08-6(CAS DataBase Reference)
EPA Substance Registry System: Lead(II) 2-ethylhexanoate (301-08-6)



FIRST AID MEASURES of LEAD OCTOATE PB-36:
-Description of first-aid measures:
*If inhaled:
If breathed in, move person into fresh air.
*In case of skin contact:
Wash off with soap and plenty of water.
*In case of eye contact:
Flush eyes with water as a precaution.
*If swallowed:
Never give anything by mouth to an unconscious person. Rinse mouth with water.
-Indication of any immediate medical attention and special treatment needed:
No data available



ACCIDENTAL RELEASE MEASURES of LEAD OCTOATE PB-36:
-Environmental precautions:
Do not let product enter drains.
-Methods and materials for containment and cleaning up:
Keep in suitable, closed containers for disposal.



FIRE FIGHTING MEASURES of LEAD OCTOATE PB-36:
-Extinguishing media:
*Suitable extinguishing media:
Use water spray, alcohol-resistant foam, dry chemical or carbon dioxide.
-Further information:
No data available



EXPOSURE CONTROLS/PERSONAL PROTECTION of LEAD OCTOATE PB-36:
-Control parameters:
--Ingredients with workplace control parameters:
-Exposure controls:
--Personal protective equipment:
*Eye/face protection:
Use equipment for eye protection.
*Skin protection:
Handle with gloves.
Wash and dry hands.
*Body Protection:
Impervious clothing
*Respiratory protection:
Respiratory protection not required.
-Control of environmental exposure:
Do not let product enter drains.



HANDLING and STORAGE of LEAD OCTOATE PB-36:
-Conditions for safe storage, including any incompatibilities:
*Storage conditions:
Store in cool place.
Keep container tightly closed in a dry and well-ventilated place.
Containers which are opened must be carefully resealed and kept upright to prevent leakage.



STABILITY and REACTIVITY of LEAD OCTOATE PB-36:
-Reactivity:
No data available
-Chemical stability:
Stable under recommended storage conditions.
-Possibility of hazardous reactions:
No data available
-Conditions to avoid:
No data available

LEAD OXIDE = MASSICOT = GALENA


CAS Number: 1317-36-8
EC Number: 215-267-0
MDL Number: MFCD00011164
Chemical formula: PbO


Lead oxide is an inorganic lead salt composed from lead(2+) and oxide.
Lead oxide is an inorganic lead salt and a metal oxide.
Lead oxide contains a lead(2+).
Lead oxides are amphoteric and dissolve in aqueous solution under both acidic and basic conditions.


Lead oxide can be found in many forms including α-PbO (litharge) and β-PbO (massicot), α-PbO2 (scrutinyite) and β-PbO2 (plattnerite), and Pb3O4 (minium).
Lead oxide (PbO) exists in two crystalline modifications: red tetragonal (α-PbO) and yellow orthorhombic (β-PbO).
β-PbO is obtained at temperatures higher than 486°C and α-PbO, at lower temperatures.


Lead oxide, also called lead monoxide, is the inorganic compound with the molecular formula PbO.
Lead oxide occurs in two polymorphs: litharge having a tetragonal crystal structure, and massicot having an orthorhombic crystal structure.
Modern applications for Lead oxide are mostly in lead-based industrial glass and industrial ceramics, including computer components.
Lead oxide is an amphoteric oxide.

Lead oxide is a general term and can be either lead monoxide or "litharge" (PbO); lead tetroxide or "red lead" (Pb3O4); or black or "gray" oxide which is a mixture of 70 percent lead monoxide and 30 percent metallic lead.
Black lead is made for specific use in the manufacture of lead
acid storage batteries.


Because of the size of the lead acid battery industry, Lead oxide is the most important commercial compound of lead, based on volume.
Total oxide production in 1989 was 57,984 megagrams (64,000 tons).
Lead oxide is soluble in concentrated alkali, hydrochloric acid, and ammonium chloride.
Lead oxide is insoluble in water, dilute alkali and alcohol.


Lead oxide is an inorganic lead salt composed from lead(2+) and oxide
Lead oxide, or litharge, is a yellow oxide of lead of formula PbO, created by heating lead in air.
Lead oxide can also be formed by heating lead(II) nitrate(V) (Pb(NO3)2).
Lead oxide is amphoteric, meaning it reacts with acids to form Pb2+ and with bases to form plumbate(II)


In 2020, Lead Oxides were the world's 1148th most traded product, with a total trade of $136M.
Between 2019 and 2020 the exports of Lead Oxides decreased by -12.9%, from $156M to $136M.
Trade in Lead Oxides represent 0.00081% of total world trade.
Lead Oxides are a part of Inorganic chemicals.


They include Lead monoxide (litharge, massicot), Lead oxides other than monoxide, red and orange lead, and Red lead and orange lead.
Lead oxide, also called lead monoxide, is the inorganic compound with the molecular formula PbO.
Lead oxide occurs in two polymorphs: litharge having a tetragonal crystal structure, and massicot having an orthorhombic crystal structure.
Lead oxide is an amphoteric oxide.


Lead oxide, often known as litharge, is a yellow oxide of lead with the formula PbO formed by heating lead in the presence of oxygen.
Lead oxide is red to orange powder.
Lead Oxide (Litharge)(PBO) is available in two crystalline modifications at temperatures higher than 486C or lower temperatures.
This is provided in 99% pure form without any adulteration to meet varied demands of different sectors.


Lead oxide, known also as lead peroxide, lead brown, lead oxide brown, and lead (IV) oxide (PbO(2)), is a very strong oxidizer and may react violently with reducing agents.
As a solid, Lead oxide forms a dark brown powder that is odorless and insoluble in water, with a melting point of about 290 degrees Celsius.
Lead oxide is yellow in color, water insoluble, and is odorless.


Lead oxide constitutes a family of compounds with varying numbers of oxygen atoms per molecule, depending on the valence state (+2 or +4) of the lead, and varying crystal morphs, even with the same chemical formulas.
These compounds are familiar to geologists as ores and crystal minerals, to inorganic chemists, and to manufacturers as pigments.
Massicot, an orthorhombic crystal of Lead oxide (PbO), and the mineral litharge, the tetragonal morph, are found on the edges of lead ore bodies, and to a petrologist, are very indicative of the degree of oxidation.


A minor ore of lead, massicot is used as a pigment and is collected by rock hounds as a mineral specimen.
Litharge figures prominently in the manufacturing of ceramic products, including capacitors, Vidicon tubes, and electrophotographic plates.
Lead from litharge supplies the lead salts used as stabilizers for polyvinyl chloride and other plastics, soaps (lead stearate), oil refining, and driers for paints.


Lead monoxide, also known as lead protoxide, has a molecular weight of 233.19, a boiling point of 1,472 degrees Celsius, and a melting point of 888 degrees Celsius.
Adding carbon to lead monoxide will yield elemental lead and carbon monoxide.
Another lead oxide mineral, minium, is also known as "red lead" and is an oxidation product of other lead minerals.


Minium is more widely used as a pigment in paints and dyes and less important to rock collectors.
To the novice chemist or geologist, it might appear that lead takes on a third valance state based on the chemical formula for red lead.
However, these compounds are actually composed of lead having the two valence states (Pb+2 and Pb+4), and are typical members of the spinel group of oxide minerals.


Known as lead tetraoxide, minium red lead, or Saturn red, minium has a molecular weight of 695.60, appears as a heavy, odorless red powder, and features a melting point of about 500 degrees Celsius.
Crystals of minium are red, ranging from scarlet to brick red, tetragonal, opaque, and generally well striated.
Under ultraviolet light (UV), some specimens of this variety of lead oxide fluoresce an orange color.


In contrast, massicot crystals are yellow to reddish yellow, opaque, and orthorhombic.
Both feature specific gravities well above average for any mineral (8.9-9.2 for minium; 9.6-9.7 for massicot).
As with other lead compounds, lead monoxide and lead tetraoxide are considered toxic if ingested or released into the environment.
Annual lead oxide production exceeds 64,000 tons.


Lead oxide is right-red crystalline substance or amorphous powder; density 9.1 g/cm3; decomposes on heating to 500°C, melts at 830°C under pressure and oxygen; insoluble in water and alcohol.
Lead oxide is soluble in glacial acetic acid, hot hydrochloric acid, and a dilute nitric acid-hydrogen peroxide mixture.
Together with ZnO, PbO is considered one of the Metallic oxide fluxes.


Lead oxide reacts easily with silica to form low melting lead silicates of high gloss and deep character.
Lead is very easy to use.
Lead oxide is the heaviest oxide and produces incredible colors with most pigments.
Lead oxide is especially recommended for iron tan, browns and reds and titanium yellows and reds.


Lead has 'blemish healing' and flow characteristics that are unmatched.
Lead glazes tend to have high resistance to chipping.
In addition, lead is a 'forgiving material' that tends to hide imperfections on the finished fired surface.
Lead glazes have been demanded for fine China for many years, although substitutes have been developed.


Lead carbonate, a favorite source is highly pure and has a very fine particle size.
It also promotes good suspension in raw glazes as well as rapid fusion.
Lead oxides are a group of inorganic compounds with formulas including lead (Pb) and oxygen (O).


Common lead oxides include:
Lead(II) oxide, PbO, litharge (red), massicot (yellow)
Lead(II,IV) oxide, Pb3O4, minium, red lead
Lead dioxide (lead(IV) oxide), PbO2


Less common lead oxides are:
Lead(II,IV) oxide, Pb2O3, lead sesquioxide (reddish yellow)
Pb12O19 (monoclinic, dark-brown or black crystals)
The so-called black lead oxide, which is a mixture of PbO and fine-powdered metal Pb and used in the production of lead–acid batteries.


Lead oxides are basically an oxide’s family varying in color (grey/green, red, and yellow), in degree of oxidation (PbO, Pb3O4, PbO2) and in crystal structure (in forms of PbO, orthogonal and tetragonal).
Lead oxide is a term that can be either Lead monoxide or litharge Lead tetroxide or Red Lead or Gray or Black oxide which is a mixture of 30 percent metallic Lead and 70 percent Lead monoxide.
Black Lead is made for specific use in Lead acid storage batteries manufacturing.


Due to large use in the Lead acid battery industry, Lead monoxide is one of the most important compounds of Lead, based on volume.
Due to its electrical and electronic properties, litharge is also used in various components for different types of use like capacitors, electro photographic plates, and Video tubes, even in ferromagnetic and ferroelectric materials.
Their wide range of chemical and physical properties, Lead oxides have been know and used worldwide since before the ancient Romans.



USES and APPLICATIONS of LEAD OXIDE:
Lead oxide is used primarily in the manufacture of various ceramic products.
Because of its electrical and electronic properties, Lead oxide is also used in capacitors, and electrophotographic plates, as well as in ferromagnetic and ferroelectric materials.


Lead oxide is also used as an activator in rubber, a curing agent in elastomers, a sulfur removal agent in the production of thioles and in oil refining, and an oxidation catalyst in several organic chemical processes.
Lead oxide also has important markets in the production of many lead chemicals, dry colors, soaps (i. e., lead stearate), and driers for paint.
Another important use of Lead oxide is the production of lead salts, particularly those used as stabilizers for plastics, notably polyvinyl chloride materials.


Lead oxide is employed mostly in lead-based industrial glass and industrial ceramics, including computer components.
Lead oxide is used as an intermediate/precursor in the manufacture of several products, for example water proof cements, lubricants, lubricating oils, inorganic pigments, lead soaps, petroleum refining, rubber, cathode ray tube glass, and polyvinyl chloride (PVC).
Lead oxide is useful for lead acid batteries as cathode and anode.


Lead oxide scores significant applications in oil, gas and chemical manufactures.
Lead oxide is an efficient catalyst for condensation reactions in organic synthesis.
Lead oxide is a component of lead paints and is used extensively in manufacturing of lead glasses and ceramic glazes.
Lead oxide is the main ingredient of the paste used for filling the plates during manufacturing of lead-acid batteries.


A mixture of Lead oxide with glycerine sets to a hard, waterproof cement that has been used to join the flat glass sides and bottoms of aquaria, and was also once used to seal glass panels in window frames.
Lead oxide is used in vulcanization of rubber.
Lead oxide is used in certain condensation reactions in organic synthesis.


Lead oxide is used in cathode ray tube glass to block X-ray emission, but mainly in the neck and funnel because it can cause discoloration when used in the faceplate.
Heated lead nitrate can also be used to make Lead oxide.
Because lead is still a significant component of automotive lead-acid batteries, the consumption of lead, and therefore the processing of Lead oxide, is proportional to the number of vehicles.


Lead oxide has been widely used in batteries, gas sensors, pigments, ceramics, and glass industries.
High purity Lead Oxide (minio), predominantly used as an essential element to create brightness and transparency in glass, is today also used in various manufacturing fields such as ceramics, crystal, paints and batteries.
Lead oxide is used as an industrial oxidizing agent, in storage batteries, and in the textile industry.


Lead oxide is a raw material for the production of “lead paste” for battery manufacture.
Lead Oxide, Lead(II) Oxide, or Litharge is commonly used for fire assaying of gold and silver ores.
A mixture of 70 percent lead monoxide and 30 percent metallic lead, sometimes referred to as black or gray oxide, is used to manufacture lead acid batteries.


Because of the size of the lead acid battery industry due to the large number of automobiles and airplanes worldwide, lead monoxide is the most important commercial compound of lead, based on volume.
Lead oxide is used in ointments, plasters, pottery glazes, glass flux, lead glass, varnishes, metal cements, colorants (brass, bronze, hair, nails, wool, and horn), and rubber pigments.


Lead oxide is also used to make boiled linseed oil and to assay gold and silver ores.
Lead oxide is used in storage batteries, high-temperature lubricants, capacitors, electrophotographic plates, transducers, and magnetic materials.
Lead oxide has many applications.
The most important use of Lead oxide is in paint and storage-batteries.


Lead oxide is used as a pigment in corrosion-protecting paints for steel surfaces.
Lead oxide also is used in positive battery plates; in colored glasses and ceramics; in glass sealants for television picture tubes; in propellants and explosives; in radiation shields for x-rays and gamma rays; in the vulcanization of rubber; in glass-writing pencils; in adhesives for tire cords; in foaming agents and waterproofing materials; in plasters and ointments; in lead dioxide matches; and as a catalyst for oxidation of carbon monoxide in exhausts.


Lead oxide is used Plasters and ointments; manufacture of colorless glass; glaze for faience; flux for porcelain painting, protective paint for iron and steel; oil-color for ship paints, varnishes; coloring rubber; cement for glass, gas and steam pipes; storage batteries; pencils for writing on glass; manufacture of lead peroxide, matches.
Red lead (Pb3O4) is a brilliant red-orange colored synthetic inorganic pigment used mainly as a protective priming coat for steel work rather than a coloring pigment in paints.


Lead oxide is used to prepare colorless glass, faience glaze, porcelain painting flux, iron and steel coatings, rubber pigment and in glass cement.
Lead oxide is also used in gas and steam pipes, storage batteries, writing on glass and to make lead peroxide and matches.
Lead oxide is associated with linseed oil and used as a thick, long-lasting anti-corrosive paint.


Lead oxide gives better water resistant properties by replacing magnesium oxide.
Further, Lead oxide is used in the manufacture of lead glass and rustproof primer paints.
In addition to this, Lead oxide acts as a pigment for primer paints for iron objects.


Lead oxide is widely used in glazing pottery, lead glass, storage batteries, glass flux for painting, metal cement with glycerol, etc.
Besides this, Lead oxide is also utilized in the preparation of lead subacetate solutions, ointments and plasters, iridescent colors, coloring sulfur-containing substances, etc.


-Typical Applications of Lead oxide:
Glazing pottery, Glass flux for painting, Lead glass; Metal cement with Glycerol; Storage batteries; Ointments and Plasters; Preparing lead subacetate solutions.
Lead oxide is used producing iridescent colors on brass and bronze; Coloring sulfur-containing substances; Pigment for rubber; Oil refining; Varnishes, Paints, and Enamels; Aassays for precious metal ores



CHEMICAL of LEAD OXIDE:
Lead oxide is a general term and can be either lead monoxide or "litharge" (PbO); lead tetroxide or "red lead" (Pb3O4); or black or "gray" oxide which is a mixture of 70 percent lead monoxide and 30 percent metallic lead.
Black lead is made for specific use in the manufacture of lead acid storage batteries.
Because of the size of the lead acid battery industry, lead monoxide is the most important commercial compound of lead, based on volume.
Red lead is produced by oxidizing litharge in a reverberatory furnace.
The major lead pigment is red lead(Pb3O4), which is used principally in ferrous metal protective paints.



TYPES of LEAD OXIDE:
Lead oxide exists in two types:
Red tetragonal (α-PbO), obtained at lower temperatures than the β-PbO
Yellow orthorhombic (β-PbO), which is obtained temperatures higher than 486 °C (907 °F)



STRUCTURE of LEAD OXIDE:
As determined by X-ray crystallography, both polymorphs, tetragonal and orthorhombic feature a pyramidal four-coordinate lead center.
In the tetragonal form the four lead–oxygen bonds have the same length, but in the orthorhombic two are shorter and two longer.
The pyramidal nature indicates the presence of a stereochemically active lone pair of electrons.
When Lead oxide occurs in tetragonal lattice structure it is called litharge; and when the PbO has orthorhombic lattice structure it is called massicot.

Lead oxide can be changed from massicot to litharge or vice versa by controlled heating and cooling.
The tetragonal form is usually red or orange color, while the orthorhombic is usually yellow or orange, but the color is not a very reliable indicator of the structure.
The tetragonal and orthorhombic forms of Lead oxide occur naturally as rare minerals.



SYNTHESIS of LEAD OXIDE:
PbO may be prepared by heating lead metal in air at approximately 600 °C (1,100 °F).
At this temperature Lead oxide is also the end product of decomposition of other oxides of lead in air.
Thermal decomposition of lead(II) nitrate or lead(II) carbonate also results in the formation of PbO:
2 Pb(NO3)2 → 2 PbO + 4 NO2 + O2
PbCO3 → PbO + CO2

Lead oxide is produced on a large scale as an intermediate product in refining raw lead ores into metallic lead.
The usual lead ore is galena (lead(II) sulfide).
At a temperature of around 1,000 °C (1,800 °F) the sulfide is converted to the oxide:
2 PbS + 3 O2 → 2 PbO + 2 SO2
From lead
There are two principal methods to make lead monoxide both of which resemble combustion of the lead at high temperature.

Barton pot method:
The refined molten lead droplets are oxidized in a vessel under a forced air flow which carries them out to the separation system (e.g. cyclonic separators) for further processing. 
Oxides produced by this method are mostly a mixture of α-PbO and β-PbO. The overall reaction is:
2Pb + O2 450 °C (842 °F)→ 2PbO

Ball mill method:
The lead balls are oxidized in a cooled rotating drum.
The oxidation is achieved by collisions of the balls.
Just like in Barton pot method, the supply of air and separators may also be used.



PHYSICAL and CHEMICAL PROPERTIES of LEAD OXIDE:
Chemical formula: PbO
Molar mass: 223.20 g/mol
Appearance: red or yellow powder
Density: 9.53 g/cm3
Melting point: 888 °C (1,630 °F; 1,161 K)
Boiling point: 1,477 °C (2,691 °F; 1,750 K)
Solubility in water: 0.017 g/L
Solubility: insoluble in dilute alkalis, alcohol
soluble in concentrated alkalis
soluble in HCl, ammonium chloride
Magnetic susceptibility (χ): 4.20×10−5 cm3/mol
Crystal structure: Tetragonal, tP4
Space group: P4/nmm, No. 129

Molecular Weight: 223
Hydrogen Bond Donor Count: 0
Hydrogen Bond Acceptor Count: 1
Rotatable Bond Count: 0
Exact Mass: 223.97157
Monoisotopic Mass: 223.97157
Topological Polar Surface Area: 1 Ų
Heavy Atom Count: 2
Formal Charge: 0
Complexity: 0
Isotope Atom Count: 0
Defined Atom Stereocenter Count: 0
Undefined Atom Stereocenter Count: 0
Defined Bond Stereocenter Count: 0
Undefined Bond Stereocenter Count: 0
Covalently-Bonded Unit Count: 2
Compound Is Canonicalized: Yes

Melting point: 500 °C
Boiling point: 800°C
Density: 9,1 g/cm3
vapor pressure: 10 mm Hg ( 0 °C)
form: red powder
color: Orange
Water Solubility: Soluble in hydrochloric acid, glacial acetic acid and nitric acid and hydrogen peroxide.
Merck: 14,5425
Exposure limits ACGIH: TWA 0.05 mg/m3
NIOSH: IDLH 100 mg/m3; TWA 0.050 mg/m3
Stability: Stable.

Physical state: powder
Color: yellowlight yellow
Odor: odorless
Melting point/range: 886 °C - lit.
Initial boiling pointand boiling range: > 600 °C at ca.1.013 hPa
Flammability (solid, gas): The product is not flammable.
Upper/lower flammability or explosive limits: No data available
Flash point: Not applicable
Autoignition temperature: No data available
Decomposition temperature: No data available
pH: 8 - 9 at 100 g/l at 20 °C (slurry)

Viscosity
Viscosity, kinematic: No data available
Viscosity, dynamic: No data available
Water solubility: 0,0702 g/l at 20 °C
Partition coefficient: n-octanol/water: Not applicable for inorganic substances
Vapor pressure: No data available
Density: 9,530 g/cm3 at 20 °C
Relative density: 9,96 at 22,5 °C
Particle characteristics: No data available
Explosive properties: No data available
Oxidizing properties: none
Other safety information: No data available



FIRST AID MEASURES of LEAD OXIDE:
-After inhalation:
fresh air.
Immediately call in physician.
-In case of skin contact:
Take off immediately all contaminated clothing.
Rinse skin with water/ shower.
Consult a physician.
-After eye contact:
Rinse out with plenty of water.
Call in ophthalmologist.
Remove contact lenses.
-After swallowing:
Immediately make victim drink water (two glasses at most).
Consult a physician.
-Indication of any immediate medical attention and special treatment needed:
No data available



ACCIDENTAL RELEASE MEASURES of LEAD OXIDE:
-Environmental precautions:
Do not let product enter drains.
-Methods and materials for containment and cleaning up:
Cover drains.
Collect, bind, and pump off spills.
Take up carefully.
Dispose of properly.



FIRE FIGHTING MEASURES of LEAD OXIDE:
-Extinguishing media:
*Suitable extinguishing media:
Use extinguishing measures that are appropriate to local circumstances and the surrounding environment.
*Unsuitable extinguishing media:
For this substance/mixture no limitations of extinguishing agents are given.
-Further information:
Prevent fire extinguishing water from contaminating surface water or the ground water system.



EXPOSURE CONTROLS/PERSONAL PROTECTION of LEAD OXIDE:
-Control parameters:
*Ingredients with workplace control parameters:
-Exposure controls:
--Personal protective equipment:
*Eye/face protection:
Use equipment for eye protection.
Safety glasses.
*Skin protection:
Handle with gloves.
Wash and dry hands.
Full contact:
Material: Nitrile rubber
Minimum layer thickness: 0,11 mm
Break through time: 480 min
Splash contact:
Material: Nitrile rubber
Minimum layer thickness: 0,11 mm
Break through time: 480 min
*Body Protection:
protective clothing
-Control of environmental exposure:
Do not let product enter drains.



HANDLING and STORAGE of LEAD OXIDE:
-Precautions for safe handling:
*Advice on safe handling:
Work under hood.
*Hygiene measures:
Immediately change contaminated clothing.
Apply preventive skin protection.
Wash hands and face after working with substance.
-Conditions for safe storage, including any incompatibilities:
*Storage conditions:
Tightly closed.
Dry.
Keep in a well-ventilated place.
Keep locked up or in an area accessible only to qualified or authorized persons.
*Storage class:
Storage class (TRGS 510): 6.1D: Non-combustible



STABILITY and REACTIVITY of LEAD OXIDE:
-Reactivity:
No data available
-Chemical stability:
The product is chemically stable under standard ambient conditions (room temperature) .



SYNONYMS:
Lead(II) oxide
Lead monoxide
Litharge
Massicot
Plumbous oxide
Galena
1335-25-7
Lead oxide (PbO), lead-contg.
68411-78-9
Leady lead monoxide
EINECS 215-626-1
LEAD OXIDE [HSDB]
LEAD MONOXIDE [MI]
LEAD MONOXIDE [VANDF]
LEAD MONOXIDE [WHO-DD]
DTXSID0029638
CHEBI:8104
EINECS 270-148-0
A26757
C17379
J-52163
Lead Dioxide
Lead (IV) oxideLead peroxide
lead (IV) oxide
Plumbic oxide
Plattnerite
Bleimonoxid; Bleioxyd
C.I. 77577
C.I. Pigment Yellow 46
CI 77577
CI Pigment Yellow 46
Lead Oxide Yellow
Lead monooxide
Lead monoxide
Lead oxide
Lead oxide (PbO)
Lead oxide
Lead protoxide
Lead(2+) oxide
Lead(II) oxide
Litharge
Litharge Pure
Litharge Yellow L-28
Massicot
Massicotite
Plumbi monoxidum
Plumbous oxide
Plumbum oxydatum
Yellow Lead Ocher
UN3288

Stearic acid, lead salt; Octadecanoic acid, lead salt; Lead(II) n-octadecanoate; Lead (II) stearate; Stearinsäure, Bleisalz; ácido esteárico, sal de plomo; Acide stéarique, sel de plomb; CAS NO: 1072-35-1, 7428-48-0, 52652-59-2

LECIGEL is a versatile phospholipid-based ingredient which combines in the same time emulsifying properties of lecithin with thickening and texturizing effects of a polymer.
Easier-to-use, LECIGEL allows a better dispersion either in oil or water phase, can be easily added at any stage of the formulation process and is suitable for both hot and cold processes.

LECIGEL offers unique white oil-free gel-cream with the typical “phospholipid touch” characterized by a cool, soft and silky skin feel, for a unique sensorial skin feel.
Also, LECIGEL is perfectly adapted to high level of ethanol, over a wide range of pH and is compatible with electrolytes.

LECIGEL is a preservative-free, multi-functional sensorial ingredient.
LECIGEL is a gelling-emulsifying agent and efficacy booster.

LECIGEL is a smart 4-in-1 lab partner with sensory coolness and outstanding textures.
LECIGEL shows high versatility of use and maximum oil phase.

This easy-to-use ingredient is suitable for hot or cold process.
LECIGEL is based on phospholipids and LECIGEL brings active properties.

LECIGEL offers light, supple & slippery textures, high spreadability with quick absorption, ultra-cool skin feel, quick break effect upon application, non-tacky and non-greasy properties.
LECIGEL brings hydration for a 100% active formula base and improves skin hydration with a long-lasting effect.

LECIGEL acts as a powerful delivery system by boosting penetration & bioavailability of active ingredients for a maximum efficacy.
LECIGEL triggers positive emotions and provides moments of happiness upon application.

LECIGEL is used in feel aqueous gels, gel creams and emulsions (O/W, O/G, Si/W).
LECIGEL is used in face-, body-, sun-, hair-, baby-, men care & make-up formulations.

The multifunctional sensorial gelling and emulsifying LECIGEL.
Phospholipid-based gelling agent with emulsifying properties.

LECIGEL is a gelling agent with emulsifying properties.
LECIGEL allows the increase in the viscosity and the stability of formulas.

Suitable for both cold and hot processes, LECIGEL also helps to adjust the viscosity at the end of the formulation process.
Easy-to-use, LECIGEL is compatible with most emulsifiers and is stable over a wide range of pH.
Especially adapted for the formulation of gel-creams, LECIGEL provides the typical “phospholipid touch” with a cool, soft and non-greasy skin feel.'

The following dose is recommended:
As stabiliser: 0.2% and above
As thickener: 0.5% and above
As emulsifier: 0.5% and above for LECIGEL

LECIGEL comes in the form of a beige powder that can be added at virtually any stage of formulation.
This means that you can either put LECIGEL in with the liquid oil phase and then disperse in with the water which will make LECIGEL almost instantly thicken or you can add LECIGEL to the water and then introduce LECIGEL to the oil.

Putting LECIGEL in a small amount of liquid that is not water, helps a little with dispersion but LECIGEL is not necessary to do so.
LECIGEL can also dusted in at the end of the process if you want.

LECIGEL is not shear sensitive which means blending at high speeds will not break the gel.
You can use LECIGEL hot so that comes in handy if you want to use hard butters that need melting.

If you are using ingredients that need melting / heating I suggest that you heat the oil and water phase (lecigel can be in either) and then when the fat is melted and both phases are at a similar temperature, combine them.
LECIGEL suggest doing this as you don't want the cold water causing your fats to solidify before they have a chance to blend with the water/emulsifier.

LECIGEL can emulsify up to 20% oil phase, 10% oils can be emulsified per each 1% of LECIGEL and the final viscosity depends on the type of oils and butters used.

Surprisingly, 1.5% LECIGEL can take 20% ethanol (alcohol) too so if you wanted to use that as your preservative LECIGEL is possible.
LECIGEL can tolerate up to 50% ethanol with 2% LECIGEL.

LECIGEL is also fairly resistant against electrolytes but the manufacturer advises to add them after emulsification if possible.
They also suggest that LECIGEL has a synergy with xanthan and sclerotium gum which helps if you want to use electrolytes.

LECIGEL is a texturizing agent with emulsifying properties.

LECIGEL is a mutivalent ingredient that combines the emulsifying properties of lecithin with the thickening and texturizing effects of a polymer at the same time.
LECIGEL has been optimized from various points of view such as use, versatility and impact on the color of the emulsion, while still producing white gel creams.

Thanks to the concentration of active raw material, LECIGEL powder is effective even if used at low percentages.

Applications of LECIGEL:
Emulsifier for cream-gels starting from 0.5%
Stabilizer of emulsions starting from 0.2%

Uses of LECIGEL:
LECIGEL can be incorporated into many types of face, body, sun and hair care products.
LECIGEL produces gel creams with the typical phospholipid touch characterized by freshness and a soft and silky texture.
The initially greasy texture of LECIGEL melts during application without leaving a sticky sensation and giving the skin a velvety touch for a long time and a feeling of comfort and well-being.

LECIGEL is easy to use, disperses well in both the fat and aqueous phase or can be added at any time in the formulation process.
LECIGEL can be used both in hot and cold processes or in one-pot processes.

LECIGEL is not sensitive to shear force and this allows the use of any type of mixer.
As an O / A emulsifier, LECIGEL can be formulated with any type of fat phase, either alone at a percentage starting from 0.5% or in combination with a wide variety of other emulsifiers.

LECIGEL is used starting from 0.1% LECIGEL perfectly stabilizes the emulsions.
LECIGEL can be formulated with high amounts of ethanol and in a wide pH range, LECIGEL is also compatible with electrolytes.

Ethanol levels over 20% can be reached.
Recommended use percentages: 0.2 - 4.0%.

Mode of Action of LECIGEL:
Hot or cold process gelling agents with emulsifying properties
Introduction into water or oil phase or after emulsion

Stability And Reactivity of LECIGEL:

Stability: Stable at temperature lower than 25°C and under normal conditions of use.

Hazardous reactions:
- Conditions to avoid: Heat, direct light, humidity.
- Materials to avoid: Strong oxidizing agents, strong acids and bases.

Hazardous decomposition products:
During combustion or thermal decomposition (pyrolysis), LECIGEL may release: toxic and irritating vapours (CO, CO2) and NOx.

Dosage:
Recommended dosage: 0.1 - 2.0%
Gelling agent for aqueous gels: 0.5 - 2.0%
Emulsifier for gel-creams: 0.5 - 2.0%
Viscosity adjuster: >0.5%
Stabilizer of emulsions: >0.1%

Handling And Storage of LECIGEL:

Handling:

Technical measures:
Do not require specific or particular technical measures.
Close well packaging after use.

Precautions:
Avoid contact with skin and eyes.
Avoid the formation of dust.

Do not breathe dust.
Keep aways from food and drinks.
Wash hands and any other zone exposed with soap and water before eating, drinking, smoking and before leaving work.

Storage of LECIGEL:
Store the container tightly closed, protected from air, direct light and humidity, in a cool and dry area, and attemperatures lower than 25°C.
Store in LECIGEL packaging in a cool place away from heat sources.

Recommended packaging materials:
Original packaging (carton with inner polyethylene bag).

First Aid Measures of LECIGEL:

Skin contact:
Wash with soap and plenty of water.
Consult a doctor if necessary.

Eye contact:
Rinse with plenty of water immediately and extended in keeping the eyes disregarded.
Consult an ophthalmologist.

Ingestion:
No dangers which require special measures of first aid.
On the basis of studies carried out on similar products, LECIGEL should not be toxic.

Inhalation:
Move the affected person away from the contaminated area and into the fresh air.

Fire-Fighting Measures of LECIGEL:

Flammability:
LECIGEL is not flammable.

Suitable extinguishing media:
Water,Carbon dioxide (CO2), foam.

Not suitable extinguishing media:
water jet.

Specific hazards:

Under the action of heat or during combustion:
May form toxic and irritating vapours (carbon oxides).
Wet powder can cause extremely slipping conditions.

Specific fire fighting methods:
Avoid the dumping of extinguishing water in the environment.
Do not attempt to fight the fire without suitable protective equipment.

Protection of fire-fighters:
Complete protective clothing.
Self-contained and insulating breathing apparatus.

Accidental Release Measures of LECIGEL:

Personal precautions:
Avoid contact with skin and eyes.
Avoid the formation of dust.

Environmental precautions:
Do not allow product to spread into the soil and to enter sewers/ surface or ground water.

Methods for cleaning up:
Clean quickly with a shovel or by using a suction cleaning equipment.
Store the residues in adapted closed containers.

After cleaning, rinse the remaining traces with water.
Dispose of at a licensed waste collection point.

Properties of LECIGEL:
Provides gels & gel-creams,
Stabilizes and adjusts viscosity of emulsions,
Cold & hot process,
Quick-break effect,
High cooling effect: immediately lowers skin temperature with a lasting effect up to 20 minutes,
Decreases TEWL,
Increases skin hydration,
Enhances penetration and bioavailability of active ingredients to get better and/or faster results,
Triggers positive emotions and provides moments of happiness upon application.

INCI Name of LECIGEL:
Sodium Acrylates Copolymer (and) Lecithin

SYNONYMS PHOSPHATIDYCHOLINE1-ACYLHYDROLASE CAS NO:9043-29-2

E322, CAS No. 8002-43-5, Noms français : Lécithine, Lécithine de soya, Phosphatidylcholine. Noms anglais : Lecithin, soybean, Lecithins, Lexithin, Soya lecithin, Soybean lecithin. Utilisation et sources d'émission, PC;kelecin;LECITHIN;froM Egg;Alcolec-S;granulestin;L-α-Lecithin;Lecithin, NF;LIPOID(R)E80;Lecithin Agent anti-oxydant, agent dispersant. Émulsifiant (pour éviter que les graisses et l'eau ne se séparent de l'aliment) dérivé de l'huile de soja et composée principalement de phospholipides, un assemblage d’acides gras, de phosphates et de glycérol. C'est une substance alimentaire controversée sur ses éventuels danger pour la santé. On peut pourtant la trouver dans l'usage alimentaire et pharmaceutique.La lécithine de soja est une substance riche en acides gras polyinsaturés essentiels (indispensables à l'organisme), les acides linoléique et linolénique

Monostéarate de sorbitane (Span 60), Tristéarate de sorbitane (Span 65),Monolaurate de sorbitane (Span 20), Monooléate de sorbitane (Span 80), Monopalmitate de sorbitane (Span 40), Trioléate de sorbitane (Span 85), Les esters de sorbitane forment une classe de tensioactifs non ioniques dérivés du sorbitane par estérification d'une ou plusieurs de ses fonctions alcool ou phénol. Ils sont utilisés comme émulsifiants dans la préparation d'émulsions et de crèmes à usage pharmaceutique et cosmétique. Certains d'entre eux sont également utilisés comme additifs alimentaires. Lorsqu'ils sont utilisés seuls, ils produisent des émulsions stables de type w/O (les plus courants ont une HLB comprise entre 1,8 et 8,6), mais ils sont fréquemment utilisés avec un polysorbate dans des proportions variables pour produire des émulsions w/O ou o/W à volonté avec différentes textures et consistances. Les esters de sorbitane sont parfois désignés par le nom de marque Span. Six d'entre eux sont utilisés comme additifs alimentaires.

Lemon Juice Concentrate; Capsaicin; 8-Methyl-N-vanillyl-trans-6-nonenamide cas no: 404-86-4

acide cis-linoleique; acide linoleique;Linoelaidic Acid; acido linoleico; LEINOLEIC ACID; Acide linoléique; LINOLEIC ACID, N° CAS : 60-33-3 (CIS). Nom INCI : LINOLEIC ACID. Nom chimique : 9,12-Octadecadienoic acid (9Z, 12Z)-. N° EINECS/ELINCS : 200-470-9 (CIS), Utilisation et sources d'émission: Fabrication de peintures, agent dispersantSes fonctions (INCI) : Agent nettoyant : Aide à garder une surface propre. Emollient : Adoucit et assouplit la peau. Conditionneur capillaire : Laisse les cheveux faciles à coiffer, souples, doux et brillants et / ou confèrent volume, légèreté et brillance. Agent d'entretien de la peau : Maintient la peau en bon état.Tensioactif : Réduit la tension superficielle des cosmétiques et contribue à la répartition uniforme du produit lors de son utilisation. Linoleic acid. Noms français : (Z,Z)-9,12-OCTADECADIENOIC ACID; 9,12-OCTADECADIENOIC ACID; 9,12-OCTADECADIENOIC ACID (Z,Z)-; 9,12-OCTADECADIENOIC ACID, (Z)-; 9,12-OCTADECADIENOIC ACID, (Z,Z); Acide linoléique; CIS,CIS-9,12; OCTADECADIENOIC ACID; CIS,CIS-ACIDE OCTADIDECENE 9,12-OIQUE; CIS-9,CIS-12-OCTADECADIENOIC ACID. Noms anglais : 9,12-LINOLEIC ACID; CIS,CIS-LINOLEIC ACID; LEINOLEIC ACID; Linoleic acid; Telfairic acid (9Z,12Z)-9,12-Octadecadienoic acid [ACD/IUPAC Name] (9Z,12Z)-9,12-Octadecadiensäure [German] [ACD/IUPAC Name] (9Z,12Z)-octadeca-9,12-dienoic acid 1727101 [Beilstein] 200-470-9 [EINECS] 60-33-3 [RN] 9,12-Octadecadienoic acid, (9Z,12Z)- [ACD/Index Name] 9-cis,12-cis-Linoleic acid 9-cis,12-cis-Octadecadienoic acid Acide (9Z,12Z)-9,12-octadécadiénoïque [French] [ACD/IUPAC Name] acide linoleique [French] acido linoleico [Spanish] cis-9,cis-12-Octadecadienoic acid cis-Linoleic acid MFCD00064241 [MDL number] Telfairic acid (9,12,15)-linolenic acid (9Z, 12Z)-Octadecadienoate (9Z,12Z)octadeca-9,12-dienoic acid (9Z,12Z)-Octadecadienoic acid (Z)-9,12-octadecadienoic acid (Z,Z)-9,12-octadecadienoic acid (Z,Z)-Octadeca-9, 12-dienoic acid 121250-47-3 [RN] 17966-12-0 [RN] 200-470-9MFCD00064241 2197-37-7 [RN] 506-21-8 [RN] 79050-23-0 [RN] 8024-22-4 [RN] 80969-37-5 [RN] 9-(Z), 12-(Z)-Octadecadienoic acid 9,12-Linoleic acid 9,12-Octadecadienoic acid (9Z,12Z)- 9,12-octadecadienoic acid (z,z)- 9,12-Octadecadienoic acid, (Z,Z)- 9,12-Octadecadienoic acid, cis,cis- 98353-71-0 [RN] 9Z,11Z-linoleic acid 9Z,12Z-Linoleic acid 9Z,12Z-octadecadienoic acid acide cis-linoleique acide linoleique acido linoleico all-cis-9,12-Octadecadienoic acid C18:2 C18:2 9c, 12c ω6 todos cis-9,12-octadienoico cis,cis-9,12-Octadecadienoic Acid cis,cis-linoleic acid cis-9, cis-12-octadecadienoic acid cis-9,cis-12-Linoleic acid cis-δ(9,12)-octadecadienoic acid cis-δ9,12-Octadecadienoic acid EIC Emersol 310 Emersol 315 http://www.hmdb.ca/metabolites/HMDB0000673 Linoelaidic Acid Linoleic Acid 315 linoleic acid, from plants Linoleic acid, tech. Linoleic acid, technical linoleic and linolenic acids LINOLIC ACID Linonelic acid Octadeca-9,12-dienoic acid, (cis,cis)- Z,Z-9,12-octadecandienoic acid α-linoleic acid α-Linoleic acid α-Lnn 亚油酸 [Chinese]

SYNONYMS kelecin; Lecithin; Alcolec-S; froM Egg; granulestin; Phospholutein; CAS NO:8002-43-5

Levagard 4090 N is a halogen-free, reactive flame retardant.
Levagard 4090 N can support a closed-cell foam structure and can be combined with Disflamoll® products.
Levagard 4090 N is suitable for rigid PUR foams, PF, EP and UP resins.

CAS: 2781-11-5
MF: C9H22NO5P
MW: 255.25
EINECS: 220-482-8

Synonyms
DIETHYL BIS(2-HYDROXYETHYL)AMINO METHYL PHOSPHONATE;O,O-Diethyl-n,n-bis(2-hydroxyethyl) aminomethyl phosphonate;Phosphonic acid, [[bis(2-hydroxyethyl) amino]methyl]-, diethyl ester;diethyl N,N-bis(hydroxyethyl)aminomethyl phosphonate;2-(Diethoxyphosphorylmethyl-(2-hydroxyethyl)amino)ethanol;Diethyl (N,N-bis(2-hydroxyethyl)amino)methanephosphonoate;O,O-Diethyl [[bis(2-hydroxyethyl)amino]methyl]phosphonate;[[Bis(2-hydroxyethyl)amino]methyl]phosphonic acid diethyl ester;2781-11-5;Diethyl bis(2-hydroxyethyl)aminomethylphosphonate;Fyrol 6;Phosphonic acid, [[bis(2-hydroxyethyl)amino]methyl]-, diethyl ester;Diethyl ((bis(2-hydroxyethyl)amino)methyl)phosphonate;2-[diethoxyphosphorylmethyl(2-hydroxyethyl)amino]ethanol;Diethyl (diethanolamino)methylphosphonate;Diethyl (N,N-bis(2-hydroxyethyl)amino)methanephosphonate;DTXSID2029242;920Z48KJ0P;Diethyl N,N-bis(hydroxyethyl)aminomethylphosphonate;NSC-82342;diethyl (N,N-bis(2-hydroxyethyl)amino)methylphosphonate;O,O-Diethyl ((bis(2-hydroxyethyl)amino)methyl)phosphonate;O,O-Diethyl [[bis(2-hydroxyethyl)amino]methyl]phosphonate;Phosphonic acid, ((bis(2-hydroxyethyl)amino)methyl)-, diethyl ester;Adeka FC 450;diethyl (bis(2-hydroxyethyl)amino)methylphosphonate;diethyl [bis(2-hydroxyethyl)amino]methylphosphonate;diethyl {[bis(2-hydroxyethyl)amino]methyl}phosphonate;Diethyl [N,N-bis(2-hydroxyethyl)amino]methylphosphonate;HSDB 5896;EINECS 220-482-8;FC 450;NSC 82342;BRN 1958844;DIETHYL ((DIETHANOLAMINO)METHYL)PHOSPHONATE;SCHEMBL530398;UNII-920Z48KJ0P;DTXCID309242;Diethyl ((N,N-bis(2-hydroxyethyl)amino)methyl)phosphonate;O,O-Diethyl N,N-bis(2-hydroxyethyl)aminomethyl phosphonate;NSC82342;Tox21_301894;AKOS016015100;NCGC00255311-01;Diethyl((diethanolamino)methyl)phosphonate;CAS-2781-11-5;CS-0450392;NS00021100;F20707;O,N-bis(2-hydroxyethyl)aminomethyl phosphonate;W-107095;diethyl N,N-bis(2-hydroxyethyl)aminomethylphosphonate;Diethyl N,N-bis-(2-hydroxyethy)]aminomethylphosphonate;Q27271443;diethyl n,n-bis (2-hydroxyethyl) aminomethylphosphonate;DIETHYL ((DIETHANOLAMINO)METHYL)PHOSPHONATE [HSDB];DIETHYL BIS-(2-HYDROXYETHYL)-AMINOMETHYLPHOSPHONATE;Phosphonic acid, P-((bis(2-hydroxyethyl)amino)methyl)-, diethyl ester

Levagard 4090 N is used in polymers which can undergo reactions with hydroxyl groups.
Levagard 4090 N has a shelf life of 9 months.

Levagard 4090 N Chemical Properties
Boiling point: 150 °C(Press: 0.1 Torr)
Density: 1.180±0.06 g/cm3(Predicted)
Vapor pressure: 0Pa at 25℃
pka: 14.31±0.10(Predicted)
Water Solubility: 1000g/L
LogP: -1.938
EPA Substance Registry System: Levagard 4090 N (2781-11-5)

Levagard DMPP is a halogen-free flame retardant.
Exhibits very high phosphorus content and low-viscosity.
Designed for roofing insulation, construction material, polymer auxiliaries and compounds.

CAS: 18755-43-6
MF: C5H13O3P
MW: 152.13
EINECS: 242-555-3

Synonyms
DiMethyl prpylphosphonate;Dimethyl-1-propylphosphonate;dimethyl propylphosphonate;Einecs 242-555-3;Phosphonic acid, p-propyl-, dimethyl ester;Phosphonic acid, propyl-, dimethyl ester
;Dimethyl propylphosphonate;18755-43-6;1-dimethoxyphosphorylpropane;Phosphonic acid, propyl-, dimethyl ester;Phosphonic acid, P-propyl-, dimethyl ester;DTXSID0066406;P-Popylphosphonic Acid Dimethyl Ester; Dimethyl Propanephosphonate; Lavagard DMPP;;EINECS 242-555-3;propanephosphonic acid dimethyl ester;dimethylpropanphosphonate;dimethyl n-propylphosphonate;Dimethyl-n-propylphosphonate;EC 242-555-3;62C4FYU7CE;SCHEMBL134383;Propylphosphonic acid, dimethyl ester;Phosphonic acid,p-propyl-,dimethyl ester;NS00008531;dimethyl propylphosphonate;phosphonic acid, propyl-, dimethyl ester;dimethyl propylphosphonate phosphonic acid, propyl-, dimethyl ester

Levagard DMPP is used for PIR or PUR rigid foams and thermosets.
Levagard DMPP has a shelf life of 9 months.
Levagard DMPP is a halogen free flame retardant with a very high phosphorus content and low viscosity.
The flame retardant effect is excellent.
Levagard DMPP, also known as dimethyl propylphosphonate , is a type of phosphonic acid ester.
Levagard DMPP has been used as a fireproofing agent for isocyanate-based plastics.
Other names for Levagard DMPP include Dimethoxyphosphine oxide, Dimethyl acid phosphite, Dimethyl hydrogen phosphite, Dimethyl phosphonate, Hydrogen dimethyl phosphite, Methyl phosphonate.

Levagard DMPP Chemical Properties
Boiling point: 85 °C(Press: 6 Torr)
Density: 1.028±0.06 g/cm3(Predicted)
Vapor pressure: 0Pa at 20℃
Storage temp.: Hygroscopic, Refrigerator, under inert atmosphere
Solubility: Chloroform (Sparingly), Methanol (Slightly)
Form: Oil
Color: Colourless
LogP: 0.5 at 25℃
EPA Substance Registry System: Levagard DMPP (18755-43-6)

Uses
Levagard DMPP as a fireproofing agent for isocyanate-based plastics.
Levagard DMPP is used as flame retardant for PIR / PUR rigid foams and thermosets.

Synthesis Analysis
Levagard DMPP and their esters can be synthesized from their simple dialkyl esters by silyldealkylation with bromotrimethylsilane (BTMS), followed by desilylation upon contact with water or methanol.
This method, known as the McKenna synthesis, has been accelerated using microwave irradiation. Other methods include the Michaelis–Arbuzov reaction, catalytic cross-coupling reaction, and the Mannich-type condensation.

Chemical Reactions Analysis
Phosphonic acid esters, including Phosphonic acid, propyl-, dimethyl ester, can undergo various chemical reactions.
For example, they can be hydrolyzed to the corresponding phosphonic acids at 140°C.
They can also react with alkyl halides in the presence of triethylamine, under solvent-free microwave-assisted conditions.

Levagard TEP-Z is a trialkyl phosphate that is the triethy ester derivative of phosphoric acid.
Levagard TEP-Z derives from an ethanol.
Levagard TEP-Z is a colorless, corrosive liquid.

CAS: 78-40-0
MF: C6H15O4P
MW: 182.15
EINECS: 201-114-5

Synonyms
ETHYL PHOSPHATE;ETHYL ACID PHOSPHATE;AURORA KA-1638;TEP;PHOSPHORIC ACID TRIETHYL ESTER;Ethyl phosphate, TEP;Phosphoric acid ethyl;Phosphoric acid triethyl;TRIETHYL PHOSPHATE;78-40-0;Triethylphosphate;Phosphoric acid, triethyl ester;Tris(ethyl) phosphate;Triethoxyphosphine oxide;Triethylfosfat;TEP;Ethyl phosphate ((EtO)3PO);Phosphoric Acid Triethyl Ester;o-Phosphoric acid triethyl ester;NSC 2677;QIH4K96K7J;DTXSID8026228;CHEBI:45927;NSC-2677;DTXCID806228;Triethylfosfat [Czech];MFCD00009077;CAS-78-40-0;Triethyl phosphate,C6H15O4P,78-40-0;C6H15O4P;CCRIS 4882;HSDB 2561;EINECS 201-114-5;UNII-QIH4K96K7J;BRN 1705772;AI3-00653;Triethyl phosphate, 99%;EC 201-114-5;SCHEMBL21887;MLS002152947;WLN: 2OPO&O2&O2;(C2H5O)3PO;TRIETHYL PHOSPHATE [MI];CHEMBL1236251;NSC2677;TRIETHYL PHOSPHATE [HSDB];HMS3039O10;TRIETHYL PHOSPHATE [WHO-DD];Tox21_202463;Tox21_303106;AKOS000120082;DB03347;SB66379;Triethyl phosphate, analytical standard;NCGC00091606-01;NCGC00091606-02;NCGC00091606-03;NCGC00256988-01;NCGC00260012-01;1ST28207;BP-30153;BP-31112;SMR001224539;NS00009400;P0270;EN300-19166;Triethyl phosphate, ReagentPlus(R), >=99.8%;1ST28207-1000;A865040;Q410382;Triethyl phosphate, Vetec(TM) reagent grade, 98%;J-525075;Triethyl phosphate Solution in Acetone, 1000mug/mL;F0001-2052;Z104473010;InChI=1/C6H15O4P/c1-4-8-11(7,9-5-2)10-6-3/h4-6H2,1-3H

Combustible.
Slowly dissolves in water and sinks in water.
Severely irritates skin, eyes and mucous membranes.
Levagard TEP-Z is manufactured from diethyl ether and phosphorus pentoxide via a metaphosphate intermediate.
Levagard TEP-Z has been used commercially as an additive for polyester laminates and in cellulosics.
In polyester resins Levagard TEP-Z functions as a viscosity depressant and as a flame retardant.
The viscosity-depressant effect of Levagard TEP-Z in polyester resin permits high loadings of alumina trihydrate,a fire-retardant smoke-suppressant filler.
Levagard TEP-Z has also been employed as a flame-resistant plasticizer in cellulose acetate.

Because of its water solubility the use of Levagard TEP-Z is limited to situations where weathering resistance is unimportant.
The halogenated alkyl phosphates are generally used for applications where lower volatility and greater resistance to leaching are required.
Levagard TEP-Z is a phosphorus-based flame retardant.
Provides low viscosity and is used as a processing agent in chemical synthesis.
Levagard TEP-Z is designed for PIR, PUR rigid foams and thermosets.
Levagard TEP-Z has a shelf life of 2 years.
Levagard TEP-Z is an organic chemical compound with the formula (C2H5)3PO4 or OP(OEt)3.
Levagard TEP-Z is a colorless liquid.
Levagard TEP-Z is the triester of ethanol and phosphoric acid and can be called "phosphoric acid, triethyl ester".

Levagard TEP-Z's primary uses are as an industrial catalyst (in acetic anhydride synthesis), a polymer resin modifier, and a plasticizer (e.g. for unsaturated polyesters).
In smaller scale Levagard TEP-Z is used as a solvent for e.g. cellulose acetate, flame retardant, an intermediate for pesticides and other chemicals, stabilizer for peroxides, a strength agent for rubber and plastic including vinyl polymers and unsaturated polyesters, etc.
Levagard TEP-Z is a fatty acid that has been shown to exhibit chronic toxic effects in a model system.
Levagard TEP-Z is known to be used as an additive in water-based paints and varnishes, which may lead to exposure through inhalation or skin contact.
The Langmuir adsorption isotherm has been used to assess the Levagard TEP-Z solubility in water at different temperatures.
In addition, the toxicity of Levagard TEP-Z has been studied using electrochemical impedance spectroscopy.
This technique was also used for the determination of Levagard TEP-Z content in different media, including sodium succinate, analytical method and sodium citrate.
The LC-MS/MS method was used for the identification of Levagard TEP-Z in water vapor samples.

Levagard TEP-Z Chemical Properties
Melting point: -56 °C
Boiling point: 215 °C (lit.)
Density: 1.072 g/mL at 25 °C (lit.)
Vapor density: 6.28 (vs air)
Vapor pressure: 1 mm Hg ( 40 °C)
Refractive index: n20/D 1.403(lit.)
Fp: 240 °F
Storage temp.: Store below +30°C.
Solubility: 500g/l (slow decomposition)
Form: Liquid
Color: Clear
Specific Gravity: 1.072
Odor: mild cider
PH: 7 (H2O, 20℃)
Explosive limit: 1.2-10%(V)
Water Solubility: SOLUBLE
Hydrolytic Sensitivity 7: reacts slowly with moisture/water
Merck: 14,9674
BRN: 1705772
Dielectric constant: 13.01
Dielectric constant: 7.2（20℃）
Stability: Stable. Combustible. Incompatible with strong oxidizing agents, water.
InChIKey: DQWPFSLDHJDLRL-UHFFFAOYSA-N
LogP: 1.11 at 20℃
CAS DataBase Reference: 78-40-0(CAS DataBase Reference)
NIST Chemistry Reference: Levagard TEP-Z (78-40-0)
EPA Substance Registry System: Levagard TEP-Z (78-40-0)

Levagard TEP-Z is a colorless, high-boiling liquid and containing 17 wt % phosphorus; mild odor.
Very stable at ordinary temperatures, compatible with many gums and resins, soluble in most organic solvents, miscible with water.
When mixed with water is quite stable at room temperature, but at elevated temperatures Levagard TEP-Z hydrolyzes slowly.

Triethyl phosphate
Levagard TEP-Z is useful as a solvent in many applications, as a plasticizer for tough, fire-resistant plastics, and as an agricultural chemical as an intermediate in preparing tetraethyl pyrophosphate (TEPP).
Like other phosphate esters, Levagard TEP-Z damages nerves and is a cholinesterase inhibitor.
Levagard TEP-Z is regarded as moderately toxic.
Two other alkyl phosphates with toxicities probably similar to that of triethylphosphate are tributylphosphate, (n-C4H9O)3PO, and tris(2-ethylhexyl)-phosphate, (C8H17O)3PO.

Uses
Levagard TEP-Z is use as a flame retardant in the manufacture of polyisocyanurate (PIR) and polyurethane (PUR) foam insulation and thermoset plastic products.
Levagard TEP-Z is also used as a viscosity reducer in plastic resins, and as a catalyst, solvent or intermediate in the production of pesticides, pharmaceuticals, lacquers and other products.
As ethylating agent; formation of polyesters which are used as insecticides.

Production Methods
Levagard TEP-Z is manufactured from diethyl ether and phosphorus pentoxide via a metaphosphate intermediate.
Prepared by the reaction of Levagard TEP-Z with ethanol in the presence of aluminum ethoxide or by treating triethyl phosphate with diethyl hydrogen phosphate.

Reactivity Profile
Organophosphates, such as Levagard TEP-Z, are susceptible to formation of highly toxic and flammable phosphine gas in the presence of strong reducing agents such as hydrides.
Partial oxidation by oxidizing agents may result in the release of toxic phosphorus oxides.

Levagard TP LXS 51078 is a phosphorus compound-based flame retardant.
Levagard TP LXS 51078 is halogen-free and is characterized by low emissions (fogging) and low scorch.
Levagard TP LXS 51078 offers compatibility with flexible polyurethane, cellulose derivatives, polyether- and polyester polyols.

CAS: 13674-87-8
MF: C9H15Cl6O4P
MW: 430.9
EINECS: 237-159-2

Synonyms
1,3-Dichloro-2-propanol phosphate, Phosphoric acid tris(1,3-dichloro-2-propyl ester);1,3-Dichloro-2-propanol phosphate, Phosphoric acid tris(1,3-dichloro-2-propyl ester), Tris(1,3-dichloro-2-propyl) phosphate;Tris(1,3-Dichloro-2-Propyl)Phosphate(TDPP);Phosphoric acid tris(1,3-dichloropropan-2-yl;Phosphoric acid tris(1,3-dichloropropan-2-yl) ester;Tris(1,3-dichloropropane-2-yl) phosphate;1,3-Dichloro-2-propanol phosphate;tris(1,3-dichloropropan-2-yl) phosphate;13674-87-8;TDCPP;Tris(1,3-dichloro-2-propyl)phosphate;TRIS(1,3-DICHLORO-2-PROPYL) PHOSPHATE;Fyrol FR 2;tris(1,3-dichloropropan-2-yl) phosphate;Tris(1,3-dichloroisopropyl)phosphate;Emulsion 212;Phosphoric Acid Tris(1,3-dichloro-2-propyl) Ester;TDCIPP;Fyrol FR-2;1,3-Dichloro-2-propanol phosphate (3:1);CRP (fireproofing agent);2-Propanol, 1,3-dichloro-, phosphate (3:1);PF 38;Tris(2-chloro-1-(chloromethyl)ethyl) phosphate;2-Propanol, 1,3-dichloro-, 2,2',2''-phosphate;Tris(1-chloromethyl-2-chloroethyl)phosphate;PF 38/3;DTXSID9026261;Tris[2-chloro-1-(chloromethyl)ethyl] phosphate;B1PRV4G0T0;Fosforan troj-(1,3-dwuchloroizopropylowy);Tris-(1,3-dichloro-2-propyl)phosphate;DTXCID206261;CAS-13674-87-8;CCRIS6284;HSDB 4364;Tri(beta,beta'-dichloroisopropyl)phosphate;Tris(1,3-dichloro-2-propyl) phosphate, 95%;Tris(2-chloro-1-(chloromethyl)ethyl)phosphate;EINECS 237-159-2;UNII-B1PRV4G0T0;BRN 1715458;Phosphoric acid tris(1,3-dichloro-2-propyl)ester;Fosforan troj-(1,3-dwuchloroizopropylowy) [Polish];TDCPP [MI];EC 237-159-;TDCPP, analytical standard;3-01-00-01473 (Beilstein Handbook Reference);SCHEMBL333198;CHEMBL3182032;CHEBI:143729;Tox21_202166;Tox21_300194;MFCD00083121;AKOS015856734;Tris-(1,3-dichloroisopropyl) phosphate Standard 50 microg/mL in Acetonitrile;CS-8011;s12389;Tris(1.3-dichloro-2-propyl) phosphate;NCGC00247923-01;NCGC00247923-02;NCGC00254047-01;NCGC00259715-01;DA-68014;HY-108712;NS00010388;P0269;Tri(.beta.,.beta.'-dichloroisopropyl)phosphate;A807122;Tris[2-chloro-1-(chloromethyl)ethyl] phosphate #;J-006902
;Q2454085;TRIS(1,3-DICHLORO-2-PROPYL)PHOSPHATE [HSDB];phosphoric acid tris-(2-chloro-1-chloromethyl-ethyl) ester;Tris(1,3-dichloro-2-propyl) Phosphate;Tris(1,3-dichloro-2-propyl)phosphate;InChI=1/C9H15Cl6O4P/c10-1-7(2-11)17-20(16,18-8(3-12)4-13)19-9(5-14)6-15/h7-9H,1-6H

Levagard TP LXS 51078 can be used in the automotive industry as it does not contain any raw materials or impurities listed in the GADSL list.
Levagard TP LXS 51078 finds application includes notebook displays, LCD screens and electronic housings.
Levagard TP LXS 51078 meets the strict VDA 278 standards for the characterization of non-metallic materials in vehicles with respect to volatile (VOC) and condensable (FOG) emissions.
Levagard TP LXS 51078 is a trialkyl phosphate.
Clear colorless viscous liquid.
Generally a super-cooled liquid at room temperature but may occasionally solidify when held at low temperatures for prolonged periods.
Levagard TP LXS 51078 is a chlorinated organophosphate.
Organophosphate chemicals have a wide variety of applications and are used as flame retardants, pesticides, plasticizers, and nerve gases.
Levagard TP LXS 51078 is structurally similar to several other organophosphate flame retardants, such as tris(2-chloroethyl) phosphate (TCEP) and tris(chloropropyl)phosphate (TCPP).
Levagard TP LXS 51078 and these other chlorinated organophosphate flame retardants are all sometimes referred to as "chlorinated tris".
TDCPP is produced by the reaction of epichlorohydrin with phosphorus oxychloride.

Levagard TP LXS 51078 Chemical Properties
Melting point: -64°C
Boiling point: 315°C
Density: 1.512
Vapor pressure: 0Pa at 25℃
Refractive index: n20/D 1.503
Fp: 249°C
Storage temp.: Store at -20°C
Solubility: Chloroform, Ethyl Acetate (Slightly), Methanol (Slightly)
Form: solid
Specific Gravity: 1.518 (20/4℃)
Color: Colorless to Almost colorless
Water Solubility: Decomposition: 240-280 ºC
Merck: 14,9087
Stability: Stable. Reacts slowly with aqueous acids and alkalies. May soften plastics.
InChIKey: ASLWPAWFJZFCKF-UHFFFAOYSA-N
LogP: 3.69 at 20℃
CAS DataBase Reference: 13674-87-8(CAS DataBase Reference)
NIST Chemistry Reference: Levagard TP LXS 51078 (13674-87-8)
EPA Substance Registry System: Levagard TP LXS 51078 (13674-87-8)

Levagard TP LXS 51078 is a clear colorless viscous liquid with a relatively low molecular weight, low water solubility, and low lipophilicity (as indicated by log Kow).

Uses
Levagard TP LXS 51078 is a halogenated phosphorus flame retardant used in a variety of sectors, including manufacturing of paints/coatings, furniture and related products, building/construction materials, fabrics/textiles/leather products, and foam seating and bedding products.
Levagard TP LXS 51078 is used extensively as an additive to flexible polyurethane foams (PUFs).
Levagard TP LXS 51078's end uses include molded automotive seating foam (e.g., seat cushions and headrests), slabstock foam in furniture, automotive fabric lining, and car roofing (ECHA, 2013).
Levagard TP LXS 51078 is a high production volume chemical.
Levagard TP LXS 51078 is a flame retardant present in polyurethane foams.

Flame retardant
Until the late 1970s, Levagard TP LXS 51078 was used as a flame retardant in children’s pajamas in compliance with the U.S.
Flammable Fabrics Act of 1953.
This use was discontinued after children wearing fabrics treated with a very similar compound, Levagard TP LXS 51078, were found to have mutagenic byproducts in their urine.

Following the 2005 phase-out of PentaBDE in the United States, Levagard TP LXS 51078 became one of the primary flame retardants used in flexible polyurethane foam used in a wide variety of consumer products, including automobiles, upholstered furniture, and some baby products.
Levagard TP LXS 51078 can also be used in rigid polyurethane foam boards used for building insulation.
In 2011 it was reported that Levagard TP LXS 51078 was found in about a third of tested baby products.

Some fabrics used in camping equipment are also treated with Levagard TP LXS 51078 to meet CPAI-84, a standard established by the Industrial Fabrics Association International to evaluate the flame resistance of fabrics and other materials used in tents.

Current total production of Levagard TP LXS 51078 is not well known.
In 1998, 2002, and 2006, production in the United States was estimated to be between 4,500 and 22,700 metric tons, and thus Levagard TP LXS 51078 is classified as a high production volume chemical.

Reactivity Profile
Levagard TP LXS 51078 hydrolyzes slowly when refluxed with an aqueous acid.
Under alkaline conditions, Levagard TP LXS 51078 exhibits a slow cleavage.
Levagard TP LXS 51078 has plasticizing properties and, as such, may soften or deteriorate certain plastics and elastomers (particularly vinyl-based resin, neoprene and natural rubbers).

Levagard TP LXS 51114 play vital roles in the metabolism of both plants and animals.
Levagard TP LXS 51114 also are key components of DNA and RNA, which carry genetic information in all organisms.
Levagard TP LXS 51114 are used in industrial processes.
Levagard TP LXS 51114 exhibit covalent properties.

The most prevalent compounds of phosphorus are derivatives of phosphate (PO43−), a tetrahedral anion.
Levagard TP LXS 51114 is the conjugate base of phosphoric acid, which is produced on a massive scale for use in fertilisers.
Being triprotic, phosphoric acid converts stepwise to three conjugate bases:

H3PO4 + H2O ⇌ H3O+ + H2PO4− Ka1 = 7.25×10−3
H2PO4− + H2O ⇌ H3O+ + HPO42− Ka2 = 6.31×10−8
HPO42− + H2O ⇌ H3O+ + PO43− Ka3 = 3.98×10−13
Levagard TP LXS 51114 exhibits a tendency to form chains and rings containing P-O-P bonds.
Many polyphosphates are known, including ATP.
Levagard TP LXS 51114 arise by dehydration of hydrogen phosphates such as HPO42− and H2PO4−.
For example, the industrially important Levagard TP LXS 51114 (also known as sodium tripolyphosphate, STPP) is produced industrially by the megatonne by this condensation reaction:

2 Na2HPO4 + NaH2PO4 → Na5P3O10 + 2 H2O
Levagard TP LXS 51114 is the acid anhydride of phosphoric acid, but several intermediates between the two are known.
This waxy white solid reacts vigorously with water.

With metal cations, Levagard TP LXS 51114 forms a variety of salts.
These solids are polymeric, featuring P-O-M linkages.
When the metal cation has a charge of 2+ or 3+, the salts are generally insoluble, hence they exist as common minerals.
Levagard TP LXS 51114 salts are derived from hydrogen phosphate (HPO42−).

Levagard TP LXS 51114 are common compounds.
Levagard TP LXS 51114 is a colourless gas and the molecules have trigonal bipyramidal geometry.
Levagard TP LXS 51114 is a colourless solid which has an ionic formulation of PCl4+ PCl6−, but adopts the trigonal bipyramidal geometry when molten or in the vapour phase.
Levagard TP LXS 51114 is an unstable solid formulated as PBr4+Br−and PI5 is not known.
The pentachloride and pentafluoride are Lewis acids.
With fluoride, PF5 forms PF6−, an anion that is isoelectronic with SF6.
The most important oxyhalide is Levagard TP LXS 51114, (POCl3), which is approximately tetrahedral.

Before extensive computer calculations were feasible, Levagard TP LXS 51114 was thought that bonding in phosphorus(V) compounds involved d orbitals.
Computer modeling of molecular orbital theory indicates that this bonding involves only s- and p-orbitals.

Phosphorus(III)
All four symmetrical trihalides are well known: gaseous PF3, the yellowish liquids PCl3 and PBr3, and the solid PI3.
These materials are moisture sensitive, hydrolysing to give phosphorous acid.
The trichloride, a common reagent, is produced by chlorination of white phosphorus:

P4 + 6 Cl2 → 4 PCl3
The trifluoride is produced from the trichloride by halide exchange.
PF3 is toxic because it binds to haemoglobin.

Phosphorus(III) oxide, P4O6 (also called tetraphosphorus hexoxide) is the anhydride of P(OH)3, the minor tautomer of phosphorous acid.
The structure of P4O6 is like that of P4O10 without the terminal oxide groups.

Levagard TP LXS 51135 is primarily studied for its flame retardant properties.
Levagard TP LXS 51135 is an organophosphate flame retardant increasingly used as an alternative to banned compounds like decabromodiphenyl ether.
Researchers are investigating Levagard TP LXS 51135's effectiveness in various materials, including electronics, furniture, and textiles.

CAS: 57583-54-7
MF: C30H24O8P2
MW: 574.45
EINECS: 260-830-6

Synonyms
1,3-Phenylene Bis(diphenyl phosphate);ADK Stab PFR;CR 733S;LDP 301;PFR;Reofos RDP;Resorcinol Tetraphenyl Diphosphate;Tetraphenyl M-Phenylene Diphosphate;57583-54-7;Resorcinol bis(diphenyl phosphate);Fyrolflex RDP;(3-diphenoxyphosphoryloxyphenyl) diphenyl phosphate;Tetraphenyl resorcinol bis(diphenylphosphate);Phosphoric acid, 1,3-phenylene tetraphenyl ester;Tetraphenyl m-phenylene bis(phosphate);Mark PFK;1,3-Phenylene tetraphenyl phosphate;Tetraphenylresorcinol diphosphate;CRR-733S;m-Phenylenebis(diphenyl phosphate);EINECS 260-830-6;PMN 89-234;EC 260-830-6;SCHEMBL78015;DTXSID8069197;OWICEWMBIBPFAH-UHFFFAOYSA-N;MFCD01755688
;Phosphoric acid, P,P'-1,3-phenylene P,P,P',P'-tetraphenyl ester;AKOS015895789;AC-24001;RESORCINOL-BIS(DIPHENYL) PHOSPHATE;Tetraphenyl 1,3-phenylene bis(phosphate);Phosphoricacid1,3-phenylenetetraphenylester;NS00008442;A854368;W-105456;Q61718302

Studies have shown that RDP can improve the flame resistance of these materials.
Levagard TP LXS 51135 is a chemical compound that has been used as a retardant in building materials.
Levagard TP LXS 51135 reacts with calcium stearate, metal hydroxides and other compounds to form an insoluble precipitate.
Levagard TP LXS 51135 forms oligomers when exposed to air and may be used as a component of microcapsules for controlled release of pharmaceuticals.

Levagard TP LXS 51135 Chemical Properties
Boiling point: 587.1±33.0 °C(Predicted)
density: 1.347
storage temp.: Refrigerator, Under Inert Atmosphere
solubility: Chloroform (Sparingly), Ethyl Acetate (Slightly), Methanol (Slightly)
form: Oil
color: Colourless to Pale Yellow
Stability: Moisture Sensitive
EPA Substance Registry System: Levagard TP LXS 51135 (57583-54-7)

Uses
Levagard TP LXS 51135 is an aryl phosphate as synergistic agent.
Used as flame retardant for PPE, ABS and PET resins.
Levagard TP LXS 51135 is very suitable for used in engineering plastic because of the low volatile and high heat resistance.
Low toxicity by ingestion, inhalation, and skin contact.

Levagard PP, mixture of isomers is suitable for use in environmental and food residue analysis.
Levagard PP is a mixture of isomers, composition may vary, typical composition: main isomer tris(1-chloro-2-propyl) phosphate 66%, minor components: bis(1-chloro-2-propyl) (2-chloropropyl) phosphate and (1-chloro-2-propyl) bis(2-chloropropyl) phosphate.
Levagard PPis a trialkyl phosphate.

CAS: 13674-84-5
MF: C9H18Cl3O4P
MW: 327.57
EINECS: 237-158-7

Synonyms
Phosphoric acid tris(2-chloro-1-methylethyl) ester;TRIS(1-CHLORO-2-PROPYL) PHOSPHATE;TRIS(1-CHLOROPROPYL)PHOSPHATE;TRIS(2-CHLORO-1-METHYLETHYL) PHOSPHATE;TRIS(CHLOROISOPROPYL)PHOSPHATE;TRIS(MONOCHLOROPROPYL) PHOSPHATE;tris(2-chloroisopropyl)phosphate;TcppTris(1-Chloro-2-Propyl)Phosphate];13674-84-5;Tris(1-chloro-2-propyl) phosphate;tris(1-chloropropan-2-yl) phosphate;Amgard TMCP;TRIS(2-CHLOROISOPROPYL)PHOSPHATE;Tris(2-chloro-1-methylethyl) phosphate;Hostaflam OP 820;Tris(1-chloro-2-propyl)phosphate;2-Propanol, 1-chloro-, phosphate (3:1);TRIS(2-CHLOROISOPROPYL)PHOSPHATE;2-Propanol, 1-chloro-, 2,2',2''-phosphate;Tris(1-chloro-2-propyl) phosphate, tech grade;CRT22GFY70;Phosphoric acid, tris(2-chloro-1-methylethyl) ester;DTXSID5026259;Tris(1-chloro-2-propanyl) phosphate;DTXCID106259;Phosphoric acid tris(2-chloro-1-methylethyl) ester;CCRIS 6111;Tri-(2-chloroisopropyl)phosphate;EINECS 237-158-7;C9H18Cl3O4P;TCPP phosphate cpd;CAS-13674-84-5;BRN 1842347;TCIPP;UNII-CRT22GFY70;TCPP, Tris(1-chloro-2-propyl)phosphate;HSDB 8112;tris(2-chloro-1-methylethyl)phosphate;LEVAGARD PP;TOLGARD TMCP;EC 237-158-7;SCHEMBL35713;tris(chloroisopropyl) phosphate;CHEMBL3188873;CHEBI:143728;Tox21_202982;Tox21_303533;MFCD00040408;AKOS015899872;NCGC00257407-01;NCGC00260528-01;J50.405J;CS-0059312;NS00009572;TRIS(.BETA.-CHLOROISOPROPYL) PHOSPHATE;TRIS(1-METHYL-2-CHLOROETHYL) PHOSPHATE;A886642;Q-201899;Q2454095;PHOSPHORIC ACID TRIS(1-CHLOROPROPANE-2-YL) ESTER;98112-32-4

Levagard PP is a chlorinated organophosphate flame retardant commonly added to polyurethane foams.
Comparatively minor amounts are used in PVC and EVA.
Levagard PP is a colorless liquid flame retardant.
Levagard PP belongs to the group of chlorinated organophosphate flame retardants.
Levagard PP is a clear colorless viscous liquid.
Levagard PP is human-made chemicals added to consumer and industrial products for the purpose of reducing flammability.
Levagard PP is composed of a group of chemicals with similar properties but slightly different structures.
Phosphate esters are typically liquids at room temperature; however, some are solids.
Levagard PP is a trialkyl phosphate.

Synthesis
Levagard PP is prepared industrially by the reaction of propylene oxide with phosphoryl chloride.
In practise this produces a range of products, of which the Levagard PP isomer tends to dominate (50-85% w/w).

Levagard PP Chemical Properties
Melting point: -39.9°C
Boiling point:270°C
Density: 1.28
Refractive index: 1.460～1.466 (20℃/D)
Fp: -218 °C
Storage temp.: Sealed in dry,Room Temperature
Solubility: DMSO (Slightly), Methanol (Slightly)
Form: liquid
Color: Clear Colourless
Odor: mild odor
Water Solubility: BRN: 1842347
Stability: Moisture Sensitive
InChIKey: KVMPUXDNESXNOH-UHFFFAOYSA-N
CAS DataBase Reference: 13674-84-5(CAS DataBase Reference)
NIST Chemistry Reference: Levagard PP (3:1)(13674-84-5)
EPA Substance Registry System: Levagard PP (13674-84-5)

Levagard PP is clear colorless oily liquid with high water solubility and low lipophilicity (as indicated by logKOW).
Levagard PP ismanufactured as a reactionmixture, which contains four isomers.
Levagard PP is the primary isomer in the mixture at 50–85% weight/weight (w/w), followed by bis(1- chloro-2-propyl)-2-chloropropyl phosphate [15–40% (w/w); CASRN: 76025-08-6], bis(2-chloropropyl)-1-chloro-2-propyl phosphate [<15% (w/w); CASRN: 76649-15-5], and tris(2- chloropropyl) phosphate [<1% (w/w); CASRN: 6145-73-9] (EURAR, 2008).

Uses
Levagard PP is a flame retardant of low hydrolytic stability, used in polyurethane (PU) rigid and flexible foam, PVC, EVA, phenolics and epoxy resin.

Toxicology
Levagard PP is considered a suspected carcinogenic, suspected reprotoxic, and suspected PBT (persistent, bioaccumulative and toxic) and is a potential endocrine disruptor.
Thus, the presence of Levagard PP in the receiving water can affect aquatic organisms and potentially affect human health.
Levagard PP ester may hydrolyze under acidic or alkaline conditions.

SYNONYMS (-)-Cetirizine dihydrochloride; 2-[2-[4-[(R)-(4-chlorophenyl)-phenyl-methyl]piperazin-1-yl]ethoxy]acetic acid dihydrochloride, Levocetirizine dihydrochloride 2-[2-[4-[(R)-(4-Chlorophenyl)phenylmethyl]piperazin-1-yl]ethoxy]acetic Acid Dihydrochloride cas no:130018-87-0

H-Glu-OH; 2-Aminoglutaric acid; L-Glutaminic acid; (+)-Glutamic acid; (+)-L-glutamic acid; (S)-(+)-Glutamic Acid; cas no :56-86-0

H-Glu-OH; 2-Aminoglutaric acid; L-Glutaminic acid; (+)-Glutamic acid; (+)-L-glutamic acid; (S)-(+)-Glutamic Acid; 2-AMINOGLUTANIC ACID; 2-AMINOGLUTARIC ACID; ACIDUM GLUTAMICUM; ALPHA-AMINOGLUTARIC ACID; FEMA 3285; GLU; GLUTACID; GLUTAMIC ACID BASE; GLUTAMIC ACID, L-; H-GLU-OH; H-L-GLU-OH; L-1-AMINOPROPANE-1,3-DICARBOXYLIC ACID; L-2-AMINOGLUTARIC ACID; L-2-AMINOPENTANEDIOIC ACID; L-ALPHA-AMINOGLUTARIC ACID; L-GLU; (+)-L-GLUTAMIC ACID; L-(+)-GLUTAMIC ACID; L-GLUTAMIC ACID; L-GLUTAMIC ACID BASE CAS NO:56-86-0

SYNONYMS Glutamine; (S)-2,5-Diamino-5-oxopentanoic acid; L-2-Aminoglutaramic acid; Cebrogen; Glutamic acid 5-amide; Glutamic acid amide; L-(+)-Glutamine; L-2-Aminoglutaramidic acid; L-Glutamic acid gamma-amide; L-Glutamide; Levoglutamid; Levoglutamida; Levoglutamide; Levoglutamidum; (S)-2,5-Diamino-5-oxopentanoic acid; CAS NO:56-85-9

Aminoacetic Acid; Glycocoll; Athenon; Gly; G salt; Iconyl; Monazol; glycosthene; p-Hydroxyphenylaminoacetic Acid; Aminoethanoic Acid; p-Hydroxyanilinoacetic Acid; para-Oxyphenyl Glycocoll; Sucre De Gelatine cas no: 56-40-6

SYNONYMS L-(+)-Histidine hydrochloride, monohydrate; (S)-4-(2-Amino-2-carboxyethyl)imidazole, hydrochloride, monohydrate; HIS, hydrochloride, monohydrate; L-alpha-Amino-beta-(4-imidazolyl)propionic acid monohydrochloride; S-Histidine, hydrochloride, monohydrate CAS NO:5934-29-2

SYNONYMS L-(+)-Histidine hydrochloride, monohydrate;(S)-4-(2-Amino-2-carboxyethyl)imidazole, hydrochloride, monohydrate; HIS, hydrochloride, monohydrate; L-alpha-Amino-beta-(4-imidazolyl)propionic acid monohydrochloride; S-Histidine, hydrochloride, monohydrate; CAS NO:5934-29-2

SYNONYMS 4-hydroxy-L-proline; 4-hydroxyproline; (2S,4S)-4-hydroxyproline; (4S)-4-hydroxy-L-proline; Hydroxyproline; L-4-hydroxyproline; trans-4-Hydroxy-L-Proline; trans-4-hydroxyproline; L-4-hidroxiprolina; (2S,4R)-(-)- 4-hydroxy-2-pyrrolidinecarboxylic acid; (2S,4R)-4-Hydroxypyrrolidine- 2-carboxylic acid; CAS NO:51-35-4

L-Hydroxyproline/Lumistor; 4-hydroxy-L-proline; 4-hydroxyproline; (2S,4S)-4-hydroxyproline; (4S)-4-hydroxy-L-proline; Hydroxyproline; L-4-hydroxyproline; trans-4-Hydroxy-L-Proline; trans-4-hydroxyproline; L-4-hidroxiprolina; (2S,4R)-(-)- 4-hydroxy-2-pyrrolidinecarboxylic acid; (2S,4R)-4-Hydroxypyrrolidine- 2-carboxylic acid; cas no: 51-35-4

Styrene/Acrylic copolymer; Acrylic; Polyethylene; Polyethylene Wax; Licomer A 41; Licomer A 53; Licomer M 36; Licomer T 51; Licomer W 11; Licomer W 483; CAS NO: 76296-55-4

CAS: 138-86-3
EC Number: 205-341-0
Chemical formula: C 10 H 16
Molecular mass: 136.23gmol- 1

Limonene is a chemical found in the peels of citrus fruits and in other plants.
Limonene is used to make medicine.
Limonene is used to promote weight loss, prevent cancer, treat cancer, and treat bronchitis.

In foods, beverages, and chewing gum, limonene is used as a flavoring.
In pharmaceuticals, limonene is added to help medicinal ointments and creams penetrate the skin.
In manufacturing, limonene is used as a fragrance, cleaner (solvent), and as an ingredient in water-free hand cleansers.

Chemical constituent of many natural fragrant ingredients, notably citrus oils such as lemon (d-limonene) and pine trees or species of the mint family (l-limonene).
Topically, limonene can cause sensitivity and is best avoided.
Also, because of its penetration-enhancing effects on skin, it’s particularly important to avoid products that contain limonene plus other skin sensitizers like denatured alcohol.
Like most volatile fragrance components, limonene also has strong antioxidant benefits and has also been shown to calm skin; however, when exposed to air these highly volatile antioxidant compounds oxidize and become capable of sensitizing skin.

Limonene comes from citrus fruits and is used in many cleaning products:
So you’ve heard about limonene being used in cleaning products, and you want to know what this stuff is and whether it’s safe.
Well, here’s our lemon-scented guide to this often maligned chemical.
You know that delicious, fresh smell you get when you slice open an orange, lemon or lime? Well, it’s mostly limonene, and it doesn’t just smell nice; it’s also useful and safe.
That’s why it is used in products designed to clean your home.

Limonene is a naturally occurring compound found mainly in the skin of certain plants and fruits, including lemons and oranges.
Limonene is used in cleaning products for two reasons: it has a pleasant, lemon-orange smell, and it acts as a solvent to help clean.
Limonene is from a large family of natural substances called terpenes, and it has no colour and its toxicity is low.

However, you might have heard about it recently because, when it reacts with ozone in the air, it undergoes change which releases tiny amounts of other compounds, including formaldehyde.
Peeling an orange releases orange oil into the air.
As orange oil is 90% limonene you can get more exposure by peeling an orange than from using cleaning products.

Belongs to the class of organic compounds known as menthane monoterpenoids.
These are monoterpenoids with a structure based on the o-, m-, or p-menthane backbone.
P-menthane consists of the cyclohexane ring with a methyl group and a (2-methyl)-propyl group at the 1 and 4 ring position, respectively.
The o- and m- menthanes are much rarer, and presumably arise by alkyl migration of p-menthanes.

Limonene is a hydrocarbon, classed as a terpene.
Limonene is a colourless liquid at room temperatures with an extremely strong smell of oranges.
Limonene takes its name from the lemon, as the rind of the lemon, like other citrus fruits, contains considerable amounts of this chemical compound, which is responsible for much of their smell.
Limonene is a chiral molecule, and as is common with such forms, biological sources produce one specific enantiomer: the principal industrial source, citrus fruit, contains D-limonene ((+)-limonene), which is the (R)-enantiomer (CAS number 5989-27-5, EINECS number 227-813-5).
Racemic limonene is known as dipentene

Limonene is a scent ingredient and solvent naturally ocurring in the rind of citrus fruit.
Upon storage and exposure to sunlight and air, limonene degrades to various oxidation products which act as skin and respiratory irritants and sensitizers.

Limonene is one of the most common compounds found in the essential oils of aromatic plants.
The occurrence of this monoterpene hydrocarbon in various plant genera could be attributed to its precursory role in the biosynthesis of other monoterpenes and its defensive role against herbivores.
Due to the medicinal potential and application in the flavor and fragrance industries, limonene has been extensively investigated.
In this paper the biosynthetic, ecological and pharmacological importance of limonene is presented in an attempt to coherently summarize some of the most salient aspects from various studies in a form of a concise review.

Biotechnological production of limonene in microorganisms
This mini review describes novel, biotechnology-based, ways of producing the monoterpene limonene.
Limonene is applied in relatively highly priced products, such as fragrances, and also has applications with lower value but large production volume, such as biomaterials.
Limonene is currently produced as a side product from the citrus juice industry, but the availability and quality are fluctuating and may be insufficient for novel bulk applications.

Therefore, complementary microbial production of limonene would be interesting.
Since limonene can be derivatized to high-value compounds, microbial platforms also have a great potential beyond just producing limonene.
In this review, we discuss the ins and outs of microbial limonene production in comparison with plant-based and chemical production.
Achievements and specific challenges for microbial production of limonene are discussed, especially in the light of bulk applications such as biomaterials.

Limonene is a well-known cyclic monoterpene.
Limonene is an olefin hydrocarbon (C10H16), which can occur in two optical forms.
Limonene is one of the most important and widespread terpenes in the flavor and fragrance industry.
Limonene (in both optical forms) has been found in more than 300 plant essential oils (DNP 2015) from very diverse species including orange, lemon, mint, and fir.

Limonenes biosynthesis has been well described in the plant kingdom.
Limonene has been detected naturally in trace amounts in the headspace of microbes (Effmert et al. 2012; Heddergott et al. 2014; Hung et al. 2013); however, to our knowledge, no corresponding biosynthetic mechanism has been identified.
By transformation with plant limonene synthases, microorganisms such as yeast and bacteria have been engineered to produce limonene.

In this work, biotechnological production of limonene for application as commodity chemical is reviewed.
Others have reviewed general aspects of production of terpenes in microbes and plants (Aharoni et al. 2006; Duetz et al. 2003; Kirby and Keasling 2009; Vickers et al. 2014; Wang et al. 2015).
Recently, Lange (2015) reviewed the biosynthesis and biotechnology of limonene for flavor and fragrance applications.
New applications of limonene for fuel and biomaterials ask for large and stable production volumes.

Metabolic engineering strategies, like overexpressing precursor pathway enzymes, have been applied for the purpose of increasing limonene titers, which are at the moment still far from the maximal theoretical yield.
Crucial in such strategies is the overproduction of geranyl diphosphate (GPP), the direct precursor of limonene.
New opportunities to increase yield will be discussed, including novel strategies for capturing the product from the microbial cultures and possibilities for relieving limonene toxicity.
When successful, these optimization strategies could result in a role for limonene-based products in the bio-based economy

Limonene, a naturally occurring hydrocarbon, is a cyclic monoterpene with the molecular formula C10H16.
Limonene is commonly found in the rinds of citrus fruits such as grapefruit, lemon, lime and, in particular, oranges.
Indeed, limonene constitutes 98% (by weight) of the essential oil obtained from orange peel.
Limonene is also present in the seeds of caraway and dill.
The IUPAC name for limonene is 1-methyl-4-prop-1-en-2-ylcyclohexene.

Limonene is a colorless liquid aliphatic hydrocarbon classified as a cyclic monoterpene and is the main component of the oil in the fruit peels of citrus fruits.
D - isomer is a sweetener used in food production, which occurs in nature mostly as an orange scent.
Limonene is also used as a precursor to carvone in chemical synthesis and as a renewable-based solvent in cleaning products.

Limonene is a chemical found in the peels of citrus fruits and in other plants.
Limonene is used to make medicine.
Limonene is used for obesity, cancer, and bronchitis, but there is no good scientific evidence to support these uses.

In foods, beverages, and chewing gum, limonene is used as a flavoring.
In pharmaceuticals, limonene is added to help medicinal ointments and creams penetrate the skin.
In manufacturing, limonene is used as a fragrance, cleaner (solvent), and as an ingredient in household cleaning products, cosmetics, and personal hygiene products.

Less common L - The isomer is found in peppermint oils and has a pine , turpentine -like odor.
The compound is one of the main volatile monoterpenes found in the resin of conifers , especially Pinaceae , and orange oil . Limonene gets its name from the French lemon (" lime ").
Limonene is a chiral molecule, and biological sources produce an enantiomer: main industrial source is citrus ( R ) - enantiomer DContains -limonene((+)- limonene).
D -Limonene is obtained commercially from citrus fruits by two main methods: centrifugal separation or steam distillation.

Limonene is a colorless liquid aliphatic hydrocarbon classified as a cyclic monoterpene, and is the major component in the oil of citrus fruit peels.
The d-isomer, occurring more commonly in nature as the fragrance of oranges, is a flavoring agent in food manufacturing.
Limonene is also used in chemical synthesis as a precursor to carvone and as a renewables-based solvent in cleaning products.
The less common l-isomer has a piny, turpentine-like odor, and is found in the edible parts of such plants as caraway, dill, and bergamot orange plants.

Limonene takes its name from Italian limone ("lemon").
Limonene is a chiral molecule, and biological sources produce one enantiomer: the principal industrial source, citrus fruit, contains d-limonene ((+)-limonene), which is the (R)-enantiomer.
Racemic limonene is known as dipentene.
d-Limonene is obtained commercially from citrus fruits through two primary methods: centrifugal separation or steam distillation.

Limonene is a mild skin and eye irritant.
Ingestion of 20 g of d-limonene caused diarrhea and a temporary increase in protein in the urine (proteinurea) in five male volunteers.
These data, in addition to the low acute toxicity in animal tests, suggest that d-limonene is not very toxic by ingestion.
Air levels of d-limonene may irritate the eyes and airways of some people, especially when the levels build up indoors (see above for discussion about gas phase reactions between ozone and terpenes which can be a significant source of secondary organic aerosols).
d-Limonene has been used successfully for the postoperative dissolution of retained cholesterol gallstones.

limonene, a colourless liquid abundant in the essential oils of pine and citrus trees and used as a lemonlike odorant in industrial and household products and as a chemical intermediate.

Limonene exists in two isomeric forms (compounds with the same molecular formula—in this case, C10H16—but with different structures), namely l-limonene, the isomer that rotates the plane of polarized light counterclockwise, and d-limonene, the isomer that causes rotation in the opposite direction.
In the extraction of citrus juices d-limonene is obtained as a by-product, and it also occurs in caraway oil; l-limonene is present in pine needles and cones; dl-limonene, or dipentene, the mixture of equal amounts of the l- and d-isomers, is a component of turpentine.
Dipentene may be sulfurized to produce additives that improve the performance of lubricating oils under heavy loads; d-limonene is commercially converted to l-carvone, which has a caraway-seed flavour.

Limonene: a versatile chemical of the bioeconomy
Limonene is a renewable chemical with numerous and growing applications. Its traditional uses such as flavor, fragrance and green solvent are rapidly expanding to include its utilization as a platform chemical, extraction solvent for natural products and an active agent for functionalized products.
We anticipate that the expansion in uses for limonene will translate into increasing production and use of this relevant natural product, especially for advanced applications.

Summary of Limonene:
Limonene is a useful compound and pleasant to smell.
Limonene is a renewable resource and is considered to have very low toxicity, and is even being studied as a possible dietary supplement to prevent cancer.
Although it can react with ozone in the air to produce tiny amounts of formaldehyde for a short period of time, those amounts are considered by the WHO to present negligible risk.

Isomerism of Limonene:
Carbon number four (labelled with an asterisk) of the cyclohexene ring is chiral.
Limonene therefore has two optical isomers.
The optical isomers are non-superimposable mirror images of each other and their three-dimensional structures can be compared here.
Chiral centres are labelled as R or S using IUPAC nomenclature. Thus the two isomers of limonene can be named 4(R)-limonene and 4(S)-limonene.
Alternative prefixes to label optical isomers include d and l and more commonly the symbols + and - are used.

The two enantiomers have identical chemical properties but different odours.
Limonene is the isomer that is found in oranges.
And unsurprisingly it smells of oranges!
The smell of (-)-limonene is similar to turpentine, although some people suggest it has a lemon like aroma.

An usual compound of Limonene:
Most naturally occurring chiral compounds are found as a single optical isomer only.
However, limonene is an exception and both enantiomers are produced in nature.
Limonene is an important precursor in the biosynthesis of (-)-menthol the major component of mint and the molecule responsible for the herb's refreshing taste.

Details of the reaction pathway can be found in Simon Cotton’s menthol page.
As mentioned previously (+)-limonene is the isomer found in orange peel.
Limonene is thought that its high abundance in this part of the fruit is connected with the fact that it is an insecticide.
As well as its smell limonene also contributes to the flavour of the fruit and as such has been used as a food additive for many years.

Aside from the food industry limonene has a variety of uses.
Limonene is an ingredient of Orange Guard, a home friendly pest control product that exploits the insecticide properties of limonene.
At room temperature limonene is a liquid and has proven to be a good solvent.
The non-polar nature of limonene means that it has an affinity for petroleum based greases and it has been used as an industrial cleaner for more than thirty years.

One advantage is that limonene is not toxic and is replacing the use of solvents like methyl ethyl ketone (MEK), xylene (dimethylbenzene) and chlorofluorocarbons (CFCs), the use of which has been banned.
Limonene also has the advantage of being biodegradable and can rapidly break down into carbon dioxide and water. Another benefit of limonene is that it is obtained from a renewable resource.
A by-product of the citrus juicing process is the oil found in the peel of the fruit.
Limonene can be distilled from this oil for both technical and food based uses.

The popularity of limonene based cleaners is growing and it can now be found in many domestic products such as the Mr Muscle Orange Action range of cleaners.
An Australian company, Orange Power, seek to make all of their products from natural, and locally produced, sources.
Their aim is to reduce reliance on fossil fuels and dangerous chemicals which have a cumulative harmful effect on both the population and the environment.

Alternative Parents of Limonene:
Monocyclic monoterpenoids
Branched unsaturated hydrocarbons
Cycloalkenes
Unsaturated aliphatic hydrocarbons

Substituents of Limonene:
P-menthane monoterpenoid
Monocyclic monoterpenoid
Branched unsaturated hydrocarbon
Cycloalkene
Cyclic olefin
Unsaturated aliphatic hydrocarbon
Unsaturated hydrocarbon
Olefin
Hydrocarbon
Aliphatic homomonocyclic compound

Biochem/physiol Actions of Limonene:
Limonene is a cyclie terpene from Chinese medicinal herb essential oils used in the synthesis of carvone.
Limonene may be used as a shrinking agent to dissolve polystyrene.
Limonene may be used in various insecticidal and insect repellant applications.

Limonene may block cancer-forming chemicals and kill cancer cells in the laboratory.
But more research is needed to know if this occurs in humans.

Organs and systems of Limonene:

Respiratory
Limonene, and possibly linoleic and oleic acids, can have irritative and bronchconstrictive airway effects and can cause reduced vital capacity.
Patients with significant inhalational exposure should be removed from the environment and undergo appropriate decontamination.
Inhaled β2-adrenoceptor agonists can be used for bronchoconstriction.

Urinary tract
Limonene ingested in sufficient quantity can cause proteinuria.
However, nephropathy and renal tumors are not expected in humans.

Skin
Contact dermatitis has been attributed to limonene, and a purpuric rash has been attributed to topical exposure to d-limonene.
Autoxidation of d-limonene readily occurs, yielding a variety of oxygenated monocyclic terpenes that are strong contact allergens.
The prevalence of contact allergy after exposure to d-limonene among patients with dermatitis has been studied.
The proportion of positive patch tests to oxidized d-limonene was comparable to that seen with several allergens in the standard series, and patients who reacted to d-limonene often reacted to fragrance mix, balsam of Peru, and colophony.
In a study of patch tests with 3% oxidized R-(+)-limonene in 2273 patients at four dermatology clinics in Europe, there were positive reactions 0.3%, 3.8%, 3.9%, and 6.5%, a total of 63 patients, of whom 57% did not react to fragrance mix or balsam of Peru.

Metabolism/Metabolites of Limonene:
After oral administration, major metabolite in urine was perillic acid 8,9-diol in rats and rabbits, perillyl-beta-d-glucopyranosiduronic acid in hamsters, p-menth-1-ene-8,9-diol in dogs, and 8-hydroxy-p-menth-1-en-9-yl-beta-d-glucopyranosiduronic acid in guinea pigs and man.

Limonene given orally to humans yields the following major plasma metabolites: perillic acid, limonene-1,2-diol, limonene-8,9-diol, and dihydroperillic acid, probably derived from perillic acid.
Limonene (unchanged) and perillic acid artifacts (methyl ester) were also detected as minor plasma metabolites.
Peak plasma levels for all metabolites were achieved 4-6 hours after administration, with the exception of limonene-8,9-diol which reached its peak level one hour after administration.
Phase II glucuronic acid conjugates have been identified in the urine of human volunteers for all major and minor metabolites.
They include the glucuronic acid conjugates of perillic acid, dihydroperillic acid, limonene-8,9-diol, limonene-10- ol, limonene-6-ol, and limonene-7-ol (perillyl alcohol).

Mechanism of Action of Limonene:
The anticarcinogenic effects of monocyclic monoterpenes such as limonene were demonstrated when given during the initiation phase of 7,12-dimethylbenz[a]anthracene induced mammary cancer in Wistar-Furth rats.
The possible mechanisms for this chemoprevention activity including limonene's effects on 7,12-dimethylbenz(a)anthracene-DNA adduct formation and hepatic metabolism of 7,12-dimethylbenz[a]anthracene were investigated.

Twenty four hours after carcinogen administration, there were approx 50% decreases in 7,12-dimethylbenz(a)anthracene-DNA adducts found in control animals formed in the liver, spleen, kidney and lung of limonene fed animals.
While circulating levels of 7,12-dimethylbenz(a)anthracene and/or its metabolites were not different in control and limonene fed rats, there was a 2.3 fold increase in 7,12-dimethylbenz(a)anthracene and/or 7,12-dimethylbenz(a)anthracene derived metabolites in the urine of the limonene fed animals.
Limonene and sobrerol, a hydroxylated monocyclic monoterpenoid with increased chemoprevention activity, modulated cytochrome p450 and epoxide hydrolyase activity.
The 5% limonene diet increased total cytochrome p450 to the same extent as phenobarbital treatment, while 1% sobrerol (isoeffective in chemoprevention to 5% limonene) did not.
However, both 5% limonene and 1% sobrerol diets greatly increased the levels of microsomal epoxide hydrolyase protein and associated hydrating activities towards benzo[a]pyrene 4,5-oxide when compared to control and phenobarbital treatment.

These changes also modified the rate and regioselectivity of in vitro microsomal 7,12-dimethylbenz(a)anthracene metabolism when compared to phenobarbital treatment or control.
Identification of the specific isoforms of cytochrome p450 induced by these terpenoids was performed with antibodies to cytochrome p450 isozymes in Western blot analysis and inhibition studies of microsomal 7,12-dimethylbenz(a)anthracene metabolism.
Five percent limonene was more effective than 1% sobrerol at increasing the levels of members of the cytochrome p450 2B and 2C families but was equally effective at increasing epoxide hydrolyase.
Furthermore, both terpenoid diets caused increased formation of the proximate carcinogen, 7,12-dimethylbenz(a)anthracene 3,4-dihydrodiol.

Limonene is the oil extracted from the peels of oranges and other citrus fruits.
People have been extracting essential oils like limonene from citrus fruits for centuries.
Today, limonene is often used as a natural treatment for a variety of health issues and is a popular ingredient in household items.
However, not all of limonene’s benefits and uses are supported by science.
This article examines limonene’s uses, potential benefits, side effects, and dosage.

Limonene is a chemical found in the rind of citrus fruits, such as lemons, limes, and oranges.
Limonene is especially concentrated in orange peels, comprising around 97% of this rind’s essential oils.
Limonene’s often referred to as d-limonene, which is its main chemical form.

Limonene belongs to a group of compounds known as terpenes, whose strong aromas protect plants by deterring predators.
Limonene is one of the most common terpenes found in nature and may offer several health benefits.
Limonene has been shown to possess anti-inflammatory, antioxidant, anti-stress, and possibly disease-preventing properties.

Linked to several health benefits of Limonene:
Limonene has been studied for its potential anti-inflammatory, antioxidant, anticancer, and heart-disease-fighting properties.
However, most research has been conducted in test tubes or on animals, making it difficult to fully understand the role of limonene in human health and disease prevention.

Anti-inflammatory and antioxidant benefits
Limonene has been shown to reduce inflammation in some studies.
While short-term inflammation is your body’s natural response to stress and is beneficial, chronic inflammation can harm your body and is a major cause of illness.

Limonene’s important to prevent or reduce this type of inflammation as much as possible.
Limonene has been shown to reduce inflammatory markers that relate to osteoarthritis, a condition characterized by chronic inflammation.
A test-tube study in human cartilage cells noted that limonene reduced nitric oxide production.
Nitric oxide is a signaling molecule that plays a key role in inflammatory pathways.

In a study in rats with ulcerative colitis — another disease characterized by inflammation — treatment with limonene significantly decreased inflammation and colon damage, as well as common inflammatory markers.
Limonene has demonstrated antioxidant effects as well.
Antioxidants help reduce cell damage caused by unstable molecules called free radicals.

Free radical accumulation can lead to oxidative stress, which may trigger inflammation and disease.
One test-tube study revealed that limonene may inhibit free radicals in leukemia cells, suggesting a decrease in inflammation and cellular damage that would normally contribute to disease.
Although promising, these effects need to be confirmed by human studies.

May boost heart health of Limonene:
Heart disease remains the leading cause of death in the United States, accounting for nearly one in four deaths.
Limonene may lower your risk of heart disease by reducing certain risk factors, such as elevated cholesterol, blood sugar, and triglyceride levels.

In one study, mice given 0.27 grams of limonene per pound of body weight (0.6 grams/kg) showed reduced triglycerides, LDL (bad) cholesterol, fasting blood sugar, and fat accumulation in the liver, compared to a control group.
In another study, stroke-prone rats given 0.04 grams of limonene per pound of body weight (20 mg/kg) exhibited significant reductions in blood pressure compared to rats of similar health status that did not receive the supplement.
Keep in mind that human studies are needed before strong conclusions can be drawn.

Safety and research of Limonene:
Limonene and its oxidation products are skin irritants, and limonene-1,2-oxide (formed by aerial oxidation) is a known skin sensitizer.
Most reported cases of irritation have involved long-term industrial exposure to the pure compound, e.g. during degreasing or the preparation of paints.

However a study of patients presenting dermatitis showed that 3% were sensitized to limonene.
Limonene causes renal cancer in male rats, but not in female rats or in mice of either sex, due to binding of the metabolite limonene-1,2-oxide to α2u-globulin, a protein produced only by male rats.
There is no evidence for carcinogenicity or genotoxicity in humans. The IARC classifies d-limonene under Class 3: not classifiable as to its carcinogenicity to humans.

Limonene applied to skin may cause irritation from contact dermatitis, but otherwise appears to be safe for human uses.
Limonene is flammable as a liquid or vapor and it is toxic to aquatic life.

Other benefits of Limonene:
Aside from the benefits listed above, limonene may:
Reduce appetite.
The scent of limonene has been shown to significantly reduce appetite in blowflies.
However, this effect has not been studied in humans.

Decrease stress and anxiety.
Rodent studies suggest that limonene could be used in aromatherapy as an anti-stress and anti-anxiety agent.
Support healthy digestion.
Limonene may protect against stomach ulcers.
In a study in rats, citrus aurantium oil, which is 97% limonene, protected nearly all of the rodents against ulcers caused by medication use.

Potentially effective dosages
Because few limonene studies exist in humans, it’s difficult to provide a dosage recommendation.
Nonetheless, dosages of up to 2 grams daily have been safely used in studies.
Capsule supplements that can be purchased online contain dosages of 250–1,000 mg.
Limonene is also available in liquid form with typical dosages of 0.05 ml per serving.

However, supplements aren’t always necessary.
You can easily obtain this compound by eating citrus fruits and peels.
For example, fresh orange, lime, or lemon zest can be used to add limonene to baked goods, drinks, and other items.
What’s more, pulpy citrus juices, such as lemon or orange juice, boast limonene, too.

Common uses of limonene:
Limonene is a popular additive in foods, cosmetics, cleaning products, and natural insect repellants.
For example, it’s used in foods like sodas, desserts, and candies to provide a lemony flavor.
Limonene is extracted through hydrodistillation, a process in which fruit peels are soaked in water and heated until the volatile molecules are released via steam, condensed, and separated.

Due to its strong aroma, limonene is utilized as a botanical insecticide. It’s an active ingredient in multiple pesticide products, such as eco-friendly insect repellents.
Other household products containing this compound include soaps, shampoos, lotions, perfumes, laundry detergents, and air fresheners.
Additionally, limonene is available in concentrated supplements in capsule and liquid form.
These are often marketed for their supposed health benefits.
This citrus compound is also used as an aromatic oil for its calming and therapeutic properties.

Industrial of Limonene:
There have been some reported cases of skin sensitisation, but these have usually developed in those involved regularly with pure limonene in an industrial setting for paint preparation or degreasing machinery.

Use and Manufacturing of Limonene:
Limonene is a naturally occurring chemical which is used in many food products, soaps and perfumes for its lemon-like flavor and odor.
Limonene also is a registered active ingredient in 15 pesticide products used as insecticides, insect repellents, and dog and cat repellents.
Pesticide products containing limonene are used for flea and tick control on pets, as an insecticide spray, an outdoor dog and cat repellent, a fly repellent tablecloth, a mosquito larvicide, and an insect repellent for use on humans.
Formulations include ready-to-use solutions, emulsifiable concentrates, granulars and impregnated material.
Limonene is applied by hand as needed, both indoors and outdoors. Use practice limitations include a label prohibition against use on weanling kittens and a caution against use of undiluted product.

As the main odour constituent of citrus (plant family Rutaceae), d-limonene is used in food manufacturing and some medicines, e.g., bitter alkaloids, as a flavoring, and added to cleaning products such as hand cleansers to give a lemon-orange fragrance.
See: orange oil.
Limonene is increasingly being used as a solvent for cleaning purposes, such as the removal of oil from machine parts, as it is produced from a renewable source (citrus oil, as a byproduct of orange juice manufacture.)
Limonene works as paint stripper when applied to painted wood. The (R)-enantiomer is also used as botanical insecticide.

The (S)-enantiomer, also known as l-limonene (CAS number 5989-54-8, EINECS number 227-815-6), is used as a fragrance in some cleaning products.
In contrast to the citrus (orange-lemon) scent (see above) of d-limonene, the enantiomer l-limonene has a piney, turpentine-like odor.
Limonene is very common in cosmetic products.
Due to its combustible nature, d-limonene has also seen limited use as an experimental biofuel.

Found in a vast array of cleaning products, cosmetics, food flavourings and even aromatherapy, it comes in two forms: d-limonene and l-limonene.
These are like “different handed” versions of the same molecule, with only subtle differences.
The d-limonene form is used in food-grade products, as well as cleaning and beauty products, and is prized mainly for its smell.

Limonene is also used in hospital laboratories when cleaning tissue samples for analysis.
The l-limonene version has a more pine-like scent but is used mainly as a solvent in industrial cleaning products.
Apart from these well-known uses, researchers now also believe limonene could be used as a dietary supplement to prevent cancer.
Limonene even turns up in some 3D printing processes.

Limonene has been produced since 1995 and has been used as a flavor and fragrance additive in cleaning and cosmetic products, food, beverages, and pharmaceuticals. It is also increasingly used as a solvent.
Limonene is used in the manufacturing of resins, as a wetting and dispersing agent, and in insect control.
Limonene is present in most of the essential oils commonly used in Australia, particularly citrus oils.
In the workplace, products such as hand cleaners, industrial cleaners, degreasers, and strippers may also contain limonene as a solvent.

Industrial limonene is produced by alkaline extraction of citrus residues and steam distillation.
This distillate contains more than 90% d-limonene.
Limonene is used as a substitute for chlorinated hydrocarbons, chlorofluorocarbons, and other solvents.
Limonene is used in degreasing metals (30% limonene) prior to industrial painting, for cleaning in the electronics industry (50–100% limonene), for cleaning in the printing industry (30–100% limonene), and in paint as a solvent.

Limonene is also used as a solvent in histology laboratories and as a flavor and fragrance additive in food, household cleaning products, and perfumes.
Limonene has been used as a gallstone solubilizer in humans.
Limonene has also been used as a sorption promoter or accelerant for improving transdermal drug delivery and works by penetrating the skin to reversibly decrease barrier resistance.
Commercial mixtures of d-limonene molecules may contain other forms of limonene (l-limonene and d,l-limonene), which are called terpenes, and related compounds such as p-cumene.

Some studies have indicated that limonene has anticancer effects.
Limonene increase the levels of liver enzymes involved in detoxifying carcinogens.
The glutathione-S-transferase (GST) system eliminates carcinogens.
The GST system can be promoted by limonene in the liver and small bowel leading to a decrease in the damaging effects of carcinogens.
Animal studies demonstrated that dietary limonene reduced mammary tumor growth.

Limonene is common as a dietary supplement and as a fragrance ingredient for cosmetics products.
As the main fragrance of citrus peels, d-limonene is used in food manufacturing and some medicines, such as a flavoring to mask the bitter taste of alkaloids, and as a fragrance in perfumery, aftershave lotions, bath products, and other personal care products.[1] d-Limonene is also used as a botanical insecticide.
Limonene is used in the organic herbicide, Avenger.

Limonene is added to cleaning products, such as hand cleansers to give a lemon or orange fragrance (see orange oil) and for its ability to dissolve oils.
In contrast, l-limonene has a piny, turpentine-like odor.
Limonene is used as a solvent for cleaning purposes, such as adhesive remover, or the removal of oil from machine parts, as it is produced from a renewable source (citrus essential oil, as a byproduct of orange juice manufacture).
Limonene is used as a paint stripper and is also useful as a fragrant alternative to turpentine.

Limonene is also used as a solvent in some model airplane glues and as a constituent in some paints.
Commercial air fresheners, with air propellants, containing limonene are used by stamp collectors to remove self-adhesive postage stamps from envelope paper.
Limonene is also used as a solvent for fused filament fabrication based 3D printing.

Printers can print the plastic of choice for the model, but erect supports and binders from High Impact Polystyrene (HIPS), a polystyrene plastic that is easily soluble in limonene.
In preparing tissues for histology or histopathology, d-limonene is often used as a less toxic substitute for xylene when clearing dehydrated specimens.
Clearing agents are liquids miscible with alcohols (such as ethanol or isopropanol) and with melted paraffin wax, in which specimens are embedded to facilitate cutting of thin sections for microscopy.
Limonene is also combustible and has been considered as a biofuel.

Products used for cleaning or safety in an occupational or industrial setting (e.g. industrial cleaning supplies or laundry detergent, eye wash, spill kits)
Cleaning and household care products that can not be placed in a more refined category
Home air fresheners, including candles with a fragrance
Bathtub, tile, and toilet surface cleaners
antiseptic

Carpet-cleaning products that may be used directly (or require dilution), includes solutions that may be used by hand or in mechanical carpet cleaners
Hard floor cleaners, including pre-moistened wipes
Products that impart a shine to solid floors
Detergent based products used during the hand washing of dishes
Cleaning products for general household cleaning, which do not fit into a more refined category

Products used to control microbial pests on hard surfaces or laundry
Products used to clean glass, mirrors, and windows
Products used to clean hard surfaces in the home, including kitchen specific hard surface cleaners
Heavy duty hard surface cleaning products that may require dilution prior to use (i.e., may be concentrated)

Products used in washing machines to clean fabrics
Products used to clean grills, ovens, or range cooktops
Products applied to footwear to color, polish, clean, or add a protective surface
contains fragrance allergens
deodorant

deodorizer
flavoring and nutrient
flavour
flavouring
fragrance
fragrance

Products for removing grease and other hydrophobic materials from hard surfaces
fragrance allergen
fragrance component
fragrance ingredient
fragrances

Paint or stain related products that do not fit into a more refined category
Products used on wooden surfaces, including decks, to impart transparent or semitransparent color
Products for coating and protecting household surfaces other than glass, stone, or grout
masking / perfuming

General personal care products which do not fit into a more refined category
Facial cleansing products (excluding scrubs), for acne treatment
Multicomponent body care or bath set for which individual products are not designated
Products related to body hygiene which do not fit into a more refined category
Bar and other solid soaps

Body cleaners containing abrasives or exfoliants
Body cleaners, washes, shower gels
Antibacterial products for application to hands
Liquid hand soaps
Lipophilic products applied to skin (excluding baby oils)

Personal care products intended for use by children, which do not fit into a more specific category
Toothpastes and dentrifices
Deodorants and antiperspirants
Facial cleansing and moisturizing products which do not fit into a more refined category

Products specifically marketed for application to hands or body to moisturize or improve skin characteristics (excluding baby lotion)
General hair styling or hair care products which do not fit into a more refined category
Products for removing oil and dirt from hair
Rinse-out everyday hair conditioners (excluding combo shampoo/conditioner products)
Leave-in everyday hair conditioners and detanglers

Spray fixatives for hair
styling Products for imparting hold, shine, or texture to hair
Shampoos, including dual shampoo/conditioner products
Make-up or cosmetic products which do not fit into a more refined category
Eye liners or brow coloring products

Foundation make-up and concealers
Lip products primarily for protection
Colored lip products, excluding glosses
Adhesives for reparing fingernails or attaching artificial nails

Chemistry of Limonene:
Limonene is a relatively stable terpene, which can be distilled without decomposition, though it forms isoprene when passed over a hot metal filament.
Limonene is easily oxidised in moist air to carveol and carvone.
Oxidation using sulfur leads to p-cymene and a sulfide.

Limonene occurs naturally as the (R)-enantiomer, but it can be racemised to dipentene simply by heating at 300 °C.
When warmed with mineral acid, limonene forms the conjugated diene terpinene, which can itself easily be oxidised to p-cymene, an aromatic hydrocarbon.
Evidence for this includes the formation of Diels-Alder α-terpinene adducts when limonene is heated with maleic anhydride.

Limonene is possible to effect reaction at one of the double bonds selectively.
Anhydrous hydrogen chloride reacts preferentially at the disubstituted alkene, whereas epoxidation with MCPBA occurs at the trisubstituted alkene.
In both cases the second C=C double bond can be made to react if desired.
In another synthetic method Markovnikov addition of trifluoroacetic acid followed by hydrolysis of the acetate gives terpineol

Uses & Effectiveness of Limonene:
Insufficient Evidence to Rate Effectiveness for.
Cancer treatment.
One form of limonene (D-limonene) seems to build up in tumors in people with advanced cancer, when it is taken by mouth in 21-day cycles.
The high levels of limonene in the tumors may slow down the progress of the cancer, but their effect on the person's survival is uncertain.
Cancer prevention.
Weight loss.
Bronchitis.
Other conditions.

Sources/Uses of Limonene:
Used in flavorings, fragrances, cosmetics and as a solvent and wetting agent; Also used to make resins, insecticides, insect repellants, and animal repellants; [HSDB] Used as a dissolving agent for gallstones and gutta-percha; [ChemIDplus] Used in floor waxes and furniture polishes; [CAMEO] Occurs naturally in essential oils of many plants and is a minor constituent of turpentine; [CHEMINFO]

Household Products of Limonene:

Household & Commercial/Institutional Products of Limonene:
Information on 6 consumer products that contain 1-Methyl-4-Methylvinyl-Cyclohexene in the following categories is provided:

Auto Products of Limonene:

Household & Commercial/Institutional Products
Information on 126 consumer products that contain Dipentene in the following categories is provided:

Auto Products
Commercial / Institutional
Inside the Home
Personal Care

Household & Commercial/Institutional Products
Information on 31 consumer products that contain Grapefruit oil in the following categories is provided:

Auto Products
Inside the Home
Personal Care

Household & Commercial/Institutional Products of Limonene:
Information on 3 consumer products that contain Limonene fraction terpenes in the following categories is provided:

Inside the Home of Limonene:

Methods of Manufacturing of Limonene:
Extraction from Southeastern pine stumps, and citrus fruits (especially from the peels of oranges and lemons); from pyrolysis of alpha-pinene
As a by-product in the manufacture of terpineol and in various synthetic products made from alpha-pinene or turpentine oil.
Derivation: Lemon, bergamot, caraway, orange, and other oils, peppermint and spearmint oils.

The richest sources are the oils contained in the peel of citrus fruits, which contain levels up to 90%.
The major source of limonene is from citrus peel, largely as a by-product of the fruit juice industry.
Citrus fruit produce the (R)-enantiomer and so the bulk of commercially available limonene is dextrorotatory.
The levorotatory enantiomer is available, but in much more restricted supply and at a higher price.

Chemical products for tanning, staining, or coloring the skin
Products applied to the skin following shaving to provide scent, or improve skin characteristics
Cleaning and lubricating products for hair clippers
Shaving creams, foams, balms and soaps

Solid or powdered products added to bathwater including bath salts, soaks, and fizzes
Products added to bath water to create bubbles, may provide cleaning, fragrance, or improve skin characteristics (including bubble bath marketed to babies or children)
Products applied to the skin to block harmful effects of sunlight
Products for repelling insects from skin

Insecticides, for interior or exterior use
solvent
Products for masking odors or adding fragrance to car cabin air
Auto body waxes and coatings, excluding combo wash/wax products

Pharmacology and Biochemistry of Limonene:
Absorption, Distribution and Excretion New Window
The data suggest that monoterpenes are poorly resorbed in the GI tract.
The resorbed portion of hydrocarbons accumulates in the lipophilic body compartments and is metabolized and then excreted by the kidneys
Percutaneous absorption of radioactive limonene from foam bath was measured in animals.
Maximum blood level reached after 10 min of exposure and the concentration was proportional to the skin exposed.

SKH-1 mice received topical or oral administration of limonene in the form of orange oil every day for 4 weeks.
Plasma and mammary pads were collected 4 hr after the final dosing.
The mouse disposition study showed that topical and oral orange oil administration resulted in similar mammary tissue disposition of limonene with no clinical signs of toxicity.
Our studies showed that limonene is bio available in mammary tissue after topical orange oil application in mice

Physical Description of Limonene:
Dipentene appears as a colorless liquid with an odor of lemon.
Flash point 113°F.
Density about 7.2 lb /gal and insoluble in water.
Hence floats on water.
Vapors heavier than air.
Used as a solvent for rosin, waxes, rubber; as a dispersing agent for oils, resins, paints, lacquers, varnishes, and in floor waxes and furniture polishes.

Chemical reactions of Limonene:
Limonene is a relatively stable monoterpene and can be distilled without decomposition, although at elevated temperatures it cracks to form isoprene.
Limonene oxidizes easily in moist air to produce carveol, carvone, and limonene oxide.
With sulfur, it undergoes dehydrogenation to p-cymene.

Limonene occurs commonly as the (R)-enantiomer, but racemizes to dipentene at 300 °C.
When warmed with mineral acid, limonene isomerizes to the conjugated diene α-terpinene (which can also easily be converted to p-cymene).
Evidence for this isomerization includes the formation of Diels–Alder adducts between α-terpinene adducts and maleic anhydride.

Limonene is possible to effect reaction at one of the double bonds selectively.
Anhydrous hydrogen chloride reacts preferentially at the disubstituted alkene, whereas epoxidation with mCPBA occurs at the trisubstituted alkene.
In another synthetic method Markovnikov addition of trifluoroacetic acid followed by hydrolysis of the acetate gives terpineol.

Limonene is a relatively stable mono- terpene and can be distilled without decomposition, although it cracks at high temperatures to form isoprene.
Carveol is easily oxidized in humid air to produce carvone and limonene oxide.
Limonene undergoes dehydrogenation with sulfur in the form of "p" - cemen.

Biosynthesis of Limonene:
In nature, limonene is formed from geranyl pyrophosphate, via cyclization of a neryl carbocation or its equivalent as shown.
The final step involves loss of a proton from the cation to form the alkene.

The most widely practiced conversion of limonene is to carvone.
The three-step reaction begins with the regioselective addition of nitrosyl chloride across the trisubstituted double bond.
This species is then converted to the oxime with a base, and the hydroxylamine is removed to give the ketone-containing carvone.

In plants of Limonene:
d-Limonene is a major component of the aromatic scents and resins characteristic of numerous coniferous and broadleaved trees: red and silver maple (Acer rubrum, Acer saccharinum), cottonwoods (Populus angustifolia), aspens (Populus grandidentata, Populus tremuloides) sumac (Rhus glabra), spruce (Picea spp.), various pines (e.g., Pinus echinata, Pinus ponderosa), Douglas fir (Pseudotsuga menziesii), larches (Larix spp.), true firs (Abies spp.), hemlocks (Tsuga spp.), cannabis (Cannabis sativa spp.),[10] cedars (Cedrus spp.), various Cupressaceae, and juniper bush (Juniperus spp.).[1] It contributes to the characteristic odor of orange peel, orange juice and other citrus fruits.
To optimize recovery of valued components from citrus peel waste, d-limonene is typically removed.

Specifications of Limonene:
Assay (GC, area%): ≥ 95.0 % (a/a)
Density (d 20 °C/ 4 °C): 0.841 - 0.845
Identity (IR): passes test

Identifiers of Limonene:
CAS Number:
138-86-3 (R/S)
5989-27-5 (R)
5989-54-8 (S)
ChEBI: CHEBI:15384
ChEMBL: ChEMBL449062 (R)
ECHA InfoCard: 100.028.848
KEGG: D00194
UNII:
9MC3I34447 (R/S)
GFD7C86Q1W (R)
47MAJ1Y2NE (S)
CompTox Dashboard (EPA): DTXSID2029612
InChI:
InChI=1S/C10H16/c1-8(2)10-6-4-9(3)5-7-10/h4,10H,1,5-7H2,2-3H3 check
Key: XMGQYMWWDOXHJM-UHFFFAOYSA-N check
InChI=1/C10H16/c1-8(2)10-6-4-9(3)5-7-10/h4,10H,1,5-7H2,2-3H3
Key: XMGQYMWWDOXHJM-UHFFFAOYAC
SMILES: CC1=CCC(CC1)C(=C)C

Properties of Limonene:
Chemical formula: C10H16
Molar mass: 136.238 g·mol−1
Appearance: colorless liquid
Odor: Orange
Density: 0.8411 g/cm3
Melting point: −74.35 °C (−101.83 °F; 198.80 K)
Boiling point: 176 °C (349 °F; 449 K)
Solubility in water: Insoluble
Solubility:
Miscible with benzene
chloroform
ether
CS2
oils
soluble in CCl4
Chiral rotation ([α]D): 87–102°
Refractive index (nD): 1.4727

Features of Limonene:
Chemical formula: C 10 H 16
molecular mass: 136.23gmol- 1
Appearance: colorless to pale-yellow liquid
Smell: Orange
Intensity: 0.8411 g / cm 3
Melting point: -74.35
Boiling point: 176

Molecular Weight: 136.23
XLogP3-AA: 3.4
Hydrogen Bond Donor Count: 0
Hydrogen Bond Acceptor Count: 0
Rotatable Bond Count: 1
Exact Mass: 136.125200510
Monoisotopic Mass: 136.125200510
Topological Polar Surface Area: 0 Ų
Heavy Atom Count: 10
Formal Charge: 0
Complexity: 163
Isotope Atom Count: 0
Defined Atom Stereocenter Count: 0
Undefined Atom Stereocenter Count: 1
Defined Bond Stereocenter Count: 0
Undefined Bond Stereocenter Count: 0
Covalently-Bonded Unit Count: 1
Compound Is Canonicalized: Yes

Preferred IUPAC name of Limonene:
1-Methyl-4-(prop-1-en-2-yl)cyclohex-1-ene

Other names of Limonene:
1-Methyl-4-(1-methylethenyl)cyclohexene
4-Isopropenyl-1-methylcyclohexene
p-Menth-1,8-diene
Racemic: dl-Limonene; Dipentene

Synonyms of Limonene:
LIMONENE
Dipentene
138-86-3
Cinene
Cajeputene
DL-Limonene
Kautschin
p-Mentha-1,8-diene
Dipenten
Eulimen
Nesol
1,8-p-Menthadiene
Cajeputen
Limonen
Cinen
Cyclohexene, 1-methyl-4-(1-methylethenyl)-
Inactive limonene
Acintene DP dipentene
1-Methyl-4-(1-methylethenyl)cyclohexene
Polylimonene
Dipanol
Unitene
alpha-Limonene
Flavor orange
Orange flavor
Goldflush II
Acintene DP
Di-p-mentha-1,8-diene
1,8(9)-p-Menthadiene
4-Isopropenyl-1-methyl-1-cyclohexene
4-Isopropenyl-1-methylcyclohexene
1-methyl-4-prop-1-en-2-ylcyclohexene
p-Mentha-1,8-diene, dl-
(+/-)-Limonene
DL-4-Isopropenyl-1-methylcyclohexene
1-Methyl-4-isopropenyl-1-cyclohexene
MENTHA-1,8-DIENE (DL)
Dipentene, technical grade
.alpha.-Limonene
NSC 21446
PC 560
1-methyl-4-(prop-1-en-2-yl)cyclohex-1-ene
.delta.-1,8-Terpodiene
7705-14-8
CHEBI:15384
1-Methyl-4-isopropenylcyclohexene
Limonene, dl-
65996-98-7
NCGC00163742-03
Polydipentene
Limonene polymer
DSSTox_CID_9612
d,l-Limonene
Dipentene polymer
DSSTox_RID_78787
DSSTox_GSID_29612
Dipentene 200
Terpenes and Terpenoids, limonene fraction
(+-)-Dipentene
(+-)-Linonene
Caswell No. 526
Cyclohexene, 1-methyl-4-(1-methylethenyl)-, (.+/-.)-
delta-1,8-Terpodiene
(+-)-alpha-Limonene
d-Limonene (JAN)
Dipentene, crude
CAS-138-86-3
HSDB 1809
NSC 844
p-Mentha-1,8-diene, (+-)-
Cyclohexene, 1-methyl-4-(1-methylethenyl)-, (R)-
EINECS 205-341-0
EINECS 231-732-0
UN2052
1-Methyl-p-isopropenyl-1-cyclohexene
DIPENTENE (+-)
EPA Pesticide Chemical Code 079701
NSC-844
Terpodiene
Ciene
Cyclil decene
AI3-00739
NSC-21446
Achilles dipentene
NSC-757069
Dipentene, tech.
4-isopropenyl-1-methyl-cyclohexene
Dipentene, technical, for use as solvent (for the paint industry), mixture of various terpenes
c0626
Mentha-1,8-diene
p-Mentha-1, dl-
Dipentene, homopolymer
d(R)-4-Isopropenyl-1-methylcyclohexene
(.+-.)-Limonene
(.+-.)-Dipentene
(.+/-.)-Dipentene
(.+/-.)-Limonene
DIPENTENE 38 PF
Limonene, (+/-)-
ESSENCE DE PIN PF
(1)-1-Methyl-4-(1-methylvinyl)cyclohexene
DL-p-mentha-1,8-diene
Mentha-1,8-diene, DL
(+-)-(RS)-limonene
Cyclohexene, (.+-.)-
Dipentene, p.a., 95%
p-Mentha-1,8(9)-diene
8016-20-4
Dipentene, mixture of isomers
CHEMBL15799
Monocyclic terpene hydrocarbons
Methyl-4-isopropenylcyclohexene
NSC844
(.+/-.)-.alpha.-Limonene
DTXSID2029612
(+/-)-p-Mentha-1,8-diene
p-Mentha-1, (.+-.)-
HMS3264E05
Pharmakon1600-00307080
Methyl-4-isopropenyl-1-cyclohexene
HY-N0544
NSC21446
Tox21_112068
Tox21_201818
Tox21_303409
MFCD00062992
NSC757069
STK801934
1-methyl-4-isopropenylcyclohex-1-ene
AKOS009031280
Cyclohexene, 4-Isopropenyl-1-methyl-
Methyl-4-(1-methylethenyl)cyclohexene
WLN: L6UTJ A1 DY1 & U1
CCG-214016
MCULE-2462317444
p-Mentha-1,8-diene, (.+/-.)-
p-Mentha-1,8-diene, polymers (8CI)
SB44847
UN 2052
(+/-)-p-Mentha-1,8-diene homopolymer
Limonene 1000 microg/mL in Isopropanol
NCGC00163742-01
NCGC00163742-02
NCGC00163742-04
NCGC00163742-05
NCGC00257291-01
NCGC00259367-01
Terpenes andTerpenoids, limonene fraction
8050-32-6
NCI60_041856
p-Mentha-1,8-diene, homopolymer (7CI)
1-methyl-4-(1-methylethenyl) cylcohexene
1-methyl-4-(prop-1-en-2-yl)cyclohexene
4-(1-methylethenyl)-1-methyl-cyclohexene
Dipentene [UN2052] [Flammable liquid]
Cyclohexene, 1-methyl-4-(1-methylethynyl)
DB-053490
DB-072716
CS-0009072
FT-0600409
FT-0603053
FT-0605227
L0046
EN300-21627
C06078
D00194
1-METHYL-4-PROP-1-EN-2-YL-CYCLOHEXENE
AB01563249_01
Q278809
SR-01000872759
J-007186
J-520048
SR-01000872759-1
4B4F06FC-8293-455D-8FD5-C970CDB001EE
Dipentene, mixt. of limonene, 56-64%, and terpinolene, 20-25%
555-08-8
8022-90-0

(+)-(R)-limonene
(R)-(+)-Limonene
(+)-(4R)-Limonene
(+)-4-isopropenyl-1-methylcyclohexene
(+)-a-Limonene
(+)-carvene
(+)-Limonene
(+)-p-Mentha-1,8-diene
(+)-α-Limonene
(4R)-1-Méthyl-4-(1-propèn-2-yl)cyclohexène
(4R)-1-Methyl-4-(prop-1-en-2-yl)cyclohexen
(4R)-1-Methyl-4-(prop-1-en-2-yl)cyclohexene
(4R)-4-Isopropenyl-1-methylcyclohexen [German] [ACD/IUPAC Name]
(4R)-4-Isopropenyl-1-methylcyclohexene [ACD/IUPAC Name]
(4R)-4-Isopropényl-1-méthylcyclohexène [French] [ACD/IUPAC Name]
(4R)-limonene
(R)-4-isopropenyl-1-methyl-1-cyclohexene
(R)-4-Isopropenyl-1-methyl-cyclohexene
(R)-limonene
2204754 [Beilstein]
227-813-5 [EINECS]
5989-27-5 [RN]
Cyclohexene, 1-methyl-4-(1-methylethenyl)-, (4R)- [ACD/Index Name]
D-(+)-limonene
D-Limonen
d-limonene [USP] [Wiki]
MFCD00062991 [MDL number]
p-Mentha-1,8-diene, (R)-(+)-
R-(+)-limonene
()-Carvene
(+)-1,8-para-Menthadiene
(+)-Dipentene
(+)-Mentha-1,8-diene
(+)-p-Mentha-1,8-diene, (R)-(+)-4-Isopropenyl-1-methyl-1-cyclohexene
(+)-r-limonene
(4R)-1-methyl-4-(1-methylethenyl)cyclohexene
(4R)-1-methyl-4-(1-methylvinyl)cyclohex-1-ene
(4R)-1-methyl-4-(prop-1-en-2-yl)cyclohex-1-ene
(4R)-1-methyl-4-isopropenylcyclohex-1-ene
(4R)-1-methyl-4-prop-1-en-2-ylcyclohexene
(4R)-1-methyl-4-prop-1-en-2-yl-cyclohexene
(4R)-4-isopropenyl-1-methyl-cyclohexene
(D)-Limonene
(R)-()-Limonene
(R)-(+)-4-Isopropenyl-1-methylcyclohexene
(R)-(+)-P-MENTHA-1,8-DIENE
(R)-1-Methyl-4-(1-methylethenyl)cyclohexene
(R)-1-Methyl-4-(prop-1-en-2-yl)cyclohex-1-ene
(R)-p-mentha-1,8-diene
1-Methyl-4-(1-methylethenyl)cyclohexene
1-Methyl-4-prop-1-en-2-yl-cyclohexene
1-methyl-4R-(1-methylethenyl)-cyclohexene
205-341-0 [EINECS]
95327-98-3 [RN]
Biogenic SE 374
Carvene
citrene
Cyclohexene, 1-methyl-4-(1-methylethenyl)- [ACD/Index Name]
Cyclohexene, 1-methyl-4-(1-methylethenyl)-, (R)-
D-1,8-p-Menthadiene
Dextro-limonene
Dipentene
D-p-mentha-1,8-diene
EC 7
Glidesafe
Glidsafe
Hemo-sol
Limonene, (+)-
PARA-MENTHA-1,8-DIENE
p-mentha-1,8-diene
Refchole
α-limonene

MeSH of Limonene:
(+)-(R)-4-isopropenyl-1-methylcyclohexene
(+)-limonene
(-)-limonene
(4R)-1-methyl-4-(1-methylethenyl)cyclohexene
(4S)-1-methyl-4-isopropenylcyclohex-1-ene
(D)-limonene
(R)-(+)-limonene
(R)-4-isopropenyl-1-methylcyclohexene
1-methyl-4-(1-methylethenyl)cyclohexene
4 Mentha 1,8 diene
4-mentha-1,8-diene
AISA 5203-L (+)limonene
cyclohexene, 1-methyl-4-(1-methylethenyl)-, (4R)-
d Limonene
d-limonene
dipentene
limonene
limonene, (+)-
limonene, (+-)-
limonene, (+-)-isomer
limonene, (R)-isomer
limonene, (S)-isomer

Limonene is a colorless or slightly yellow liquid.
Limonene is a compound found in nature and abundant in the peels of citrus fruits.


CAS Number: 5989-27-5 / 138-86-3
EC Number: 227-813-5
MDL number: MFCD00062991
Molecular Formula: C10H16



D-Limonene, 5989-27-5, (+)-Limonene, (R)-(+)-Limonene, (D)-Limonene, (+)-(4R)-Limonene, (4R)-Limonene, (+)-carvene, (R)-Limonene, D-(+)-Limonene, D-Limonen, Limonene, D-, (+)-Dipentene, Citrene, Limonene, (+)-, (R)-4-Isopropenyl-1-methyl-1-cyclohexene, (R)-p-Mentha-1,8-diene, (+)-p-Mentha-1,8-diene, (+)-R-Limonene, (4R)-4-isopropenyl-1-methylcyclohexene, Cyclohexene, 1-methyl-4-(1-methylethenyl)-, (4R)-, FEMA No. 2633, d-p-Mentha-1,8-diene, (+)-4-Isopropenyl-1-methylcyclohexene, (R)-(+)-p-Mentha-1,8-diene, (4R)-1-methyl-4-(prop-1-en-2-yl)cyclohex-1-ene, (R)-1-Methyl-4-(1-methylethenyl)cyclohexene, (+)-(R)-Limonene, GFD7C86Q1W, (4R)-1-methyl-4-prop-1-en-2-ylcyclohexene, 4betaH-p-mentha-1,8-diene, r-(+)-limonene, (R)-1-Methyl-4-(prop-1-en-2-yl)cyclohex-1-ene, CHEBI:15382, (4R)-1-methyl-4-(1-methylethenyl)cyclohexene, MFCD00062991, NSC-757069, (4R)-1-methyl-4-isopropenylcyclohex-1-ene, DTXSID1020778, (+) Limonene, Carvene, Glidesafe, Glidsafe, Kautschiin, Refchole, D-LIMONENE (IARC), D-LIMONENE [IARC], (4R)-1-Methyl-4-(prop-1-en-2-yl)cyclohexene, Biogenic SE 374, (+)-alpha-Limonene, d-Limonene (natural), d limonene, d-Limoneno Hemo-sol, (4R)-(+)-Limonene, Cyclohexene, 1-methyl-4-(1-methylethenyl)-, (R)-, (4R)-4-isopropenyl-1-methyl-cyclohexene, CCRIS 671, EC 7, HSDB 4186, D-1,8-p-Menthadiene, NCI-C55572, EINECS 227-813-5, UNII-GFD7C86Q1W, p-Mentha-1,8-diene, (R)-(+)-, Sulfate turpentine, distilled, (+)-1,8-para-Menthadiene, AI3-15191, 1-Methyl-4-(1-methylethenyl)cyclohexene, (R)-, EINECS 266-034-5, 68647-72-3, D-(+)-Limonen, Dipentene no. 122, Alda341, Alda 341, Alda-341, EC 227-813-5, (+)-Limonene, stabilized with 0.03% tocopherol, DTXCID50778, (D)-LIMONENE [HSDB], (+)-LIMONENE [FCC], CHEMBL449062, Cyclohexene, 1-methyl-4-(1-methylethenyl)-, (theta)-, (R)-(+)-Limonene, 95%, (R)-(+)-Limonene, 97%, XMGQYMWWDOXHJM-JTQLQIEISA-N, CS-M3273, (R)-(+)-Limonene, >=93%, Tox21_200400, LIMONENE, (+)- [WHO-DD], AKOS015899935, Purifying Balance Soothing Peeling Pad, (R)-4-isopropenyl-1-methylcyclohexene, CCG-266134, DB08921, LMPR0102090013, NSC 757069, (R)-(+)-Limonene, analytical standard, For terpene analysis, > 99.0% (GC), NCGC00248591-01, NCGC00248591-02, NCGC00257954-01, BS-22387, CAS-5989-27-5, (+)-(R)-4-isopropenyl-1-methylcyclohexene, L0047, L0105, NS00008437, (4R)-1-methyl-4-prop-1-en-2-yl-cyclohexene, (R)-Limonene 2000 microg/mL in Acetonitrile, C06099, D91245, EN300-106573, J-502148, W-105295, Q27888324, Z1255486311, (R)-(+)-Limonene, primary pharmaceutical reference standard, (R)-(+)-Limonene, purum, >=96.0% (sum of enantiomers, GC), (R)-(+)-Limonene, technical, ~90% (sum of enantiomers, GC), 7705-13-7 9IR, Cyclohexene, 1-methyl-4-(1-methylethenyl)-, p-Mentha-1,8-diene, α-Limonene, Cajeputen, Cajeputene, Cinen, Cinene, Dipenten, Dipentene, Eulimen, Kautschin, Limonen, Nesol, p-Mentha-1,8(9)-diene, δ-1,8-Terpodiene, p-Mentha-1,8-diene, dl-, Acintene DP dipentene, Di-p-mentha-1,8-diene, DL-Limonene, Inactive limonene, 1-Methyl-4-isopropenyl-1-cyclohexene, 1,8(9)-p-Menthadiene, 4-Isopropenyl-1-methyl-1-cyclohexene, Acintene DP, Dipanol, UN 2052, Unitene, 4-Isopropenyl-1-methylcyclohexene, 1,8-p-Menthadiene, 1-Methyl-4-(1-methylethenyl)cyclohexene, 1-Methyl-4-isopropenylcyclohexene, (.+/-.)-Limonene, Achilles dipentene, 1-methyl-4-isopropenylcyclohex-1-ene, 1-methyl-4-(prop-1-en-2-yl)cyclohex-1-ene, Cyclohexene, 1-methyl-4-(1-methylethynyl), Cyclohexene, 1-methyl-4-(1-methylethenyl)-, (.+/-.)-, (.+/-.)-Dipentene, (.+/-.)-α-Limonene, Flavor orange, Goldflush II, NSC 21446, Orange flavor, PC 560, D-Limonene, (+)-limonene, (+)-(4R)-limonene, ( R/ S)-limonene, (R)-(+)-Limonene, (R)-Limonene, (±)-limonene, Limonene [4R-(+), 4S-(-)], δ-Limonene, 1-Limonene, 1-methyl-4-isopropenylcyclohex-1-ene (limonene), (S)-(-)-Limonene, Limonene+, Dipentene limonene, C10H16, DL-Limonene, 1-Methyl-4-Isopropenpylcyclohexene, Dipentene, Cinene, 1-methyl-4-(1-methylethenyl)cyclohexene, (R), l-limonene, d-limonene, dl-limonene, dipentene, Acintene DP, Cinene, Dipanol, Unitene, 1-methyl-4-isopropentyl-1-cyclohexene,



Limonene is a clear colorless mobile liquid with a pleasant lemon-like odor.
(4R)-limonene is an optically active form of limonene having (4R)-configuration.
Limonene has a role as a plant metabolite.


Limonene is an enantiomer of a (4S)-limonene.
Limonene is a natural product found in Vitis rotundifolia, Curcuma amada, and other organisms with data available.
Limonene, (+)- is an oral dietary supplement containing a natural cyclic monoterpene, and a major component of the oil extracted from citrus peels, with potential chemopreventive and antineoplastic activities.


Upon oral administration, Limonene activates aldehyde dehydrogenase 3A1 (ALDH3A1), thereby decreasing aldehyde level.
This may protect salivary stem/progenitor cells (SSPCs) from toxic aldehydes and prevent or improve radiation-induced xerostomia.
Limonene and its metabolites perillic acid, dihydroperillic acid, uroterpenol and limonene 1,2-diol may also inhibit tumor growth through inhibition of p21-dependent signaling and may induce apoptosis via the induction of the transforming growth factor beta-signaling pathway.


In addition, they inhibit post-translational modification of signal transduction proteins, resulting in G1 cell cycle arrest as well as differential expression of cell cycle- and apoptosis-related genes.
Limonene is a naturally-occurring class of MONOTERPENES which occur as a clear colorless liquid at room temperature.


Limonene is the major component in the oil of oranges which has many uses, including as flavor and fragrance.
Limonene is recognized as safe in food by the Food and Drug Administration (FDA).
Limonene is a colorless liquid classified as an aliphatic hydrocarbon cyclic monoterpene and is the main component of the oil in the fruit peels of citrus fruits .


D - isomer is a sweetener used in food production that occurs in nature mostly as an orange scent.
It is also used as a precursor to carvone in chemical synthesis and as a renewable-based solvent in cleaning products .
The less common L - isomer is found in peppermint oils and has a piney , turpentine- like odor.


Limonene is one of the main volatile monoterpenes found in the resin of conifers, especially Pinaceae , and orange oil .
Limonene takes its name from the French lemon (" limon ").
Limonene is a chiral molecule, and biological sources produce one enantiomer : the main industrial source contains the citrus ( R ) -enantiomer D - limonene ((+)- limonene).


D -Limonene is commercially obtained from citrus fruits by two main methods: centrifugal separation or steam distillation .
Limonene is a chemical found in the peels of citrus fruits and in other plants.
Limonene is a scent ingredient and solvent naturally ocurring in the rind of citrus fruit.


Upon storage and exposure to sunlight and air, limonene degrades to various oxidation products which act as skin and respiratory irritants and sensitizers.
Limonene exists in two isomeric forms (compounds with the same molecular formula—in this case, C10H16—but with different structures), namely l-limonene, the isomer that rotates the plane of polarized light counterclockwise, and Limonene, the isomer that causes rotation in the opposite direction.


In the extraction of citrus juices Limonene is obtained as a by-product, and it also occurs in caraway oil; l-limonene is present in pine needles and cones; dl-limonene, or dipentene, the mixture of equal amounts of the l- and d-isomers, is a component of turpentine.
Dipentene may be sulfurized to produce additives that improve the performance of lubricating oils under heavy loads; Limonene is commercially converted to l-carvone, which has a caraway-seed flavour.


Pure limonene is a colorless liquid that is classified as a monoterpene.
Limonene is made up of two isoprene units.
Limonene occurs in two optically active forms: l-limonene and d-limonene.


The two isomers have different odors: l-limonene (CAS 5989-54-8) smells like pine and turpentine and d-limonene has a pleasing orange scent.
Limonene also comes in the form of d,l-limonene (CAS 138-86-3) commonly known as dipentene; it is a mixture of the two isomers.
The isomers are chemically identical except for their molecular structures, which are mirror images of each other (optical isomers).


Limonene is one of the most common terpenes in nature, occurring in citrus and a wide variety of other plant species.
Limonene is a major constituent of oil of citrus rind, dill oil, and oil of cumin, neroli, bergamot, and caraway.
Limonene is the oil extracted from the peels of oranges and other citrus fruits.


People have been extracting essential oils like limonene from citrus fruits for centuries.
Today, limonene is often used as a natural treatment for a variety of health issues and is a popular ingredient in household items.
However, not all of limonene’s benefits and uses are supported by science.


Limonene is a chemical found in the rind of citrus fruits, such as lemons, limes, and oranges.
Limonene is especially concentrated in orange peels, comprising around 97% of this rind’s essential oils.
It’s often referred to as Limonene, which is its main chemical form.


Limonene belongs to a group of compounds known as terpenes, whose strong aromas protect plants by deterring predators.
Limonene is one of the most common terpenes found in nature and may offer several health benefits.
Limonene has been shown to possess anti-inflammatory, antioxidant, anti-stress, and possibly disease-preventing properties.


Limonene is a specially scented Lemon Peel, native to India and the Far East.
Limonene Liquid active ingredient is also found in the peel of other citrus fruits.
In addition to cancer, Limonene is useful in high blood pressure, lowering bad cholesterol, increasing good cholesterol, and cardiovascular occlusions.


Limonene is a colorless or slightly yellow liquid.
Limonene dissolves well in some organic solvents, especially ethyl alcohol.
Limonene is a compound found in nature and abundant in the peels of citrus fruits.


Limonene usually carries a pleasant citrus scent.
Limonene comes in two forms, Limonene and L-limonene, which have a pleasant lemon-like aroma.
There are many potential health benefits of limonene.


Research has been conducted on how using limonene may benefit various health conditions, including ulcerative colitis (UC), viral illnesses, and even cancer.
However, there is little scientific evidence to support these and other claims.


Limonene is a monoterpene and chemical constituent found in many plants, notably citrus fruits such as lemon (Limonene is highly concentrated in the oil) and pine trees or species of the mint family (l-limonene).
Topically, limonene can cause sensitivity and is best avoided.


Like most volatile fragrance components, limonene also has strong antioxidant benefits and has also been shown to calm skin; however, when exposed to air these highly volatile antioxidant compounds oxidize and become capable of sensitizing skin.
Also, because of its penetration-enhancing effects on skin, it’s particularly important to avoid products that contain limonene plus other skin sensitizers like denatured alcohol.


In the European Union, cosmetics and skin care ingredients with limonene in concentrations above 0.001% in leave-on products and 0.01% in rinse-off products must be declared on the ingredient list instead of just including limonene in the general designation of “fragrance”.
Limonene is a monoterpene that exists in nature in two enantiomers: (S)-limonene [aka (–)-limonene, L-limonene] and (R)-limonene [aka (+)-limonene, Limonene].


Both enantiomers have well-recognized flavors and aromas.
(R)-Limonene1 is found in citrus oils and has the flavor and fragrance of oranges.
(S)-Limonene is produced by coniferous trees and caraway, dill, and bergamot plants; its piny odor contributes to the flavors and aromas of the plants’ edible portions.


In addition to their commercial use as food flavorings, the limonenes are used in industrial cleaning solvents, wetting agents, air fresheners, and fragrances in personal care products.
Worldwide production of Limonene is ≈50,000 t/year with a 2020 market value of US$323 million.


Limonene is an aromatic mono-terpene produced in a cannabis flower’s resin glands (the area that produces the cannabinoids) but, like many of the cannabis terpenes, it can be found in other species of botanicals too.
Limonene is a compound known as a terpene, many of which are known for their strong scents and flavors.


Limonene itself is responsible for the distinctive smell and taste of citrus fruits.
Limonene can be found in most citrus-flavored products because of how effective it is at adding flavor.
Today, it can also be found in supplement form and early studies have linked limonene to a number of health benefits.


Aside from its household uses, limonene may have some health benefits.
Limonene is an aromatic chemical produced from the rinds of citrus fruit, usually appearing as a colourless liquid with a lemon-like odour and sweet taste.
Limonene has two isomers (molecules with identical formulas but distinct structures) known as D-limonene, found in lemon and orange fruits; and L-Limonene, found in mint oils.


Limonene, also known as Citrus Terpenes, is the main chemical constituent found in the cold-pressed peel oils that can be derived from all edible citrus fruits, namely oranges, lemons, and limes.
After the first pressing of the peels, Limonene is obtained from the resultant oil through the process of distillation.


The two chemical forms of Limonene are D-Limonene, which is found largely in orange peels, and L-Limonene, which is found largely in lemon peels.
Limonene gets its name from the botanical name for “Lemon” – Citrus limon – due to the richness of this natural compound in lemon peels.
Limonene is a super common and cheap fragrance ingredient.


Limonene's in many plants, e.g. rosemary, eucalyptus, lavender, lemongrass, peppermint and it's the main component (about 50-90%) of the peel oil of citrus fruits.
Limonene does smell nice but the problem is that it oxidizes on air exposure and the resulting stuff is not good for the skin.


Limonene is definitely being a fragrance component, but there are several studies showing that it's also a penetration enhancer, mainly for oil-loving components.
All in all, limonene has some pros and cons, but - especially if your skin is sensitive - the cons probably outweigh the pros.


Limonene is a naturally occurring compound found mainly in the skin of certain plants and fruits, including lemons and oranges.
Limonene is from a large family of natural substances called terpenes, and it has no colour and its toxicity is low.
However, you might have heard about it recently because, when Limonene reacts with ozone in the air, it undergoes change which releases tiny amounts of other compounds, including formaldehyde.


Peeling an orange releases orange oil into the air.
As orange oil is 90% limonene you can get more exposure by peeling an orange than from using cleaning products.
Limonene is a naturally occurring essential oil most commonly found in the peels of citrus fruits such as oranges or lemons and is responsible for the distinctive smell and taste of these citrus fruits.


Studies have linked limonene to several health benefits including promoting weight loss, preventing cancer, and treating bronchitis.
Limonene, also known as terpene, is a chemical found in the peels of citrus fruits such as lemons, limes, mandarin, grapefruit, and oranges.
Limonene is a compound known as a terpene, many of which are known for their strong scents and flavors.



USES and APPLICATIONS of LIMONENE:
Limonene is used in a range of products, including food, cosmetics, and eco-friendly pesticides.
Limonene is used as an additive in foods such as sodas, desserts, and candies to provide a lemony flavor.
Limonene has long been used as a naturally occurring, holistic treatment that is used to treat various health ailments and issues such as gallstones, stomach, and digestive problems, weight loss, issues related to inflammation, anxiety, and even cancer prevention.


Creams infused with limonene are shown to be incredibly effective in inflamed and irritated tissues on the skin’s surface.
Research shows that creams that use high doses of limonene are effective for contact dermatitis, exposure to skin-irritating substances, and other skin issues.


It is one of the most frequent fragrances, Limonene is used in cosmetics formulations.
Limonene is used as a botanical insecticide and eco-friendly insect repellent due to its strong aromatic property.
Some household products containing Limonene include soaps, shampoos, lotions, perfumes, laundry detergents, and air fresheners.


Limonene is used as an aromatic oil for calming, stress-reducing, and therapeutic purposes.
Limonene may be used at full strength, that is without dilution, as an eco-friendly detergent; however, direct application to painted surfaces, plexiglass, plastics, or fiberglass is not recommended.


Conversely, Limonene may be added to wetting agents, such as water or vinegar bases, to achieve better solubilization.
Either method will make for a natural yet equally effective industrial-strength “green” surface disinfectant that Limonene is ideal for household cleaning.
Limonene is a popular additive in foods, cosmetics, cleaning products, and natural insect repellants.


For example, Limonene’s used in foods like sodas, desserts, and candies to provide a lemony flavor.
Limonene is extracted through hydrodistillation, a process in which fruit peels are soaked in water and heated until the volatile molecules are released via steam, condensed, and separated.


Due to its strong aroma, limonene is utilized as a botanical insecticide.
Limonene’s an active ingredient in multiple pesticide products, such as eco-friendly insect repellents.
Other household products containing Limonene include soaps, shampoos, lotions, perfumes, laundry detergents, and air fresheners.


Additionally, limonene is available in concentrated supplements in capsule and liquid form.
These are often marketed for their supposed health benefits.
This citrus compound, Limonene, is also used as an aromatic oil for its calming and therapeutic properties.


Limonene has solvent properties, and is used in many cleaning products to help break down fats and oils, improving cleaning performance.
Limonene is also used as a fragrance and flavouring ingredient in food, personal care products and cosmetics.
Limonene is naturally present as a component of many of the essential oils we use as fragrances for our products.


Although this molecule is found in nature, Limonene can still have a negative effect on some people who may be sensitive to its oxidized compounds, which can be irritating to the skin.
Limonene is used to make medicine.


Limonene is common in cosmetic products.
As the main odor constituent of citrus (plant family Rutaceae), Limonene is used in food manufacturing and some medicines, e.g. as a flavoring to mask the bitter taste of alkaloids, and as a fragrant in perfumery.


Limonene is used for obesity, cancer, and bronchitis, but there is no good scientific evidence to support these uses.
In foods, beverages, and chewing gum, limonene is used as a flavoring.
Limonene, a colourless liquid abundant in the essential oils of pine and citrus trees and used as a lemonlike odorant in industrial and household products and as a chemical intermediate.


Limonene is used in many different industries, from cleaning products to perfumes, from aromatherapy to food additives.
Limonene is a compound used especially in fragrances due to its citrus aroma.
The usage rate varies between 1% and 5% depending on the effect of Limonene and its interaction with other substances.


Limonene is a chemical found in fruits from the genus Citrus.
Limonene is a terpene and is abundant in the peels and essential oils of oranges, lemons, mandarins, and other citrus fruits.
Due to its smell, limonene is commonly used in fragrances, soaps, shampoos, and other health and cosmetic items.


Limonene is also used as a flavoring agent in food products.
Limonene also has applications in the food industry.
In cosmetics and skin care, limonene is primarily used as a fragrant ingredient and solvent.


Its wide range of beneficial applications has made Limonene one of the most prominent natural Terpenes.
With a light, pleasantly dry, and refreshingly-sweet citrusy scent, Limonene is valued for its aroma and is mostly used in fragrances as well as green cleaning products rather than for therapeutic applications.


Limonene is a thin, clear, colorless, oily fluid that is derived from steam distilled citrus rinds.
Limonene is safer to use, works more effectively, and is more environmentally-friendly than most commercial and industrial cleaners.
Limonene is used in cleaning products for two reasons: it has a pleasant, lemon-orange smell, and it acts as a solvent to help clean.


Limonene is found in a vast array of cleaning products, cosmetics, food flavourings and even aromatherapy, it comes in two forms: d-limonene and l-limonene.
These are like “different handed” versions of the same molecule, with only subtle differences.
The Limonene form is used in food-grade products, as well as cleaning and beauty products, and is prized mainly for its smell.


Limonene is also used in hospital laboratories when cleaning tissue samples for analysis.
The l-limonene version has a more pine-like scent but is used mainly as a solvent in industrial cleaning products.
Apart from these well-known uses, researchers now also believe limonene could be used as a dietary supplement to prevent cancer.


Limonene even turns up in some 3D printing processes.
Consumption of limonene is a successful alternative in the treatment of several diseases, triggering beneficial biological effects in clinical and preclinical studies, and seems to possess anti-inflammatory, antioxidant, anticancer, and heart-disease-fighting properties.


Limonene oil is extracted from the peels of oranges and other citrus fruits to make medicine and is used in perfumes and deodorants, beverages such as tea, and essential oil-infused supplements.
Because limonene has strong scents and flavors, it is used in various ways.


In food products: Limonene is used as a flavoring agent in beverages and chewing gum
In pharmaceuticals: Limonene is added to help medicinal ointments and creams penetrate the skin
In manufacturing industries: Limonene is used as a fragrance, cleaner (solvent), and an ingredient in water-free hand cleansers.



HOW DOES LIMONENE WORK?
Limonene is a fragrance agent, a degumming agent, and a gentle yet powerful cleaner that is reputed to effectively remove stains, grease, tar, and more, thus making a natural replacement for more popular solvents, which usually contain chlorine or petroleum.

Its mildness has also made Limonene a popular ingredient in water-free hand soaps, in which it is said to not only cleanse but to also leave the hands smelling fresh.
When applied to various types of hard surfaces, such as counter tops, windows, mirrors, floors, bath tubs, refrigerators, cars, and electronic items, Limonene is reputed to bring a high shine to all cleaned items.



POTENTIAL HEALTH BENEFITS OF LIMONENE:
Like many terpenes, limonene appears to interact with a number of systems in the body.
Studies are still being done on how limonene in particular affects your health, but early results suggest limonene may have several health benefits.
Currently, studies suggest that limonene may provide benefits like:

*Reduced Inflammation:
Consuming limonene may help reduce chronic inflammation in the body.
While more studies must be done, early trials suggest that limonene may help reduce a number of factors connected to chronic inflammation.

Since inflammation factors into a number of chronic conditions, such as rheumatoid arthritis and certain forms of cancer, reducing inflammation may help lower your risk of developing these conditions and improve the health of people living with them.



LIMONENE AT A GLANCE:
*Monoterpene commonly found in citrus oils
*Primarily used as a fragrance in cosmetics
*Oxidizes when exposed to air
*Can cause skin sensitization



LINKED TO SEVERAL HEALTH BENEFITS OF LIMONENE:
Limonene has been studied for its potential anti-inflammatory, antioxidant, anticancer, and heart-disease-fighting properties.

*Anti-inflammatory and antioxidant benefits of Limonene:
Limonene has been shown to reduce inflammation in some studies.
While short-term inflammation is your body’s natural response to stress and is beneficial, chronic inflammation can harm your body and is a major cause of illness.

It’s important to prevent or reduce this type of inflammation as much as possible.
Limonene has been shown to reduce inflammatory markers that relate to osteoarthritis, a condition characterized by chronic inflammation.


*Limonene has demonstrated antioxidant effects as well:
Antioxidants help reduce cell damage caused by unstable molecules called free radicals.
Free radical accumulation can lead to oxidative stress, which may trigger inflammation and disease.
One test-tube study revealed that limonene may inhibit free radicals in leukemia cells, suggesting a decrease in inflammation and cellular damage that would normally contribute to disease.


*May have anticancer effects:
Limonene may have anticancer effects.


*May boost heart health:
Heart disease remains the leading cause of death in the United States, accounting for nearly one in four deaths.
Limonene may lower your risk of heart disease by reducing certain risk factors, such as elevated cholesterol, blood sugar, and triglyceride levels.



BENEFITS OF LIMONENE:
*Reduce appetite:

*Decrease stress and anxiety:
Support healthy digestion.
Limonene may protect against stomach ulcers.



5 POTENTIAL HEALTH BENEFITS OF LIMONENE:
Five potential health benefits of limonene include:

*Reduces inflammation (anti-inflammatory):
Some studies report that limonene may help reduce the number of factors connected to chronic inflammation, thus lowering the risk of certain conditions such as rheumatoid arthritis, osteoarthritis, and certain types of cancer.


*Has an antioxidant effect:
Early trials suggest that limonene acts as an antioxidant in the body, absorbing and removing damaging free radicals and unstable molecules before they can injure cells.
Moreover, dietary limonene may help lower the risk of signs of aging by reducing the amount of oxidative stress on the body.


*Has an anticancer effect:
Early research shows that limonene is linked to cancer-killing and tumor growth-inhibiting properties, especially in breast cancer.


*Improves heart health:
Laboratory studies suggest that consuming limonene lowers the risk of heart diseases by reducing triglycerides, cholesterol, and blood sugar levels.
Limonene promotes an increase in good cholesterol levels and is connected to a lower risk of atherosclerosis and coronary events.


*Decreases stress and anxiety:



WHAT ARE THE POTENTIAL BENEFITS OF LIMONENE:
Studies on the effects of Limonene reveal that the compound has the ability to relieve stress, provide anti-fungal and antibacterial properties, increase energy and improve one’s mood.

Consequently, research also reveals inhalation of the terpenes vapour can aid in the production of serotonin and dopamine in areas of the brain associated with anxiety and depression.
Thanks to such energizing and mood-boosting properties, cannabis strains containing high doses of Limonene maybe beneficial for managing symptoms associated with conditions such as Attention Deficit Disorder (ADHD), depression and chronic fatigue syndrome.

It’s worth noting, that this zesty terpene does not just improve mood and serotonin production.
Limonene can enhance the way our bodies absorb cannabinoids and other much needed terpenes through the skin and gut.
Explaining why some experts suggest that cannabis strains with high doses can help regulate healthy digestion and gut functioning.



RESEARCHE ON LIMONENE:
Research on limonene has increased in recent years.
Through research, it's become apparent that limonene has several properties that may benefit human health.


*Antioxidant and Anti-Inflammatory Activity:
As a terpene, limonene contains chemical substances with known antioxidant and anti-inflammatory activity.
Anti-inflammatory substances can help reduce inflammation in the body, while antioxidants help prevent and reduce cell damage.
Due to these properties, limonene has been looked into for its possible effects on health conditions such as neurodegenerative diseases.
In vitro research shows that limonene's antioxidant and anti-inflammatory activities may protect your brain from damage and certain diseases.


*Anticancer Potential:
Some people with cancer choose to use various dietary supplements as complementary treatments to chemotherapy, radiation, and other cancer treatments.
Limonene has been studied for its potential anticancer properties.


*Antiviral Properties:
There is some evidence that limonene may have a role in the treatment of viruses like the flu, COVID-19, and herpesvirus.
A laboratory study found that both L- and Limonene act as a disinfectant against influenza A virus H1N1.

Limonene was found to be the major component in the essential oil from orange peels and responsible for the antiviral properties displayed in the study.
Other lab research has suggested that limonene has antiviral properties against COVID-19, although much more research is needed.
Limonene has also been found to have a potential role in treating human herpesvirus.

In an in vivo study, limonene was shown to directly inhibit herpesvirus.
Limonene was most effective when added to cells just before herpes virus infection.
Research on the role of limonene as an antiviral agent is in the very early stages.
More research must be conducted to determine if limonene can in fact treat or prevent any viruses in humans.


*Heart Protection:
Limonene supplementation was also found to reverse changes in inflammatory markers and, thus, cardiac toxicity risk.



CHEMICAL REACTIONS OF LIMONENE:
Limonene is a relatively stable mono terpene and can be distilled without decomposition, although it cracks at high temperatures to form isoprene .
Carveol is readily oxidized in moist air to produce carvone and limonene oxides.
Limonene undergoes dehydrogenation with sulfur to form p - cymene .



PHYSICAL and CHEMICAL PROPERTIES of LIMONENE:
Molecular Weight: 136.23 g/mol
XLogP3-AA: 3.4
Hydrogen Bond Donor Count: 0
Hydrogen Bond Acceptor Count: 0
Rotatable Bond Count: 1
Exact Mass: 136.125200510 g/mol
Monoisotopic Mass: 136.125200510 g/mol
Topological Polar Surface Area: 0Ų
Heavy Atom Count: 10
Formal Charge: 0
Complexity: 163
Isotope Atom Count: 0
Defined Atom Stereocenter Count: 1
Undefined Atom Stereocenter Count: 0
Defined Bond Stereocenter Count: 0
Undefined Bond Stereocenter Count: 0
Covalently-Bonded Unit Count: 1
Compound Is Canonicalized: Yes

Molecular Formula: C10H16
Molecular Weight: 136.2 g/mol
Purity: >=98%
Type of Compound: Monoterpenoids
Physical state: liquid, clear
Color: colorless
Odor: characteristic
Melting point/freezing point:
Melting point/range: -73,97 °C
Initial boiling point and boiling range: 176 - 177 °C
Flammability (solid, gas): No data available
Upper/lower flammability or explosive limits:
Upper explosion limit: 6,1 %(V)
Lower explosion limit: 0,7 %(V)
Flash point: 51 °C - closed cup

Autoignition temperature: 245 °C at 995,44 hPa
Decomposition temperature: No data available
pH: No data available
Viscosity
Viscosity, kinematic: No data available
Viscosity, dynamic: No data available
Water solubility: 0,00569 g/l at 20 °C
Partition coefficient: n-octanol/water:
log Pow: 4,38 at 37 °C
Vapor pressure: 2 hPa at 24,85 °C
Density: 0,842 g/mL at 20 °C
Relative density: 0,8400 - 0,8440 at 20 °C
Relative vapor density: 4,70 - (Air = 1.0)
Particle characteristics: No data available

Explosive properties: No data available
Oxidizing properties: none
Other safety information:
Relative vapor density: 4,70 - (Air = 1.0)
Physical description: A colorless liquid with an odor of lemon.
Boiling point: 352°F
Molecular weight: 136.2
Freezing point/melting point: -40°F
Flash point: 115°F
Specific gravity: 0.842 at 69.8°F
Ionization potential:
Lower explosive limit (LEL): 0.7%
Upper explosive limit (UEL): 6.1%
NFPA health rating: 2
NFPA fire rating: 2
NFPA reactivity rating: 0



FIRST AID MEASURES of LIMONENE:
-Description of first-aid measures:
*General advice:
Show this material safety data sheet to the doctor in attendance.
*If inhaled:
After inhalation:
Fresh air.
*In case of skin contact:
Take off immediately all contaminated clothing.
Rinse skin with water/ shower.
Consult a physician.
*In case of eye contact:
After eye contact:
Rinse out with plenty of water.
Remove contact lenses.
*If swallowed:
After swallowing:
Call a physician immediately.
-Indication of any immediate medical attention and special treatment needed:
No data available



ACCIDENTAL RELEASE MEASURES of LIMONENE:
-Environmental precautions:
Do not let product enter drains.
-Methods and materials for containment and cleaning up:
Cover drains.
Collect, bind, and pump off spills.
Observe possible material restrictions.
Take up carefully with liquid-absorbent material.
Dispose of properly.
Clean up affected area.



FIRE FIGHTING MEASURES of LIMONENE:
-Extinguishing media:
*Suitable extinguishing media:
Carbon dioxide (CO2)
Foam
Dry powder
*Unsuitable extinguishing media:
For this substance/mixture no limitations of extinguishing agents are given.
-Further information:
Remove container from danger zone and cool with water.
Prevent fire extinguishing water from contaminating surface water or the ground water system.



EXPOSURE CONTROLS/PERSONAL PROTECTION of LIMONENE:
-Control parameters:
--Ingredients with workplace control parameters:
-Exposure controls:
--Personal protective equipment:
*Eye/face protection:
Use equipment for eye protection.
Safety glasses
*Skin protection:
Full contact:
Material: butyl-rubber
Minimum layer thickness: 0,7 mm
Break through time: 480 min
Splash contact:
Material: Latex gloves
Minimum layer thickness: 0,6 mm
Break through time: 30 min
*Body Protection:
Flame retardant antistatic protective clothing.
*Respiratory protection:
Recommended Filter type: Filter A (acc. to DIN 3181)
-Control of environmental exposure:
Do not let product enter drains.



HANDLING and STORAGE of LIMONENE:
-Precautions for safe handling:
*Advice on protection against fire and explosion:
Take precautionary measures against static discharge.
*Hygiene measures:
Immediately change contaminated clothing.
Apply preventive skin protection.
Wash hands and face after working with substance.
-Conditions for safe storage, including any incompatibilities:
*Storage conditions
Keep container tightly closed in a dry and well-ventilated place.



STABILITY and REACTIVITY of LIMONENE:
-Chemical stability:
The product is chemically stable under standard ambient conditions (room temperature) .
-Incompatible materials:
No data available

LINEAR ALKYL BENZENE SULPHONIC ACID Linear Alkyl Benzene Sulphonic Acid Chemical Name: Linear Alkyl Benzene Sulphonic Acid; Linear Alkyl Benzene Sulphonic Acid Description and Uses: Linear Alkyl Benzene Sulphonic Acid; is an anionic surfactant commonly used in the manufacture of detergents and emulsifiers. It is environmentally friendly as it can be dried as powder. Usage areas LABSA is formed by the reaction of Linear Alkyl Benzene Sulphonic Acid (LAB) with SO3 (sulfonation). Today, LABSA is used as the main surfactant in liquid, gel or powder detergent production processes. It is one of the main raw materials of synthetic detergent industry. Laundry, dishwasher powder detergents, detergent gels, liquid soaps, cleaning powders, oily soaps and so on. as. It is used as mercerizing and washing agent in textile sector. As the raw material of detergent, it is used in the production of alkynbenzene solphonic acid sodium in decontamination, emulsion, dispersion performance, wetting and foam properties. It is widely used in various detergent and emulsion production such as washing powder, dishwashing detergent, light or hard dirt detergent, textile industry cleaner, paint assistant, coating and leather making industry and paper making industry. PRODUCT IDENTIFICATION CAS NO. 27176-87-0 LINEAR ALKYL BENZENE SULPHONIC ACID EINECS NO. 248-289-4 FORMULA CH3(CH2)11C6H4SO3H SYNONYMS Dodecylbenzene Sulfonic Acid (Strait Chain); LAS; LABSA; Laurylbenzenesulfonic Acid; Laurylbenzenesulfonate; n-Dodecylbenzene Sulfonic Acid; Alkylbenzene sulphonate, sodium salt; Linear Alkyl benzene Sulphonic Acid; Dodecylbenzolsulfonsäure (German); ácido dodecilbenceno sulfónico (Spanish); Acide dodécylbenzènesulfonique (French); CLASSIFICATION Anionic Surfactant DESCRIPTION OF LABSA Linear alkyl benzene sulphonic acid is the largest-volume synthetic surfactant because of its relatively low cost, good performance, the fact that it can be dried to a stable powder and the biodegradable environmental friendliness as it has straight chain. LABSA is an anionic surfactants with molecules characterized by a hydrophobic and a hydrophilic group. Alpha-olefin sulfonates (AOS) alkyl sulfates (AS) are also examples of commercial anionic surfactants. They are nonvolatile compounds produced by sulfonation. LABSA are complex mixtures of homologues of different alkyl chain lengths (C10 to C13 or C14) and phenyl positional isomers of 2 to 5-phenyl in proportions dictated by the starting materials and reaction conditions, each containing an aromatic ring sulfonated at the para position and attached to a linear alkyl chain at any position with the exception of terminal one (1-phenyl). The properties of LABSA differ in physical and chemical properties according to the alkyl chain length, resulting in formulations for various applications. The starting material LABSA (linear alkylbenzene) is produced by the alkylation of benzene with n-paraffins in the presence of hydrogen fluoride (HF) or aluminium chloride (AlCl3) as a catalyst. LABSA is produced by the sulfonation of LAB with oleum in batch reactors. Other sulfonation alternative reagents are sulfuric acid, diluted sulfur trioxide, chlorosulfonic acid and sulfamic acid on falling film reactors. LABSA are then neutralized to the desired salt (sodium, ammonium, calcium, potassium, and triethanolamine salts). Surfactants are widely used in the industry needed to improve contact between polar and non-polar media such as between oil and water or between water and minerals. Linear alkyl benzene sulphonic acid is mainly used to produce household detergents including laundry powders, laundry liquids, dishwashing liquids and other household cleaners as well as in numerous industrial applications like as a coupling agent and as an emulsifier for agricultural herbicides and in emulsion polymerization. PHYSICAL AND CHEMICAL PROPERTIES Household detergents including laundry powders, laundry liquids, dishwashing liquids and other household cleaners. Industrial applications of wetting agent, emulsifier for agricultural herbicides and in polymerization. LABSA HOMOLOGUES AND SALTS Linear Alkyl benzene sulphonic acid 27176-87-0 25155-30-0 (Sodium) Tridecylbenzene sulfonic acid 25496-01-9 26248-24-8 (Sodium) Tetradecylbenzene sulfonic acid 30776-59-1 28348-61-0 (Sodium) Pentadecylbenzene sulfonic acid 61215-89-2 64716-02-5 (Potassium) Hexadecylbenzene sulfonic acid 16722-32-0 64716-00-3 (Potassium) Heptadecylbenzene sulfonic acid 39735-13-2 Linear Alkyl benzene Sulphonic Acid (LABSA)/Linear Alkylate Sulfonate (LAS) Linear alkyl benzene sulphonic acid (LABSA) is prepared commercially by sulfonating linear alkylbenzene (LAB). Linear alkylbenzene sulfonate (LABSA), the world’s largest-volume synthetic surfactant, which includes the various salts of sulfonated alkylbenzenes, is widely used in household detergents as well as in numerous industrial applications. The LABSA market is driven by the markets for LABSA, primarily household detergents. Linear alkylbenzene sulfonate was developed as a biodegradable replacement for nonlinear (branched) alkylbenzene sulfonate (BAS) and has largely replaced BAS in household detergents throughout the world. The pattern of LABSA consumption demonstrates the overwhelming preference by consumers for liquid laundry detergents in North America, whereas powders continue to be the dominant products in Western Europe, Japan, and China. Comparable and reliable data in other world regions are generally unavailable. In these less-developed world areas, LABSA is essentially used only in laundry powders (particularly in India and Indonesia) and hand dishwashing liquids. The latter are often used as general-purpose cleaners. The following pie chart shows world consumption of LABSA: About 82–87% of LABSA is used in household detergents, including laundry powders, laundry liquids, dishwashing liquids, and other household cleaners. Industrial, institutional, and commercial cleaners account for most of the other applications, but LABSA is also used as an emulsifier (e.g., for agricultural herbicides and in emulsion polymerization) and as a wetting agent. Very small volumes are also used in personal care applications. Demand in the North American household segment fell sharply in 2000–11, as a result of several developments, including reformulations away from LABSA to alternative surfactants because of cost considerations, the greater use of enzymes, and adverse economic conditions that resulted in lower overall surfactant levels in detergents. However, consumption stabilized during 2011–17. Although consumption of LABSA will likely stabilize or decline slightly in the highly developed regions, it will increase by 3.0–5.0% in some less-developed regions or countries, such as the Middle East, Africa, India, and China, as well as Southeast Asia. As a result of the rapid growth of LABSA demand in the Asia Pacific region, demand in the region accounted for over half of global demand in 2017. The worldwide growth of LABSA will be negatively impacted by the efforts of detergent manufacturers to reduce the active content in their surfactant formulations, by the shift to liquid detergents in some countries (which benefits competing surfactants), and by less consumer overdosing (particularly in North America with unit dose laundry products, assuming they continue to take some market share from traditional liquid detergents). However, consumption of LABSA will be positively affected in countries/regions such as India, China, Africa, and the Middle East, where powder detergents are still a very large part of the laundry detergent market. Linear alkylbenzene sulfonate competes with several other major surfactants for use in household detergents. Some of the competitive surfactants have greater hard-water tolerance and better compatibility with enzymes and are milder than LABSA. Historically, however, LABSA has most often been lower in cost and has had other more favorable properties compared with competing surfactants. During 2002–06, very high crude oil prices made LABSA far less competitive than had been true in most years since its introduction. During 2007–11, LABSA prices tracked more closely those of the competitive surfactants. This led to a more stable pattern of consumption, even as prices for all surfactants continued to be very volatile. From late 2014 through 2017, low crude oil prices helped LABSA become more competitive. LABSA/LAS production is impacted by the supply situation for competing products—mainly alcohol ether sulfates (AES). Shortages in AES supply or its high price has usually favored the use of LABSA/LAS. In the developing world, LABSA competes with soaps. Alkylbenzene sulfonates are a class of anionic surfactants, consisting of a hydrophilic sulfonate head-group and a hydrophobic alkylbenzene tail-group. Along with sodium laureth sulfate they are one of the oldest and most widely used synthetic detergents and may be found in numerous personal-care products (soaps, shampoos, toothpaste etc.) and household-care products (laundry detergent, dishwashing liquid, spray cleaner etc.).[1] They were first introduced in the 1930s in the form of branched alkylbenzene sulfonates (BAS) however following environmental concerns these were replaced with linear alkylbenzene sulfonates (LABSA) during the 1960s.[2] Since then production has increased significantly from about 1 million tons in 1980, to around 3.5 million tons in 2016, making them most produced anionic surfactant after soaps. Contents 1 Branched alkylbenzene sulfonates 2 Linear alkyl benzene Sulphonic Acid sulfonates 3 Structure property relationships 4 Environmental fate 5 References Branched alkylbenzene sulfonates An example of a branched alkylbenzene sulfonate (BAS) Branched alkylbenzene sulfonates (BAS) were first introduced in the early 1930s and saw significant growth from the late 1940s onwards,[3] in early literature these synthetic detergents are often abbreviated as syndets. They were prepared by the Friedel–Crafts alkylation of benzene with 'propylene tetramer' (also called tetrapropylene) followed by sulfonation. Propylene tetramer being a broad term for a mixture of compounds formed by the oligomerization of propene, its use gave a mixture of highly branched structures.[4] Compared to traditional soaps BAS offered superior tolerance to hard water and better foaming.[5] However, the highly branched tail made it difficult to biodegrade.[6] BAS was widely blamed for the formation of large expanses of stable foam in areas of wastewater discharge such as lakes, rivers and coastal areas (sea foams), as well as foaming problems encountered in sewage treatment[7] and contamination of drinking water.[8] As such BAS was phased out of most detergent products during the 1960s, being replaced with linear alkylbenzene sulfonates (LABSA). It is still important in certain agrochemical and industrial applications, where rapid biodegradability is of reduced importance. Linear alkylbenzene sulfonates An example of a linear alkylbenzene sulfonate (LAS) Linear alkylbenzene sulfonates (LAS) are prepared industrially by the sulfonation of linear alkylbenzenes (LABSA), which can themselves be prepared in several ways.[2] In the most common route benzene is alkylated by long chain monoalkenes (e.g. dodecene) using hydrogen fluoride as a catalyst.[9] The purified dodecylbenzenes (and related derivatives) are then sulfonated with sulfur trioxide to give the sulfonic acid.[10] The sulfonic acid is subsequently neutralized with sodium hydroxide.[1] The term "linear" refers to the starting alkenes rather than the final product, perfectly linear addition products are not seen, in-line with Markovnikov's rule. Thus, the alkylation of linear alkenes, even 1-alkenes such as 1-dodecene, gives several isomers of phenyldodecane.[11] Structure property relationships Under ideal conditions the cleaning power of BAS and LABSA is very similar, however LABSA performs slightly better in normal use conditions, due to it being less affected by hard water.[12] Within LABSA itself the detergency of the various isomers are fairly similar,[13][14] however their physical properties (Krafft point, foaming etc.) are noticeably different.[15][16] In particular the Krafft point of the high 2-phenyl product (i.e. the least branched isomer) remains below 0 °C up to 25% LABSA whereas the low 2-phenyl cloud point is ∼15 °C.[17] This behavior is often exploited by producers to create either clear or cloudy products. Environmental fate Biodegradability has been well studied,[6][18][19] and is affected by isomerization, in this case, branching. The salt of the linear material has an LD50 of 2.3 mg/liter for fish, about four times more toxic than the branched compound; however the linear compound biodegrades far more quickly, making it the safer choice over time. It is biodegraded rapidly under aerobic conditions with a half-life of approximately 1–3 weeks;[18] oxidative degradation initiates at the alkyl chain.[1] Under anaerobic conditions it degrades very slowly or not at all, causing it to exist in high concentrations in sewage sludge, but this is not thought to be a cause for concern as it will rapidly degrade once returned to an oxygenated environment. LABSA Linear Alkyl Benzene Sulphonic Acid Product Information LABSA Linear alkyl benzene Sulphonic Acid is a chemical which is colorless and have viscous properties. LABSA Linear alkyl benzene sulphonic acid mainly using in detergent formulations. It is one of the most important and cheapest surfactants in powder formulation and detergent fluids. It has excellent cleansing properties. Usages of Linear Alkyl Benzene Sulphonic Acid LABSA Linear Alkyl Benzene sulphonic acid is a batch of organic sulfur compounds that are used in most home detergents, dishwashing detergents, detergent powder, cleaning powder, washing powders, detergent cake, liquid soap, soaps etc. LABSA, sulfonic acid compound is used as a foaming agent, cleaning agent in more formulations and toilet soaps for foaming. Sulfonic acid, LABSA is using in detergent industries, in textile industry as a washing agent, pesticides industries to improve the quality of spray. Sulfonic acid, LABSA is not inflammable substance and can dissolve in water, but not in organic solvent. Application of Linear Alkyl Benzene Sulphonic Acid Linear alkyl benzene Sulphonic Acid used in the industry to increase the contact of polar and non-polar phases, such as oil, water, or water and minerals. Linear alkyl benzene Sulphonic Acid sulfonate is mainly used for the manufacture of household detergents such as laundry powder, washing liquid, dishwashing liquid and other household cleaners and other industrial uses. LABSA Linear alkyl benzene Sulphonic Acid uses in produce sulfonic acid. LABSA is an additive as a lubricating agent oils and have as corrosion and rust prevention. his product is a very effective intermediate surfactant. Specification of Linear Alkyl Benzene Sulphonic Acid Product Name: Linear Alkyl benzene Sulphonic Acid ROW Characteristi LABSA Linear alkyl benzene Sulphonic Acid packing Basekim Chemical Production can supply LABSA Linear alkyl benzene Sulphonic Acid with drum. Each drum can take 220 kg and 80 drum can easily load in a container. It also depends on customer demands as well. LABSA Linear alkyl benzene Sulphonic Acid LABSA Linear alkyl benzene Sulphonic Acid is a chemical which is colorless and have viscous properties. LABSA Linear alkyl benzene Sulphonic Acid mainly using in detergent formulations. It is one of the most important and cheapest surfactants in powder formulation and detergent fluids. It has excellent cleansing properties. LABSA Linear alkyl benzene Sulphonic Acid in the formulation of anionic, non-anionic, and amphoteric surfactants, and it is extremely important for its degradability in nature. It is soluble in water and emulsifying agent. Linear Alkyl benzene sulphonic acid is one of the most widely used anionic surfactants due to its low cost, high efficiency and biocompatibility due to its linear chain. This anionic surfactant has hydrophilic and hydrophobic groups. These are non-volatile compounds produced by the sulfonation process. These compounds consist of mixtures of carbon chains of 10 to 14 carbon lengths that are a phenyl group with a sulfonate group LABSA Linear alkyl benzene Sulphonic Acid LABSA Linear alkyl benzene Sulphonic Acid application The properties of LABSA Linear alkyl benzene Sulphonic Acid depend on the length of the alkane chains that give them different functionality. Surfactants are used in the industry to increase the contact of polar and non-polar phases, such as oil, water, or water and minerals. Linear alkyl benzene Sulphonic Acid sulfonate is mainly used for the manufacture of household detergents such as laundry powder, washing liquid, dishwashing liquid and other household cleaners and other industrial uses. LABSA Linear alkyl benzene Sulphonic Acid uses in produce sulfonic acid. LABSA is an additive as an lubricating agent oils and have as corrosion and rust prevention. his product is a very effective intermediate surfactant. It is usually neutralized with alkali types and forms sulphonates used in different fields. This product can be used in acidic environments. LABSA Linear alkyl benzene Sulphonic Acid packing can supply LABSA Linear alkyl benzene Sulphonic Acid with drum . Each drum can take 220 kg and 80 drum can easily load in a container LABSA Linear alkyl benzene Sulphonic Acid PACKING Linear Alkyl Benzene Sulphonic Acid (LABSA) Specification LABSA properties: Trade Name: Sulfonic Acid COMMITTEE FOR VETERINARY MEDICINAL PRODUCTS LINEAR ALKYL BENZENE SULPHONIC ACIDS SUMMARY REPORT (1) 1. Linear alkyl benzene sulphonic acids (LABSA) are anionic surfactants. Linear alkyl benzene sulphonic acids are a mixtures of benzene sulphonic acids containing linear alkyl chains of different lengths (C9: less than 1%, C10: 8 to 16%, C11: 26 to 38%, C12: 26 to 38%, C13: 15 to 27% and longer than C13: less than 2.5%). The amount of linear alkyl benzene sulphonic acid in the products is 2% and these products are indicated for post-dipping or teat-spraying of dairy cows. The average dose per teat is assumed to be about 1 ml of the product, which equals to 80 mg of linear alkyl benzene sulphonic acid per cow per milking. Linear alkyl benzene sulphonic acids are commonly used as cleaning agents (household and personal care products). Linear alkyl benzene sulphonic acid is included as surface active agent in Commission establishing an inventory and a common nomenclature of ingredients employed in cosmetic products. The occupational and environmental exposure to linear alkyl benzene sulphonic acid has been assessed by WHO in 1996: The worldwide consumption of linear alkyl benzene sulphonic acids in 1990 was about 2 million tonnes. Linear dodecyl benzene sulphonic acid, under the synonym sodium dodecyl benzene sulphonate, has been included in 1987 on the food additive list of the Food and Drug Administration (FDA) of the United States of America as a surface active agent in commercial detergents used in washing fruits and vegetables or to assist in lye peeling these products. The tolerance limit has been set on equal to or less than 0.2% in wash water. 2. Hydrophobic and hydrophilic groups of the molecule are both essential for action of surfactants in detergents. According to a published study on the in vitro germicidal activity of teat dips the linear alkyl benzene sulphonic acid-containing product (1.94%) was shown to be completely effective against suspensions of Escherichia coli, Staphylococcus aureus and Streptococcus agalactiae containing bacteria/ml each following a contact time of 2 minutes. According to a published review document on in vitro studies, the 50% haemolytic concentration for linear alkyl benzene sulphonic acid was 9 mg/l and the 50% inhibitory concentration for prothrombin time was 0.05 mmol/l (16.3 mg/l). Linear alkyl benzene sulphonic acid influenced the thermal denaturation of proteins in vitro indicating protein-linear alkyl benzene sulphonic acid interaction. 3. Pharmacokinetic data are presented based on published reports. In rats, 14C-labelled alkyl benzene sulphonate was administered daily in the diet at a concentration of 1.4 mg/kg feed (dose per kg bw not given) to 12 male Wistar rats (120 to 140 g) for 5 weeks. Radioactivity was mostly excreted in faeces (52%) and in urine (29%) during the 5-week feeding period. After a single intraperitoneal administration of 14C-labelled alkyl benzene sulphonate (384.7 µg/rat), 85% of the dose was excreted during the first 24 hours and 95% within 10 days follow-up period. The main elimination route was via urine (50% of radioactivity), while 35% was excreted into faeces. However, during days 2 to 10 the percentage of radioactivity excreted into faeces was higher than that excreted into urine. No parent compound could be detected in faeces or urine but radioactivity was found in polar metabolites which were not further characterised. In another study, 35S-labelled linear alkyl benzene Sulphonic Acid was administered to male albino rats (Charles River strain, 150 to 200 g bodyweight) as a single per oral dose of 0.6, 1.2, 8 and 40 mg/rat (3 to 5 rats/group). During the 3-day follow-up period, 40 to 58% of radioactivity was excreted in urine and 39 to 56% in faeces. In faeces, the proportion of parent compound was 19% of total radioactivity. About 70% of linear alkyl benzene Sulphonic Acid was absorbed after oral administration. Two urine metabolites chemically close to methyl 4-(4'-methylsulfophenyl)- pentanoate were identified and were found to be a mixture of sulfophenyl butanoic acids and sulfophenyl pentanoic acids. Decomposition of linear alkyl benzene Sulphonic Acid sulphonate in rats was suggested to occur by ϖ-oxidation followed by catabolism through a β-oxidation mechanism. In vitro studies have not shown any penetration of 14C-labelled linear alkyl benzene sulphonic acid through intact rat or human skin. In in vivo studies in rats, 0.2 ml of 3 mM 14C linear alkyl benzene sulphonic acid (equivalent to 250 µg) was applied on 7.5 cm2 area of skin. These studies revealed deposition of 14C-labelled linear alkyl benzene sulphonic acid on the skin surface and in the upper regions of the hair follicles, however, no penetration of the substance could be detected after an exposure of 15 minutes. 4. The oral toxicity of linear alkyl benzene sulphonic acid is not very high. LD50 values for rats and mice range from 404 to 1525 mg/kg bw and 1575 to 1950 mg/kg bw, respectively. Both species showed diarrhoea and death occurred within 24 hours. 5. Repeated dose toxicity have been carried out using linear alkyl benzene sulphonic acids or their sodium salts containing alkyl chains of different lengths. Repeated dose toxicity has been documented on rats using 5 published articles, one of which was done in rats (60 females and 60 males/group) using only 1 dose level (0 and 100 mg of linear alkyl benzene sulphonic acid (chain length varying between C10 to C14)/l drinking water for 100 weeks). No differences were seen between test and control groups. No NOEL can be established due to deficiencies in the study design. Wistar rats (about 150 g, 10 per sex and group) received the test product (dishwashing detergent containing linear alkyl benzene sulphonic acid) was mixed into drinking water at corresponding to 0, 0.015, 0.075 and 0.375 ml linear alkyl benzene sulphonic acid/kg bw for 6 months. In the 3rd group the dose was increased after 9 weeks to 0.563 and again after 8 weeks to 0.75 ml/kg bw for 9 weeks. No differences were seen in haematological urine examinations between control and treated animals. Males showed decreased weight gain in the 3rd dose group, but the change was reversible once the treatment was stopped. Organ weights of the third group animals (5 per sex) killed immediately after the treatment were lower than those of the controls. Only control and the 3rd treatment groups were examined histologically. The animals in 3rd treatment group had small petechial bleedings (kidney, myocardium, lungs) and mucosal necrotis spots in gastrointestinal canal. They also had massive atrophy in adrenal glands and some atrophy in thymus. It is not possible to assess if changes showed correlation with dose or not, because only highest group was studied. No NOEL can be drawn from the study due to limited data available. Albino rats (FDRL strain, 15 animals per sex and group) received linear alkyl benzene sulphonic acid in feed at 0, 50 and 250 mg/kg bw for 12 weeks. Growth responses and food intake, haematological and urinary examinations showed no abnormalities. Histological findings revealed no abnormalities in lower dose group compared with control. Females in higher dose group had higher liver weight to body weight ratio than controls (p<0.01). The lower dose-group of 50 mg/kg bw/day showed no treatment-related changes. No NOEL can be established due to limited data available. Sprague-Dawley rat (10 animals per sex and group) received linear alkyl benzene sulphonic acid in feed (0, 0.02, 0.1 and 0.5%) for 90 days (corresponding to 8.8, 44 and 220 mg/kg bw). No statistically significant differences were seen in weight gains, food utilisation, haematological and urinary examinations. Organ to body ratios as well as macroscopic and microscopic findings were comparable in treated and control groups. No NOEL can be established due to limited data available. Charles River rat (50 animals per sex and group) received linear alkyl benzene sulphonic acid in feed (0, 0.02, 0.1 and 0.5%) for 2 years (dose per kg bw is not given). No statistically significant differences were seen in weight gains and food utilisation during the first 12 weeks. Organ to body ratios did not show any statistically significant differences when control and highest dose group were compared. At 8 months, male rats in 0.02 and 0.1% group had lower liver weight to bw ratios but this was not seen at later time points and never in the highest dose group. Haematological examinations revealed no treatment related changes. No abnormal macroscopic findings were seen and microscopic findings did not differ between the groups. No NOEL can be established due to limited data available. The highest dose (0.5% in feed for 2 years) did not show any treatment-related changes. A published repeated dose toxicity study has been carried out using 6 to 7 months old Beagle dogs (2 animals per sex and group). A linear alkyl benzene sulphonic acid-containing product (15% linear alkyl benzene sulphonic acid) was administered in doses of 0, 10, 100 and 1000 mg/kg bw daily for 6 months by gavage (corresponding to 0, 1.5, 15, and 150 mg linear alkyl benzene sulphonic acid/kg bw). Lowest dose group showed no treatment-related changes. One female dog in middle dose level group had drooling from the second week forward and one animal regurgitated part of one dose which lead to sedation and decreased appetite. In the highest dose group, 3 to 4 animals had marked salivation. No animals died. In the highest dose group feed intake was moderately reduced. Marked reduction in weight gain was only seen in the highest dose group (more pronounced in females). No changes were seen in blood and urinary tests. Eyes and hearing were normal in all groups. In highest dose group mucosal erosions were found in stomach (mainly in cardia) of one male and one female. Presence of haemosiderosis in spleen was more pronounced in highest dose group. One dog in the same group had small necroses in pancreas and 2 dogs had some iron-free pigment in kidneys. No NOEL can be established due to small number of animals and limited data available. According to a WHO report, minimal effects, including biochemical and histopathological changes in the liver, have been reported in subchronic studies in which rats were administered linear alkyl benzene sulphonic acid in the diet or drinking water at concentrations equivalent to doses greater than 120 mg/kg bw per day. These changes appeared to be reversible. In the absence of the original data, no firm conclusion on the data reported in the WHO report can be drawn. 6. Tolerance in dairy cows was studied using commercial teat dip containing 2% linear alkyl benzene sulphonic acid. The product was used post-milking twice daily for 10 days. The product was well-tolerated. 7. Effects on reproduction have been documented using 2 published articles, one of which described a study in rats (10 females and 10 males/group) using only one dose level of linear alkyl benzene Sulphonic Acid sulphonic acid (0 and 100 mg/l drinking water). The data provided are too limited for the assessment. Charles River rat (20 males and 20 females/group) received linear alkyl benzene sulphonic acid in feed (0, 0.02, 0.1 and 0.5% daily) in the 3-generation study (dose per kg bw is not given). No gross abnormalities were noted in pups. Rats of the F1 and F2 generations had similar growth patterns and organ to body weight ratios in control and test groups. No abnormalities were seen in histological examinations. In haematological studies, a statistically significant difference (level of significance not indicated) was seen in red blood cell count between control and females of highest test group. F3-weanlings were normal with respect to growth, organ to body weight ratios, macroscopic and microscopic examinations. Haematological values showed no treatment related trend or pattern in this study. The studies provided showed no indication of any reproduction toxicity. 8. Teratogenicity data were available from studies conducted using different linear alkyl benzene Sulphonic Acid sulphonic acids in mouse, rat and rabbit using oral, dermal and subcutaneous administration published in five articles. In two mouse studies the exposure times are not in accordance with the present guidelines. One study in mouse using dermal or subcutaneous administration was carried out using smaller group sizes and exposure times other than recommended in present guidelines. Linear alkyl benzene sulphonic acid (0, 0.2, 2, 300 and 600 mg/kg bw daily) was administered orally to female mice (n = 20), rats (n = 20) (days 6 to 15 of gestation) and rabbits (n = 13) days 6 to 18 of gestation). In all species primary toxic effects in dams were generally associated with disturbance of the gastrointestinal tract (diarrhoea, anorexia, retarded weight gain, weight loss, death). Rabbits were found to be the most susceptible species followed by mice and rats. The two highest dose groups showed maternal toxicity in mice and rabbits resulting in increased foetal loss and reduced litter size. No effects were seen in dams at 2 mg/kg bw in mice and rabbits. In rats, the highest dose caused maternal toxicity also, but did not affect litter parameters. No dose-related trend was seen in foetal weights. No difference was seen in number of major malformations between treated groups and controls. In mice, minor skeletal abnormalities increased to 33.7% in 300 mg/kg bw group compared with 11.7 to 13.3% in controls and lower dose groups. No teratological changes different from controls were seen except an increase in minor skeletal anomalies in 300 mg/kg bw group in mice. From the highest dose group no viable young were available as a result of marked maternal toxicity. When dermal exposure (linear alkyl benzene sulphonic acid in water) was used in mouse, rat and rabbit, the two highest doses caused severe skin reactions in mice (50 and 500 mg/kg bw) and rabbits (9 and 90 mg/kg bw). The highest dose in rats (60 mg/kg bw) showed also skin irritation: erythema and oedema with peak response on days 4 to 5. Except for the highest dose group in mice, no treatment related effects were seen in dams and litter data. In mice, a significant (p<0.05) increase in embryonic deaths was seen at 50 and 500 mg/kg bw compared with controls. In rats, no significant changes in litter parameters were seen in treated animals. In rabbits, the highest dose group had somewhat higher foetal loss and smaller litter size (statistically not significant). No statistically significant differences in anomalies were seen. The studies provided showed no indication of any teratogenic potential of the substanc

LINOLENIC ACID, N° CAS : 463-40-1 (CIS).Nom INCI : LINOLENIC ACID.Nom chimique : 9,12,15-Octadecatrienoic acid (9Z, 12Z, 15Z). N° EINECS/ELINCS : 207-334-8 (CIS).Noms français : Acide linolénique; Acide octatridécène-9,12,15 oïque (cis,cis,cis); cis, cis, cis,-Acide octatridécène-9,12,15 oïque. Noms anglais : (Z,Z,Z)-9,12,15-Octadecatrienoic acid; 9,12,15-Octadecatrienoic acid; 9,12,15-Octadecatrienoic acid, (Z,Z,Z)-; alpha-Linolenic acid; cis,cis,cis-9,12,15-Octadecatrienoic acid; Linolenic acid. Utilisation et sources d'émission; Produit alimentaireSes fonctions (INCI) Antistatique : Réduit l'électricité statique en neutralisant la charge électrique sur une surface. Agent nettoyant : Aide à garder une surface propre Emollient : Adoucit et assouplit la peau. Conditionneur capillaire : Laisse les cheveux faciles à coiffer, souples, doux et brillants et / ou confèrent volume, légèreté et brillance Agent d'entretien de la peau : Maintient la peau en bon état Tensioactif : Réduit la tension superficielle des cosmétiques et contribue à la répartition uniforme du produit lors de son utilisation Agent parfumant : Utilisé pour le parfum et les matières premières aromatiques. α-Linolenic acid [Wiki] (9Z,12Z,15Z)-9,12,15-Octadecatrienoic acid [ACD/IUPAC Name] (9Z,12Z,15Z)-9,12,15-Octadecatriensäure [German] [ACD/IUPAC Name] (9Z,12Z,15Z)-Octadeca-9,12,15-trienoic acid (all-Z)-9,12,15-Octadecatrienoic acid 1727693 [Beilstein] 207-334-8 [EINECS] 463-40-1 [RN] 9,12,15-all-cis-Octadecatrienoic acid 9,12,15-Octadecatrienoic acid, (9Z,12Z,15Z)- [ACD/Index Name] 9,12,15-OCTADECATRIENOIC ACID, (Z,Z,Z)- 9Z,12Z,15Z-Octadecatrienoic acid Acide (9Z,12Z,15Z)-9,12,15-octadécatriénoïque [French] [ACD/IUPAC Name] a-Linolenic Acid cis,cis,cis-9,12,15-octadecatrienoic acid Linolenic acid MFCD00065720 [MDL number] α-Lnn &α;-LA &α;-linolenic acid (9,12,15)-linolenic acid (9Z,12Z,15Z)octadeca-9,12,15-trienoic acid (9Z,12Z,15Z)-Octadecatrienoic acid (Z,Z,Z)-9,12,15-Octadecatrienoate (Z,Z,Z)-9,12,15-Octadecatrienoic acid (Z,Z,Z)-Octadeca-9,12,15-trienoic acid 104639-58-9 [RN] 32460-00-7 [RN] 68424-45-3 [RN] 9-cis,12-cis,15-cis-octadecatrienoic acid ¦Ã-Linolenic Acid a-Linolenate all-cis-9,12,15-Octadecatrienoate all-cis-9,12,15-octadecatrienoic acid alpha.-Linolenic Acid C18:3 cis,cis,cis-9,12,15-Octadecatrienoate cis-9, cis-12, cis-15-octadecatrienoic acid cis-9,12,15-octadecatrienoate cis-9,12,15-octadecatrienoic acid cis-9,cis-12,cis-15-Octadecatrienoic acid cis-δ(9,12,15)-octadecatrienoic acid cis-δ9,12,15-Octadecatrienoic acid http://www.hmdb.ca/metabolites/HMDB0001388 α-Linolenic Acid MaxSpec® Standard Industrene 120 Linolenic acid 10 µg/mL in Methanol LNL Octadecatrienoic acid, 9,12,15-(Z,Z,Z)- α linolenic acid α-linolenic acid α-Linolenic Acid α-Linolenic Acid α-Linolenic Acid MaxSpec® Standard|9Z,12Z,15Z-octadecatrienoic acid α-linolenic acid(c18:3) α-linolenic acid, from plants α-Linolenic Acid|9Z,12Z,15Z-octadecatrienoic acid α-LNA Α-亞麻酸 [Chinese]

LINSEED ACID, N° CAS : 68424-45-3, Nom INCI : LINSEED ACID, N° EINECS/ELINCS : 270-304-8. Ses fonctions (INCI). Agent nettoyant : Aide à garder une surface propre.Emollient : Adoucit et assouplit la peau. Agent émulsifiant : Favorise la formation de mélanges intimes entre des liquides non miscibles en modifiant la tension interfaciale (eau et huile) Tensioactif : Réduit la tension superficielle des cosmétiques et contribue à la répartition uniforme du produit lors de son utilisation

L 75; TRLA 50; ALPHA-LNN; Emery 644; L 75 (acid); Toenol 8183; Toenol LOFA; LINSEED ACID; Toenol 1140A; Nouracid LE 80; LINOLENIC ACID CAS NO:68424-45-3

LIPASE, N° CAS : 9001-62-1, Nom INCI : LIPASE, N° EINECS/ELINCS : 232-619-9. Classification : Enzymes. Ses fonctions (INCI) : Agent d'entretien de la peau : Maintient la peau en bon état; Lipase; Lipase fongique. Noms anglais : FUNGAL LIPASE; LIPASE, FUNGAL; LIPASE, TRIACYLGLYCEROL; PANCREAS LIPASE; Triacylglycerol lipase (EC 3.1.1.3); TRIGLYCERIDE LIPASE; Triacylglycerol lipase

Linseed oil, also known as flaxseed oil, is a vegetable oil derived from the seeds of the flax plant, scientifically known as Linum usitatissimum.
Linseed Oil is golden yellow, amber, or brown drying oil with a peculiar odor and bland taste.
Linseed Oil soluble in ether, chloroform, carbon disulfide, and turpentine; slightly soluble in alcohol, spontaneous heating.

CAS Number: 8001-26-1
EINECS Number: 232-278-6

Linseed Oil polymerizes on exposure to air.
Chief constituents are glycerides of Linseed Oil, oleic, linoleic, and saturated fatty acids.

The drying property is due to the Linseed Oil and linolenic groups.
Derivation is from seeds of the flax plant Linum usitatissimum by expression or solvent extraction.

Various refining and bleaching methods are used.
The grades of linseed oil are raw; boiled, double-boiled, blown, varnish makers' and refilled.
Linseed oil is an pale yellow oil extracted from the seeds of flax (linseed).

Linseed Oil hardens on exposure to air (it is a drying oil) because it contains linoleic acid and linolenic acid, and is used in enamels, oilpaints, putty, linoleum and varnishes.
Linseed oil is currently one of the highest known vegetable oils with the highest content of essential fatty acids (omega-3 and omega-6 fatty acids).
Linseed Oil is used in paints, varnishes, oilcloth, putty, printing inks, core oils, linings, and packings, alkyd resins, soap, and pharmaceuticals.

Linseed Oil has been used for various purposes for centuries, including as a dietary supplement, a drying oil in paints, and as an ingredient in various industrial and cosmetic products.
Linseed oil is a natural triglyceride and a well known drying oil.
Drying of the triglyceride mainly leads to the oxidation of the unsaturated fatty acid segments and polymerization.

Linseed Oil oxidative degradation studies of linseed oil show hardening and oxidation of alkylic sections followed by partial fragmentation of the triglyceride structure.
Linseed oil, also known as flaxseed oil or flax oil (in its edible form), is a colourless to yellowish oil obtained from the dried, ripened seeds of the flax plant (Linum usitatissimum).
The oil is obtained by pressing, sometimes followed by solvent extraction.

Owing to its polymer-forming properties, linseed oil is often blended with combinations of other oils, resins or solvents as an impregnator, drying oil finish or varnish in wood finishing, as a pigment binder in oil paints, as a plasticizer and hardener in putty, and in the manufacture of linoleum.
Linseed oil use has declined over the past several decades with increased availability of synthetic alkyd resins—which function similarly but resist yellowing.
Linseed oil is an edible oil in demand as a dietary supplement, as a source of α-Linolenic acid, an omega-3 fatty acid.

Linseed Oil is traditionally eaten with potatoes and quark.
Linseed oil comes from the seed of the flax plant and comes in two different forms, as Raw or Boiled.
Linseed Oil is a very traditional finish, used for hundreds of years and still very popular for treating and finishing wood.

Linseed oil is used to protect and maintain interior and exterior woods, concrete and is also one of the main ingredients in many paints and varnishes.
Linseed Oil is a natural oil so not as bad for the environment as many other solvent based finishes and has a variety of uses from a furniture finish to treating wooden floors.
Linseed oil is a triglyceride, like other fats.

Linseed oil is distinctive for its unusually large amount of α-linolenic acid, which oxidises in air.
Having a high content of di- and tri-unsaturated esters, linseed oil is susceptible to polymerization reactions upon exposure to oxygen in air.
This polymerization, which is called autoxidation, results in the rigidification of the material.

To prevent premature drying, linseed oil-based products (oil paints, putty) are stored in airtight containers.
Rags soaked with linseed oil pose fire hazard because they provide a large surface area for rapid oxidation.
The oxidation of linseed oil is exothermic, which may lead to spontaneous combustion.

In 1991, One Meridian Plaza, in Philadelphia, was severely damaged in a fire, in which three firefighters perished, thought to be caused by rags soaked with linseed oil.
Linseed oil has numerous well-documented qualities and is extracted from the seeds of the flaxseed plant.
Linseed Oil is used in food preparation and as a dietary supplement due to its many health benefits.

One of its most enduring uses, however, is as a protective finish for wood surfaces.
Linseed oil is used as a base in some ecological and craft paints because of its characteristics.
Applying the oil prior to varnishing a surface is not recommended as it might prevent the varnish from adhering smoothly.

Wood oils today are all-in-one products that seal and stain both indoor and outdoor wood surfaces all at once, leaving a quality finish and long-lasting protection.
Boiled Linseed Oil is a superior quality oil due to its preparation at high temperatures it dries more quickly, forming a tough and long lasting finish and natural lustre to wood furniture.
Suitable to use internally or externally on unpolished softwood surfaces.

For replacing the natural sheen that wood may lose after long periods in the sun.
Prevents wood from turning grey due to weathering and splitting or wrapping.
The oil-based properties of this product improve the grain definition of treated timbers.

Linseed oil is suitable for use on all types of wood except external hardwoods such as Oak and Teak.
For these wood types Teak Oil should be used.
Linseed oil is the best option to protect natural wood that is neither varnished nor previously stripped of other coatings.

Linseed Oil is used to coat wood and protect it from the effects of deteriorating agents.
Linseed Oil’s extremely easy to use and dries rapidly.
The oil must be applied on virgin wood, but the process can be repeated over time to maintain adequate protection.

Linseed Oil exterior wood surfaces exposed to weathering conditions generally need maintenance every two years.
Maintenance is quite easy and inexpensive—only a small amount of oil is necessary to treat dull or damaged areas.
Completely sanding your wood surface is not necessary, which saves you time and money.

Linseed oil must be applied to unvarnished wood, otherwise the oil will fail to deeply penetrate the wood surface.
Because linseed oil is a wood-penetrating solution, it nourishes your wood surfaces while sealing, staining, and finishing them at the same time.
Linseed oil is rich in alpha-linolenic acid (ALA), an omega-3 fatty acid.

As a dietary supplement, Linseed Oil is often consumed for its potential health benefits, including supporting heart health and reducing inflammation.
Linseed Oil is available in both liquid and capsule forms.
Linseed Oil is commonly used as a drying oil in the production of paints and coatings.

Linseed Oil is particularly valued in oil-based paints because it polymerizes (hardens) when exposed to air, forming a solid, protective film.
This property makes it suitable for use in both artistic and industrial paints.
Linseed Oil is used in wood finishing to protect and enhance the appearance of wooden surfaces.

Linseed Oil can be applied to wooden furniture, floors, and other items to provide a protective, glossy finish.
Artists often use linseed oil as a medium for oil painting.
Linseed Oil can be mixed with pigments to create oil paints with various viscosities and drying times, allowing artists to work with different techniques.

Linseed Oil can be found in cosmetics and personal care products, such as lotions, moisturizers, and hair conditioners.
Linseed Oil is valued for its moisturizing and skin-nourishing properties.
Linseed Oil is used as a dietary ingredient in traditional dishes.

Ground flaxseeds and linseed oil may be added to foods for their nutritional value.
Linseed Oil has been used in machinery and mechanical applications, including lubrication.

However, its use for this purpose has declined with the availability of more advanced lubricants.
Beyond Linseed Oil is potential dietary benefits, linseed oil is also used in complementary and alternative medicine for various purposes, including natural remedies for conditions like constipation and inflammation.

Melting point: -24.0℃
Boiling point: >316 °C
Density: 0.93 g/mL at 25 °C(lit.)
refractive index: n20/D 1.4795(lit.)
Flash point: >230 °F
storage temp.: room temp
form: neat
Odor: bland
Stability: Stable, but polymerizes gradually upon exposure to air. Combustible. Incompatible with strong oxidizing agents. Reacts violently with chlorine. Material such as rags impregnated with linseed oil may spontaneously combust after a long induction period due to gradual exothermic reaction with oxygen.
Indirect Additives used in Food Contact Substances: LINSEED OIL
FDA 21 CFR: 181.26
EWG's Food Scores: 1

Linseed Oil is known for its potential health benefits. It is a good source of alpha-linolenic acid (ALA), which is an omega-3 fatty acid.
ALA has been associated with a reduced risk of heart disease and may help lower blood pressure and cholesterol levels.
Some people take linseed oil as a dietary supplement for these potential health benefits.

Linseed Oil has been used as a natural remedy for digestive issues. It may help alleviate constipation when consumed, particularly when taken with water.
Linseed Oil is not suitable for cooking due to its low smoke point, there are some processed varieties known as "linseed oil varnish" that have a higher smoke point.
These are used for coating cookware, providing a non-stick surface, and for seasoning cast iron pans.

In addition to its use in cosmetics and personal care products, linseed oil is sometimes applied topically to the skin to soothe dryness and skin irritations.
Linseed Oil can be used as a natural moisturizer.
Linseed oil is a good source of polyunsaturated fats, particularly omega-3 fatty acids, but it is also high in calories.

Linseed Oil is important to consume it in moderation as part of a balanced diet.
Linseed oil is closely related to ground flaxseeds. Ground flaxseeds are also a popular dietary addition, and they provide similar nutritional benefits, including fiber and omega-3 fatty acids.
They can be added to foods like yogurt, cereal, or smoothies.

There are different varieties of linseed oil, including cold-pressed, expeller-pressed, and refined varieties.
Cold-pressed linseed oil is often considered a higher-quality option because it is produced without the use of heat, which can help preserve more of the oil's natural flavor and nutrients.
Some individuals may be allergic to linseed oil.

Linseed oil is susceptible to oxidation and can become rancid if not stored properly.
Linseed Oil should be kept in a cool, dark place and refrigerated if possible to extend its shelf life.
Linseed Oil is used as an ingredient in traditional dishes.

Linseed Oil may be drizzled over salads or used as a dressing for various culinary preparations.
Linseed oil can be applied to wood without the need for complex surface prep.
Linseed Oil’s an ecological and natural alternative to varnish on both indoor and outdoor surfaces owing to its protective properties.

In fact, in terms of quality and cost, Linseed Oil is probably the most attractive alternative wood oil product on the market.
Linseed oil is useful for protecting wood surfaces, but it is not a paint.
Linseed Oil has waterproofing capacity, but it does not protect from dirt or intense sunlight (though some manufacturers add UV protection to their formulations).

Linseed oil works well on wood with a natural or rustic finish and on exotic woods, and it holds up on poorly maintained wood and wood that is exposed to high levels of friction.
Linseed Oil react with acids to liberate heat.
Heat is also generated by interaction with caustic solutions.

Strong oxidizing acids may cause a vigorous reaction that is sufficiently exothermic to ignite the reaction products.
Flammable hydrogen is generated by mixing with alkali metals and hydrides.
React with oxygen in the air to harden.

Can react with air fast enough to cause ignition of near-by combustible material if the heat builds up in an unventilated space (called "spontaneous combustion" in oily rags).
Linseed oil, also called flaxseed oil, edible and industrial vegetable oil made from the seeds of the flax plant (Linum usitatissimum).

Flaxseeds and food-grade linseed oil (called flaxseed oil in some places) are considered to have health benefits and are ingested as a food.
Lower quality linseed oil, which typically has a less pleasant flavour and smell, is used for a variety of industrial purposes.

Uses:
The botanical properties of linseed oil are listed as emollient, antiinflammatory, and healing.
Derived from the flax plant seed, the oil is obtained by expression with little or no heat.
Linseed oil is a drying oil, meaning it can oxidise into a solid form.

Due to this property, linseed oil is used on its own or blended with other oils, resins, and solvents as an impregnator and varnish in wood finishing, as a pigment binder in oil paints, as a plasticizer and hardener in putty, and in the manufacture of linoleum.
Linseed oil is still widely used for the finishing and refinishing of furniture and timber products.

Most applications of linseed oil exploit its drying properties, i.e., the initial material is liquid or at least pliable and the aged material is rigid but not brittle.
The water-repelling (hydrophobic) nature of the resulting hydrocarbon-based material is advantageous.
Linseed oil is the carrier used in oil paint.

Linseed Oil can also be used as a painting medium, making oil paints more fluid, transparent and glossy.
Linseed Oil is available in varieties such as cold-pressed, alkali-refined, sun-bleached, sun-thickened, and polymerised (stand oil).
The introduction of linseed oil was a significant advance in the technology of oil painting.

Traditional glazing putty, consisting of a paste of chalk powder and linseed oil, is a sealant for glass windows that hardens within a few weeks of application and can then be painted over.
The durability of putty is owed to the drying properties of linseed oil.
When used as a wood finish, linseed oil dries slowly and shrinks little upon hardening.

A linseed oil finish is easily scratched and liquid water penetrates a linseed oil finish in mere minutes, and water vapour bypasses it almost completely.
Garden furniture treated with linseed oil may develop mildew.
Oiled wood may be yellowish and is likely to darken with age.

Even though the oil feels dry to the touch, studies show linseed oil does not fully cure.
Linseed oil is a common finish for wooden items, though very fine finish may require months to obtain.
Studies show the fatty-acid structure of linseed oil has problems cross-linking and oxidizing, frequently turning black.

Boiled linseed oil is used as sizing in traditional oil gilding to adhere sheets of gold leaf to a substrate (parchment, canvas, Armenian bole, etc.).
Linseed Oil has a much longer working time than water-based size and gives a firm smooth surface that is adhesive enough in the first 12–24 hours after application to cause the gold to attach firmly to the intended surface.
Linseed oil is used to bind wood dust, cork particles, and related materials in the manufacture of the floor covering linoleum.

After its invention in 1860 by Frederick Walton, linoleum, or "lino" for short, was a common form of domestic and industrial floor covering from the 1870s until the 1970s, when it was largely replaced by PVC ("vinyl") floor coverings.
However, since the 1990s, linoleum is returning to favor, being considered more environmentally sound than PVC.
Linoleum has given its name to the printmaking technique linocut, in which a relief design is cut into the smooth surface and then inked and used to print an image.

The results are similar to those obtained by woodcut printing.
Linseed oil is consumed as a dietary supplement due to its high content of alpha-linolenic acid (ALA), an omega-3 fatty acid.
Linseed Oil is often taken in capsule form or added to foods and beverages to support heart health and provide anti-inflammatory benefits.

Artists use linseed oil as a medium for oil painting. It is mixed with pigments to create oil paints with various viscosities and drying times, allowing artists to work with different techniques and achieve desired effects.
Linseed oil is used to finish and protect wooden surfaces, such as furniture, floors, and woodworking projects.
Linseed Oil enhances the natural beauty of the wood and provides a protective finish.

In the industrial sector, linseed oil is used as a drying oil in the production of oil-based paints, varnishes, and coatings.
Linseed Oil polymerizes when exposed to air, forming a solid and durable film.
Linseed oil is an ingredient in cosmetic and personal care products like lotions, moisturizers, and hair conditioners.

Linseed Oil is valued for its skin-nourishing and moisturizing properties.
Some people use linseed oil for seasoning and maintaining cast iron cookware, creating a non-stick surface and protecting the cookware from rust.
In some cultures, linseed oil is used as an ingredient in traditional dishes.

Linseed Oil is drizzled over salads or added to various culinary preparations to provide its nutritional benefits.
Linseed oil is sometimes used in complementary and alternative medicine for its potential health benefits, such as reducing inflammation and supporting digestive health.
Ground flaxseeds and linseed oil are sources of essential nutrients, including fiber, omega-3 fatty acids, and lignans.

They are used as nutritional ingredients in a variety of foods, from cereals to smoothies.
A processed variety known as "linseed oil varnish" with a higher smoke point is used for coating cookware, providing a non-stick surface, and seasoning cast iron pans.
Linseed oil is sometimes applied topically to the skin to soothe dryness and skin irritations.

Linseed Oil serves as a natural moisturizer and can be found in skincare products.
Linseed Oil was used for lubrication in machinery and mechanical applications.
However, its use for this purpose has decreased with the availability of more advanced lubricants.

Linseed Oil is often used by woodworkers to create a protective finish on wooden items, such as cutting boards, bowls, and wooden furniture.
Linseed Oil enhances the grain and color of the wood while providing durability.
In historical restoration projects, linseed oil is used to maintain and preserve antique wooden objects and structures.

Linseed Oil can help revitalize and protect old wood surfaces.
Linseed oil has been used to seal and protect natural fibers such as hemp, jute, and sisal.
This application is common in the production of natural fiber ropes and twine.

Linseed oil can be used to seal and protect concrete and masonry surfaces.
Linseed Oil can help reduce water absorption and extend the life of these structures.
In antique restoration and preservation, linseed oil is sometimes used to restore and rejuvenate old leather items, such as saddles, boots, and vintage leather furniture.

In gilding, linseed oil can be used as an adhesive for applying gold or metal leaf to various surfaces, creating a decorative effect.
In holistic and natural medicine, linseed oil has been used for various remedies, including soothing minor skin irritations, promoting hair health, and addressing minor gastrointestinal discomfort.
Linseed oil is sometimes added to animal feed as a dietary supplement for livestock to improve their coat quality and overall health.

Linseed Oil can also be used in pet care products to promote healthy skin and fur.
Historically, linseed oil was used as a fuel for oil lamps, often with added colorants or fragrances.

This application has largely been replaced by more modern fuels.
In traditional crafts and folk art, linseed oil may be used for various purposes, such as weatherproofing handwoven baskets or creating handcrafted items.

Fire Hazard:
Linseed oil is flammable.
If used and stored correctly, there is very little risk of linseed oil spontaneously combusting.
However, the fire hazard increases under certain circumstances.

Be very careful with rags that have been used to apply linseed oil.
In many cases of spontaneous combustion of drying oils the cause has been a pile of oil soaked rags.
As the oil oxidizes it generates heat.

The rags act as an insulator, allowing the heat to build up until the cloth smokes and eventually ignites.
The bigger the pile, the greater the possible heat and the greater the risk.
Linseed Oil used rags should be stored in a metal can with a top and soaked with water to limit the risk of fire since the drying process is exothermic.

Safety Profile:
Linseed oil is non-toxic and completely food-safe.
Linseed Oil is often given as a health supplement in both people and animals, including dogs, horses, and more.
Linseed oil is a drying oil, and it can undergo a chemical reaction with oxygen when exposed to air, which generates heat.

This process can lead to spontaneous combustion if linseed oil-soaked rags or materials are improperly stored or disposed of.
To avoid this hazard, used rags should be spread out to dry in a well-ventilated area or stored in a sealed, airtight container filled with water.
Linseed oil is flammable and should be kept away from open flames, sparks, or other sources of ignition.

Linseed Oil should also be stored in a cool, dry place away from direct sunlight.
Some individuals may be sensitive or allergic to linseed oil, particularly when it comes into contact with the skin.
Skin contact with linseed oil may lead to contact dermatitis in susceptible individuals.

Synonyms
Linseed Oil
8001-26-1
Flaxseed Oil
84XB4DV00W
Fats and Glyceridic oils, flaxseed
Fats and Glyceridic oils, linseed
Flax oil
Groco
L-310
Linseed oil, bleached
Oils, glyceridic, flaxseed or linseed
Aceite de Linaza
Acid refined linseed oil
Acidulated linseed soapstock
Bodied linseed oil
Huile de Lin
Leinol
Linseed absolute
Linseed fatty acids, glycerin ester
Linseed oil absolute
Linseed oil extract
Linseed oil fatty acids, glycerol triester
Linseed oil, alkali refined
Linseed oil, wash recovered
Linum Usitatissimum (Linseed) Seed Oil
Oleum Lini
Scan-Oil
B1700
Caswell No. 527A
DTXSID2025507
EINECS 232-278-6
EPA Pesticide Chemical Code 031603
FLAX SEED OIL (USP-RS)
HSDB 5155
LINSEED OIL (MART.)
LINSEED SEED OIL
Oil, Flaxseed
Oil, Linseed
Oils, linseed
SOLIN OIL
UNII-84XB4DV00W

LIPASE IUPAC Name 8-anilinonaphthalene-1-sulfonic acid LIPASE InChI InChI=1S/C16H13NO3S/c18-21(19,20)15-11-5-7-12-6-4-10-14(16(12)15)17-13-8-2-1-3-9-13/h1-11,17H,(H,18,19,20) LIPASE InChI Key FWEOQOXTVHGIFQ-UHFFFAOYSA-N LIPASE Canonical SMILES C1=CC=C(C=C1)NC2=CC=CC3=C2C(=CC=C3)S(=O)(=O)O LIPASE Molecular Formula C16H13NO3S LIPASE CAS 82-76-8 LIPASE Related CAS 1445-19-8 (mono-hydrochloride) LIPASE Deprecated CAS 54784-66-6 LIPASE European Community (EC) Number 201-438-7 LIPASE NSC Number 1746 LIPASE UNII 630I4V6051 LIPASE DSSTox Substance ID DTXSID7058882 LIPASE 1-anilino-8-naphthalenesulfonic acid Property Name Property Value Reference LIPASE Molecular Weight 299.3 g/mol LIPASE XLogP3-AA 3.5 LIPASE Hydrogen Bond Donor Count 2 LIPASE Hydrogen Bond Acceptor Count 4 LIPASE Rotatable Bond Count 3 LIPASE Exact Mass 299.061614 g/mol LIPASE Monoisotopic Mass 299.061614 g/mol LIPASE Topological Polar Surface Area 74.8 Ų LIPASE Heavy Atom Count 21 LIPASE Formal Charge 0 LIPASE Complexity 439 LIPASE Isotope Atom Count 0 LIPASE Defined Atom Stereocenter Count 0 LIPASE Undefined Atom Stereocenter Count 0 LIPASEDefined Bond Stereocenter Count 0 Undefined Bond Stereocenter Count 0 LIPASE Covalently-Bonded Unit Count 1 LIPASE Compound Is Canonicalized Yes LIPASE Hazard Classes and Categories Acute Tox. 4 (78.57%) Skin Irrit. 2 (21.43%) Eye Irrit. 2 (100%) STOT SE 3 (14.29%) Lipase A computer-generated image of a type of pancreatic lipase (PLRP2) from the guinea pig. PDB: 1GPL​.A lipase (/ˈlaɪpeɪs/, /-peɪz/) is any enzyme that catalyzes the hydrolysis of fats (lipids).Lipases are a subclass of the esterases.Lipases perform essential roles in digestion, transport and processing of dietary lipids (e.g. triglycerides, fats, oils) in most, if not all, living organisms. Genes encoding lipases are even present in certain viruses.Most lipases act at a specific position on the glycerol backbone of a lipid substrate (A1, A2 or A3)(small intestine). For example, human pancreatic lipase (HPL), which is the main enzyme that breaks down dietary fats in the human digestive system, converts triglyceride substrates found in ingested oils to monoglycerides and two fatty acids.Several other types of lipase activities exist in nature, such as phospholipases and sphingomyelinases; however, these are usually treated separately from "conventional" lipases.Some lipases are expressed and secreted by pathogenic organisms during an infection. In particular, Candida albicans has many different lipases, possibly reflecting broad-lipolytic activity, which may contribute to the persistence and virulence of C. albicans in human tissue. Contents 1.Structure and catalytic mechanism -> LIPASE 2.Physiological distribution -> LIPASE 3.Human lipases -> LIPASE 4.Industrial uses -> LIPASE 5.Diagnostic use -> LIPASE 6.Medical use -> LIPASE 7.Additional images -> LIPASE 8.See also -> LIPASE 9.References -> LIPASE 10.External links -> LIPASE Structure and catalytic mechanism -> LIPASE A diverse array of genetically distinct lipase enzymes are found in nature, and they represent several types of protein folds and catalytic mechanisms. However, most are built on an alpha/beta hydrolase fold and employ a chymotrypsin-like hydrolysis mechanism using a catalytic triad consisting of a serine nucleophile, a histidine base, and an acid residue, usually aspartic acid. Physiological distribution -> LIPASE Lipases are involved in diverse biological processes which range from routine metabolism of dietary triglycerides to cell signaling and inflammation.Thus, some lipase activities are confined to specific compartments within cells while others work in extracellular spaces.In the example of lysosomal lipase, the enzyme is confined within an organelle called the lysosome.Other lipase enzymes, such as pancreatic lipases, are secreted into extracellular spaces where they serve to process dietary lipids into more simple forms that can be more easily absorbed and transported throughout the body.Fungi and bacteria may secrete lipases to facilitate nutrient absorption from the external medium (or in examples of pathogenic microbes, to promote invasion of a new host).Certain wasp and bee venoms contain phospholipases that enhance the effects of injury and inflammation delivered by a sting.As biological membranes are integral to living cells and are largely composed of phospholipids, lipases play important roles in cell biology.Malassezia globosa, a fungus thought to be the cause of human dandruff, uses lipase to break down sebum into oleic acid and increase skin cell production, causing dandruff. Human lipases -> LIPASE The main lipases of the human digestive system are pancreatic lipase (PL) and pancreatic lipase related protein 2 (PLRP2), which are secreted by the pancreas. Humans also have several related enzymes, including hepatic lipase, endothelial lipase, and lipoprotein lipase. Not all of these lipases function in the gut (see table).Name Gene Location Description Disorder bile salt-dependent lipase BSDL pancreas, breast milk aids in the digestion of fats pancreatic lipase PNLIP digestive juice In order to exhibit optimal enzyme activity in the gut lumen, PL requires another protein, colipase, which is also secreted by the pancreas.lysosomal lipase LIPA interior space of organelle: lysosome Also referred to as lysosomal acid lipase (LAL or LIPA) or acid cholesteryl ester hydrolase Cholesteryl ester storage disease (CESD) and Wolman disease are both caused by mutations in the gene encoding lysosomal lipase.[18]hepatic lipase LIPC endothelium Hepatic lipase acts on the remaining lipids carried on lipoproteins in the blood to regenerate LDL (low density lipoprotein).lipoprotein lipase LPL or "LIPD" endothelium Lipoprotein lipase functions in the blood to act on triacylglycerides carried on VLDL (very low density lipoprotein) so that cells can take up the freed fatty acids. Lipoprotein lipase deficiency is caused by mutations in the gene encoding lipoprotein lipase. hormone-sensitive lipase LIPE intracellular gastric lipase LIPF digestive juice Functions in the infant at a near-neutral pH to aid in the digestion of lipids endothelial lipase LIPG endothelium - -pancreatic lipase related protein 2 PNLIPRP2 or "PLRP2" - digestive juice - pancreatic lipase related protein 1 PNLIPRP1 or "PLRP1" digestive juice Pancreatic lipase related protein 1 is very similar to PLRP2 and PL by amino acid sequence (all three genes probably arose via gene duplication of a single ancestral pancreatic lipase gene). However, PLRP1 is devoid of detectable lipase activity and its function remains unknown, even though it is conserved in other mammals. -lingual lipase ? saliva Active at gastric pH levels. Optimum pH is about 3.5-6. Secreted by several of the salivary glands (Ebner's glands at the back of the tongue (lingua), the sublingual glands, and the parotid glands) -Other lipases include LIPH, LIPI, LIPJ, LIPK, LIPM, LIPN, MGLL, DAGLA, DAGLB, and CEL. There also are a diverse array of phospholipases, but these are not always classified with the other lipases. Industrial uses -> LIPASE Lipases serve important roles in human practices as ancient as yogurt and cheese fermentation. However, lipases are also being exploited as cheap and versatile catalysts to degrade lipids in more modern applications. For instance, a biotechnology company has brought recombinant lipase enzymes to market for use in applications such as baking, laundry detergents and even as biocatalysts in alternative energy strategies to convert vegetable oil into fuel. High enzyme activity lipase can replace traditional catalyst in processing biodiesel, as this enzyme replaces chemicals in a process which is otherwise highly energy intensive, and can be more environmentally friendly and safe. Industrial application of lipases requires process intensification for continuous processing using tools like continuous flow microreactors at small scale. Lipases are generally animal sourced, but can also be sourced microbially[citation needed]. Diagnostic use -> LIPASE Blood tests for lipase may be used to help investigate and diagnose acute pancreatitis and other disorders of the pancreas. Measured serum lipase values may vary depending on the method of analysis. Medical use -> LIPASE Lipase can also assist in the breakdown of fats into lipids in those undergoing pancreatic enzyme replacement therapy (PERT). It is a key component in Sollpura (Liprotamase). Additional images -> LIPASE Lipase is an enzyme that breaks down triglycerides into free fatty acids and glycerol. Lipases are present in pancreatic secretions and are responsible for fat digestion. There are many different types of lipases; for example, hepatic lipases are in the liver, hormone-sensitive lipases are in adipocytes, lipoprotein lipase is in the vascular endothelial surface, and pancreatic lipase in the small intestine. Understanding lipase is crucial for understanding the pathophysiology of fat necrosis and is clinically significant in the understanding of acute and chronic pancreatitis. The role of lipase is also crucial in the mechanism of some medications indicated for lowering cholesterol. This review will explore the function, pathophysiology, and clinical significance of the lipase enzyme. Molecular The lipase group of enzymes is built on alpha and beta hydrolase folds. They work by employing chymotrypsin-like hydrolysis, which uses a histidine base, a serine nucleophile, and aspartic acid. Function -> LIPASE Lipase is an enzyme that breaks down triglycerides into free fatty acids and glycerol. Lipases are present in pancreatic secretions and are responsible for fat digestion. Lipases are enzymes that play a crucial role in lipid transport. There are many different types of lipases; hepatic lipases are in the liver, hormone-sensitive lipases are in adipocytes, lipoprotein lipase is in the vascular endothelial surface, and pancreatic lipase is in the small intestine, each serving individual functions. Hepatic lipase in the liver is responsible for degrading the triglycerides that remain in intermediate density lipoprotein (IDL). Hormone-sensitive lipase is found within fat tissue and is responsible for degrading the triglycerides that are stored within adipocytes. Lipoprotein lipase is found on the vascular endothelial surface and is responsible for degrading triglycerides that circulating from chylomicrons and VLDLs. Pancreatic lipase is found within the small intestine and is responsible for degrading dietary triglycerides. Hepatic lipase plays a crucial role in the formation and delivery of low-density lipoprotein(LDL). LDL is formed by the modification of intermediate density lipoprotein in the peripheral tissue and liver by hepatic lipase. These LDL particles are taken up, or endocytosed, via receptor-mediated endocytosis by target cell tissue. LDL serves to ultimately transport cholesterol from the liver to peripheral tissue. Pathophysiology -> LIPASE Fat necrosis occurs enzymatically and non-enzymatically. In acute pancreatitis, saponification of peripancreatic fat occurs. During traumatic events, such as physical injury in breast tissue, non-enzymatic fat necrosis takes place. This is due to the damage to fat cells causing the release of lipase, leading to triglyceride breakdown, and causing the release of fatty acids. These fatty acids are charged negatively and once released in the bloodstream, bind to positively charged calcium ions. This process of salt formation between negatively charged fatty acids and positively charged calcium ions is called saponification.Histologically, saponified cells appear as dead fat cells outlining the tissue, which do not contain peripheral nuclei. Saponification of the fatty acid and calcium ion combined on hematoxylin and eosin staining appears dark blue. Clinical Significance -> LIPASE High levels of serum lipase may be indicative of pancreatitis. In the case of acute pancreatitis, diagnosis is based on results with two of the three criteria. The criteria used for diagnosis include acute epigastric pain radiating to the back, increased serum amylase, or increased lipase levels which are up to three times the upper limit of normal serum lipase levels. The latter is a more specific diagnostic marker than amylase or imaging with CT or MRI. Acute pancreatitis is due to autodigestion of pancreas by pancreatic enzymes, causing surrounding edema around the pancreas. Causes of this pathology include excessive ethanol use, gallstones, trauma, mumps, steroids, autoimmune disease, hypertriglyceridemia with levels above 1000 mg/dL, hypercalcemia, ERCP, Scorpion sting, or drugs such as nucleoside reverse transcriptase inhibitors, protease inhibitors, or sulfa drugs. Acute pancreatitis can lead to complications including pseudocyst, in which the pancreatic lining is composed of granulation tissue rather than epithelium, necrosis, abscess, infection, hemorrhage, hypocalcemia precipitation of calcium soaps, or organ failure including acute respiratory distress syndrome, shock, or renal failure. Elevated serum levels of lipase and amylase may or may not also be present in chronic pancreatitis, in contrast to acute pancreatitis where serum lipase is almost always elevated. Chronic pancreatitis is due to chronic inflammation, calcification, and atrophy of the pancreas. The primary causes of this pathology include chronic alcohol abuse in adults and genetic predisposition such as cystic fibrosis in children. It can also be due to idiopathic causes. Complications of chronic pancreatitis include deficiency of pancreatic enzymes and pseudocysts. Pancreatic insufficiency usually occurs when there is less than ten percent of pancreatic function remaining, due to a deficiency in pancreatic enzymes contained within the pancreas to digest fats such as lipase. This pancreatic enzyme deficiency leads to clinical manifesions of steatorrhea, as fat is not absorbed properly in the small intestine and it is instead excreted. Because of this inability to absorb fats properly, this can also clinically manifest as fat-soluble vitamin deficiency of vitamins A, D, E, and K. Pancreatic insufficiency can also lead to diabetes mellitus, due to lack of sufficient insulin release from pancreatic tissue. Clinically, orlistat is a medication used for weight loss that acts on lipase. Specifically, this medication inhibits pancreatic and gastric lipases. This inhibition of lipase leads to reduced breakdown and absorption of dietary fats. This can lead to side effects as a consequence of decreased absorption of fats, such as decreased absorption of fat-soluble vitamins A, D, E, and K. Side effects also include abdominal pain, frequent bowel movements or bowel urgency, and flatulence.Some cholesterol-lowering medications act on lipases. Fibrates, such as bezafibrate, gemfibrozil, and fenofibrate, work by activating Peroxisome prolifeator-activated receptor alpha(PPAR-alpha), and upregulating lipoprotein lipase, which leads to a decrease in serum triglyceride levels along with induction of increased synthesis of HDL. Fibrates are clinically indicated primarily for lowering triglycerides. Side effects of fibrates include cholesterol gallstones, rhabdomyolysis, especially if used with statins, and increased LDL.Niacin, or vitamin B3, is another cholesterol-lowering medication that acts on lipase. Specifically, lipase acts to inhibit hormone-sensitive lipase, which leads to inhibition of VLDL synthesis in the liver. Niacin is clinically indicated primarily for increasing HDL levels. Side effects erythema and flushing of the upper body, increased glucose levels, increased uric acid levels, acanthosis nigricans, and pruritus.A lipase test measures the level of a protein called lipase in your blood.Lipase helps your body absorb fats. It's released by the pancreas, a long, flat gland between your stomach and spine.When your pancreas is inflamed or injured, it releases more lipase than usual. Your doctor may want to find out the level of this protein in your blood to find how your pancreas is doing.A lipase test may also be referred to as a serum lipase or LPS. What Conditions Can This Test Find? A doctor will order a lipase test if she suspects that you may have acute pancreatitis -- an inflammation of the pancreas that causes abdominal pain.The following symptoms can be a sign of pancreas inflammation:Severe abdominal or back pain,Fever,Loss of appetite,Nausea The test may also be used to monitor your pancreas if you've already been diagnosed with acute (sudden, severe) or chronic (ongoing) pancreatitis. It can find out whether lipase levels are increasing or decreasing. It can also be used to find out whether a treatment is working well.Sometimes, a lipase test will also be used to monitor other conditions including:Peritonitis (inflammation of the lining of your inner abdominal wall) Strangulated or infarcted bowel (bowel that has restricted blood supply) Pancreatic cyst Cystic fibrosis (an inherited disease in which thick mucus can damage organs) Crohn's disease (inflammation of your digestive tract) Celiac disease (triggered by the protein gluten, your immune system attacks your small intestine) How Do I Prepare? If you have a lipase test scheduled ahead of time, you'll need to fast.You'll likely be asked to stop eating or drinking anything other than water for 8 to 12 hours beforehand.Your doctor may also ask you to stop taking some medications that can affect the test results. Be sure she knows all the prescription medications, over-the-counter meds, and supplements you take. What Happens During a Test? In a lipase test, a lab tech will take a small blood sample. He will likely put a band around your upper arm to help make your veins easier to find.He will then insert a needle into one of your veins. After enough blood goes into a tube, the band will come off and he'll take out the needle. He'll put a bandage on where the needle went in. What Do the Results Mean? A high level of lipase in the blood indicates that you may have a condition affecting the pancreas.Normal levels vary slightly between labs, so you and your doctor will look at the ranges given with your results to figure out how your lipase levels compare with the normal.In acute pancreatitis, levels are often 5 to 10 times higher than the highest reference value. Other conditions can also cause slightly increased lipase levels, including: Lipase Tests Email this page to a friend Print Facebook Twitter Pinterest What is a lipase test? Lipase is a type of protein made by your pancreas, an organ located near your stomach. Lipase helps your body digest fats. It's normal to have a small amount of lipase in your blood. But, a high level of lipase can mean you have pancreatitis, an inflammation of the pancreas, or another type of pancreas disease. Blood tests are the most common way of measuring lipase. Other names: serum lipase, lipase, LPS What is it used for? A lipase test may be used to: Diagnose pancreatitis or another disease of the pancreas Find out if there is a blockage in your pancreas Check for chronic diseases that affect the pancreas, including cystic fibrosis Why do I need a lipase test? You may need a lipase test if you have symptoms of a pancreas disease. These include: Nausea and vomiting Diarrhea Severe back pain Severe abdominal pain Fever Loss of appetite You may also need a lipase test if you certain risk factors for pancreatitis. These include: A family history of pancreatitis Diabetes Gallstones High triglycerides Obesity You may also be at a higher risk if you are a smoker or heavy alcohol user. What happens during a lipase test? A lipase test is usually in the form of a blood test. During a blood test, a health care professional will take a blood sample from a vein in your arm, using a small needle. After the needle is inserted, a small amount of blood will be collected into a test tube or vial. You may feel a little sting when the needle goes in or out. This usually takes less than five minutes.Lipase can also be measured in urine. Usually, a lipase urine test can be taken at any time of day, with no special preparation needed. Will I need to do anything to prepare for the test? You may need to fast (not eat or drink) for 8-12 hours before a lipase blood test. If your health care provider has ordered a lipase urine test, be sure to ask if you need to follow any special instructions. Are there any risks to the test? There is very little risk to having a blood test. You may have slight pain or bruising at the spot where the needle was put in, but most symptoms go away quickly.There are no known risks to a urine test. What do the results mean? A high level of lipase may indicate: Pancreatitis A blockage in the pancreas Kidney disease Peptic ulcer A problem with your gall bladder A low level of lipase may mean there is damage to cells in the pancreas that make lipase. This happens in certain chronic diseases such as cystic fibrosis.If your lipase levels are not normal, it doesn't necessarily mean you have a medical condition needing treatment. Certain medicines, including codeine and birth control pills, can affect your lipase results. If you have questions about your lipase test results, talk to your health care provider. Is there anything else I need to know about a lipase test? A lipase test is commonly used to diagnose pancreatitis. Pancreatitis can be acute or chronic. Acute pancreatitis is a short-term condition that usually goes away after a few days of treatment. Chronic pancreatitis is a long-lasting condition that gets worse over time. But it can be managed with medicine and lifestyle changes, such as quitting drinking. Your health care provider may also recommend surgery to repair the problem in your pancreas. Lipase lipase (CSL) came out with the highest catalytic activity, thereby suggesting that the catalytic activities depend mainly on the lipase origin. Uses Most people do not need additional lipase. However, people with the following conditions may find lipase supplements helpful. Precautions Side effects may include nausea and stomach upset. High doses of lipase may exacerbate symptoms of cystic fibrosis. Scientists do not know enough about the effects of lipase during pregnancy or breastfeeding, so speak with your doctor before taking lipase. Lipases (triacylglycerol hydrolases E.C. 3.1.1.3) are enzymes that catalyze the hydrolysis of triacylglycerols (TAGs) to glycerol and fatty acids (FAs). Lipases, together with amylases and proteases, constitute the three major known digestive enzymes. Plants, animals, and microorganisms produce lipases. Animal lipases are found in several different organs, such as the pancreas and digestive tract. Recently, increasingly more attention is being paid to lipases produced by bacteria and fungi. Microbial lipases are relatively stable and are capable of catalyzing a variety of reactions; they are of potential importance for diverse industrial applications. In recent years, information on the mechanistic properties of lipases has become available. In contrast to proteases, lipases share the common feature that the active site is buried in the protein. The lipase-active site is covered by a short amphipathic helix or ‘lid’ of two nearly parallel amphiphathic helices. The lid moves away upon interaction with the substrate. It has been proposed that this conformational change results in the activation of these enzymes at an oil–water interface. Lipases can be defined as esterases that are able to catalyze the hydrolysis of long-chain TAGs. Lipases have been used as an ingredient in detergents, and an immobilized 1,3-position-specific lipase was applied for the industrial production of cocoa butter substitute using a fixed-bed bioreactor. The use of lipases has been increasing steadily in the oil and fat industry.Lipases are water-soluble, ester hydrolases that are traditionally defined by their marked preference for apolar, water-insoluble ester substrates. This group of enzymes also includes species referred to as cholesterol esterases. Lipases and cholesterol esterases are distinguished from phospholipases that catalyze the hydrolysis of acyl ester bonds of highly amphipathic phospholipids having an sn-glycero-3-phospho-X moiety and from carboxylesterases that hydrolyze polar, water-soluble esters. These distinctions are relative, however, because some lipases exhibit activity toward phospholipids or soluble esters. Typical natural lipase substrates include, in order of amphipathicity, long aliphatic chain acyl esters of cholesterol (cholesteryl esters), triacyl esters of glycerol (triacylglycerols), acyl esters of long chain alcohols (wax esters), diacyl esters of glycerol (diacylglycerols), and monoacyl esters of glycerol. Because lipase substrates tend to be oily and only weakly amphipathic, they reside primarily in a bulk oil phase in preference to the aqueous phase or to the interface, that is, monomolecular surface phase that separates the bulk oil and aqueous phases. It follows, because lipases are water-soluble enzymes, that the site of lipolysis is the quasi-two-dimensional interface. The focus of basic research on lipases has been to understand how a reaction involving such a change in dimensionality can occur and how it is regulated. Medically, lipases are targets for therapeutic intervention in the treatment of obesity. The focus of applied research with lipases has been to exploit the unusual properties of lipolytic systems for the production of chiral pharmaceuticals, improved detergents, and designer fats.All lipases except BSL and RML were dissolved in distilled water, centrifuged to remove insoluble matter, dialysed against distilled water for three days at 4°C and lyophilised prior to use (crude lipase preparations). Under these conditions no loss of enzymatic activity occurred. BSL was dialysed against 10 mM glycine buffer pH 10 to prevent precipitation. Because RML contains cellulases it was passed over a PD-10 column for desalting.In the dairy industry, lipases are applied to hydrolyze the fats in milk and to impart pleasant flavors to cheeses. The characteristic flavor is the result of fatty acids produced from the free fat released during milk hydrolysis (Jooyandeh et al., 2009). Lipases of microbial and animal origin are used in several enzyme companies. Lipases from animals are processed from lambs and calves, but microbial production of lipase is mainly by bacteria and the fungal sp. Rhizomucor meihei. Both animal and microbial lipases have varied mechanisms of action and food companies use both based on the required cheese flavor.Lipase can be classified into three different classes based on its positional and fatty acid specificity. Most of the lipases belong to sn-1,3 specific lipase. These lipases hydrolyse/esterify fatty acid specifically at the either/both sn-1 and sn-3 position. The sn-2 fatty acids are prevented from binding to the active site of lipase due to steric hindrance effect. Example of this group of lipase includes human pancreatic lipase, Aspergillus niger, Rhizomucor delemar, Rhizomucor miehei, and Mucor javanicus. Meanwhile, another group of lipase which belongs to non-specific lipase catalyses the hydrolysis/esterification of fatty acid in a random manner regardless of its position. Examples of these lipases are Candida rugosa, Corynebacterium acnes, Staphylococcus aureus. Additionally, lipases showing fatty acid specificity is much less common compared to other groups of lipases. Geotrichum candidum is the most common fatty acid specific lipase that shows preferences toward oleic acid. There are also lipases which show negative specificity. For instance, lipase from Candida cylindracea which discriminates against docosahexanoic acid, G. candidum against γ-linolenate in borage oil and Mucor miehei against polyunsaturated fatty acid GLA and DHA. Lipases of negative selectivity are often being utilized to concentrate and enrich certain polyunsaturated fatty acid (PUFA) in TAG.Lipase is an enzyme produced, either extra- or intracellular, by microorganisms such as fungi and bacteria, animals, and plants [4]. Lipase is regioselective as it can hydrolyze triglycerides at R1 and R3, only R2, or nonspecifically. It also has substrate specificity in that the enzyme can differentiate between acyl chains attached to the glycerol, preferentially cleaving certain types [4]. For the production of biodiesel, either extra- or intracellular lipases can be used. Extracellular lipases are the most commonly studied; they are often immobilized on carriers for industrial use [4]. This attachment to carriers allows them to be recovered and recycled.Lipases catalyze the hydrolysis of ester bonds in lipid substrates and play a vital role in digestion and the transport and processing of dietary lipids substrate (Svendsen, 2000). Lipases catalyze the biochemical reaction like esterification, interesterification, and transesterification in nonaqueous media which frequently hydrolyze triglycerides into diglycerides, monoglycerides, fatty acids, and glycerol. Microorganism like Pseudomonas aeruginosa, Serratia marcescens, Staphylocococcus aureus, and Bacillus subtilis are the best sources of lipase enzymes. Lipases are widely used in pharmacological, chemical, and food industries. The commercial applications of lipases in the food industry are the hydrolysis of milk fats, pronounced cheese flavor, low bitterness, and prevention of rancidity.Lipases are amongst the most important biocatalysts that are used to carry out a broad spectrum of organic transformations in both aqueous and nonaqueous media to generate biologically relevant organic molecules of potential practical interest, both in research laboratories and in industry. Lipases have the remarkable ability to carry out a wide variety of chemo-, regio-, and enantioselective transformations, and also have very broad substrate specificity. The present chapter offers a recent update on the lipase-catalyzed organic transformations reported during 2013–mid-2015. This overview reflects the biocatalytic efficacy of the enzyme in carrying out various types of organic reactions, including esterifications, transesterifications, additions, ring-closing, oxidation, reduction, amidation, and many others. Ease of handling, broad substrate tolerance, high stability towards temperatures and solvents, high enantioselectivity, convenient commercial availability, and reusability are the key advantages of choosing lipase as a biocatalyst in a huge number of organic transformations. The author hopes that this overview should boost ongoing research in chemoenzymatic organic transformations, particularly the biocatalyic applications of lipases. It is noteworthy that each lipase has its own unique properties, and that fine-tuning of any methodology employing lipases to suit the individual enzyme should be screened carefully. To widen the usage level of lipases, there is an urgent need to understand the mechanisms behind the lipase-catalyzed reactions in more depth. Protein engineering of lipases and the further improvement of lipase preparations and reaction methodology have great potential to generate even better bioconversions in the future.

Liquid paraffin, also known as mineral oil, is a transparent, colorless, odorless, or almost odorless, oily liquid composed of saturated hydrocarbons obtained from petroleum.
Liquid paraffin typically contains 15 to 40 carbons and has a density of approximately 0.8 grams per centimeter cubed (g/cm³).
Liquid paraffin is a common ingredient in a variety of products with a wide range of uses, including cosmetics, pharmaceuticals, lubricants, and as a base for nasal sprays.

CAS Number: 8042-47-5
EC Number: 232-455-8
Molecular Formula: C20H42​
Molar Mass: 282.536g/mol

Synonyms: Liquid paraffin (petroleum), Slab oil (Obs.), Mineral oil, white, Liquid paraffin, petroleum, Liquid paraffin, (petroleum), [ChemIDplus] Paraffinum liquidum, Paraffin oil, CLAIRSOL 370, CLAIRSOL 430, CLAIRSOL 440, Hydrocarbon oils, Mineral oil, Ondina/Risella, PARASET 26 L, PARASET 29 L, PARASET 32 L, PILOT 261, PILOT 291, ROLLSOLV 100, White oil, Medicinal white oil, Technical white oil, Liquid paraffin, Weissoel, Pharmacytical White Oil, Marcol 52,82,172, Primol 187,352, Plastol 135, Bayol 82, [IUCLID], coal oil, kerosene, kerosine, lamp oil, c15-50 Alkanes, CAS: 8042-47-5 EC:232-455-8, highly refined and hydrogenated mineral oil, Highly refined base oils, Hydrotreated highly refined base oil, industrial oil, MINERAL OIL, paraffin oil, paraffin oil (C17-C30), Paraffin oils. Liquid hydrocarbons from petroleum, petroleum, Renoil (TM) white mineral oil, WHITE MINERAL OIL, Saturated hydrocarbons having carbon numbers predominantly in the range of C15 through C50

Liquid paraffin or mineral oil is a transparent, colourless, odourless, or almost odourless, oily liquid composed of saturated hydrocarbons obtained from petroleum.
Liquid paraffin is any of various colorless, odorless, light mixtures of higher alkanes from a mineral source, particularly a distillate of petroleum, as distinct from usually edible vegetable oils.

The name 'Liquid paraffin' by itself is imprecise, having been used for many specific oils over the past few centuries.
Other names, similarly imprecise, include 'white oil', 'paraffin oil', 'liquid paraffin' (a highly refined medical grade), paraffinum liquidum (Latin), and 'liquid petroleum'.
Baby oil is a perfumed Liquid paraffin.

Most often, Liquid paraffin is a liquid by-product of refining crude oil to make gasoline and other petroleum products.
This type of Liquid paraffin is a transparent, colorless oil, composed mainly of alkanes and cycloalkanes, related to petroleum jelly.

Liquid paraffin has a density of around 0.8–0.87 g/cm3 (0.029–0.031 lb/cu in).
Liquid paraffin, more technically known as pharmaceutical white and technical Liquid paraffin, are highly refined Liquid paraffin consisting of highly non-polar paraffinic hydrocarbons.
Due to their colourless, odourless, tasteless and hydrophobic properties, Liquid paraffins are used in many different industries with the cosmetics, pharmaceuticals, chemistry and plastics and rubber industries leading the field in usage.

Liquid paraffin is a common ingredient in a variety of products with a wide-range of uses.
Liquid paraffin comes in various forms, but pure Liquid paraffin is colorless and odorless.

Liquid paraffin is also referred to as paraffin oil, liquid paraffin, liquid petroleum, and saturated hydrocarbons.
Liquid paraffin written both with and without the adjectives "light" and "white."
The term Liquid paraffin most often refers to a byproduct of the distillation of petroleum as occurs during the production of gasoline and other petroleum-based substances.

Liquid paraffin is not to be confused with 'mineral spirits', as they are very different types of products.
Liquid paraffin is made up primarily of alkanes and cyclic paraffin, which is related to petroleum jelly.

Liquid paraffin typically contains 15 to 40 carbons and has a density of approximately 0.8 grams per centimeter cubed (g/cm3).
While those three sectors use this element most widely, Liquid paraffin has a variety of other applications.

Liquid paraffin is a standard household item, but has also found uses in some niche markets.
Liquid paraffin is versatile and has many properties making Liquid paraffin useful in a range of applications.

Liquid Paraffin is an emollient (substance that softens or soothes the skin).
Liquid paraffin works by preventing water loss from the outer layer of skin.
This relieves dryness and leaves the skin soft and hydrated.

Liquid paraffin (petrolatum) is a highly refined distilled fraction of petroleum that contains a mixture of liquid saturated hydrocarbons Sweetman.
Liquid paraffin is used as a laxative Sharif et al (2001), a lubricant, and as a base for nasal sprays.

Other paraffins, such as soft white paraffin, are semi-solid mixtures of hydrocarbons and are used as ointment bases and lubricants.
As a result of Liquid paraffins side effects and the availability of better products, liquid paraffin is not recommended for routine use.
Liquid paraffin is available without prescription.

Liquid paraffin has a variety of names that correspond towards the intended use of the oil.
The general, and interchangeable, names are white oil and mineral oil.

A few other names include paraffinum perliquidum, paraffin oil, liquid paraffin, and liquid petroleum.
Liquid paraffin is a colorless and odorless mixture of higher alkanes from a mineral source.

Liquid paraffin source is usually from a distillate of petroleum.
Liquid paraffins are highly refined mineral oils, and are composed of saturated aliphatic and alicyclic nonpolar hydrocarbons.

They are odorless, tasteless, colorless, hydrophobic, and don’t change their color over time.
Liquid paraffin is biologically and chemically stable, and doesn’t support pathogenic bacterial growth, which makes Liquid paraffin the standard choice of oil in most industries.

Liquid paraffin is tasteless, transparent, colorless, non-fluorescent and oily hydrocarbon blend, which includes saturated hydrocarbons that come from the distillation of light fractions.
They are used in different ways, which include refining crude petroleum.

The hydrogeneration methods are also used in distillation, and this process is used to remove the Sulphur compounds, unsaturated hydrocarbons, aromatic amines, and aromatic compounds from the oil.
The best thing about while mineral oil is that Liquid paraffin doesn’t dissolve in alcohol or water, but dissolves in organic solvents like benzene, and chloroform.

Liquid paraffin is known as white mineral oil because of Liquid paraffins transparent and colorless structure, and goes by the name of liquid paraffin or paraffin.
Liquid paraffin is also labelled as pharma grade or technical based on Liquid paraffins chemical composition.

An indispensable material for cosmetics and pharmaceutical industries.
There are a lot of industries that use Liquid paraffin, which includes the plastics, food, pharmaceutical, and cosmetics industries.

In the cosmetic industry, the oil is used sole as an auxiliary or primary material in the manufacture of bath oils, depilatories, makeup removers, makeup products, sun protection creams, sun tanning products, baby oil, lotion formulations, and creams.
In the pharmaceutical industry, the oil is used in the manufacture of gelatin capsules, ointment and pomade formulations, and laxatives.

In the veterinary drug industry, the oil is used for the manufacture of animal vaccines.
The Liquid paraffin that is used in the drug and cosmetics industry can’t contain any hazardous substances that may harm human health and must be pharma grade.

The raw materials added to the products should meet the international and national cosmetic regulations, along with pharma copies like USP/NF, PH. Eur., since the product is applied directly or indirectly on to the body.
Liquid paraffin doesn’t stay for long in the body as Liquid paraffin doesn’t have any chemical group, and is therefore removed from the body naturally.

Liquid paraffin is widely used in the food industry.
Liquid paraffin is commonly used in the food industry, and is favored in some food processes, especially in the manufacture of lubricating oils used by drink and food producers.
The lubricating oil used in food manufacturing plants can come in contact with the compressor oils, gear oils, hydraulic system oils, greases, and food product.

That is why Liquid paraffin are preferred, since they can minimize serious health risks.
All products that include Liquid paraffin are strictly monitored, and must obtain the necessary certificates and meet the relevant conditions.

The elastomer and plastics industry also uses Liquid paraffin heavily, as Liquid paraffin is used in the production of thermoplastic rubber, polystyrene, and PVC.
Apart from that, Liquid paraffin also feature heavily in common products like toys, glues, lamp oil, cleaning products, wood products, polishes, and glossing products.

The range of products that use Liquid paraffin is expected to increase in the future, with growing human needs and advancing technology playing a major role in that.
There is no denying that Liquid paraffin is among the most common oils used and consumed on the planet, and Liquid paraffin popularity and uses are only going to increase in the future.
Liquid paraffin is found in everything from a children’s toy, to a sunscreen cream, and is bound to be in everything that you use and consume in your daily life.

Liquid paraffins have a long history of safe use by humans in orally ingested and topically applied products.
A re-evaluation of the use of certain mineral hydrocarbons in the preparation of food items by regulators in the UK, however, has prompted additional safety studies and a critical assessment of the toxicological effects of Liquid paraffin.
As Liquid paraffin are present in many topically applied drug and non-drug products, Liquid paraffin is of interest to review the toxicological effects of Liquid paraffin produced by this route of exposure.

Liquid paraffins that are low grade are toxic, and the best thing to do is look at the different grades and viscosities of these Liquid paraffins.
That depends on their purposes, which are different in industrial, electrical, mechanical, cosmetics, and biomedicine uses.

Medical grade Liquid paraffin are safe to be used as lubricant laxatives, which have been used to ease constipation for people.
They are great for treating chronic constipation, but the potential side effects should also be considered.

The industrial grade Liquid paraffin are commonly used in electric power, petroleum chemical, chemical fiber, textile, and the agriculture industries.
They are used as machine lubricants.
The cosmetic grade Liquid paraffin are used as makeup removers or are used in skincare and cosmetic products like ointments, creams, or lotions to increase skin health.

Liquid paraffin is a clear liquid carrier that can also be found in a wide variety of cosmetics, personal care and household products.
A carrier does just what Liquid paraffin sounds like - Liquid paraffin helps carry a product to a surface by thinning or thickening the formula or simply ensuring even distribution of the other ingredients in the formula.

We use Liquid paraffin because without a carrier, the product would not work with the same consistency across a surface.
Liquid paraffin can also be used as a cleaning agent, or "surfactant," that removes dust, dirt and soils, or as a stabilizer that helps maintain a product formula when exposed to air, light or heat, or as a defoaming agent that helps reduce the formation of foam to avoid defects on surface coating post-use.

Applications of Liquid paraffin:
Liquid paraffins are the best for use as a blending base for pharmaceutical products and personal care, but Liquid paraffin is their inert nature that makes them so beneficial.
Liquid paraffins resist moisture, extend, soften, smoothen, and lubricate in most formulations.

You can easily find NF grade and USP grade Liquid paraffin in most products, typically antibiotics, tissues, sunscreens, lotions, and baby oils.
The plastics industry also uses Liquid paraffins, typically in the product of polymers, thermoplastic elastomers, polyolefins, and polystyrene.

This is done to control and improve the melt flow rate of finished polymer for releasing properties or changing Liquid paraffins physical characteristics.
The food grade Liquid paraffin are used in pan oils and dough dividers to suppress dust in grain silos, and they are also used as lubricants in food-handling equipment, for controlling foam in vinegar production, beet sugar, improving the leather tanning process and in food wrapping paper to keep foods crisp in packaging.

Pure Liquid paraffin is registered by NSF as been food safe when been in both incidental and direct contact with food, therefore this makes the product an ideal choice for the treatment of wooden chopping boards, food preparation areas, wooden bowls, bread & cheese boards as well as kitchen & dining utensils to protect blades etc.
The product may also be utilised as a release agent to prevent food from adhering to surfaces and blades on slicing machines.
Due to Liquid paraffins high pure, non-toxic, odourless characteristics the product may also be used as a skin lotion, in home reed diffusers, hair clipper blades, internal hinges and in aromatherapy.

Liquid paraffins are integral to many applications throughout a breadth of industries.
Liquid paraffin is also known as white oil, mineral oil, liquid petroleum, paraffin oil, liquid paraffin and paraffinum.

At a glance, Liquid paraffin are odorless and colorless.
These ultra-pure, refined mineral oils are a mixture of paraffinic isoalkanes and naphthenic molecules.

Liquid paraffin is used as a blending base in a variety of applications, including cosmetic, pharmaceutical, food and general industry.

While those three sectors use this element most widely, Liquid paraffin has a variety of other applications.
Liquid paraffin is a standard household item, but has also found uses in some niche markets.
Liquid paraffin is versatile and has many properties making Liquid paraffin useful in a range of applications.

Liquid paraffin is used as a laxative to alleviate constipation by retaining water in stool and the intestines.
Although generally considered safe, as noted above, there is a concern of mist inhalation leading to serious health conditions such as pneumonia.

Liquid paraffin can be administered either orally or as an enema.
Liquid paraffin is sometimes used as a lubricant in enema preparations as most of the ingested material is excreted in the stool rather than being absorbed by the body.

Liquid paraffin is inert, which makes Liquid paraffin easy to use.
Both consumers and businesses in a range of industries use Liquid paraffin for a variety of applications.

The three sectors named above primarily use Liquid paraffin, but Liquid paraffin appears across a wide range of industries and applications.
Here are some of the most common uses in the industrial, personal care, and food production sectors.

A mixture of highly refined paraffinic and naphthenic liquid hydrocarbons with boiling point above 200°.
Obtained from mineral crude oils through various refining steps (eg. distillation, extraction and crystallisation) and subsequent purification by acid and/or catalytic hydrotreatment.

May contain antioxidants approved for food use.
DESCRIPTION Colourless, transparent and odourless oily liquid, without fluorescence in daylight.

Liquid paraffin make an ideal blending base for personal care and pharmaceutical products.
Their inert nature makes them easy to use, as they lubricate, smooth, soften, extend and resist moisture in many formulations.

You can find our USP and NF grade Liquid paraffin in products ranging from baby oils and lotions to sunscreens, tissues and antibiotics.
The plastics industry uses our Hydrobrite line of low-volatility Liquid paraffin in the production of plastics such as polystyrene, polyolefins, thermoplastic elastomers, and various other polymers to improve and control the melt flow rate of the finished polymer to provide release properties, or change the physical characteristics.

Our food grade Liquid paraffin have proven themselves in food applications as wide ranging as dough divider and pan oils to dust suppression in grain silos.
They lubricate food-handling equipment, impregnate wrapping paper to keep foods crisp, control foam in beet sugar and vinegar production, and enhance the leather tanning process.
As one of the leading hot melt adhesive manufacturers, our low pour-point naphthenic grades improve hot melt adhesives and lubricate air conditioner and refrigerator compressors.

Some other applications for Liquid paraffin in general include:
Liquid paraffin is being used as a brake fluid,
The use of Liquid paraffin as a principle fuel in some scented candles,
As a honing oil when sharpening edge tools,
Liquid paraffin being an inexpensive alternative for storing reactive metals,
Liquid paraffin being used within adhesives.
And as an anti-rust agent for blades.
Biomedicine,
Laxative.

Uses of Liquid paraffin:
Liquid paraffin is used to relieve dry, irritated eyes.
Common causes for dry eyes include wind, sun, heating/air conditioning, computer use/reading, and certain medications.

Liquid paraffin may contain 1 or more of the following ingredients: carboxymethylcellulose, dextran, glycerin, hypromellose, polyethylene glycol 400 (PEG 400), polysorbate, polyvinyl alcohol, povidone, or propylene glycol, among others.
Eye lubricants keep the eye moist, help to protect the eye from injury and infection, and decrease symptoms of dry eyes such as burning, itching, and feeling as if something is in the eye.

Liquid paraffin can act as a non-conductive coolant, thermal fluid, lubricant, release agent, binder, defoamer, protective coating or float, sealing and polishing agent, dust control agent, and more.

Liquid paraffin has applications in three main areas:
Liquid paraffins are colorless, odorless, tasteless mixtures of saturated paraffinic and naphthenic hydrocarbons which meet or exceed FDA 21 CFR 172.878, 178.3620(a) and NF or USP requirements.
Liquid paraffins are available in a broad range of viscosities ranging from 55-550 SUS@40°C and are exceptionally suited as ingredients in pharmaceutical and cosmetic preparations, food environments where direct or indirect contact with food may occur and in applications where odor and staining must be minimized.
Custom formulations of Liquid paraffin may be available to meet specific criteria such as smoke, flash and pour points upon request.

Industry Uses:
Liquid paraffins are food- and medical-grade, making them popular in the pharmaceutical, cosmetic and food industries.
This type of Liquid paraffin can be safely used as a lubricating agent in food processing plants as Liquid paraffin is approved for food contact.
This allows manufacturing without concern of contamination of the products that can happen with less pure standard lubricants.

Liquid paraffin are also popular in the plastics and rubber manufacturing industries.
They help with the softening of rubber products and are essential in the production of polystyrene, PVC and different types of rubbers.

This is critical for producing food packaging and utensils out of plastic.
Liquid paraffin can also be readily found in glues, cleaning products, polishes and plastic toys.
The range of uses for Liquid paraffin has only grown in the past couple of decades, and Liquid paraffin is expected to keep growing in the future with the focus on protecting the public.

The process oils commonly found in rubber manufacturing typically have a viscosity between 70 and 1,500 SUS at 100 degrees Fahrenheit.
Liquid paraffin distributors typically offer a range of Liquid paraffin products that vary in viscosity, as you’ll see below.

Food-Grade Liquid paraffin:
To use Liquid paraffin in food preparation, Liquid paraffin must be classified as a food-grade mineral oil.
This is vital for health and safety as well as legal compliance.

The Food and Drug Administration (FDA) has established standards any 'food-grade' substance must meet for both direct additions to foods and uses that may result in incidental contact with food.
The requirements for purity, amount used, and processes vary based on how one uses Liquid paraffin.

The United States Pharmacopoeia (USP) and the National Formulary (NF) first created guidelines for the use of Liquid paraffin in manufacturing.
The FDA requires that food-grade Liquid paraffin meet USP XX test requirements for readily carbonizable substances, which USP released in 1980, and USP XVII test requirements for sulfur compounds.
Liquid paraffin also needs to meet the specifications in Volume 45 of the Journal of the Association of Official Analytical Chemists.

Liquid paraffin used as a lubricant for food-processing machinery must be registered with NSF International, an independent global food safety organization, as lubricants for incidental food contact to be used in food-processing plants under the jurisdiction of the U.S. Department of Agriculture (USDA).
Liquid paraffin can also receive Kosher certification.

Other organizations oversee Liquid paraffin use in other industries.
For example, the Association of American Feed Control Officials (AAFCO) governs Liquid paraffins use as a dust control agent for animal feeds.

This classification is different, however, from food-grade Liquid paraffin.
Liquid paraffin used in the production of pharmaceuticals must be considered pharmaceutical-grade.
The cosmetics and medical industry use highly refined Liquid paraffin to avoid irritating the skin, eyes, and other body parts.

Liquid paraffin Carrier Oil is a multipurpose odourless oil and can be used in aromatherapy/mouldings/butchers block oil/home reed diffusers and many other uses.
Liquid paraffin absorbs into the skin leaving a very light feeling of oil.

The food processing and preparation industries frequently use Liquid paraffin.
Sometimes, manufacturers add Liquid paraffin directly to food.

At other times, Liquid paraffin assists in the production process but is not added to food directly.
As mentioned earlier, all Liquid paraffin that may come into contact with food must achieve classification as food-grade, and Liquid paraffin must be used in accordance with all relevant laws and regulations.

Liquid paraffin plays a role in some of the non-food products used to prepare, serve, and eat food.
In these situations, the oil should also be food-grade.

When applied to cookware, bakeware, and cooking utensils, Liquid paraffin prevents food from sticking to them.
People rub Liquid paraffin onto the surface of wooden cutting boards, bowls, and utensils to prevent them from absorbing water, which can damage them.

Liquid paraffin also prevents wood-based cooking tools from absorbing food liquids and odors, which makes cleaning easier.
Liquid paraffin acts as a lubricant for food processing equipment as well.

Food Producers Use Liquid paraffin As:
As a Binder, release agent, or lubricant in bakery products, dehydrated foods, egg white solids, and in tablets or capsules for adding nutrients, flavoring, spices, or for use as a dietary supplement.

As a release agent, sealing agent, and polishing agent in confectioners.
As a protective coating on raw fruits and vegetables.

As a defoamer in vinegar and beet sugar production.
As a dough divider.

As a dust control agent for grains.
As a binder, release agent, and lubricant in the manufacturing of yeast.

In Personal lubricant:
Liquid paraffin is recommended by the American Society for Reproductive Medicine for use as a fertility-preserving vaginal lubrication.
However, Liquid paraffin is known that oils degrade latex condoms.

In Cell Culture:
Liquid paraffin of special purity is often used as an overlay covering microdrops of culture medium in petri dishes, during the culture of oocytes and embryos in IVF and related procedures.

The use of Liquid paraffin several advantages over the open culture system:
Liquid paraffin allows for several oocytes and embryos to be cultured simultaneously, but observed separately, in the same dish.
Liquid paraffin minimizes concentration and pH changes by preventing evaporation of the medium.

Liquid paraffin allows for a significant reduction of the medium volume used (as few as 20 microlitres (0.0012 cu in) per oocyte instead of several millilitres for the batch culture).
And Liquid paraffin serves as a temperature buffer minimizing thermal shock to the cells while the dish is taken out of the incubator for observation.

In Veterinary:
Over-the-counter veterinarian-use Liquid paraffin is intended as a mild laxative for pets and livestock.
Certain Liquid paraffin are used in livestock vaccines, as an adjuvant to stimulate a cell-mediated immune response to the vaccinating agent.

In the poultry industry, plain Liquid paraffin can also be swabbed onto the feet of chickens infected with scaly mites on the shank, toes, and webs.
Liquid paraffin suffocates these tiny parasites.

In beekeeping, food grade Liquid paraffin-saturated paper napkins placed in hives are used as a treatment for tracheal and other mites.
Liquid paraffin is also used along with a cotton swab to remove un-shed skin (ashes) on reptiles such as lizards and snakes.

In Cosmetics:
Liquid paraffin is a common ingredient in baby lotions, cold creams, ointments, and cosmetics.
Liquid paraffin is a lightweight inexpensive oil that is odorless and tasteless.

Liquid paraffin can be used on eyelashes to prevent brittleness and breaking and, in cold cream, is also used to remove creme make-up and temporary tattoos.
One of the common concerns regarding the use of Liquid paraffin is Liquid paraffins presence on several lists of comedogenic substances.

These lists of comedogenic substances were developed many years ago and are frequently quoted in the dermatological literature.
The type of highly refined and purified Liquid paraffin found in cosmetic and skincare products is noncomedogenic (does not clog pores).
Pharmaceutical Liquid paraffin are used in the cosmetics industry to form the basis of many widely used product formulations, including skin care cream, cleaning cream, beauty lotion, baby oil and hair care products.

You can find Liquid paraffin in many different cosmetics products including baby lotions, ointment, make-up remover, sunscreens, hair conditioner, and even tissues.
Liquid paraffin is an ideal base material for many of these products because Liquid paraffin is inert, colorless, and odorless.
Liquid paraffin may appear in cosmetics as liquid oils or solid waxes.

Some kinds of Liquid paraffin are comedogenic, meaning they clog pores.
Because of this, the Liquid paraffin used in skincare and cosmetic products is noncomedogenic and does not clog pores.

In fact, cosmetics companies often describe Liquid paraffin as having moisturizing, protective, and cleansing properties for the skin.
Additionally, these oils are used to give cosmetic products film-forming and water-repellent features as well as increased firmness.

Liquid Paraffin is used in the treatment of dry Skin.
Liquid paraffin relieves dry skin conditions such as eczema, ichthyosis and pruritus of the elderly.

In Mechanical, Electrical, And Industrial:
An electrical radiator that uses Liquid paraffin as a heat transfer fluid
Liquid paraffin is used in a variety of industrial/mechanical capacities as a non-conductive coolant or thermal fluid in electric components as Liquid paraffin does not conduct electricity and functions to displace air and water.

Some examples are in transformers, where Liquid paraffin is known as transformer oil, and in high-voltage switchgear, where Liquid paraffin is used as an insulator and as a coolant to disperse switching arcs.
The dielectric constant of Liquid paraffin ranges from 2.3 at 50 °C (122 °F) to 2.1 at 200 °C (392 °F).
Liquid paraffin is used as a lubricant, a cutting fluid, and as a conditioning oil for jute fibres selected for textile production, a process known as 'jute batching'.

Spindle oils are light Liquid paraffin used as lubricants in textile industries.
Electric space heaters sometimes use Liquid paraffin as a heat transfer oil.

Liquid paraffins are used in a variety of applications in the textile industry ranging from fibre lubricant, sewing machine oil and yarn lubrication oil.
Because Liquid paraffin is noncompressible, Liquid paraffin is used as a hydraulic fluid in hydraulic machinery and vehicles.
An often-cited limitation of Liquid paraffin is that Liquid paraffin is poorly biodegradable; in some applications, vegetable oils such as cottonseed oil or rapeseed oil may be used instead.

Liquid paraffin serves to assist with various industrial, mechanical, and electrical purposes.
Liquid paraffin is an effective lubricant for industrial equipment and often functions as a processing aid.

Liquid paraffin is an element that helps make up various substances used in industrial processes, such as lubricants, greases, dyes, polymers, and surface treatment products.
Liquid paraffin also acts as a thermal fluid or non-conductive coolant in various electric components.

In refrigerators and oil-based electric heaters, Liquid paraffin is used as a cooling liquid.
In switchgear, Liquid paraffin serves as an insulator and a coolant to diffuse switching arcs.

In the production of plastics, Liquid paraffin is used to control the melt flow rate of finished polymer and act as a release agent.
Automotive equipment frequently uses Liquid paraffin, primarily as a component in hydraulic liquids in automotive suspension, as well as in lubricants in brake fluids and motor oil.

In Drug Industry:
Pharmaceutical Liquid paraffin are used as internal lubricants for laxative applications in the pharmaceutical industry.
In addition, these products are used as bases for ointments and creams, as carriers for solid and semi-solid ingredients and additionally used as a separator on capsules and tablets.

In Food Preparation:
Because of Liquid paraffins properties that prevent water absorption, combined with Liquid paraffin lack of flavor and odor, food grade Liquid paraffin is a popular preservative for wooden cutting boards, salad bowls, and utensils.
Rubbing a small amount of Liquid paraffin into a wooden kitchen item periodically impedes absorption of food liquids, and thereby food odors, easing the process of hygienically cleaning wooden utensils and equipment.

The use of Liquid paraffin to impede water absorption can also prevent cracks and splits from forming in wooden utensils due to wetting and drying cycles.
However, some of the Liquid paraffin used on these items, if in contact with food, will be picked up by Liquid paraffin and therefore ingested.

Outside of the European Union, Liquid paraffin is occasionally used in the food industry, particularly for confectionery.
In this application, Liquid paraffin is typically used for the glossy effect Liquid paraffin produces, and to prevent the candy pieces from adhering to each other.

Liquid paraffin has been discouraged for use in children's foods, though Liquid paraffin is still found in many confectioneries, including Swedish Fish.
The use of food grade Liquid paraffin is self-limiting because of Liquid paraffins laxative effect.
The maximum daily intake is calculated to be about 100 mg (1.5 gr), of which some 80 mg (1.2 gr) are contributed from Liquid paraffins use on machines in the baking industry.

In Agriculture:
Due to Liquid paraffins low toxicity and non-harmful properties making Liquid paraffin safe to use with regards to the environment and human health, Liquid paraffin are used in the production of spray oils to treat and protect fruit trees.

In Chemicals:
Liquid paraffin are used in the chemicals sector, particularly in adhesives, hot-melts, the paper industry and in the production of leather and explosives.

In Plastics & Rubber:
Liquid paraffins are used extensively in the plastics and rubber industry to produce different types of plastics and rubber applications.
Used to control the melt flow rate of input products for Polystyrene (PS), high impact resistance polystyrene (HIPS), polyolefin and thermoplastic elastomer, Liquid paraffins are also used as internal and external lubricant in polymer formulations of PS, PVC, PP, TPE.
Plasticiser, catalyst carrier and mould release and pigment dispersion agents are other applications of Liquid paraffin in this industry.

In Textiles:
Liquid paraffins are used in a variety of applications in the textile industry ranging from fibre lubricant, sewing machine oil and yarn lubrication oil.

Other uses of Liquid paraffin:
Liquid paraffin can be found in a variety of other products, or in the actual production processes of other items.
Liquid paraffin plays a role in the manufacture of leather, paper, pulp, textiles, fur, plastics, fabricated metal, lubricants, greases, and chemicals.

Because Liquid paraffin has applications for so many materials, Liquid paraffin is essential for the production of items as varied as tires, shoes, mobile phones, packaging, clothing, cutlery, and jewelry.
Liquid paraffin is an element in leather treatment products, textile treatment products and dyes, and paper chemicals and dyes.

In the medical field, Liquid paraffin can be used to relieve constipation and as a lubricant in enema preparation.
In veterinary medicine, Liquid paraffin is also used as a mild laxative, an ingredient in vaccines, and to remove any unshed skin from reptiles.

In laboratories, researchers may use tiny amounts of the substance to cover culture medium in petri dishes to prevent evaporation and thermal shock.
In biotechnology, Liquid paraffin overlays polymerase chain reactions to prevent water loss during heating.
In X-ray crystallography, the study of crystals using X-ray technology, Liquid paraffin is used to suspend crystals.

Liquid paraffin's ubiquity has led to Liquid paraffins use in some niche applications as well:
Liquid paraffin is used for treating and preserving wooden butcher block counter tops.

Liquid paraffin is commonly used to create a wear effect on new clay poker chips, which can otherwise be accomplished only through prolonged use.
Either the chips are placed in Liquid paraffin for a short time, or the oil is applied to each chip then rubbed off.

This removes any chalky residue left over from manufacture, and also improve the look and feel of the chips.
Liquid paraffin is used as the principal fuel in some types of gel-type scented candles.

Liquid paraffin is used for cooling, such as in the liquid submersion cooling of components in some custom-built computers.
Veterinarian-grade Liquid paraffin is inexpensive, and is frequently used by amateur radio operators as coolant in RF dummy loads, as Liquid paraffin is typically used as the insulating and cooling fluid in large electrical equipment such as transformers.

Liquid paraffin is used as a brake fluid in some cars, such as Citroën models with hydrodynamic suspension, and bicycle disc brakes.
Liquid paraffin is burned in specialized machines (both manufactured and home-made) to produce a thick white smoke that is then blown into automotive evaporative emissions (EVAP) systems to find leaks.

Liquid paraffin is used for polishing alabaster in stonework and lubricating and cleaning pocket knives or food handling tools that use an open bearing, thus needing periodic lubrication.
Light Liquid paraffin (paraffinum perliquidum) is used as a honing oil when sharpening edge tools (such as chisels) on abrasive oil stones.

Liquid paraffin USP or light Liquid paraffin can be used as an anti-rust agent for blades.
Liquid paraffin is an inexpensive alternative for storing reactive metals, such as lithium and sodium.

Horticultural oil is often made of a combination of Liquid paraffin and detergent.
Liquid paraffin is sprayed on plants to control scale, aphid, and other pest populations by suffocation.

Before the widespread adoption of thermocyclers with heated lids, Liquid paraffin was common practice to use Liquid paraffin to overlay polymerase chain reactions in biotechnology to prevent loss of water during heating cycles.
Liquid paraffin is often used to suspend crystals for use in X-ray crystallography.

Liquid paraffin is used as a transparent collision material for reactions in particle physics, as in the MiniBooNE neutrino oscillation experiment.
As a relatively low heat combustible with no flavor or odor, Liquid paraffin can be used in fire breathing and firedancing for entertainment, but there is a risk of injury.

Liquid paraffin is commonly used to fill Galileo thermometers.
Due to Liquid paraffin's freezing temp being lower than water (approx. 24 °F (−4 °C)), this makes them less susceptible to freezing during shipment or when stored in a cold environment.

Chemical Formula of Liquid paraffin:
Liquid paraffin coming from crude petroleum oils vary in their make-up and contain complex structures.
Liquid paraffin include mixtures of straight and branched-chain paraffinic, naphthenic, and aromatic hydrocarbons.

Alkanes, which are acyclic saturated hydrocarbons, are a significant component.
Liquid paraffin are made up of hydrogen and carbon atoms in a tree structure where all the carbon-to-carbon bonds are single.
Liquid paraffin typically contains between 15 and 40 hydrocarbons.

Manufacturing of Liquid paraffin:
Liquid paraffin are highly refined Liquid paraffin that consist of saturated aliphatic and alicyclic nonpolar hydrocarbons.
They are hydrophobic, colorless, tasteless, odorless, and do not change color over time.

As a leading Liquid paraffin manufacturer and supplier to multiple industries, our Liquid paraffin are chemically and biologically stable, non-comedogenic, and do not support pathogenic bacterial growth.
These properties make Liquid paraffin the standard in many industries.

Nomenclature of Liquid paraffin:
Some of the imprecision in the definition of the names used for Liquid paraffin (such as 'white oil') reflects usage by consumers and merchants who did not know, and usually had no need of knowing, the oil's precise chemical makeup.
Merriam-Webster states the first use of the term "Liquid paraffin" as being 1771.

Prior to the late 19th century, the chemical science to determine the makeup of an oil was unavailable in any case.
A similar lexical situation occurred with the term "white metal".

Liquid paraffin sold widely and cheaply in the US, is not sold as such in Britain.
Instead, British pharmacologists use the terms "paraffinum perliquidum" for light Liquid paraffin and "paraffinum liquidum" or "paraffinum subliquidum" for somewhat more viscous varieties.

The term "paraffinum liquidum" is often seen on the ingredient lists of baby oil and cosmetics.
British aromatherapists commonly use the term "Liquid paraffin".

In lubricating oils, Liquid paraffin is termed from groups 1 to 2 worldwide and group 3 in certain regions.
This is because the high end of group 3 mineral lubricating oils are so pure that they exhibit properties similar to polyalphaolefin – PAO oils (group 4 synthetics)

Properties of Liquid paraffin:
Understanding the physical and chemical properties of Liquid paraffin will help you to determine how best to use Liquid paraffin in your industrial, food-processing, or other processes.
These attributes may differ depending on the type of mineral used, how you use Liquid paraffin, and whether any other substances get added to the oil.

Liquid paraffin is a clear, colorless, and odorless liquid.
This lack of strong physical qualities helps make Liquid paraffin valuable in a variety of applications.
Manufacturers can add Liquid paraffin to products without changing their color, scent, flavor, or other crucial aspects.

Liquid paraffin is also generally regarded as safe for human consumption, but in limited amounts.
These features enable Liquid paraffins use in the food processing and pharmaceutical sectors.

Refined Liquid paraffin does not clog pores, which allows for Liquid paraffins use in cosmetics.
Liquid paraffin has a density of 0.85 grams per milliliter (g/ml), and Liquid paraffin specific gravity is 0.845 - 0.905.

Liquid paraffins kinematic viscosity is greater than or equal to 38.1 millimeters squared per second (mm2/s).
Liquid paraffin is insoluble in water.

Liquid paraffin has an initial boiling point of 424.4 degrees Fahrenheit (°F) and a boiling range that extends up to 1189.4 °F.
Liquid paraffins flash point is 275.00 °F closed cup and 380.00 °F open cup.

Liquid paraffin has an auto-ignition temperature of 500 °F, and Liquid paraffins heat of combustion is 31.5 kilojoules per gram (kJ/g).
As mentioned above, Liquid paraffin has an NFPA flammability rating of one, a health rating of zero, and a reactivity rating of zero, meaning Liquid paraffin is not a high fire risk.

One of the most beneficial attributes of Liquid paraffin is Liquid paraffins lubrication capabilities.
This is the primary reason Liquid paraffin has so many industrial, mechanical, food-processing, and medical applications.

This property plays a crucial role in many Liquid paraffin manufacturing and food production processes.
Liquid paraffins ability to transfer heat and Liquid paraffins non-conductivity enable Liquid paraffin's use as a coolant in a various electronic and mechanical equipment, as well as in industrial processes.
Liquid paraffins resistance to water and other liquids, as well as insolubility in water, allow Liquid paraffin to function as a sealant and binder in a variety of products.

Liquid paraffin, also known as paraffinum liquidum or Russian Liquid paraffin, is a very highly refined Liquid paraffin used in cosmetics and medicine.
Cosmetic or medicinal liquid paraffin should not be confused with the paraffin (or kerosene) used as a fuel.

Liquid paraffin is a transparent, colorless, nearly odorless, and oily liquid that is composed of saturated hydrocarbons derived from petroleum.
The term paraffinum perliquidum is sometimes used to denote light liquid paraffin, while the term paraffinum subliquidum is sometimes used to denote a thicker Liquid paraffin.

The History of Liquid paraffin:
Liquid paraffin was first used in the 1870s when ChesebroughBrooklyin found that Liquid paraffin was very good for healing injuries he had sustains.
Liquid paraffin then spiraled from there and was used regularly in cosmetics, food, and pharmaceutical industries.

Liquid paraffins have been used in petroleum products and in cosmetic and pharmaceutical industries for years.
The first known Liquid paraffin where found in Azerbaijan, when they were pumped out of wells in the 11th century and were traded in caravans.

The famous traveler Marco Polo found Liquid paraffin in the 13th century, and even mentioned Liquid paraffin in texts -- the use of petroleum in pharmacy and medicine.
In modern times Vaseline has become an essential raw material for skincare products.

Liquid paraffin was Chesebrough Brooklyn who had first found out that the sticky clear material he found in oil wells is great for healing skin injuries.
He started to produce and sell Liquid paraffin, and that was the first use of Vaseline, which is still used regularly in different skincare and cosmetic products today.

Most people don’t know that there are more uses of petroleum, instead of Liquid paraffin just being used as fuels in automobiles and machines.
Liquid paraffin is used heavily in the manufacture of chemical raw materials, cosmetic products, and health products, which impact directly on the health of humans.
Petroleum has also given us Liquid paraffin, which is one of the most frequent oils that is used and consumed in the daily lives of people all over the world.

Liquid paraffin are manufactured from a particularly refining process of traditional paraffinic base stocks.
This process gives particular characteristics of purity, absence of color, smell and taste.

These products satisfy the lubrication requirements of the food, pharmaceutical and cosmetic industry.
They are also suitable for production of perfumes, cosmetics and pesticides.
Technical Liquid paraffin are used as plasticizers for production of polymers as well.

Identifiers of Liquid paraffin:
CAS Number: 8042-47-5
Grade: Technical
Appearance: liquid
Auto Ignition Temperature: 325 - 355 °C (617 - 671 °F)
Boiling Point: > 218 °C (> 424 °F)
Color: Clear, Colorless
Density: 0.81 - 0.89 g/cm3 @ 20 °C (68 °F)
Flash Point: > 112 °C (> 234 °F)
Kinematic Viscosity: 15.73 mm2/s @ 40 °C (104 °F)
Melting Point: -60 - -9 °C (-76 - 16 °F)
Odor: hydrocarbon-like
Partition Coefficient: Pow: > 6
Recommended Use: Industrial chemical
Relative Density: < 1 @ 20 °C (68 °F) Reference Material: (water = 1)
Solubility in Water: insoluble
Vapor Pressure: 0.08 - 0.75 mmHg @ 20 °C (68 °F)

Properties of Liquid paraffin:
Boiling point: 218-643°C
Solubility in water, g/100ml at 20°C:
Vapour pressure at 20°C: negligible
Flash point: >115°C o.c.
Auto-ignition temperature: 260-371°C
Octanol/water partition coefficient as log Pow: >6

Appearance: Clear, colorless, oily liquid.
Odor: Odorless or very mild petroleum odor.
Viscosity: Highly viscous, with specific viscosity depending on the grade.
Density: Approximately 0.82–0.88 g/cm³ at 20°C.
Boiling Point: Generally above 300°C (varies with composition).
Melting Point: Below -20°C (varies with composition).
Solubility:
Water: Insoluble.
Organic Solvents: Soluble in chloroform, ether, benzene, and most organic solvents.
Flash Point: Typically in the range of 120-200°C, depending on the grade.
Autoignition Temperature: Approximately 260°C.
Refractive Index: Approximately 1.47-1.48 at 20°C.
Surface Tension: Around 30-35 mN/m at 25°C.
Chemical Stability: Chemically stable under normal conditions. Non-reactive with most substances.
Reactivity: Inert under most conditions; does not readily react with acids, bases, or oxidizing agents.
Viscosity Index: Typically high, indicating minimal change in viscosity with temperature.
Thermal Conductivity: Low, making it a poor conductor of heat.
Electrical Conductivity: Very low, acting as an insulator.

Specifications of Liquid paraffin:
SAE Grade 10, ISO Viscosity Grade 32
Meets requirements of USDA H-1 and 21CFR, Paragraphs 178.3570, 178.3620(b) and 573.680 of FDA Regulation
Flash Point: >350°F, COC
Flammable Limits: LEL:0.9 UEL:7.0
Melting Point: N/A
Freezing Point: N/A
Evaporate Rate: N/A
Auto-ignition Temperature: N/D
Boiling Point: N/A
pH: N/A
Specific Gravity: 0.818-0.880 @ 25°C (77°F)
Vapor Pressure (mm Hg.): Vapor Density (Air=1): >1
Appearance:Colorless, oily liquid
Odor: Odorless
Water Solubility: Insoluble

Appearance: Clear, colorless, and odorless oily liquid.
Purity:
High purity, often exceeding 99% paraffinic hydrocarbons.
Free from polycyclic aromatic hydrocarbons (PAHs).

Density: Typically 0.82–0.88 g/cm³ at 20°C.
Viscosity:
Light liquid paraffin: 10-35 cSt (centistokes) at 40°C.
Heavy liquid paraffin: 35-70 cSt at 40°C.
Refractive Index: 1.470–1.480 at 20°C.
Acidity/Alkalinity: Neutral, pH range typically around 6-8.
Boiling Point: Typically above 300°C.
Melting Point: Below -20°C.
Flash Point: Usually above 150°C.
Viscosity Index: High, indicating minimal change in viscosity with temperature.
Specific Gravity: 0.82–0.88 at 20°C.
Solubility: Insoluble in water. Soluble in most organic solvents like chloroform, ether, and benzene.
Heavy Metals: Very low or non-detectable levels, often specified as Peroxide Value: Typically very low, indicating minimal oxidation (often Sulfur Compounds: Minimal, often specified as non-detectable.
UV Absorbance: Meets stringent absorbance criteria to ensure purity (typically low absorbance in the UV range indicating absence of impurities).

(2S,3S)-(+)-Isoleucine; Ile; I; Isoleucine; L-2-Amino-3-methylvaleric Acid; L-Isoleucine; (2S)-2-Amino-3-methylpentanoic acid; 2-Amino-3-methylvaleric acid; cas no: 73-32-5

LITHENE P4 150 P Description LITHENE P4 150P is a medium viscosity, low molecular weight, liquid polybutadiene. It is unsaturated and can be used in chlorinated rubber feedstocks or in formulations where high water resistance is required. LITHENE P4-150P can be incompatible with many polar systems making it suitable for use in the formulation of specialized mould release coatings. LITHENE ULTRA P4 150P Lithene ultra P4 150P is a highly viscous, low molecular weight, liquid polybutadiene with microstructure containing 1,2 vinyl groups. It is very low in both odour and volatiles and can be used in chlorinated rubber feedstocks or automotive sealants. TYPICAL APPLICATIONS Feedstock for chlorinated rubber Automotive sound damping sealants & adhesives Property Value/ Unit /Method Vinyl 1,2 /17.0 - 20.0 /% /LTM 03 Viscosity, @ 25C /120 - 180 /dPa.s/LTM 01 Non volatile content/ >99.8 % /LTM 51 Colour/ 200 max/ Hazen /LTM 04 Typical molecular weight/ 3200 /Mn Molecular weight distribution/ Broad Appearance /Colourless to pale yellow liquid Technical Informations Application Advice/Typical Applications Handling - Lithene P4 150P is a viscous liquid polymer. The viscosity of the product will decrease rapidly with heating and the product may be warmed to allow easier processing. Compatibility - Liquid polybutadienes are generally compatible with most aliphatic and aromatic hydrocarbon solvents. They have limited solubility in alcohols, ketones and esters. Further details are available on request. Lithene P4 150P can be used in chlorinated rubber feedstocks and in other applications requiring a high degree of hydrophobicity. Thin films of the product can be dried oxidatively at 160 - 200°C, or metallic driers may be used to accelerate ambient cure. Lithene P4 150P is extremely low in odour and volatiles and can be used as the binder in formulation of sulphur cured direct to oily metal automotive sealants and adhesives. Further application and formulation advice is available on request. LITHENE ULTRA P4 150P Lithene P4 150P is a highly viscous, low molecular weight, liquid polybutadiene with microstructure containing 1,2 vinyl groups. It is very low in both odour and volatiles and can be used in chlorinated rubber feedstocks or automotive sealants. TYPICAL APPLICATIONS Feedstock for chlorinated rubber Automotive sound damping sealants & adhesives

LITHENE PM4 LITHENE ULTRA PM4 LITHENE ultra PM4 is a low viscosity, low molecular weight, liquid polybutadiene with a medium content of 1,2 vinyl microstructure. It is extremely low in both odour and volatiles and is used as the binder in automotive sound damping sealants, polyurethane mould release systems and solvent based coating additives. TYPICAL APPLICATIONS Automotive sound damping sealants Antifoaming coating additives Non volatile drying oil in alkyd coatings Sand binder for paving and moulds Property Value /Unit/ Method Vinyl 1,2 /15 - 25 /% /LTM 03 Viscosity, @ 25 C /7.0 - 9.5 /dPa.s /LTM 01 Non volatile content />99.8 % /LTM 51 Colour /200 max /Hazen /LTM 04 Typical molecular weight /1500/ Mn Molecular weight distribution /Broad Appearance/ Colourless to pale yellow liquid Application Advice & Processing Handling - LITHENE ultra PM4 is a low viscosity, easily processed liquid polymer. It will flow readily at ambient temperatures but the product viscosity will decrease rapidly with increasing temperature and the product may be warmed to allow easier processing. Compatibility - Liquid polybutadienes are generally compatible with most aliphatic and aromatic hydrocarbon solvents. They have limited solubility in alcohols, ketones and esters. Further details are available on request. LITHENE ultra PM4 is extremely low in odour and volatiles and can be readily formulated into sulphur cured automotive sealants and acoustic dampers, cured at 160 - 200 C. LITHENE ultra PM4 provides excellent adhesion, flexibility and acoustic damping although metal adhesion can be further increased by inclusion of a functional LITHENE grade such as LITHENE ultra AL-15MA or LITHENE ultra PM4-7.5MA. LITHENE ultra PM4 can be dried oxidatively at ambient temperatures in combination with metallic driers and can be used as a replacement to solvent in alkyd based coatings and as an air dry binder in sand for paving and moulds. LITHENE ultra PM4 can be incompatible with many polar systems making it suitable for use in the formulation of specialised mould release coatings for polyurethanes. Further application and formulation advice is available on request Shipping and Storage LITHENE ultra PM4 should be stored in a cool, dry location below +30 C (+86 F). If stored in the original sealed packaging the product has a shelf life of at least 12 months from date of delivery. Product which has been stored for longer than 12 months should betested before use. Containers which have been opened should be purged with dry nitrogen before resealing to protect the remainingproduct from oxidative skinning. Further information is available on the datasheet Storage of LITHENE Liquid Polybutadienes. LITHENE ultra PM4 is packed in bung top 200litre steel drums containing 175kg. The minimum order quantity is one pallet (four drums). 900kg IBCs or bulk deliveries are also available. Product Type: Polybutadiene Master Product Number: MITM08755 Product SKUs: ITM13098, ITM13099 CAS: 9003-17-2 LITHENE ULTRA PM4-7.5MA LITHENE ultra PM4-7.5MA is a medium viscosity, low molecular weight, liquid polybutadiene. It is very low in odour and volatiles and is produced from LITHENE ultra PM4, adducted with 7.5 parts maleic anhydride. TYPICAL APPLICATIONS Adhesion promoter in automotive sealants Rubber to metal adhesion promoter Soft, isocyanate free electrical encapsulants LITHENE products are 100% active, highly unsaturated, liquid polybutadienes available in a range of molecular weights and micro-structures. They are reactive, viscous liquids, have excellent low temperature flexibility, high electrical resistance and are very hydrophobic. Their excellent compatibility with hydrocarbon solvents and many rubbers makes them extremely versatile in a variety of ambient, UV and heat curable applications. Maleic anhydride grafting additonally allows the liquid polybutadienes to react with amines and polyols, while increasing polarity to enhance adhesion direct to metal. LITHENEs are widely used for: Sulphur cured flexible automotive sealants. Direct to metal adhesion promotors for the automotive industry. Sulphur or peroxide curable co-agents in rubber and TPEs. Electrical potting resins. Reactive plasticisers in rubber compounds. Solvent coating defoaming additives. Non volatile reactive coating diluents LITHENE ultra PM4 LITHENE non functional Name LITHENE® ultra PM4 Appearance colourless to pale yellow Molecular weight distribution broad Molecular weight average [Mn] approx. 1.500 Viscosity 25°C [mPas] approx. 700 Viscosity 50°C [mPas] approx. 200 Microstructure Vinyl 1,2 [%] 15 - 25 Microstructure cyclic [%] - Polybutadiene [butadiene rubber BR] is a synthetic rubber. Polybutadiene rubber is a polymer formed from the polymerization of the monomer 1,3-butadiene. Polybutadiene has a high resistance to wear and is used especially in the manufacture of tires, which consumes about 70% of the production. Another 25% is used as an additive to improve the toughness (impact resistance) of plastics such as polystyrene and acrylonitrile butadiene styrene (ABS). Polybutadiene rubber accounted for about a quarter of total global consumption of synthetic rubbers in 2012.[1] It is also used to manufacture golf balls, various elastic objects and to coat or encapsulate electronic assemblies, offering high electrical resistivity.[2] The IUPAC refers to polybutadiene as: poly (buta-1,3-diene) as poly (buta-1,3-diene). Buna rubber is a term used to describe an early generation of synthetic polybutadiene rubber produced in Germany by Bayer using sodium as a catalyst. Polymerization of butadiene 1,3-Butadiene is an organic compound that is a simple conjugated diene hydrocarbon (dienes have two carbon-carbon double bonds). Polybutadiene forms by linking many 1,3-butadiene monomers to make a much longer polymer chain molecule. In terms of the connectivity of the polymer chain, butadiene can polymerize in three different ways, called cis, trans and vinyl. The cis and trans forms arise by connecting the butadiene molecules end-to-end, so-called 1,4-polymerisation. The properties of the resulting isomeric forms of polybutadiene differ. For example, "high cis"-polybutadiene has a high elasticity and is very popular, whereas the so-called "high trans" is a plastic crystal with few useful applications. The vinyl content of polybutadiene is typically no more than a few percent. In addition to these three kinds of connectivity, polybutadienes differ in terms of their branching and molecular weights. 1,3-Butadiene Polymerization.PNG The trans double bonds formed during polymerization allow the polymer chain to stay rather straight, allowing sections of polymer chains to align to form microcrystalline regions in the material. The cis double bonds cause a bend in the polymer chain, preventing polymer chains from aligning to form crystalline regions, which results in larger regions of amorphous polymer. It has been found that a substantial percentage of cis double bond configurations in the polymer will result in a material with flexible elastomer (rubber-like) qualities. In free radical polymerization, both cis and trans double bonds will form in percentages that depend on temperature. The catalysts influence the cis vs trans ratio. Production The annual production of polybutadiene was 2.0 million tons in 2003.[17] This makes it the second most produced synthetic rubber by volume, behind the styrene-butadiene rubber (SBR).[15][23] The production processes of high cis polybutadiene and low cis used to be quite different and were carried out in separate plants. Lately, the trend has changed to use a single plant to produce as many different types of rubber as possible, including, low cis polybutadiene, high cis (with neodymium used as a catalyst) and SBR. Processing Polybutadiene rubber is seldom used alone, but is instead mixed with other rubbers. Polybutadiene is difficult to band in a two roll mixing mill. Instead, a thin sheet of polybutadiene may be prepared and kept separate. Then, after proper mastication of natural rubber, the polybutadiene rubber may be added to the two roll mixing mill. A similar practice may be adopted, for example, if polybutadiene is to be mixed with Styrene Butadiene Rubber (SBR). *Polybutadiene rubber may be added with Styrene as an impact modifier. High dosages may affect clarity of Styrene. In an internal mixer, natural rubber and/or styrene-butadiene rubber may be placed first, followed by polybutadiene. The plasticity of polybutadiene is not reduced by excessive mastication. Uses The annual production of polybutadiene is 2.1 million tons (2000). This makes it the second most produced synthetic rubber by volume, behind styrene-butadiene rubber (SBR).[24] Tires Racing tires Polybutadiene is largely used in various parts of automobile tires; the manufacture of tires consumes about 70% of the world production of polybutadiene,[18][19] with a majority of it being high cis. The polybutadiene is used primarily in the sidewall of truck tires, this helps to improve fatigue to failure life due to the continuous flexing during run. As a result, tires will not blow out in extreme service conditions. It is also used in the tread portion of giant truck tires to improve the abrasion, i.e. less wearing, and to run the tire comparatively cool, since the internal heat comes out quickly. Both parts are formed by extrusion.[25] Its main competitors in this application are styrene-butadiene rubber (SBR) and natural rubber. Polybutadiene has the advantage compared to SBR in its lower liquid-glass transition temperature, which gives it a high resistance to wear and a low rolling resistance.[18][26] This gives the tires a long life and low fuel consumption. However, the lower transition temperature also lowers the friction on wet surfaces, which is why polybutadiene almost always is used in combination with any of the other two elastomers.[15][27] About 1 kg of polybutadiene is used per tire in automobiles, and 3.3 kg in utility vehicles.[28] Plastics About 25% of the produced polybutadiene is used to improve the mechanical properties of plastics, in particular of high-impact polystyrene (HIPS) and to a lesser extent acrylonitrile butadiene styrene (ABS).[19][29] The addition of between 4 and 12% polybutadiene to polystyrene transforms it from a fragile and delicate material to a ductile and resistant one. The quality of the process is more important in the use in plastics than in tires, especially when it comes to color and content of gels which have to be as low as possible. In addition, the products need to meet a list of health requirements due to its use in the food industry. Golf balls A cross section of a golf ball; its core consists of polybutadiene Most golf balls are made of an elastic core of polybutadiene surrounded by a layer of a harder material. Polybutadiene is preferred to other elastomers due to its high resilience.[30] The core of the balls are formed by compression molding with chemical reactions. First, polybutadiene is mixed with additives, then extruded, pressed using a calender and cut into pieces which are placed in a mold. The mold is subjected to high pressure and high temperature for about 30 minutes, enough time to vulcanize the material. The golf ball production consumes about 20,000 tonnes of polybutadiene per year (1999).[19] Other uses Polybutadiene rubber may be used in the inner tube of hoses for sandblasting, along with natural rubber, to increase resilience. This rubber can also be used in the cover of hoses, mainly pneumatic and water hoses. Polybutadiene rubber can also be used in railway pads, bridge blocks, etc. Polybutadiene rubber can be blended with nitrile rubber for easy processing. However large use may affect the oil resistance of nitrile rubber. Polybutadiene is used in the manufacturing of the high-restitution toy Super Ball.[31] Due to the high resilience property, 100% polybutadiene rubber based vulcanizate is used as crazy balls — i.e. a ball if dropped from 6th floor of a house will rebound up to 5½ to 6th floor (assuming no air resistance). Polybutadiene is also used as binder in combination with an oxidizer and a fuel in various Solid Rocket Boosters such as Japan's H-IIB launch vehicle; commonly is employed as hydroxyl-terminated polybutadiene (HTPB) or carboxyl-terminated polybutadiene (CTPB).

DESCRIPTION:
LITHENE PM4 is a medium viscosity, low molecular weight, liquid polybutadiene.
LITHENE PM4 is very low in odour and volatiles and is produced from Lithene ultra PM4, adducted with 7.5 parts maleic anhydride


APPLICATIONS OF LITHENE PM4:
LITHENE PM4 is Adhesion promoter in automotive sealants
LITHENE PM4 is used in Rubber to metal adhesion promoter
LITHENE PM4 is Soft, isocyanate free electrical encapsulants
LITHENE PM4 is is despatched from our UK production plant.


SAFETY INFORMATION ABOUT LITHENE PM4:
First aid measures:
Description of first aid measures:
General advice:
Consult a physician.
Show this safety data sheet to the doctor in attendance.
Move out of dangerous area:

If inhaled:
If breathed in, move person into fresh air.
If not breathing, give artificial respiration.
Consult a physician.
In case of skin contact:
Take off contaminated clothing and shoes immediately.
Wash off with soap and plenty of water.
Consult a physician.

In case of eye contact:
Rinse thoroughly with plenty of water for at least 15 minutes and consult a physician.
Continue rinsing eyes during transport to hospital.

If swallowed:
Do NOT induce vomiting.
Never give anything by mouth to an unconscious person.
Rinse mouth with water.
Consult a physician.

Firefighting measures:
Extinguishing media:
Suitable extinguishing media:
Use water spray, alcohol-resistant foam, dry chemical or carbon dioxide.
Special hazards arising from the substance or mixture
Carbon oxides, Nitrogen oxides (NOx), Hydrogen chloride gas

Advice for firefighters:
Wear self-contained breathing apparatus for firefighting if necessary.
Accidental release measures:
Personal precautions, protective equipment and emergency procedures
Use personal protective equipment.

Avoid breathing vapours, mist or gas.
Evacuate personnel to safe areas.

Environmental precautions:
Prevent further leakage or spillage if safe to do so.
Do not let product enter drains.
Discharge into the environment must be avoided.

Methods and materials for containment and cleaning up:
Soak up with inert absorbent material and dispose of as hazardous waste.
Keep in suitable, closed containers for disposal.

Handling and storage:
Precautions for safe handling:
Avoid inhalation of vapour or mist.

Conditions for safe storage, including any incompatibilities:
Keep container tightly closed in a dry and well-ventilated place.
Containers which are opened must be carefully resealed and kept upright to prevent leakage.
Storage class (TRGS 510): 8A: Combustible, corrosive hazardous materials

Exposure controls/personal protection:
Control parameters:
Components with workplace control parameters
Contains no substances with occupational exposure limit values.
Exposure controls:
Appropriate engineering controls:
Handle in accordance with good industrial hygiene and safety practice.
Wash hands before breaks and at the end of workday.

Personal protective equipment:
Eye/face protection:
Tightly fitting safety goggles.
Faceshield (8-inch minimum).
Use equipment for eye protection tested and approved under appropriate government standards such as NIOSH (US) or EN 166(EU).

Skin protection:
Handle with gloves.
Gloves must be inspected prior to use.
Use proper glove
removal technique (without touching glove's outer surface) to avoid skin contact with this product.
Dispose of contaminated gloves after use in accordance with applicable laws and good laboratory practices.
Wash and dry hands.

Full contact:
Material: Nitrile rubber
Minimum layer thickness: 0.11 mm
Break through time: 480 min
Material tested:Dermatril (KCL 740 / Aldrich Z677272, Size M)
Splash contact
Material: Nitrile rubber
Minimum layer thickness: 0.11 mm
Break through time: 480 min
Material tested:Dermatril (KCL 740 / Aldrich Z677272, Size M)
It should not be construed as offering an approval for any specific use scenario.

Body Protection:
Complete suit protecting against chemicals, The type of protective equipment must be selected according to the concentration and amount of the dangerous substance at the specific workplace.
Respiratory protection:
Where risk assessment shows air-purifying respirators are appropriate use a fullface respirator with multi-purpose combination (US) or type ABEK (EN 14387) respirator cartridges as a backup to engineering controls.

If the respirator is the sole means of protection, use a full-face supplied air respirator.
Use respirators and components tested and approved under appropriate government standards such as NIOSH (US) or CEN (EU).
Control of environmental exposure
Prevent further leakage or spillage if safe to do so.
Do not let product enter drains.
Discharge into the environment must be avoided.

Stability and reactivity:
Chemical stability:
Stable under recommended storage conditions.
Incompatible materials:
Strong oxidizing agents:
Hazardous decomposition products:
Hazardous decomposition products formed under fire conditions.
Carbon oxides, Nitrogen oxides (NOx), Hydrogen chloride gas.

Disposal considerations:
Waste treatment methods:
Product:
Offer surplus and non-recyclable solutions to a licensed disposal company.
Contact a licensed professional waste disposal service to dispose of this material.
Contaminated packaging:
Dispose of as unused product

CHEMICAL AND PHYSICAL PROPERTIES OF LITHENE PM4:
Viscosity@ 25 °C 20 - 60
Total Acid 35 - 45 mg KOH/g
Residual maleic anhydride 0.1 max %
NVC (180 °C 30mins) >99.8 %
Typical molecular weight Mn 1600
Molecular weight distribution Broad
Appearance Dark brown viscous liquid

Lithium (+1) chloride is an ionic compound or salt that is highly polar and soluble in water.
The chemical formula for Lithium (+1) chloride is LiCl.
Lithium (+1) chloride is an inorganic chloride and a lithium salt.


CAS Number: 7447-41-8
EC Number: 231-212-3
MDL number: MFCD00011078
Chemical formula: LiCl



SYNONYMS:
LITHIUM CHLORIDE, 7447-41-8, LiCl, Lithiumchloride, chlorure de lithium, Chlorku litu, chlorolithium, Lithiumchlorid, Lithium chloride (LiCl), lithium;chloride, CCRIS 5924, CHEBI:48607, lithii chloridum, HSDB 4281, Lithium Cholride, cloruro de litio, Lithium chloride (powder), EINECS 231-212-3, MFCD00011078, NSC 327172, UNII-G4962QA067, LITHIUM MURIATICUM, G4962QA067, NSC-327172, Lithium Chloride, Anhydrous, CHEMBL69710, DTXSID2025509, EC 231-212-3, NSC327172, ClLi, LithiumChlorideGr(Anhydrous), 2M Lithium Chloride Electrolyte, Electrode Filling Solution, Lithium Chloride (2.3% in Tetrahydrofuran, ca. 0.5mol/L), lithim chloride, Lithium chloride, anhydrous, chunks, 99.99% trace metals basis, Lithium chloride anhydrous, Lopac-L-4408, LITHIUM MONOCHLORIDE, MolMap_000071, WLN: LI G, Lithium chloride, ultra dry, Lithium chloride, ACS grade, Lopac0_000604, LITHIUM CHLORIDE [MI], Lithium chloride battery grade, Lithium chloride, ACS reagent, DTXCID105509, LITHIUM CHLORIDE [HSDB], LITHIUM CHLORIDE [INCI], LITHIUM MURIATICUM [HPUS], LITHIUM CHLORIDE [WHO-DD], Lithium chloride, 3-5% in THF, Ultra dry, 99.9% metals basis, HMS3261J10, Tox21_500604, BDBM50494542, AKOS015902822, AKOS015950647, AKOS024438070, CCG-204693, lithium chloride, gamma irradiated, 8m, LP00604, SDCCGSBI-0050586.P002, Lithium chloride, ACS reagent, >=99%, Lithium chloride, ReagentPlus(R), 99%, NCGC00015607-01, NCGC00015607-02, NCGC00015607-03, NCGC00015607-04, NCGC00015607-07, NCGC00093980-01, NCGC00093980-02, NCGC00261289-01, 59217-69-5, BP-13612, SY002997, Lithium chloride, Vetec(TM) reagent grade, EU-0100604, L0204, L0222, Lithium chloride, Trace metals grade 99.9%, NS00075680, L 4408, Lithium chloride, SAJ first grade, >=98.0%, Lithium chloride, for molecular biology, >=99%, Lithium chloride, SAJ special grade, >=99.0%, A838146, Lithium chloride, BioXtra, >=99.0% (titration), Q422930, SR-01000076252, SR-01000076252-1, Lithium chloride, powder, >=99.99% trace metals basis, Lithium chloride, puriss. p.a., anhydrous, >=99.0% (AT), Lithium chloride, anhydrous, beads, -10 mesh, >=99.9% trace metals basis, Lithium chloride, anhydrous, beads, -10 mesh, 99.998% trace metals basis, Lithium chloride, puriss. p.a., ACS reagent, anhydrous, >=99.0% (AT), Lithium chloride, anhydrous, free-flowing, Redi-Dri(TM), ACS reagent, >=99%, Lithium chloride, anhydrous, free-flowing, Redi-Dri(TM), ReagentPlus(R), 99%, Lithium chloride, BioUltra, for molecular biology, anhydrous, >=99.0% (AT), Lithium (+1) chloride, BioXtra, >=99.0% (titration), Q422930, SR-01000076252, SR-01000076252-1, Lithium (+1) chloride, powder, >=99.99% trace metals basis, Lithium (+1) chloride, puriss. p.a., anhydrous, >=99.0% (AT), Lithium (+1) chloride, anhydrous, beads, -10 mesh, >=99.9% trace metals basis, Lithium (+1) chloride, anhydrous, beads, -10 mesh, 99.998% trace metals basis, Lithium (+1) chloride, puriss. p.a., ACS reagent, anhydrous, >=99.0% (AT), Lithium (+1) chloride, anhydrous, free-flowing, Redi-Dri(TM), ACS reagent, >=99%, Lithium (+1) chloride, anhydrous, free-flowing, Redi-Dri(TM), ReagentPlus(R), 99%, Lithium (+1) chloride, BioUltra, for molecular biology, anhydrous, >=99.0% (AT), 59217-69-5, Hydrochloric acid lithium salt, Lithium (+1) chloride, Lithium (+1) chloride licl, lithiumchloride, licl, chlorure de lithium, chlorku litu, chlorolithium, lithiumchlorid, chlorku litu polish, luthium chloride, Lithium (+1) chloride, Lithium (+1) chloride licl, lithiumchloride, licl, chlorure de lithium, chlorku litu, chlorolithium, lithiumchlorid, chlorku litu polish, luthium chloride, Lithium (+1) chloride, Lithium(1+) chloride, LITHIUM (+1) CHLORIDE, 7447-41-8, LiCl, Lithiumchloride, chlorure de lithium, chlorolithium, Lithiumchlorid, Lithium (+1) chloride (LiCl), lithium;chloride, CCRIS 5924, CHEBI:48607, lithii chloridum, HSDB 4281, Lithium Cholride, cloruro de litio, Lithium (+1) chloride (powder), EINECS 231-212-3, MFCD00011078, NSC 327172, UNII-G4962QA067, LITHIUM MURIATICUM, G4962QA067, NSC-327172, Lithium (+1) chloride, Anhydrous, LithiumChlorideG (Anhydrous), CHEMBL69710, DTXSID2025509, EC 231-212-3, NSC327172, Lithium (+1) chloride, ultra dry, Luthium chloride, Chloride, Lithium, Lithium (+1) chloride (2.3% in Tetrahydrofuran, ca. 0.5mol/L), lithim chloride, Lopac-L-4408, LITHIUM MONOCHLORIDE, MolMap_000071, WLN: LI G, Lithium (+1) chloride, ACS grade, Lopac0_000604, LITHIUM (+1) CHLORIDE [MI], Lithium (+1) chloride battery grade, Lithium (+1) chloride, ACS reagent, DTXCID105509, LITHIUM (+1) CHLORIDE [HSDB], LITHIUM (+1) CHLORIDE [INCI], LITHIUM MURIATICUM [HPUS], KWGKDLIKAYFUFQ-UHFFFAOYSA-M, LITHIUM (+1) CHLORIDE [WHO-DD], Lithium (+1) chloride, 3-5% in THF, HMS3261J10, Tox21_500604, BDBM50494542, AKOS015902822, AKOS015950647, AKOS024438070, CCG-204693, Lithium (+1) chloride, gamma irradiated, 8m, LP00604, SDCCGSBI-0050586.P002, Lithium (+1) chloride, ACS reagent, >=99%, Lithium (+1) chloride, ReagentPlus(R), 99%, NCGC00015607-01, NCGC00015607-02, NCGC00015607-03, NCGC00015607-04, NCGC00015607-07, NCGC00093980-01, NCGC00093980-02, NCGC00261289-01, BP-13612, SY002997, Lithium (+1) chloride, Vetec(TM) reagent grade, EU-0100604, FT-0627896, L0204, L0222, Lithium (+1) chloride, Trace metals grade 99.9%, L 4408, Lithium (+1) chloride, SAJ first grade, >=98.0%, Lithium (+1) chloride, for molecular biology, >=99%, Lithium (+1) chloride, SAJ special grade, >=99.0%, A838146, lithium chloride, lithium chloride licl, lithiumchloride, licl, chlorure de lithium, chlorku litu, chlorolithium, lithiumchlorid, chlorku litu polish, luthium chloride



Lithium (+1) chloride is a typical ionic compound (with certain covalent characteristics), although the small size of the Li+ ion gives rise to properties not seen for other alkali metal chlorides, such as extraordinary solubility in polar solvents (83.05 g/100 mL of water at 20 °C) and its hygroscopic properties.


Lithium (+1) chloride appears as colorless crystals or powder.
Lithium (+1) chloride is for assays to study cell-fate, neurobiology and antiviral properties; noted to inhibit GSK-3β
Lithium (+1) chloride is hygroscopic in nature.


Lithium (+1) chloride is incompatible with strong oxidizing agents, strong acids, bromine trichloride and bromine trifluoride.
Lithium (+1) chloride is an ionic compound or salt that is highly polar and soluble in water.
The chemical formula for Lithium (+1) chloride is LiCl.


Lithium (+1) chloride is an inorganic chloride and a lithium salt.
Lithium (+1) chloride is a chemical compound with a chemical formula “LiCl”.
The salt is a normal ionic compound, although the Li+ ion is small in size, Lithium (+1) chloride produces unrecognized effects for other alkali metal chlorides, such as exceptional solubility in polar solvents and its hygroscopic properties.


Lithium (1+) chloride is registered under the REACH Regulation and is manufactured in and / or imported to the European Economic Area, at ≥ 1 000 to < 10 000 tonnes per annum.
Lithium (+1) chloride is an injection indicated for cardiac output measurement.


Crystallization grade Lithium (+1) chloride for formulating screens or for optimization.
The chemical formula of anhydrous Lithium (+1) chloride is LiCl, the relative molecular weight is 42.39, which is cubic crystal white particles or powder, which is easy to deliquesce and tastes salty.


Lithium (+1) chloride belongs to the low-toxicity category, but has a strong irritating and corrosive effect on the eyes and mucous membranes.
The specific gravity of Lithium (+1) chloride is 2.068, the melting point is 605°C, the boiling point is 1360°C, and it is easily soluble in water grams (0°C) in 100 grams of water, 127.5 grams (100°C)].


Lithium (+1) chloride has a typical shelf life of 2 years if kept in dry conditions.
Lithium (+1) chloride appears as colorless crystals or powder.
The resulting solution is evaporated to get a mixture of saturated solution and Lithium (+1) chloride crystals.


Lithium (+1) chloride is hygroscopic and highly soluble in water, and is highly polar.
Lithium (+1) chloride is more soluble in polar organic solvents such as methanol and acetone than is sodium chloride or potassium chloride.
Lithium (+1) chloride is a chemical compound with the formula LiCl.


Deliquescent salt forms a solution when exposed to humid air.
Store Lithium (+1) chloride in a cool and dry place in closed tight containers.
Lithium (+1) chloride is a typical ionic compound and a salt of lithium.


Due to the small size of the lithium-ion ( Li+ ), Lithium (+1) chloride gives rise to properties that we cannot see in other alkali metal chlorides.
Lithium (+1) chloride is an antiviral metal halide utilized in a variety of assays to study cell-fate and neurobiology.
In developing Xenopus embryos, Lithium (+1) chloride is observed to exert inhibition of GSK-3β (glycogen synthase kinase-3β), yet not reported to be a general inhibitor of other protein kinases.


Lithium (+1) chloride is more soluble in organic solvents such as acetone and methanol than potassium chloride or sodium chloride.
Lithium (+1) chloride is a salt of Lithium chlorine, an alkali metal similar to sodium chloride.
Although the Li+ ion is minuscule, Lithium (+1) chloride creates unrecognized effects for other alkali metal chlorides, such as being soluble in polar solvents and having hygroscopic (holding water molecules) properties.


The solid and the solution is separated and the supernatant solution is recycled for further evaporation.
Lithium (+1) chloride is a solid which absorbs water to form a hydrate, LiCl.H2O
Lithium (+1) chloride is a solid which absorbs water to form a hydrate, LiCl.H2O.


Lithium (+1) chloride is soluble in alcohol, slightly soluble in acetone, pyridine and liquid ammonia.
Lithium (+1) chloride is a chemical compound with the formula LiCl.
Lithium (+1) chloride behaves as a fairly typical ionic compound, although the Li+ ion is very small.


Lithium (+1) chloride acts as an electrolyte for dry cells used at low temperatures, catalyst in certain oxidation reactions, solubilizer for polyamides and cellulose when used with amide solvents, chlorinating agent for steroid substrates.
Lithium (+1) chloride is registered under the REACH Regulation and is manufactured in and / or imported to the European Economic Area, at ≥ 1 000 to < 10 000 tonnes per annum.


Lithium (+1) chloride is a metal chloride salt with a Li (+) counterion.
Lithium (+1) chloride has a role as an antimanic drug and a geroprotector.
Lithium (+1) chloride is an inorganic chloride and a lithium salt.


Lithium (+1) chloride is a salt of lithium that has been used experimentally as an immunomodulator.
Lithium (+1) chloride is a white solid hygroscopic soluble in water, alcohol and ether.
Lithium (+1) chloride is made by the action of hydrochloric acid on lithium hydroxide.
These observations may have implications for Lithium (+1) chloride on cell-fate determination in several organisms including Xenopus and Dictyostelium.


The antiviral properties of Lithium (+1) chloride were noted in a study which showed that the compound inhibited pseudorabis virus infection in vitro.
In Drosophila, it was observed that in the nervous system, Lithium (+1) chloride may have an effect on amino acid metabolism.
Futhermore, in glial primary cell cultures, Lithium (+1) chloride has been noted to provide protection against glutamate excitotoxicity by potentially reducing NR1 mRNA, the major N-methyl-D-aspartate receptor (NMDAR) subunit in the cells.



USES and APPLICATIONS of LITHIUM (1+) CHLORIDE:
Lithium (1+) chloride is used in air-conditioning, welding and soldering flux, dry batteries, heat-exchange media, salt baths, and desiccants.
Lithium (1+) chloride is useful for the production of lithium metal, and for the generation of Mn(0) species which can be used in free radical cyclizations.


Release to the environment of Lithium (1+) chloride can occur from industrial use: in processing aids at industrial sites, as an intermediate step in further manufacturing of another substance (use of intermediates), as processing aid, of substances in closed systems with minimal release and in the production of articles.


Lithium (+1) chloride is also used as a flame colorant to produce dark red flames.
Molten Lithium (+1) chloride is used for the preparation of carbon nanotubes, graphene and lithium niobate.
Lithium (+1) chloride has been shown to have strong acaricidal properties, being effective against Varroa destructor in populations of honey bees.


Lithium (+1) chloride is used as an aversive agent in lab animals to study conditioned place preference and aversion.
Lithium (+1) chloride is widely used in several industrial applications.
Lithium (+1) chloridet is used as a flame colorant to form dark crimson flames.


Lithium (1+) chloride can serve as a flame colorant to generate dark red flames, a brazing flux for aluminum in automobiles, a hygrometer, and a desiccant for drying air streams.
Lithium (1+) chloride is used by consumers, in articles, by professional workers (widespread uses), in formulation or re-packing, at industrial sites and in manufacturing.


Lithium (+1) chloride is a very effective antimanic drug for the treatment of bipolar disorder.
Lithium (+1) chloride is well soluble in water, alcohol, acetone, and amyl alcohol and Lithium (+1) chloride is also used as a flame colorant to produce dark red flames.


Lithium (+1) chloride is used as an electrolyte in voltaic cells.
Lithium (+1) chloride is used in supplements.
Lithium (1+) chloride is used in the following products: coating products, metal surface treatment products, non-metal-surface treatment products, adhesives and sealants, inks and toners, pH regulators and water treatment products, photo-chemicals, polishes and waxes and welding & soldering products.


Lithium (+1) chloride is used fluxes for welding and soldering techniques; salt bath for heat-treatment by low temperature and for dip brazing; raw material for other lithium compounds; tracer for chemical products (denaturation of wine etc.); absorption and desinfection reagent (Lithium (+1) chloride solution) for absorbers.


Other release to the environment of Lithium (1+) chloride is likely to occur from: indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners), outdoor use, indoor use in close systems with minimal release (e.g. cooling liquids in refrigerators, oil-based electric heaters), outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids), outdoor use in long-life materials with low release rate (e.g. metal, wooden and plastic construction and building materials) and indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment).


Release to the environment of Lithium (1+) chloride can occur from industrial use: industrial abrasion processing with low release rate (e.g. cutting of textile, cutting, machining or grinding of metal).
On exposure to air, Lithium (1+) chloride becomes a solution with the concentration directly related to relative humidity of the atmosphere, and hence serves as a relative humidity standard in calibrating hygrometers.


Lithium (1+) chloride is used for the manufacture of: chemicals, plastic products and pulp, paper and paper products.
Industries use Lithium (+1) chloride's molten form to prepare carbon nanotubes, lithium niobate, and grapheme.
Besides, Lithium (+1) chloride shows very strong acaricidal properties.


Lithium (+1) chloride is a chemical compound that is extremely soluble in polar solvents and is used in order to obtain lithium metal.
In organic synthesis Lithium (+1) chloride is used as an additive in the Stille Reaction.
Ungraded products supplied by Spectrum are indicative of a grade suitable for general industrial use or research purposes and typically are not suitable for consumption.


Lithium (+1) chloride is used by consumers, in articles, by professional workers (widespread uses), in formulation or re-packing, at industrial sites and in manufacturing.
Lithium (+1) chloride is used in the following products: coating products, metal surface treatment products, non-metal-surface treatment products, adhesives and sealants, inks and toners, pH regulators and water treatment products, photo-chemicals, polishes and waxes and welding & soldering products.


Lithium (+1) chloride is useful for the production of lithium metal and for the generation of Mn(0) species which can be used in free radical cyclizations.
Lithium (+1) chloride can serve as a flame colorant to generate dark red flames, a brazing flux for aluminum in automobiles, a hygrometer and a desiccant for drying air streams.


Other release to the environment of this substance is likely to occur from: indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment). This substance can be found in products with material based on: stone, plaster, cement, glass or ceramic (e.g. dishes, pots/pans, food storage containers, construction and isolation material) and paper (e.g. tissues, feminine hygiene products, nappies, books, magazines, wallpaper).


Lithium (+1) chloride is used in the following products: laboratory chemicals, pH regulators and water treatment products, metal working fluids, pharmaceuticals, polymers, water treatment chemicals and welding & soldering products.
Lithium (+1) chloride is used in the following areas: scientific research and development and health services.


Lithium (+1) chloride is used in the following products: pharmaceuticals, air care products, inks and toners, laboratory chemicals, metal working fluids, paper chemicals and dyes, polymers, water treatment chemicals and welding & soldering products.
Release to the environment of Lithium (+1) chloride can occur from industrial use: formulation of mixtures and formulation in materials.


Being biologically significant, Lithium (1+) chloride finds applications in a wide variety of assays to study cell-fate and neurobiology.
Release to the environment of Lithium (1+) chloride can occur from industrial use: manufacturing of the substance.
Lithium (+1) chloride is used in the precipitation of RNA in biological applications.


Lithium (+1) chloride is an aluminum blazing flux in automobile parts.
Lithium (+1) chloride can be used as a hygrometer. In addition, when exposed to air it salts from deliquescent self-solution.
Furthermore, the equilibrium Lithium (+1) chloride concentration of the resulting solution may directly relate to the relative humidity of the air.


It depends on the low equilibrium pressure of water vapour above solutions of Lithium (+1) chloride.
Lithium (+1) chloride is used in a number of salt mixtures exist low melting points allowing the material to be used in brazing fluxes and brazing baths.
Lithium Metal by Electrolysis: Lithium (+1) chloride is primarily used at 450 ° C (842 ° F) for the preparation of lithium metal by electrolysis of a LiCl / KCl.


As Brazing Flux uses of Lithium (+1) chloride: Lithium (+1) chloride is also used as a brazing flux for aluminum in automobile parts.
Lithium (+1) chloride is used as desiccant in drying air streams.
Lithium (+1) chloride is used in organic synthesis.


For example, as an additive in the Stille reaction.
Apart from being a source of chloride, Lithium (1+) chloride serves as an additive in the Stille reaction in organic synthesis, and to precipitate RNA from cellular extracts.


Other release to the environment of Lithium (+1) chloridee is likely to occur from: indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners), outdoor use, indoor use in close systems with minimal release (e.g. cooling liquids in refrigerators, oil-based electric heaters), outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids), outdoor use in long-life materials with low release rate (e.g. metal, wooden and plastic construction and building materials) and indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment).


Lithium (1+) chloride is used in the following areas: scientific research and development and health services.
On exposure to air, Lithium (+1) chloride becomes a solution with the concentration directly related to relative humidity of the atmosphere and hence serves as a relative humidity standard in calibrating hygrometers.


Apart from being a source of chloride, Lithium (+1) chloride serves as an additive in the Stille reaction in organic synthesis and to precipitate RNA from cellular extracts.
Lithium (+1) chloride is used for the manufacture of: chemicals and plastic products.


Lithium (+1) chloride is used for the manufacture of: chemicals, plastic products and pulp, paper and paper products.
Lithium (+1) chloride is used for several soldering and welding techniques and salt bath heat treatment at low temperatures.
Lithium (+1) chloride is used in massive dehumidification systems in the AC industry.


This depends on the low equilibrium pressure of vapor above Lithium (+1) chloride solutions.
Lithium (+1) chloride is used in large dehumidification systems in the air conditioning industry.
Release to the environment of Lithium (+1) chloride can occur from industrial use: manufacturing of the substance.


As a flame colorant, Lithium (+1) chloride is used to produce dark red flames.
Lithium (+1) chloride is used as a Relative humidity standard in the calibration of hygrometers and itself can be used as a hygrometer.
Molten Lithium (+1) chloride is used for the preparation of lithium niobite, graphene and carbon nanotubes.


Lithium (+1) chloride has been found to inhibit virus infection.
Lithium (+1) chloride has strong acaricidal properties (Varroa destructor in populations of honey bees).
Biochemical Applications: LiCl is used to precipitate RNA from cellular extracts.


Lithium (+1) chloride is used to produce a dark red flame.
Lithium (+1) chloride is used as a brazing flux, as a desiccant in drying air streams, as a component in organic synthesis, as an additive in the Stille reaction, in some biochemical applications, and as soldering aluminum metal.


Lithium (+1) chloride is used for the production of lithium metal, by electrolysis of a LiCl/KCl melt at 450 °C.
Lithium (+1) chloride is also used as a brazing flux for aluminium in automobile parts.
Lithium (+1) chloride can be used to improve the efficiency of the Stille reaction.


Lithium (+1) chloride's desiccant properties can be used to generate potable water by absorbing moisture from the air, which is then released by heating the salt.
Other release to the environment of Lithium (1+) chloride is likely to occur from: indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment).


Lithium (+1) chloride is also used in organic synthesis.
Lithium (+1) chloride is used to precipitate RNA.
Lithium (+1) chloride has many applications.


Lithium (+1) chloride is extremely hygroscopic, and is widely used in dehumidification systems to remove moisture from the air in industries such as food processing and horticulture.
Lithium (+1) chloride is used as an electrolyte for the production of lithium metal and used as an electrolyte in voltaic cells.


Other release to the environment of Lithium (+1) chloride is likely to occur from: indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners), outdoor use, indoor use in close systems with minimal release (e.g. cooling liquids in refrigerators, oil-based electric heaters), outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids), outdoor use in long-life materials with low release rate (e.g. metal, wooden and plastic construction and building materials) and indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment).


Lithium (1+) chloride can be found in products with material based on: stone, plaster, cement, glass or ceramic (e.g. dishes, pots/pans, food storage containers, construction and isolation material) and paper (e.g. tissues, feminine hygiene products, nappies, books, magazines, wallpaper).
Lithium (+1) chloride has also been utilized in: Large scale plasmid DNA isolation without ultracentrifugation; Protein extraction and protein crystallization;


Crystallization of other biological structures, including vitamin B12-RNA aptamer and the L-A virus particle; Inhibits the expression and secretion of insulin-like growth factor-binding protein-1 in H4-II-E cells; Used in the synthesis of beta-substituted alpha-amino acid derivatives; May be used to selectively pre­cipitate RNA.


Lithium (1+) chloride is used in the following products: laboratory chemicals, pH regulators and water treatment products, metal working fluids, pharmaceuticals, polymers, water treatment chemicals and welding & soldering products.
Lithium (1+) chloride is used in the following areas: scientific research and development and health services.


Other release to the environment of Lithium (1+) chloride is likely to occur from: indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners), outdoor use, indoor use in close systems with minimal release (e.g. cooling liquids in refrigerators, oil-based electric heaters), outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids), outdoor use in long-life materials with low release rate (e.g. metal, wooden and plastic construction and building materials) and indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment).


Lithium (+1) chloride is also used as a tracer for waste water, as a brazing flux, and as an electrolyte component for the manufacture of speciality batteries.
Lithium (+1) chloride is used as an electrolyte for low temperature dry battery cells and as an oxidation catalyst.


Lithium (+1) chloride is a solubilizer for polyamides and cellulose when used with amide solvents, and is a chlorinating agent for steroid substrates.
Lithium (+1) chloride is mainly we use it for the production of lithium metal by electrolysis of LiCl/KCl which melt at 450oC.
Moreover, industries use Lithium (+1) chloride as a brazing flux for aluminum in automobile parts.


In addition, we use Lithium (+1) chloride as a desiccant for drying air streams.
Release to the environment of Lithium (1+) chloride can occur from industrial use: formulation of mixtures and formulation in materials.
Lithium (1+) chloride is used in the following products: welding & soldering products, laboratory chemicals, air care products, inks and toners, pH regulators and water treatment products, metal working fluids, pharmaceuticals, polymers and water treatment chemicals.


In organic synthesis, Lithium (+1) chloride has some specialized applications such as an additive in the Stille reaction.
Most noteworthy, Lithium (+1) chloride has biochemical applications that we use to precipitate RNA from cellular extracts.
Another application of Lithium (+1) chloride is that we use it as a flame colorant to produce dark red flames.


In the calibration of hygrometers, they use Lithium (+1) chloride as a relative humidity standard.
Lithium (1+) chloride has been found to inhibit virus infection.
Lithium (1+) chloride is also used for air conditioning, pyrotechnics, dry batteries and lithium metal, also used as a flux and desiccant.


Lithium (+1) chloride is useful for the production of lithium metal and for the generation of Mn(0) species which can be used in free radical cyclizations.
Lithium (+1) chloride can serve as a flame colorant to generate dark red flames, a brazing flux for aluminum in automobiles, a hygrometer and a desiccant for drying air streams.


Being biologically significant, Lithium (+1) chloride finds applications in a wide variety of assays to study cell-fate and neurobiology.
Lithium (+1) chloride has been found to inhibit virus infection.
Lithium (1+) chloride is used for the manufacture of: chemicals and plastic products.


Release to the environment of Lithium (+1) chloride can occur from industrial use: industrial abrasion processing with low release rate (e.g. cutting of textile, cutting, machining or grinding of metal).
Lithium (+1) chloride is used in the following products: welding & soldering products, laboratory chemicals, air care products, inks and toners, pH regulators and water treatment products, metal working fluids, pharmaceuticals, polymers and water treatment chemicals.


Release to the environment of Lithium (+1) chloride can occur from industrial use: in processing aids at industrial sites, as an intermediate step in further manufacturing of another substance (use of intermediates), as processing aid, of substances in closed systems with minimal release and in the production of articles.


Lithium (1+) chloride is used in the following products: pharmaceuticals, air care products, inks and toners, laboratory chemicals, metal working fluids, paper chemicals and dyes, polymers, water treatment chemicals and welding & soldering products.
Lithium (+1) chloride is used in the following areas: scientific research and development and health services.



PROPERTIES OF LITHIUM (+1) CHLORIDE:
1. Physical Properties of Lithium (+1) chloride Licl:
Lithium (+1) chloride is Deliquescent in nature, appear as cubic crystals, granules or crystalline powder
Lithium (+1) chloride has sharp saline taste

Lithium (+1) chloride has Boiling point of 2417 to 2480 °F at 760 mm Hg
Lithium (+1) chloride's Melting point is 1121 °F
Lithium (+1) chloride has Density of 2.068 at 77 °F

Aqueous solution of Lithium (+1) chloride is neutral or slightly alkaline.
Lithium (+1) chloride is very soluble in water alcohols, ether, pyridine, nitrobenzene



FEATURES OF LITHIUM (+1) CHLORIDE:
Sterile filtered solution:
Formulated in Type 1+ ultrapure water: 18.2 megaohm-cm resistivity at 25°C, < 5 ppb Total Organic Carbon, bacteria free (<1 Bacteria (CFU/ml)), pyrogen free (<0.03 Endotoxin (EU/ml)), RNase-free (< 0.01 ng/mL) and DNase-free (< 4 pg/µL)



PHYSICAL PROPERTIES OF LITHIUM (+1) CHLORIDE:
Lithium (+1) chloride appears as an odorless white crystalline hygroscopic solid.
Lithium (+1) chloride has a density of 2.068g/cm3 and its boiling point is 1382oC and its melting point is in between 605–614oC.
Lithium (+1) chloride is soluble in water, methanol, ethanol, isopropanol, butanol, formic acid, n- mehtylformamide, hydrazine, and THF.

In addition, Lithium (+1) chloride is slightly soluble in acetone and ammonia and is completely insoluble in dichloromethane.
Lithium (+1) chloride has a sharp, saline taste.
Lithium (+1) chloride has cubic crystals, crystalline powder, or granule appearance.

Lithium (+1) chloride has a melting point of 121°F and 2.068 density at 77°F.
Lithium (+1) chloride's aqueous solution is neutral and a bit alkaline.
Lithium (+1) chloride is soluble in ether, nitrobenzene, and water alcohols.



PREPARATION OF LITHIUM (+1) CHLORIDE:
Lithium (+1) chloride is produced by treatment of lithium carbonate with hydrochloric acid.
Anhydrous Lithium (+1) chloride is prepared from the hydrate by heating in a stream of hydrogen chloride.



FUNCTION AND PURPOSE OF LITHIUM (+1) CHLORIDE:
Raw material for preparing metallic lithium.
Flux in the production of metal by electrolysis (such as the production of titanium and aluminum), used as aluminum welding agent, air conditioning dehumidifier and special cement raw material, also used in flames, in the battery industry for the production of lithium manganese battery electrolyte, etc.
Anhydrous Lithium (+1) chloride is mainly used for electrolytic preparation of metallic lithium and aluminum fluxes and fluxes, as well as moisture absorbing (dehumidifying) agents in non-refrigerated air conditioners.



WHAT HAPPENS WHEN LITHIUM (1+) CHLORIDE IS DISSOLVED IN WATER?
When Lithium (1+) chloride is dissolved in water, it has less energy than the reactant, thus losing energy during the reaction.
The energy is transferred around by heat, which is a heat-releasing reaction.
Therefore, the solution should be very hot.



CHEMICAL PROPERTIES OF LITHIUM (+1) CHLORIDE:
Like other metal chlorides Lithium (+1) chloride's salt form crystalline hydrates.
Furthermore, Lithium (+1) chloride's mono-, tri-, pentahydrate are known.
We can regenerate Lithium (+1) chloride's anhydrous salts by heating the hydrates.

In addition, Lithium (+1) chloride easily absorbs up to four equivalents of ammonia/mol.
However, with another ionic chloride, the solution of Lithium (+1) chloridecan serve as a source of chloride ion.
Lithium (+1) chloride reaction with sulfuric acid forms lithium sulfate and hydrogen chloride.
The chemical equation is given below.

2LiCl + H2SO4 → 2 HCl + Li2SO4
Lithium (+1) chloride reacts with a base like sodium hydroxide and forms lithium hydroxide and sodium chloride.
LiCl + NaOH → LiOH + NaCl

Lithium (+1) chloride Reaction with Sulfuric Acid:
When Lithium (+1) chloride reacts with sulfuric acid, it forms lithium sulfate and hydrogen chloride.
The chemical equation is given below.
2LiCl+H2SO4→2HCl+Li2SO4

The salt forms crystalline hydrates, unlike the other alkali metal chlorides.
Mono-, tri-, and pentahydrates are known.
The anhydrous salt can be regenerated by heating the hydrates.

Lithium (+1) chloride also absorbs up to four equivalents of ammonia/mol.
As with any other ionic chloride, solutions of Lithium (+1) chloride can serve as a source of chloride ion, e.g., forming a precipitate upon treatment with silver nitrate:
LiCl + AgNO3 → AgCl + LiNO3

Reaction with Sulfuric Acid:
Lithium (+1) chloride and sulfuric acid reaction form hydrogen chloride and lithium sulfate.
Here is the reaction’s chemical equation:
2LiCl+H2SO4→2HCl+Li2SO4

When Lithium (+1) chloride reacts with H2SO4 it gives lithium sulfate and hydrogen chloride.
2LiCl + H2SO4 → 2 HCl + Li2SO4
When Lithium (+1) chloride reacts with a base like NaOH it gives lithium hydroxide and sodium chloride.
LiCl + NaOH → LiOH + NaCl



STRUCTURE OF LITHIUM (+1) CHLORIDE:
Lithium (+1) chloride structure LiCl is drawn with the help of lewis dots
Lithium (+1) chloride is ionic compound, in which Lithium is a metal compound and chloride is a non-metal.

Where electrons are transferred from metal ion to non-metal ion.
One electron is transferred from lithium and makes Lithium (+1) chloride electro-positive and by gaining one electron from lithium, chlorine becomes electronegative.



PHYSICAL and CHEMICAL PROPERTIES of LITHIUM (1+) CHLORIDE:
Boiling Point: 1325°C to 1360°C
Melting Point: 605°C
Physical Form: Granules
Assay Percent Range: 99%
Solubility Information: Very soluble in water, alcohol, ether, pyridine, and nitrobenzene.
Formula Weight: 42.39
Grade: ACS Reagent
Sensitivity: Hygroscopic
Density: 2.068 g/mL
Chemical Name or Material: Lithium chloride
Chemical Formula: LiCl
Molar Mass: 42.39 g·mol−1
Appearance: White solid, hygroscopic, sharp
Density: 2.068 g/cm3
Melting Point: 605–614 °C (1,121–1,137 °F; 878–887 K)
Boiling Point: 1,382 °C (2,520 °F; 1,655 K)

Solubility in Water:
68.29 g/100 mL (0 °C)
74.48 g/100 mL (10 °C)
84.25 g/100 mL (25 °C)
88.7 g/100 mL (40 °C)
123.44 g/100 mL (100 °C)
Solubility:
Soluble in hydrazine, methylformamide, butanol,
selenium(IV) oxychloride, 1-propanol
Solubility in Methanol:
45.2 g/100 g (0 °C)
43.8 g/100 g (20 °C)
42.36 g/100 g (25 °C)
44.6 g/100 g (60 °C)
Solubility in Ethanol:
14.42 g/100 g (0 °C)
24.28 g/100 g (20 °C)
25.1 g/100 g (30 °C)
23.46 g/100 g (60 °C)

Solubility in Formic Acid:
26.6 g/100 g (18 °C)
27.5 g/100 g (25 °C)
Solubility in Acetone:
1.2 g/100 g (20 °C)
0.83 g/100 g (25 °C)
0.61 g/100 g (50 °C)
Solubility in Liquid Ammonia:
0.54 g/100 g (-34 °C)
3.02 g/100 g (25 °C)
Vapor Pressure:
1 torr (785 °C)
10 torr (934 °C)
100 torr (1130 °C)
Magnetic Susceptibility (χ): −24.3·10−6 cm3/mol
Refractive Index (nD): 1.662 (24 °C)
Viscosity: 0.87 cP (807 °C)

Structure:
Coordination Geometry: Octahedral
Molecular Shape: Linear (gas)
Dipole Moment: 7.13 D (gas)
Thermochemistry:
Heat Capacity (C): 48.03 J/mol·K
Std Molar Entropy (S⦵298): 59.31 J/mol·K
Std Enthalpy of Formation (ΔfH⦵298): -408.27 kJ/mol
Gibbs Free Energy (ΔfG⦵): -384 kJ/mol
Appearance: White solid hygroscopic
Covalently-Bonded Unit: 2
Specific Gravity: 2.068 at 77 ° F
Complexity: 2
Solubility: Insoluble in water
CAS: 7447-41-8

MF: LiCl
MW: 42.39
EINECS: 231-212-3
Mol File: 7447-41-8.mol
Lithium chloride Chemical Properties:
Melting point: 605 °C(lit.)
Boiling point: 1382°C
density: 2.06
vapor pressure: 1.33 hPa (547 °C)
refractive index: n20/D 1.381
Fp: -4 °F
storage temp.: 2-8°C
solubility: H2O: soluble
form: beads
color: White to gray

Specific Gravity: 2.068
Odor: Odorless
PH: 5.5-7.5 (25℃, 50mg/mL in H2O)
PH Range: 6
Water Solubility: 832 g/L (20 ºC)
λmax: λ: 260 nm Amax: 0.01
λ: 280 nm Amax: 0.01
Sensitive: Hygroscopic
Merck: 145,528
Stability: Stable.
InChIKey: KWGKDLIKAYFUFQ-UHFFFAOYSA-M
CAS DataBase Reference: 7447-41-8(CAS DataBase Reference)
NIST Chemistry Reference: Lithium chloride(7447-41-8)
EPA Substance Registry System: Lithium chloride (7447-41-8)
Linear Formula: LiCl
UN Number: NONH for all modes of transport

Formula Weight: 42.39g/mol
Chemical Name or Material: Lithium Chloride
Chemical formula: LiCl
Molar mass: 42.39 g•mol−1
Appearance: white solid
hygroscopic, sharp
Density: 2.068 g/cm3
Melting point: 605–614 °C (1,121–1,137 °F; 878–887 K)
Boiling point: 1,382 °C (2,520 °F; 1,655 K)
Solubility in water: 68.29 g/100 mL (0 °C)
74.48 g/100 mL (10 °C)
84.25 g/100 mL (25 °C)
88.7 g/100 mL (40 °C)
123.44 g/100 mL (100 °C)
Solubility: soluble in hydrazine, methylformamide,
butanol, selenium(IV) oxychloride, 1-propanol

Solubility in methanol: 45.2 g/100 g (0 °C)
43.8 g/100 g (20 °C)
42.36 g/100 g (25 °C)
44.6 g/100 g (60 °C)
Solubility in ethanol: 14.42 g/100 g (0 °C)
24.28 g/100 g (20 °C)
25.1 g/100 g (30 °C)
23.46 g/100 g (60 °C)
Solubility in formic acid: 26.6 g/100 g (18 °C)
27.5 g/100 g (25 °C)
Solubility in acetone: 1.2 g/100 g (20 °C)
0.83 g/100 g (25 °C)
0.61 g/100 g (50 °C)
Solubility in liquid ammonia: 0.54 g/100 g (-34 °C)
3.02 g/100 g (25 °C)

Vapor pressure: 1 torr (785 °C)
10 torr (934 °C)
100 torr (1130 °C)
Magnetic susceptibility (χ): −24.3•10−6 cm3/mol
Refractive index (nD): 1.662 (24 °C)
Viscosity: 0.87 cP (807 °C)
Structure:
Coordination geometry: Octahedral
Molecular shape: Linear (gas)
Dipole moment: 7.13 D (gas)
Thermochemistry:
Heat capacity (C): 48.03 J/mol•K
Std molar entropy (S⦵298): 59.31 J/mol•K
Std enthalpy of formation (ΔfH⦵298): -408.27 kJ/mol
Gibbs free energy (ΔfG⦵): -384 kJ/mol
Molecular Weight: 42.4 g/mol

Hydrogen Bond Donor Count: 0
Hydrogen Bond Acceptor Count: 1
Rotatable Bond Count: 0
Exact Mass: 41.9848561 g/mol
Monoisotopic Mass: 41.9848561 g/mol
Topological Polar Surface Area: 0Ų
Heavy Atom Count: 2
Formal Charge: 0
Complexity: 2
Isotope Atom Count: 0
Defined Atom Stereocenter Count: 0
Undefined Atom Stereocenter Count: 0
Defined Bond Stereocenter Count: 0
Undefined Bond Stereocenter Count: 0
Covalently-Bonded Unit Count: 2
Compound Is Canonicalized: Yes

Physical state: powder
Color: colorless
Odor: odorless
Melting point/freezing point:
Melting point/range: 605 °C
Initial boiling point and boiling range: 1.360 °C at 1.013 hPa
Flammability (solid, gas): The product is not flammable.
Upper/lower flammability or explosive limits: No data available
Flash point: Not applicable
Autoignition temperature: No data available
Decomposition temperature: No data available
pH: ca.6 at 50 g/l at 20 °C
Viscosity
Viscosity, kinematic: No data available
Viscosity, dynamic: No data available

Water solubility: 569 g/l at 20 °C
Partition coefficient: n-octanol/water: Not applicable for inorganic substances
Vapor pressure: 1,33 hPa at 547 °C
Density: 2,07 g/cm3 at 20 °C
Relative density: No data available
Relative vapor density: No data available
Particle characteristics: No data available
Explosive properties: No data available
Oxidizing properties: none
Other safety information: No data available
LiCl: Lithium Chloride
Density: 2.07 g/cm³
Molecular Weight/ Molar Mass: 42.394 g/mol
Boiling Point: 1,382 °C
Melting Point: 605 °C
Chemical Formula: LiCl
Odour: Odourless



FIRST AID MEASURES of LITHIUM (1+) CHLORIDE:
-Description of first-aid measures:
*General advice:
Show this material safety data sheet to the doctor in attendance.
*If inhaled:
After inhalation:
Fresh air.
*In case of skin contact:
Take off immediately all contaminated clothing.
Rinse skin with water/ shower.
*In case of eye contact:
After eye contact:
Rinse out with plenty of water.
Call in ophthalmologist.
Remove contact lenses.
*If swallowed:
After swallowing:
Immediately make victim drink water (two glasses at most).
Consult a physician.
-Indication of any immediate medical attention and special treatment needed:
No data available



ACCIDENTAL RELEASE MEASURES of LITHIUM (1+) CHLORIDE:
-Environmental precautions:
Do not let product enter drains.
-Methods and materials for containment and cleaning up:
Cover drains.
Collect, bind, and pump off spills.
Observe possible material restrictions.
Take up dry.
Dispose of properly.
Clean up affected area.



FIRE FIGHTING MEASURES of LITHIUM (1+) CHLORIDE:
-Extinguishing media:
*Suitable extinguishing media:
Use extinguishing measures that are appropriate to local circumstances and the
surrounding environment.
*Unsuitable extinguishing media:
For this substance/mixture no limitations of extinguishing agents are given.
-Further information:
Suppress (knock down) gases/vapors/mists with a water spray jet.
Prevent fire extinguishing water from contaminating surface water or the ground water system.



EXPOSURE CONTROLS/PERSONAL PROTECTION of LITHIUM (1+) CHLORIDE:
-Exposure controls:
--Personal protective equipment:
*Eye/face protection:
Use equipment for eye protection.
Safety glasses
*Skin protection:
Full contact:
Material: Nitrile rubber
Minimum layer thickness: 0,11 mm
Break through time: 480 min
Splash contact:
Material: Nitrile rubber
Minimum layer thickness: 0,11 mm
Break through time: 480 min
*Body Protection:
protective clothing
*Respiratory protection:
Recommended Filter type: Filter type P2
-Control of environmental exposure:
Do not let product enter drains.



HANDLING and STORAGE of LITHIUM (1+) CHLORIDE:
-Conditions for safe storage, including any incompatibilities:
*Storage conditions:
Tightly closed.
Dry.
hygroscopic
*Storage class:
Storage class (TRGS 510): 13:
Non Combustible Solids



STABILITY and REACTIVITY of LITHIUM (1+) CHLORIDE:
-Reactivity:
No data available
-Chemical stability:
The product is chemically stable under standard ambient conditions (room temperature) .
-Conditions to avoid:
no information available
-Incompatible materials:
No data available

Lithium (+1) chloride is an ionic compound or salt that is highly polar and soluble in water.
The chemical formula for Lithium (+1) chloride is LiCl.
Lithium (+1) chloride is an inorganic chloride and a lithium salt.


CAS Number: 7447-41-8
EC Number: 231-212-3
MDL number: MFCD00011078
Chemical formula: LiCl



Lithium (+1) chloride, BioXtra, >=99.0% (titration), Q422930, SR-01000076252, SR-01000076252-1, Lithium (+1) chloride, powder, >=99.99% trace metals basis, Lithium (+1) chloride, puriss. p.a., anhydrous, >=99.0% (AT), Lithium (+1) chloride, anhydrous, beads, -10 mesh, >=99.9% trace metals basis, Lithium (+1) chloride, anhydrous, beads, -10 mesh, 99.998% trace metals basis, Lithium (+1) chloride, puriss. p.a., ACS reagent, anhydrous, >=99.0% (AT), Lithium (+1) chloride, anhydrous, free-flowing, Redi-Dri(TM), ACS reagent, >=99%, Lithium (+1) chloride, anhydrous, free-flowing, Redi-Dri(TM), ReagentPlus(R), 99%, Lithium (+1) chloride, BioUltra, for molecular biology, anhydrous, >=99.0% (AT), 59217-69-5, Hydrochloric acid lithium salt, Lithium (+1) chloride, Lithium (+1) chloride licl, lithiumchloride, licl, chlorure de lithium, chlorku litu, chlorolithium, lithiumchlorid, chlorku litu polish, luthium chloride, Lithium (+1) chloride, Lithium (+1) chloride licl, lithiumchloride, licl, chlorure de lithium, chlorku litu, chlorolithium, lithiumchlorid, chlorku litu polish, luthium chloride, Lithium (+1) chloride, Lithium(1+) chloride, LITHIUM (+1) CHLORIDE, 7447-41-8, LiCl, Lithiumchloride, chlorure de lithium, chlorolithium, Lithiumchlorid, Lithium (+1) chloride (LiCl), lithium;chloride, CCRIS 5924, CHEBI:48607, lithii chloridum, HSDB 4281, Lithium Cholride, cloruro de litio, Lithium (+1) chloride (powder), EINECS 231-212-3, MFCD00011078, NSC 327172, UNII-G4962QA067, LITHIUM MURIATICUM, G4962QA067, NSC-327172, Lithium (+1) chloride, Anhydrous, LithiumChlorideG (Anhydrous), CHEMBL69710, DTXSID2025509, EC 231-212-3, NSC327172, Lithium (+1) chloride, ultra dry, Luthium chloride, Chloride, Lithium, Lithium (+1) chloride (2.3% in Tetrahydrofuran, ca. 0.5mol/L), lithim chloride, Lopac-L-4408, LITHIUM MONOCHLORIDE, MolMap_000071, WLN: LI G, Lithium (+1) chloride, ACS grade, Lopac0_000604, LITHIUM (+1) CHLORIDE [MI], Lithium (+1) chloride battery grade, Lithium (+1) chloride, ACS reagent, DTXCID105509, LITHIUM (+1) CHLORIDE [HSDB], LITHIUM (+1) CHLORIDE [INCI], LITHIUM MURIATICUM [HPUS], KWGKDLIKAYFUFQ-UHFFFAOYSA-M, LITHIUM (+1) CHLORIDE [WHO-DD], Lithium (+1) chloride, 3-5% in THF, HMS3261J10, Tox21_500604, BDBM50494542, AKOS015902822, AKOS015950647, AKOS024438070, CCG-204693, Lithium (+1) chloride, gamma irradiated, 8m, LP00604, SDCCGSBI-0050586.P002, Lithium (+1) chloride, ACS reagent, >=99%, Lithium (+1) chloride, ReagentPlus(R), 99%, NCGC00015607-01, NCGC00015607-02, NCGC00015607-03, NCGC00015607-04, NCGC00015607-07, NCGC00093980-01, NCGC00093980-02, NCGC00261289-01, BP-13612, SY002997, Lithium (+1) chloride, Vetec(TM) reagent grade, EU-0100604, FT-0627896, L0204, L0222, Lithium (+1) chloride, Trace metals grade 99.9%, L 4408, Lithium (+1) chloride, SAJ first grade, >=98.0%, Lithium (+1) chloride, for molecular biology, >=99%, Lithium (+1) chloride, SAJ special grade, >=99.0%, A838146,



Lithium (1+) chloride is registered under the REACH Regulation and is manufactured in and / or imported to the European Economic Area, at ≥ 1 000 to < 10 000 tonnes per annum.
Lithium (+1) chloride is an injection indicated for cardiac output measurement.


Crystallization grade Lithium (+1) chloride for formulating screens or for optimization.
The chemical formula of anhydrous Lithium (+1) chloride is LiCl, the relative molecular weight is 42.39, which is cubic crystal white particles or powder, which is easy to deliquesce and tastes salty.


Lithium (+1) chloride belongs to the low-toxicity category, but has a strong irritating and corrosive effect on the eyes and mucous membranes.
The specific gravity of Lithium (+1) chloride is 2.068, the melting point is 605°C, the boiling point is 1360°C, and it is easily soluble in water grams (0°C) in 100 grams of water, 127.5 grams (100°C)].


Lithium (+1) chloride has a typical shelf life of 2 years if kept in dry conditions.
Lithium (+1) chloride appears as colorless crystals or powder.
The resulting solution is evaporated to get a mixture of saturated solution and Lithium (+1) chloride crystals.


The solid and the solution is separated and the supernatant solution is recycled for further evaporation.
Lithium (+1) chloride is a solid which absorbs water to form a hydrate, LiCl.H2O
Lithium (+1) chloride is a solid which absorbs water to form a hydrate, LiCl.H2O.


Lithium (+1) chloride is soluble in alcohol, slightly soluble in acetone, pyridine and liquid ammonia.
Lithium (+1) chloride is a chemical compound with the formula LiCl.
Lithium (+1) chloride behaves as a fairly typical ionic compound, although the Li+ ion is very small.


Lithium (+1) chloride acts as an electrolyte for dry cells used at low temperatures, catalyst in certain oxidation reactions, solubilizer for polyamides and cellulose when used with amide solvents, chlorinating agent for steroid substrates.
Lithium (+1) chloride is registered under the REACH Regulation and is manufactured in and / or imported to the European Economic Area, at ≥ 1 000 to < 10 000 tonnes per annum.


Lithium (+1) chloride is a metal chloride salt with a Li (+) counterion.
Lithium (+1) chloride has a role as an antimanic drug and a geroprotector.
Lithium (+1) chloride is an inorganic chloride and a lithium salt.


Lithium (+1) chloride is a typical ionic compound (with certain covalent characteristics), although the small size of the Li+ ion gives rise to properties not seen for other alkali metal chlorides, such as extraordinary solubility in polar solvents (83.05 g/100 mL of water at 20 °C) and its hygroscopic properties.
Lithium (+1) chloride appears as colorless crystals or powder.


Lithium (+1) chloride is for assays to study cell-fate, neurobiology and antiviral properties; noted to inhibit GSK-3β
Lithium (+1) chloride is hygroscopic in nature.
Lithium (+1) chloride is incompatible with strong oxidizing agents, strong acids, bromine trichloride and bromine trifluoride.


Deliquescent salt forms a solution when exposed to humid air.
Store Lithium (+1) chloride in a cool and dry place in closed tight containers.
Lithium (+1) chloride is a typical ionic compound and a salt of lithium.


Due to the small size of the lithium-ion ( Li+ ), Lithium (+1) chloride gives rise to properties that we cannot see in other alkali metal chlorides.
Lithium (+1) chloride is an antiviral metal halide utilized in a variety of assays to study cell-fate and neurobiology.
In developing Xenopus embryos, Lithium (+1) chloride is observed to exert inhibition of GSK-3β (glycogen synthase kinase-3β), yet not reported to be a general inhibitor of other protein kinases.


Lithium (+1) chloride is more soluble in organic solvents such as acetone and methanol than potassium chloride or sodium chloride.
Lithium (+1) chloride is a salt of Lithium chlorine, an alkali metal similar to sodium chloride.
Although the Li+ ion is minuscule, Lithium (+1) chloride creates unrecognized effects for other alkali metal chlorides, such as being soluble in polar solvents and having hygroscopic (holding water molecules) properties.


Lithium (+1) chloride is hygroscopic and highly soluble in water, and is highly polar.
Lithium (+1) chloride is more soluble in polar organic solvents such as methanol and acetone than is sodium chloride or potassium chloride.
Lithium (+1) chloride is a chemical compound with the formula LiCl.


Lithium (+1) chloride is a salt of lithium that has been used experimentally as an immunomodulator.
Lithium (+1) chloride is a white solid hygroscopic soluble in water, alcohol and ether.
Lithium (+1) chloride is made by the action of hydrochloric acid on lithium hydroxide.
These observations may have implications for Lithium (+1) chloride on cell-fate determination in several organisms including Xenopus and Dictyostelium.


Lithium (+1) chloride is a chemical compound with a chemical formula “LiCl”.
The salt is a normal ionic compound, although the Li+ ion is small in size, Lithium (+1) chloride produces unrecognized effects for other alkali metal chlorides, such as exceptional solubility in polar solvents and its hygroscopic properties.


The antiviral properties of Lithium (+1) chloride were noted in a study which showed that the compound inhibited pseudorabis virus infection in vitro.
In Drosophila, it was observed that in the nervous system, Lithium (+1) chloride may have an effect on amino acid metabolism.
Futhermore, in glial primary cell cultures, Lithium (+1) chloride has been noted to provide protection against glutamate excitotoxicity by potentially reducing NR1 mRNA, the major N-methyl-D-aspartate receptor (NMDAR) subunit in the cells.



USES and APPLICATIONS of LITHIUM (1+) CHLORIDE:
Lithium (1+) chloride is used by consumers, in articles, by professional workers (widespread uses), in formulation or re-packing, at industrial sites and in manufacturing.
Lithium (+1) chloride is a very effective antimanic drug for the treatment of bipolar disorder.


Lithium (+1) chloride is well soluble in water, alcohol, acetone, and amyl alcohol and Lithium (+1) chloride is also used as a flame colorant to produce dark red flames.
Lithium (+1) chloride is used as an electrolyte in voltaic cells.


Lithium (+1) chloride is used in supplements.
Lithium (1+) chloride is used in the following products: coating products, metal surface treatment products, non-metal-surface treatment products, adhesives and sealants, inks and toners, pH regulators and water treatment products, photo-chemicals, polishes and waxes and welding & soldering products.


Lithium (+1) chloride is used fluxes for welding and soldering techniques; salt bath for heat-treatment by low temperature and for dip brazing; raw material for other lithium compounds; tracer for chemical products (denaturation of wine etc.); absorption and desinfection reagent (Lithium (+1) chloride solution) for absorbers.


Other release to the environment of Lithium (1+) chloride is likely to occur from: indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners), outdoor use, indoor use in close systems with minimal release (e.g. cooling liquids in refrigerators, oil-based electric heaters), outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids), outdoor use in long-life materials with low release rate (e.g. metal, wooden and plastic construction and building materials) and indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment).


Release to the environment of Lithium (1+) chloride can occur from industrial use: industrial abrasion processing with low release rate (e.g. cutting of textile, cutting, machining or grinding of metal).
Lithium (+1) chloride is used to produce a dark red flame.


Lithium (+1) chloride is used as a brazing flux, as a desiccant in drying air streams, as a component in organic synthesis, as an additive in the Stille reaction, in some biochemical applications, and as soldering aluminum metal.
Lithium (+1) chloride is used for the production of lithium metal, by electrolysis of a LiCl/KCl melt at 450 °C.


Lithium (+1) chloride is also used as a brazing flux for aluminium in automobile parts.
Lithium (+1) chloride can be used to improve the efficiency of the Stille reaction.
Lithium (+1) chloride's desiccant properties can be used to generate potable water by absorbing moisture from the air, which is then released by heating the salt.


Other release to the environment of Lithium (1+) chloride is likely to occur from: indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment).
Lithium (+1) chloride is also used in organic synthesis.


Lithium (+1) chloride is used to precipitate RNA.
Lithium (+1) chloride has many applications.
Lithium (+1) chloride is extremely hygroscopic, and is widely used in dehumidification systems to remove moisture from the air in industries such as food processing and horticulture.


Other release to the environment of Lithium (+1) chloride is likely to occur from: indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners), outdoor use, indoor use in close systems with minimal release (e.g. cooling liquids in refrigerators, oil-based electric heaters), outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids), outdoor use in long-life materials with low release rate (e.g. metal, wooden and plastic construction and building materials) and indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment).


Lithium (1+) chloride can be found in products with material based on: stone, plaster, cement, glass or ceramic (e.g. dishes, pots/pans, food storage containers, construction and isolation material) and paper (e.g. tissues, feminine hygiene products, nappies, books, magazines, wallpaper).
Lithium (+1) chloride has also been utilized in: Large scale plasmid DNA isolation without ultracentrifugation; Protein extraction and protein crystallization;

Crystallization of other biological structures, including vitamin B12-RNA aptamer and the L-A virus particle; Inhibits the expression and secretion of insulin-like growth factor-binding protein-1 in H4-II-E cells; Used in the synthesis of beta-substituted alpha-amino acid derivatives; May be used to selectively pre­cipitate RNA.


Lithium (1+) chloride is used in the following products: laboratory chemicals, pH regulators and water treatment products, metal working fluids, pharmaceuticals, polymers, water treatment chemicals and welding & soldering products.
Lithium (1+) chloride is used in the following areas: scientific research and development and health services.


Other release to the environment of this substance is likely to occur from: indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment). This substance can be found in products with material based on: stone, plaster, cement, glass or ceramic (e.g. dishes, pots/pans, food storage containers, construction and isolation material) and paper (e.g. tissues, feminine hygiene products, nappies, books, magazines, wallpaper).


Lithium (+1) chloride is used in the following products: laboratory chemicals, pH regulators and water treatment products, metal working fluids, pharmaceuticals, polymers, water treatment chemicals and welding & soldering products.
Lithium (+1) chloride is used in the following areas: scientific research and development and health services.


Lithium (+1) chloride is used in the following products: pharmaceuticals, air care products, inks and toners, laboratory chemicals, metal working fluids, paper chemicals and dyes, polymers, water treatment chemicals and welding & soldering products.
Release to the environment of Lithium (+1) chloride can occur from industrial use: formulation of mixtures and formulation in materials.


Other release to the environment of Lithium (1+) chloride is likely to occur from: indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners), outdoor use, indoor use in close systems with minimal release (e.g. cooling liquids in refrigerators, oil-based electric heaters), outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids), outdoor use in long-life materials with low release rate (e.g. metal, wooden and plastic construction and building materials) and indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment).


Lithium (+1) chloride is also used as a tracer for waste water, as a brazing flux, and as an electrolyte component for the manufacture of speciality batteries.
Lithium (+1) chloride is used as an electrolyte for low temperature dry battery cells and as an oxidation catalyst.
Lithium (+1) chloride is a solubilizer for polyamides and cellulose when used with amide solvents, and is a chlorinating agent for steroid substrates.


Lithium (+1) chloride is mainly we use it for the production of lithium metal by electrolysis of LiCl/KCl which melt at 450oC.
Moreover, industries use Lithium (+1) chloride as a brazing flux for aluminum in automobile parts.
In addition, we use Lithium (+1) chloride as a desiccant for drying air streams.


Lithium (+1) chloride is useful for the production of lithium metal and for the generation of Mn(0) species which can be used in free radical cyclizations.
Lithium (+1) chloride can serve as a flame colorant to generate dark red flames, a brazing flux for aluminum in automobiles, a hygrometer and a desiccant for drying air streams.


Being biologically significant, Lithium (+1) chloride finds applications in a wide variety of assays to study cell-fate and neurobiology.
Lithium (+1) chloride has been found to inhibit virus infection.
Lithium (1+) chloride is used for the manufacture of: chemicals and plastic products.


Release to the environment of Lithium (+1) chloride can occur from industrial use: industrial abrasion processing with low release rate (e.g. cutting of textile, cutting, machining or grinding of metal).
Lithium (+1) chloride is used in the following products: welding & soldering products, laboratory chemicals, air care products, inks and toners, pH regulators and water treatment products, metal working fluids, pharmaceuticals, polymers and water treatment chemicals.


Lithium (+1) chloride is used in the following areas: scientific research and development and health services.
Release to the environment of Lithium (+1) chloride can occur from industrial use: in processing aids at industrial sites, as an intermediate step in further manufacturing of another substance (use of intermediates), as processing aid, of substances in closed systems with minimal release and in the production of articles.


Lithium (1+) chloride is used in the following products: pharmaceuticals, air care products, inks and toners, laboratory chemicals, metal working fluids, paper chemicals and dyes, polymers, water treatment chemicals and welding & soldering products.
Release to the environment of Lithium (1+) chloride can occur from industrial use: formulation of mixtures and formulation in materials.


Lithium (1+) chloride is used in the following products: welding & soldering products, laboratory chemicals, air care products, inks and toners, pH regulators and water treatment products, metal working fluids, pharmaceuticals, polymers and water treatment chemicals.
In organic synthesis, Lithium (+1) chloride has some specialized applications such as an additive in the Stille reaction.


Most noteworthy, Lithium (+1) chloride has biochemical applications that we use to precipitate RNA from cellular extracts.
Another application of Lithium (+1) chloride is that we use it as a flame colorant to produce dark red flames.
In the calibration of hygrometers, they use Lithium (+1) chloride as a relative humidity standard.


Lithium (+1) chloride can be used as a hygrometer. In addition, when exposed to air it salts from deliquescent self-solution.
Furthermore, the equilibrium Lithium (+1) chloride concentration of the resulting solution may directly relate to the relative humidity of the air.
It depends on the low equilibrium pressure of water vapour above solutions of Lithium (+1) chloride.


Lithium (+1) chloride is used in a number of salt mixtures exist low melting points allowing the material to be used in brazing fluxes and brazing baths.
Lithium Metal by Electrolysis: Lithium (+1) chloride is primarily used at 450 ° C (842 ° F) for the preparation of lithium metal by electrolysis of a LiCl / KCl.
As Brazing Flux uses of Lithium (+1) chloride: Lithium (+1) chloride is also used as a brazing flux for aluminum in automobile parts.


Lithium (+1) chloride is used as desiccant in drying air streams.
Lithium (+1) chloride is used in organic synthesis.
For example, as an additive in the Stille reaction.


Other release to the environment of Lithium (+1) chloridee is likely to occur from: indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners), outdoor use, indoor use in close systems with minimal release (e.g. cooling liquids in refrigerators, oil-based electric heaters), outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids), outdoor use in long-life materials with low release rate (e.g. metal, wooden and plastic construction and building materials) and indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment).


Lithium (1+) chloride is used in the following areas: scientific research and development and health services.
On exposure to air, Lithium (+1) chloride becomes a solution with the concentration directly related to relative humidity of the atmosphere and hence serves as a relative humidity standard in calibrating hygrometers.


Apart from being a source of chloride, Lithium (+1) chloride serves as an additive in the Stille reaction in organic synthesis and to precipitate RNA from cellular extracts.
Lithium (+1) chloride is used for the manufacture of: chemicals and plastic products.


Lithium (+1) chloride is used for the manufacture of: chemicals, plastic products and pulp, paper and paper products.
Release to the environment of Lithium (+1) chloride can occur from industrial use: manufacturing of the substance.
As a flame colorant, Lithium (+1) chloride is used to produce dark red flames.


Lithium (+1) chloride is used as a Relative humidity standard in the calibration of hygrometers and itself can be used as a hygrometer.
Molten Lithium (+1) chloride is used for the preparation of lithium niobite, graphene and carbon nanotubes.
Lithium (+1) chloride has been found to inhibit virus infection.


Lithium (+1) chloride has strong acaricidal properties (Varroa destructor in populations of honey bees).
Biochemical Applications: LiCl is used to precipitate RNA from cellular extracts.
Lithium (+1) chloride is used as an electrolyte for the production of lithium metal and used as an electrolyte in voltaic cells.


Lithium (1+) chloride is used for the manufacture of: chemicals, plastic products and pulp, paper and paper products.
Industries use Lithium (+1) chloride's molten form to prepare carbon nanotubes, lithium niobate, and grapheme.
Besides, Lithium (+1) chloride shows very strong acaricidal properties.


Lithium (+1) chloride is a chemical compound that is extremely soluble in polar solvents and is used in order to obtain lithium metal.
In organic synthesis Lithium (+1) chloride is used as an additive in the Stille Reaction.
Ungraded products supplied by Spectrum are indicative of a grade suitable for general industrial use or research purposes and typically are not suitable for consumption.


Lithium (+1) chloride is used by consumers, in articles, by professional workers (widespread uses), in formulation or re-packing, at industrial sites and in manufacturing.
Lithium (+1) chloride is used in the following products: coating products, metal surface treatment products, non-metal-surface treatment products, adhesives and sealants, inks and toners, pH regulators and water treatment products, photo-chemicals, polishes and waxes and welding & soldering products.


Lithium (+1) chloride is useful for the production of lithium metal and for the generation of Mn(0) species which can be used in free radical cyclizations.
Lithium (+1) chloride can serve as a flame colorant to generate dark red flames, a brazing flux for aluminum in automobiles, a hygrometer and a desiccant for drying air streams.


Release to the environment of Lithium (1+) chloride can occur from industrial use: in processing aids at industrial sites, as an intermediate step in further manufacturing of another substance (use of intermediates), as processing aid, of substances in closed systems with minimal release and in the production of articles.


Lithium (+1) chloride is also used as a flame colorant to produce dark red flames.
Molten Lithium (+1) chloride is used for the preparation of carbon nanotubes, graphene and lithium niobate.
Lithium (+1) chloride has been shown to have strong acaricidal properties, being effective against Varroa destructor in populations of honey bees.


Lithium (+1) chloride is used as an aversive agent in lab animals to study conditioned place preference and aversion.
Lithium (+1) chloride is widely used in several industrial applications.
Lithium (+1) chloridet is used as a flame colorant to form dark crimson flames.


Release to the environment of Lithium (1+) chloride can occur from industrial use: manufacturing of the substance.
Lithium (+1) chloride is used in the precipitation of RNA in biological applications.
Lithium (+1) chloride is an aluminum blazing flux in automobile parts.


Lithium (+1) chloride is used for several soldering and welding techniques and salt bath heat treatment at low temperatures.
Lithium (+1) chloride is used in massive dehumidification systems in the AC industry.
This depends on the low equilibrium pressure of vapor above Lithium (+1) chloride solutions.
Lithium (+1) chloride is used in large dehumidification systems in the air conditioning industry.



CHEMICAL PROPERTIES OF LITHIUM (+1) CHLORIDE:
Like other metal chlorides Lithium (+1) chloride's salt form crystalline hydrates.
Furthermore, Lithium (+1) chloride's mono-, tri-, pentahydrate are known.
We can regenerate Lithium (+1) chloride's anhydrous salts by heating the hydrates.

In addition, Lithium (+1) chloride easily absorbs up to four equivalents of ammonia/mol.
However, with another ionic chloride, the solution of Lithium (+1) chloridecan serve as a source of chloride ion.
Lithium (+1) chloride reaction with sulfuric acid forms lithium sulfate and hydrogen chloride.
The chemical equation is given below.

2LiCl + H2SO4 → 2 HCl + Li2SO4
Lithium (+1) chloride reacts with a base like sodium hydroxide and forms lithium hydroxide and sodium chloride.
LiCl + NaOH → LiOH + NaCl

Lithium (+1) chloride Reaction with Sulfuric Acid:
When Lithium (+1) chloride reacts with sulfuric acid, it forms lithium sulfate and hydrogen chloride.
The chemical equation is given below.
2LiCl+H2SO4→2HCl+Li2SO4

The salt forms crystalline hydrates, unlike the other alkali metal chlorides.
Mono-, tri-, and pentahydrates are known.
The anhydrous salt can be regenerated by heating the hydrates.

Lithium (+1) chloride also absorbs up to four equivalents of ammonia/mol.
As with any other ionic chloride, solutions of Lithium (+1) chloride can serve as a source of chloride ion, e.g., forming a precipitate upon treatment with silver nitrate:
LiCl + AgNO3 → AgCl + LiNO3

Reaction with Sulfuric Acid:
Lithium (+1) chloride and sulfuric acid reaction form hydrogen chloride and lithium sulfate.
Here is the reaction’s chemical equation:
2LiCl+H2SO4→2HCl+Li2SO4

When Lithium (+1) chloride reacts with H2SO4 it gives lithium sulfate and hydrogen chloride.
2LiCl + H2SO4 → 2 HCl + Li2SO4
When Lithium (+1) chloride reacts with a base like NaOH it gives lithium hydroxide and sodium chloride.
LiCl + NaOH → LiOH + NaCl



STRUCTURE OF LITHIUM (+1) CHLORIDE:
Lithium (+1) chloride structure LiCl is drawn with the help of lewis dots
Lithium (+1) chloride is ionic compound, in which Lithium is a metal compound and chloride is a non-metal.

Where electrons are transferred from metal ion to non-metal ion.
One electron is transferred from lithium and makes Lithium (+1) chloride electro-positive and by gaining one electron from lithium, chlorine becomes electronegative.



PHYSICAL PROPERTIES OF LITHIUM (+1) CHLORIDE:
Lithium (+1) chloride appears as an odorless white crystalline hygroscopic solid.
Lithium (+1) chloride has a density of 2.068g/cm3 and its boiling point is 1382oC and its melting point is in between 605–614oC.
Lithium (+1) chloride is soluble in water, methanol, ethanol, isopropanol, butanol, formic acid, n- mehtylformamide, hydrazine, and THF.

In addition, Lithium (+1) chloride is slightly soluble in acetone and ammonia and is completely insoluble in dichloromethane.
Lithium (+1) chloride has a sharp, saline taste.
Lithium (+1) chloride has cubic crystals, crystalline powder, or granule appearance.

Lithium (+1) chloride has a melting point of 121°F and 2.068 density at 77°F.
Lithium (+1) chloride's aqueous solution is neutral and a bit alkaline.
Lithium (+1) chloride is soluble in ether, nitrobenzene, and water alcohols.



PREPARATION OF LITHIUM (+1) CHLORIDE:
Lithium (+1) chloride is produced by treatment of lithium carbonate with hydrochloric acid.
Anhydrous Lithium (+1) chloride is prepared from the hydrate by heating in a stream of hydrogen chloride.



PROPERTIES OF LITHIUM (+1) CHLORIDE:
1. Physical Properties of Lithium (+1) chloride Licl:
Lithium (+1) chloride is Deliquescent in nature, appear as cubic crystals, granules or crystalline powder
Lithium (+1) chloride has sharp saline taste

Lithium (+1) chloride has Boiling point of 2417 to 2480 °F at 760 mm Hg
Lithium (+1) chloride's Melting point is 1121 °F
Lithium (+1) chloride has Density of 2.068 at 77 °F

Aqueous solution of Lithium (+1) chloride is neutral or slightly alkaline.
Lithium (+1) chloride is very soluble in water alcohols, ether, pyridine, nitrobenzene



FEATURES OF LITHIUM (+1) CHLORIDE:
Sterile filtered solution:
Formulated in Type 1+ ultrapure water: 18.2 megaohm-cm resistivity at 25°C, < 5 ppb Total Organic Carbon, bacteria free (


FUNCTION AND PURPOSE OF LITHIUM (+1) CHLORIDE:
Raw material for preparing metallic lithium.
Flux in the production of metal by electrolysis (such as the production of titanium and aluminum), used as aluminum welding agent, air conditioning dehumidifier and special cement raw material, also used in flames, in the battery industry for the production of lithium manganese battery electrolyte, etc.
Anhydrous Lithium (+1) chloride is mainly used for electrolytic preparation of metallic lithium and aluminum fluxes and fluxes, as well as moisture absorbing (dehumidifying) agents in non-refrigerated air conditioners.



PHYSICAL and CHEMICAL PROPERTIES of LITHIUM (1+) CHLORIDE:
Appearance: White solid hygroscopic
Covalently-Bonded Unit: 2
Specific Gravity: 2.068 at 77 ° F
Complexity: 2
Solubility: Insoluble in water
CAS: 7447-41-8
MF: LiCl
MW: 42.39
EINECS: 231-212-3
Mol File: 7447-41-8.mol
Lithium chloride Chemical Properties:
Melting point: 605 °C(lit.)
Boiling point: 1382°C
density: 2.06
vapor pressure: 1.33 hPa (547 °C)
refractive index: n20/D 1.381
Fp: -4 °F
storage temp.: 2-8°C
solubility: H2O: soluble
form: beads
color: White to gray

Specific Gravity: 2.068
Odor: Odorless
PH: 5.5-7.5 (25℃, 50mg/mL in H2O)
PH Range: 6
Water Solubility: 832 g/L (20 ºC)
λmax: λ: 260 nm Amax: 0.01
λ: 280 nm Amax: 0.01
Sensitive: Hygroscopic
Merck: 145,528
Stability: Stable.
InChIKey: KWGKDLIKAYFUFQ-UHFFFAOYSA-M
CAS DataBase Reference: 7447-41-8(CAS DataBase Reference)
NIST Chemistry Reference: Lithium chloride(7447-41-8)
EPA Substance Registry System: Lithium chloride (7447-41-8)
Linear Formula: LiCl
UN Number: NONH for all modes of transport
Formula Weight: 42.39g/mol
Chemical Name or Material: Lithium Chloride

Chemical formula: LiCl
Molar mass: 42.39 g•mol−1
Appearance: white solid
hygroscopic, sharp
Density: 2.068 g/cm3
Melting point: 605–614 °C (1,121–1,137 °F; 878–887 K)
Boiling point: 1,382 °C (2,520 °F; 1,655 K)
Solubility in water: 68.29 g/100 mL (0 °C)
74.48 g/100 mL (10 °C)
84.25 g/100 mL (25 °C)
88.7 g/100 mL (40 °C)
123.44 g/100 mL (100 °C)
Solubility: soluble in hydrazine, methylformamide,
butanol, selenium(IV) oxychloride, 1-propanol

Solubility in methanol: 45.2 g/100 g (0 °C)
43.8 g/100 g (20 °C)
42.36 g/100 g (25 °C)
44.6 g/100 g (60 °C)
Solubility in ethanol: 14.42 g/100 g (0 °C)
24.28 g/100 g (20 °C)
25.1 g/100 g (30 °C)
23.46 g/100 g (60 °C)
Solubility in formic acid: 26.6 g/100 g (18 °C)
27.5 g/100 g (25 °C)
Solubility in acetone: 1.2 g/100 g (20 °C)
0.83 g/100 g (25 °C)
0.61 g/100 g (50 °C)
Solubility in liquid ammonia: 0.54 g/100 g (-34 °C)
3.02 g/100 g (25 °C)

Vapor pressure: 1 torr (785 °C)
10 torr (934 °C)
100 torr (1130 °C)
Magnetic susceptibility (χ): −24.3•10−6 cm3/mol
Refractive index (nD): 1.662 (24 °C)
Viscosity: 0.87 cP (807 °C)
Structure:
Coordination geometry: Octahedral
Molecular shape: Linear (gas)
Dipole moment: 7.13 D (gas)
Thermochemistry:
Heat capacity (C): 48.03 J/mol•K
Std molar entropy (S⦵298): 59.31 J/mol•K
Std enthalpy of formation (ΔfH⦵298): -408.27 kJ/mol
Gibbs free energy (ΔfG⦵): -384 kJ/mol
Molecular Weight: 42.4 g/mol

Hydrogen Bond Donor Count: 0
Hydrogen Bond Acceptor Count: 1
Rotatable Bond Count: 0
Exact Mass: 41.9848561 g/mol
Monoisotopic Mass: 41.9848561 g/mol
Topological Polar Surface Area: 0Ų
Heavy Atom Count: 2
Formal Charge: 0
Complexity: 2
Isotope Atom Count: 0
Defined Atom Stereocenter Count: 0
Undefined Atom Stereocenter Count: 0
Defined Bond Stereocenter Count: 0
Undefined Bond Stereocenter Count: 0
Covalently-Bonded Unit Count: 2
Compound Is Canonicalized: Yes

Physical state: powder
Color: colorless
Odor: odorless
Melting point/freezing point:
Melting point/range: 605 °C
Initial boiling point and boiling range: 1.360 °C at 1.013 hPa
Flammability (solid, gas): The product is not flammable.
Upper/lower flammability or explosive limits: No data available
Flash point: Not applicable
Autoignition temperature: No data available
Decomposition temperature: No data available
pH: ca.6 at 50 g/l at 20 °C
Viscosity
Viscosity, kinematic: No data available
Viscosity, dynamic: No data available

Water solubility: 569 g/l at 20 °C
Partition coefficient: n-octanol/water: Not applicable for inorganic substances
Vapor pressure: 1,33 hPa at 547 °C
Density: 2,07 g/cm3 at 20 °C
Relative density: No data available
Relative vapor density: No data available
Particle characteristics: No data available
Explosive properties: No data available
Oxidizing properties: none
Other safety information: No data available
LiCl: Lithium Chloride
Density: 2.07 g/cm³
Molecular Weight/ Molar Mass: 42.394 g/mol
Boiling Point: 1,382 °C
Melting Point: 605 °C
Chemical Formula: LiCl
Odour: Odourless



FIRST AID MEASURES of LITHIUM (1+) CHLORIDE:
-Description of first-aid measures:
*General advice:
Show this material safety data sheet to the doctor in attendance.
*If inhaled:
After inhalation:
Fresh air.
*In case of skin contact:
Take off immediately all contaminated clothing.
Rinse skin with water/ shower.
*In case of eye contact:
After eye contact:
Rinse out with plenty of water.
Call in ophthalmologist.
Remove contact lenses.
*If swallowed:
After swallowing:
Immediately make victim drink water (two glasses at most).
Consult a physician.
-Indication of any immediate medical attention and special treatment needed:
No data available



ACCIDENTAL RELEASE MEASURES of LITHIUM (1+) CHLORIDE:
-Environmental precautions:
Do not let product enter drains.
-Methods and materials for containment and cleaning up:
Cover drains.
Collect, bind, and pump off spills.
Observe possible material restrictions.
Take up dry.
Dispose of properly.
Clean up affected area.



FIRE FIGHTING MEASURES of LITHIUM (1+) CHLORIDE:
-Extinguishing media:
*Suitable extinguishing media:
Use extinguishing measures that are appropriate to local circumstances and the
surrounding environment.
*Unsuitable extinguishing media:
For this substance/mixture no limitations of extinguishing agents are given.
-Further information:
Suppress (knock down) gases/vapors/mists with a water spray jet.
Prevent fire extinguishing water from contaminating surface water or the ground water system.



EXPOSURE CONTROLS/PERSONAL PROTECTION of LITHIUM (1+) CHLORIDE:
-Exposure controls:
--Personal protective equipment:
*Eye/face protection:
Use equipment for eye protection.
Safety glasses
*Skin protection:
Full contact:
Material: Nitrile rubber
Minimum layer thickness: 0,11 mm
Break through time: 480 min
Splash contact:
Material: Nitrile rubber
Minimum layer thickness: 0,11 mm
Break through time: 480 min
*Body Protection:
protective clothing
*Respiratory protection:
Recommended Filter type: Filter type P2
-Control of environmental exposure:
Do not let product enter drains.



HANDLING and STORAGE of LITHIUM (1+) CHLORIDE:
-Conditions for safe storage, including any incompatibilities:
*Storage conditions:
Tightly closed.
Dry.
hygroscopic
*Storage class:
Storage class (TRGS 510): 13:
Non Combustible Solids



STABILITY and REACTIVITY of LITHIUM (1+) CHLORIDE:
-Reactivity:
No data available
-Chemical stability:
The product is chemically stable under standard ambient conditions (room temperature) .
-Conditions to avoid:
no information available
-Incompatible materials:
No data available

Carbonic Acid, Dilithium Salt; Carbonic Acid Lithium Salt; Camcolit; Liskonum; Priadel; Lithane; Lithea; Lithicarb; Lithinate; Lithionate; Candamide; Quilonum Retard; Teralithe; Carbonato de litio; Carbonate de lithium CAS NO:554-13-2

SYNONYMS Carbonic Acid, Dilithium Salt; Carbonic Acid Lithium Salt; Camcolit; Liskonum; Priadel; Lithane; Lithea; Lithicarb; Lithinate; Lithionate; Candamide; Quilonum Retard;CAS NO. 554-13-2

Lithium(1+) chloride; LITHIUM CHLORIDE GRAN; lithium atomic spectroscopy standard concentrate 1.00 g li; lithium chloride, acs; lithium chloride, ultra dry; lithium ion standard solution; LITHIUMCHLORIDE,CRYSTAL,REAGENT,ACS; LITHIUMCHLORIDE,POWDER,REAGENT,ACS; Lithiumchlorid CAS NO:7447-41-8

Lithium chloride is an ionic compound or salt that is highly polar and soluble in water.
Lithium chloride is more soluble in organic solvents such as acetone and methanol than potassium chloride or sodium chloride.


CAS Number: 7447-41-8
EC Number: 231-212-3
MDL number: MFCD00011078
Chemical formula: LiCl
Molecular Formula: ClLi / LiCl



LITHIUM CHLORIDE, 7447-41-8, LiCl, Lithiumchloride, chlorure de lithium, Chlorku litu, chlorolithium, Lithiumchlorid, Lithium chloride (LiCl), lithium;chloride, CCRIS 5924, CHEBI:48607, lithii chloridum, HSDB 4281, Lithium Cholride, cloruro de litio, Lithium chloride (powder), EINECS 231-212-3, MFCD00011078, NSC 327172, UNII-G4962QA067, LITHIUM MURIATICUM, G4962QA067, NSC-327172, Lithium Chloride, Anhydrous, LithiumChlorideGr(Anhydrous),
CHEMBL69710, DTXSID2025509, EC 231-212-3, NSC327172, ClLi, 2M Lithium Chloride Electrolyte, Electrode Filling Solution, Lithium Chloride (2.3% in Tetrahydrofuran, ca. 0.5mol/L), lithim chloride, Lithium chloride, anhydrous, chunks, 99.99% trace metals basis, Lithium chloride anhydrous,
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Lithium Chloride is a white solid hygroscopic soluble in water, alcohol and ether.
The chemical formula for lithium chloride is LiCl.
Lithium chloride is made by the action of hydrochloric acid on lithium hydroxide.


The resulting solution is evaporated to get a mixture of saturated solution and lithium chloride crystals.
The solid and the solution of Lithium chloride are separated and the supernatant solution is recycled for further evaporation.
Lithium chloride is a solid which absorbs water to form a hydrate, LiCl.H2O


Lithium chloride is an ionic compound or salt that is highly polar and soluble in water.
Lithium chloride is more soluble in organic solvents such as acetone and methanol than potassium chloride or sodium chloride.
Lithium chloride is registered under the REACH Regulation and is manufactured in and / or imported to the European Economic Area, at ≥ 1 000 to < 10 000 tonnes per annum.


Lithium chloride appears as colorless crystals or powder.
Lithium chloride is a metal chloride salt with a Li(+) counterion.
Lithium chloride has a role as an antimanic drug and a geroprotector.


Lithium chloride is an inorganic chloride and a lithium salt.
Lithium chloride Formula is a typical ionic compound and a salt of lithium.
Due to the small size of the lithium-ion ( Li+ ), Lithium chloride gives rise to properties that we cannot see in other alkali metal chlorides.


Lithium chloride is a salt of lithium that has been used experimentally as an immunomodulatory.
Lithium chloride is a chemical compound with the formula LiCl.
The salt is a typical ionic compound (with certain covalent characteristics), although the small size of the Li+ ion gives rise to properties not seen for other alkali metal chlorides, such as extraordinary solubility in polar solvents (83.05 g/100 mL of water at 20 °C) and its hygroscopic properties.



USES and APPLICATIONS of LITHIUM CHLORIDE:
Lithium chloride is used Molten salt chemistry and metallurgy, brazing fluxes, catalyst for organic oxidation reactions, electrolyte in dry cells used in low temperatures, and stabilizer in textile fiber spinning solutions.
Lithium chloride is used solubilizer for polyamides and cellulose when used with amide solvents, chlorinating agent for steroid agents.


Lithium chloride is used desiccant for drying applications, tracer in wastewater.
Lithium chloride is used Fluxes for welding and soldering techniques; salt bath for heat-treatment by low temperature and for dip brazing; raw material for other lithium compounds; tracer for chemical products (denaturation of wine etc.); absorption and desinfection reagent (lithium chloride solution) for absorbers.


Lithium chloride is used as a flame colorant to form dark crimson flames.
Lithium chloride is used in the precipitation of RNA in biological applications.
Lithium chloride is an aluminum blazing flux in automobile parts.


Lithium chloride is used for several soldering and welding techniques and salt bath heat treatment at low temperatures.
Lithium chloride is used in massive dehumidification systems in the AC industry.
This depends on the low equilibrium pressure of vapor above lithium chloride solutions.


Lithium chloride is widely used in several industrial applications.
Molten lithium is contained in a carbon steel pot, while the chlorine gas is collected in a stainless steel or glass pipe for applications in other processes.


The molten lithium flows into a collecting tank and is later cast into ingots.
A mesh or stainless-steel screen separates the two compartments to prevent the products from mixing.
Lithium chloride is an injection indicated for cardiac output measurement.


Lithium Chloride is a chemical compound that is extremely soluble in polar solvents and is used in order to obtain lithium metal.
In organic synthesis Lithium chloride is used as an additive in the Stille Reaction.
Ungraded products supplied by Spectrum are indicative of a grade suitable for general industrial use or research purposes and typically are not suitable for consumption.


Lithium chloride is used by consumers, in articles, by professional workers (widespread uses), in formulation or re-packing, at industrial sites and in manufacturing.
Lithium chloride is used in the following products: coating products, metal surface treatment products, non-metal-surface treatment products, adhesives and sealants, inks and toners, pH regulators and water treatment products, photo-chemicals, polishes and waxes and welding & soldering products.


Other release to the environment of Lithium chloride is likely to occur from: indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners), outdoor use, indoor use in close systems with minimal release (e.g. cooling liquids in refrigerators, oil-based electric heaters), outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids), outdoor use in long-life materials with low release rate (e.g. metal, wooden and plastic construction and building materials) and indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment).


Release to the environment of Lithium chloride can occur from industrial use: industrial abrasion processing with low release rate (e.g. cutting of textile, cutting, machining or grinding of metal).
Other release to the environment of Lithium chloride is likely to occur from: indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment).


Lithium chloride can be found in products with material based on: stone, plaster, cement, glass or ceramic (e.g. dishes, pots/pans, food storage containers, construction and isolation material) and paper (e.g. tissues, feminine hygiene products, nappies, books, magazines, wallpaper).
Lithium chloride is used in the following products: laboratory chemicals, pH regulators and water treatment products, metal working fluids, pharmaceuticals, polymers, water treatment chemicals and welding & soldering products.


Other release to the environment of Lithium chloride is likely to occur from: indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners), outdoor use, indoor use in close systems with minimal release (e.g. cooling liquids in refrigerators, oil-based electric heaters), outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids), outdoor use in long-life materials with low release rate (e.g. metal, wooden and plastic construction and building materials) and indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment).


Lithium chloride is used in the following products: pharmaceuticals, air care products, inks and toners, laboratory chemicals, metal working fluids, paper chemicals and dyes, polymers, water treatment chemicals and welding & soldering products.
Release to the environment of Lithium chloride can occur from industrial use: formulation of mixtures and formulation in materials.


Lithium chloride is used in the following products: welding & soldering products, laboratory chemicals, air care products, inks and toners, pH regulators and water treatment products, metal working fluids, pharmaceuticals, polymers and water treatment chemicals.
Lithium chloride is used in the following areas: scientific research and development and health services.


Lithium chloride is used for the manufacture of: chemicals, plastic products and pulp, paper and paper products.
Lithium chloride is used in the following areas: scientific research and development and health services.
Lithium chloride is used for the manufacture of: chemicals and plastic products.


Release to the environment of Lithium chloride can occur from industrial use: in processing aids at industrial sites, as an intermediate step in further manufacturing of another substance (use of intermediates), as processing aid, of substances in closed systems with minimal release and in the production of articles.


Release to the environment of Lithium chloride can occur from industrial use: manufacturing of the substance.
Lithium chloride is used in large dehumidification systems in the air conditioning industry. It depends on the low equilibrium pressure of water vapour above solutions of lithium chloride.


Lithium chloride is used in a number of salt mixtures exist low melting points allowing the material to be used in brazing fluxes and brazing baths.
Lithium chloride is used as an electrolyte for the production of lithium metal and used as an electrolyte in voltaic cells.
Lithium chloride is used in the following products: pharmaceuticals, air care products, inks and toners, laboratory chemicals, metal working fluids, paper chemicals and dyes, polymers, water treatment chemicals and welding & soldering products.


Release to the environment of Lithium chloride can occur from industrial use: formulation of mixtures and formulation in materials.
Lithium chloride is used in the following products: welding & soldering products, laboratory chemicals, air care products, inks and toners, pH regulators and water treatment products, metal working fluids, pharmaceuticals, polymers and water treatment chemicals.


Release to the environment of Lithium chloride can occur from industrial use: in processing aids at industrial sites, as an intermediate step in further manufacturing of another substance (use of intermediates), as processing aid, of substances in closed systems with minimal release and in the production of articles.


Release to the environment of Lithium chloride can occur from industrial use: manufacturing of the substance.
Lithium Chloride is for assays to study cell-fate, neurobiology and antiviral properties; noted to inhibit GSK-3β
Lithium Chloride is an antiviral metal halide utilized in a variety of assays to study cell-fate and neurobiology.


In developing Xenopus embryos, lithium chloride is observed to exert inhibition of GSK-3β (glycogen synthase kinase-3β), yet not reported to be a general inhibitor of other protein kinases.
These observations may have implications for lithium chloride on cell-fate determination in several organisms including Xenopus and Dictyostelium.


Additionally, in transfected Chinese Hamster Ovary cells (CHO) stimulated with angiotension II (Ang II), it was noted that lithium chloride enhanced the production of inositol triphosphate.
The antiviral properties of lithium chloride were noted in a study which showed that the compound inhibited pseudorabis virus infection in vitro.


In Drosophila, it was observed that in the nervous system, lithium chloride may have an effect on amino acid metabolism.
Futhermore, in glial primary cell cultures, lithium chloride has been noted to provide protection against glutamate excitotoxicity by potentially reducing NR1 mRNA, the major N-methyl-D-aspartate receptor (NMDAR) subunit in the cells.


Mainly we use Lithium chloride for the production of lithium metal by electrolysis of LiCl/KCl which melt at 450oC.
Moreover, industries use Lithium chloride as a brazing flux for aluminum in automobile parts.
In addition, we use Lithium chloride as a desiccant for drying air streams.


In organic synthesis, Lithium chloride has some specialized applications such as an additive in the Stille reaction.
Most noteworthy, Lithium chloride has biochemical applications that we use to precipitate RNA from cellular extracts.
Another application o Lithium chloride is that we use it as a flame colorant to produce dark red flames.


In the calibration of hygrometers, they use Lithium chloride as a relative humidity standard.
Lithium chloride can be used as a hygrometer.
In addition, when exposed to air Lithium chloride salts from deliquescent self-solution.
Furthermore, the equilibrium Lithium chloride concentration of the resulting solution may directly relate to the relative humidity of the air.


Industries use Lithium chloride's molten form to prepare carbon nanotubes, lithium niobate, and grapheme.
Besides, Lithium chloride shows very strong acaricidal properties.
Lithium chloride has been shown to have strong acaricidal properties, being effective against Varroa destructor in populations of honey bees.


Lithium chloride is used as an aversive agent in lab animals to study conditioned place preference and aversion.
Lithium chloride is used in the following areas: scientific research and development and health services.
Lithium chloride is used for the manufacture of: chemicals, plastic products and pulp, paper and paper products.


-Industrial Applications of Lithium Chloride:
Electrochemistry:
Lithium metal is produced by electrolysis of lithium chloride and potassium chloride, which melts at 450°C.
High-purity lithium chloride is used as the feedstock in the process and makes about 99.5% pure lithium metal.


-Commercial applications of Lithium chloride
Lithium chloride is mainly used for the production of lithium metal by electrolysis of a LiCl/KCl melt at 450 °C (842 °F).
Lithium chloride is also used as a brazing flux for aluminium in automobile parts.
Lithium chloride is used as a desiccant for drying air streams.

In more specialized applications, Lithium chloride finds some use in organic synthesis, e.g., as an additive in the Stille reaction.
Also, in biochemical applications, Lithium chloride can be used to precipitate RNA from cellular extracts.
Lithium chloride is also used as a flame colorant to produce dark red flames.


-Niche uses of Lithium chloride:
Lithium chloride is used as a relative humidity standard in the calibration of hygrometers.
At 25 °C (77 °F) a saturated solution (45.8%) of the salt will yield an equilibrium relative humidity of 11.30%.
Additionally, Lithium chloride can be used as a hygrometer.

This deliquescent salt forms a self-solution when exposed to air.
The equilibrium Lithium chloride concentration in the resulting solution is directly related to the relative humidity of the air.

The percent relative humidity at 25 °C (77 °F) can be estimated, with minimal error in the range 10–30 °C (50–86 °F), from the following first-order equation: RH=107.93-2.11C, where C is solution Lithium chloride concentration, percent by mass.
Molten Lithium chloride is used for the preparation of carbon nanotubes, graphene and lithium niobate.



CHEMICAL PROPERTIES OF LITHIUM CHLORIDE:
The salt forms crystalline hydrates, unlike the other alkali metal chlorides.
Mono-, tri-, and pentahydrates are known.
The anhydrous salt can be regenerated by heating the hydrates.

Lithium chloride also absorbs up to four equivalents of ammonia/mol.
As with any other ionic chloride, solutions of Lithium chloride can serve as a source of chloride ion, e.g., forming a precipitate upon treatment with silver nitrate:
LiCl + AgNO3 → AgCl + LiNO3



PREPARATION OF LITHIUM CHLORIDE:
Lithium chloride is produced by treatment of lithium carbonate with hydrochloric acid.
Anhydrous Lithium chloride is prepared from the hydrate by heating in a stream of hydrogen chloride.



INDUSTRIAL GRADE OF LITHIUM CHLORIDE:
Lithium chloride is free-flowing white crystals.
Occasional dark particles may be visible and scattered in Lithium chloride.
The particles have no detectable effect on product purity and will not be cause for rejection.



PHYSICAL PROPERTIES OF LITHIUM CHLORIDE:
Lithium chloride appears as an odorless white crystalline hygroscopic solid.
Lithium chloride has a density of 2.068g/cm3 and its boiling point is 1382oC and its melting point is in between 605–614oC.

Lithium chloride is soluble in water, methanol, ethanol, isopropanol, butanol, formic acid, n- mehtylformamide, hydrazine, and THF.
In addition, Lithium chloride is slightly soluble in acetone and ammonia and is completely insoluble in dichloromethane.



CHEMICAL PROPERTIES OF LITHIUM CHLORIDE:
Lithium chloride reaction with sulfuric acid forms lithium sulfate and hydrogen chloride.
The chemical equation is given below.
2LiCl + H2SO4 → 2 HCl + Li2SO4

Lithium chloride reacts with a base like sodium hydroxide and forms lithium hydroxide and sodium chloride.
LiCl + NaOH → LiOH + NaCl

Like other metal chlorides its salt form crystalline hydrates. Furthermore, its mono-, tri-, pentahydrate are known.
We can regenerate its anhydrous salts by heating the hydrates.
In addition, Lithium chloride easily absorbs up to four equivalents of ammonia/mol.
However, with another ionic chloride, the solution of Lithium chloride can serve as a source of chloride ion.



CHEMICAL CHARACTERISTICS OF LITHIUM CHLORIDE:
Reaction with Sulfuric Acid:
Lithium chloride and sulfuric acid reaction form hydrogen chloride and lithium sulfate.
Here is the reaction’s chemical equation:
2LiCl+H2SO4→2HCl+Li2SO4



REACTION WITH BASE OF LITHIUM CHLORIDE:
Lithium chloride reacts with an alkali (such as Sodium Hydroxide) to form Sodium Chloride and Lithium Hydroxide.
LiCl+NaOH→LiOH+NaCl
Like other metal chlorides, lithium chloride salt produces crystalline hydrates.

You can regenerate its anhydrous salts after heating the hydrates.
Besides, Lithium chloride can easily absorb four equivalents of ammonia per mol.
However, lithium chloride can mainly serve as a chloride ion source when combined with an ionic chloride.



PHYSICAL PROPERTIES OF LITHIUM CHLORIDE:
Lithium chloride has a sharp, saline taste
Lithium chloride has cubic crystals, crystalline powder, or granule appearance

Lithium chloride has a melting point of 121°F and 2.068 density at 77°F
Lithium chloride's aqueous solution is neutral and a bit alkaline
Lithium chloride is soluble in ether, nitrobenzene, and water alcohols



FORMULA AND STRUCTURE OF LITHIUM CHLORIDE:
The chemical formula of Lithium chloride is LiCl.
Lithium chloride has a molar mass of 42.394 g/mol.
On molecular level the positively charged lithium-ion ( Li+ ) reacts with the negatively charged chloride ion ( Cl− ) to form Lithium chloride (LiCl).



PREPARATION OF LITHIUM CHLORIDE:
It can produce Lithium chloride by treatment of lithium carbonate with hydrochloric acid.
In addition, we can also generate Lithium chloride by the highly exothermic reaction of lithium metal with ether chlorine or anhydrous hydrogen chloride gas.
Furthermore, we can prepare anhydrous Lithium chloride from the hydrating and heating with a stream of hydrogen chloride.



PHYSICAL and CHEMICAL PROPERTIES of LITHIUM CHLORIDE:
Chemical formula: LiCl
Molar mass: 42.39 g·mol−1
Appearance: white solid
hygroscopic, sharp
Density: 2.068 g/cm3
Melting point: 605–614 °C (1,121–1,137 °F; 878–887 K)
Boiling point: 1,382 °C (2,520 °F; 1,655 K)
Solubility in water: 68.29 g/100 mL (0 °C)
74.48 g/100 mL (10 °C)
84.25 g/100 mL (25 °C)
88.7 g/100 mL (40 °C)
123.44 g/100 mL (100 °C)
Solubility: soluble in hydrazine, methylformamide,
butanol, selenium(IV) oxychloride, 1-propanol

Solubility in methanol: 45.2 g/100 g (0 °C)
43.8 g/100 g (20 °C)
42.36 g/100 g (25 °C)
44.6 g/100 g (60 °C)
Solubility in ethanol: 14.42 g/100 g (0 °C)
24.28 g/100 g (20 °C)
25.1 g/100 g (30 °C)
23.46 g/100 g (60 °C)
Solubility in formic acid: 26.6 g/100 g (18 °C)
27.5 g/100 g (25 °C)
Solubility in acetone: 1.2 g/100 g (20 °C)
0.83 g/100 g (25 °C)
0.61 g/100 g (50 °C)
Solubility in liquid ammonia: 0.54 g/100 g (-34 °C)
3.02 g/100 g (25 °C)

Vapor pressure: 1 torr (785 °C)
10 torr (934 °C)
100 torr (1130 °C)
Magnetic susceptibility (χ): −24.3·10−6 cm3/mol
Refractive index (nD): 1.662 (24 °C)
Viscosity: 0.87 cP (807 °C)
Structure:
Coordination geometry: Octahedral
Molecular shape: Linear (gas)
Dipole moment: 7.13 D (gas)
Thermochemistry:
Heat capacity (C): 48.03 J/mol·K
Std molar entropy (S⦵298): 59.31 J/mol·K
Std enthalpy of formation (ΔfH⦵298): -408.27 kJ/mol
Gibbs free energy (ΔfG⦵): -384 kJ/mol
Molecular Weight: 42.4 g/mol

Hydrogen Bond Donor Count: 0
Hydrogen Bond Acceptor Count: 1
Rotatable Bond Count: 0
Exact Mass: 41.9848561 g/mol
Monoisotopic Mass: 41.9848561 g/mol
Topological Polar Surface Area: 0Ų
Heavy Atom Count: 2
Formal Charge: 0
Complexity: 2
Isotope Atom Count: 0
Defined Atom Stereocenter Count: 0
Undefined Atom Stereocenter Count: 0
Defined Bond Stereocenter Count: 0
Undefined Bond Stereocenter Count: 0
Covalently-Bonded Unit Count: 2
Compound Is Canonicalized: Yes

Physical state: powder
Color: colorless
Odor: odorless
Melting point/freezing point:
Melting point/range: 605 °C
Initial boiling point and boiling range: 1.360 °C at 1.013 hPa
Flammability (solid, gas): The product is not flammable.
Upper/lower flammability or explosive limits: No data available
Flash point: Not applicable
Autoignition temperature: No data available
Decomposition temperature: No data available
pH: ca.6 at 50 g/l at 20 °C
Viscosity
Viscosity, kinematic: No data available
Viscosity, dynamic: No data available

Water solubility: 569 g/l at 20 °C
Partition coefficient: n-octanol/water: Not applicable for inorganic substances
Vapor pressure: 1,33 hPa at 547 °C
Density: 2,07 g/cm3 at 20 °C
Relative density: No data available
Relative vapor density: No data available
Particle characteristics: No data available
Explosive properties: No data available
Oxidizing properties: none
Other safety information: No data available
LiCl: Lithium Chloride
Density: 2.07 g/cm³
Molecular Weight/ Molar Mass: 42.394 g/mol

Boiling Point: 1,382 °C
Melting Point: 605 °C
Chemical Formula: LiCl
Odour: Odourless
Boiling Point/Range: 1.360 °C (1.013 hPa)
Color: Colorless
Density: 2.07 g/cm3 (20 °C)
Flashpoint: Not applicable
Form: Solid
Grade: Reagent Grade
Incompatible Materials: Strong acids
Lower Explosion Limit: Not applicable
Melting Point/Range: 605 °C
Partition Coefficient: No data available
Purity Percentage: 99.00
Purity Details: >=99.00%

Solubility in Water: Soluble
Upper Explosion Limit: Not applicable
Vapor Pressure: No data available
pH-Value: 6.0-8.0 at 50 g/l (20 °C)
Storage Temperature: Ambient
Appearance: White solid hygroscopic
Covalently-Bonded Unit: 2
Specific Gravity: 2.068 at 77 ° F
Complexity: 2
Solubility: Insoluble in water
CAS: 7447-41-8
MF: LiCl
MW: 42.39
EINECS: 231-212-3
Mol File: 7447-41-8.mol

Lithium chloride Chemical Properties:
Melting point: 605 °C(lit.)
Boiling point: 1382°C
density: 2.06
vapor pressure: 1.33 hPa (547 °C)
refractive index: n20/D 1.381
Fp: -4 °F
storage temp.: 2-8°C
solubility: H2O: soluble
form: beads
color: White to gray
Specific Gravity: 2.068
Odor: Odorless

PH: 5.5-7.5 (25℃, 50mg/mL in H2O)
PH Range: 6
Water Solubility: 832 g/L (20 ºC)
λmax: λ: 260 nm Amax: 0.01
λ: 280 nm Amax: 0.01
Sensitive: Hygroscopic
Merck: 145,528
Stability: Stable.
InChIKey: KWGKDLIKAYFUFQ-UHFFFAOYSA-M
CAS DataBase Reference: 7447-41-8(CAS DataBase Reference)
NIST Chemistry Reference: Lithium chloride(7447-41-8)
EPA Substance Registry System: Lithium chloride (7447-41-8)
Linear Formula: LiCl
UN Number: NONH for all modes of transport
Formula Weight: 42.39g/mol
Chemical Name or Material: Lithium Chloride



FIRST AID MEASURES of LITHIUM CHLORIDE:
-Description of first-aid measures:
*General advice:
Show this material safety data sheet to the doctor in attendance.
*If inhaled:
After inhalation:
Fresh air.
*In case of skin contact:
Take off immediately all contaminated clothing.
Rinse skin with water/ shower.
*In case of eye contact:
After eye contact:
Rinse out with plenty of water.
Call in ophthalmologist.
Remove contact lenses.
*If swallowed:
After swallowing:
Immediately make victim drink water (two glasses at most).
Consult a physician.
-Indication of any immediate medical attention and special treatment needed:
No data available



ACCIDENTAL RELEASE MEASURES of LITHIUM CHLORIDE:
-Environmental precautions:
Do not let product enter drains.
-Methods and materials for containment and cleaning up:
Cover drains.
Collect, bind, and pump off spills.
Observe possible material restrictions.
Take up dry.
Dispose of properly.
Clean up affected area.



FIRE FIGHTING MEASURES of LITHIUM CHLORIDE:
-Extinguishing media:
*Suitable extinguishing media:
Use extinguishing measures that are appropriate to local circumstances and the
surrounding environment.
*Unsuitable extinguishing media:
For this substance/mixture no limitations of extinguishing agents are given.
-Further information:
Suppress (knock down) gases/vapors/mists with a water spray jet.
Prevent fire extinguishing water from contaminating surface water or the ground water system.



EXPOSURE CONTROLS/PERSONAL PROTECTION of LITHIUM CHLORIDE:
-Exposure controls:
--Personal protective equipment:
*Eye/face protection:
Use equipment for eye protection.
Safety glasses
*Skin protection:
Full contact:
Material: Nitrile rubber
Minimum layer thickness: 0,11 mm
Break through time: 480 min
Splash contact:
Material: Nitrile rubber
Minimum layer thickness: 0,11 mm
Break through time: 480 min
*Body Protection:
protective clothing
*Respiratory protection:
Recommended Filter type: Filter type P2
-Control of environmental exposure:
Do not let product enter drains.



HANDLING and STORAGE of LITHIUM CHLORIDE:
-Conditions for safe storage, including any incompatibilities:
*Storage conditions:
Tightly closed.
Dry.
hygroscopic
*Storage class:
Storage class (TRGS 510): 13:
Non Combustible Solids



STABILITY and REACTIVITY of LITHIUM CHLORIDE:
-Reactivity:
No data available
-Chemical stability:
The product is chemically stable under standard ambient conditions (room temperature) .
-Conditions to avoid:
no information available
-Incompatible materials:
No data available

Lithium chloride is an ionic compound or salt that is highly polar and soluble in water.
Lithium chloride is more soluble in organic solvents such as acetone and methanol than potassium chloride or sodium chloride.
The chemical formula for Lithium chlorideis LiCl.


CAS Number: 7447-41-8
EC Number: 231-212-3
MDL number: MFCD00011078
Chemical formula: LiCl



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Lithium chloride is a salt of Lithium chlorine, an alkali metal similar to sodium chloride.
Although the Li+ ion is minuscule, Lithium chloride creates unrecognized effects for other alkali metal chlorides, such as being soluble in polar solvents and having hygroscopic (holding water molecules) properties.


Lithium chloride has a typical shelf life of 2 years if kept in dry conditions.
Lithium chloride appears as colorless crystals or powder.
Lithium chloride is a solid which absorbs water to form a hydrate, LiCl.H2O.


Lithium chloride is an injection indicated for cardiac output measurement.
Crystallization grade Lithium chloride for formulating screens or for optimization.
The chemical formula of anhydrous Lithium chloride is LiCl, the relative molecular weight is 42.39, which is cubic crystal white particles or powder, which is easy to deliquesce and tastes salty.


Lithium chloride belongs to the low-toxicity category, but has a strong irritating and corrosive effect on the eyes and mucous membranes.
The specific gravity of Lithium chloride is 2.068, the melting point is 605°C, the boiling point is 1360°C, and it is easily soluble in water grams (0°C) in 100 grams of water, 127.5 grams (100°C)].


Lithium chloride is soluble in alcohol, slightly soluble in acetone, pyridine and liquid ammonia.
Lithium chloride is a chemical compound with the formula LiCl.
Lithium chloride behaves as a fairly typical ionic compound, although the Li+ ion is very small.


Lithium chloride is hygroscopic and highly soluble in water, and is highly polar.
Lithium chloride is more soluble in polar organic solvents such as methanol and acetone than is sodium chloride or potassium chloride.
Lithium chloride is a chemical compound with the formula LiCl.


Lithium chloride is a typical ionic compound (with certain covalent characteristics), although the small size of the Li+ ion gives rise to properties not seen for other alkali metal chlorides, such as extraordinary solubility in polar solvents (83.05 g/100 mL of water at 20 °C) and its hygroscopic properties.
Lithium chloride appears as colorless crystals or powder.


Lithium chloride is a metal chloride salt with a Li(+) counterion.
Lithium chloride has a role as an antimanic drug and a geroprotector.
Lithium chloride is an inorganic chloride and a lithium salt.


Lithium chloride is a salt of lithium that has been used experimentally as an immunomodulator.
Lithium chloride is a white solid hygroscopic soluble in water, alcohol and ether.
Lithium chloride is made by the action of hydrochloric acid on lithium hydroxide.


The resulting solution is evaporated to get a mixture of saturated solution and Lithium chloride crystals.
The solid and the solution is separated and the supernatant solution is recycled for further evaporation.
Lithium chloride is a solid which absorbs water to form a hydrate, LiCl.H2O


Lithium chloride acts as an electrolyte for dry cells used at low temperatures, catalyst in certain oxidation reactions, solubilizer for polyamides and cellulose when used with amide solvents, chlorinating agent for steroid substrates.
Lithium chloride is registered under the REACH Regulation and is manufactured in and / or imported to the European Economic Area, at ≥ 1 000 to < 10 000 tonnes per annum.


Lithium chloride is a chemical compound with a chemical formula “LiCl”.
The salt is a normal ionic compound, although the Li+ ion is small in size, Lithium chloride produces unrecognized effects for other alkali metal chlorides, such as exceptional solubility in polar solvents and its hygroscopic properties.


Lithium chloride is for assays to study cell-fate, neurobiology and antiviral properties; noted to inhibit GSK-3β
Lithium chloride is hygroscopic in nature.
Lithium chloride is incompatible with strong oxidizing agents, strong acids, bromine trichloride and bromine trifluoride.


Deliquescent salt forms a solution when exposed to humid air.
Store Lithium chloride in a cool and dry place in closed tight containers.
Lithium chloride is a typical ionic compound and a salt of lithium.


Due to the small size of the lithium-ion ( Li+ ), Lithium chloride gives rise to properties that we cannot see in other alkali metal chlorides.
Lithium chloride is an antiviral metal halide utilized in a variety of assays to study cell-fate and neurobiology.
In developing Xenopus embryos, Lithium chloride is observed to exert inhibition of GSK-3β (glycogen synthase kinase-3β), yet not reported to be a general inhibitor of other protein kinases.


These observations may have implications for Lithium chloride on cell-fate determination in several organisms including Xenopus and Dictyostelium.
Additionally, in transfected Chinese Hamster Ovary cells (CHO) stimulated with angiotension II (Ang II), it was noted that Lithium chloride enhanced the production of inositol triphosphate.


The antiviral properties of Lithium chloride were noted in a study which showed that the compound inhibited pseudorabis virus infection in vitro.
In Drosophila, it was observed that in the nervous system, Lithium chloride may have an effect on amino acid metabolism.
Futhermore, in glial primary cell cultures, Lithium chloride has been noted to provide protection against glutamate excitotoxicity by potentially reducing NR1 mRNA, the major N-methyl-D-aspartate receptor (NMDAR) subunit in the cells.



USES and APPLICATIONS of LITHIUM CHLORIDE:
Lithium chloride is a very effective antimanic drug for the treatment of bipolar disorder.
Lithium chloride is well soluble in water, alcohol, acetone, and amyl alcohol and Lithium chloride is also used as a flame colorant to produce dark red flames.


Lithium chloride is used as an electrolyte in voltaic cells.
Lithium chloride is used to produce a dark red flame.
Lithium chloride is used in supplements.


Lithium chloride is also used in organic synthesis.
Lithium chloride is used to precipitate RNA.


Lithium chloride is used fluxes for welding and soldering techniques; salt bath for heat-treatment by low temperature and for dip brazing; raw material for other lithium compounds; tracer for chemical products (denaturation of wine etc.); absorption and desinfection reagent (lithium chloride solution) for absorbers.


Lithium chloride is used as a brazing flux, as a desiccant in drying air streams, as a component in organic synthesis, as an additive in the Stille reaction, in some biochemical applications, and as soldering aluminum metal.
Lithium chloride is used for the production of lithium metal, by electrolysis of a LiCl/KCl melt at 450 °C.


Lithium chloride is also used as a brazing flux for aluminium in automobile parts.
Lithium chloride can be used to improve the efficiency of the Stille reaction.
Lithium chloride's desiccant properties can be used to generate potable water by absorbing moisture from the air, which is then released by heating the salt.


Lithium chloride has many applications.
Lithium chloride is extremely hygroscopic, and is widely used in dehumidification systems to remove moisture from the air in industries such as food processing and horticulture.


Lithium chloride is also used as a tracer for waste water, as a brazing flux, and as an electrolyte component for the manufacture of speciality batteries.
Lithium chloride is used as an electrolyte for low temperature dry battery cells and as an oxidation catalyst.
Lithium chloride is a solubilizer for polyamides and cellulose when used with amide solvents, and is a chlorinating agent for steroid substrates.


Lithium chloride has also been utilized in: Large scale plasmid DNA isolation without ultracentrifugation; Protein extraction and protein crystallization; Crystallization of other biological structures, including vitamin B12-RNA aptamer and the L-A virus particle; Inhibits the expression and secretion of insulin-like growth factor-binding protein-1 in H4-II-E cells; Used in the synthesis of beta-substituted alpha-amino acid derivatives; May be used to selectively pre­cipitate RNA.


Lithium chloride is mainly we use it for the production of lithium metal by electrolysis of LiCl/KCl which melt at 450oC.
Moreover, industries use Lithium chloride as a brazing flux for aluminum in automobile parts.
In addition, we use Lithium chloride as a desiccant for drying air streams.


In organic synthesis, Lithium chloride has some specialized applications such as an additive in the Stille reaction.
Most noteworthy, Lithium chloride has biochemical applications that we use to precipitate RNA from cellular extracts.
Another application of Lithium chloride is that we use it as a flame colorant to produce dark red flames.


In the calibration of hygrometers, they use Lithium chloride as a relative humidity standard.
Lithium chloride can be used as a hygrometer. In addition, when exposed to air it salts from deliquescent self-solution.
Furthermore, the equilibrium Lithium chloride concentration of the resulting solution may directly relate to the relative humidity of the air.


Industries use Lithium chloride's molten form to prepare carbon nanotubes, lithium niobate, and grapheme.
Besides, Lithium chloride shows very strong acaricidal properties.
Lithium chloride is a chemical compound that is extremely soluble in polar solvents and is used in order to obtain lithium metal.


In organic synthesis Lithium chloride is used as an additive in the Stille Reaction.
Ungraded products supplied by Spectrum are indicative of a grade suitable for general industrial use or research purposes and typically are not suitable for consumption.


Lithium chloride is also used as a flame colorant to produce dark red flames.
Molten Lithium chloride is used for the preparation of carbon nanotubes, graphene and lithium niobate.
Lithium chloride has been shown to have strong acaricidal properties, being effective against Varroa destructor in populations of honey bees.


Lithium chloride is used as an aversive agent in lab animals to study conditioned place preference and aversion.
Lithium chloride is widely used in several industrial applications.
Lithium chloridet is used as a flame colorant to form dark crimson flames.


Lithium chloride is used in the precipitation of RNA in biological applications.
Lithium chloride is an aluminum blazing flux in automobile parts.
Lithium chloride is used for several soldering and welding techniques and salt bath heat treatment at low temperatures.


Lithium chloride is used in massive dehumidification systems in the AC industry.
This depends on the low equilibrium pressure of vapor above Lithium chloride solutions.
Lithium chloride is used in large dehumidification systems in the air conditioning industry.


It depends on the low equilibrium pressure of water vapour above solutions of Lithium chloride.
Lithium chloride is used in a number of salt mixtures exist low melting points allowing the material to be used in brazing fluxes and brazing baths.
Lithium chloride is used as an electrolyte for the production of lithium metal and used as an electrolyte in voltaic cells.


Lithium chloride is used by consumers, in articles, by professional workers (widespread uses), in formulation or re-packing, at industrial sites and in manufacturing.
Lithium chloride is used in the following products: coating products, metal surface treatment products, non-metal-surface treatment products, adhesives and sealants, inks and toners, pH regulators and water treatment products, photo-chemicals, polishes and waxes and welding & soldering products.


Other release to the environment of Lithium chloridee is likely to occur from: indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners), outdoor use, indoor use in close systems with minimal release (e.g. cooling liquids in refrigerators, oil-based electric heaters), outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids), outdoor use in long-life materials with low release rate (e.g. metal, wooden and plastic construction and building materials) and indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment).


Lithium chloride is useful for the production of lithium metal and for the generation of Mn(0) species which can be used in free radical cyclizations.
Lithium chloride can serve as a flame colorant to generate dark red flames, a brazing flux for aluminum in automobiles, a hygrometer and a desiccant for drying air streams.


On exposure to air, Lithium chloride becomes a solution with the concentration directly related to relative humidity of the atmosphere and hence serves as a relative humidity standard in calibrating hygrometers.
Apart from being a source of chloride, Lithium chloride serves as an additive in the Stille reaction in organic synthesis and to precipitate RNA from cellular extracts.


Being biologically significant, Lithium chloride finds applications in a wide variety of assays to study cell-fate and neurobiology.
Lithium chloride has been found to inhibit virus infection.
Release to the environment of Lithium chloride can occur from industrial use: industrial abrasion processing with low release rate (e.g. cutting of textile, cutting, machining or grinding of metal).


Other release to the environment of this substance is likely to occur from: indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment). This substance can be found in products with material based on: stone, plaster, cement, glass or ceramic (e.g. dishes, pots/pans, food storage containers, construction and isolation material) and paper (e.g. tissues, feminine hygiene products, nappies, books, magazines, wallpaper).


Lithium chloride is used in the following products: laboratory chemicals, pH regulators and water treatment products, metal working fluids, pharmaceuticals, polymers, water treatment chemicals and welding & soldering products.
Lithium chloride is used in the following areas: scientific research and development and health services.


Other release to the environment of Lithium chloride is likely to occur from: indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners), outdoor use, indoor use in close systems with minimal release (e.g. cooling liquids in refrigerators, oil-based electric heaters), outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids), outdoor use in long-life materials with low release rate (e.g. metal, wooden and plastic construction and building materials) and indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment).


Lithium chloride is used in the following products: pharmaceuticals, air care products, inks and toners, laboratory chemicals, metal working fluids, paper chemicals and dyes, polymers, water treatment chemicals and welding & soldering products.
Release to the environment of Lithium chloride can occur from industrial use: formulation of mixtures and formulation in materials.


Lithium chloride is used in the following products: welding & soldering products, laboratory chemicals, air care products, inks and toners, pH regulators and water treatment products, metal working fluids, pharmaceuticals, polymers and water treatment chemicals.
Lithium chloride is used in the following areas: scientific research and development and health services.


Release to the environment of Lithium chloride can occur from industrial use: in processing aids at industrial sites, as an intermediate step in further manufacturing of another substance (use of intermediates), as processing aid, of substances in closed systems with minimal release and in the production of articles.


Lithium chloride is used for the manufacture of: chemicals and plastic products.
Lithium chloride is used for the manufacture of: chemicals, plastic products and pulp, paper and paper products.
Release to the environment of Lithium chloride can occur from industrial use: manufacturing of the substance.


Lithium Metal by Electrolysis: Lithium chloride is primarily used at 450 ° C (842 ° F) for the preparation of lithium metal by electrolysis of a LiCl / KCl.
As Brazing Flux uses of Lithium chloride: Lithium chloride is also used as a brazing flux for aluminum in automobile parts.
Lithium chloride is used as desiccant in drying air streams.


Lithium chloride is used in organic synthesis.
For example, as an additive in the Stille reaction.
Biochemical Applications: LiCl is used to precipitate RNA from cellular extracts.


As a flame colorant, Lithium chloride is used to produce dark red flames.
Lithium chloride is used as a Relative humidity standard in the calibration of hygrometers and itself can be used as a hygrometer.
Molten Lithium chloride is used for the preparation of lithium niobite, graphene and carbon nanotubes.


Lithium chloride is useful for the production of lithium metal and for the generation of Mn(0) species which can be used in free radical cyclizations.
Lithium chloride can serve as a flame colorant to generate dark red flames, a brazing flux for aluminum in automobiles, a hygrometer and a desiccant for drying air streams.


On exposure to air, Lithium chloride becomes a solution with the concentration directly related to relative humidity of the atmosphere and hence serves as a relative humidity standard in calibrating hygrometers.
Apart from being a source of chloride, Lithium chloride serves as an additive in the Stille reaction in organic synthesis and to precipitate RNA from cellular extracts.


Being biologically significant, Lithium chloride finds applications in a wide variety of assays to study cell-fate and neurobiology.
Lithium chloride has been found to inhibit virus infection.
Lithium chloride has strong acaricidal properties (Varroa destructor in populations of honey bees).


-Commercial applications of Lithium chloride:
Lithium chloride is mainly used for the production of lithium metal by electrolysis of a LiCl/KCl melt at 450 °C (842 °F).
Lithium chloride is also used as a brazing flux for aluminium in automobile parts.

Lithium chloride is used as a desiccant for drying air streams.
In more specialized applications, Lithium chloride finds some use in organic synthesis, e.g., as an additive in the Stille reaction.
Also, in biochemical applications, Lithium chloride can be used to precipitate RNA from cellular extracts.


-Niche uses of Lithium chloride:
Lithium chloride is used as a relative humidity standard in the calibration of hygrometers.
At 25 °C (77 °F) a saturated solution (45.8%) of the salt will yield an equilibrium relative humidity of 11.30%.

Additionally, Lithium chloride can be used as a hygrometer.
This deliquescent salt forms of Lithium chloride a self-solution when exposed to air.
The equilibrium Lithium chloride concentration in the resulting solution is directly related to the relative humidity of the air.

The percent relative humidity at 25 °C (77 °F) can be estimated, with minimal error in the range 10–30 °C (50–86 °F), from the following first-order equation: RH=107.93-2.11C, where C is solution Lithium chloride concentration, percent by mass.


-Electrochemistry uses of Lithium chloride:
Lithium metal is produced by electrolysis of Lithium chloride and potassium chloride, which melts at 450°C.
High-purity Lithium chloride is used as the feedstock in the process and makes about 99.5% pure lithium metal.

Molten lithium is contained in a carbon steel pot, while the chlorine gas is collected in a stainless steel or glass pipe for applications in other processes.
The molten lithium flows into a collecting tank and is later cast into ingots.
A mesh or stainless-steel screen separates the two compartments to prevent the products from mixing.



CHEMICAL PROPERTIES OF LITHIUM CHLORIDE:
Like other metal chlorides Lithium chloride's salt form crystalline hydrates.
Furthermore, Lithium chloride's mono-, tri-, pentahydrate are known.
We can regenerate Lithium chloride's anhydrous salts by heating the hydrates.
In addition, Lithium chloride easily absorbs up to four equivalents of ammonia/mol.
However, with another ionic chloride, the solution of Lithium chloridecan serve as a source of chloride ion.



PREPARATION OF LITHIUM CHLORIDE:
Lithium chloride is prepared by treating lithium carbonate with hydrochloric acid.
Lithium chloride is the highly exothermic reaction of lithium metal with either chlorine or anhydrous hydrogen chloride gas.
When hydrate is heated along with a stream of hydrogen chloride, then anhydrous Lithium chloride is produced



CHEMICAL PROPERTIES OF LITHIUM CHLORIDE:
Lithium chloride reaction with sulfuric acid forms lithium sulfate and hydrogen chloride.
The chemical equation is given below.

2LiCl + H2SO4 → 2 HCl + Li2SO4
Lithium chloride reacts with a base like sodium hydroxide and forms lithium hydroxide and sodium chloride.
LiCl + NaOH → LiOH + NaCl



PHYSICAL PROPERTIES OF LITHIUM CHLORIDE:
Lithium chloride appears as an odorless white crystalline hygroscopic solid.
Lithium chloride has a density of 2.068g/cm3 and its boiling point is 1382oC and its melting point is in between 605–614oC.
Lithium chloride is soluble in water, methanol, ethanol, isopropanol, butanol, formic acid, n- mehtylformamide, hydrazine, and THF.
In addition, Lithium chloride is slightly soluble in acetone and ammonia and is completely insoluble in dichloromethane.



CHEMICAL PROPERTIES OF LITHIUM CHLORIDE:
Lithium Chloride Reaction with Sulfuric Acid:
When Lithium chloride reacts with sulfuric acid, it forms lithium sulfate and hydrogen chloride.
The chemical equation is given below.
2LiCl+H2SO4→2HCl+Li2SO4



LITHIUM CHLORIDE REACTS WITH BASE:
When Lithium chloride reacts with sodium hydroxide, it forms lithium hydroxide and sodium chloride.
LiCl+NaOH→LiOH+NaCl
Step-by-Step Explanation of How to Draw the Lithium Chloride Lewis



STRUCTURE OF LITHIUM CHLORIDE:
Lithium chloride structure LiCl is drawn with the help of lewis dots
Lithium chloride is ionic compound, in which Lithium is a metal compound and chloride is a non-metal.

Where electrons are transferred from metal ion to non-metal ion.
One electron is transferred from lithium and makes Lithium chloride electro-positive and by gaining one electron from lithium, chlorine becomes electronegative.



CHEMICAL PROPERTIES OF LITHIUM CHLORIDE:
The salt forms crystalline hydrates, unlike the other alkali metal chlorides.
Mono-, tri-, and pentahydrates are known.
The anhydrous salt can be regenerated by heating the hydrates.

Lithium chloride also absorbs up to four equivalents of ammonia/mol.
As with any other ionic chloride, solutions of Lithium chloride can serve as a source of chloride ion, e.g., forming a precipitate upon treatment with silver nitrate:
LiCl + AgNO3 → AgCl + LiNO3



PREPARATION OF LITHIUM CHLORIDE:
Lithium chloride is produced by treatment of lithium carbonate with hydrochloric acid.
Anhydrous Lithium chloride is prepared from the hydrate by heating in a stream of hydrogen chloride.



PROPERTIES OF LITHIUM CHLORIDE:
1. Physical Properties of Lithium Chloride Licl:
Lithium chloride is Deliquescent in nature, appear as cubic crystals, granules or crystalline powder
Lithium chloride has sharp saline taste

Lithium chloride has Boiling point of 2417 to 2480 °F at 760 mm Hg
Lithium chloride's Melting point is 1121 °F
Lithium chloride has Density of 2.068 at 77 °F

Aqueous solution of Lithium chloride is neutral or slightly alkaline.
Lithium chloride is very soluble in water alcohols, ether, pyridine, nitrobenzene



LITHIUM CHLORIDE FORMULA AND STRUCTURE:
The chemical formula of Lithium chloride is LiCl.
Lithium chloride has a molar mass of 42.394 g/mol.
On molecular level the positively charged lithium-ion ( Li+ ) reacts with the negatively charged chloride ion ( Cl− ) to form Lithium chloride (LiCl).



PREPARATION OF LITHIUM CHLORIDE:
We can produce Lithium chloride by treatment of lithium carbonate with hydrochloric acid.
In addition, we can also generate Lithium chloride by the highly exothermic reaction of lithium metal with ether chlorine or anhydrous hydrogen chloride gas.
Furthermore, we can prepare anhydrous Lithium chloride from the hydrating and heating with a stream of hydrogen chloride.



PHYSICAL PROPERTIES OF LITHIUM CHLORIDE:
Lithium chloride has a sharp, saline taste.
Lithium chloride has cubic crystals, crystalline powder, or granule appearance.
Lithium chloride has a melting point of 121°F and 2.068 density at 77°F.
Lithium chloride's aqueous solution is neutral and a bit alkaline.
Lithium chloride is soluble in ether, nitrobenzene, and water alcohols.



CHEMICAL CHARACTERISTICS OF LITHIUM CHLORIDE:
Reaction with Sulfuric Acid:
Lithium chloride and sulfuric acid reaction form hydrogen chloride and lithium sulfate.
Here is the reaction’s chemical equation:
2LiCl+H2SO4→2HCl+Li2SO4



REACTION WITH BASE OF LITHIUM CHLORIDE:
Lithium chloride reacts with an alkali (such as Sodium Hydroxide) to form Sodium Chloride and Lithium Hydroxide.
LiCl+NaOH→LiOH+NaCl
Like other metal chlorides, Lithium chloride salt produces crystalline hydrates.

You can regenerate its anhydrous salts after heating the hydrates.
Besides, Lithium chloride can easily absorb four equivalents of ammonia per mol.
However, Lithium chloride can mainly serve as a chloride ion source when combined with an ionic chloride.



FEATURES OF LITHIUM CHLORIDE:
Sterile filtered solution:
Formulated in Type 1+ ultrapure water: 18.2 megaohm-cm resistivity at 25°C, < 5 ppb Total Organic Carbon, bacteria free (


FUNCTION AND PURPOSE OF LITHIUM CHLORIDE:
Raw material for preparing metallic lithium.
Flux in the production of metal by electrolysis (such as the production of titanium and aluminum), used as aluminum welding agent, air conditioning dehumidifier and special cement raw material, also used in flames, in the battery industry for the production of lithium manganese battery electrolyte, etc.
Anhydrous Lithium chloride is mainly used for electrolytic preparation of metallic lithium and aluminum fluxes and fluxes, as well as moisture absorbing (dehumidifying) agents in non-refrigerated air conditioners.



PREPARATION OF LITHIUM CHLORIDE:
Lithium chloride can be prepared by reacting lithium carbonate with Hydrochloric acid.
Lithium chloride is an exothermic reaction of lithium with either chlorine or hydrogen chloride gas.
Li2CO3 + HCl ⇢ LiCl + CO2 + H2O
When Lithium chloride is heated along with hydrogen chloride then LiCl is produced.



PHYSICAL PROPERTIES OF LITHIUM CHLORIDE:
Lithium chloride is an odorless white crystalline solid.
The density of Lithium chloride is 2.068 g/cm3.
Lithium chloride is well soluble in water, alcohol, and ester nitrobenzene.
Lithium chloride has a boiling point of 1,382°C.
Lithium chloride has a melting point of 605 – 614°C.



CHEMICAL PROPERTIES OF LITHIUM CHLORIDE:
When Lithium chloride reacts with H2SO4 it gives lithium sulfate and hydrogen chloride.
2LiCl + H2SO4 → 2 HCl + Li2SO4
When Lithium chloride reacts with a base like NaOH it gives lithium hydroxide and sodium chloride.
LiCl + NaOH → LiOH + NaCl



FORMULA OF LITHIUM CHLORIDE:
Lithium chloride also known as LiCl is presented in this article. when the positively charged lithium-ion (Li+) reacts with the negatively charged chloride ion (Cl−) then the obtained formula is known as Lithium chloride (LiCl).
The molecule is formed by one lithium cation Li+ and one chlorine anion Cl–.
The molar mass of Lithium chloride is 42.39 g/mol.
The chemical and molecular formula of Lithium chloride is LiCl.



STRUCTURE OF LITHIUM CHLORIDE:
Lithium chloride is an ionic compound in which lithium is a metal compound and chloride is a nonmetal compound where electrons are transferred from metal ion to nonmetal ion.
In this type of structure, one electron is transferred by lithium and Lithium chloride becomes electropositive chlorine gain one electron then it becomes electronegative.



CHEMICAL PROPERTIES OF LITHIUM CHLORIDE:
Lithium chloride can react as a source of chloride ion.
As with any other soluble ionic chloride, Lithium chloride will precipitate insoluble chlorides when added to a solution of an appropriate metal salt such as lead(II) nitrate:

2 LiCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 LiNO3(aq)
The Li+ ion acts as a weak Lewis acid under certain circumstances; for example one mole of Lithium chloride is capable of absorbing up to four moles of ammonia.



PREPARATION OF LITHIUM CHLORIDE:
Lithium chloride may be prepared most simply by reaction of lithium hydroxide or lithium carbonate with hydrochloric acid.
Lithium chloride may also be prepared by the highly exothermic reaction of lithium metal with either chlorine or anhydrous hydrogen chloride gas.
Anhydrous Lithium chloride is prepared from the hydrate by gently heating under an atmosphere of hydrogen chloride, used to prevent hydrolysis.



PHYSICAL and CHEMICAL PROPERTIES of LITHIUM CHLORIDE:
Chemical formula: LiCl
Molar mass: 42.39 g·mol−1
Appearance: white solid
hygroscopic, sharp
Density: 2.068 g/cm3
Melting point: 605–614 °C (1,121–1,137 °F; 878–887 K)
Boiling point: 1,382 °C (2,520 °F; 1,655 K)
Solubility in water: 68.29 g/100 mL (0 °C)
74.48 g/100 mL (10 °C)
84.25 g/100 mL (25 °C)
88.7 g/100 mL (40 °C)
123.44 g/100 mL (100 °C)
Solubility: soluble in hydrazine, methylformamide,
butanol, selenium(IV) oxychloride, 1-propanol

Solubility in methanol: 45.2 g/100 g (0 °C)
43.8 g/100 g (20 °C)
42.36 g/100 g (25 °C)
44.6 g/100 g (60 °C)
Solubility in ethanol: 14.42 g/100 g (0 °C)
24.28 g/100 g (20 °C)
25.1 g/100 g (30 °C)
23.46 g/100 g (60 °C)
Solubility in formic acid: 26.6 g/100 g (18 °C)
27.5 g/100 g (25 °C)
Solubility in acetone: 1.2 g/100 g (20 °C)
0.83 g/100 g (25 °C)
0.61 g/100 g (50 °C)
Solubility in liquid ammonia: 0.54 g/100 g (-34 °C)
3.02 g/100 g (25 °C)

Vapor pressure: 1 torr (785 °C)
10 torr (934 °C)
100 torr (1130 °C)
Magnetic susceptibility (χ): −24.3·10−6 cm3/mol
Refractive index (nD): 1.662 (24 °C)
Viscosity: 0.87 cP (807 °C)
Structure:
Coordination geometry: Octahedral
Molecular shape: Linear (gas)
Dipole moment: 7.13 D (gas)
Thermochemistry:
Heat capacity (C): 48.03 J/mol·K
Std molar entropy (S⦵298): 59.31 J/mol·K
Std enthalpy of formation (ΔfH⦵298): -408.27 kJ/mol
Gibbs free energy (ΔfG⦵): -384 kJ/mol
Molecular Weight: 42.4 g/mol

Hydrogen Bond Donor Count: 0
Hydrogen Bond Acceptor Count: 1
Rotatable Bond Count: 0
Exact Mass: 41.9848561 g/mol
Monoisotopic Mass: 41.9848561 g/mol
Topological Polar Surface Area: 0Ų
Heavy Atom Count: 2
Formal Charge: 0
Complexity: 2
Isotope Atom Count: 0
Defined Atom Stereocenter Count: 0
Undefined Atom Stereocenter Count: 0
Defined Bond Stereocenter Count: 0
Undefined Bond Stereocenter Count: 0
Covalently-Bonded Unit Count: 2
Compound Is Canonicalized: Yes

Physical state: powder
Color: colorless
Odor: odorless
Melting point/freezing point:
Melting point/range: 605 °C
Initial boiling point and boiling range: 1.360 °C at 1.013 hPa
Flammability (solid, gas): The product is not flammable.
Upper/lower flammability or explosive limits: No data available
Flash point: Not applicable
Autoignition temperature: No data available
Decomposition temperature: No data available
pH: ca.6 at 50 g/l at 20 °C
Viscosity
Viscosity, kinematic: No data available
Viscosity, dynamic: No data available

Water solubility: 569 g/l at 20 °C
Partition coefficient: n-octanol/water: Not applicable for inorganic substances
Vapor pressure: 1,33 hPa at 547 °C
Density: 2,07 g/cm3 at 20 °C
Relative density: No data available
Relative vapor density: No data available
Particle characteristics: No data available
Explosive properties: No data available
Oxidizing properties: none
Other safety information: No data available
LiCl: Lithium Chloride
Density: 2.07 g/cm³
Molecular Weight/ Molar Mass: 42.394 g/mol
Boiling Point: 1,382 °C
Melting Point: 605 °C
Chemical Formula: LiCl
Odour: Odourless

Appearance: White solid hygroscopic
Covalently-Bonded Unit: 2
Specific Gravity: 2.068 at 77 ° F
Complexity: 2
Solubility: Insoluble in water
CAS: 7447-41-8
MF: LiCl
MW: 42.39
EINECS: 231-212-3
Mol File: 7447-41-8.mol
Lithium chloride Chemical Properties:
Melting point: 605 °C(lit.)
Boiling point: 1382°C
density: 2.06
vapor pressure: 1.33 hPa (547 °C)
refractive index: n20/D 1.381
Fp: -4 °F
storage temp.: 2-8°C
solubility: H2O: soluble
form: beads
color: White to gray

Specific Gravity: 2.068
Odor: Odorless
PH: 5.5-7.5 (25℃, 50mg/mL in H2O)
PH Range: 6
Water Solubility: 832 g/L (20 ºC)
λmax: λ: 260 nm Amax: 0.01
λ: 280 nm Amax: 0.01
Sensitive: Hygroscopic
Merck: 145,528
Stability: Stable.
InChIKey: KWGKDLIKAYFUFQ-UHFFFAOYSA-M
CAS DataBase Reference: 7447-41-8(CAS DataBase Reference)
NIST Chemistry Reference: Lithium chloride(7447-41-8)
EPA Substance Registry System: Lithium chloride (7447-41-8)
Linear Formula: LiCl
UN Number: NONH for all modes of transport
Formula Weight: 42.39g/mol
Chemical Name or Material: Lithium Chloride



FIRST AID MEASURES of LITHIUM CHLORIDE:
-Description of first-aid measures:
*General advice:
Show this material safety data sheet to the doctor in attendance.
*If inhaled:
After inhalation:
Fresh air.
*In case of skin contact:
Take off immediately all contaminated clothing.
Rinse skin with water/ shower.
*In case of eye contact:
After eye contact:
Rinse out with plenty of water.
Call in ophthalmologist.
Remove contact lenses.
*If swallowed:
After swallowing:
Immediately make victim drink water (two glasses at most).
Consult a physician.
-Indication of any immediate medical attention and special treatment needed:
No data available



ACCIDENTAL RELEASE MEASURES of LITHIUM CHLORIDE:
-Environmental precautions:
Do not let product enter drains.
-Methods and materials for containment and cleaning up:
Cover drains.
Collect, bind, and pump off spills.
Observe possible material restrictions.
Take up dry.
Dispose of properly.
Clean up affected area.



FIRE FIGHTING MEASURES of LITHIUM CHLORIDE:
-Extinguishing media:
*Suitable extinguishing media:
Use extinguishing measures that are appropriate to local circumstances and the
surrounding environment.
*Unsuitable extinguishing media:
For this substance/mixture no limitations of extinguishing agents are given.
-Further information:
Suppress (knock down) gases/vapors/mists with a water spray jet.
Prevent fire extinguishing water from contaminating surface water or the ground water system.



EXPOSURE CONTROLS/PERSONAL PROTECTION of LITHIUM CHLORIDE:
-Exposure controls:
--Personal protective equipment:
*Eye/face protection:
Use equipment for eye protection.
Safety glasses
*Skin protection:
Full contact:
Material: Nitrile rubber
Minimum layer thickness: 0,11 mm
Break through time: 480 min
Splash contact:
Material: Nitrile rubber
Minimum layer thickness: 0,11 mm
Break through time: 480 min
*Body Protection:
protective clothing
*Respiratory protection:
Recommended Filter type: Filter type P2
-Control of environmental exposure:
Do not let product enter drains.



HANDLING and STORAGE of LITHIUM CHLORIDE:
-Conditions for safe storage, including any incompatibilities:
*Storage conditions:
Tightly closed.
Dry.
hygroscopic
*Storage class:
Storage class (TRGS 510): 13:
Non Combustible Solids



STABILITY and REACTIVITY of LITHIUM CHLORIDE:
-Reactivity:
No data available
-Chemical stability:
The product is chemically stable under standard ambient conditions (room temperature) .
-Conditions to avoid:
no information available
-Incompatible materials:
No data available

Lithium chloride is a chemical compound composed of lithium, a alkali metal, and chlorine, a halogen.
Lithium chloride is an ionic compound or salt that is highly polar and soluble in water.
Lithium chloride is more soluble in organic solvents such as acetone and methanol than potassium chloride or sodium chloride.

CAS Number: 7447-41-8
Molecular Formula: LiCl
Molecular Weight: 42.39
EINECS Number: 231-212-3

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Lithium chloride is widely used in several industrial applications.
Lithium chloride is a chemical compound with the formula LiCl.
The salt is a typical ionic compound (with certain covalent characteristics), although the small size of the Li+ ion gives rise to properties not seen for other alkali metal chlorides, such as extraordinary solubility in polar solvents (83.05 g/100 mL of water at 20 °C) and its hygroscopic properties.

Lithium chloride is produced by treatment of lithium carbonate with hydrochloric acid.
Anhydrous Lithium chloride is prepared from the hydrate by heating in a stream of hydrogen chloride.
Lithium chloride is mainly used for the production of lithium metal by electrolysis of a LiCl/KCl melt at 450 °C (842 °F).

Lithium chloride is also used as a brazing flux for aluminium in automobile parts.
Lithium chloride is used as a desiccant for drying air streams.
In more specialized applications, lithium chloride finds some use in organic synthesis, e.g., as an additive in the Stille reaction.

Also, in biochemical applications, Lithium chloride can be used to precipitate RNA from cellular extracts.
Lithium chloride is also used as a flame colorant to produce dark red flames.
Lithium Chloride has many applications.

Lithium chloride is extremely hygroscopic, and is widely used in dehumidification systems to remove moisture from the air in industries such as food processing and horticulture.
Lithium chloride is also used as a tracer for waste water, as a brazing flux, and as an electrolyte component for the manufacture of speciality batteries.
Lithium chloride is a white solid hygroscopic soluble in water, alcohol and ether.

The chemical formula for lithium chloride is Lithium chloride.
Lithium chloride is made by the action of hydrochloric acid on lithium hydroxide. The resulting solution is evaporated to get a mixture of saturated solution and lithium chloride crystals.
The solid and the solution is separated and the supernatant solution is recycled for further evaporation.

Lithium chloride is a solid which absorbs water to form a hydrate, LiCl.H2O
Lithium chloride is a white, crystalline solid at room temperature.
Lithium chloride has a high melting point of about 605 degrees Celsius (1,121 degrees Fahrenheit).

Lithium chloride is highly soluble in water, and its aqueous solution conducts electricity.
Lithium chloride is a White cubic crystals; granules or powder; hygroscopic; sharp salt-like taste; melts at 605°C; vaporizes around 1360°C, It has an unusually high water solubility when compared to the other alkali metal chlorides; readily dissolves in water (64g/100mL at 0°C); also highly soluble in alcohol and pyridine; moderately soluble in acetone (4.1 g/100mL at 25°C).
The following hydrates are known: LiCl·H2O, LiCl-3H20 and LiCl- 5H2O. The higher hydrates are stable at progressively lower temperatures.

Lithium chloride is deliquescent under normal atmospheric conditions.
Lithium chloride is soluble to a significant extent in many polar organic liquids.
Lithium chloride is generally most soluble in alcohols in which the solubility decreases as the size of the organic radical increases.

Lithium chloride dehumidifies air for industrial drying and for air conditioning.
Lithium chloride bums with a chrims on flame and is used in pyrotechnics.
Lithium chloride is also used as a pyrotechnic in welding and brazing fluxes.

Lithium chloride is a metal chloride salt with a Li(+) counterion.
Lithium chloride has a role as an antimanic drug and a geroprotector.
Lithium chloride is an inorganic chloride and a lithium salt.

Lithium Chloride is a chemical compound that is extremely soluble in polar solvents and is used in order to obtain lithium metal.
In organic synthesis it is used as an additive in the Stille Reaction. Ungraded products supplied by Spectrum are indicative of a grade suitable for general industrial use or research purposes and typically are not suitable for consumption.
Lithium chloride is a chemical compound with a chemical formula “LiCl”.

The salt is a normal ionic compound, although the Li+ ion is small in size, it produces unrecognized effects for other alkali metal chlorides, such as exceptional solubility in polar solvents and its hygroscopic properties.
Lithium chloride is an excellent water soluble crystalline Lithium source for uses compatible with Chlorides.
Lithium Chloride is generally immediately available in most volumes.

Lithium chloride compounds can conduct electricity when fused or dissolved in water.
Lithium chloride materials can be decomposed by electrolysis to chlorine gas and the metal.
They are formed through various chlorination processes whereby at least one chlorine anion (Cl-) is covalently bonded to the relevant metal or cation.

Ultra high purity and proprietary formulations can be prepared.
The chloride ion controls fluid equilibrium and pH levels in metabolic systems.
They can form either inorganic or organic compounds.

Lithium chloride Formula is a typical ionic compound and a salt of lithium.
Due to the small size of the lithium-ion ( Li+ ), it gives rise to properties that we cannot see in other alkali metal chlorides.
During the year the 1940s for a short while they produce Lithium chloride as a compound to replace common salt (Sodium Chloride NaCl).

Lithium chloride is used in absorption refrigeration and air conditioning systems.
In these systems, lithium chloride absorbs water vapor, and the resulting solution is then subjected to temperature changes to release the absorbed water, thus providing a cooling effect.
Lithium chloride has been used in the hydraulic fracturing (fracking) process in the oil and gas industry.

Lithium chloride is sometimes employed as a component in fluids used to prevent clay swelling and control shale stability.
Lithium chloride is utilized as a catalyst or co-catalyst in certain chemical reactions, particularly in organic synthesis and polymerization processes.
In the pharmaceutical industry, lithium chloride is used in the production of certain antibiotics and pharmaceutical compounds.

Lithium chloride can be employed in metal surface treatment processes, where it may play a role in enhancing the corrosion resistance of certain metals.
In analytical chemistry, lithium chloride can be used as a reagent or standard in specific testing procedures.
Lithium chloride is used as a drying agent for gases in some laboratory and industrial applications.

Lithium chloride has been investigated for its potential use in magnetic refrigeration systems, which is an alternative refrigeration technology that relies on the magnetocaloric effect.
In the development of molten salt batteries, lithium chloride may be used as an electrolyte component in certain designs.
Lithium chloride has historical significance in photography, where it was used in certain processes related to developing and fixing photographs.

Researchers may use lithium chloride in studies related to thermophysical properties, such as specific heat capacity and thermal conductivity.
Lithium chloride is used in some wood preservation treatments to protect wood from decay and insect infestation.
In certain designs of nuclear reactors, lithium chloride may be considered as a potential coolant due to its high boiling point.

Lithium chloride can be involved in hydrometallurgical processes for the extraction of metals from ores.
Lithium chloride is used in the textile industry for certain dyeing and finishing processes.
The salt forms crystalline hydrates, unlike the other alkali metal chlorides.

Mono-, tri-, and pentahydrates are known.
The anhydrous salt can be regenerated by heating the hydrates.
Lithium chloride also absorbs up to four equivalents of ammonia/mol.

As with any other ionic chloride, solutions of lithium chloride can serve as a source of chloride ion, e.g., forming a precipitate upon treatment with silver nitrate: LiCl + AgNO3 → AgCl + LiNO3
Lithium chloride reacts with an alkali (such as Sodium Hydroxide) to form Sodium Chloride and Lithium Hydroxide.
LiCl+NaOH→LiOH+NaCl

Like other metal chlorides, lithium chloride salt produces crystalline hydrates.
Besides, it can easily absorb four equivalents of ammonia per mol.
However, lithium chloride can mainly serve as a chloride ion source when combined with an ionic chloride.

Lithium chloride has been explored for its potential use in magnetic resonance imaging (MRI) contrast agents, as lithium ions exhibit interesting magnetic properties.
Lithium chloride is considered in some thermal energy storage systems, where it may be used as a component in phase change materials for storing and releasing thermal energy.
Lithium chloride finds applications in the dye industry, where it may be used in certain dyeing processes.

In analytical chemistry, lithium chloride can be used as a reagent for specific tests and analyses, particularly in the determination of certain ions.
Lithium chloride is used in the Kjeldahl method for the determination of nitrogen content in organic compounds.
Lithium chloride can be involved in the synthesis of certain phosphors, which are materials that emit light when exposed to radiation.

Lithium chloride has been studied for its potential use in cryopreservation processes, where it may contribute to the preservation of biological samples at very low temperatures.
In metallurgy, lithium chloride can be used in heat treatment processes for certain metals, contributing to desired changes in the material properties.

Lithium chloride is known for producing a crimson flame color when burned.
This property is sometimes used in flame tests to identify the presence of lithium ions.

Melting point: 605 °C (lit.)
Boiling point: 1383 °C/1 atm (lit.)
Density: 2.06
vapor pressure: 1.33 hPa (547 °C)
refractive index: n20/D 1.381
Flash point: -4 °F
storage temp.: 2-8°C
solubility: H2O: soluble
form: beads
pka: 2.256[at 20 ℃]
Specific Gravity: 2.068
color: White to gray
PH: 5.5-7.5 (25℃, 50mg/mL in H2O)
Odor: Odorless
PH Range: 6
Water Solubility: 832 g/L (20 ºC)
Sensitive: Hygroscopic
λmax.λ: 260 nm Amax: 0.01
λ: 280 nm Amax: 0.01
Merck: 14,5528
Stability: Stable. Incompatible with strong oxidizing agents, strong acids, bromine trichloride, bromine trifluoride. Very hygroscopic. Protect from moisture.
InChIKey: KWGKDLIKAYFUFQ-UHFFFAOYSA-M
LogP: -1

These materials have weak oxidizing or reducing powers.
Redox reactions can however still occur.
For example, CO2, which is often regarded as chemically inert, vigorously oxidizes the strong reducing agent Mg if the two are heated together.

The majority of compounds in this class are slightly soluble or insoluble in water.
If soluble in water, then the solutions are usually neither strongly acidic nor strongly basic.
Lithium chlorides are not water-reactive.

Carbonates generate carbon dioxide and heat when treated with acids; fluorides, sulfites and sulfides generate toxic gases (hydrogen fluoride, sulfur dioxide and hydrogen sulfide, respectively) when treated with acids.
Lithium chloride has the ability to block glycogen synthase kinase (GSK).
Lithium chloride may also possess anti-inflammatory effects at low and non-toxic concentrations.

Lithium chloride salts affect the central nervous system in a variety of ways.
While the citrate, carbonate, and orotate salts are currently used to treat bipolar disorder, other lithium salts including the chloride were used in the past.
For a short time in the 1940s lithium chloride was manufactured as a salt substitute for people with hypertension, but this was prohibited after the toxic effects of the compound (tremors, fatigue, nausea) were recognized.

Lithium chloride was, however, noted by J. H. Talbott that many symptoms attributed to lithium chloride toxicity may have also been attributable to sodium chloride deficiency, to the diuretics often administered to patients who were given lithium chloride, or to the patients' underlying conditions.
Lithium chloride is a chemical compound with the formula LiCl.
The salt is a typical ionic compound, although the small size of the Li+ ion gives rise to properties not seen for other alkali metal chlorides, such as extraordinary solubility in polar solvents (83.05 g/100 mL of water at 20 °C) and its hygroscopic properties.

Lithium chloride has been investigated as a potential electrolyte material in certain types of fuel cells, where it could play a role in ion conduction.
Lithium chloride is involved in the hydrometallurgical extraction of lithium from lithium-bearing ores, where it plays a role in separating lithium from other elements.
Lithium chloride is not used directly as a food additive, but lithium compounds are sometimes used in trace amounts in certain food and beverage products.

Lithium chloride can be used in the synthesis of certain metal hydrides, which are compounds of metal and hydrogen.
In the glass industry, lithium chloride may be used in specific glass formulations to impart certain properties.
Lithium chloride is utilized as a component in some welding flux formulations, aiding in the removal of impurities during welding processes.

Lithium chloride is sometimes used in the oil and gas industry for applications such as drilling fluids and well completion fluids.
Lithium chloride is used in dental alginate impression materials, which are commonly used in dentistry to create molds of teeth and surrounding structures.
Lithium chloride is employed in some studies and experiments related to seed germination and plant growth.

Lithium chloride may influence the germination process under certain conditions.
Lithium chloride is a precursor in the production of metallic lithium.
Through processes like electrolysis, lithium metal can be obtained from lithium chloride.

In soil science, lithium chloride is sometimes used as a tracer element for studying the movement and behavior of water in soil profiles.
Lithium chloride is used in the construction of heat pipes, which are devices that transfer heat efficiently from one point to another.
Lithium chloride is utilized in some soldering flux formulations, aiding in the soldering process by removing oxides from metal surfaces.

Lithium chloride has been studied for potential applications in photovoltaic cells and solar energy systems.
In historical photography processes, lithium chloride was used in certain developing solutions.
Lithium chloride has been investigated for its potential use in hydrogen storage systems, which is crucial for various hydrogen-based energy applications.

Lithium chloride is used in some antifreeze mixtures, contributing to the lowering of the freezing point of solutions.
Lithium chloride can be used in certain formulations in the cement and concrete industry to improve certain properties of the materials.
In the production of magnesium metal, lithium chloride may be used as a flux to remove impurities during the refining process.

Lithium chloride is employed as a catalyst or co-catalyst in various organic synthesis reactions, facilitating specific chemical transformations.
In some water treatment processes, lithium chloride is used for specific applications, such as controlling algae growth in water systems.
Lithium chloride has been studied for its potential use in nuclear waste treatment processes, particularly in separating certain elements from radioactive waste streams.

Lithium chloride is used in some surface treatment processes in metalworking to enhance the properties of metal surfaces.
In semiconductor manufacturing, lithium chloride may be used in specific processes related to the production of electronic components.
Lithium chloride has been considered in the development of lithium-air batteries, a type of battery technology with high energy density.

Lithium chloride is used in chlorination reactions, where it may act as a source of chlorine atoms for specific chemical transformations.
Lithium metal is produced by electrolysis of lithium chloride and potassium chloride, which melts at 450°C.
High-purity lithium chloride is used as the feedstock in the process and makes about 99.5% pure lithium metal.

Molten Lithium chloride is contained in a carbon steel pot, while the chlorine gas is collected in a stainless steel or glass pipe for applications in other processes.
The molten lithium flows into a collecting tank and is later cast into ingots.
A mesh or stainless-steel screen separates the two compartments to prevent the products from mixing.

Preparation:
Lithium chloride may be prepared by reaction of lithium carbonate or lithium hydroxide with hydrochloric acid followed by crystallization: Li2CO3+ 2HCl →2LiCl + CO2+ H2O
LiOH + HCl →LiCl + H2O
Crystallization above 95°C yields anhydrous salt.

Hot solution upon cooling forms crystals of monohydrate, LiCl.H2O.
The solid and solution are separated and the supernatant solution is recycled for further evaporation.
The crystals are dried to yield anhydrous lithium chloride.

Lithium chloride can be synthesized from its elements by heating lithium metal with chlorine gas.
Lithium chloride also may be obtained from natural brine.

Uses:
Lithium chloride is useful for the production of lithium metal, and for the generation of Mn(0) species which can be used in free radical cyclizations.
Lithium chloride can serve as a flame colorant to generate dark red flames, a brazing flux for aluminum in automobiles, a hygrometer, and a desiccant for drying air streams.
On exposure to air, it becomes a solution with the concentration directly related to relative humidity of the atmosphere, and hence serves as a relative humidity standard in calibrating hygrometers.

Apart from being a source of Lithium chloride, it serves as an additive in the Stille reaction in organic synthesis, and to precipitate RNA from cellular extracts.
Being biologically significant, it finds applications in a wide variety of assays to study cell-fate and neurobiology.
Lithium chloride has been found to inhibit virus infection.

Lithium chloride solutions are used in large dehumidification systems in the air-conditioning industry.
This use depends on the low equilibrium pressure of water vapor above solutions of lithium chloride.
After the solutions have absorbed water, they are regenerated by heating.

Lithium chloride is used in a number of salt mixtures.
Such salt mixtures have low melting points allowing the material to be used in brazing fluxes and brazing baths.
The molten lithium chloride-potassium chloride eutectic mixture can be used as an electrolyte.

The mixture is electrolyzed for the production of lithium metal and is used as an electrolyte in voltaic cells.
Lithium chloride is also used in manufacture of mineral waters; in pyrotechnics; soldering aluminum; in refrigerating machines.
Lithium chloride is used as a flame colorant to form dark crimson flames.

Lithium chloride is used in the precipitation of RNA in biological applications.
Lithium chloride is an aluminum blazing flux in automobile parts.
Lithium chloride is commonly used as a desiccant in air conditioning systems to absorb moisture and control humidity.

Lithium chloride is utilized in absorption refrigeration systems where it helps absorb water vapor, contributing to the cooling process.
Lithium chloride is employed in dental alginate impression materials, crucial in dentistry for creating molds of teeth and oral structures.
Lithium chloride is used in scientific studies and experiments related to seed germination and plant growth.

Lithium chloride applied in drilling fluids and well completion fluids in the oil and gas industry.
Lithium chloride is used as a component in fluids for hydraulic fracturing processes.
Lithium chloride utilized in the construction of heat pipes for efficient heat transfer.

Investigated for potential applications in photovoltaic cells and solar energy systems.
Considered in certain designs of nuclear reactors as a potential coolant.
Lithium chloride used in chemical and pharmaceutical processes, including the synthesis of lithium compounds and pharmaceutical products.

Precursor in the production of metallic lithium through processes like electrolysis.
Employed as a catalyst or co-catalyst in various organic synthesis reactions.
Lithium chloride is used in molecular biology for the precipitation of DNA and RNA from solution.

Involved in the extraction of metals from ores through hydrometallurgical processes.
Lithium chloride is used in certain formulations to improve properties of cement and concrete.
Lithium chloride is used in some antifreeze mixtures to lower the freezing point of solutions.

Lithium chloride applied in certain water treatment processes for controlling algae growth.
Lithium chloride is used in metal surface treatment processes to enhance corrosion resistance.
Lithium chloride produces a crimson flame color when burned, used in flame tests for identifying lithium ions.

Investigated for potential use in lithium-air batteries, a high-energy-density battery technology.
Lithium chloride is used as a tracer element in soil science to study water movement in soil profiles.
Lithium chloride is used in heat treatment processes for certain metals to achieve desired material properties.

Lithium chloride utilized in some welding flux formulations to aid in the soldering process.
Lithium chloride is used as a reagent in analytical chemistry for specific tests and analyses.
Explored for potential use in MRI contrast agents due to interesting magnetic properties.

Lithium chloride is used for several soldering and welding techniques and salt bath heat treatment at low temperatures.
Lithium chloride is used in massive dehumidification systems in the AC industry.
This depends on the low equilibrium pressure of vapor above lithium chloride solutions.

Lithium chloride is used as a relative humidity standard in the calibration of hygrometers.
Additionally, lithium chloride can be used as a hygrometer.
This deliquescent salt forms a self-solution when exposed to air.

The equilibrium LiCl concentration in the resulting solution is directly related to the relative humidity of the air.
The percent relative humidity at 25 °C (77 °F) can be estimated, with minimal error in the range 10–30 °C (50–86 °F), from the following first-order equation: RH=107.93-2.11C, where C is solution LiCl concentration, percent by mass.
Lithium chloride is used for the preparation of carbon nanotubes, graphene[10] and lithium niobate.

Lithium chloride has been shown to have strong acaricidal properties, being effective against Varroa destructor in populations of honey bees.
Lithium chloride is used as an aversive agent in lab animals to study conditioned place preference and aversion.
Lithium chloride is used in the following products: laboratory chemicals, pH regulators and water treatment products, metal working fluids, pharmaceuticals, polymers, water treatment chemicals and welding & soldering products.

Lithium chloride is used in the following areas: scientific research and development and health services.
Lithium chloride is used for the manufacture of: chemicals and plastic products.
Other release to the environment of Lithium chloride is likely to occur from: indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners), outdoor use, indoor use in close systems with minimal release (e.g. cooling liquids in refrigerators, oil-based electric heaters), outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids), outdoor use in long-life materials with low release rate (e.g. metal, wooden and plastic construction and building materials) and indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment).

Lithium chloride is used in the following products: pharmaceuticals, air care products, inks and toners, laboratory chemicals, metal working fluids, paper chemicals and dyes, polymers, water treatment chemicals and welding & soldering products.
Release to the environment of Lithium chloride can occur from industrial use: formulation of mixtures and formulation in materials.
Lithium chloride is used in the following products: welding & soldering products, laboratory chemicals, air care products, inks and toners, pH regulators and water treatment products, metal working fluids, pharmaceuticals, polymers and water treatment chemicals.

Lithium chloride is used in the following areas: scientific research and development and health services.
Lithium chloride is used for the manufacture of: chemicals, plastic products and pulp, paper and paper products.
Release to the environment of Lithium chloride can occur from industrial use: in processing aids at industrial sites, as an intermediate step in further manufacturing of another substance (use of intermediates), as processing aid, of substances in closed systems with minimal release and in the production of articles.

Lithium chloride is used as a flux in the production of magnesium metal to remove impurities during the refining process.
Studied for potential use in cryopreservation processes, contributing to the preservation of biological samples at very low temperatures.
Investigated as a potential electrolyte material in certain types of fuel cells, contributing to ion conduction.

Studied for potential use in nuclear waste treatment processes, particularly in separating certain elements from radioactive waste streams.
Lithium chloride is used in surface treatment processes in metalworking to enhance the properties of metal surfaces.
Lithium chloride is used in semiconductor manufacturing for specific processes related to the production of electronic components.

Lithium chloride is used in chlorination reactions, where it may act as a source of chlorine atoms for specific chemical transformations.
Historically used in certain developing solutions in photography processes.
Lithium chloride is used in the heat treatment of certain alloys to achieve specific material properties.

Employed in metal plating processes to improve the surface properties of metals.
Studied for potential agricultural applications, including the enhancement of plant growth under specific conditions.
Lithium chloride is used in certain formulations in the glass industry to improve certain properties of the materials.

While lithium chloride itself is not typically used in lithium-ion batteries, it is part of the broader lithium supply chain, contributing to lithium compounds used in battery manufacturing.
Investigated for potential use in molten salt batteries, where it may contribute to the electrolyte formulation.
Lithium chloride is used in geochemical studies for specific chemical analyses and experiments.

Studied for potential use in magnetic refrigeration systems, which rely on the magnetocaloric effect for cooling.
Lithium chloride is used in the synthesis of certain metal hydrides, compounds of metal and hydrogen.
Lithium chloride utilized as a catalyst in amidation reactions, contributing to the formation of amide bonds.

Investigated for potential use as an electrolyte component in lithium-air batteries.
Lithium chloride is used in gas absorption systems for selective removal of gases from mixtures.
Lithium chloride applied in crystal growth processes for specific applications in materials science.

Explored for potential use in the growth of certain laser crystals.
Involved in the hydrometallurgical recovery of certain metals from various sources.
Considered for potential use in lithium-ion capacitors, an energy storage technology.

Lithium chloride utilized in the production of certain ion exchange resins used in water treatment.
Lithium Chloride is used as an electrolyte for low temperature dry battery cells and as an oxidation catalyst.
Lithium chloride is a solubilizer for polyamides and cellulose when used with amide solvents, and is a chlorinating agent for steroid substrates.

Lithium chloride is used in large dehumidification systems in the air conditioning industry.
Lithium chloride depends on the low equilibrium pressure of water vapour above solutions of lithium chloride.
Lithium chloride is used in a number of salt mixtures exist low melting points allowing the material to be used in brazing fluxes and brazing baths.

Lithium chloride is used as an electrolyte for the production of lithium metal and used as an electrolyte in voltaic cells.
Lithium chloride is used for the production of lithium metal, by electrolysis of a LiCl/KCl melt at 450 °C.
Lithium chloride is also used as a brazing flux for aluminium in automobile parts.

Lithium chloride can be used to improve the efficiency of the Stille reaction. Its desiccant properties can be used to generate potable water by absorbing moisture from the air, which is then released by heating the salt.
For a short time in the 1940s lithium chloride was manufactured as a substitute for salt, but this was prohibited after the toxic effects of the compound were recognised.
Lithium chloride is often used as a desiccant (drying agent) in air conditioning systems and industrial drying processes.

Lithium chloride has a high affinity for water and can absorb moisture from the air.
Lithium chloride is used in certain chemical and pharmaceutical processes, including the synthesis of lithium compounds and pharmaceutical products.
Lithium chloride is considered as a potential material for use in molten salt reactors, which are a type of advanced nuclear reactor design.

Lithium chloride is a key starting material in the production of metallic lithium through processes such as electrolysis.
While lithium chloride is not commonly used as an electrolyte in batteries, it is a source of lithium, a crucial component in lithium-ion batteries.
Lithium chloride is used in laboratories as a reagent in certain chemical reactions and experiments.

In molecular biology, lithium chloride is used for the precipitation of DNA and RNA from solution, aiding in their isolation and purification.
Lithium chloride is used as a flux in metallurgical processes, helping to lower the melting point of metal oxides during the production of certain metals.

Lithium chloride is used in some types of fire extinguishing agents.
Due to its hygroscopic nature (ability to absorb moisture), lithium chloride is used in humidity control systems and certain industrial processes where water needs to be removed.

Safety Profile:
Human poison by ingestion.
Lithium chloride experimental poison by intravenous and intracerebral routes.
Lithium chloride moderately toxic by subcutaneous and intraperitoneal routes.

Experimental teratogenic and reproductive effects.
Human systemic effects by ingestion: somnolence, tremors, nausea or vomiting.
An eye and severe skin irritant.

Questionable carcinogen with experimental neoplastigenic data.
This material has been recommended and used as a substitute for sodwm chloride in "saltfree" diets, but cases have been reported in which the ingestion of lithium chloride has produced dminess, ringing in the ears, visual disturbances, tremors, and mental confusion.
In most cases, the symptoms disappeared when use was discontinued.

Prolonged absorption may cause disturbed electrolyte balance, impaired renal function.
When heated to decomposition it emits toxic fumes of Cl-.
Lithium chloride is used for dehumidification in the air conditioning industry.

Lithium chloride is a chemical compound with the formula LiCl.
Lithium chloride is a typical ionic compound (with certain covalent characteristics), although the small size of the Li+ ion gives rise to properties not seen for other alkali metal chlorides, such as extraordinary solubility in polar solvents (83.05 g/100 mL of water at 20 °C) and its hygroscopic properties.
Lithium chloride forms crystalline hydrates, unlike the other alkali metal chlorides.

CAS: 7447-41-8
MF: LiCl
MW: 42.39
EINECS: 231-212-3

A metal chloride salt with a Li(+) counterion.
Lithium Chloride has many applications.
It is extremely hygroscopic, and is widely used in dehumidification systems to remove moisture from the air in industries such as food processing and horticulture.
It is also used as a tracer for waste water, as a brazing flux, and as an electrolyte component for the manufacture of speciality batteries.

Lithium chloride Chemical Properties
Melting point: 605 °C (lit.)
Boiling point: 1383 °C/1 atm (lit.)
Density: 2.06
Vapor pressure: 1.33 hPa (547 °C)
Refractive index: n20/D 1.381
Fp: -4 °F
Storage temp.: 2-8°C
Solubility H2O: soluble
Form: beads
Pka: 2.256[at 20 ℃]
Specific Gravity: 2.068
Color: White to gray
PH: 5.5-7.5 (25℃, 50mg/mL in H2O)
Odor: Odorless
PH Range: 6
Water Solubility: 832 g/L (20 ºC)
Sensitive: Hygroscopic
λmax λ: 260 nm Amax: 0.01
λ: 280 nm Amax: 0.01
Merck: 14,5528
Stability: Stable. Incompatible with strong oxidizing agents, strong acids, bromine trichloride, bromine trifluoride. Very hygroscopic. Protect from moisture.
InChIKey: KWGKDLIKAYFUFQ-UHFFFAOYSA-M
LogP: -1
CAS DataBase Reference: 7447-41-8(CAS DataBase Reference)
NIST Chemistry Reference: Lithium chloride(7447-41-8)
EPA Substance Registry System: Lithium chloride (7447-41-8)

Mono-, tri-, and pentahydrates are known.
The anhydrous salt can be regenerated by heating the hydrates.
Lithium chloride also absorbs up to four equivalents of ammonia/mol.
As with any other ionic chloride, solutions of lithium chloride can serve as a source of chloride ion, e.g., forming a precipitate upon treatment with silver nitrate:
LiCl + AgNO3 → AgCl + LiNO3

Lithium chloride is a White cubic crystals; granules or powder; hygroscopic; sharp salt-like taste; melts at 605°C; vaporizes around 1360°C, Lithium chloride has an unusually high water solubility when compared to the other alkali metal chlorides; readily dissolves in water (64g/100mL at 0°C); also highly soluble in alcohol and pyridine; moderately soluble in acetone (4.1 g/100mL at 25°C).
The following hydrates are known: LiCl·H2O, LiCl-3H20 and LiCl- 5H2O.
The higher hydrates are stable at progressively lower temperatures.
Lithium chloride is deliquescent under normal atmospheric conditions.
Lithium chloride is soluble to a significant extent in many polar organic liquids.
Lithium chloride is generally most soluble in alcohols in which the solubility decreases as the size of the organic radical increases.
Lithium chloride dehumidifies air for industrial drying and for air conditioning.
Lithium chloride bums with a chrims on flame and is used in pyrotechnics.
Lithium chloride is also used as a pyrotechnic in welding and brazing fluxes.

Lithium Chloride Anhydrous is known by the name of 7447-41-8, Lithium chloride, Chlorku litu, as chlorure de lithium, Lithium chloride (LiCl), LiCl, CHEBI:48607, choro lithium, Lithium chloride and has Molecular Formula of ClLi with Molecular Weight of 42.394.
Lithium chloride is manufactured through reaction of lithium hydroxide/ lithium carbonate with a hydrochloric acid and can be extracted from other alkali-metal chlorides using amyl alcohol.

Having form of deliquescent, cubic crystals in granules or as crystalline powder, white cubic crystals or powder form, Lithium chloride has a sharp saline taste with boiling point of 1383°C and melting point of 610°C.
Lithium chloride's other properties include Density/Specific Gravity of 2.07 g/cu cm, neutral or slightly alkaline pH and solubility of 84.5 g/100 g water at 25°C; soluble in ethanol, acetone, pyridine as well a s in water alcohols, ether, pyridine, nitrobenzene.

Physical properties
White cubic crystals; granules or powder; hygroscopic; sharp salt-like taste; refractive index 1.662; density 2.068 g/cm3; melts at 605°C; vaporizes around 1,360°C; readily dissolves in water (64g/100mL at 0°C); also highly soluble in alcohol and pyridine; moderately soluble in acetone (4.1 g/100mL at 25°C).

Uses
Lithium chloride is mainly used for the production of lithium metal by electrolysis of a LiCl/KCl melt at 450 °C (842 °F).
Lithium chloride is also used as a brazing flux for aluminium in automobile parts.
Lithium chloride is used as a desiccant for drying air streams.
In more specialized applications, lithium chloride finds some use in organic synthesis, e.g., as an additive in the Stille reaction.
Also, in biochemical applications, Lithium chloride can be used to precipitate RNA from cellular extracts.
Lithium chloride is also used as a flame colorant to produce dark red flames.

Lithium chloride is useful for the production of lithium metal, and for the generation of Mn(0) species which can be used in free radical cyclizations.
Lithium chloride can serve as a flame colorant to generate dark red flames, a brazing flux for aluminum in automobiles, a hygrometer, and a desiccant for drying air streams.
On exposure to air, Lithium chloride becomes a solution with the concentration directly related to relative humidity of the atmosphere, and hence serves as a relative humidity standard in calibrating hygrometers.
Apart from being a source of chloride, Lithium chloride serves as an additive in the Stille reaction in organic synthesis, and to precipitate RNA from cellular extracts.
Being biologically significant, Lithium chloride finds applications in a wide variety of assays to study cell-fate and neurobiology.
Lithium chloride has been found to inhibit virus infection.
Lithium chloride is used as an antidepressant, especially in the treatment of manic depression and bipolar disorders.

Lithium chloride solutions are used in large dehumidification systems in the air-conditioning industry.
Lithium chloride use depends on the low equilibrium pressure of water vapor above solutions of lithium chloride.
After the solutions have absorbed water, they are regenerated by heating.
Lithium chloride is used in a number of salt mixtures.
Such salt mixtures have low melting points allowing the material to be used in brazing fluxes and brazing baths.
The molten lithium chloride-potassium chloride eutectic mixture can be used as an electrolyte.
The mixture is electrolyzed for the production of lithium metal and is used as an electrolyte in voltaic cells.
Manufacture of mineral waters; in pyrotechnics; soldering aluminum; in refrigerating machines.

Niche uses
Lithium chloride is used as a relative humidity standard in the calibration of hygrometers.
At 25 °C (77 °F) a saturated solution (45.8%) of the salt will yield an equilibrium relative humidity of 11.30%.
Additionally, lithium chloride can be used as a hygrometer.
This deliquescent salt forms a self-solution when exposed to air.
The equilibrium Lithium chloride concentration in the resulting solution is directly related to the relative humidity of the air.
The percent relative humidity at 25 °C (77 °F) can be estimated, with minimal error in the range 10–30 °C (50–86 °F), from the following first-order equation: RH=107.93-2.11C, where C is solution Lithium chloride concentration, percent by mass.

Molten Lithium chloride is used for the preparation of carbon nanotubes, graphene and lithium niobate.
Lithium chloride has been shown to have strong acaricidal properties, being effective against Varroa destructor in populations of honey bees.
Lithium chloride is used as an aversive agent in lab animals to study conditioned place preference and aversion.

Preparation
Lithium chloride is produced by treatment of lithium carbonate with hydrochloric acid. Anhydrous Lithium chloride is prepared from the hydrate by heating in a stream of hydrogen chloride.

Lithium chloride may be prepared by reaction of lithium carbonate or lithium hydroxide with hydrochloric acid followed by crystallization:
(1) Li2CO3+ 2HCl →2LiCl + CO2+ H2O
(2) LiOH + HCl →LiCl + H2O
Crystallization above 95°C yields anhydrous salt. Hot solution upon cooling forms crystals of monohydrate, LiCl.H2O.
The solid and solution are separated and the supernatant solution is recycled for further evaporation.
The crystals are dried to yield anhydrous lithium chloride.
Lithium chloride can be synthesized from its elements by heating lithium metal with chlorine gas.
Lithium chloride also may be obtained from natural brine.

Reactivity Profile
These materials have weak oxidizing or reducing powers.
Redox reactions can however still occur.
For example, CO2, which is often regarded as chemically inert, vigorously oxidizes the strong reducing agent Mg if the two are heated together.
The majority of compounds in this class are slightly soluble or insoluble in water.
If soluble in water, then the solutions are usually neither strongly acidic nor strongly basic.

These compounds are not water-reactive.
Some do react with acids: carbonates generate carbon dioxide and heat when treated with acids; fluorides, sulfites and sulfides generate toxic gases (hydrogen fluoride, sulfur dioxide and hydrogen sulfide, respectively) when treated with acids.

Biochem/physiol Actions
Lithium chloride has the ability to block glycogen synthase kinase (GSK).
Lithium chloride may also possess anti-inflammatory effects at low and non-toxic concentrations.

Synonyms
LITHIUM CHLORIDE
7447-41-8
LiCl
Lithiumchloride
chlorure de lithium
Chlorku litu
chlorolithium
Lithiumchlorid
Lithium chloride (LiCl)
lithium;chloride
ClLi
Chlorku litu [Polish]
CCRIS 5924
CHEBI:48607
lithii chloridum
HSDB 4281
Luthium chloride
Lithium Cholride
cloruro de litio
Lithium chloride (powder)
EINECS 231-212-3
MFCD00011078
Chlorure de lithium [French]
NSC 327172
UNII-G4962QA067
LITHIUM MURIATICUM
G4962QA067
NSC-327172
LithiumChlorideGr(Anhydrous)
CHEMBL69710
DTXSID2025509
EC 231-212-3
NSC327172
Lithium Chloride, Anhydrous
Lithium chloride, ultra dry
Chloride, Lithium
2M Lithium Chloride Electrolyte, Electrode Filling Solution
Lithium Chloride (2.3% in Tetrahydrofuran, ca. 0.5mol/L)
lithim chloride
Lithium chloride, anhydrous, chunks, 99.99% trace metals basis
Cloruro de litio (licl)
Lopac-L-4408
LITHIUM MONOCHLORIDE
D07WXT
MolMap_000071
WLN: LI G
Lithium chloride, ACS grade
Lopac0_000604
LITHIUM CHLORIDE [MI]
Lithium chloride battery grade
Lithium chloride, ACS reagent
DTXCID105509
LITHIUM CHLORIDE [HSDB]
LITHIUM CHLORIDE [INCI]
LITHIUM MURIATICUM [HPUS]
KWGKDLIKAYFUFQ-UHFFFAOYSA-M
LITHIUM CHLORIDE [WHO-DD]
Lithium chloride, 3-5% in THF
HMS3261J10
Tox21_500604
BDBM50494542
AKOS015902822
AKOS015950647
AKOS024438070
CCG-204693
lithium chloride, gamma irradiated, 8m
LP00604
LS-1644
SDCCGSBI-0050586.P002
Lithium chloride, ACS reagent, >=99%
Lithium chloride, ReagentPlus(R), 99%
NCGC00015607-01
NCGC00015607-02
NCGC00015607-03
NCGC00015607-04
NCGC00015607-07
NCGC00093980-01
NCGC00093980-02
NCGC00261289-01
BP-13612
SY002997
Lithium chloride, Vetec(TM) reagent grade
EU-0100604
FT-0627896
L0204
L0222
Lithium chloride, Trace metals grade 99.9%
L 4408
Lithium chloride, SAJ first grade, >=98.0%
Lithium chloride, for molecular biology, >=99%
Lithium chloride, SAJ special grade, >=99.0%
A838146
Lithium chloride, BioXtra, >=99.0% (titration)
Q422930
SR-01000076252
SR-01000076252-1
Lithium chloride, powder, >=99.99% trace metals basis
Lithium chloride, puriss. p.a., anhydrous, >=99.0% (AT)
Lithium chloride, anhydrous, beads, -10 mesh, >=99.9% trace metals basis
Lithium chloride, anhydrous, beads, -10 mesh, 99.998% trace metals basis
Lithium chloride, puriss. p.a., ACS reagent, anhydrous, >=99.0% (AT)
Lithium chloride, anhydrous, free-flowing, Redi-Dri(TM), ACS reagent, >=99%
Lithium chloride, anhydrous, free-flowing, Redi-Dri(TM), ReagentPlus(R), 99%
Lithium chloride, BioUltra, for molecular biology, anhydrous, >=99.0% (AT)
59217-69-5

LITHIUM HYDROXIDE; lithium hydrate; Lithium Hydroxide hydrate; Lithiumhydroxid (German); Hidróxido de litio (Spanish); Hydroxyde de lithium cas no: 1310-65-2

Lithium Chloride (LiCl) is an excellent water soluble crystalline Lithium source for uses compatible with Chlorides.
Lithium Chloride (LiCl) is more soluble in polar organic solvents such as methanol and acetone than is sodium chloride or potassium chloride.


CAS Number: 7447-41-8
EC Number: 231-212-3
MDL number: MFCD00011078
Chemical formula: LiCl



SYNONYMS:
lithium chloride, lithium chloride licl, lithiumchloride, licl, chlorure de lithium, chlorku litu, chlorolithium, lithiumchlorid, chlorku litu polish, luthium chloride, Lithium chloride, Lithium(1+) chloride, LITHIUM CHLORIDE, 7447-41-8, LiCl, Lithiumchloride, chlorure de lithium, chlorolithium, Lithiumchlorid, Lithium chloride (LiCl), lithium;chloride, CCRIS 5924, CHEBI:48607, lithii chloridum, HSDB 4281, Lithium Cholride, cloruro de litio, Lithium chloride (powder), EINECS 231-212-3, MFCD00011078, NSC 327172, UNII-G4962QA067, LITHIUM MURIATICUM, G4962QA067, NSC-327172, Lithium Chloride, Anhydrous, LithiumChlorideG (Anhydrous), CHEMBL69710, DTXSID2025509, EC 231-212-3, NSC327172, Lithium chloride, ultra dry, Luthium chloride, Chloride, Lithium, Lithium Chloride (2.3% in Tetrahydrofuran, ca. 0.5mol/L), lithim chloride, Lopac-L-4408, LITHIUM MONOCHLORIDE, MolMap_000071, WLN: LI G, Lithium chloride, ACS grade, Lopac0_000604, LITHIUM CHLORIDE [MI], Lithium chloride battery grade, Lithium chloride, ACS reagent, DTXCID105509, LITHIUM CHLORIDE [HSDB], LITHIUM CHLORIDE [INCI], LITHIUM MURIATICUM [HPUS], KWGKDLIKAYFUFQ-UHFFFAOYSA-M, LITHIUM CHLORIDE [WHO-DD], Lithium chloride, 3-5% in THF, HMS3261J10, Tox21_500604, BDBM50494542, AKOS015902822, AKOS015950647, AKOS024438070, CCG-204693, lithium chloride, gamma irradiated, 8m, LP00604, SDCCGSBI-0050586.P002, Lithium chloride, ACS reagent, >=99%, Lithium chloride, ReagentPlus(R), 99%, NCGC00015607-01, NCGC00015607-02, NCGC00015607-03, NCGC00015607-04, NCGC00015607-07, NCGC00093980-01, NCGC00093980-02, NCGC00261289-01, BP-13612, SY002997, Lithium chloride, Vetec(TM) reagent grade, EU-0100604, FT-0627896, L0204, L0222, Lithium chloride, Trace metals grade 99.9%, L 4408, Lithium chloride, SAJ first grade, >=98.0%, Lithium chloride, for molecular biology, >=99%, Lithium chloride, SAJ special grade, >=99.0%, A838146, Lithium chloride, BioXtra, >=99.0% (titration), Q422930, SR-01000076252, SR-01000076252-1, Lithium chloride, powder, >=99.99% trace metals basis, Lithium chloride, puriss. p.a., anhydrous, >=99.0% (AT), Lithium chloride, anhydrous, beads, -10 mesh, >=99.9% trace metals basis, Lithium chloride, anhydrous, beads, -10 mesh, 99.998% trace metals basis, Lithium chloride, puriss. p.a., ACS reagent, anhydrous, >=99.0% (AT), Lithium chloride, anhydrous, free-flowing, Redi-Dri(TM), ACS reagent, >=99%, Lithium chloride, anhydrous, free-flowing, Redi-Dri(TM), ReagentPlus(R), 99%, Lithium chloride, BioUltra, for molecular biology, anhydrous, >=99.0% (AT), 59217-69-5, Hydrochloric acid lithium salt, lithium chloride, lithium chloride licl, lithiumchloride, licl, chlorure de lithium, chlorku litu, chlorolithium, lithiumchlorid, chlorku litu polish, luthium chloride, lithium chloride, lithium chloride licl, lithiumchloride, licl, chlorure de lithium, chlorku litu, chlorolithium, lithiumchlorid, chlorku litu polish, luthium chloride, lithium chloride, acs, lithium chloride, ultra dry, lithium ion standard solution, LITHIUMCHLORIDE,CRYSTAL,REAGENT, ACS, LITHIUMCHLORIDE, POWDER, REAGENT, ACS, Lithiumchlorid, Lithium Chloride (LiCl), Lithium(1+) chloride, LITHIUM CHLORIDE (LICL), 7447-41-8, LiCl, Lithiumchloride, chlorure de lithium, chlorolithium, Lithiumchlorid, Lithium Chloride (LiCl) (LiCl), lithium;chloride, CCRIS 5924, CHEBI:48607, lithii chloridum, HSDB 4281, Lithium Cholride, cloruro de litio, Lithium Chloride (LiCl) (powder), EINECS 231-212-3, MFCD00011078, NSC 327172, UNII-G4962QA067, LITHIUM MURIATICUM, G4962QA067, NSC-327172, Lithium Chloride (LiCl), Anhydrous, LithiumChlorideG (Anhydrous), CHEMBL69710, DTXSID2025509, EC 231-212-3, NSC327172, Lithium Chloride (LiCl), ultra dry, Luthium chloride, Chloride, Lithium, Lithium Chloride (LiCl) (2.3% in Tetrahydrofuran, ca. 0.5mol/L), lithim chloride, Lopac-L-4408, LITHIUM MONOCHLORIDE, MolMap_000071, WLN: LI G, Lithium Chloride (LiCl), ACS grade, Lopac0_000604, LITHIUM CHLORIDE (LICL) [MI], Lithium Chloride (LiCl) battery grade, Lithium Chloride (LiCl), ACS reagent, DTXCID105509, LITHIUM CHLORIDE (LICL) [HSDB], LITHIUM CHLORIDE (LICL) [INCI], LITHIUM MURIATICUM [HPUS], KWGKDLIKAYFUFQ-UHFFFAOYSA-M, LITHIUM CHLORIDE (LICL) [WHO-DD], Lithium Chloride (LiCl), 3-5% in THF, HMS3261J10, Tox21_500604, BDBM50494542, AKOS015902822, AKOS015950647, AKOS024438070, CCG-204693, Lithium Chloride (LiCl), gamma irradiated, 8m, LP00604, SDCCGSBI-0050586.P002, Lithium Chloride (LiCl), ACS reagent, >=99%, Lithium Chloride (LiCl), ReagentPlus(R), 99%, NCGC00015607-01, NCGC00015607-02, NCGC00015607-03, NCGC00015607-04, NCGC00015607-07, NCGC00093980-01, NCGC00093980-02, NCGC00261289-01, BP-13612, SY002997, Lithium Chloride (LiCl), Vetec(TM) reagent grade, EU-0100604, FT-0627896, L0204, L0222, Lithium Chloride (LiCl), Trace metals grade 99.9%, L 4408, Lithium Chloride (LiCl), SAJ first grade, >=98.0%, Lithium Chloride (LiCl), for molecular biology, >=99%, Lithium Chloride (LiCl), SAJ special grade, >=99.0%, A838146, Lithium Chloride (LiCl), BioXtra, >=99.0% (titration), Q422930, SR-01000076252, SR-01000076252-1, Lithium Chloride (LiCl), powder, >=99.99% trace metals basis, Lithium Chloride (LiCl), puriss. p.a., anhydrous, >=99.0% (AT), Lithium Chloride (LiCl), anhydrous, beads, -10 mesh, >=99.9% trace metals basis, Lithium Chloride (LiCl), anhydrous, beads, -10 mesh, 99.998% trace metals basis, Lithium Chloride (LiCl), puriss. p.a., ACS reagent, anhydrous, >=99.0% (AT), Lithium Chloride (LiCl), anhydrous, free-flowing, Redi-Dri(TM), ACS reagent, >=99%, Lithium Chloride (LiCl), anhydrous, free-flowing, Redi-Dri(TM), ReagentPlus(R), 99%, Lithium Chloride (LiCl), BioUltra, for molecular biology, anhydrous, >=99.0% (AT), 59217-69-5, Hydrochloric acid lithium salt, Lithium Chloride (LiCl), Lithium Chloride (LiCl) licl, lithiumchloride, licl, chlorure de lithium, chlorku litu, chlorolithium, lithiumchlorid, chlorku litu polish, luthium chloride, Lithium Chloride (LiCl), Lithium Chloride (LiCl) licl, lithiumchloride, licl, chlorure de lithium, chlorku litu, chlorolithium, lithiumchlorid, chlorku litu polish, luthium chloride



Lithium Chloride (LiCl) is a chemical compound.
Lithium Chloride (LiCl)'s chemical formula is LiCl.
Lithium Chloride (LiCl) contains lithium and chloride ions.


Lithium Chloride (LiCl) acts as an electrolyte for dry cells used at low temperatures, catalyst in certain oxidation reactions, solubilizer for polyamides and cellulose when used with amide solvents, chlorinating agent for steroid substrates.
Lithium Chloride (LiCl) is a chemical compound.


Lithium Chloride (LiCl) is a metal chloride salt with a Li(+) counterion.
Lithium Chloride (LiCl) has a role as an antimanic drug and a geroprotector.
Lithium Chloride (LiCl) is an inorganic chloride and a lithium salt.


Lithium Chloride (LiCl) is a salt of lithium that has been used experimentally as an immunomodulator.
Lithium Chloride (LiCl) is a white solid hygroscopic soluble in water, alcohol and ether.
Lithium Chloride (LiCl) is an ionic compound or salt that is highly polar and soluble in water.


Lithium Chloride (LiCl) is soluble in alcohol, slightly soluble in acetone, pyridine and liquid ammonia.
Lithium Chloride (LiCl) is a chemical compound with the formula LiCl.
Lithium Chloride (LiCl) behaves as a fairly typical ionic compound, although the Li+ ion is very small.


Lithium Chloride (LiCl) is hygroscopic and highly soluble in water, and is highly polar.
Lithium Chloride (LiCl) is an excellent water soluble crystalline Lithium source for uses compatible with Chlorides.
Lithium Chloride (LiCl) is generally immediately available in most volumes.


Chloride compounds can conduct electricity when fused or dissolved in water.
Chloride materials can be decomposed by electrolysis to chlorine gas and the metal.
They are formed through various chlorination processes whereby at least one chlorine anion (Cl-) is covalently bonded to the relevant metal or cation.


Lithium Chloride (LiCl) appears as colorless crystals or powder.
The resulting solution is evaporated to get a mixture of saturated solution and Lithium Chloride (LiCl) crystals.
The solid and the solution is separated and the supernatant solution is recycled for further evaporation.


Lithium Chloride (LiCl) is a solid which absorbs water to form a hydrate, LiCl.H2O
Lithium Chloride (LiCl) is more soluble in organic solvents such as acetone and methanol than potassium chloride or sodium chloride.
The chemical formula for Lithium Chloride (LiCl) is LiCl.


Lithium Chloride (LiCl) belongs to the low-toxicity category, but has a strong irritating and corrosive effect on the eyes and mucous membranes.
Ultra high purity and proprietary formulations can be prepared.
The chloride ion controls fluid equilibrium and pH levels in metabolic systems.


They can form either inorganic or organic compounds.
Lithium Chloride (LiCl)'s chemical formula is LiCl.
Lithium Chloride (LiCl) is an inorganic compound supplied as a white crystalline solid for molecular biology studies and diagnostics manufacturing.


Lithium Chloride (LiCl) is made by the action of hydrochloric acid on lithium hydroxide.
Lithium Chloride (LiCl)'s chemical formula is LiCl.
Lithium Chloride (LiCl) contains lithium and chloride ions.


Lithium Chloride (LiCl) is a white powder or small particles, it is the most deliquescent salt known.
Lithium Chloride (LiCl) is more soluble in polar organic solvents such as methanol and acetone than is sodium chloride or potassium chloride.
Lithium Chloride (LiCl) is a chemical compound with the formula LiCl.


Lithium Chloride (LiCl) is a typical ionic compound (with certain covalent characteristics), although the small size of the Li+ ion gives rise to properties not seen for other alkali metal chlorides, such as extraordinary solubility in polar solvents (83.05 g/100 mL of water at 20 °C) and its hygroscopic properties.


The specific gravity of Lithium Chloride (LiCl) is 2.068, the melting point is 605°C, the boiling point is 1360°C, and it is easily soluble in water grams (0°C) in 100 grams of water, 127.5 grams (100°C)].
Lithium Chloride (LiCl) acts as an electrolyte for dry cells used at low temperatures, catalyst in certain oxidation reactions, solubilizer for polyamides and cellulose when used with amide solvents, chlorinating agent for steroid substrates.


Lithium Chloride (LiCl) is registered under the REACH Regulation and is manufactured in and / or imported to the European Economic Area, at ≥ 1 000 to < 10 000 tonnes per annum.
Lithium Chloride (LiCl) is a chemical compound with a chemical formula “LiCl”.


The salt is a normal ionic compound, although the Li+ ion is small in size, Lithium Chloride (LiCl) produces unrecognized effects for other alkali metal chlorides, such as exceptional solubility in polar solvents and its hygroscopic properties.
Lithium Chloride (LiCl) is an inorganic compound supplied as a white crystalline solid for molecular biology studies and diagnostics manufacturing.


Lithium Chloride (LiCl) tastes very salty, like chlorination.
Lithium Chloride (LiCl) is an alkali metal halide, which is a white deliquescent solid at room temperature.
Due to the smaller ion radius and higher hydration energy of lithium, the solubility of Lithium Chloride (LiCl) is much higher than other congeneric chlorides (83g / 100mL, 20 ° C).


Lithium Chloride (LiCl)'s aqueous solution is alkaline.
Lithium Hcl is a sodium chloride type structure, in which the chemical bond is not a typical ionic bond, so it can be dissolved in many organic solvents, and can form adducts with ethanol, methanol and amines.


This property can be used to separate Lithium Chloride (LiCl) from alkali metal chlorides.
Lithium Chloride (LiCl) is a chemical compound with the formula LiCl.
Lithium Chloride (LiCl) behaves as a fairly typical ionic compound, although the Li+ ion is very small.


The salt is hygroscopic and highly soluble in water, and is highly polar.
Lithium Chloride (LiCl) is more soluble in polar organic solvents such as methanol and acetone than is sodium chloride or potassium chloride.
Lithium Chloride (LiCl) is a white solid hygroscopic soluble in water, alcohol and ether.


The chemical formula for Lithium Chloride (LiCl) is LiCl.
Lithium Chloride (LiCl) is made by the action of hydrochloric acid on lithium hydroxide.
The resulting solution is evaporated to get a mixture of saturated solution and Lithium Chloride (LiCl) crystals.


The solid and the solution is separated and the supernatant solution is recycled for further evaporation.
Lithium Chloride (LiCl) is a solid which absorbs water to form a hydrate, LiCl.H2O
Crystallization grade Lithium Chloride (LiCl) for formulating screens or for optimization.


The chemical formula of anhydrous Lithium Chloride (LiCl) is LiCl, the relative molecular weight is 42.39, which is cubic crystal white particles or powder, which is easy to deliquesce and tastes salty.
Lithium Chloride (LiCl) is a salt of Lithium chlorine, an alkali metal similar to sodium chloride.


Lithium Chloride (LiCl) has a typical shelf life of 2 years if kept in dry conditions.
Lithium Chloride (LiCl) appears as colorless crystals or powder.
Lithium Chloride (LiCl) is a solid which absorbs water to form a hydrate, LiCl.H2O.


Lithium Chloride (LiCl) is a typical ionic compound and a salt of lithium.
Although the Li+ ion is minuscule, Lithium Chloride (LiCl) creates unrecognized effects for other alkali metal chlorides, such as being soluble in polar solvents and having hygroscopic (holding water molecules) properties.


Lithium Chloride (LiCl) is an ionic compound or salt that is highly polar and soluble in water.
Lithium Chloride (LiCl) is more soluble in organic solvents such as acetone and methanol than potassium chloride or sodium chloride.
Lithium Chloride (LiCl) melts into a clear liquid when heated to a dark red color, and volatilizes when it is white hot.


Lithium Chloride (LiCl) is an injection indicated for cardiac output measurement.
Lithium Chloride (LiCl) is for assays to study cell-fate, neurobiology and antiviral properties; noted to inhibit GSK-3β
Lithium Chloride (LiCl) is hygroscopic in nature.


Lithium Chloride (LiCl) is incompatible with strong oxidizing agents, strong acids, bromine trichloride and bromine trifluoride.
Deliquescent salt forms a solution when exposed to humid air.
Store Lithium Chloride (LiCl) in a cool and dry place in closed tight containers.



USES and APPLICATIONS of LITHIUM CHLORIDE (LiCl):
Lithium Chloride (LiCl) is used for the production of lithium metal, by electrolysis of a LiCl/KCl melt at 450 °C.
Lithium Chloride (LiCl) is also used as a brazing flux for aluminium in automobile parts.
Another application of Lithium Chloride (LiCl) is that we use it as a flame colorant to produce dark red flames.


Apart from being a source of chloride, Lithium Chloride (LiCl) serves as an additive in the Stille reaction in organic synthesis and to precipitate RNA from cellular extracts.
Being biologically significant, Lithium Chloride (LiCl) finds applications in a wide variety of assays to study cell-fate and neurobiology.


Lithium Chloride (LiCl) has been found to inhibit virus infection.
Release to the environment of Lithium Chloride (LiCl) can occur from industrial use: industrial abrasion processing with low release rate (e.g. cutting of textile, cutting, machining or grinding of metal).


Lithium Chloride (LiCl) is used in the following products: welding & soldering products, laboratory chemicals, air care products, inks and toners, pH regulators and water treatment products, metal working fluids, pharmaceuticals, polymers and water treatment chemicals.
Lithium Chloride (LiCl) is used in the following areas: scientific research and development and health services.


In the calibration of hygrometers, they use Lithium Chloride (LiCl) as a relative humidity standard.
Lithium Chloride (LiCl) can be used as a hygrometer. In addition, when exposed to air it salts from deliquescent self-solution.
Furthermore, the equilibrium Lithium Chloride (LiCl) concentration of the resulting solution may directly relate to the relative humidity of the air.


Industries use Lithium Chloride (LiCl)'s molten form to prepare carbon nanotubes, lithium niobate, and grapheme.
Lithium Chloride (LiCl) can be used to improve the efficiency of the Stille reaction.
Lithium Chloride (LiCl)'s desiccant properties can be used to generate potable water by absorbing moisture from the air, which is then released by heating the salt.


Lithium Chloride (LiCl) is a chemical compound that is extremely soluble in polar solvents and is used in order to obtain lithium metal.
Other release to the environment of Lithium Chloride (LiCl) is likely to occur from: indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners), outdoor use, indoor use in close systems with minimal release (e.g. cooling liquids in refrigerators, oil-based electric heaters), outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids), outdoor use in long-life materials with low release rate (e.g. metal, wooden and plastic construction and building materials) and indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment).


Lithium Chloride (LiCl) is used in the following products: pharmaceuticals, air care products, inks and toners, laboratory chemicals, metal working fluids, paper chemicals and dyes, polymers, water treatment chemicals and welding & soldering products.
Release to the environment of Lithium Chloride (LiCl) can occur from industrial use: formulation of mixtures and formulation in materials.


For a short time in the 1940s Lithium Chloride (LiCl) was manufactured as a substitute for salt, but this was prohibited after the toxic effects of the compound were recognised
Lithium Chloride (LiCl) is the raw material of making lithium metal.


Besides, Lithium Chloride (LiCl) shows very strong acaricidal properties.
Lithium Chloride (LiCl) has been found to inhibit virus infection.
Lithium Chloride (LiCl) is used as an electrolyte for low temperature dry battery cells and as an oxidation catalyst.


Lithium Chloride (LiCl) is a solubilizer for polyamides and cellulose when used with amide solvents, and is a chlorinating agent for steroid substrates.
In organic synthesis Lithium Chloride (LiCl) is used as an additive in the Stille Reaction.
Ungraded products supplied by Spectrum are indicative of a grade suitable for general industrial use or research purposes and typically are not suitable for consumption.


Lithium Chloride (LiCl) is also used as a flame colorant to produce dark red flames.
Molten Lithium Chloride (LiCl) is used for the preparation of carbon nanotubes, graphene and lithium niobate.
Lithium Chloride (LiCl) has been shown to have strong acaricidal properties, being effective against Varroa destructor in populations of honey bees.


Other release to the environment of this substance is likely to occur from: indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment). This substance can be found in products with material based on: stone, plaster, cement, glass or ceramic (e.g. dishes, pots/pans, food storage containers, construction and isolation material) and paper (e.g. tissues, feminine hygiene products, nappies, books, magazines, wallpaper).


Lithium Chloride (LiCl) is used as aluminum welding agent, glass fiber, gelatin, air conditioning dehumidifier and special cement raw materials.
Lithium Chloride (LiCl) is also used in the production of lithium manganese battery electrolyte and biopharmaceutical intermediates in the battery industry.
Lithium Chloride (LiCl) is used in the following products: laboratory chemicals, pH regulators and water treatment products, metal working fluids, pharmaceuticals, polymers, water treatment chemicals and welding & soldering products.


Lithium Chloride (LiCl) is used in the following areas: scientific research and development and health services.
Lithium Chloride (LiCl) has also been utilized in: Large scale plasmid DNA isolation without ultracentrifugation, protein extraction and protein crystallization, crystallization of other biological structures including vitamin B12-RNA aptamer and the L-A virus particle.


Lithium Chloride (LiCl) inhibits the expression and secretion of insulin-like growth factor-binding protein-1 in H4-II-E cells, used in the synthesis of beta-substituted alpha-amino acid derivatives.
Lithium Chloride (LiCl) is used as an aversive agent in lab animals to study conditioned place preference and aversion.


Lithium Chloride (LiCl) is used by consumers, in articles, by professional workers (widespread uses), in formulation or re-packing, at industrial sites and in manufacturing.
Lithium Chloride (LiCl) is used the raw material for the preparation of metallic lithium.


Flux for metal production by electrolysis (such as titanium and aluminum production), Lithium Chloride (LiCl) is used as aluminum welding agent, air conditioner dehumidifier and special cement raw material.
Apart from being a source of chloride, Lithium Chloride (LiCl) serves as an additive in the Stille reaction in organic synthesis and to precipitate RNA from cellular extracts.


Being biologically significant, Lithium Chloride (LiCl) finds applications in a wide variety of assays to study cell-fate and neurobiology.
Release to the environment of Lithium Chloride (LiCl) can occur from industrial use: in processing aids at industrial sites, as an intermediate step in further manufacturing of another substance (use of intermediates), as processing aid, of substances in closed systems with minimal release and in the production of articles.


Lithium Chloride (LiCl) is mainly we use it for the production of lithium metal by electrolysis of LiCl/KCl which melt at 450oC.
Moreover, industries use Lithium Chloride (LiCl) as a brazing flux for aluminum in automobile parts.
In addition, we use Lithium Chloride (LiCl) as a desiccant for drying air streams.


In organic synthesis, Lithium Chloride (LiCl) has some specialized applications such as an additive in the Stille reaction.
Most noteworthy, Lithium Chloride (LiCl) has biochemical applications that we use to precipitate RNA from cellular extracts.
Lithium Chloride (LiCl) is also used in flame, in the battery industry for the production of lithium-manganese battery electrolyte, etc.


Anhydrous Lithium Chloride (LiCl) is mainly used for electrolytic preparation of metal lithium, aluminum flux and flux and moisture absorption (dehumidification) agent in non-refrigerated air conditioners.
Metal lithium can be obtained by electrolyzing the mixed molten salt of LiCl/KCl at 600 °C.


Lithium Chloride (LiCl) is used in the following products: coating products, metal surface treatment products, non-metal-surface treatment products, adhesives and sealants, inks and toners, pH regulators and water treatment products, photo-chemicals, polishes and waxes and welding & soldering products.
Lithium Chloride (LiCl) is widely used in several industrial applications.


Other release to the environment of Lithium Chloride (LiCl)e is likely to occur from: indoor use (e.g. machine wash liquids/detergents, automotive care products, paints and coating or adhesives, fragrances and air fresheners), outdoor use, indoor use in close systems with minimal release (e.g. cooling liquids in refrigerators, oil-based electric heaters), outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids), outdoor use in long-life materials with low release rate (e.g. metal, wooden and plastic construction and building materials) and indoor use in long-life materials with low release rate (e.g. flooring, furniture, toys, construction materials, curtains, foot-wear, leather products, paper and cardboard products, electronic equipment).


Lithium Chloride (LiCl) is useful for the production of lithium metal and for the generation of Mn(0) species which can be used in free radical cyclizations.
Lithium Chloride (LiCl) can serve as a flame colorant to generate dark red flames, a brazing flux for aluminum in automobiles, a hygrometer and a desiccant for drying air streams.


Lithium Chloride (LiCl)t is used as a flame colorant to form dark crimson flames.
Lithium Chloride (LiCl) is used in the precipitation of RNA in biological applications.
Lithium Chloride (LiCl) is an aluminum blazing flux in automobile parts.


Industrial metal is produced by this method.
Lithium Chloride (LiCl) is also used as a moisture scavenger in air conditioning systems, as a good flux in the electrolytic production of metals or in the preparation of powders (such as in the production of titanium and aluminum), as a precipitant for RNA, and as an additive in the Stille reaction .


Lithium Chloride (LiCl) can be formulated with DMF in different concentrations as a solvent for dissolving polymers.
Lithium Chloride (LiCl) is commonly used as an eluent for GPC measurements of molecular weight.
Lithium Chloride (LiCl) is used to make lithium metal.

Lithium chloride is melted and electrolyzed.
Lithium Chloride (LiCl) is useful for the production of lithium metal and for the generation of Mn(0) species which can be used in free radical cyclizations.


Lithium Chloride (LiCl) has also been utilized in: Large scale plasmid DNA isolation without ultracentrifugation; Protein extraction and protein crystallization; Crystallization of other biological structures, including vitamin B12-RNA aptamer and the L-A virus particle; Inhibits the expression and secretion of insulin-like growth factor-binding protein-1 in H4-II-E cells; Used in the synthesis of beta-substituted alpha-amino acid derivatives; May be used to selectively pre­cipitate RNA.


Lithium Chloride (LiCl) is used as desiccant in drying air streams.
Lithium Chloride (LiCl) can serve as a flame colorant to generate dark red flames, a brazing flux for aluminum in automobiles, a hygrometer and a desiccant for drying air streams.


On exposure to air, Lithium Chloride (LiCl) becomes a solution with the concentration directly related to relative humidity of the atmosphere and hence serves as a relative humidity standard in calibrating hygrometers.
On exposure to air, Lithium Chloride (LiCl) becomes a solution with the concentration directly related to relative humidity of the atmosphere and hence serves as a relative humidity standard in calibrating hygrometers.


Lithium Chloride (LiCl) is used to dry air.
Lithium Chloride (LiCl) is also used as a flux for aluminium.
Lithium Chloride (LiCl) can be used in making organic compounds.


Lithium Chloride (LiCl) can be used to color flames red.
Lithium Chloride (LiCl) is mainly we use it for the production of lithium metal by electrolysis of LiCl/KCl which melt at 450oC.
Moreover, industries use Lithium Chloride (LiCl) as a brazing flux for aluminum in automobile parts.


In addition, we use Lithium Chloride (LiCl) as a desiccant for drying air streams.
Lithium Chloride (LiCl) is used for several soldering and welding techniques and salt bath heat treatment at low temperatures.
Chlorolithium is mainly used in the manufacturing of lithium metals by the method of electrolysis.


In this method, Lithium Chloride (LiCl) or potassium chloride is melted at 450 °C.
Lithium Chloride (LiCl) is also has wide application as a brazing flux for aluminium used in automobile parts.
Lithium Chloride (LiCl) is used in massive dehumidification systems in the AC industry.


This depends on the low equilibrium pressure of vapor above Lithium Chloride (LiCl) solutions.
Lithium Chloride (LiCl) is used in large dehumidification systems in the air conditioning industry.
It depends on the low equilibrium pressure of water vapour above solutions of Lithium Chloride (LiCl).


Lithium Chloride (LiCl) is used in a number of salt mixtures exist low melting points allowing the material to be used in brazing fluxes and brazing baths.
Lithium Chloride (LiCl) is used as an electrolyte for the production of lithium metal and used as an electrolyte in voltaic cells.
In organic synthesis, Lithium Chloride (LiCl) has some specialized applications such as an additive in the Stille reaction.


Most noteworthy, Lithium Chloride (LiCl) has biochemical applications that we use to precipitate RNA from cellular extracts.
Another application of Lithium Chloride (LiCl) is that we use it as a flame colorant to produce dark red flames.
In the calibration of hygrometers, they use Lithium Chloride (LiCl) as a relative humidity standard.


Lithium Chloride (LiCl) is used for the manufacture of: chemicals and plastic products.
Lithium Chloride (LiCl) is used for the manufacture of: chemicals, plastic products and pulp, paper and paper products.
Release to the environment of Lithium Chloride (LiCl) can occur from industrial use: manufacturing of the substance.


Lithium Metal by Electrolysis: Lithium Chloride (LiCl) is primarily used at 450 ° C (842 ° F) for the preparation of lithium metal by electrolysis of a LiCl/KCl.
As Brazing Flux uses of Lithium Chloride (LiCl): Lithium Chloride (LiCl) is also used as a brazing flux for aluminum in automobile parts.


Lithium Chloride (LiCl) can be used as a hygrometer. In addition, when exposed to air it salts from deliquescent self-solution.
Furthermore, the equilibrium Lithium Chloride (LiCl) concentration of the resulting solution may directly relate to the relative humidity of the air.
Industries use Lithium Chloride (LiCl)'s molten form to prepare carbon nanotubes, lithium niobate, and grapheme.


Besides, Lithium Chloride (LiCl) shows very strong acaricidal properties.
Lithium Chloride (LiCl) is used in large dehumidification systems in the air conditioning industry.
Lithium Chloride (LiCl) is also used as a brazing flux for aluminium in automobile parts.


Lithium Chloride (LiCl) can be used to improve the efficiency of the Stille reaction.
Lithium Chloride (LiCl)'s desiccant properties can be used to generate potable water by absorbing moisture from the air, which is then released by heating the salt.


Lithium Chloride (LiCl) is used to make lithium metal.
Lithium chloride is melted and electrolyzed.
This makes liquid lithium metal.


Lithium Chloride (LiCl) has many applications.
Lithium Chloride (LiCl) is extremely hygroscopic, and is widely used in dehumidification systems to remove moisture from the air in industries such as food processing and horticulture.


Lithium Chloride (LiCl) is used to dry air.
Lithium Chloride (LiCl) is also used as a flux for aluminium.
Lithium Chloride (LiCl) can be used in making organic compounds.


Lithium Chloride (LiCl) is also used as a tracer for waste water, as a brazing flux, and as an electrolyte component for the manufacture of speciality batteries.
Lithium Chloride (LiCl) is used as an electrolyte for low temperature dry battery cells and as an oxidation catalyst.


Lithium Chloride (LiCl) is a solubilizer for polyamides and cellulose when used with amide solvents, and is a chlorinating agent for steroid substrates.
Lithium Chloride (LiCl) can be used to color flames red.
Lithium Chloride (LiCl) is used in the precipitation of RNA, it can block glycogen synthase kinase (GSK) and has been used in studies on cell-fate.


Lithium Chloride (LiCl) depends on the low equilibrium pressure of water vapour above solutions of lithium chloride.
Lithium Chloride (LiCl) is used in a number of salt mixtures exist low melting points allowing the material to be used in brazing fluxes and brazing baths.
Lithium Chloride (LiCl) is used as an electrolyte for the production of lithium metal and used as an electrolyte in voltaic cells.


Lithium Chloride (LiCl) is widely used in several industrial applications.
Lithium Chloride (LiCl) is used as a flame colorant to form dark crimson flames.
Lithium Chloride (LiCl) is used in the precipitation of RNA in biological applications.


Lithium Chloride (LiCl) is an aluminum blazing flux in automobile parts.
Lithium Chloride (LiCl) is used for several soldering and welding techniques and salt bath heat treatment at low temperatures.
Lithium Chloride (LiCl) is used in massive dehumidification systems in the AC industry.


Lithium Chloride (LiCl) is used as aluminum welding agent, Chemicalbook air conditioner dehumidifier and special cement raw material.
Lithium Chloride (LiCl) is also used in organic synthesis.
Lithium Chloride (LiCl) is used to precipitate RNA.


Lithium Chloride (LiCl) is used fluxes for welding and soldering techniques; salt bath for heat-treatment by low temperature and for dip brazing; raw material for other lithium compounds; tracer for chemical products (denaturation of wine etc.); absorption and desinfection reagent (Lithium Chloride (LiCl) solution) for absorbers.


In the battery industry, Lithium Chloride (LiCl) is used as an analytical reagent for the production of lithium-manganese battery electrolyte.
Lithium Chloride (LiCl) is used as a brazing flux, as a desiccant in drying air streams, as a component in organic synthesis, as an additive in the Stille reaction, in some biochemical applications, and as soldering aluminum metal.


Lithium Chloride (LiCl) is used for the production of lithium metal, by electrolysis of a LiCl/KCl melt at 450 °C.
This depends on the low equilibrium pressure of vapor above Lithium Chloride (LiCl) solutions.
Lithium Chloride (LiCl) is useful for the production of lithium metal and for the generation of Mn(0) species which can be used in free radical cyclizations.


Lithium Chloride (LiCl) can serve as a flame colorant to generate dark red flames, a brazing flux for aluminum in automobiles, a hygrometer and a desiccant for drying air streams.
Lithium Chloride (LiCl) is used as analytical reagent, heat exchange carrier


Lithium Chloride (LiCl) is used in organic synthesis.
Biochemical Applications: LiCl is used to precipitate RNA from cellular extracts.
As a flame colorant, Lithium Chloride (LiCl) is used to produce dark red flames.


Lithium Chloride (LiCl) is used as a Relative humidity standard in the calibration of hygrometers and itself can be used as a hygrometer.
Molten Lithium Chloride (LiCl) is used for the preparation of lithium niobite, graphene and carbon nanotubes.
Lithium Chloride (LiCl) is useful for the production of lithium metal and for the generation of Mn(0) species which can be used in free radical cyclizations.


Lithium Chloride (LiCl) can serve as a flame colorant to generate dark red flames, a brazing flux for aluminum in automobiles, a hygrometer and a desiccant for drying air streams.
On exposure to air, Lithium Chloride (LiCl) becomes a solution with the concentration directly related to relative humidity of the atmosphere and hence serves as a relative humidity standard in calibrating hygrometers.


Apart from being a source of chloride, Lithium Chloride (LiCl) serves as an additive in the Stille reaction in organic synthesis and to precipitate RNA from cellular extracts.
Being biologically significant, Lithium Chloride (LiCl) finds applications in a wide variety of assays to study cell-fate and neurobiology.


Lithium Chloride (LiCl) has been found to inhibit virus infection.
Lithium Chloride (LiCl) has strong acaricidal properties (Varroa destructor in populations of honey bees).
Lithium Chloride (LiCl) is used in the pharmaceutical industry for air conditioning, pyrotechnics, dry batteries and metal lithium.


On exposure to air, Lithium Chloride (LiCl) becomes a solution with the concentration directly related to relative humidity of the atmosphere and hence serves as a relative humidity standard in calibrating hygrometers.
Apart from being a source of chloride, Lithium Chloride (LiCl) serves as an additive in the Stille reaction in organic synthesis and to precipitate RNA from cellular extracts.


Being biologically significant, Lithium Chloride (LiCl) finds applications in a wide variety of assays to study cell-fate and neurobiology.
Lithium Chloride (LiCl) has been found to inhibit virus infection.
Lithium Chloride (LiCl) is the raw material for the manufacture of welding materials, air-conditioning equipment and the manufacture of metallic lithium.


Lithium Chloride (LiCl) is a very effective antimanic drug for the treatment of bipolar disorder.
Lithium Chloride (LiCl) is well soluble in water, alcohol, acetone, and amyl alcohol and Lithium Chloride (LiCl) is also used as a flame colorant to produce dark red flames.


Lithium Chloride (LiCl) is used as an electrolyte in voltaic cells.
Lithium Chloride (LiCl) is used to produce a dark red flame.
Lithium Chloride (LiCl) is used in supplements.
Lithium Chloride (LiCl) is used to make fireworks.


-Industrial Applications of Lithium Chloride (LiCl):
*Electrochemistry
Lithium metal is produced by electrolysis of Lithium Chloride (LiCl) and potassium chloride, which melts at 450°C.

High-purity Lithium Chloride (LiCl) is used as the feedstock in the process and makes about 99.5% pure lithium metal.
Molten lithium is contained in a carbon steel pot, while the chlorine gas is collected in a stainless steel or glass pipe for applications in other processes.

The molten lithium flows into a collecting tank and is later cast into ingots.
A mesh or stainless-steel screen separates the two compartments to prevent the products from mixing.



PROPERTIES OF LITHIUM CHLORIDE (LiCl):
Lithium Chloride (LiCl) is a colorless solid. It makes a bright red color in a flame.
Lithium Chloride (LiCl) absorbs water, unlike other alkali metal chlorides.
Lithium Chloride (LiCl) is also dissolves more easily in water than other alkali metal chlorides.



PREPARATION OF LITHIUM CHLORIDE (LiCl):
Lithium Chloride (LiCl) can be made by igniting lithium and chlorine, but it is difficult because the reaction is violent.
This makes the anhydrous (without water attached) form.

Another way is mixing lithium oxide, lithium hydroxide, or lithium carbonate with hydrochloric acid.
This makes the hydrate (water attached to the molecule).
The hydrous form can be dried to the anhydrous form by heating Lithium Chloride (LiCl) with hydrogen chloride gas.



PHYSICAL PROPERTIES OF LITHIUM CHLORIDE (LiCl):
Lithium Chloride (LiCl) is a white crystal, easily soluble in water, with a solubility of 67g/100ml of water under standard conditions.
Lithium Chloride (LiCl) is also easily soluble in organic solvents such as ethanol, etc.

Therefore, if chlorohalogenated hydrocarbons are used in the preparation of hydrocarbyl lithium, free hydrocarbyl lithium reagents (lithium bromide, Lithium iodide forms adducts with lithium hydrocarbyls and acts as a stabilizer).

Lithium Chloride (LiCl) has a sharp, saline taste
Lithium Chloride (LiCl) has cubic crystals, crystalline powder, or granule appearance
Lithium Chloride (LiCl) has a melting point of 121°F and 2.068 density at 77°F

Lithium Chloride (LiCl)'s aqueous solution is neutral and a bit alkaline
Lithium Chloride (LiCl) is soluble in ether, nitrobenzene, and water alcohols



FORMULA OF LITHIUM CHLORIDE (LiCl):
Lithium Chloride (LiCl) formula, also known as Chlorolithium formula or Lithiumchlorid formula is explained in this article.
Lithium Chloride (LiCl) is formed by one lithium atom and one chlorine atom.
In the year 1940, for a short period of time, Lithium Chloride (LiCl) was produced as a salt substitute.

Due to its toxic effects, Lithium Chloride (LiCl) was prohibited immediately.
The molecular or chemical formula of Lithium Chloride (LiCl) is LiCl.
Lithium Chloride (LiCl) occurs as a colourless to white hygroscopic and deliquescent powder or crystals.

Lithium Chloride (LiCl) has sharp saline like a taste.
Chlorolithium can be produced by treating lithium carbonate (Li2CO3) with hydrochloric acid (HCl).
Lithium Chloride (LiCl) can also be synthesized by high exothermic reaction of lithium metal with anhydrous hydrogen chloride gas or chlorine.
Anhydrous Lithium Chloride (LiCl) is obtained from the hydrate by heating it with a stream of hydrogen chloride (HCl).



NOTES OF LITHIUM CHLORIDE (LiCl):
Lithium Chloride (LiCl) is hygroscopic in nature. Incompatible with strong oxidizing agents, strong acids, bromine trichloride and bromine trifluoride.
Deliquescent salt forms a solution when exposed to humid air.
Store Lithium Chloride (LiCl) in a cool and dry place in closed tight containers.



PREPARATION OF LITHIUM CHLORIDE (LiCl):
Lithium Chloride (LiCl) can be made by igniting lithium and chlorine, but it is difficult because the reaction is violent.
This makes the anhydrous (without water attached) form.

Another way is mixing lithium oxide, lithium hydroxide, or lithium carbonate with hydrochloric acid.
This makes the hydrate (water attached to the molecule).
The hydrous form can be dried to the anhydrous form by heating Lithium Chloride (LiCl) with hydrogen chloride gas.



PROPERTIES OF LITHIUM CHLORIDE (LiCl):
Lithium Chloride (LiCl) is a colorless solid.
Lithium Chloride (LiCl) makes a bright red color in a flame.
Lithium Chloride (LiCl) absorbs water, unlike other alkali metal chlorides.
Lithium Chloride (LiCl) also dissolves more easily in water than other alkali metal chlorides.



CHEMICAL CHARACTERISTICS OF LITHIUM CHLORIDE (LiCl):
*Reaction with Sulfuric Acid:
Lithium Chloride (LiCl) and sulfuric acid reaction form hydrogen chloride and lithium sulfate.

Here is the reaction’s chemical equation:
2LiCl+H2SO4→2HCl+Li2SO4

*Reaction with Base
Lithium Chloride (LiCl) reacts with an alkali (such as Sodium Hydroxide) to form Sodium Chloride and Lithium Hydroxide.
LiCl+NaOH→LiOH+NaCl

Like other metal chlorides, Lithium Chloride (LiCl) salt produces crystalline hydrates.
You can regenerate Lithium Chloride (LiCl)'s anhydrous salts after heating the hydrates.

Besides, Lithium Chloride (LiCl) can easily absorb four equivalents of ammonia per mol.
However, Lithium Chloride (LiCl) can mainly serve as a chloride ion source when combined with an ionic chloride.



CHARACTERISTICS OF LITHIUM CHLORIDE (LiCl):
At room temperature, Lithium Chloride (LiCl) is white powder or small granules, which is the most deliquescent among the known salts.
Lithium Chloride (LiCl) tastes very salty, like chlorination; it melts into clear liquid when heated to dark red, and volatilizes when it is white hot.

Lithium Chloride (LiCl) is a sodium chloride type structure Chemicalbook, the chemical bond is not a typical ionic bond, so Lithium Chloride (LiCl) is easily soluble in water, and the solubility is 67g/100ml water under standard conditions.
Lithium Chloride (LiCl) is also soluble in organic solvents such as ethanol, acetone, pyridine, etc., but insoluble in ether.



CHEMICAL PROPERTIES OF LITHIUM CHLORIDE (LiCl):
Lithium Chloride (LiCl) reaction with sulfuric acid forms lithium sulfate and hydrogen chloride.
The chemical equation is given below.

2LiCl + H2SO4 → 2 HCl + Li2SO4
Lithium Chloride (LiCl) reacts with a base like sodium hydroxide and forms lithium hydroxide and sodium chloride.
LiCl + NaOH → LiOH + NaCl



NOTES OF LITHIUM CHLORIDE (LiCl):
Lithium Chloride (LiCl) is hygroscopic in nature.
Lithium Chloride (LiCl) is incompatible with strong oxidizing agents, strong acids, bromine trichloride and bromine trifluoride.
Deliquescent salt forms a solution when exposed to humid air.
Store Lithium Chloride (LiCl) in a cool and dry place in closed tight containers.



CHEMICAL PROPERTIES OF LITHIUM CHLORIDE (LICL):
Like other metal chlorides Lithium Chloride (LiCl)'s salt form crystalline hydrates.
Furthermore, Lithium Chloride (LiCl)'s mono-, tri-, pentahydrate are known.
We can regenerate Lithium Chloride (LiCl)'s anhydrous salts by heating the hydrates.

In addition, Lithium Chloride (LiCl) easily absorbs up to four equivalents of ammonia/mol.
However, with another ionic chloride, the solution of Lithium Chloride (LiCl)can serve as a source of chloride ion.
Lithium Chloride (LiCl) reaction with sulfuric acid forms lithium sulfate and hydrogen chloride.
The chemical equation is given below.

2LiCl + H2SO4 → 2 HCl + Li2SO4
Lithium Chloride (LiCl) reacts with a base like sodium hydroxide and forms lithium hydroxide and sodium chloride.
LiCl + NaOH → LiOH + NaCl



PHYSICAL PROPERTIES OF LITHIUM CHLORIDE (LICL):
Lithium Chloride (LiCl) appears as an odorless white crystalline hygroscopic solid.
Lithium Chloride (LiCl) has a density of 2.068g/cm3 and its boiling point is 1382oC and its melting point is in between 605–614oC.
Lithium Chloride (LiCl) is soluble in water, methanol, ethanol, isopropanol, butanol, formic acid, n- mehtylformamide, hydrazine, and THF.

In addition, Lithium Chloride (LiCl) is slightly soluble in acetone and ammonia and is completely insoluble in dichloromethane.
Lithium Chloride (LiCl) has a sharp, saline taste.
Lithium Chloride (LiCl) has cubic crystals, crystalline powder, or granule appearance.

Lithium Chloride (LiCl) has a melting point of 121°F and 2.068 density at 77°F.
Lithium Chloride (LiCl)'s aqueous solution is neutral and a bit alkaline.
Lithium Chloride (LiCl) is soluble in ether, nitrobenzene, and water alcohols.



FORMULA AND STRUCTURE OF LITHIUM CHLORIDE (LiCl):
The chemical formula of Lithium Chloride (LiCl) is LiCl.
Lithium Chloride (LiCl) has a molar mass of 42.394 g/mol.
On molecular level the positively charged lithium-ion ( Li+ ) reacts with the negatively charged chloride ion ( Cl− ) to form Lithium Chloride (LiCl).

Lithium Chloride (LiCl) Formula is a typical ionic compound and a salt of lithium.
Due to the small size of the lithium-ion ( Li+ ), Lithium Chloride (LiCl) gives rise to properties that we cannot see in other alkali metal chlorides.

We also know Lithium Chloride (LiCl) by the name of Chlorolithium or lithiumchloride.
During the year the 1940s for a short while they produce Lithium Chloride (LiCl) as a compound to replace common salt (Sodium Chloride NaCl).



PREPARATION OF LITHIUM CHLORIDE (LiCl):
We can produce Lithium Chloride (LiCl) by treatment of lithium carbonate with hydrochloric acid.
In addition, we can also generate Lithium Chloride (LiCl) by the highly exothermic reaction of lithium metal with ether chlorine or anhydrous hydrogen chloride gas.
Furthermore, we can prepare anhydrous Lithium Chloride (LiCl) from the hydrating and heating with a stream of hydrogen chloride.



PHYSICAL PROPERTIES OF LITHIUM CHLORIDE (LiCl):
Lithium Chloride (LiCl) appears as an odorless white crystalline hygroscopic solid.
Lithium Chloride (LiCl) has a density of 2.068g/cm3 and its boiling point is 1382oC and its melting point is in between 605–614oC.

Lithium Chloride (LiCl) is soluble in water, methanol, ethanol, isopropanol, butanol, formic acid, n- mehtylformamide, hydrazine, and THF.
In addition, Lithium Chloride (LiCl) is slightly soluble in acetone and ammonia and is completely insoluble in dichloromethane.



CHEMICAL PROPERTIES OF LITHIUM CHLORIDE (LiCl):
Like other metal chlorides Lithium Chloride (LiCl)'s salt form crystalline hydrates.
Furthermore, Lithium Chloride (LiCl)'s mono-, tri-, pentahydrate are known.

We can regenerate Lithium Chloride (LiCl)'s anhydrous salts by heating the hydrates.
In addition, Lithium Chloride (LiCl) easily absorbs up to four equivalents of ammonia/mol.
However, with another ionic chloride, the solution of Lithium Chloride (LiCl) can serve as a source of chloride ion.

Lithium Chloride (LiCl) Reaction with Sulfuric Acid:
When Lithium Chloride (LiCl) reacts with sulfuric acid, it forms lithium sulfate and hydrogen chloride.
The chemical equation is given below.
2LiCl+H2SO4→2HCl+Li2SO4

The salt forms crystalline hydrates, unlike the other alkali metal chlorides.
Mono-, tri-, and pentahydrates are known.
The anhydrous salt can be regenerated by heating the hydrates.

Lithium Chloride (LiCl) also absorbs up to four equivalents of ammonia/mol.
As with any other ionic chloride, solutions of Lithium Chloride (LiCl) can serve as a source of chloride ion, e.g., forming a precipitate upon treatment with silver nitrate:
LiCl + AgNO3 → AgCl + LiNO3



PROPERTIES OF LITHIUM CHLORIDE (LICL):
1. Physical Properties of Lithium Chloride (LiCl) Licl:
Lithium Chloride (LiCl) is Deliquescent in nature, appear as cubic crystals, granules or crystalline powder
Lithium Chloride (LiCl) has sharp saline taste

Lithium Chloride (LiCl) has Boiling point of 2417 to 2480 °F at 760 mm Hg
Lithium Chloride (LiCl)'s Melting point is 1121 °F
Lithium Chloride (LiCl) has Density of 2.068 at 77 °F

Aqueous solution of Lithium Chloride (LiCl) is neutral or slightly alkaline.
Lithium Chloride (LiCl) is very soluble in water alcohols, ether, pyridine, nitrobenzene



CHEMICAL PROPERTIES OF LITHIUM CHLORIDE (LiCl):
Lithium Chloride (LiCl) can react as a source of chloride ion.
As with any other soluble ionic chloride, Lithium Chloride (LiCl) will precipitate insoluble chlorides when added to a solution of an appropriate metal salt such as lead(II) nitrate:

2 LiCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 LiNO3(aq)

The Li+ ion acts as a weak Lewis acid under certain circumstances; for example one mole of Lithium Chloride (LiCl) is capable of absorbing up to four moles of ammonia.



PREPARATION OF LITHIUM CHLORIDE (LiCl):
Lithium Chloride (LiCl) may be prepared most simply by reaction of lithium hydroxide or lithium carbonate with hydrochloric acid.
Lithium Chloride (LiCl) may also be prepared by the highly exothermic reaction of lithium metal with either chlorine or anhydrous hydrogen chloride gas.
Anhydrous Lithium Chloride (LiCl) is prepared from the hydrate by gently heating under an atmosphere of hydrogen chloride, used to prevent hydrolysis.



PHYSICAL and CHEMICAL PROPERTIES of LITHIUM CHLORIDE (LiCl):
Boiling Point: 1,360°C
Melting Point: 605°C (literature)
CAS Max %: ≤100.0000%
Quantity: 500 g
Linear Formula: LiCl
IUPAC Name: lithium chloride
Formula Weight: 42.39
Percent Purity: 99%
Grade: Reagent
Packaging: Poly Bottle
Density: 2.07 g/cm³
Chemical Name or Material: Lithium chloride,
Free-flowing, Reagent Grade, anhydrous, 99%

Formula: ClLi
InChI: InChI=1S/ClH.Li/h1H;/q;+1/p-1
InChI key: InChIKey=KWGKDLIKAYFUFQ-UHFFFAOYSA-M
SMILES: [Li]Cl
Compound Formula: ClLi
Molecular Weight: 42.39
Appearance: White powder
Density: 2.07 g/cm³
Solubility in H2O: N/A
Exact Mass: 41.9849
Monoisotopic Mass: 41.9849
Vapor pressure: 1 torr (785 °C)
10 torr (934 °C)
100 torr (1130 °C)

Magnetic susceptibility (χ): −24.3•10−6 cm3/mol
Refractive index (nD): 1.662 (24 °C)
Viscosity: 0.87 cP (807 °C)
Structure:
Coordination geometry: Octahedral
Molecular shape: Linear (gas)
Dipole moment: 7.13 D (gas)
Thermochemistry:
Heat capacity (C): 48.03 J/mol•K
Std molar entropy (S⦵298): 59.31 J/mol•K
Std enthalpy of formation (ΔfH⦵298): -408.27 kJ/mol
Gibbs free energy (ΔfG⦵): -384 kJ/mol
Molecular Weight: 42.4 g/mol
Physical state: powder

Color: colorless
Odor: odorless
Melting point/freezing point:
Melting point/range: 605 °C
Initial boiling point and boiling range: 1.360 °C at 1.013 hPa
Flammability (solid, gas): The product is not flammable.
Upper/lower flammability or explosive limits: No data available
Flash point: Not applicable
Autoignition temperature: No data available
Decomposition temperature: No data available
pH: ca.6 at 50 g/l at 20 °C
Viscosity
Viscosity, kinematic: No data available
Viscosity, dynamic: No data available
Hydrogen Bond Donor Count: 0

Hydrogen Bond Acceptor Count: 1
Rotatable Bond Count: 0
Exact Mass: 41.9848561 g/mol
Monoisotopic Mass: 41.9848561 g/mol
Topological Polar Surface Area: 0Ų
Heavy Atom Count: 2
Formal Charge: 0
Complexity: 2
Isotope Atom Count: 0
Defined Atom Stereocenter Count: 0
Undefined Atom Stereocenter Count: 0
Defined Bond Stereocenter Count: 0
Undefined Bond Stereocenter Count: 0
Covalently-Bonded Unit Count: 2
Compound Is Canonicalized: Yes

Color: Colorless
Physical Form: Liquid
Linear Formula: LiCl
IUPAC Name: lithium(1+) chloride
Formula Weight: 42.39
Odor: Odorless
Chemical Name or Material: Lithium chloride
Chemical formula: LiCl
Molar mass: 42.39 g•mol−1
Appearance: white solid
hygroscopic, sharp
Density: 2.068 g/cm3
Melting point: 605–614 °C (1,121–1,137 °F; 878–887 K)
Boiling point: 1,382 °C (2,520 °F; 1,655 K)

Solubility in water: 68.29 g/100 mL (0 °C)
74.48 g/100 mL (10 °C)
84.25 g/100 mL (25 °C)
88.7 g/100 mL (40 °C)
123.44 g/100 mL (100 °C)
Solubility: soluble in hydrazine, methylformamide,
butanol, selenium(IV) oxychloride, 1-propanol
Solubility in methanol: 45.2 g/100 g (0 °C)
43.8 g/100 g (20 °C)
42.36 g/100 g (25 °C)
44.6 g/100 g (60 °C)

Solubility in ethanol: 14.42 g/100 g (0 °C)
24.28 g/100 g (20 °C)
25.1 g/100 g (30 °C)
23.46 g/100 g (60 °C)
Solubility in formic acid: 26.6 g/100 g (18 °C)
27.5 g/100 g (25 °C)
Solubility in acetone: 1.2 g/100 g (20 °C)
0.83 g/100 g (25 °C)
0.61 g/100 g (50 °C)
Solubility in liquid ammonia: 0.54 g/100 g (-34 °C)
3.02 g/100 g (25 °C)

Water solubility: 569 g/l at 20 °C
Partition coefficient: n-octanol/water:
Not applicable for inorganic substances
Vapor pressure: 1,33 hPa at 547 °C
Density: 2,07 g/cm3 at 20 °C
Relative density: No data available
Relative vapor density: No data available
Particle characteristics: No data available
Explosive properties: No data available
Oxidizing properties: none
Other safety information: No data available
LiCl: Lithium Chloride
Density: 2.07 g/cm³
Molecular Weight/ Molar Mass: 42.394 g/mol

Boiling Point: 1,382 °C
Melting Point: 605 °C
Chemical Formula: LiCl
Odour: Odourless
λ: 280 nm Amax: 0.01
Sensitive: Hygroscopic
Merck: 145,528
Stability: Stable.
Incompatible with strong oxidizing agents, strong acids,
bromine trichloride, bromine trifluoride. Very hygroscopic.
Protect from moisture.
InChIKey: KWGKDLIKAYFUFQ-UHFFFAOYSA-M
CAS DataBase Reference: 7447-41-8(CAS DataBase Reference)
NIST Chemistry Reference: Lithium chloride(7447-41-8)

EPA Substance Registry System: Lithium chloride (7447-41-8)
Appearance: White solid hygroscopic
Covalently-Bonded Unit: 2
Specific Gravity: 2.068 at 77 ° F
Complexity: 2
Solubility: Insoluble in water
CAS: 7447-41-8
MF: LiCl
MW: 42.39
EINECS: 231-212-3
Mol File: 7447-41-8.mol
Lithium chloride Chemical Properties:
Melting point: 605 °C(lit.)

Boiling point: 1382°C
density: 2.06
vapor pressure: 1.33 hPa (547 °C)
refractive index: n20/D 1.381
Fp: -4 °F
storage temp.: 2-8°C
solubility: H2O: soluble
form: beads
color: White to gray
Specific Gravity: 2.068
Odor: Odorless
PH: 5.5-7.5 (25℃, 50mg/mL in H2O)
PH Range: 6

Water Solubility: 832 g/L (20 ºC)
λmax: λ: 260 nm Amax: 0.01
λ: 280 nm Amax: 0.01
Sensitive: Hygroscopic
Merck: 145,528
Stability: Stable.
InChIKey: KWGKDLIKAYFUFQ-UHFFFAOYSA-M
CAS DataBase Reference: 7447-41-8(CAS DataBase Reference)
NIST Chemistry Reference: Lithium chloride(7447-41-8)
EPA Substance Registry System: Lithium chloride (7447-41-8)
Linear Formula: LiCl
UN Number: NONH for all modes of transport
Formula Weight: 42.39g/mol
Chemical Name or Material: Lithium Chloride



FIRST AID MEASURES of LITHIUM CHLORIDE (LiCl):
-Description of first-aid measures:
*General advice:
Show this material safety data sheet to the doctor in attendance.
*If inhaled:
After inhalation:
Fresh air.
*In case of skin contact:
Take off immediately all contaminated clothing.
Rinse skin with water/ shower.
*In case of eye contact:
After eye contact:
Rinse out with plenty of water.
Call in ophthalmologist.
Remove contact lenses.
*If swallowed:
After swallowing:
Immediately make victim drink water (two glasses at most).
Consult a physician.
-Indication of any immediate medical attention and special treatment needed:
No data available



ACCIDENTAL RELEASE MEASURES of LITHIUM CHLORIDE (LiCl):
-Environmental precautions:
Do not let product enter drains.
-Methods and materials for containment and cleaning up:
Cover drains.
Collect, bind, and pump off spills.
Observe possible material restrictions.
Take up dry.
Dispose of properly.
Clean up affected area.



FIRE FIGHTING MEASURES of LITHIUM CHLORIDE (LiCl):
-Extinguishing media:
*Suitable extinguishing media:
Use extinguishing measures that are appropriate to local circumstances and the
surrounding environment.
*Unsuitable extinguishing media:
For this substance/mixture no limitations of extinguishing agents are given.
-Further information:
Suppress (knock down) gases/vapors/mists with a water spray jet.
Prevent fire extinguishing water from contaminating surface water or the ground water system.



EXPOSURE CONTROLS/PERSONAL PROTECTION of LITHIUM CHLORIDE (LiCl):
-Exposure controls:
--Personal protective equipment:
*Eye/face protection:
Use equipment for eye protection.
Safety glasses
*Skin protection:
Full contact:
Material: Nitrile rubber
Minimum layer thickness: 0,11 mm
Break through time: 480 min
Splash contact:
Material: Nitrile rubber
Minimum layer thickness: 0,11 mm
Break through time: 480 min
*Body Protection:
protective clothing
*Respiratory protection:
Recommended Filter type: Filter type P2
-Control of environmental exposure:
Do not let product enter drains.



HANDLING and STORAGE of LITHIUM CHLORIDE (LiCl):
-Conditions for safe storage, including any incompatibilities:
*Storage conditions:
Tightly closed.
Dry.
hygroscopic
*Storage class:
Storage class (TRGS 510): 13:
Non Combustible Solids



STABILITY and REACTIVITY of LITHIUM CHLORIDE (LiCl):
-Reactivity:
No data available
-Chemical stability:
The product is chemically stable under standard ambient conditions (room temperature) .
-Conditions to avoid:
no information available
-Incompatible materials:
No data available