COLLOIDAL SILVER, N° CAS : 7440-22-4 - Colorant argent, Nom INCI : COLLOIDAL SILVER, N° EINECS/ELINCS : 231-131-3 Additif alimentaire : E174. Ses fonctions (INCI): Antimicrobien : Aide à ralentir la croissance de micro-organismes sur la peau et s'oppose au développement des microbes

Colloidal silver consists of tiny silver particles in a liquid.
Colloidal silver is sometimes promoted on the internet as a dietary supplement; however, evidence supporting health-related claims is lacking.
Colloidal silver is used for wound healing, improving skin disorders, and preventing certain diseases.

CAS Number: 7440-22-4
EC Number: 231-131-3
Molecular Formula: Ag
Molecular Weight: 107.87

7440-22-4, 7761-88-8, Silver, Silver Paste DGP80 TESM8020, Silver atomic spectroscopy standard concentrate 1.00 g Ag, Colloidal silver ink, Silver nanowires, Silver nitrate concentrate, Silver nitrate solution, Silver standard solution, Silver, dispersion, Silverjet DGH-55HTG, Silverjet DGH-55LT-25C, Silverjet DGP-40LT-15C, Silverjet DGP-40TE-20C, SunTronic® Silver

Colloidal silver has been used in a variety of ways.
However, Colloidal silver is not approved for medical use by the FDA and should not be consumed, injected, or inhaled.
Use of colloidal silver can result in short-term and long term side effects.

Colloidal silver, also known as silver proteins or colloidal silver proteins, is a suspension of tiny silver particles in liquid.
Although silver has been used for medicinal and health purposes for thousands of years, colloidal silver has recently become popular amongst wellness enthusiasts hoping to boost their overall health.

Colloidal silver is a suspension of tiny silver particles.
Commercial products are made by mixing silver, sodium hydroxide, and gelatin.
Homemade suspensions have also been made using different ingredients and an electrical current.

Most commonly, people swallow the suspension; however, Colloidal silver has also been inhaled using a nebulizer machine, and used topically on the skin and in the eyes.
Colloidal silver has even been used as a nasal spray.

Colloidal silver is a liquid suspension of microscopic particles of silver.
Colloidal silver has been promoted for its supposed antibacterial, antiviral, and antifungal properties.

Colloidal silver is one of the basic elements present in the earth's crust.
Colloidal silver is alloyed with many other metals to improve strength and hardness and to achieve corrosion resistance.

Colloidal silvers are one of the most commonly utilized nanomaterials due to their anti-microbial properties, high electrical conductivity, and optical properties.
Colloidal silvers (colloidal silver) have unique optical, electronic, and antibacterial properties, and are widely used in areas such as biosensing, photonics, electronics, and antimicrobial applications.
Colloidal silver is rare, but occurs naturally in the environment as a soft, “silver”-colored metal or as a white powdery compound (silver nitrate).

Metallic Colloidal silver and silver alloys are used to make jewelry, eating utensils, electronic equipment, and dental fillings.
Colloidal silvers of silver have been developed into meshes, bandages, and clothing as an antibacterial.
Colloidal silver is used in photographic materials, electric and electronic products, brazing alloys and solders, electroplated and sterling ware, as a catalyst, and in coinage.

Colloidal silvers are nanoparticles of silver, i.e. silver particles of between 1 nm and 100 nm in size.
The metal Colloidal silver is described as a white, lustrous solid.

In Colloidal silver is pure form it has the highest thermal and electrical conductivity and lowest contact resistance of all metals.
With the exception of gold, silver is the most malleable metal.

Colloidal silvers are nanoscale-sized particles composed of silver atoms.
Colloidal silvers, in particular, have attracted significant attention due to their distinct characteristics and potential applications.
Silver has no known functions or benefits in the body when taken by mouth, and Colloidal silver is not an essential mineral.

Colloidal silver products are often marketed as dietary supplements to take by mouth.
These products also come in forms to use on the skin.
Colloidal silver is a controversial alternative medicine.

A common form of Colloidal silver that is used to treat infections is silver nitrate.
Recent advancement in technology has introduced Colloidal silvers into the medical field.
Their small size and ability to induce cell death through multiple mechanisms makes them fantastic pharmacological candidates.

Colloidal silver is one of the earliest known metals.
Silver has no known physiologic or biologic function, though colloidal silver is widely sold in health food stores.
Colloidal silver has high thermal and electrical conductivity and resists oxidation in air that is devoid of hydrogen sulfide.

While frequently described as being 'silver' some are composed of a large percentage of silver oxide due to their large ratio of surface to bulk silver atoms.
Numerous shapes of Colloidal silvers can be constructed depending on the application at hand.

Commonly used Colloidal silvers are spherical, but diamond, octagonal, and thin sheets are also common.
Colloidal silver is widely used in many consumer products due to its unique optical, electrical, and thermal properties and extraordinarily efficient at absorbing and scattering light.

Colloidal silver has a face-centered cubic crystal structure.
Colloidal silver is a white metal, softer than copper and harder than gold.

When molten, Colloidal silver is luminescent and occludes oxygen, but the oxygen is released upon solidification.
As a conductor of heat and electricity, Colloidal silver is superior to all other metals.

Colloidal silver is soluble in HNO3 containing a trace of nitrate.
Colloidal silver is soluble in hot 80% H2SO4.

Colloidal silver is insoluble in HCl or acetic acid.
Colloidal silver is tarnished by H2S, soluble sulfides and many sulfur-containing organic substances (e.g., proteins).

Colloidal silver is not affected by air or H2O at ordinary temperatures, but at 200 C, a slight film of silver oxide is formed.
Colloidal silver is not affected by alkalis, either in solution or fused.

There are two stable, naturally occurring isotopes, 107Ag and 109Ag.
In addition, there are reported to be 25 less stable isotopes, ranging in half-life from 5 seconds to 253 days.
Colloidal silver is a white lustrous metal that is extremely ductile and malleable.

Colloidal silver does not oxidize in O2 by heating.
While frequently described as being 'silver' some are composed of a large percentage of silver oxide due to their large ratio of surface to bulk silver atoms.

Numerous shapes of nanoparticles can be constructed depending on the application at hand.
Commonly used Colloidal silvers are spherical, but diamond, octagonal, and thin sheets are also common.

Their extremely large surface area permits the coordination of a vast number of ligands.
The properties of Colloidal silvers applicable to human treatments are under investigation in laboratory and animal studies, assessing potential efficacy, biosafety, and biodistribution.

Most applications in biosensing and detection exploit the optical properties of Colloidal silvers, as conferred by the localized surface plasmon resonance effect.
That is, a specific wavelength (frequency) of incident light can induce collective oscillation of the surface electrons of Colloidal silvers.
The particular wavelength of the localized surface plasmon resonance is dependant on the Colloidal silver size, shape, and agglomeration state.

Colloidal silvers are the most common commercialized nano technological product on the market.
Due to its unique antibacterial properties, Colloidal silvers have been hailed as a breakthrough germ killing agent and have been incorporated into a number of consumer products such as clothing, kitchenware, toys and cosmetics.
Many consider silver to be more toxic than other metals when in nanoscale form and that these particles have a different toxicity mechanism compared to dissolved silver.

Colloidal silver can be synthesized using ethylene glycol as a reducing agent and PVP as a capping agent, in a polyol synthesis reaction (vide supra).
A typical synthesis using these reagents involves adding fresh Colloidal silver nitrate and PVP to a solution of ethylene glycol heated at 140 °C.

This procedure can actually be modified to produce another anisotropic silver nanostructure, nanowires, by just allowing the silver nitrate solution to age before using Colloidal silver in the synthesis.
By allowing the silver nitrate solution to age, the initial nanostructure formed during the synthesis is slightly different than that obtained with fresh silver nitrate, which influences the growth process, and therefore, the morphology of the final product.

Silver nanopaticles are widely incorporated into wound dressings, and are used as an antiseptic and disinfectant in medical applications and in consumer goods.
Colloidal silver becomes Ag2O3 in O3 and black Ag2S3 in S2 and H2S.

Colloidal silver is soluble in HNO3 and concentrated H2SO4.
Colloidal silver is not soluble in alkali.

Nanoscience and nanotechnology have now become the topic research that many developed.
Colloidal silver materials are developed in many applications because of their unique optical characteristic.

Colloidal silver is a noble metal, extensively used in SERS, photocatalysis and solar cells.
The surface of Colloidal silver can be functionalized to attain specific properties such as biocompatibility and vapor selectivity of sensors.

Iodized Colloidal silver foils and thin films find potential use as SERS-active metal substrates.
Cu substrates laminated with Ag foils, have compatible coefficient of thermal expansion (CTE), to be used for electronic packaging.

Their extremely large surface area permits the coordination of a vast number of ligands.
The properties of Colloidal silvers applicable to human treatments are under investigation in laboratory and animal studies, assessing potential efficacy, biosafety, and biodistribution.

Colloidal silvers are nanoparticles of silver in the range of 1 nm and 100 nm in size.
While frequently described as being 'Colloidal silver' some are composed of a large percentage of silver oxide due to their large ratio of surface-to-bulk silver atoms.

As studies of Colloidal silvers improve, several Colloidal silvers medical applications have been developed to help prevent the onset of infection and promote faster wound healing.
Colloidal silvers are materials with dimensions typically in the range of 1 to 100 nanometers.
At this scale, materials often exhibit unique and enhanced properties compared to their bulk counterparts.

Colloidal silvers have a high surface area per unit mass and release a continuous level of silver ions into their environment.
Colloidal silvers exhibit catalytic activity, making them useful in certain chemical reactions and processes.

This property is of interest in fields such as catalysis and environmental remediation.
Colloidal silvers display unique optical properties, including the ability to interact with light in ways that depend on their size and shape.

This has led to applications in sensors, imaging, and as components in optical devices.
Due to the conductive nature of silver, nanoparticles made from silver can exhibit enhanced electrical conductivity.

This property is advantageous in applications related to electronics and sensors.
The interaction of light with the electrons in Colloidal silvers leads to a phenomenon known as surface plasmon resonance (SPR).
This optical effect is widely exploited in sensing applications.

Colloidal silvers have been investigated for various biomedical applications, including drug delivery systems, imaging agents, and as components in diagnostic tools.
Colloidal silvers are used in the formulation of conductive inks and coatings for applications in printed electronics, flexible electronics, and RFID tags.
Colloidal silvers are incorporated into textiles and fabrics to impart antimicrobial properties, making them useful for applications such as antibacterial clothing and wound dressings.

Incorporation of silver particles into plastics, composites, and adhesives increases the electrical conductivity of the material.
Silver pastes and epoxies are widely utilized in the electronics industries.

Colloidal silver based inks are used to print flexible electronics and have the advantage that the melting point of the small Colloidal silvers in the ink is reduced by hundreds of degrees compared to bulk silver.
When scintered, these Colloidal silver based inks have excellent conductivity.

Colloidal silvers have attract increasing attention for the wide range of applications in biomedicine.
Colloidal silvers, generally smaller than 100 nm and contain 20–15,000 silver atoms, have distinct physical, chemical and biological properties compared to their bulk parent materials.

The optical, thermal, and catalytic properties of Colloidal silvers are strongly influenced by their size and shape.
Additionally, owning to their broad-spectrum antimicrobial ability, Colloidal silvers have also become the most widely used sterilizing nanomaterials in consuming and medical products, for instance, textiles, food storage bags, refrigerator surfaces, and personal care products.

Colloidal silvers are those having diameters of nanometer size.
With the advent of modern technology, humans can make nano-sized particles that were not present in nature.
Manufactured nanomaterials are materials with diameters of nanometer size, while nanotechnology is one of the fastest growing sectors of the hi-tech economy.

The application of nanotechnology has recently been extended to areas in medicine, biotechnology, materials and process development, energy and the environment.
Colloidal silver is the 66th most abundant element on the Earth, which means Colloidal silver is found at about0.05 ppm in the Earth’s crust.

Mining silver requires the movement of many tons of ore torecover small amounts of the metal.
Nevertheless, Colloidal silver is 10 times more abundant than gold and though silver is sometimes found as a free metal in nature, mostly Colloidal silver is mixed with theores of other metals.
When found pure, Colloidal silver is referred to as “native silver.”

Colloidal silver’s major ores areargentite (silver sulfide, Ag2S) and horn silver (silver chloride, AgCl).
Colloidal silver can also be recovered throughthe chemical treatment of a variety of ores.

Colloidal silvers have unique optical properties because they support surface plasmons.
At specific wavelengths of light the surface plasmons are driven into resonance and strongly absorb or scatter incident light.

This effect is so strong that Colloidal silver allows for individual nanoparticles as small as 20 nm in diameter to be imaged using a conventional dark field microscope.
This strong coupling of metal nanostructures with light is the basis for the new field of plasmonics.

Applications of plasmonic Colloidal silvers include biomedical labels, sensors, and detectors.
Colloidal silver is also the basis for analysis techniques such as Surface Enhanced Raman Spectroscopy (SERS) and Surface Enhanced Fluorescent Spectroscopy.

There are many ways Colloidal silvers can be synthesized; one method is through monosaccharides.
This includes glucose, fructose, maltose, maltodextrin, etc., but not sucrose.

Colloidal silver is also a simple method to reduce silver ions back to Colloidal silvers as it usually involves a one-step process.
There have been methods that indicated that these reducing sugars are essential to the formation of Colloidal silvers.

Many studies indicated that this method of green synthesis, specifically using Cacumen platycladi extract, enabled the reduction of silver.
Additionally, the size of the Colloidal silver could be controlled depending on the concentration of the extract.

The studies indicate that the higher concentrations correlated to an increased number of Colloidal silvers.
Smaller Colloidal silvers were formed at high pH levels due to the concentration of the monosaccharides.

Another method of Colloidal silver synthesis includes the use of reducing sugars with alkali starch and silver nitrate.
The reducing sugars have free aldehyde and ketone groups, which enable them to be oxidized into gluconate.

However, most Colloidal silver isrecovered as a by-product of the refining of copper, lead, gold, and zinc ores.
Colloidal silvers have been explored for their potential in water treatment and purification due to their antimicrobial properties.

The silver ions are bioactive and have broad spectrum antimicrobial properties against a wide range of bacteria.
By controlling the size, shape, surface and agglomeration state of the nanoparticles, specific silver ion release profiles can be developed for a given application.

Colloidal silvers typically have dimensions ranging from 1 to 100 nanometers.
The size and shape of these particles can influence their physical, chemical, and optical properties.

One of the notable features of Colloidal silvers is their strong antibacterial and antimicrobial activity.
The Colloidal silver must have a free ketone group because in order to act as a reducing agent Colloidal silver first undergoes tautomerization.

When inhaled, Colloidal silvers can go deeper into the lungs reaching more sensitive areas.
The most common methods for Colloidal silver synthesis fall under the category of wet chemistry, or the nucleation of particles within a solution.

This nucleation occurs when a Colloidal silver ion complex, usually AgNO3 or AgClO4, is reduced to colloidal Ag in the presence of a reducing agent.
When the concentration increases enough, dissolved metallic Colloidal silver ions bind together to form a stable surface.

The surface is energetically unfavorable when the cluster is small, because the energy gained by decreasing the concentration of dissolved particles is not as high as the energy lost from creating a new surface.
When the cluster reaches a certain size, known as the critical radius, Colloidal silver becomes energetically favorable, and thus stable enough to continue to grow.

This nucleus then remains in the system and grows as more Colloidal silver atoms diffuse through the solution and attach to the surface.
When the dissolved concentration of atomic Colloidal silver decreases enough, it is no longer possible for enough atoms to bind together to form a stable nucleus.

The most common capping ligands are trisodium citrate and polyvinylpyrrolidone (PVP), but many others are also used in varying conditions to synthesize particles with particular sizes, shapes, and surface properties.
There are many different wet synthesis methods, including the use of reducing sugars, citrate reduction, reduction via sodium borohydride, the Colloidal silver mirror reaction, the polyol process, seed-mediated growth, and light-mediated growth.

Each of these methods, or a combination of methods, will offer differing degrees of control over the size distribution as well as distributions of geometric arrangements of the nanoparticle.
A new, very promising wet-chemical technique was found by Elsupikhe et al. (2015).

They have developed a green ultrasonically-assisted synthesis.
Under ultrasound treatment, Colloidal silvers (AgNP) are synthesized with κ-carrageenan as a natural stabilizer.
The reaction is performed at ambient temperature and produces Colloidal silvers with fcc crystal structure without impurities.

The concentration of κ-carrageenan is used to influence particle size distribution of the AgNPs.

The synthesis of Colloidal silvers by sodium borohydride (NaBH4) reduction occurs by the following reaction:
Ag+ + BH4− + 3 H2O → Ag0 +B(OH)3 +3.5 H2

The reduced metal atoms will form nanoparticle nuclei.
Overall, this process is similar to the above reduction method using citrate.
The benefit of using sodium borohydride is increased monodispersity of the final particle population.

The reason for the increased Colloidal silver when using NaBH4 is that it is a stronger reducing agent than citrate.
The impact of reducing agent strength can be seen by inspecting a LaMer diagram which describes the nucleation and growth of nanoparticles.

When Colloidal silver nitrate (AgNO3) is reduced by a weak reducing agent like citrate, the reduction rate is lower which means that new nuclei are forming and old nuclei are growing concurrently.
This is the reason that the citrate reaction has low monodispersity.

Because NaBH4 is a much stronger reducing agent, the concentration of silver nitrate is reduced rapidly which shortens the time during which new nuclei form and grow concurrently yielding a monodispersed population of Colloidal silvers.
Particles formed by reduction must have their surfaces stabilized to prevent undesirable particle agglomeration (when multiple particles bond together), growth, or coarsening.

The driving force for these phenomena is the minimization of surface energy (nanoparticles have a large surface to volume ratio).
This tendency to reduce surface energy in the system can be counteracted by adding species which will adsorb to the surface of the nanoparticles and lowers the activity of the particle surface thus preventing particle agglomeration according to the DLVO theory and preventing growth by occupying attachment sites for metal atoms.

Chemical species that adsorb to the surface of Colloidal silvers are called ligands.

Some of these surface stabilizing species are:
NaBH4 in large amounts, poly(vinyl pyrrolidone) (PVP), sodium dodecyl sulfate (SDS), and/or dodecanethiol.
Once the particles have been formed in solution they must be separated and collected.

There are several general methods to remove nanoparticles from solution, including evaporating the solvent phase or the addition of chemicals to the solution that lower the solubility of the nanoparticles in the solution.
Both methods force the precipitation of the Colloidal silvers.

The polyol process is a particularly useful method because Colloidal silver yields a high degree of control over both the size and geometry of the resulting Colloidal silvers.
At this nucleation threshold, new Colloidal silvers stop being formed, and the remaining dissolved silver is absorbed by diffusion into the growing nanoparticles in the solution.

As the particles grow, other molecules in the solution diffuse and attach to the surface.
This process stabilizes the surface energy of the particle and blocks new Colloidal silver ions from reaching the surface.

The attachment of these capping/stabilizing agents slows and eventually stops the growth of the particle.
In addition, if the aldehydes are bound, Colloidal silver will be stuck in cyclic form and cannot act as a reducing agent.
For example, glucose has an aldehyde functional group that is able to reduce Colloidal silver cations to silver atoms and is then oxidized to gluconic acid.

The reaction for the sugars to be oxidized occurs in aqueous solutions.
The polyol process is highly sensitive to reaction conditions such as temperature, chemical environment, and concentration of substrates.

Therefore, by changing these variables, various sizes and geometries can be selected for such as quasi-spheres, pyramids, spheres, and wires.
Further study has examined the mechanism for this process as well as resulting geometries under various reaction conditions in greater detail.

Colloidal silvers can be synthesized in a variety of non-spherical (anisotropic) shapes.
Because Colloidal silver, like other noble metals, exhibits a size and shape dependent optical effect known as localized surface plasmon resonance (LSPR) at the nanoscale, the ability to synthesize Ag nanoparticles in different shapes vastly increases the ability to tune their optical behavior.

For example, the wavelength at which LSPR occurs for a nanoparticle of one morphology (e.g. a sphere) will be different if that sphere is changed into a different shape.
This shape dependence allows a Colloidal silver to experience optical enhancement at a range of different wavelengths, even by keeping the size relatively constant, just by changing Colloidal silver shape.
This aspect can be exploited in synthesis to promote change in shape of nanoparticles through light interaction.

The applications of this shape-exploited expansion of optical behavior range from developing more sensitive biosensors to increasing the longevity of textiles.
Colloidal silvers have been shown to have synergistic antibacterial activity with commonly used antibiotics such as; penicillin G, ampicillin, erythromycin, clindamycin, and vancomycin against E. coli and S. aureus.
Furthermore, synergistic antibacterial activity has been reported between Colloidal silvers and hydrogen peroxide causing this combination to exert significantly enhanced bactericidal effect against both Gram negative and Gram positive bacteria.

This antibacterial synergy between Colloidal silvers and hydrogen peroxide can be possibly attributed to a Fenton-like reaction that generates highly reactive oxygen species such as hydroxyl radicals.
Colloidal silvers can prevent bacteria from growing on or adhering to the surface.

This can be especially useful in surgical settings where all surfaces in contact with the patient must be sterile.
Colloidal silvers can be incorporated on many types of surfaces including metals, plastic, and glass.

In medical equipment, Colloidal silver has been shown that Colloidal silvers lower the bacterial count on devices used compared to old techniques.
However, the problem arises when the procedure is over and a new one must be done.

In the process of washing the instruments a large portion of the Colloidal silvers become less effective due to the loss of silver ions.
They are more commonly used in skin grafts for burn victims as the Colloidal silvers embedded with the graft provide better antimicrobial activity and result in significantly less scarring of the victim.
These new applications are direct decedents of older practices that used silver nitrate to treat conditions such as skin ulcers.

Now, Colloidal silvers are used in bandages and patches to help heal certain burns and wounds.
An alternative approach is to use AgNP to sterilise biological dressings (for example, tilapia fish skin) for burn and wound management.
In this method, polyvinylpyrrolidone (PVP) is dissolved in water by sonication and mixed with silver colloid particles.

Active stirring ensures the PVP has adsorbed to the nanoparticle surface.
Centrifuging separates the PVP coated nanoparticles which are then transferred to a solution of ethanol to be centrifuged further and placed in a solution of ammonia, ethanol and Si(OEt4) (TES).
Stirring for twelve hours results in the silica shell being formed consisting of a surrounding layer of silicon oxide with an ether linkage available to add functionality.

Varying the amount of TES allows for different thicknesses of shells formed.
This technique is popular due to the ability to add a variety of functionality to the exposed silica surface.
Colloidal silver have unique physical, chemical and optical properties that are being leveraged for a wide variety of applications.

A resurgence of interest in the utility of Colloidal silver as a broad based antimicrobial agent has led to the development of hundreds of products that incorporate Colloidal silvers to prevent bacterial growth on surfaces and in clothing.
The optical properties of Colloidal silvers are of interest due to the strong coupling of the Colloidal silvers to specific wavelengths of incident light.
This gives them a tunable optical response, and can be utilized to develop ultra-bright reporter molecules, highly efficient thermal absorbers, and nanoscale “antennas” that amplify the strength of the local electromagnetic field to detect changes to the nanoparticle environment.

Colloidal silver is said to be a “key technology of the 21st century”, which is the result of its interdisciplinary nature.
Colloidal silvers are some of the most widely used nanomaterials in commerce, with numerous uses in consumer and medical products.

Workers who produce or use Colloidal silvers are potentially exposed to those materials in the workplace.
Previous authoritative assessments of occupational exposure to silver did not account for particle size.

In studies that involved human cells, Colloidal silvers were associated with toxicity (cell death and DNA damage) that varied according to the size of the particles.
In animals exposed to Colloidal silvers by inhalation or other routes of exposure, silver tissue concentrations were elevated in all organs tested.

Exposure to silver nanomaterials in animals was associated with decreased lung function, inflamed lung tissue, and histopathological (microscopic tissue) changes in the liver and kidney.
In the relatively few studies that compared the effects of exposure to nanoscale or microscale silver, nanoscale particles had greater uptake and toxicity than did microscale particles.

Colloidal silvers of different shapes and sizes are synthesized through chemical, physical, and green methods.
Obtained nanoparticles are generally utilized in the medical industry, catalytic applications, sensors, and special displays.

Colloidal silvers have been an important component of various different applications for a very long time.
Colloidal silvers are explored for their potential use in food packaging materials due to their antimicrobial properties.

They may help extend the shelf life of packaged foods by inhibiting the growth of microorganisms.
Colloidal silvers are utilized in the fabrication of solar cells and other photovoltaic devices.

They can enhance light absorption and electron transport within the devices, contributing to improved efficiency.
In the field of medicine, Colloidal silvers are being investigated for their use in photothermal therapy.

When exposed to specific wavelengths of light, they can generate heat, which may be utilized for targeted treatment of cancer cells.
Some studies suggest that Colloidal silvers may exhibit antiviral properties, making them a subject of interest in the development of antiviral drugs or materials.

Colloidal silvers can be incorporated into textile coatings to provide UV protection.
This is particularly useful in outdoor clothing and fabrics to shield against harmful ultraviolet radiation.

Colloidal silvers are employed in the production of conductive inks for printed electronics and flexible displays.
Their conductivity and compatibility with flexible substrates make them valuable in these applications.

Due to their antimicrobial properties, Colloidal silvers are explored for use in air and water purification systems.
They can help eliminate or reduce the presence of harmful microorganisms.

Colloidal silvers are incorporated into sensors for various applications, including gas sensors, biosensors, and environmental sensors.
Their unique optical and electrical properties make them suitable for sensing platforms.

Colloidal silvers may be included in certain cosmetic and personal care products for their potential antibacterial and preservative properties.
In the medical field, efforts are made to develop biocompatible Colloidal silvers for applications such as drug delivery and imaging.

These nanoparticles aim to interact safely with biological systems.
Colloidal silvers are used in the formulation of conductive inks for printed radio-frequency identification (RFID) tags.

This application is relevant in the field of logistics and inventory tracking.
The capping agent is also not present when heated.

Colloidal silvers can become airborne easily due to their size and mass.
Colloidal silver is located in group 11 (IB) of period 5, between copper (Cu) above Colloidal silver in period 4 andgold (Au) below it in period 6.

Colloidal silver products have not undergone safety studies and are not recommended by the FDA.
In addition, there have been serious adverse effects such as seizures, psychosis, neuropathy (burning pain usually in hands and feet), and even deaths reported from colloidal silver use.
Because there is no information to suggest colloidal silver is effective for the treatment of any condition, the risks of using Colloidal silver outweigh the benefits.

Colloidal silver is only slightly harder than gold.
Colloidal silver is insoluble in water, but it will dissolve in hot concentrated acids.

Freshly exposed silver has a mirror-like shine thatslowly darkens as a thin coat of tarnish forms on Colloidal silver surface (from the small amount ofnatural hydrogen sulfide in the air to form silver sulfide, AgS).
Colloidal silvers can also be produced via γ-irradiation using polysaccharide alginate as stabilizer, and photochemical reduction.

A relatively new biological method can be used to make gold Colloidal silvers by dissolving gold in sodium chloride solution, using natural chitosan without any stabilizer and reductant.
Colloidal silver’s modern chemical symbol (Ag) is derived from its Latin word argentum, which means silver.
The word “silver” is from the Anglo-Saxon world “siolfor.”

Ancients who first refined and worked with Colloidal silver used the symbol of a crescent moon to represent the metal.
Colloidal silvers can undergo coating techniques that offer a uniform functionalized surface to which substrates can be added.
When the Colloidal silver is coated, for example, in silica the surface exists as silicic acid.

Colloidal silvers can thus be added through stable ether and ester linkages that are not degraded immediately by natural metabolic enzymes.
Recent chemotherapeutic applications have designed anti cancer drugs with a photo cleavable linker, such as an ortho-nitrobenzyl bridge, attaching Colloidal silver to the substrate on the nanoparticle surface.
The low toxicity Colloidal silver complex can remain viable under metabolic attack for the time necessary to be distributed throughout the bodies systems.

If a cancerous tumor is being targeted for treatment, ultraviolet light can be introduced over the tumor region.
The electromagnetic energy of the light causes the photo responsive linker to break between the drug and the nanoparticle substrate.
The drug is now cleaved and released in an unaltered active form to act on the cancerous tumor cells.

Advantages anticipated for this method is that the drug is transported without highly toxic compounds, the drug is released without harmful radiation or relying on a specific chemical reaction to occur and the drug can be selectively released at a target tissue.
Colloidal silver is somewhat rare and is considered a commercially precious metal with many uses.
Pure Colloidal silver is too soft and usually too expensive for many commercial uses, and thus Colloidal silver isalloyed with other metals, usually copper, making it not only stronger but also less expensive.

The purity of Colloidal silver is expressed in the term “fitness,” which describes the amount of silverin the item.
Fitness is just a multiple of 10 times the Colloidal silver content in an item.
For instance,sterling Colloidal silver should be 93% (or at least 92.5%) pure silver and 7% copper or some othermetal.

The fitness rating for pure Colloidal silver is 1000.
Therefore, the rating for sterling Colloidal silver is 930,and most sliver jewelry is rated at about 800.
This is another way of saying that most Colloidal silver jewelry is about 20% copper or other less valuable metal.

Many people are fooled when they buy Mexican or German silver jewelry, thinking theyare purchasing a semiprecious metal.
These forms of “Colloidal silver” jewelry go under many names,including Mexican silver, German silver, Afghan silver, Austrian silver, Brazilian silver, Nevadasilver, Sonara silver, Tyrol silver, Venetian silver, or just the name “silver” with quotes aroundit.
None of these jewelry items, under these names or under any other names, contain anysilver.

These metals are alloys of copper, nickel, and zinc.
A transition metal that occurs native and as the sulfide (Ag2S) and chloride (AgCl).
Colloidal silver is extracted as a by-product in refining copper and lead ores.

Colloidal silver darkens in air due to the formation of silver sulfide.
Colloidal silver is used in coinage alloys, tableware, and jewelry.
Of all the metals, Colloidal silver isthe best conductor of heat and electricity.

This property determines much of Colloidal silver commercialusefulness.
Colloidal silver is melting point is 961.93°C.
Colloidal silver boiling point is 2,212°C.
Colloidal silver density is10.50 g/cm3.

The beneficial effects of Colloidal silvers are also manifested in their action against inflammation and suppression of tumor growth.
Colloidal silvers can induce apoptosis, or programmed cell death, in tumor cells.

The activity of Colloidal silvers in the human body can be used for imaging of living cells and tissues, both in diagnosis and research.
Colloidal silvers are also used in biosensors, can detect tumor cells, and have potential in phototherapy, where they absorb radiation, heat up and selectively eliminate selected cells.

Colloidal silvers are highly commercial due to properties such as good conductivity, chemical stability, catalytic activity, and their antimicrobial activity.
Due to their properties, they are commonly used in medical and electrical applications.

Colloidal silver compounds are used in photography symbol:
Ag
m.p. 961.93°C
b.p. 2212°C
r.d. 10.5 (20°C)
p.n. 47
r.a.m. 107.8682.

Synthetic protocols for Colloidal silver production can be modified to produce Colloidal silvers with non-spherical geometries and also to functionalize nanoparticles with different materials, such as silica.
Creating Colloidal silvers of different shapes and surface coatings allows for greater control over their size-specific properties.
There are instances in which Colloidal silvers and colloidal silver are used in consumer goods.

Samsung for example claimed that the use of Colloidal silvers in washing machines would help to sterilize clothes and water during the washing and rinsing functions, and allow clothes to be cleaned without the need for hot water.
The nanoparticles in these appliances are synthesized using electrolysis.
Through electrolysis, Colloidal silver is extracted from metal plates and then turned into Colloidal silvers by a reduction agent.

This method avoids the drying, cleaning, and re-dispersion processes, which are generally required with alternative colloidal synthesis methods.
Importantly, the electrolysis strategy also decreases the production cost of Ag nanoparticles, making these washing machines more affordable to manufacture.
Colloidal silver can form explosive salts with azidrine.

Ammonia forms explosive compounds with gold, mercury, or Silver.
Acetylene and ammonia can form explosive Silver salts in contact with Ag.
Dust may form explosive mixture with air.

Powders are incompatible with strong oxidizers (chlorates, nitrates, peroxides, permanganates, perchlorates, chlorine, bromine, fluorine, etc.); contact may cause fires or explosions.
Keep away from alkaline materials, strong bases, strong acids, oxoacids, epoxides May react and/or form dangerous or explosive compounds, with acetylene, ammonia, halogens, hydrogen peroxide; bromoazide, concentrated or strong acids, oxalic acid, tartaric acid, chlorine trifluoride, ethyleneimine.
Factors contributing toward Colloidal silvers market growth include rise in demand for Colloidal silvers for anti-microbial applications and increase in demand from electronics sector.

Colloidal silvers are investigated in the field of tissue engineering for their potential to support cell growth and enhance the properties of scaffolds used in regenerative medicine.
In marine applications, Colloidal silvers are used in anti-fouling coatings on ship hulls.
They help prevent the accumulation of marine organisms, reducing drag and improving fuel efficiency.

Colloidal silvers are explored for their potential use in pesticide formulations.
Their antimicrobial properties could be leveraged for crop protection and pest control.
Colloidal silvers are employed in the development of electrochemical sensors for detecting various analytes.

These sensors find applications in fields such as environmental monitoring and healthcare.
Colloidal silvers can be utilized in the fabrication of sensors for detecting hydrogen peroxide.
This application is relevant in fields such as clinical diagnostics and industrial processes.

Colloidal silvers are studied for their potential application in energy storage devices, such as batteries and supercapacitors, where their unique properties can influence performance.
An early, and very common, method for synthesizing Colloidal silvers is citrate reduction.
This method was first recorded by M. C. Lea, who successfully produced a citrate-stabilized silver colloid in 1889.

Citrate reduction involves the reduction of a silver source particle, usually AgNO3 or AgClO4, to colloidal silver using trisodium citrate, Na3C6H5O7.
The synthesis is usually performed at an elevated temperature (~100 °C) to maximize the monodispersity (uniformity in both size and shape) of the particle.
In this method, the citrate ion traditionally acts as both the reducing agent and the capping ligand, making Colloidal silver a useful process for AgNP production due to its relative ease and short reaction time.

However, the silver particles formed may exhibit broad size distributions and form several different particle geometries simultaneously.
The addition of stronger reducing agents to the reaction is often used to synthesize particles of a more uniform size and shape.

Colloidal silver mirror reaction involves the conversion of Colloidal silver nitrate to Ag(NH3)OH.
Ag(NH3)OH is subsequently reduced into colloidal silver using an aldehyde containing molecule such as a sugar.

The silver mirror reaction is as follows:
2(Ag(NH3)2)+ + RCHO + 2OH− → RCOOH + 2Ag + 4NH3.

The size and shape of the Colloidal silvers produced are difficult to control and often have wide distributions.
However, this method is often used to apply thin coatings of Colloidal silver particles onto surfaces and further study into producing more uniformly sized nanoparticles is being done.

The biological synthesis of Colloidal silvers has provided a means for improved techniques compared to the traditional methods that call for the use of harmful reducing agents like sodium borohydride.
Many of these methods could improve their environmental footprint by replacing these relatively strong reducing agents.
The commonly used biological methods are using plant or fruit extracts, fungi, and even animal parts like insect wing extract.

The problems with the chemical production of Colloidal silvers is usually involves high cost and the longevity of the particles is short lived due to aggregation.
The harshness of standard chemical methods has sparked the use of using biological organisms to reduce silver ions in solution into colloidal Colloidal silvers.
Colloidal silvers can provide a means to overcome MDR.

In general, when using a targeting agent to deliver nanocarriers to cancer cells, Colloidal silver is imperative that the agent binds with high selectivity to molecules that are uniquely expressed on the cell surface.
Hence NPs can be designed with proteins that specifically detect drug resistant cells with overexpressed transporter proteins on their surface.
Colloidal silver a pitfall of the commonly used nano-drug delivery systems is that free drugs that are released from the nanocarriers into the cytosol get exposed to the MDR transporters once again, and are exported.

To solve this, 8 nm Colloidal silvers were modified by the addition of trans-activating transcriptional activator (TAT), derived from the HIV-1 virus, which acts as a cell-penetrating peptide (CPP).
Generally, AgNP effectiveness is limited due to the lack of efficient cellular uptake; however, CPP-modification has become one of the most efficient methods for improving intracellular delivery of Colloidal silvers.
Once ingested, the export of the AgNP is prevented based on a size exclusion.

The concept is simple: the nanoparticles are too large to be effluxed by the MDR transporters, because the efflux function is strictly subjected to the size of Colloidal silver substrates, which is generally limited to a range of 300-2000 Da.
Thereby the Colloidal silvers remain insusceptible to the efflux, providing a means to accumulate in high concentrations.
In addition, increased demand from pharmaceutical industry as Colloidal silver is used in the field of biomarkers, biosensors, implant technology, tissue engineering, nanorobots & nanomedicine, and image enhancement devices.

The bactericidal activity of Colloidal silvers is due to the silver cations, which have the potential to disrupt physiological activity of microbes such as bacteria.
Growth in concerns regarding environmental impact and toxicity of Colloidal silvers is hindering the Colloidal silvers market.
Furthermore, high Colloidal silver product prices are likely to hinder market growth during the forecast period.

On the contrary, rise in trend of biological synthesis method is expected to create lucrative opportunities for the market during the forecast period.
Colloidal silvers are investigated for their potential role in drug delivery systems.
They can be designed to carry therapeutic agents and release them in a controlled manner, offering targeted drug delivery.

Colloidal silvers can exhibit photocatalytic activity, which means they can accelerate chemical reactions under light exposure.
This property is explored in applications like environmental remediation and water treatment.
In the field of electronics, Colloidal silvers are used to create flexible and transparent conductive films.

These films have applications in flexible electronics, touch screens, and electronic displays.
Colloidal silvers are integrated into textiles to impart anti-odor properties by inhibiting the growth of odor-causing bacteria.
This application is common in sportswear and undergarments.

Colloidal silvers are incorporated into various nanocomposite materials to enhance their mechanical, thermal, and electrical properties.
These nanocomposites find applications in materials science and engineering.
Some studies explore the use of Colloidal silvers as contrast agents in magnetic resonance imaging (MRI) for medical diagnostics.

Colloidal silvers can be very effective against fungal infections that are otherwise difficult to treat.
This is of great importance for patients with weakened immunity who are especially vulnerable to fungi.
These Colloidal silvers not only suppress pathogenic fungi, including yeasts, but also fungi that grow in households, such as various mold species.

Colloidal silver reacts violently with chlorine trifluoride (in the presence of carbon).
Bromoazide explodes on contact with Silver foil.
Acetylene forms an insoluble acetylide with Silver.

When Colloidal silver is treated with nitric acid in the presence of ethyl alcohol, Silver fulminate, which can detonated may be formed.
Ethyleneimine forms explosive compounds with Colloidal silver, hence Silver solder should not be used to fabricate equipment for handling ethyleneimine.
Finely divided Silver and strong solutions of hydrogen peroxide may explode.

Colloidal silvers optical properties are also dependent on the nanoparticle size.
Smaller nanospheres absorb light and have peaks near to 400 nm, and larger nanoparticles have increased scattering to gives peaks that broaden and shift towards longer wavelengths.
Larger shifts into the infrared region of the electromagnetic spectrum are achieved by changing the nanoparticles shape to rods or plates.

Colloidal silvers can be synthesized by a variety of different techniques that are chemical, physical or biological.
The most common method for making colloidal gold is by a chemical citrate reduction method, but gold nanoparticles can also be grown by being encapsulated and immersed in polyethylene glycol dendrimers before being reduced by formaldehyde under near infra-red treatment.

Uses of Colloidal silver:
Because silver has antibacterial properties, colloidal silver was used to treat skin infections before antibiotics were available.
More recently, colloidal silver has been used to treat a variety of infections, including COVID-19, to boost the immune system, and decrease inflammation.

Colloidal silver is important to know, there is no clinical evidence to support the efficacy of colloidal silver and the U.S. Food and Drug Administration (FDA) recommends against Colloidal silver use.
There are some topical silver creams and other topical products that are approved by the FDA to prevent and treat infections.

These are different than colloidal silver.
Several of Colloidal silver compounds were not only useful but even essential for the predigital photographicindustry.

Colloidal silver has no known active biological role in the human body, and the levels of Ag+ within the body are below detection limits.
The metal has been used for thousands of years mainly as ornamental metal or for coins.
Furthermore, Colloidal silver has been used for medicinal purposes since 1000 BC.

Colloidal silver was known that water would keep fresh if it was kept in a silver pitcher; for example, Alexander the Great (356–323 BC) used to transport his water supplies in Colloidal silver pitchers during the Persian War.
A piece of Colloidal silver was also used, for example, to keep milk fresh, before any household refrigeration was developed.
In 1869, Ravelin proved that Colloidal silver in low doses acts as an antimicrobial.

Around the same time, the Swiss botanist showed that already at very low concentration Ag+ can kill the green algae spirogyra in fresh water.
This work inspired the gynaecologist Crede to recommended use of AgNO3 drops on new born children with conjunctivitis.

Using Colloidal silvers for catalysis has been gaining attention in recent years.
Although the most common applications are for medicinal or antibacterial purposes, Colloidal silvers have been demonstrated to show catalytic redox properties for dyes, benzene, and carbon monoxide.

Other untested compounds may use Colloidal silvers for catalysis, but the field is not fully explored.
Colloidal silvers supported on aerogel are advantageous due to the higher number of active sites.

Several of the Colloidal silver salts, such as silver nitrate, silver bromide, and silverchloride, are sensitive to light and, thus, when mixed with a gel-type coating on photographicfilm or paper, can be used to form light images.
Most of the Colloidal silver used in the United Statesis used in photography.

Photochromic (transition) eyeglasses that darken as they are exposed to sunlight have asmall amount of silver chloride imbedded in the glass that forms a thin layer of metallic silverthat darkens the lens when struck by sunlight.
This photosensitive chemical activity is thenreversed when the eyeglasses are removed from the light.

Colloidal silver reversal results from asmall amount of copper ions placed in the glass.
This reaction is repeated each time the lensesare exposed to sunlight.

This malleable white metal is found as argentite (Ag2S) and horn silver (AgCl) or in lead and copper ore.
Colloidal silvers coated with a thin layer of elemental silver and fumed with iodine were used by Niépce and Daguerre.

Aside from the heliograph and physautotype, Colloidal silver halide compounds were the basis of all photographic processes used in the camera and most of the printing processes during the 19th century.
Colloidal silver are one of the most fascinating, promising and widely used nano materials, particularly for their interesting antibacterial, antiviral and antifungal effects.

However, their potential uses are much wider.
Colloidal silvers are used in antibacterial products, industrial production, catalysis, household products and consumer goods.

Colloidal silver was used to treat infections and wounds before antibiotics became available.
Colloidal silvers are commonly used in biomedical and medical applications due to their antibacterial, antifungal, antiviral, anti-inflammatory, and anti-tumor effects.

Due to their favorable surface-to-volume ratio and crystal structure, nano silver particles are a promising alternative to antibiotics.
They can penetrate bacterial walls and effectively deal with bacterial biofilms and mucous coatings, which are usually well-protected environments for bacteria.

Colloidal silver are one of the most commonly used nanomaterials because of their high electrical conductivity, optical properties, and anti-microbial properties.
The biological activity of Colloidal silvers depends on factors such as particle composition, size distribution, surface chemistry, size; shape, coating/capping, particle morphology, dissolution rate, agglomeration, efficiency of ion release, and particle reactivity in solution.

Colloidal silvers have found a wide range of applications including their use as catalysts, as optical sensors of zeptomole (10−21) concentrations, in textile engineering, in electronics, in optics, as anti-reflection coatings, and most importantly in the medical field as a bactericidal and therapeutic agent.
Colloidal silver is used in the formulation of dental resin composites, in coatings of medical devices, as a bactericidal coating in water filters, as an antimicrobial agent in air sanitizer sprays, pillows, respirators, socks, keyboards, detergents, soaps, shampoos, toothpastes, washing machines and many other consumer products, in bone cement and in many wound dressings.

Colloidal silvers are also commonly used in colloidal solutions to enhance Raman spectroscopy.
The size and shape of nanoparticles have been shown to affect the enhancement.

Colloidal silvers are the most common shape of nanoparticles, but other shapes such as nanostars, nanocubes, nanorods and nanowires can be produced through a polymer-mediated polyol process.
Colloidal silvers can also be capped or hollowed using various chemical methods.
For a more accurate spread for detection, nanoparticles can be deposited or spin-coated onto multiple surfaces.

Coating is metallic silver and Colloidal silver salts are popularly used in medicinal purposes and in medical devices.
Colloidal silver is a precious metal, used in jewelryand ornaments Other applications includeColloidal silver use in photography, electroplating, dentalalloys, high-capacity batteries, printed circuits,coins, and mirrors.

Colloidal silver is stable in air, and it is utilized in reflecting mirrors.
The film vacuum evaporated on a quartz plate with the thickness of 2–55 nm shows the transmittance maximum at λ: 321.5 nm and works as a narrow band filter.

The name Colloidal silver is derived from the Saxon word ‘siloflur’, which has been subsequently transformed into the German word ‘Silabar’ followed by ‘Silber’ and the English word ‘silver’.
Romans called the element ‘argentum’, and this is where the symbol Ag derives from.

Colloidal silver is widely distributed in nature.
Colloidal silver can be found in its native form and in various ores such as argentite (Ag2S), which is the most important ore mineral for silver, and horn silver (AgCl).

The principal sources of silver are copper, copper–nickel, gold, lead and lead–zinc ores, which can be mainly found in Peru, Mexico, China and Australia.
Colloidal silver and its alloys and compounds have numerous applications.

As a precious metal, Colloidal silver is used in jewelry.
Also, one of its alloys, sterling Colloidal silver, containing 92.5 weight % silver and 7.5 weight % copper, is a jewelry item and is used in tableware and decorative pieces.

The metal and Colloidal silver copper alloys are used in coins.
Colloidal silvers are widely recognized for their strong antimicrobial properties.
They are incorporated into products such as wound dressings, bandages, and medical devices to prevent bacterial and microbial growth.

In medical diagnostics, Colloidal silvers are explored for their use as contrast agents in imaging techniques such as magnetic resonance imaging (MRI).
Their unique properties contribute to enhanced imaging quality.

Colloidal silvers are investigated for drug delivery applications.
They can be designed to carry therapeutic agents and release them in a controlled manner, offering targeted drug delivery.

Colloidal silvers are integrated into textiles and clothing to provide antimicrobial and anti-odor properties.
This application is common in sportswear, undergarments, and fabrics used in healthcare settings.

Colloidal silvers are used in a variety of consumer products, including socks, kitchenware, and appliances, to impart antimicrobial properties and reduce the growth of bacteria that cause odors.
Colloidal silvers are employed in water treatment technologies to eliminate or reduce the presence of harmful microorganisms.

They can be part of filters, coatings, or solutions used for purifying water.
Due to their antimicrobial properties, Colloidal silvers are explored for use in food packaging materials.

They can help extend the shelf life of packaged foods by inhibiting the growth of microorganisms.
Colloidal silvers are used in the electronics industry to create conductive inks for printed electronics, flexible displays, and sensors.

Their electrical conductivity and compatibility with flexible substrates make them valuable in these applications.
Colloidal silvers exhibit catalytic activity and are employed in various catalytic reactions.

This has implications for applications in chemical synthesis and industrial processes.
In the medical field, Colloidal silvers are investigated for their use in photothermal therapy.

When exposed to specific wavelengths of light, they can generate heat, which may be utilized for targeted treatment of cancer cells.
Colloidal silvers may be included in certain cosmetic and personal care products for their potential antibacterial and preservative properties.

In the electronics industry, Colloidal silvers are used to create flexible and transparent conductive films, with applications in flexible electronics, touch screens, and electronic displays.
Colloidal silvers can exhibit photocatalytic activity, accelerating chemical reactions under light exposure.

This property is explored in applications like environmental remediation and water treatment.
Due to their antimicrobial properties, Colloidal silvers are employed in air purification systems to help eliminate or reduce the presence of harmful microorganisms.

Colloidal silvers find applications in various biomedical areas, including tissue engineering, biosensors, and the development of biocompatible materials.
Colloidal silvers are utilized in coatings for materials like glass and plastics to provide UV-blocking properties.

This is particularly important in products such as sunglasses, protective eyewear, and sunscreens.
In dentistry, Colloidal silvers are incorporated into dental materials such as composites and coatings to provide antimicrobial properties and reduce the risk of bacterial infections.

Colloidal silvers are being studied for potential applications in cancer treatment.
Their unique properties, including their ability to generate heat under light exposure, make them candidates for targeted cancer therapy.

Colloidal silvers are used in the production of transparent conductive films for solar cells.
These films enhance light absorption and electron transport within the solar cells, contributing to improved efficiency.

In electronics manufacturing, Colloidal silvers are employed in the fabrication of flexible printed circuit boards (FPCBs).
Their use supports the development of flexible and bendable electronic devices.

Colloidal silvers can be incorporated into coatings for eyewear and surfaces to provide anti-fog properties.
This is particularly beneficial in applications where clear visibility is essential.

Colloidal silvers are integrated into smart textiles, enabling the development of fabrics with electronic and sensing capabilities.
These textiles find applications in wearable technology and healthcare monitoring.

Colloidal silvers are studied for potential applications in the oil and gas industry, particularly in enhanced oil recovery processes and as additives in drilling fluids.
Colloidal silvers are used in packaging materials for electronic components to provide a conductive barrier and protect against environmental factors such as moisture and corrosion.

Colloidal silvers are utilized in the development of photonic devices, including sensors, waveguides, and components for optical communication systems.
Colloidal silvers are added to heat transfer fluids to enhance their thermal conductivity.

This is relevant in applications where efficient heat transfer is crucial, such as in cooling systems.
Colloidal silvers can be incorporated into 3D printing materials, allowing the production of conductive and functional 3D-printed objects for electronic and sensing applications.

Colloidal silvers are explored for their potential role in soil remediation, assisting in the removal of contaminants and pollutants from soil environments.
Colloidal silvers can be added to construction materials such as concrete to impart antimicrobial properties and reduce the growth of bacteria on surfaces.

Colloidal silver-copper brazing alloys and solders have many applications.
They are used in automotive radiators, heat exchangers, electrical contacts, steam tubes, coins, and musical instruments.
Some other uses of Colloidal silver metal include its applications as electrodes, catalysts, mirrors, and dental amalgam.

Colloidal silver is used as a catalyst in oxidation-reductions involving conversions of alcohol to aldehydes, ethylene to ethylene oxide, and ethylene glycol to glyoxal.
Colloidal silver has a multitude of uses and practical applications both in Colloidal silver elemental metallic formand as a part of its many compounds.

Colloidal silver is excellent electrical conductivity makes it ideal for usein electronic products, such a computer components and high-quality electronic equipment.
Colloidal silver would be an ideal metal for forming the wiring in homes and transmission lines, if Colloidal silver weremore abundant and less expensive.

Metallic Colloidal silver has been used for centuries as a coinage metal in many countries.
Theamount of silver now used to make coins in the United States has been reduced drastically byalloying other metals such as copper, zinc, and nickel with Colloidal silver.

Colloidal silver is used as a catalyst to speed up chemical reactions, in water purification, and inspecial high-performance batteries (cells).
Colloidal silver is high reflectivity makes it ideal as a reflectivecoating for mirrors.

Production Methods of Colloidal silver:
Many processes are known for recovery of Colloidal silver from its ores.
These depend mostly on the nature of the mineral, its silver content, and recovery of other metals present in the ore.

Colloidal silver is usually extracted from high-grade ores by three common processes that have been known for many years.
These are amalgamation, leaching, and cyanidation.

In one amalgamation process, ore is crushed and mixed with sodium chloride, copper sulfate, sulfuric acid, and mercury, and roasted in cast iron pots.
The amalgam is separated and washed.
Silver is separated from Colloidal silver amalgam by distillation of mercury.

In the cyanidation process the ore is crushed and roasted with sodium chloride and then treated with a solution of sodium cyanide.
Colloidal silver forms a stable Colloidal silver cyanide complex, [Ag(CN)2]–.

Adding metallic zinc to this complex solution precipitates Colloidal silver.
One such process, known as the Patera process, developed in the mid 19th century, involves roasting ore with sodium chloride followed by leaching with sodium thiosulfate solution.

Colloidal silver 834 SILVERis precipitated as silver sulfide, Ag2S, by adding sodium sulfide to the leachate.
In the Clandot process, leaching is done with ferric chloride solution.

Addition of zinc iodide precipitates Colloidal silver iodide, AgI.
AgI is reduced with zinc to obtain Colloidal silver.

The above processes are applied for extraction of Colloidal silver from high-grade ores.
However, with depletion of these ores, many processes were developed subsequently to extract Colloidal silver from low-grade ores, especially lead, copper, and zinc ores that contain very small quantities of silver.

Low grade ores are concentrated by floatation.
The concentrates are fed into smelters (copper, lead, and zinc smelters).

The concentrates are subjected to various treatments before and after smelting including sintering, calcination, and leaching.
Copper concentrates are calcined for removal of sulfur and smelted in a reverberatory furnace to convert into blister copper containing 99 wt% Cu.

The blister copper is fire-refined and cast into anodes.
The anodes are electrolytically refined in the presence of cathodes containing 99.9% copper.

Insoluble anode sludges from electrolytic refining contain silver, gold, and platinum metals.
Colloidal silver is recovered from the mud by treatment with sulfuric acid.

Base metals dissolve in sulfuric acid leaving Colloidal silver mixed with any gold present in the mud.
Colloidal silver is separated from gold by electrolysis.

Lead and zinc concentrates can be treated in more or less the same manner as copper concentrates.
Sintering lead concentrates removes sulfur and following that smelting with coke and flux in a blast furnace forms impure lead bullion.

The lead bullion is drossed with air and sulfur and softened with molten bullion in the presence of air to remove most impurities other than Colloidal silver and gold.
Copper is recovered from the dross and zinc converts to Colloidal silver oxide and is recovered from blast furnace slag.

The softened lead obtained above also contains some Colloidal silver.
The Colloidal silver is recovered by the Parkes Process.

The Parkes process involves adding zinc to molten lead to dissolve Colloidal silver at temperatures above the melting point of zinc.
On cooling, zinc-silver alloy solidifies, separating from the lead and rising to the top.

The alloy is lifted off and zinc is separated from silver by distillation leaving behind metallic Colloidal silver.
The unsoftened lead obtained after the softening operation contains Colloidal silver in small but significant quantities.

Such unsoftened lead is cast into anode and subjected to electrolytic refining.
The anode mud that is formed adhering to these anodes is removed by scraping.

Colloidal silver contains bismuth, silver, gold, and other impurity metals.
Colloidal silver is obtained from this anode mud by methods similar to the extraction of anode mud from the copper refining process discussed earlier.

If the low–grade ore is a zinc mineral, then zinc concentrate obtained from the flotation process is calcined and leached with water to remove zinc.
Colloidal silver and lead are left in leach residues.

Residues are treated like lead concentrates and fed into lead smelters.
Colloidal silver is recovered from this lead concentrate by various processes described above.

Environmental Fate of Colloidal silver:
Colloidal silver exists in four oxidation states (0,+1,+2,and +3).
Colloidal silver occurs primarily as sulfides with iron, lead, tellurides, and with gold.

Colloidal silver is a rare element, which occurs naturally in its pure form.
Colloidal silver is a white, lustrous, relatively soft, and very malleable metal.
Colloidal silver has an average abundance of about 0.1 ppm in the Earth’s crust and about 0.3 ppm in soils.

History of Colloidal silver:
Slag dumps in Asia Minor and on islands in the Aegean Sea indicate that man learned to separate Colloidal silver from lead as early as 3000 B.C.
Colloidal silver occurs native and in ores such as argentite (Ag2S) and horn silver (AgCl); lead, lead-zinc, copper, gold, and copper-nickel ores are principal sources.

Mexico, Canada, Peru, and the U.S. are the principal Colloidal silver producers in the western hemisphere.
Colloidal silver is also recovered during electrolytic refining of copper.

Commercial fine silver contains at least 99.9% silver.
Purities of 99.999+% are available commercially.

Pure silver has a brilliant white metallic luster.
Colloidal silver is a little harder than gold and is very ductile and malleable, being exceeded only by gold and perhaps palladium.

Pure Colloidal silver has the highest electrical and thermal conductivity of all metals, and possesses the lowest contact resistance.
Colloidal silver is stable in pure air and water, but tarnishes when exposed to ozone, hydrogen sulfide, or air containing sulfur.

The alloys of Colloidal silver are important.
Sterling Colloidal silver is used for jewelry, silverware, etc. where appearance is paramount.

This alloy contains 92.5% silver, the remainder being copper or some other metal.
Colloidal silver is of utmost importance in photography, about 30% of the U.S. industrial consumption going into this application.

Colloidal silver is used for dental alloys.
Colloidal silver is used in making solder and brazing alloys, electrical contacts, and high capacity silver–zinc and silver–cadmium batteries.

Colloidal silver paints are used for making printed circuits.
Colloidal silver is used in mirror production and may be deposited on glass or metals by chemical deposition, electrodeposition, or by evaporation.

When freshly deposited, Colloidal silver is the best reflector of visible light known, but is rapidly tarnishes and loses much of Colloidal silver reflectance.
Colloidal silver is a poor reflector of ultraviolet.

Colloidal silver fulminate (Ag2C2N2O2), a powerful explosive, is sometimes formed during the silvering process.
Colloidal silver iodide is used in seeding clouds to produce rain.

Colloidal silver chloride has interesting optical properties as Colloidal silver can be made transparent.
Colloidal silver also is a cement for glass.
Colloidal silver nitrate, or lunar caustic, the most important silver compound, is used extensively in photography.

While Colloidal silver itself is not considered to be toxic, most of its salts are poisonous.
Natural silver contains two stable isotopes.
Fifty-six other radioactive isotopes and isomers are known.

Colloidal silver compounds can be absorbed in the circulatory system and reduced silver deposited in the various tissues of the body.
A condition, known as argyria, results with a greyish pigmentation of the skin and mucous membranes.

Colloidal silver has germicidal effects and kills many lower organisms effectively without harm to higher animals.
Colloidal silver for centuries has been used traditionally for coinage by many countries of the world.

In recent times, however, consumption of Colloidal silver has at times greatly exceeded the output.
In 1939, the price of silver was fixed by the U.S. Treasury at 71￠/troy oz., and at 90.5￠/troy oz. in 1946.

In November 1961 the U.S. Treasury suspended sales of nonmonetized Colloidal silver, and the price stabilized for a time at about $1.29, the melt-down value of silver U.S. coins.
The Coinage Act of 1965 authorized a change in the metallic composition of the three U.S. subsidiary denominations to clad or composite type coins.

This was the first change in U.S. coinage since the monetary system was established in 1792.
Clad dimes and quarters are made of an outer layer of 75% Cu and 25% Ni bonded to a central core of pure Cu.

The composition of the oneand five-cent pieces remains unchanged.
One-cent coins are 95% Cu and 5% Zn.
Earlier subsidiary coins of 90% Ag and 10% Cu officially were to circulate alongside the clad coins; however, in practice they have largely disappeared (Gresham’s Law), as the value of the silver is now greater than their exchange value.

Colloidal silver coins of other countries have largely been replaced with coins made of other metals.
On June 24, 1968, the U.S. Government ceased to redeem U.S. Silver Certificates with silver.
The price of Colloidal silver in 2001 was only about four times the cost of the metal about 150 years ago.

This has largely been caused by Central Banks disposing of some of their silver reserves and the development of more productive mines with better refining methods.
Also, Colloidal silver has been displaced by other metals or processes, such as digital photography.

Safety Profile of Colloidal silver:

Human systemic effects by inhalation: skin effects.
The acute toxicity of silver metal is low.
The acute toxicity of soluble silver compounds depends on the counterion and must be evaluated case by case.

For example, silver nitrate is strongly corrosive and can cause burns and permanent damage to the eyes and skin.
Chronic exposure to silver or silver salts can cause a local or generalized darkening of the mucous membranes, skin, and eyes known as argyria.
The other chronic effects of silver compounds must be evaluated individually.

Although Colloidal silvers are widely used in a variety of commercial products, there has only recently been a major effort to study their effects on human health.
Inhalation of dusts can cause argyrosis.
Questionable carcinogen with experimental tumorigenic data.

Flammable in the form of dust when exposed to flame or by chemical reaction with C2H2, NH3, bromoazide, ClF3 ethyleneimine, H2O2, oxalic acid, H2SO4, tartaric acid.
Incompatible with acetylene, acetylene compounds, aziridine, bromine azide, 3-bromopropyne, carboxylic acids, copper + ethylene glycol, electrolytes + zinc, ethanol + nitric acid, ethylene oxide, ethyl hydroperoxide, ethyleneimine, iodoform, nitric acid, ozonides, peroxomonosulfuric acid, peroxyformic acid.

Properties of Colloidal silver:
Melting point: 960 °C(lit.)
Boiling point: 2212 °C(lit.)
Density: 1.135 g/mL at 25 °C
vapor density: 5.8 (vs air)
vapor pressure: 0.05 ( 20 °C)
refractive index: n20/D 1.333
Flash point: 232 °F
storage temp.: 2-8°C
solubility: H2O: soluble
form: wool
color: Yellow
Specific Gravity: 10.49
Odor: Odorless
Resistivity: 1-3 * 10^-5 Ω-cm (conductive paste) &_& 1.59 μΩ-cm, 20°C
Water Solubility: insoluble
Sensitive: Light Sensitive
Merck: 13,8577

Colloidal silica is a surface-modified synthetic amorphous silica that is differentiated from standard synthetic amorphous silica (e.g Colloidal silicon dioxide) in having its surface-based silanol groups bonded to dimethyl silyl groups making it hydrophobic in character.
Colloidal silica occurs as a light, fine, white or almost white amorphous powder, not wettable by water.
Colloidal silica refers to a suspension of fine, solid particles of silicon dioxide (SiO2) in a liquid medium.

CAS Number: 112945-52-5
Molecular Formula: O2Si
Molecular Weight: 60.08
EINECS Number: 231-545-4

SILICON DIOXIDE, Silica, Dioxosilane, Quartz, 7631-86-9, Silica gel, Cristobalite, Silicic anhydride, Tridymite, 14808-60-7, Sand, 112945-52-5, 61790-53-2, 112926-00-8, KIESELGUHR, Diatomaceous silica, Wessalon, Aerosil, Silicon(IV) oxide, Zorbax sil, 60676-86-0, Silica, amorphous, 14464-46-1, Dicalite, Ludox, Nyacol, Amorphous silica, QUARTZ (SIO2), Cristobalite (SiO2), Cab-O-sil, Sillikolloid, Extrusil, Santocel, Sipernat, Superfloss, Acticel, Carplex, Neosil, Neosyl, Porasil, Silikil, Siloxid, Zipax, Aerosil-degussa, Silicon oxide, Aerosil 380, Synthetic amorphous silica, Quartz sand, Rose quartz, Silica particles, 91053-39-3, Cab-o-sil M-5, Silica, fumed, Snowtex O, Silica, colloidal, Tokusil TPLM, Dri-Die, SILICA, VITREOUS, Manosil vn 3, Colloidal silicon dioxide, Ultrasil VH 3, Ultrasil VN 3, Aerosil bs-50, Carplex 30, Carplex 80, Snowtex 30, Zeofree 80, Aerosil K 7, Cabosil N 5, Syton 2X, Amorphous silica gel, Positive sol 232, Siliziumdioxid, Aerogel 200, Aerosil 300, Chalcedony, Diatomite, Ludox hs 40, Silanox 101, Silica (SiO2), Vitasil 220, Agate, Positive sol 130M, Silica vitreous, Silicon dioxide (amorphous), Aerosil A 300, Aerosil E 300, Aerosil M-300, colloidal silica, Fused silica, Quartz glass, Silica slurry, Silicon dioxide, fumed, Silicone dioxide, 68855-54-9, Nalfloc N 1050, Quso 51, Silica, amorphous fused, Nalco 1050, Quso G 30, Hydrophobic silica 2482, Kieselsaeureanhydrid, Min-U-Sil, 15468-32-3, SiO2, CCRIS 3699, Silica Gel, 40-63 Micron Particles, Silica aerogel, (SiO2)n, UNII-ETJ7Z6XBU4, ETJ7Z6XBU4, Silicon Dioxide, Amorphous, Silica 2482, hydrophobic, Silicon dioxide, chemically prepared, EINECS 231-545-4, CAB-O-SIL N-70TS, EPA Pesticide Chemical Code 072605, CI 7811, Aerosil 200, 99439-28-8, CHEBI:30563, AI3-25549, Crystalline silica, N1030, U 333, Silica gel 60, 230-400 mesh, Glass, Silicon dioxide, colloidal, 15723-40-7, ENT 25,550, [SiO2], Silica, crystalline - fused, Silicagel, Silica gel, pptd.,cryst.-free, 13778-37-5, 13778-38-6, 17679-64-0, Christensenite, Crystoballite, Silica gel desiccant, indicating, Celite, INS-551, Calcined diatomite, MFCD00011232, MFCD00217788, Silica, amorphous,fumed, cryst.-free, Silica, mesostructured, Amethyst, Aquafil, Cataloid, Crysvarl, Flintshot, Nalcoag, Novaculite, Silikill, Vulkasil, Cherts, Snowit, Imsil, Metacristobalite, Quartz silica, alpha-Quartz, Fossil flour, Fumed silica, Quartz dust, Rock crystal, Silica dust, White carbon, SIMETHICONE COMPONENT SILICON DIOXIDE, Chromosorb P, Tiger-eye, E-551, Vulkasil S, Celite superfloss, Cristobalite dust, Corasil II, Silver bond B, Cab-O-sperse, alpha-Cristobalite, alpha-Crystobalite, Gold bond R, (SiO2), Cabosil st-1, Silica Standard: SiO2 @ 100 microg/mL in H2O, Sil-Co-Sil, Silica Standard: SiO2 @ 1000 microg/mL in H2O, Siderite (SiO2), Tridymite 118, Cab-O-grip II, Tridimite [French], HI-Sil, Amorphous silica dust, Silicon Oxide Hollow Nanospheres, Nyacol 830, Sibelite M 3000, Sibelite M 4000, Sibelite M 6000, Quazo puro [Italian], SILICA, AMORPHOUS (IARC), SILICA, AMORPHOUS [IARC], Caswell No. 734A, Sicron F 300, Sikron F 100, Spectrosil, Accusand, Coesite, Fuselex, Nalcast, Nyacol 1430, Optocil, Quartzine, Quarzsand, Rancosil, Suprasil, Tridimite, Siltex, Vitreous quartz, Vitreous silica, Tridymite dust, W 12 (Filler), beta-Quartz, Fused quartz, MIN-U-sil alpha quartz, Quartz-beta, Amorphous quartz, Dri-Die insecticide 67, Quazo puro, Silica, amorphous, fumed, Vitrified silica, Pyrogenic colloidal silica, Silica, fused, Suprasil W, Vitreosil IR, Borsil P, Dioxide, Silicon, Silane, dioxo-, Crystallized silicon dioxide, Optocil (quartz), CP-SilicaPLOT, Sand, Sea, Silicon oxide, di- (sand), Quarzsand [German], S-Col, Admafine SO 25H, Admafine SO 25R, Admafine SO 32H, Admafine SO-C 2, Admafine SO-C 3, Cristobalite asbestos, Keatite (SiO2), Sg-67, Tridymite (SiO2), Fumed silica, crystalline-free, Stishovite (SiO2), ED-C (silica), Fuselex ZA 30, As 1 (silica), CCRIS 2475, DQ12, Agate (SiO2), Celite 545, Fumed synthetic amorphous silica, Silica, crystalline - tridymite, FB 5 (silica), Fuselex RD 120, Corning 7940, Microcrystalline quartz, Synthetic amorphous silica, fumed, Denka F 90, Denka FB 30, Denka FB 44, Denka FB 74, Dri-Die 67, Silica gel spherical, 40-75 mum particle size, WGL 300, Cryptocrystalline quartz, FB 20 (silica), Elsil 100, F 44 (filler), D & D, SF 35, Elsil BF 100, F 125 (silica), F 160 (silica), Fuselex RD 40-60, Silica, amorphous, fused, Silica; Silica colloidal anhydrous; Silicium dioxide, EINECS 238-455-4, EINECS 238-878-4, EINECS 239-487-1, 43-63C, HK 400, TGL 16319, Silica, crystalline quartz, Silicon dioxide (vitreous), Silica, amorphous, fumed, cryst.-free, Silica, crystalline, quartz, Silica, crystalline: quartz, tripolite, GP 7I, Precipitated amorphous silica, Chrysoprase, Ronasphere, Silica, crystalline tridymite, Speriglass, Carneol, Citrine, Kieselgel, NaturasilScars, Sandstone, Silica, crystalline - quartz, Silicea, Spherica, AF-SO 25R, Quartz [Silica, crystalline], Siilca, Zorbax, quartz-glass, silica sand, Silicom dioxide, Silica flour (powdered crystalline silica), Silica marina, Silica, crystalline: tridymite, silica-gel, Fused-silica, pyrogenic silica, Silica,fumed, GP 11I, RD 8,FT-0700917, NS00096378, S0822, Silica gel, with 1-4 mm moisture indicator, Silica, amorphous, fumed (crystalline free), Silicon dioxide Nanopowder KH550 processing, Silicon dioxide Nanopowder KH570 processing, Silicon(IV) oxide, 99.0% (metals basis), Celite(R) 110, filter aid, flux calcinated, Celite(R) 512 medium, filter aid, calcined, Chromosorb(R) G/AW-DMCS, 100-120 mesh, Chromosorb(R) W/AW-DMCS, 120-140 mesh, K-411 Glass microspheres, NIST SRM 2066, Silica gel, technical grade 40, 6-12 mesh, C18 Silica Gel, Endcapped, 60A, 40-63um, D05839, D06521, D06522, D78143, Dr. Zenni GGOGGOMA ToothpasteRaspberry flavor, Sand, white quartz, 50-70 mesh particle size, Silica, mesostructured, MSU-F (cellular foam), SILICON DIOXIDE COMPONENT OF SIMETHICONE, Silicon Dioxide, Amorphous Gel, 15% In Water, Silicon Dioxide, Amorphous Gel, 40% In Water, Celite(R) 209, filter aid, natural, untreated, Celite(R) Analytical Filter Aid II (CAFA II), Glass sand, NIST(R) SRM(R) 165a, low iron, Silica gel spherical, 75-200 mum particle size, Silica gel, Davisil(R) grade 922, -200 mesh, Silica gel, large pore, P.Vol. ca. 1.65cc/g, Silicon Oxide (Silica, Silicon dioxide, quartz), Silicon oxide powder, 99.5% Nano, 15-20 nm, Q116269, Sand for sand sieve analysis, NIST(R) RM 8010, Silica gel, GF254, for thin layer chromatography, Silica gel, HF254, for thin layer chromatography, Silica gel, Type III, Indicating, for desiccation, Silica, mesostructured, MCM-41 type (hexagonal), Silicon dioxide, purum p.a., acid purified, sand, Standard Super Cel(R) fine, filter aid, calcined, Celite(R) 500 fine, filter aid, dried, untreated, Collodial Silica in Aqueous Solution (nanoparticles), Glass sand, NIST(R) SRM(R) 1413, high alumina, J-002874, Sand, white quartz, >=99.995% trace metals basis, Silica gel, large pore, P.V. ca. 1cc/g, 8 mesh, Silica gel, technical grade, 1-3 mm particle size, Silica gel, technical grade, 3-6 mm particle size, Silica gel, with moisture indicator (blue), coarse, Celpure(R) P65, meets USP/NF testing specifications, Micro particles based on silicon dioxide, size: 2 mum, Micro particles based on silicon dioxide, size: 3 mum, Micro particles based on silicon dioxide, size: 4 mum, Micro particles based on silicon dioxide, size: 5 mum, Silica gel 60, 0.060-0.2mm (70-230 mesh), Silica gel desiccant, indicating, <1% Cobalt chloride, Silica gel, -60-120 mesh, for column chromatography, Silicon(IV) oxide, 15% in H2O, colloidal dispersion, Silicon(IV) oxide, 30% in H2O, colloidal dispersion, Silicon(IV) oxide, 50% in H2O, colloidal dispersion, Celpure(R) P100, meets USP/NF testing specifications, Celpure(R) P1000, meets USP/NF testing specifications, Celpure(R) P300, meets USP/NF testing specifications, Micro particles based on silicon dioxide, size: 0.5 mum, Micro particles based on silicon dioxide, size: 1.0 mum, Silica Dispersion (SiO2, Aqueous Dispersion, Amorphous), Silica gel 60, 0.032-0.063mm (230-450 mesh), Silica gel 60, 0.036-0.071mm (215-400 mesh), Silica gel 60, 0.040-0.063mm (230-400 mesh), Silica gel desiccant, indicating, -6+16 mesh granules, Silica gel, with moisture indicator (blue), -6-20 mesh, Silica, mesostructured, MSU-H (large pore 2D hexagonal), Silica, mesostructured, SBA-15, 99% trace metals basis, Silicon Dioxide (Silica) Nanodispersion Type A (20nm), Silicon Dioxide (Silica) Nanodispersion Type B (20nm), Silicon dioxide, -325 mesh, 99.5% trace metals basis, Silicon dioxide, washed and calcined, analytical reagent, Silicon(IV) oxide, amorphous fumed, S.A. 85-115m2/g, Synthetic - fused silica: Trade Names: Suprasil; TAFQ, Zeolite - Mesoporous Silica Nanopowder (SBA-15 Type), Chromosorb(R) W, AW-DMCS, 100-120 mesh particle size, Micro particles based on silicon dioxide, size: 0.15 mum, Silica gel, high-purity grade (15111), pore size 60 ??, Silica Slurry (SiO2, Purity: 99%, Diameter: 15-20nm), Silica, mesoporous, 1 mum particle size, pore size ~2 nm, Silica, mesoporous, 1 mum particle size, pore size ~4 nm, Silica, mesoporous, 2 mum particle size, pore size ~2 nm, Silica, mesoporous, 2 mum particle size, pore size ~4 nm, Silica, mesoporous, 3 mum particle size, pore size ~2 nm, Silica, mesoporous, 3 mum particle size, pore size ~4 nm, Silica,fumed, hydrophilic, specific surface area 200 m2/g, Silica,fumed, hydrophilic, specific surface area 400 m2/g, silicon dioxide; synthetic amorphous silicon dioxide (nano), Silicon(IV) oxide, amorphous fumed, S.A. 350-420m2/g, Amorphous silica: Vitreous silica, quartz glass, fused silica, LUDOX(R) AM colloidal silica, 30 wt. % suspension in H2O, LUDOX(R) CL colloidal silica, 30 wt. % suspension in H2O, LUDOX(R) CL-X colloidal silica, 45 wt. % suspension in H2O, LUDOX(R) LS colloidal silica, 30.

Usually they are suspended in an aqueous phase that is stabilized electrostatically.
Colloidal silicas exhibit particle densities in the range of 2.1 to 2.3 g/cm3.
Most colloidal silicas are prepared as monodisperse suspensions with particle sizes ranging from approximately 30 to 100 nm in diameter.

Polydisperse suspensions can also be synthesized and have roughly the same limits in particle size.
Smaller particles Colloidal silicas are difficult to stabilize while particles much greater than 150 nanometers are subject to sedimentation.
Colloidal silicas are most often prepared in a multi-step process where an alkali-silicate solution is partially neutralized, leading to the formation of silica nuclei.

The subunits of colloidal silica particles are typically in the range of 1 to 5 nm.
Whether or not these subunits are joined depends on the conditions of polymerization.
Initial acidification of a water-glass (sodium silicate) solution yields Si(OH)4.

If the pH is reduced below 7 or if salt is added, then the units tend to fuse together in chains.
Colloidal silicas are often called silica gels. If the pH is kept slightly on the alkaline side of neutral, then the subunits stay separated, and they gradually grow.
Colloidal silicas are often called precipitated silica or silica sols.

Hydrogen ions from the surface of colloidal silica tend to dissociate in aqueous solution, yielding a high negative charge.
Substitution of some of the Si atoms by Al is known increase the negative colloidal charge, especially when it is evaluated at pH below the neutral point.
Because of the very small size, the surface area of colloidal silica is very high.

The colloidal suspension is stabilized by pH adjustment and then concentrated, usually by evaporation.
The maximum concentration obtainable depends on the on particle size.
For example, 50 nm particles can be concentrated to greater than 50 wt% solids while 10 nm particles can only be concentrated to approximately 30 wt% solids before the suspension becomes too unstable.

The term "colloidal" indicates that the particles are finely divided and dispersed evenly throughout the liquid, resulting in a stable and homogeneous mixture.
In the case of colloidal silica, the solid particles are typically in the nanometer range.
Colloidal silica is a submicroscopic fumed silica with a particle size of about 15 nm.

Colloidal silica is a light, loose, bluish-white-colored, odorless, tasteless, amorphous powder.
Colloidal silica is prepared by the flame hydrolysis of chlorosilanes, such as silicon tetrachloride, at 18008℃ using a hydrogen–oxygen flame.
Rapid cooling from the molten state during manufacture causes the product to remain amorphous.

Silicon dioxide is a silicon oxide made up of linear triatomic molecules in which a silicon atom is covalently bonded to two oxygens.
Fumed silica may be synthesized by high temperature hydrolysis of SiCl4 in O2(N2)/H2 flame.
Colloidal silica is amorphous in nature and possesses very high specific area.

The micro droplets of amorphous silica fuse into a branch and form a chain like agglomerate.
Colloidal silicas are produced in a variety of grades that range in a number of factors.
Particle size typically varies from 5nm to 40nm, and particle size distribution can vary from narrow to wide depending on the manufacturing process.

Standard colloidal silica is stable at a pH from 8 - 10.5 and carries an anionic surface charge that is stabilized with sodium or ammonium.
In certain grades, some of the Colloidal silica in the silica particle are replaced with aluminate ions to allow for enhanced stability in a wider pH range, usually 3.5 - 10.5.
Colloidal silica made by DKIC consists of dense silica particles suspended in aqueous medium.

These particles are spherical and uniform in size.
They do not have any internal structure of their own and are totally amorphous.
Colloidal silicas are discrete and non-agglomerated.

Colloidal silica with particle size ranging between 7 to 35 nanometers.
These stable aqueous dispersions of colloidal silica are available in silica concentrations from 20 to 50 weight%.
Colloidal silica can also be produced to carry a positive surface charge that is stable in the acidic pH range.

This is accomplished by modifying the surface of the particle with aluminum and charge stabilizing the particle with a chloride anion.
Colloidal silicas are defined as a stable suspension of microscopic particles or molecules distributed throughout a second substance known as a dispersion medium.
They differ from other types of suspensions in that the colloid is evenly dispersed throughout the suspension, and does not separate or settle.

Colloidal silicas may be any combination of liquid, solid, and gaseous colloids and dispersion media.
Colloidal silicas are prevalent in a variety of common products and produced by various environmental and natural circumstances as well.
Colloidal Silica suspension can produce high-quality mirror polishes.

Colloidal silica is part abrasive, part chemical polisher, which makes it well-suited to polishing materials such as aluminum, stelitte, and cobalt chrome.
Colloidal silicas are made from liquid particles suspended in a gaseous dispersion medium, such as fog, mist, and hairspray.
Colloidal silicas are solids suspended in a gaseous dispersion medium.

Common Colloidal silicas include smoke, dust, and air pollution.
Liquid foams result from gas particles suspended in a liquid dispersion medium, such as whipped cream, shaving cream, and hair-styling mousse.
Emulsion occurs when liquid Colloidal silicas are suspended in a liquid dispersion medium.

Sol refers to Colloidal silicas suspended in a liquid dispersion medium.
Pigmented ink, paint, and blood are common examples of sols.
Colloidal silicas are created when gas particles become suspended in a solid dispersion medium.

Gels are made from Colloidal silicas suspended in a liquid dispersion medium.
Gels are often treated in order to enhance the structure of the solid particles and create a more viscous solution.
Solid sol refers to solid particles suspended in a solid dispersion medium, such as metal alloys, colored glass, and gemstones.

Colloidal silica consists of silica molecules suspended in liquid, thereby forming a liquid sol.
The process of creating colloidal silica is closely monitored to ensure that the silica molecules remain stable and separate within the liquid medium without collapsing into smaller component molecules or collecting into unstable silica gels.
The liquid dispersion medium exhibits greater density than water and must be electrostatically treated for enhanced ionic stabilization.

Colloidal silica’, is a polymeric form of silicon.
The non-toxic, naturally occurring element Colloidal silica is listed in the periodic-table and is widely employed in the industry.
Colloidal silica is abundant in nature because it accounts for a sizeable portion of the Earth's crust and is the second most prevalent element after oxygen.

The water-based suspensions of crystalline Colloidal silicas are known as colloidal silicon dioxide (SiO2).
Colloidal silica nanoparticle surface is then charged, enabling the particles to repel and create a stable dispersion or colloid.
The stable dispersion formed is called colloidal Colloidal silica and has unique properties which can be applied to different applications.

Colloidal silicon dioxide has the physical characteristics of light, loose, bluish-white-colored, flavorless, and amorphous powder.
Conventional colloidal silicon dioxide consists of a negative (anionic) surface charge that is regulated with ammonium or sodium and is stable at a potential hydrogen (pH) range of 8 to 10.5.
Colloidal silica is composed of discrete, amorphous, spherical silica particles dispersed in water that do not exhibit detectable levels of crystallinity or porosity.

Several grades are available in various particle sizes within the range of 5–40 nanometers.
Each grade of LUDOX® colloidal silica has a very tight particle size distribution and varies in pH, silica sol charge, and stabilizing mechanism.
This non-crystallizing Colloidal Silica is made to be user friendly.

Colloidal silica eliminates the problems that are caused by drying or freezing that are associated with other colloidal silica products which are used for chemical/mechanical polishing
Colloidal silica is a first choice silica dispersion for optimizing polishing results such as silicon, fused quartz, fused silica, lithium niobate, YAZ, GGG, alexandrite, sapphire and many others.
Colloidal silica varies from other types of silica in several significant ways.

The most noticeable difference is that Colloidal silica's in liquid form, as opposed to powder.
In addition, Colloidal silica has the widest ranging surface area, and its aggregate size can be as small as the actual size of the primary particle.
Colloidal silica dispersions are fluid, low viscosity dispersions.

There are many grades of colloidal silica, but all of them are composed of silica particles ranging in size from about 2 nm up to about 150 nm Colloidal silicas may be spherical or slightly irregular in shape, and may be present as discrete particles or slightly structured aggregates.
Colloidal silicas may also be present in a narrow or wide particle size range, depending on the process in which they were created.
The maximum weight fraction of Colloidal silica in the dispersion is limited based on the average particle size.

Dispersions with a smaller average diameters have larger overall specific surface areas and are limited to low concentration dispersions.
Conversely, dispersions with larger average diameters have lower overall specific surface areas and are available in more concentrated dispersions.
The appearance of colloidal silica dispersion depends greatly on the particle size.

Dispersions with small silica particles (< 10 nm) are normally quite clear.
Midsize dispersions (10-20 nm) start to take on an opalescent appearance as more light is scattered.
Dispersions containing large colloidal silica particles (> 50 nm) are normally white.

Standard colloidal silica dispersions are stable against gelling and settling in pH range of 8 - 10.5.
Colloidal silica is a synthetic amorphous silica derivative in which the surface of the fumed silica particle has been modified by the addition of dimethyl silyl groups.
The surface modification is achieved via a controlled chemical process that involves the attachment of dimethyl silyl groups, rendering the silica less wettable. It

Colloidal silica is approved for use in pharmaceutical products as an excipient and is supplied as a light, fine, white or almost white amorphous fluffy powder.
Colloidal silica is a water-based, stabilized dispersion of amorphous silicon dioxide (aka silica) nanoparticles.
Manufacturers produce colloidal silicathrough the polymerization of silica nuclei derived from silicate solutions.

Polymerized under alkaline conditions, the silica nuclei convert into silica sols (solid particles) at the nano-scale and with a high surface area.
The process then applies a charge to these silica sols, causing electrostatic resistance between each particle and creating a colloid—a type of stable dispersion.
Colloidal silica, is a stable suspension of spherical silicon dioxide (SiO2) nanoparticles in a liquid, that are hydroxylated on the surface.

Colloidal silica is found in almost all industrial sectors.
The applications range from surface treatment in the paper industry, to use as a polishing agent in the electronics industry and use as an additive for varnishes, coatings and paints to improve weather and abrasion resistance.
Colloidal silica is also a common additive in cosmetics and in the food industry.

The mean particle size and distribution width define the field of application of the SiO2 particles.
Colloidal silica, is a stable suspension of spherical silicon dioxide (SiO2) nanoparticles in a liquid, that are hydroxylated on the surface.
Colloidal silica acid is found in almost all industrial sectors.

Colloidal silica is amorphous silica (oxide of silicon) prepared synthetically by the vapour-phase hydrolysis of a silicon compound.
Colloidal silica has the chemical formula SiO2 but is distinct from other types of silica, such as amorphous or crystalline silica, that exist naturally or otherwise such as silica gel or precipitated silica.
Colloidal silica is supplied as a white or almost white, light, fluffy, and extremely fine powder.

Colloidal silica is commonly used as a binder in the production of ceramic shells for investment casting.
Colloidal silica helps create intricate and detailed molds for casting metal objects.
In the paper and textile industries, Colloidal silica is sometimes used as a coating or finishing agent to improve printability, smoothness, and abrasion resistance.

Colloidal silica can be incorporated into adhesives and sealants to enhance their strength, flexibility, and adhesion properties.
Colloidal silica is employed in the production of anti-reflective coatings for optical applications, such as eyeglasses, camera lenses, and other optical devices.
In some water treatment processes, Colloidal silica can be used to flocculate and remove impurities from water.

Colloidal silica is utilized in certain personal care products, such as toothpaste and skin creams, as a thickening or abrasive agent.
Colloidal silica can be used as a clarifying agent in the production of beer and wine, helping to remove haze-producing particles.

In the oil and gas industry, colloidal silica is sometimes used in drilling fluids and cementing operations to improve wellbore stability.
Colloidal silica is used in the electronics industry for applications like planarization during semiconductor manufacturing.

Melting point: >1600°C
Density: 2.3 lb/cu.ft at 25 °C (bulk density)(lit.)
refractive index: n20/D 1.46(lit.)
solubility: Practically insoluble in organic solvents, water, and acids, except hydrofluoric acid; soluble in hot solutions of alkali hydroxide. Forms a colloidal dispersion with water. For Aerosil, solubility in water is: 150 mg/L at 258℃ (pH 7).
form: powder
Specific Gravity: 2.2

Purification of silica for high technology applications uses isopiestic vapour distillation from concentrated volatile acids and is absorbed in high purity water.
The impurities remain behind. Preliminary cleaning to remove surface contaminants uses dip etching in HF or a mixture of HCl, H2O2 and deionised water.
Colloidal silica, amorphous is a noncombustible solid.

Generally unreactive chemically.
Incompatible with fluorine, oxygen difluoride, chlorine trifluoride.
Soluble in molten alkalis and reacts with most metallic oxides at high temperature.

In a normal abrasive slurry can expect 15-20wt% concentration of abrasive particles, but in a colloidal slurry as much as 50wt% of silica particles can be present.
This greatly increases the amount of Colloidal silicas that work on a substrate making the polishing very uniform and efficient.
Also, the Colloidal silicas are incredibly uniformly spherical, which again, is difficult to match with standard abrasive particles where the shape is far less uniform.

Colloidal silica is a widely used material in industry.
Colloidal Silica is an epoxy thickening additive used to control the viscosity of the epoxy.
Colloidal silica prevents epoxy runoff in vertical and overhead joints. This is a very strong filler.

Colloidal silica creates a smooth mixture, ideal for general epoxy bonding and filleting.
Colloidal silica is also our most versatile epoxy filler.
Often used in combination with other fillers, 406 can be used to improve strength, abrasion resistance, and consistency of epoxy fairing compounds.

The result is a tougher, smoother surface.
Colloidal Silica is the most popular binder used in the precision investment casting industry today.
Colloidal silica offers the investment caster a safe, economical, easy to use slurry component that performs well as either primary or backup slurry.

Colloidal Silica systems are very stable; able to form a long life ceramic slurry with a large range of refractory materials due to the binder’s chemical inertness.
Sol-gel, hydrothermal, and chemical vapor deposition (CVD) methods have been used to fabricate Colloidal silica.
The sol-gel process is widely utilized to make pure Colloidal silicas because of its capacity to regulate the physical appearance by methodical monitoring of reaction variables under ambient temperature.

The ion-exchange procedure is a part of the technique used to produce Colloidal silica using sodium silicate through the sol-gel method.
With this technique, particle size and distribution of colloidal silicon dioxide may be easily controlled.
The technique also provides improved electric charge and high zeta for cColloidal silica particles.

This makes the solution more stable, repelling aggregation and preventing agglomeration between particles.
These colloidal silica particles can achieve additional anionic charge stability when as aluminosilicate sites are formed by incorporation of aluminum into the surface layer of the silica particles.
Low pH versions of colloidal silica are also available by the adsorption of cationic aluminum oxide onto the surface of the particles.

This results in a cationic particle that is stabilized with anionic species - commonly this is chloride.
These dispersions are stable below a pH of 4.
Low pH grades can also be obtained by completely deionizing the dispersion.

These grades do not require the presence of stabilizing ions and are also stable below a pH of 3.
Colloidal silicas can be modified to several configurations including but not limited to: adjustments to pH, stabilization ions, surface charge and surface modification.
Colloidal silica consists of silica molecules suspended in liquid, thereby forming a liquid sol.

The process of creating colloidal silica is closely monitored to ensure that the silica molecules remain stable and separate within the liquid medium without collapsing into smaller component molecules or collecting into unstable silica gels.
The liquid dispersion medium exhibits greater density than water and must be electrostatically treated for enhanced ionic stabilization.
Colloidal silica is highly fluid with low viscosity.

Uses for colloidal silica vary depending on the size of the silica particles in the solution and the modifiable pH, ionization, and surface charge.
Colloidal silica is extensively used as a rheological additive in personal care products to control flowability.
In the most general terms colloidal silica is a dispersion of amorphous silicon dioxide (silica) particles in water.

These amorphous silica particles are produced by polymerizing silica nuclei from silicate solutions under alkaline conditions to form nanometer sized silica sols with high surface area.
A charge is then induced on the silica nanoparticle surface that allows the silica particles to repel one another and form a stable dispersion, or colloid.
Colloidal silica is a stable suspension of spherical silicon dioxide (SiO2) nanoparticles in a liquid, that are hydroxylated on the surface.

Colloidal silica is found in almost all industrial sectors.
The applications range from surface treatment in the paper industry, to use as a polishing agent in the electronics industry and use as an additive for varnishes, coatings and paints to improve weather and abrasion resistance.
Colloidal silica is also a common additive in cosmetics and in the food industry.

The mean particle size and distribution width define the field of application of the SiO2 particles.
Typical sizes range from 1 nm to 100 nm.
Colloidal silicas are typically aqueous suspensions in the range of 30 – 500 nm in diameter.

Colloidal silicas are usually stabilized electrostatically and have densities in the range of 2.1 to 2.3 g/cm3.
Applications for colloidal silicas include fillers, binders, abrasives, catalysts, and absorbants.
Most size measurements of colloidal silica are performed using dynamic light scattering (DLS) instruments such as the SZ-100 Nanoparticle Analyzer.

Colloidal silica is used in many applications including catalysis, pharmaceuticals, and coatings.
Although naturally formed silica materials are widely available, they are often in forms that are difficult to process or are even harmful to health.
Therefore, uniform colloidal silicas are generally manufactured using synthetic chemical processes.

While established high temperature gaseous synthesis methods fall out of favor in our energy conscious society, liquid synthesis methods are current industrial leaders.
The precipitated Colloidal silica method provides the majority share of commercially produced specialty silicas with its economic advantages predicted to continue to grow in the future.
Colloidal silica products are stable dispersions of non-agglomerated, amorphous, nanometer-size, and spherical particles of silica.

The good stability, adjustable particle size distribution and mechanical properties have made colloidal silica a preferred abrasive for many CMP applications.
Recently, research and analytical efforts have focused on the development of colloidal products with tunable physical and chemical properties to open up new opportunities in the CMP industry segment.
Colloidal silicas are most often prepared in a multi-step process where an alkali-silicate solution is partially neutralized, leading to the formation of silica nuclei.

The subunits of colloidal silica particles are typically in the range of 1 to 5 nm.
Whether or not these subunits are joined together depends on the conditions of polymerization.
Initial acidification of a water-glass (sodium silicate) solution yields Si(OH)4.

If the pH is reduced below 7 or if salt is added, then the units tend to fuse together in chains.
Colloidal silicas are often called silica gels.
If the pH is kept slightly on the alkaline side of neutral, then the subunits stay separated, and they gradually grow.

Colloidal silicas are often called precipitated silica or silica sols.
Hydrogen ions from the surface of colloidal silica tend to dissociate in aqueous solution, yielding a high negative charge.
Substitution of some of the Si atoms by Al is known increase the negative colloidal charge, especially when it is evaluated at pH below the neutral point.

Because of the very small size, the surface area of colloidal silica is very high.
The Colloidal silica is stabilized by pH adjustment and then concentrated, usually by evaporation.

The maximum concentration obtainable depends on the on particle size.
For example, 50 nm particles can be concentrated to greater than 50 wt% solids while 10 nm particles can only be concentrated to approximately 30 wt% solids before the suspension becomes too unstable.

Uses:
Colloidal silica has interesting thickening and thixotropic properties, and an enormous external surface area.
Colloidal silica is produced by a vapor phase hydrolysis process using chlorosilanes or substituted silanes such as, silicon tetrachloride in a flame of hydrogen and oxygen.
This material is formed and collected in a dry state.

Colloidal silica contains no detectable crystalline silica.
Colloidal silica is widely used in pharmaceuticals, cosmetics, and food products.
Colloidal silica is small particle size and large specific surface area give it desirable flow characteristics that are exploited to improve the flow properties of dry powders in a number of processes such as tableting and capsule filling.

Colloidal silica is also used to stabilize emulsions and as a thixotropic thickening and suspending agent in gels and semisolid preparations.
With other ingredients of similar refractive index, transparent gels may be formed.
The degree of viscosity increase depends on the polarity of the liquid (polar liquids generally require a greater concentration of colloidal silicon dioxide than nonpolar liquids).

Viscosity is largely independent of temperature.
However, changes to the pH of a system may affect the viscosity.
In aerosols, other than those for inhalation, Colloidal silica is used to promote particulate suspension, eliminate hard settling, and minimize the clogging of spray nozzles.

Colloidal silica is also used as a tablet disintegrant and as an adsorbent dispersing agent for liquids in powders.
Colloidal silica is frequently added to suppository formulations containing lipophilic excipients to increase viscosity, prevent sedimentation during molding, and decrease the release rate.
Colloidal silica is also used as an adsorbent during the preparation of wax microspheres; as a thickening agent for topical preparations; and has been used to aid the freeze-drying of nanocapsules and nanosphere suspensions.

In papermaking colloidal silica is used as a drainage aid. It increases the amount of cationic starch that can be retained in the paper.
Colloidal silica starch is added as sizing agent to increase the dry strength of the paper.
Colloidal silica hasn't always been the versatile problem solver that it is today.

In fact, early colloidal silicas were not commercially useful because they were too unstable and contained only low levels of silica.
Colloidal silica wasn't until the production of Colloidal silica in the late 1940's that the applications for colloidal silica began to expand.
One of the earliest applications for colloidal silica was in anti-slip coatings for floors.

Colloidal silica is a very common final polishing stage for metallographic sample analysis.
This is because Colloidal silica is generally guaranteed to give a damage free specimen.
These types of samples are viewed under high magnification, so it is important when looking at the structures of a material that damage caused by the preparation processes is not confused with the material make up itself.

For modern material analysis software, a scratch free finish is critical.
Scratches or any other damage on a specimen can confuse the software giving incorrect readings.
This is particularly important with hardness testing software.

For some metallographic samples, the chemical make-up of colloidal silica can be used to etch the surface revealing grain boundaries and other structures.
Colloidal silica hasn't always been the versatile problem solver that it is today.
In fact, early colloidal silicas were not commercially useful because they were too unstable and contained only low levels of silica.

colloidal silica wasn't until the production of LUDOX in the late 1940's that the applications for colloidal silica began to expand.
One of the earliest applications for colloidal silica was in anti-slip coatings for floors.
The 1950's Dupont advertisement below explains how colloidal silica is used in floor wax.

colloidal silica is used in the production of coatings and films due to its ability to form a transparent layer with excellent adhesion properties.
colloidal silica can serve as a support material for catalysts in various chemical processes.
colloidal silica is utilized in the semiconductor and optical industries for polishing and planarizing surfaces.

In the manufacturing of refractory materials, colloidal silica can act as a binder to improve the strength and performance of the final product.
colloidal silica is sometimes added to concrete to enhance its strength and durability.
colloidal silica is used in some dental materials, including composites and impression materials.

In pharmaceuticals, colloidal silica can be employed as a carrier for drug delivery systems.
colloidal silica is highly fluid with low viscosity.
Uses for colloidal silica vary depending on the size of the silica particles in the solution and the modifiable pH, ionization, and surface charge.

Used for final polishing, colloidal silica suspensions are mixtures of abrasive particles dispersed throughout a chemically aggressive liquid carrier.
This combination provides a chemical-mechanical polishing action, resulting in deformation-free surfaces.
The modified pH of these suspensions can provide delineation of grain boundaries and other microstructural features for some sample types.

colloidal silica is used to create thin, transparent coatings and films on surfaces, providing enhanced adhesion, hardness, and durability.
colloidal silica serves as a support material for catalysts in chemical processes, improving their stability and efficiency.
In industries such as semiconductor manufacturing and optics, colloidal silica is used for polishing and planarization to achieve smooth surfaces with high precision.

colloidal silica acts as a binder in the production of refractory materials, improving their strength and resistance to high temperatures.
colloidal silica can be added to concrete to enhance its strength, durability, and resistance to chemical attack.
colloidal silica is used as a binder in ceramic shell molds for investment casting, enabling the production of intricate and detailed metal castings.

colloidal silica is incorporated into adhesives and sealants to improve their adhesive properties, flexibility, and overall performance.
In the production of optical devices, colloidal silica is used to create anti-reflective coatings, reducing glare and enhancing optical performance.
Colloidal silica can aid in water treatment processes by flocculating impurities and facilitating their removal.

colloidal silica is used in some dental composites and impression materials to improve their properties.
colloidal silica is employed in the textile and paper industries for coatings that enhance printability, smoothness, and abrasion resistance.
Found in certain personal care items such as toothpaste and skin creams, acting as a thickening or abrasive agent.

colloidal silica is used as a clarifying agent in the production of beverages like beer and wine to remove haze-producing particles.
In drilling fluids and cementing operations, colloidal silica is used to improve wellbore stability.
Employed in the electronics industry for planarization processes during the manufacturing of semiconductors.

Applications that use colloidal silica vary widely.
colloidal silica can be used to enhance or direct the movement of substances within various processes.
For example, colloidal silica is used in the paper manufacturing process to draw liquid from the finished paper quickly, thereby allowing the paper to dry faster while retaining its strengthening starch.

Similarly, colloidal silica can be used to absorb moisture in industrial settings where moisture levels are high.
Depending on the size of its constituent particles, colloidal silica may be used to enhance the movement of materials or to increase surface friction.
Colloidal silica is used in many applications including catalysis, pharmaceuticals, and coatings.

Although naturally formed silica materials are widely available, they are often in forms that are difficult to process or are even harmful to health.
Therefore, uniform colloidal silicas are generally manufactured using synthetic chemical processes.
While established high temperature gaseous synthesis methods fall out of favor in energy conscious society, liquid synthesis methods are current industrial leaders.

Colloidal silica can be used to enhance or direct the movement of substances within various processes.
For example, Colloidal silica is used in the paper manufacturing process to draw liquid from the finished paper quickly, thereby allowing the paper to dry faster while retaining its strengthening starch.
Similarly, colloidal silica can be used to absorb moisture in industrial settings where moisture levels are high.

Colloidal silica dioxide is also used to stabilize emulsions and as a thixotropic thickening and suspending agent in gels and semisolid preparations.
With other ingredients of similar refractive index, transparent gels may be formed.
The degree of viscosity increase depends on the polarity of the liquid (polar liquids generally require a greater concentration of Colloidal silica dioxide than nonpolar liquids).

Viscosity is largely independent of temperature.
However, changes to the pH of a system may affect the viscosity.
In aerosols, other than those for inhalation, Colloidal silica dioxide is used to promote particulate suspension, eliminate hard settling, and minimize the clogging of spray nozzles.

colloidal silica is also used as a tablet disintegrant and as an adsorbent dispersing agent for liquids in powders.
colloidal silica is frequently added to suppository formulations containing lipophilic excipients to increase viscosity, prevent sedimentation during molding, and decrease the release rate.
colloidal silica is also used as an adsorbent during the preparation of wax microspheres; as a thickening agent for topical preparations; and has been used to aid the freeze-drying of nanocapsules and nanosphere suspensions.

Depending on the size of its constituent particles, colloidal silica may be used to enhance the movement of materials or to increase surface friction.
Colloidal silica can also be used as a reference material for both particle size and zeta potential.
colloidal silica is a well known and characterized colloidal material that has been studied using various particle size analysis techniques including acoustic spectroscopy, laser diffraction and dynamic light scattering.

Colloidal silica is usually used in combination with a polyurethane polishing pad which has voids within the structure of the pad to hold the colloidal silica.
Colloidal silica is applied using a peristaltic pump and a constant drip feed similar to a conventional abrasive lapping process.
Colloidal silica’s important to maintain the wetness of the process so there is no drag out of material.

Colloidal silica dioxide is widely used in pharmaceuticals, cosmetics, and food products.
Colloidal silicas small particle size and large specific surface area give it desirable flow characteristics that are exploited to improve the flow properties of dry powders in a number of processes such as tableting and capsule filling.
Colloidal silica can be employed as a carrier in drug delivery systems, allowing for controlled release and improved bioavailability of pharmaceuticals.

colloidal silica is used in the formulation of abrasive pastes and polishes for applications such as metal polishing and glass grinding.
colloidal silica is sometimes used in the production of fireproofing materials, contributing to the thermal resistance of coatings and structures.
In the manufacturing of batteries, colloidal silica may be utilized to enhance electrode materials and improve battery performance.

Colloidal silica nanoparticles can be employed in photocatalytic processes, such as water purification and air treatment, due to their unique surface properties.
colloidal silica is used in some environmental remediation processes, aiding in the removal of contaminants from soil and water.
colloidal silica can be used in agriculture to improve soil structure and water retention, promoting better plant growth.

In the emerging field of printed electronics, colloidal silica is utilized in the formulation of conductive inks and coatings.
colloidal silica nanoparticles are investigated for potential biomedical applications, including imaging, drug delivery, and therapeutics.
In addition to batteries, colloidal silica may be explored for use in energy storage systems, contributing to advancements in renewable energy technologies.

colloidal silica can be employed in wastewater treatment processes to remove suspended solids and contaminants.
colloidal silica is used in certain formulations of paints and coatings to improve their adhesion, durability, and resistance to environmental factors.
colloidal silica nanoparticles are studied for their potential in enhanced oil recovery processes in the oil and gas industry.

In the production of solar cells, colloidal silica can be used to create anti-reflective coatings and improve the efficiency of light absorption.
Found in some cosmetic products, colloidal silica may contribute to formulations such as foundations and powders.

Safety Profile:
Poison by intraperitoneal, intravenous, and intratracheal routes.
Moderately toxic by ingestion.
Much less toxic than crystalhe forms.

Questionable carcinogen with experimental carcinogenic data.
Mutation data reported.
colloidal silica is widely used in oral and topical pharmaceutical products and is generally regarded as an essentially nontoxic and nonirritant excipient.

However, intraperitoneal and subcutaneous injection may produce local tissue reactions and/or granulomas.
colloidal silica should therefore not be administered parenterally.

Storage:
colloidal silica is hygroscopic but adsorbs large quantities of water without liquefying.
When used in aqueous systems at a pH 0–7.5, colloidal silica is effective in increasing the viscosity of a system.

However, at a pH greater than 7.5 the viscosityincreasing properties of colloidal silica are reduced; and at a pH greater than 10.7 this ability is lost entirely since the silicon dioxide dissolves to form silicates.
colloidal silica powder should be stored in a well-closed container.

Colloidal silver consists of tiny silver particles in a liquid.
Colloidal silver is sometimes promoted on the internet as a dietary supplement; however, evidence supporting health-related claims is lacking.
Colloidal silver is used for wound healing, improving skin disorders, and preventing certain diseases.

CAS Number: 7440-22-4
Molecular Formula: Ag
Molecular Weight: 107.87
EINECS Number: 231-131-3

7440-22-4, 7761-88-8, Silver, Silver Paste DGP80 TESM8020, Silver atomic spectroscopy standard concentrate 1.00 g Ag, Colloidal silver ink, Silver nanowires, Silver nitrate concentrate, Silver nitrate solution, Silver standard solution, Silver, dispersion, Silverjet DGH-55HTG, Silverjet DGH-55LT-25C, Silverjet DGP-40LT-15C, Silverjet DGP-40TE-20C, SunTronic® Silver

Colloidal silver has been used in a variety of ways.
However, Colloidal silver is not approved for medical use by the FDA and should not be consumed, injected, or inhaled.
Use of colloidal silver can result in short-term and long term side effects.

Colloidal silver, also known as silver proteins or colloidal silver proteins, is a suspension of tiny silver particles in liquid.
Although silver has been used for medicinal and health purposes for thousands of years, colloidal silver has recently become popular amongst wellness enthusiasts hoping to boost their overall health.

Colloidal silver is a suspension of tiny silver particles. Commercial products are made by mixing silver, sodium hydroxide, and gelatin.
Homemade suspensions have also been made using different ingredients and an electrical current.
Most commonly, people swallow the suspension; however, it has also been inhaled using a nebulizer machine, and used topically on the skin and in the eyes.
Colloidal silver has even been used as a nasal spray.

Colloidal silver is a liquid suspension of microscopic particles of silver.
Colloidal silver has been promoted for its supposed antibacterial, antiviral, and antifungal properties.

Colloidal silver is one of the basic elements present in the earth's crust.
Colloidal silver is alloyed with many other metals to improve strength and hardness and to achieve corrosion resistance.

Colloidal silvers are one of the most commonly utilized nanomaterials due to their anti-microbial properties, high electrical conductivity, and optical properties.
Colloidal silvers (colloidal silver) have unique optical, electronic, and antibacterial properties, and are widely used in areas such as biosensing, photonics, electronics, and antimicrobial applications.
Colloidal silver is rare, but occurs naturally in the environment as a soft, “silver”-colored metal or as a white powdery compound (silver nitrate).

Metallic Colloidal silver and silver alloys are used to make jewelry, eating utensils, electronic equipment, and dental fillings.
Colloidal silvers of silver have been developed into meshes, bandages, and clothing as an antibacterial.
Colloidal silver is used in photographic materials, electric and electronic products, brazing alloys and solders, electroplated and sterling ware, as a catalyst, and in coinage.

Colloidal silvers are nanoparticles of silver, i.e. silver particles of between 1 nm and 100 nm in size.
The metal Colloidal silver is described as a white, lustrous solid.
In Colloidal silver is pure form it has the highest thermal and electrical conductivity and lowest contact resistance of all metals.
With the exception of gold, silver is the most malleable metal.

Colloidal silvers are nanoscale-sized particles composed of silver atoms.
Colloidal silvers, in particular, have attracted significant attention due to their distinct characteristics and potential applications.
Silver has no known functions or benefits in the body when taken by mouth, and it is not an essential mineral.

Colloidal silver products are often marketed as dietary supplements to take by mouth.
These products also come in forms to use on the skin.
Colloidal silver is a controversial alternative medicine.

A common form of Colloidal silver that is used to treat infections is silver nitrate.
Recent advancement in technology has introduced Colloidal silvers into the medical field.
Their small size and ability to induce cell death through multiple mechanisms makes them fantastic pharmacological candidates.

Colloidal silver is one of the earliest known metals.
Silver has no known physiologic or biologic function, though colloidal silver is widely sold in health food stores.
Colloidal silver has high thermal and electrical conductivity and resists oxidation in air that is devoid of hydrogen sulfide.

While frequently described as being 'silver' some are composed of a large percentage of silver oxide due to their large ratio of surface to bulk silver atoms.
Numerous shapes of Colloidal silvers can be constructed depending on the application at hand.
Commonly used Colloidal silvers are spherical, but diamond, octagonal, and thin sheets are also common.

Colloidal silver is widely used in many consumer products due to its unique optical, electrical, and thermal properties and extraordinarily efficient at absorbing and scattering light.
Colloidal silver has a face-centered cubic crystal structure.
Colloidal silver is a white metal, softer than copper and harder than gold.

When molten, Colloidal silver is luminescent and occludes oxygen, but the oxygen is released upon solidification.
As a conductor of heat and electricity, Colloidal silver is superior to all other metals.
Colloidal silver is soluble in HNO3 containing a trace of nitrate; soluble in hot 80% H2SO4; insoluble in HCl or acetic acid; tarnished by H2S, soluble sulfides and many sulfur-containing organic substances (e.g., proteins); not affected by air or H2O at ordinary temperatures, but at 200 C, a slight film of silver oxide is formed; not affected by alkalis, either in solution or fused.

There are two stable, naturally occurring isotopes, 107Ag and 109Ag.
In addition, there are reported to be 25 less stable isotopes, ranging in half-life from 5 seconds to 253 days.
Colloidal silver is a white lustrous metal that is extremely ductile and malleable.

Colloidal silver does not oxidize in O2 by heating.
While frequently described as being 'silver' some are composed of a large percentage of silver oxide due to their large ratio of surface to bulk silver atoms.
Numerous shapes of nanoparticles can be constructed depending on the application at hand.

Commonly used Colloidal silvers are spherical, but diamond, octagonal, and thin sheets are also common.
Their extremely large surface area permits the coordination of a vast number of ligands.
The properties of Colloidal silvers applicable to human treatments are under investigation in laboratory and animal studies, assessing potential efficacy, biosafety, and biodistribution.

Most applications in biosensing and detection exploit the optical properties of Colloidal silvers, as conferred by the localized surface plasmon resonance effect.
That is, a specific wavelength (frequency) of incident light can induce collective oscillation of the surface electrons of Colloidal silvers.
The particular wavelength of the localized surface plasmon resonance is dependant on the Colloidal silver size, shape, and agglomeration state.

Colloidal silvers are the most common commercialized nano technological product on the market.
Due to its unique antibacterial properties, Colloidal silvers have been hailed as a breakthrough germ killing agent and have been incorporated into a number of consumer products such as clothing, kitchenware, toys and cosmetics.
Many consider silver to be more toxic than other metals when in nanoscale form and that these particles have a different toxicity mechanism compared to dissolved silver.

Colloidal silver can be synthesized using ethylene glycol as a reducing agent and PVP as a capping agent, in a polyol synthesis reaction (vide supra).
A typical synthesis using these reagents involves adding fresh Colloidal silver nitrate and PVP to a solution of ethylene glycol heated at 140 °C.
This procedure can actually be modified to produce another anisotropic silver nanostructure, nanowires, by just allowing the silver nitrate solution to age before using it in the synthesis.

By allowing the silver nitrate solution to age, the initial nanostructure formed during the synthesis is slightly different than that obtained with fresh silver nitrate, which influences the growth process, and therefore, the morphology of the final product.
Silver nanopaticles are widely incorporated into wound dressings, and are used as an antiseptic and disinfectant in medical applications and in consumer goods.
Colloidal silver becomes Ag2O3 in O3 and black Ag2S3 in S2 and H2S.

Colloidal silver is soluble in HNO3 and concentrated H2SO4 .
Colloidal silver is not soluble in alkali.
Nanoscience and nanotechnology have now become the topic research that many developed.

Colloidal silver materials are developed in many applications because of their unique optical characteristic
Colloidal silver is a noble metal, extensively used in SERS, photocatalysis and solar cells.
The surface of Colloidal silver can be functionalized to attain specific properties such as biocompatibility and vapor selectivity of sensors.

Iodized Colloidal silver foils and thin films find potential use as SERS-active metal substrates.
Cu substrates laminated with Ag foils, have compatible coefficient of thermal expansion (CTE), to be used for electronic packaging.
Their extremely large surface area permits the coordination of a vast number of ligands.

The properties of Colloidal silvers applicable to human treatments are under investigation in laboratory and animal studies, assessing potential efficacy, biosafety, and biodistribution.
Colloidal silvers are nanoparticles of silver in the range of 1 nm and 100 nm in size.
While frequently described as being 'Colloidal silver' some are composed of a large percentage of silver oxide due to their large ratio of surface-to-bulk silver atoms.

As studies of Colloidal silvers improve, several Colloidal silvers medical applications have been developed to help prevent the onset of infection and promote faster wound healing.
Colloidal silvers are materials with dimensions typically in the range of 1 to 100 nanometers.
At this scale, materials often exhibit unique and enhanced properties compared to their bulk counterparts.

Colloidal silvers have a high surface area per unit mass and release a continuous level of silver ions into their environment.
Colloidal silvers exhibit catalytic activity, making them useful in certain chemical reactions and processes.
This property is of interest in fields such as catalysis and environmental remediation.

Colloidal silvers display unique optical properties, including the ability to interact with light in ways that depend on their size and shape.
This has led to applications in sensors, imaging, and as components in optical devices.
Due to the conductive nature of silver, nanoparticles made from silver can exhibit enhanced electrical conductivity.

This property is advantageous in applications related to electronics and sensors.
The interaction of light with the electrons in Colloidal silvers leads to a phenomenon known as surface plasmon resonance (SPR).
This optical effect is widely exploited in sensing applications.

Colloidal silvers have been investigated for various biomedical applications, including drug delivery systems, imaging agents, and as components in diagnostic tools.
Colloidal silvers are used in the formulation of conductive inks and coatings for applications in printed electronics, flexible electronics, and RFID tags.
Colloidal silvers are incorporated into textiles and fabrics to impart antimicrobial properties, making them useful for applications such as antibacterial clothing and wound dressings.

Incorporation of silver particles into plastics, composites, and adhesives increases the electrical conductivity of the material.
Silver pastes and epoxies are widely utilized in the electronics industries.
Colloidal silver based inks are used to print flexible electronics and have the advantage that the melting point of the small Colloidal silvers in the ink is reduced by hundreds of degrees compared to bulk silver.

When scintered, these Colloidal silver based inks have excellent conductivity.
Colloidal silvers have attract increasing attention for the wide range of applications in biomedicine.
Colloidal silvers, generally smaller than 100 nm and contain 20–15,000 silver atoms, have distinct physical, chemical and biological properties compared to their bulk parent materials.

The optical, thermal, and catalytic properties of Colloidal silvers are strongly influenced by their size and shape.
Additionally, owning to their broad-spectrum antimicrobial ability, Colloidal silvers have also become the most widely used sterilizing nanomaterials in consuming and medical products, for instance, textiles, food storage bags, refrigerator surfaces, and personal care products.
Colloidal silvers are those having diameters of nanometer size. With the advent of modern technology, humans can make nano-sized particles that were not present in nature.

Manufactured nanomaterials are materials with diameters of nanometer size, while nanotechnology is one of the fastest growing sectors of the hi-tech economy.
The application of nanotechnology has recently been extended to areas in medicine, biotechnology, materials and process development, energy and the environment.
Colloidal silver is the 66th most abundant element on the Earth, which means it is found at about0.05 ppm in the Earth’s crust.

Mining silver requires the movement of many tons of ore torecover small amounts of the metal.
Nevertheless, Colloidal silver is 10 times more abundant than gold and though silver is sometimes found as a free metal in nature, mostly it is mixed with theores of other metals.
When found pure, Colloidal silver is referred to as “native silver.”

Colloidal silver’s major ores areargentite (silver sulfide, Ag2S) and horn silver (silver chloride, AgCl).
Colloidal silver can also be recovered throughthe chemical treatment of a variety of ores.

Colloidal silvers have unique optical properties because they support surface plasmons.
At specific wavelengths of light the surface plasmons are driven into resonance and strongly absorb or scatter incident light.
This effect is so strong that it allows for individual nanoparticles as small as 20 nm in diameter to be imaged using a conventional dark field microscope.

This strong coupling of metal nanostructures with light is the basis for the new field of plasmonics.
Applications of plasmonic Colloidal silvers include biomedical labels, sensors, and detectors.
Colloidal silver is also the basis for analysis techniques such as Surface Enhanced Raman Spectroscopy (SERS) and Surface Enhanced Fluorescent Spectroscopy.

There are many ways Colloidal silvers can be synthesized; one method is through monosaccharides.
This includes glucose, fructose, maltose, maltodextrin, etc., but not sucrose.
Colloidal silver is also a simple method to reduce silver ions back to Colloidal silvers as it usually involves a one-step process.

There have been methods that indicated that these reducing sugars are essential to the formation of Colloidal silvers.
Many studies indicated that this method of green synthesis, specifically using Cacumen platycladi extract, enabled the reduction of silver.
Additionally, the size of the Colloidal silver could be controlled depending on the concentration of the extract.

The studies indicate that the higher concentrations correlated to an increased number of Colloidal silvers.
Smaller Colloidal silvers were formed at high pH levels due to the concentration of the monosaccharides.
Another method of Colloidal silver synthesis includes the use of reducing sugars with alkali starch and silver nitrate.

The reducing sugars have free aldehyde and ketone groups, which enable them to be oxidized into gluconate.
However, most Colloidal silver isrecovered as a by-product of the refining of copper, lead, gold, and zinc ores.
Colloidal silvers have been explored for their potential in water treatment and purification due to their antimicrobial properties.

The silver ions are bioactive and have broad spectrum antimicrobial properties against a wide range of bacteria.
By controlling the size, shape, surface and agglomeration state of the nanoparticles, specific silver ion release profiles can be developed for a given application.
Colloidal silvers typically have dimensions ranging from 1 to 100 nanometers.

The size and shape of these particles can influence their physical, chemical, and optical properties.
One of the notable features of Colloidal silvers is their strong antibacterial and antimicrobial activity.
The Colloidal silver must have a free ketone group because in order to act as a reducing agent it first undergoes tautomerization.

When inhaled, Colloidal silvers can go deeper into the lungs reaching more sensitive areas.
The most common methods for Colloidal silver synthesis fall under the category of wet chemistry, or the nucleation of particles within a solution.
This nucleation occurs when a Colloidal silver ion complex, usually AgNO3 or AgClO4, is reduced to colloidal Ag in the presence of a reducing agent.

When the concentration increases enough, dissolved metallic Colloidal silver ions bind together to form a stable surface.
The surface is energetically unfavorable when the cluster is small, because the energy gained by decreasing the concentration of dissolved particles is not as high as the energy lost from creating a new surface.
When the cluster reaches a certain size, known as the critical radius, it becomes energetically favorable, and thus stable enough to continue to grow.

This nucleus then remains in the system and grows as more Colloidal silver atoms diffuse through the solution and attach to the surface.
When the dissolved concentration of atomic Colloidal silver decreases enough, it is no longer possible for enough atoms to bind together to form a stable nucleus.
The most common capping ligands are trisodium citrate and polyvinylpyrrolidone (PVP), but many others are also used in varying conditions to synthesize particles with particular sizes, shapes, and surface properties.

There are many different wet synthesis methods, including the use of reducing sugars, citrate reduction, reduction via sodium borohydride, the Colloidal silver mirror reaction, the polyol process, seed-mediated growth, and light-mediated growth.
Each of these methods, or a combination of methods, will offer differing degrees of control over the size distribution as well as distributions of geometric arrangements of the nanoparticle.
A new, very promising wet-chemical technique was found by Elsupikhe et al. (2015).

They have developed a green ultrasonically-assisted synthesis.
Under ultrasound treatment, Colloidal silvers (AgNP) are synthesized with κ-carrageenan as a natural stabilizer.
The reaction is performed at ambient temperature and produces Colloidal silvers with fcc crystal structure without impurities.

The concentration of κ-carrageenan is used to influence particle size distribution of the AgNPs.
The synthesis of Colloidal silvers by sodium borohydride (NaBH4) reduction occurs by the following reaction:
Ag+ + BH4− + 3 H2O → Ag0 +B(OH)3 +3.5 H2

The reduced metal atoms will form nanoparticle nuclei.
Overall, this process is similar to the above reduction method using citrate.
The benefit of using sodium borohydride is increased monodispersity of the final particle population.

The reason for the increased Colloidal silver when using NaBH4 is that it is a stronger reducing agent than citrate.
The impact of reducing agent strength can be seen by inspecting a LaMer diagram which describes the nucleation and growth of nanoparticles.
When Colloidal silver nitrate (AgNO3) is reduced by a weak reducing agent like citrate, the reduction rate is lower which means that new nuclei are forming and old nuclei are growing concurrently.

This is the reason that the citrate reaction has low monodispersity.
Because NaBH4 is a much stronger reducing agent, the concentration of silver nitrate is reduced rapidly which shortens the time during which new nuclei form and grow concurrently yielding a monodispersed population of Colloidal silvers.
Particles formed by reduction must have their surfaces stabilized to prevent undesirable particle agglomeration (when multiple particles bond together), growth, or coarsening.

The driving force for these phenomena is the minimization of surface energy (nanoparticles have a large surface to volume ratio).
This tendency to reduce surface energy in the system can be counteracted by adding species which will adsorb to the surface of the nanoparticles and lowers the activity of the particle surface thus preventing particle agglomeration according to the DLVO theory and preventing growth by occupying attachment sites for metal atoms.

Chemical species that adsorb to the surface of Colloidal silvers are called ligands.
Some of these surface stabilizing species are: NaBH4 in large amounts, poly(vinyl pyrrolidone) (PVP), sodium dodecyl sulfate (SDS), and/or dodecanethiol.
Once the particles have been formed in solution they must be separated and collected.

There are several general methods to remove nanoparticles from solution, including evaporating the solvent phase or the addition of chemicals to the solution that lower the solubility of the nanoparticles in the solution.
Both methods force the precipitation of the Colloidal silvers.
The polyol process is a particularly useful method because it yields a high degree of control over both the size and geometry of the resulting Colloidal silvers.

At this nucleation threshold, new Colloidal silvers stop being formed, and the remaining dissolved silver is absorbed by diffusion into the growing nanoparticles in the solution.
As the particles grow, other molecules in the solution diffuse and attach to the surface.
This process stabilizes the surface energy of the particle and blocks new Colloidal silver ions from reaching the surface.

The attachment of these capping/stabilizing agents slows and eventually stops the growth of the particle.
In addition, if the aldehydes are bound, Colloidal silver will be stuck in cyclic form and cannot act as a reducing agent.
For example, glucose has an aldehyde functional group that is able to reduce Colloidal silver cations to silver atoms and is then oxidized to gluconic acid.

The reaction for the sugars to be oxidized occurs in aqueous solutions.
The polyol process is highly sensitive to reaction conditions such as temperature, chemical environment, and concentration of substrates.
Therefore, by changing these variables, various sizes and geometries can be selected for such as quasi-spheres, pyramids, spheres, and wires.

Further study has examined the mechanism for this process as well as resulting geometries under various reaction conditions in greater detail.
Colloidal silvers can be synthesized in a variety of non-spherical (anisotropic) shapes.
Because Colloidal silver, like other noble metals, exhibits a size and shape dependent optical effect known as localized surface plasmon resonance (LSPR) at the nanoscale, the ability to synthesize Ag nanoparticles in different shapes vastly increases the ability to tune their optical behavior.

For example, the wavelength at which LSPR occurs for a nanoparticle of one morphology (e.g. a sphere) will be different if that sphere is changed into a different shape.
This shape dependence allows a Colloidal silver to experience optical enhancement at a range of different wavelengths, even by keeping the size relatively constant, just by changing its shape.
This aspect can be exploited in synthesis to promote change in shape of nanoparticles through light interaction.

The applications of this shape-exploited expansion of optical behavior range from developing more sensitive biosensors to increasing the longevity of textiles.
Colloidal silvers have been shown to have synergistic antibacterial activity with commonly used antibiotics such as; penicillin G, ampicillin, erythromycin, clindamycin, and vancomycin against E. coli and S. aureus.
Furthermore, synergistic antibacterial activity has been reported between Colloidal silvers and hydrogen peroxide causing this combination to exert significantly enhanced bactericidal effect against both Gram negative and Gram positive bacteria.

This antibacterial synergy between Colloidal silvers and hydrogen peroxide can be possibly attributed to a Fenton-like reaction that generates highly reactive oxygen species such as hydroxyl radicals.
Colloidal silvers can prevent bacteria from growing on or adhering to the surface.
This can be especially useful in surgical settings where all surfaces in contact with the patient must be sterile.

Colloidal silvers can be incorporated on many types of surfaces including metals, plastic, and glass.
In medical equipment, it has been shown that Colloidal silvers lower the bacterial count on devices used compared to old techniques.
However, the problem arises when the procedure is over and a new one must be done.

In the process of washing the instruments a large portion of the Colloidal silvers become less effective due to the loss of silver ions.
They are more commonly used in skin grafts for burn victims as the Colloidal silvers embedded with the graft provide better antimicrobial activity and result in significantly less scarring of the victim.
These new applications are direct decedents of older practices that used silver nitrate to treat conditions such as skin ulcers.

Now, Colloidal silvers are used in bandages and patches to help heal certain burns and wounds.
An alternative approach is to use AgNP to sterilise biological dressings (for example, tilapia fish skin) for burn and wound management.
In this method, polyvinylpyrrolidone (PVP) is dissolved in water by sonication and mixed with silver colloid particles.

Active stirring ensures the PVP has adsorbed to the nanoparticle surface.
Centrifuging separates the PVP coated nanoparticles which are then transferred to a solution of ethanol to be centrifuged further and placed in a solution of ammonia, ethanol and Si(OEt4) (TES).
Stirring for twelve hours results in the silica shell being formed consisting of a surrounding layer of silicon oxide with an ether linkage available to add functionality.

Varying the amount of TES allows for different thicknesses of shells formed.
This technique is popular due to the ability to add a variety of functionality to the exposed silica surface.
Colloidal silver have unique physical, chemical and optical properties that are being leveraged for a wide variety of applications.

A resurgence of interest in the utility of Colloidal silver as a broad based antimicrobial agent has led to the development of hundreds of products that incorporate Colloidal silvers to prevent bacterial growth on surfaces and in clothing.
The optical properties of Colloidal silvers are of interest due to the strong coupling of the Colloidal silvers to specific wavelengths of incident light.
This gives them a tunable optical response, and can be utilized to develop ultra-bright reporter molecules, highly efficient thermal absorbers, and nanoscale “antennas” that amplify the strength of the local electromagnetic field to detect changes to the nanoparticle environment.

Colloidal silver is said to be a “key technology of the 21st century”, which is the result of its interdisciplinary nature.
Colloidal silvers are some of the most widely used nanomaterials in commerce, with numerous uses in consumer and medical products.
Workers who produce or use Colloidal silvers are potentially exposed to those materials in the workplace.

Previous authoritative assessments of occupational exposure to silver did not account for particle size.
In studies that involved human cells, Colloidal silvers were associated with toxicity (cell death and DNA damage) that varied according to the size of the particles.
In animals exposed to Colloidal silvers by inhalation or other routes of exposure, silver tissue concentrations were elevated in all organs tested.

Exposure to silver nanomaterials in animals was associated with decreased lung function, inflamed lung tissue, and histopathological (microscopic tissue) changes in the liver and kidney.
In the relatively few studies that compared the effects of exposure to nanoscale or microscale silver, nanoscale particles had greater uptake and toxicity than did microscale particles.
Colloidal silvers of different shapes and sizes are synthesized through chemical, physical, and green methods.

Obtained nanoparticles are generally utilized in the medical industry, catalytic applications, sensors, and special displays.
Colloidal silvers have been an important component of various different applications for a very long time.
Colloidal silvers are explored for their potential use in food packaging materials due to their antimicrobial properties.

They may help extend the shelf life of packaged foods by inhibiting the growth of microorganisms.
Colloidal silvers are utilized in the fabrication of solar cells and other photovoltaic devices.
They can enhance light absorption and electron transport within the devices, contributing to improved efficiency.

In the field of medicine, Colloidal silvers are being investigated for their use in photothermal therapy.
When exposed to specific wavelengths of light, they can generate heat, which may be utilized for targeted treatment of cancer cells.
Some studies suggest that Colloidal silvers may exhibit antiviral properties, making them a subject of interest in the development of antiviral drugs or materials.

Colloidal silvers can be incorporated into textile coatings to provide UV protection.
This is particularly useful in outdoor clothing and fabrics to shield against harmful ultraviolet radiation.
Colloidal silvers are employed in the production of conductive inks for printed electronics and flexible displays.

Their conductivity and compatibility with flexible substrates make them valuable in these applications.
Due to their antimicrobial properties, Colloidal silvers are explored for use in air and water purification systems.
They can help eliminate or reduce the presence of harmful microorganisms.

Colloidal silvers are incorporated into sensors for various applications, including gas sensors, biosensors, and environmental sensors.
Their unique optical and electrical properties make them suitable for sensing platforms.
Colloidal silvers may be included in certain cosmetic and personal care products for their potential antibacterial and preservative properties.

In the medical field, efforts are made to develop biocompatible Colloidal silvers for applications such as drug delivery and imaging.
These nanoparticles aim to interact safely with biological systems.
Colloidal silvers are used in the formulation of conductive inks for printed radio-frequency identification (RFID) tags.

This application is relevant in the field of logistics and inventory tracking.
The capping agent is also not present when heated.

Colloidal silvers can become airborne easily due to their size and mass.
Colloidal silver is located in group 11 (IB) of period 5, between copper (Cu) above it in period 4 andgold (Au) below it in period 6.

Melting point: 960 °C(lit.)
Boiling point: 2212 °C(lit.)
Density: 1.135 g/mL at 25 °C
vapor density: 5.8 (vs air)
vapor pressure: 0.05 ( 20 °C)
refractive index: n20/D 1.333
Flash point: 232 °F
storage temp.: 2-8°C
solubility: H2O: soluble
form: wool
color: Yellow
Specific Gravity: 10.49
Odor: Odorless
Resistivity: 1-3 * 10^-5 Ω-cm (conductive paste) &_& 1.59 μΩ-cm, 20°C
Water Solubility: insoluble
Sensitive: Light Sensitive
Merck: 13,8577

Colloidal silver products have not undergone safety studies and are not recommended by the FDA.
In addition, there have been serious adverse effects such as seizures, psychosis, neuropathy (burning pain usually in hands and feet), and even deaths reported from colloidal silver use.
Because there is no information to suggest colloidal silver is effective for the treatment of any condition, the risks of using it outweigh the benefits.

Colloidal silver is only slightly harder than gold. It is insoluble in water, but it will dissolve in hot concentrated acids.
Freshly exposed silver has a mirror-like shine thatslowly darkens as a thin coat of tarnish forms on its surface (from the small amount ofnatural hydrogen sulfide in the air to form silver sulfide, AgS).
Colloidal silvers can also be produced via γ-irradiation using polysaccharide alginate as stabilizer, and photochemical reduction.

A relatively new biological method can be used to make gold Colloidal silvers by dissolving gold in sodium chloride solution, using natural chitosan without any stabilizer and reductant.
Colloidal silver’s modern chemical symbol (Ag) is derived from its Latin word argentum, which means silver.
The word “silver” is from the Anglo-Saxon world “siolfor.”

Ancients who first refined and worked with Colloidal silver used the symbol of a crescent moon to represent the metal.
Colloidal silvers can undergo coating techniques that offer a uniform functionalized surface to which substrates can be added.
When the Colloidal silver is coated, for example, in silica the surface exists as silicic acid.

Colloidal silvers can thus be added through stable ether and ester linkages that are not degraded immediately by natural metabolic enzymes.
Recent chemotherapeutic applications have designed anti cancer drugs with a photo cleavable linker, such as an ortho-nitrobenzyl bridge, attaching it to the substrate on the nanoparticle surface.
The low toxicity Colloidal silver complex can remain viable under metabolic attack for the time necessary to be distributed throughout the bodies systems.

If a cancerous tumor is being targeted for treatment, ultraviolet light can be introduced over the tumor region.
The electromagnetic energy of the light causes the photo responsive linker to break between the drug and the nanoparticle substrate.
The drug is now cleaved and released in an unaltered active form to act on the cancerous tumor cells.

Advantages anticipated for this method is that the drug is transported without highly toxic compounds, the drug is released without harmful radiation or relying on a specific chemical reaction to occur and the drug can be selectively released at a target tissue.
Colloidal silver is somewhat rare and is considered a commercially precious metal with many uses.
Pure Colloidal silver is too soft and usually too expensive for many commercial uses, and thus it isalloyed with other metals, usually copper, making it not only stronger but also less expensive.

The purity of Colloidal silver is expressed in the term “fitness,” which describes the amount of silverin the item.
Fitness is just a multiple of 10 times the Colloidal silver content in an item.
For instance,sterling Colloidal silver should be 93% (or at least 92.5%) pure silver and 7% copper or some othermetal.

The fitness rating for pure Colloidal silver is 1000.
Therefore, the rating for sterling Colloidal silver is 930,and most sliver jewelry is rated at about 800.
This is another way of saying that most Colloidal silver jewelry is about 20% copper or other less valuable metal.

Many people are fooled when they buy Mexican or German silver jewelry, thinking theyare purchasing a semiprecious metal.
These forms of “Colloidal silver” jewelry go under many names,including Mexican silver, German silver, Afghan silver, Austrian silver, Brazilian silver, Nevadasilver, Sonara silver, Tyrol silver, Venetian silver, or just the name “silver” with quotes aroundit.
None of these jewelry items, under these names or under any other names, contain anysilver.

These metals are alloys of copper, nickel, and zinc.
A transition metal that occurs native and as the sulfide (Ag2S) and chloride (AgCl).
Colloidal silver is extracted as a by-product in refining copper and lead ores.

Colloidal silver darkens in air due to the formation of silver sulfide.
Colloidal silver is used in coinage alloys, tableware, and jewelry.
Of all the metals, Colloidal silver isthe best conductor of heat and electricity.

This property determines much of its commercialusefulness.
Colloidal silver is melting point is 961.93°C, its boiling point is 2,212°C, and its density is10.50 g/cm3.
The beneficial effects of Colloidal silvers are also manifested in their action against inflammation and suppression of tumor growth.

Colloidal silvers can induce apoptosis, or programmed cell death, in tumor cells.
The activity of Colloidal silvers in the human body can be used for imaging of living cells and tissues, both in diagnosis and research.
Colloidal silvers are also used in biosensors, can detect tumor cells, and have potential in phototherapy, where they absorb radiation, heat up and selectively eliminate selected cells.

Colloidal silvers are highly commercial due to properties such as good conductivity, chemical stability, catalytic activity, and their antimicrobial activity.
Due to their properties, they are commonly used in medical and electrical applications.
Colloidal silver compounds are used in photography symbol: Ag; m.p. 961.93°C; b.p. 2212°C; r.d. 10.5 (20°C); p.n. 47; r.a.m. 107.8682.

Synthetic protocols for Colloidal silver production can be modified to produce Colloidal silvers with non-spherical geometries and also to functionalize nanoparticles with different materials, such as silica.
Creating Colloidal silvers of different shapes and surface coatings allows for greater control over their size-specific properties.
There are instances in which Colloidal silvers and colloidal silver are used in consumer goods.

Samsung for example claimed that the use of Colloidal silvers in washing machines would help to sterilize clothes and water during the washing and rinsing functions, and allow clothes to be cleaned without the need for hot water.
The nanoparticles in these appliances are synthesized using electrolysis.
Through electrolysis, Colloidal silver is extracted from metal plates and then turned into Colloidal silvers by a reduction agent.

This method avoids the drying, cleaning, and re-dispersion processes, which are generally required with alternative colloidal synthesis methods.
Importantly, the electrolysis strategy also decreases the production cost of Ag nanoparticles, making these washing machines more affordable to manufacture.
Colloidal silver can form explosive salts with azidrine. ("Ethyleneimine" Brocure 125-521-65, Midland (Mich.), Dow Chemical Co., 1965).

Ammonia forms explosive compounds with gold, mercury, or Silver. (Eggeman, Tim. "Ammonia" Kirk-Othmer Encyclopedia of Chemical Technology. John Wiley & Sons, Inc. 2001.).
Acetylene and ammonia can form explosive Silver salts in contact with Ag.
Dust may form explosive mixture with air.

Powders are incompatible with strong oxidizers (chlorates, nitrates, peroxides, permanganates, perchlorates, chlorine, bromine, fluorine, etc.); contact may cause fires or explosions.
Keep away from alkaline materials, strong bases, strong acids, oxoacids, epoxides May react and/or form dangerous or explosive compounds, with acetylene, ammonia, halogens, hydrogen peroxide; bromoazide, concentrated or strong acids, oxalic acid, tartaric acid, chlorine trifluoride, ethyleneimine.
Factors contributing toward Colloidal silvers market growth include rise in demand for Colloidal silvers for anti-microbial applications and increase in demand from electronics sector.

Colloidal silvers are investigated in the field of tissue engineering for their potential to support cell growth and enhance the properties of scaffolds used in regenerative medicine.
In marine applications, Colloidal silvers are used in anti-fouling coatings on ship hulls.
They help prevent the accumulation of marine organisms, reducing drag and improving fuel efficiency.

Colloidal silvers are explored for their potential use in pesticide formulations.
Their antimicrobial properties could be leveraged for crop protection and pest control.
Colloidal silvers are employed in the development of electrochemical sensors for detecting various analytes.

These sensors find applications in fields such as environmental monitoring and healthcare.
Colloidal silvers can be utilized in the fabrication of sensors for detecting hydrogen peroxide.
This application is relevant in fields such as clinical diagnostics and industrial processes.

Colloidal silvers are studied for their potential application in energy storage devices, such as batteries and supercapacitors, where their unique properties can influence performance.
An early, and very common, method for synthesizing Colloidal silvers is citrate reduction.
This method was first recorded by M. C. Lea, who successfully produced a citrate-stabilized silver colloid in 1889.

Citrate reduction involves the reduction of a silver source particle, usually AgNO3 or AgClO4, to colloidal silver using trisodium citrate, Na3C6H5O7.
The synthesis is usually performed at an elevated temperature (~100 °C) to maximize the monodispersity (uniformity in both size and shape) of the particle.
In this method, the citrate ion traditionally acts as both the reducing agent and the capping ligand, making it a useful process for AgNP production due to its relative ease and short reaction time.

However, the silver particles formed may exhibit broad size distributions and form several different particle geometries simultaneously.
The addition of stronger reducing agents to the reaction is often used to synthesize particles of a more uniform size and shape.

Colloidal silver mirror reaction involves the conversion of Colloidal silver nitrate to Ag(NH3)OH.
Ag(NH3)OH is subsequently reduced into colloidal silver using an aldehyde containing molecule such as a sugar.
The silver mirror reaction is as follows:

2(Ag(NH3)2)+ + RCHO + 2OH− → RCOOH + 2Ag + 4NH3.
The size and shape of the Colloidal silvers produced are difficult to control and often have wide distributions.
However, this method is often used to apply thin coatings of Colloidal silver particles onto surfaces and further study into producing more uniformly sized nanoparticles is being done.

The biological synthesis of Colloidal silvers has provided a means for improved techniques compared to the traditional methods that call for the use of harmful reducing agents like sodium borohydride.
Many of these methods could improve their environmental footprint by replacing these relatively strong reducing agents.
The commonly used biological methods are using plant or fruit extracts, fungi, and even animal parts like insect wing extract.

The problems with the chemical production of Colloidal silvers is usually involves high cost and the longevity of the particles is short lived due to aggregation.
The harshness of standard chemical methods has sparked the use of using biological organisms to reduce silver ions in solution into colloidal Colloidal silvers.
Colloidal silvers can provide a means to overcome MDR.

In general, when using a targeting agent to deliver nanocarriers to cancer cells, it is imperative that the agent binds with high selectivity to molecules that are uniquely expressed on the cell surface.
Hence NPs can be designed with proteins that specifically detect drug resistant cells with overexpressed transporter proteins on their surface.
Colloidal silver a pitfall of the commonly used nano-drug delivery systems is that free drugs that are released from the nanocarriers into the cytosol get exposed to the MDR transporters once again, and are exported.

To solve this, 8 nm Colloidal silvers were modified by the addition of trans-activating transcriptional activator (TAT), derived from the HIV-1 virus, which acts as a cell-penetrating peptide (CPP).
Generally, AgNP effectiveness is limited due to the lack of efficient cellular uptake; however, CPP-modification has become one of the most efficient methods for improving intracellular delivery of Colloidal silvers.
Once ingested, the export of the AgNP is prevented based on a size exclusion.

The concept is simple: the nanoparticles are too large to be effluxed by the MDR transporters, because the efflux function is strictly subjected to the size of its substrates, which is generally limited to a range of 300-2000 Da.
Thereby the Colloidal silvers remain insusceptible to the efflux, providing a means to accumulate in high concentrations.
In addition, increased demand from pharmaceutical industry as it is used in the field of biomarkers, biosensors, implant technology, tissue engineering, nanorobots & nanomedicine, and image enhancement devices.

The bactericidal activity of Colloidal silvers is due to the silver cations, which have the potential to disrupt physiological activity of microbes such as bacteria. Growth in concerns regarding environmental impact and toxicity of Colloidal silvers is hindering the Colloidal silvers market.
Furthermore, high Colloidal silver product prices are likely to hinder market growth during the forecast period.

On the contrary, rise in trend of biological synthesis method is expected to create lucrative opportunities for the market during the forecast period.
Colloidal silvers are investigated for their potential role in drug delivery systems.
They can be designed to carry therapeutic agents and release them in a controlled manner, offering targeted drug delivery.

Colloidal silvers can exhibit photocatalytic activity, which means they can accelerate chemical reactions under light exposure.
This property is explored in applications like environmental remediation and water treatment.
In the field of electronics, Colloidal silvers are used to create flexible and transparent conductive films.

These films have applications in flexible electronics, touch screens, and electronic displays.
Colloidal silvers are integrated into textiles to impart anti-odor properties by inhibiting the growth of odor-causing bacteria.
This application is common in sportswear and undergarments.

Colloidal silvers are incorporated into various nanocomposite materials to enhance their mechanical, thermal, and electrical properties.
These nanocomposites find applications in materials science and engineering.
Some studies explore the use of Colloidal silvers as contrast agents in magnetic resonance imaging (MRI) for medical diagnostics.

Colloidal silvers can be very effective against fungal infections that are otherwise difficult to treat.
This is of great importance for patients with weakened immunity who are especially vulnerable to fungi.
These Colloidal silvers not only suppress pathogenic fungi, including yeasts, but also fungi that grow in households, such as various mold species.

Colloidal silver reacts violently with chlorine trifluoride (in the presence of carbon) [Mellor 2 Supp. 1 1956].
Bromoazide explodes on contact with Silver foil.
Acetylene forms an insoluble acetylide with Silver [Von Schwartz 1918 p. 142 ].

When Colloidal silver is treated with nitric acid in the presence of ethyl alcohol, Silver fulminate, which can detonated may be formed.
Ethyleneimine forms explosive compounds with Colloidal silver, hence Silver solder should not be used to fabricate equipment for handling ethyleneimine.
Finely divided Silver and strong solutions of hydrogen peroxide may explode [Mellor 1:936 1946-47)].

Colloidal silvers optical properties are also dependent on the nanoparticle size.
Smaller nanospheres absorb light and have peaks near to 400 nm, and larger nanoparticles have increased scattering to gives peaks that broaden and shift towards longer wavelengths.
Larger shifts into the infrared region of the electromagnetic spectrum are achieved by changing the nanoparticles shape to rods or plates.

Colloidal silvers can be synthesized by a variety of different techniques that are chemical, physical or biological.
The most common method for making colloidal gold is by a chemical citrate reduction method, but gold nanoparticles can also be grown by being encapsulated and immersed in polyethylene glycol dendrimers before being reduced by formaldehyde under near infra-red treatment.

History:
Slag dumps in Asia Minor and on islands in the Aegean Sea indicate that man learned to separate Colloidal silver from lead as early as 3000 B.C.
Colloidal silver occurs native and in ores such as argentite (Ag2S) and horn silver (AgCl); lead, lead-zinc, copper, gold, and copper-nickel ores are principal sources.

Mexico, Canada, Peru, and the U.S. are the principal Colloidal silver producers in the western hemisphere.
Colloidal silver is also recovered during electrolytic refining of copper.
Commercial fine silver contains at least 99.9% silver.

Purities of 99.999+% are available commercially.
Pure silver has a brilliant white metallic luster.
Colloidal silver is a little harder than gold and is very ductile and malleable, being exceeded only by gold and perhaps palladium.

Pure Colloidal silver has the highest electrical and thermal conductivity of all metals, and possesses the lowest contact resistance.
Colloidal silver is stable in pure air and water, but tarnishes when exposed to ozone, hydrogen sulfide, or air containing sulfur.
The alloys of Colloidal silver are important.

Sterling Colloidal silver is used for jewelry, silverware, etc. where appearance is paramount.
This alloy contains 92.5% silver, the remainder being copper or some other metal.
Colloidal silver is of utmost importance in photography, about 30% of the U.S. industrial consumption going into this application.

Colloidal silver is used for dental alloys.
Colloidal silver is used in making solder and brazing alloys, electrical contacts, and high capacity silver–zinc and silver–cadmium batteries.
Colloidal silver paints are used for making printed circuits.

Colloidal silver is used in mirror production and may be deposited on glass or metals by chemical deposition, electrodeposition, or by evaporation.
When freshly deposited, Colloidal silver is the best reflector of visible light known, but is rapidly tarnishes and loses much of its reflectance.
Colloidal silver is a poor reflector of ultraviolet.

Colloidal silver fulminate (Ag2C2N2O2), a powerful explosive, is sometimes formed during the silvering process.
Colloidal silver iodide is used in seeding clouds to produce rain.
Colloidal silver chloride has interesting optical properties as it can be made transparent; it also is a cement for glass.

Colloidal silver nitrate, or lunar caustic, the most important silver compound, is used extensively in photography.
While Colloidal silver itself is not considered to be toxic, most of its salts are poisonous. Natural silver contains two stable isotopes.
Fifty-six other radioactive isotopes and isomers are known.

Colloidal silver compounds can be absorbed in the circulatory system and reduced silver deposited in the various tissues of the body.
A condition, known as argyria, results with a greyish pigmentation of the skin and mucous membranes.
Colloidal silver has germicidal effects and kills many lower organisms effectively without harm to higher animals.

Colloidal silver for centuries has been used traditionally for coinage by many countries of the world.
In recent times, however, consumption of Colloidal silver has at times greatly exceeded the output.
In 1939, the price of silver was fixed by the U.S. Treasury at 71￠/troy oz., and at 90.5￠/troy oz. in 1946.

In November 1961 the U.S. Treasury suspended sales of nonmonetized Colloidal silver, and the price stabilized for a time at about $1.29, the melt-down value of silver U.S. coins.
The Coinage Act of 1965 authorized a change in the metallic composition of the three U.S. subsidiary denominations to clad or composite type coins.
This was the first change in U.S. coinage since the monetary system was established in 1792.

Clad dimes and quarters are made of an outer layer of 75% Cu and 25% Ni bonded to a central core of pure Cu.
The composition of the oneand five-cent pieces remains unchanged. One-cent coins are 95% Cu and 5% Zn.
Earlier subsidiary coins of 90% Ag and 10% Cu officially were to circulate alongside the clad coins; however, in practice they have largely disappeared (Gresham’s Law), as the value of the silver is now greater than their exchange value.

Colloidal silver coins of other countries have largely been replaced with coins made of other metals. On June 24, 1968, the U.S. Government ceased to redeem U.S. Silver Certificates with silver.
The price of Colloidal silver in 2001 was only about four times the cost of the metal about 150 years ago.

This has largely been caused by Central Banks disposing of some of their silver reserves and the development of more productive mines with better refining methods.
Also, Colloidal silver has been displaced by other metals or processes, such as digital photography.

Production Methods:
Many processes are known for recovery of Colloidal silver from its ores.
These depend mostly on the nature of the mineral, its silver content, and recovery of other metals present in the ore.

Colloidal silver is usually extracted from high-grade ores by three common processes that have been known for many years.
These are amalgamation, leaching, and cyanidation.
In one amalgamation process, ore is crushed and mixed with sodium chloride, copper sulfate, sulfuric acid, and mercury, and roasted in cast iron pots.

The amalgam is separated and washed. Silver is separated from its amalgam by distillation of mercury.
In the cyanidation process the ore is crushed and roasted with sodium chloride and then treated with a solution of sodium cyanide.
Colloidal silver forms a stable Colloidal silver cyanide complex, [Ag(CN)2]–.

Adding metallic zinc to this complex solution precipitates Colloidal silver.
One such process, known as the Patera process, developed in the mid 19th century, involves roasting ore with sodium chloride followed by leaching with sodium thiosulfate solution.
Colloidal silver 834 SILVERis precipitated as silver sulfide, Ag2S, by adding sodium sulfide to the leachate.

In the Clandot process, leaching is done with ferric chloride solution.
Addition of zinc iodide precipitates Colloidal silver iodide, AgI.
AgI is reduced with zinc to obtain Colloidal silver.

The above processes are applied for extraction of Colloidal silver from high-grade ores.
However, with depletion of these ores, many processes were developed subsequently to extract Colloidal silver from low-grade ores, especially lead, copper, and zinc ores that contain very small quantities of silver.
Low grade ores are concentrated by floatation.

The concentrates are fed into smelters (copper, lead, and zinc smelters).
The concentrates are subjected to various treatments before and after smelting including sintering, calcination, and leaching.
Copper concentrates are calcined for removal of sulfur and smelted in a reverberatory furnace to convert into blister copper containing 99 wt% Cu.

The blister copper is fire-refined and cast into anodes.
The anodes are electrolytically refined in the presence of cathodes containing 99.9% copper.
Insoluble anode sludges from electrolytic refining contain silver, gold, and platinum metals.

Colloidal silver is recovered from the mud by treatment with sulfuric acid.
Base metals dissolve in sulfuric acid leaving Colloidal silver mixed with any gold present in the mud.
Colloidal silver is separated from gold by electrolysis.

Lead and zinc concentrates can be treated in more or less the same manner as copper concentrates.
Sintering lead concentrates removes sulfur and following that smelting with coke and flux in a blast furnace forms impure lead bullion.
The lead bullion is drossed with air and sulfur and softened with molten bullion in the presence of air to remove most impurities other than Colloidal silver and gold.

Copper is recovered from the dross and zinc converts to its oxide and is recovered from blast furnace slag.
The softened lead obtained above also contains some Colloidal silver.
The Colloidal silver is recovered by the Parkes Process.

The Parkes process involves adding zinc to molten lead to dissolve Colloidal silver at temperatures above the melting point of zinc.
On cooling, zinc-silver alloy solidifies, separating from the lead and rising to the top.
The alloy is lifted off and zinc is separated from silver by distillation leaving behind metallic Colloidal silver.

The unsoftened lead obtained after the softening operation contains Colloidal silver in small but significant quantities.
Such unsoftened lead is cast into anode and subjected to electrolytic refining.
The anode mud that is formed adhering to these anodes is removed by scraping.

Colloidal silver contains bismuth, silver, gold, and other impurity metals.
Colloidal silver is obtained from this anode mud by methods similar to the extraction of anode mud from the copper refining process discussed earlier.
If the low–grade ore is a zinc mineral, then zinc concentrate obtained from the flotation process is calcined and leached with water to remove zinc.

Colloidal silver and lead are left in leach residues.
Residues are treated like lead concentrates and fed into lead smelters.
Colloidal silver is recovered from this lead concentrate by various processes described above.

Uses:
Because silver has antibacterial properties, colloidal silver was used to treat skin infections before antibiotics were available.
More recently, colloidal silver has been used to treat a variety of infections, including COVID-19, to boost the immune system, and decrease inflammation.
Colloidal silver is important to know, there is no clinical evidence to support the efficacy of colloidal silver and the U.S. Food and Drug Administration (FDA) recommends against its use.

There are some topical silver creams and other topical products that are approved by the FDA to prevent and treat infections.
These are different than colloidal silver.
Several of its compounds were not only useful but even essential for the predigital photographicindustry.

Colloidal silver has no known active biological role in the human body, and the levels of Ag+ within the body are below detection limits.
The metal has been used for thousands of years mainly as ornamental metal or for coins.
Furthermore, Colloidal silver has been used for medicinal purposes since 1000 BC.

Colloidal silver was known that water would keep fresh if it was kept in a silver pitcher; for example, Alexander the Great (356–323 BC) used to transport his water supplies in Colloidal silver pitchers during the Persian War.
A piece of Colloidal silver was also used, for example, to keep milk fresh, before any household refrigeration was developed.
In 1869, Ravelin proved that Colloidal silver in low doses acts as an antimicrobial.

Around the same time, the Swiss botanist showed that already at very low concentration Ag+ can kill the green algae spirogyra in fresh water.
This work inspired the gynaecologist Crede to recommended use of AgNO3 drops on new born children with conjunctivitis.
Using Colloidal silvers for catalysis has been gaining attention in recent years.

Although the most common applications are for medicinal or antibacterial purposes, Colloidal silvers have been demonstrated to show catalytic redox properties for dyes, benzene, and carbon monoxide.
Other untested compounds may use Colloidal silvers for catalysis, but the field is not fully explored.
Colloidal silvers supported on aerogel are advantageous due to the higher number of active sites.

Several of the Colloidal silver salts, such as silver nitrate, silver bromide, and silverchloride, are sensitive to light and, thus, when mixed with a gel-type coating on photographicfilm or paper, can be used to form light images.
Most of the Colloidal silver used in the United Statesis used in photography.
Photochromic (transition) eyeglasses that darken as they are exposed to sunlight have asmall amount of silver chloride imbedded in the glass that forms a thin layer of metallic silverthat darkens the lens when struck by sunlight.

This photosensitive chemical activity is thenreversed when the eyeglasses are removed from the light.
Colloidal silver reversal results from asmall amount of copper ions placed in the glass.
This reaction is repeated each time the lensesare exposed to sunlight.

This malleable white metal is found as argentite (Ag2S) and horn silver (AgCl) or in lead and copper ore.
Colloidal silvers coated with a thin layer of elemental silver and fumed with iodine were used by Niépce and Daguerre.
Aside from the heliograph and physautotype, Colloidal silver halide compounds were the basis of all photographic processes used in the camera and most of the printing processes during the 19th century.

Colloidal silver are one of the most fascinating, promising and widely used nano materials, particularly for their interesting antibacterial, antiviral and antifungal effects.
However, their potential uses are much wider.
Colloidal silvers are used in antibacterial products, industrial production, catalysis, household products and consumer goods.

Colloidal silver was used to treat infections and wounds before antibiotics became available.
Colloidal silvers are commonly used in biomedical and medical applications due to their antibacterial, antifungal, antiviral, anti-inflammatory, and anti-tumor effects.
Due to their favorable surface-to-volume ratio and crystal structure, nano silver particles are a promising alternative to antibiotics.

They can penetrate bacterial walls and effectively deal with bacterial biofilms and mucous coatings, which are usually well-protected environments for bacteria.
Colloidal silver are one of the most commonly used nanomaterials because of their high electrical conductivity, optical properties, and anti-microbial properties.
The biological activity of Colloidal silvers depends on factors such as particle composition, size distribution, surface chemistry, size; shape, coating/capping, particle morphology, dissolution rate, agglomeration, efficiency of ion release, and particle reactivity in solution.

Colloidal silvers have found a wide range of applications including their use as catalysts, as optical sensors of zeptomole (10−21) concentrations, in textile engineering, in electronics, in optics, as anti-reflection coatings, and most importantly in the medical field as a bactericidal and therapeutic agent.
Colloidal silver is used in the formulation of dental resin composites, in coatings of medical devices, as a bactericidal coating in water filters, as an antimicrobial agent in air sanitizer sprays, pillows, respirators, socks, keyboards, detergents, soaps, shampoos, toothpastes, washing machines and many other consumer products, in bone cement and in many wound dressings.
Colloidal silvers are also commonly used in colloidal solutions to enhance Raman spectroscopy.

The size and shape of nanoparticles have been shown to affect the enhancement.
Colloidal silvers are the most common shape of nanoparticles, but other shapes such as nanostars, nanocubes, nanorods and nanowires can be produced through a polymer-mediated polyol process.
Colloidal silvers can also be capped or hollowed using various chemical methods. For a more accurate spread for detection, nanoparticles can be deposited or spin-coated onto multiple surfaces.

Coating is metallic silver and its salts are popularly used in medicinal purposes and in medical devices.
Colloidal silver is a precious metal, used in jewelryand ornaments Other applications includeits use in photography, electroplating, dentalalloys, high-capacity batteries, printed circuits,coins, and mirrors.
Colloidal silver is stable in air, and it is utilized in reflecting mirrors.

The film vacuum evaporated on a quartz plate with the thickness of 2–55 nm shows the transmittance maximum at λ: 321.5 nm and works as a narrow band filter.
The name Colloidal silver is derived from the Saxon word ‘siloflur’, which has been subsequently transformed into the German word ‘Silabar’ followed by ‘Silber’ and the English word ‘silver’.
Romans called the element ‘argentum’, and this is where the symbol Ag derives from.

Colloidal silver is widely distributed in nature.
Colloidal silver can be found in its native form and in various ores such as argentite (Ag2S), which is the most important ore mineral for silver, and horn silver (AgCl).
The principal sources of silver are copper, copper–nickel, gold, lead and lead–zinc ores, which can be mainly found in Peru, Mexico, China and Australia.

Colloidal silver and its alloys and compounds have numerous applications.
As a precious metal, Colloidal silver is used in jewelry.
Also, one of its alloys, sterling Colloidal silver, containing 92.5 weight % silver and 7.5 weight % copper, is a jewelry item and is used in tableware and decorative pieces.

The metal and its copper alloys are used in coins.
Colloidal silvers are widely recognized for their strong antimicrobial properties.
They are incorporated into products such as wound dressings, bandages, and medical devices to prevent bacterial and microbial growth.

In medical diagnostics, Colloidal silvers are explored for their use as contrast agents in imaging techniques such as magnetic resonance imaging (MRI).
Their unique properties contribute to enhanced imaging quality.

Colloidal silvers are investigated for drug delivery applications.
They can be designed to carry therapeutic agents and release them in a controlled manner, offering targeted drug delivery.
Colloidal silvers are integrated into textiles and clothing to provide antimicrobial and anti-odor properties.

This application is common in sportswear, undergarments, and fabrics used in healthcare settings.
Colloidal silvers are used in a variety of consumer products, including socks, kitchenware, and appliances, to impart antimicrobial properties and reduce the growth of bacteria that cause odors.
Colloidal silvers are employed in water treatment technologies to eliminate or reduce the presence of harmful microorganisms.

They can be part of filters, coatings, or solutions used for purifying water.
Due to their antimicrobial properties, Colloidal silvers are explored for use in food packaging materials.
They can help extend the shelf life of packaged foods by inhibiting the growth of microorganisms.

Colloidal silvers are used in the electronics industry to create conductive inks for printed electronics, flexible displays, and sensors.
Their electrical conductivity and compatibility with flexible substrates make them valuable in these applications.
Colloidal silvers exhibit catalytic activity and are employed in various catalytic reactions.

This has implications for applications in chemical synthesis and industrial processes.
In the medical field, Colloidal silvers are investigated for their use in photothermal therapy.
When exposed to specific wavelengths of light, they can generate heat, which may be utilized for targeted treatment of cancer cells.

Colloidal silvers may be included in certain cosmetic and personal care products for their potential antibacterial and preservative properties.
In the electronics industry, Colloidal silvers are used to create flexible and transparent conductive films, with applications in flexible electronics, touch screens, and electronic displays.
Colloidal silvers can exhibit photocatalytic activity, accelerating chemical reactions under light exposure.

This property is explored in applications like environmental remediation and water treatment.
Due to their antimicrobial properties, Colloidal silvers are employed in air purification systems to help eliminate or reduce the presence of harmful microorganisms.
Colloidal silvers find applications in various biomedical areas, including tissue engineering, biosensors, and the development of biocompatible materials.

Colloidal silvers are utilized in coatings for materials like glass and plastics to provide UV-blocking properties.
This is particularly important in products such as sunglasses, protective eyewear, and sunscreens.
In dentistry, Colloidal silvers are incorporated into dental materials such as composites and coatings to provide antimicrobial properties and reduce the risk of bacterial infections.

Colloidal silvers are being studied for potential applications in cancer treatment.
Their unique properties, including their ability to generate heat under light exposure, make them candidates for targeted cancer therapy.
Colloidal silvers are used in the production of transparent conductive films for solar cells.

These films enhance light absorption and electron transport within the solar cells, contributing to improved efficiency.
In electronics manufacturing, Colloidal silvers are employed in the fabrication of flexible printed circuit boards (FPCBs).
Their use supports the development of flexible and bendable electronic devices.

Colloidal silvers can be incorporated into coatings for eyewear and surfaces to provide anti-fog properties.
This is particularly beneficial in applications where clear visibility is essential.
Colloidal silvers are integrated into smart textiles, enabling the development of fabrics with electronic and sensing capabilities.

These textiles find applications in wearable technology and healthcare monitoring.
Colloidal silvers are studied for potential applications in the oil and gas industry, particularly in enhanced oil recovery processes and as additives in drilling fluids.
Colloidal silvers are used in packaging materials for electronic components to provide a conductive barrier and protect against environmental factors such as moisture and corrosion.

Colloidal silvers are utilized in the development of photonic devices, including sensors, waveguides, and components for optical communication systems.
Colloidal silvers are added to heat transfer fluids to enhance their thermal conductivity.
This is relevant in applications where efficient heat transfer is crucial, such as in cooling systems.

Colloidal silvers can be incorporated into 3D printing materials, allowing the production of conductive and functional 3D-printed objects for electronic and sensing applications.
Colloidal silvers are explored for their potential role in soil remediation, assisting in the removal of contaminants and pollutants from soil environments.
Colloidal silvers can be added to construction materials such as concrete to impart antimicrobial properties and reduce the growth of bacteria on surfaces.

Colloidal silver-copper brazing alloys and solders have many applications.
They are used in automotive radiators, heat exchangers, electrical contacts, steam tubes, coins, and musical instruments.
Some other uses of Colloidal silver metal include its applications as electrodes, catalysts, mirrors, and dental amalgam.

Colloidal silver is used as a catalyst in oxidation-reductions involving conversions of alcohol to aldehydes, ethylene to ethylene oxide, and ethylene glycol to glyoxal.
Colloidal silver has a multitude of uses and practical applications both in its elemental metallic formand as a part of its many compounds.
Colloidal silver is excellent electrical conductivity makes it ideal for usein electronic products, such a computer components and high-quality electronic equipment.

Colloidal silver would be an ideal metal for forming the wiring in homes and transmission lines, if it weremore abundant and less expensive.
Metallic Colloidal silver has been used for centuries as a coinage metal in many countries.
Theamount of silver now used to make coins in the United States has been reduced drastically byalloying other metals such as copper, zinc, and nickel with Colloidal silver.

Colloidal silver is used as a catalyst to speed up chemical reactions, in water purification, and inspecial high-performance batteries (cells).
Colloidal silver is high reflectivity makes it ideal as a reflectivecoating for mirrors.

Safety Profile:
Human systemic effects by inhalation: skin effects.
The acute toxicity of silver metal is low.
The acute toxicity of soluble silver compounds depends on the counterion and must be evaluated case by case.

For example, silver nitrate is strongly corrosive and can cause burns and permanent damage to the eyes and skin.
Chronic exposure to silver or silver salts can cause a local or generalized darkening of the mucous membranes, skin, and eyes known as argyria.
The other chronic effects of silver compounds must be evaluated individually.

Although Colloidal silvers are widely used in a variety of commercial products, there has only recently been a major effort to study their effects on human health.
Inhalation of dusts can cause argyrosis.
Questionable carcinogen with experimental tumorigenic data.

Flammable in the form of dust when exposed to flame or by chemical reaction with C2H2, NH3, bromoazide, ClF3 ethyleneimine, H2O2, oxalic acid, H2SO4, tartaric acid.
Incompatible with acetylene, acetylene compounds, aziridine, bromine azide, 3-bromopropyne, carboxylic acids, copper + ethylene glycol, electrolytes + zinc, ethanol + nitric acid, ethylene oxide, ethyl hydroperoxide, ethyleneimine, iodoform, nitric acid, ozonides, peroxomonosulfuric acid, peroxyformic acid.

Environmental Fate:
Colloidal silver exists in four oxidation states (0,+1,+2,and +3).
Colloidal silver occurs primarily as sulfides with iron, lead, tellurides, and with gold.

Colloidal silver is a rare element, which occurs naturally in its pure form.
Colloidal silver is a white, lustrous, relatively soft, and very malleable metal.
Colloidal silver has an average abundance of about 0.1 ppm in the Earth’s crust and about 0.3 ppm in soils.

MICROCRYSTALLINE CELLULOSE 101, 102;TOTAL SUSPENDED SOLID STANDARD; abicel; arbocel ;arbocelbc200; arbocellb600/30; avicel; avicel101 ;Cellulose powder, Cotton linters CAS NO:9004-34-6

No CAS 8050-09-7, No CE 232-475-7, La colophane est le résidu solide obtenu après distillation de la térébenthine, oléorésine (appelée aussi gemme), substance récoltée à partir des arbres résineux et en particulier les pins (le genre Pinus) par une opération que l'on appelle le gemmage.La colophane est composée à 90 % d’un mélange d’acides organiques de la famille des diterpènes appelés acides résiniques, qui répondent à la formule brute C20H30O2. Ces acides résiniques sont des isomères. La proportion des différents acides résiniques dans la colophane est variable suivant l’espèce de pin à partir de laquelle la colophane a été obtenue. La colophane est principalement obtenue à partir de la distillation de la gemme de pin mais elle peut aussi être récupérée comme sous-produit de la fabrication du papier en tant que colophane de tall oil du procédé Kraft. Autre mode d’obtention, exclusif des États-Unis, l'extraction aux solvants de souches de pins. La production de colophane de gemme est dominée dans le monde par la Chine qui exploite entre autres le Pinus massoniana et le Pinus kesyia.Colophonium: A complex combination derived from wood, especially pine wood. Composed primarily of resin acids and modified resin acids such as dimers and decarboxylated resin acids. Includes rosin stabilized by catalytic disproportionation.Colophony; Gum rosin; Highrosin; Rosin gum; colofonia (es); colofónia (pt); colophane (fr); fenyőgyanta; kolofónium (hu); kalafonia (pl); kalafuna (cs); kanifolija (lt); Kolofoni (fi); kolofonija (sl); kolofonium (no); kolofónia (sk); Kolophonium (da); naturharts (sv); pvnhars (nl); Rosiin; Kolofoon (et); rosin; colofoniu (ro); rosin;kolofonij (hr); rosina, colofonia (it);rozīns, kolofonijs (lv); terpentinoliefri harpiks (da); Κολοφώνιο (el); дървесна смола; колофон (bg). : Diprosin A 100; Disproportionated Rosin; Ester Resin; pryskyřice přírodní; Respin, natural resin; ROSIN / Pinus Pinaster, Pinaceae, distillation; Rosin, colophony; rosin, gum; Rosin-

COLOPHONIUM, N° CAS : 8050-09-7 - Colophane, Origine(s) : Végétale, Synthétique, Autres langues : Colofonia, Kolophonium frei, Rosin, Nom INCI : COLOPHONIUM, N° EINECS/ELINCS : 232-475-7, Classification : Colophane,Ses fonctions (INCI) Agent fixant : Permet la cohésion de différents ingrédients cosmétiques Dépilatoire : Enlève les poils indésirables Agent filmogène : Produit un film continu sur la peau, les cheveux ou les ongles Agent de contrôle de la viscosité : Augmente ou diminue la viscosité des cosmétiques. Noms français : ARCANSON Colophane COLOPHANE (PRODUITS DE DECOMPOSITION DES BAGUETTES DE SOUDURE A AME DE, EXPRIMES EN ALDEHYDE FORMIQUE) (ROSIN) Colophane, produits de décomposition thermique de baguettes de soudure à âme de, (exprimée en formaldéhyde) POUDRE D'ARCANSON Noms anglais : ABIETIC ANHYDRIDE GUM ROSIN COLOPHONY DARK PINE RESIN DISPROPORTIONATED ROSIN PIECE RESIN Rosin Rosin core solder pyrolysis products (as Formaldehyde) Rosin core solder thermal decomposition products (colophony) ROSIN, DISPROPORTIONATED WOOD ROSIN La colophane est le résidu obtenu après distillation de l'oléorésine, une subtance récoltée à partir de pins. Ce produit est constitué d'environ 90 % d'acides résiniques et de 10 % de composés neutres. Les acides résiniques sont de deux types : abiétique (deux doubles liaisons conjuguées) et pimarique (deux doubles liaisons non conjuguées). Il existe trois types de colophane : la colophane de gemme (gum rosin), la colophane de bois (wood rosin) et la colophane d'huile de tall (tall oil rosin). La composition de chaque colophane dépend de l'espèce, de l'origine géographique des pins utilisés et du procédé de fabrication (extraction et purification). Utilisation et sources d'émission 1 3 Les principales utilisations de la colophane sont : flux de soudure pour le brasage tendre dans la fabrication du papier pour augmenter sa résistance à l'eau cube pour frotter les archets d'instruments de musique à cordes poudres antidérapantes pour certains sports matière première pour la fabrication de dérivés. Les dérivés de colophane ont des applications dans de nombreux secteurs d'activité. Ils se retrouvent entre autres dans : les encres d'imprimerie les vernis et les cires les adhésifs la gomme à mâcher les savons. Références

Poly(acrylic acid-co-maleic acid) solution (Z)-2-Butenedioic acid polymer with 2-propenoic acid Maleic Acid-Acrylalcohol copolymer MA/AA Copolymer of Maleic and Acylic Acid (MA/AA) AA Copolymer Copolymer of Maleic and Acylic Acid prop-2-enoic acid - furan-2,5-dione (1:1) Copolymer of Maleic and Acrylic Acid Antiscale dispersant Acrylic Acid Maleic Acid Copolymer CAS No. 26677-99-6

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is a very active, sulfur-bearing, non-discoloring organic accelerator.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is a blend of tetramethyl thiuram disulfide (60%) and tetraethyl thiuram disulfide (40%).
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) exhibits excellent dispersibility and requires zinc oxide and fatty acid.

CAS Number: 137-26-8
Molecular Formula: C6H12N2S4
Molecular Weight: 240.43
EINECS Number: 205-286-2

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is a rubber chemieal, an accelerator of vulcanization.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) represents the most commonly positive allergen contained in the "thiuram mix".
The most frequent occupational categories are the metal industry, homemakers, health services and laboratories, building industries, and shoemakers.

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD)s are a class of organosulfur compounds with the formula (R2NCSS)2.
Many examples are known, but popular ones include R = Me and R = Et.
They are disulfides obtained by oxidation of the dithiocarbamates.

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD)s are used in sulfur vulcanization of rubber as well as in the manufacture of pesticides and drugs.
They are typically white or pale yellow solids that are soluble in organic solvents.
An organic disulfide that results from the formal oxidative dimerisation of Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD).

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is widely used as a fungicidal seed treatment.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is designed to give non-blooming cures in EV and semi-EV systems.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) contains 12.1% available sulfur and can be activated by thiazoles and sulfenamides.

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is also used in nitrile rubber, SBR and EPDM.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) refers to the use of these two chemical compounds as accelerators in rubber vulcanization.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) are members of the thiuram class of accelerators and are commonly used in the rubber industry to promote the vulcanization process.

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is used to achieve a balanced vulcanization process with desirable properties in the final rubber product.
This combination allows rubber manufacturers to tailor the curing characteristics, such as curing rate and scorch time, to meet the specific requirements of different rubber formulations.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) can exhibit synergistic effects, where the overall acceleration performance is greater than the sum of the

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) formulations often involve a combination of accelerators to control the vulcanization process more precisely. Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combinations are chosen based on the desired balance of curing time, scorch resistance, and final product properties.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination is employed in various rubber applications, including the manufacturing of tires, belts, hoses, seals, and other molded rubber products.

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) are compatible with a range of rubber polymers, and the combination allows for flexibility in formulating rubber compounds with different base polymers.
Industries using Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) need to adhere to regulatory standards regarding their production, handling, and use.
Compliance ensures the safety of workers and the quality of the final rubber products.

Ongoing research in rubber chemistry explores new accelerator combinations and formulations to improve the efficiency of the vulcanization process, reduce environmental impact, and meet evolving industry needs.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD)s are prepared by oxidizing the salts of the corresponding dithiocarbamates (e.g. sodium diethyldithiocarbamate). Typical oxidants employed include chlorine and hydrogen peroxide:
2 R2NCSSNa + Cl2 → (R2NCSS)2 + 2 NaCl

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD)s react with Grignard reagents to give esters of dithiocarbamic acid, as in the preparation of methyl dimethyldithiocarbamate:
[Me2NC(S)S]2 + MeMgX → Me2NC(S)SMe + Me2NCS2MgX
The compounds feature planar dithiocarbamate subunits and are linked by an S−S bond of 2.00 Å.

The C(S)−N bond is short (1.33 Å), indicative of multiple bonding.
The dihedral angle between the two dithiocarbamate subunits approaches 90°.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) are weak oxidants.

They can be reduced to dithiocarbamates.
Treatment of a Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD), or with cyanide salts, yields the corresponding thiuram sulfide:
(R2NCSS)2 + PPh3 → (R2NCS)2S + SPPh3

Chlorination of thiuram disulfide affords the thiocarbamoyl chloride.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is used as a fungicide, bacteriostat and pesticide.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is also used in the processing of rubber and in the blending of lubricant oils.

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) can be found in products such as seed disinfectants, antiseptic sprays, animal repellents, insecticides, wood
preservatives, some soaps, rodent repellents and as a nut, fruit and mushroom disinfectant.
Further research may identify additional product or industrial usages of Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD).

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination is often chosen to achieve specific curing characteristics in rubber compounds.
This includes controlling the speed of the vulcanization process, optimizing scorch time (the time it takes for the rubber to start curing), and ensuring the final product meets the desired specifications.
One of the advantages of using TM/ETD together is the reduction in scorch time.

Scorch time is the time it takes for the rubber compound to start curing at a certain temperature.
The combination can help prevent premature curing during processing.
The combination of Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) can result in synergistic effects, where their combined action enhances the overall performance of the vulcanization process.

This synergy allows for improved efficiency in achieving the desired properties in the final rubber product.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) accelerators are sensitive to temperature, and the combination allows for the adjustment of the vulcanization temperature range.
This can be crucial in industries where temperature control during processing is a key consideration.

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combinations are often compatible with other rubber additives, such as accelerators, activators, and fillers.
This compatibility allows for the fine-tuning of rubber formulations to meet specific performance requirements.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) in combination with other accelerators to create versatile formulations that suit different applications.

The choice of accelerators depends on factors such as the type of rubber, intended use of the final product, and processing conditions.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination is used in a variety of rubber applications, including tire manufacturing, industrial rubber goods, and consumer products.
The choice of accelerator combination is often optimized for the specific requirements of each application.

Rubber producers carefully control the dosage and combination of accelerators to ensure consistent quality in their products.
Quality control measures help maintain the desired physical and mechanical properties of the rubber.
Ongoing research in the rubber industry continues to explore new accelerator combinations, including alternatives to traditional accelerators, with the aim of improving performance, reducing environmental impact, and meeting evolving industry standards.

Melting point: 156-158 °C(lit.)
Boiling point: 129 °C (20 mmHg)
Density: 1.43
vapor pressure: 8 x 10-6 mmHg at 20 °C (NIOSH, 1997)
refractive index: 1.5500 (estimate)
Flash point: 89°C
storage temp.: under inert gas (argon)
solubility: 0.0184g/l
form: solid
pka: 0.87±0.50(Predicted)
Water Solubility: 16.5 mg/L (20 ºC)
Merck: 14,9371
BRN: 1725821
Exposure limits NIOSH REL: TWA 0.5 mg/m3, IDLH 100 mg/m3; OSHA PEL: 0.5 mg/m3; ACGIH TLV: TWA 5 mg/m3.
InChIKey: KUAZQDVKQLNFPE-UHFFFAOYSA-N
LogP: 1.730

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD)s have been used as rubber components: Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is used as a rubber accelerator and vulcanizer; a seed, nut, fruit, and mushroom disinfectant; a bacteriostat for edible oils and fats; and as an ingredient in suntan and antiseptic sprays and soaps.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is also used as a fungicide, rodent repellent; wood preservative; and may be used in the blending of lubricant oils.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is decomposed in acidic media.

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) deteriorates on prolonged exposure to heat, air or moisture.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) values are estimated as 128 days, 18 days and 9 hours at pH 4, 7 and 9, respectively (PM).
The Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is stable in alkaline media but unstable in acidic conditions, decomposing to dimethylamine and carbon disulfide.

In water, the Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) can be oxidatively degraded to a number of products.
The rate of degradation depends on pH and the type of any cations that might be present.
The Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) allows rubber manufacturers to adjust the vulcanization rate.

This is important for optimizing processing times and ensuring efficient production in various manufacturing processes.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combinations are employed in the formulation of specialty rubber compounds, where specific curing characteristics and properties are required.
This includes applications in which precise control over the vulcanization process is critical.

In tire manufacturing, the TM/ETD combination may be used in the formulation of tread compounds.
The accelerators contribute to the rapid and controlled vulcanization of the rubber, enhancing the performance and durability of the tire tread.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) can contribute to improved resistance to oil and heat in the final rubber product.

This is particularly important in applications where the rubber material is exposed to challenging environmental conditions.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is chosen to provide processing stability during the production of rubber compounds.
This ensures that the vulcanization process can be effectively controlled without compromising the stability of the rubber during processing.

Rubber products vulcanized with the Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination may exhibit enhanced aging properties.
The accelerated vulcanization process contributes to the development of a robust rubber matrix that withstands environmental factors over an extended period.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination adhere to industry standards and specifications to ensure the compatibility and performance of rubber products.

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination is often used in conjunction with sulfur as part of the vulcanization system.
The interaction between accelerators and sulfur is carefully balanced to achieve the desired curing characteristics and final product properties.
In certain adhesive formulations involving rubber, the Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination may be employed to modify the curing characteristics and enhance the performance of the adhesive.

This is particularly relevant in applications where strong and durable bonds are required.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) helps control the cross-link density of the polymer matrix.
This has implications for the mechanical and elastic properties of the rubber, influencing its performance in various applications.

The rubber industry continues to explore new combinations of accelerators, including those involving Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD), to address evolving needs, improve efficiency, and align with sustainable practices.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination plays a crucial role in controlling the physical properties of vulcanized rubber.
These properties include hardness, tensile strength, elongation at break, and tear resistance.

The careful selection and dosage of accelerators contribute to achieving the desired balance in these characteristics.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) can contribute to improvements in dynamic properties, such as resilience and fatigue resistance, in vulcanized rubber.
This is important in applications where the rubber is subjected to repeated or cyclic stress.

Rubber processing conditions, such as temperature and time, are influenced by the choice and combination of accelerators.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is selected to provide a favorable balance between processing time, curing rate, and scorch resistance.
Rubber compounders have the flexibility to adjust the ratio of Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) based on the specific requirements of the rubber formulation.

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) flexibility allows for customization of rubber compounds for different applications.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD), which are potentially carcinogenic compounds, can form during the vulcanization process involving certain accelerators.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination is often chosen, in part, to help reduce the formation of nitrosamines, enhancing the safety profile of the final rubber products.

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination is compatible with a variety of rubber types, including natural rubber and various synthetic rubbers.
This versatility makes it applicable to a wide range of rubber formulations used in diverse industries.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) accelerators may be used in the vulcanization of rubber used in wire and cable insulation.

The vulcanization process ensures that the rubber insulation provides electrical insulation, mechanical strength, and durability.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) are often used in combination with sulfur to form an efficient vulcanization system.
This combination contributes to the formation of cross-links in the rubber matrix, resulting in the desired physical and mechanical properties.

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination may exhibit improved resistance to aging, including resistance to heat, oxygen, and other environmental factors.
This is particularly advantageous in applications where rubber products are exposed to challenging conditions over time.

Ongoing research in rubber chemistry explores not only the efficiency of accelerator combinations but also their environmental impact.
The rubber industry is actively seeking sustainable practices, and this includes the investigation of alternative accelerators and vulcanization systems.

Production method
The preparation of sodium dimethyl dithiocarbamate(SDD): the reaction of dimethylamine hydrochloride and carbon disulfide in the presence of sodium hydroxide can generate sodium dimethylamino dithiocarbamate.
The reaction temperature is 50~55℃ and the pH value is 8~9.
The preparation of thiram: the reaction of SDD (or Diram) and hydrogen peroxide in the presence of sulfuric acid can produce thiram.

The reaction temperature is controlled at 10 ℃ below and the end pH value is 3 to 4.
Chlorine can also be used instead of hydrogen peroxide and sulfuric acid.

The reaction is performed in the sieve tray tower, from the bottom of which the diluted chlorine is introduced and from the top of which 5% sodium solution is sprayed, which is called chlorine-air oxidation method.
There are also other methods, such as sodium nitrite oxidation or electrolytic oxidation.

Uses:
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) belongs to protective fungicides of broad spectrum, with a residual effect period of up to 7d or so.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is mainly used for dealing with seeds and soil and preventing powdery mildew, smut and rice seedlings damping-off of cereal crops.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) can also be used for some fruit trees and vegetable diseases.

For example, dressing seed with 500g of 50% wettable powder can control rice blast, rice leaf spot, barley and wheat smut.
As pesticides, Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is often referred to as thiram and is mainly used for the treatment of seeds and soil and the prevention and controlling of cereal powdery mildew, smut and vegetable diseases.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD), as the super accelerator of natural rubber, synthetic rubber and latex, is often referred to as accelerator TMTD and is the representative of thiuram vulcanization accelerator, accounting for 85% of the total amount of similar products.

Accelerator T is also the super accelerator of natural rubber, diene synthetic rubber, Ⅱ, R and EPDM, with the highest utilization rate of all.
The vulcanization promoting force of accelerator T is very strong, but, without the presence of zinc oxide, it is not vulcanized at all.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is used for the manufacture of cables, wires, tires and other rubber products.

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is used as the super accelerator of natural rubber, synthetic rubber and latex.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is used as the late effect promoter of natural rubber, butadiene rubber, styrene-butadiene rubber and polyisoprene rubber.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is used for the pest control of rice, wheat, tobacco, sugar beet, grapes and other crops, as well as for the seed dressing and soil treatment.

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is suitable for the manufacture of natural rubber, synthetic rubber and latex, and can also be used as curing agent.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is the second accelerator of thiazole accelerators, which can be used with other accelerators as the continuous vulcanization accelerator.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) can be used as the super-vulcanization accelerator, and aften used with thiazole accelerator.

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) can also be used in combination with other accelerators as the continuous rubber accelerator.
For slowly decomposing out of free sulfur at more than 100 ℃, it can be used as curing agent too. Its products have excellent resistance to aging and heat, so it is applicable to natural rubber, synthetic rubber and is mainly used in the manufacture of tires, tubes, shoes, cables and other industrial products.
In agriculture, Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) can be used as fungicide and insecticide, and it can also be used as lubricant additives.

Production methods from Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD), carbon disulfide, ammonia condensation reaction was dimethyl dithiocarbamate, and then by the oxidation of hydrogen peroxide to the finished product.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is a protective fungicide applied to foliage to control Botrytis spp.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) also controls rust on ornamentals, scab and storage diseases on apple and pear and leaf curl and Monilia on stone fruit.

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is used in seed treatments alone or in combination with added insecticides or fungicides to control damping off diseases such as Pythium spp., and other diseases like Fusarium spp. of maize, cotton, cereals, legumes, vegetables and ornamentals.
Rubber components used in agriculture, such as conveyor belts and seals, may undergo vulcanization with the Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination.
This ensures that the rubber parts can withstand the harsh conditions encountered in agricultural operations.

Certain rubber components used in the oil and gas industry, such as seals and gaskets, may undergo vulcanization using accelerators like Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD).
This is to ensure that the rubber parts can withstand the demanding conditions of oil and gas applications.
In the manufacturing of vibration control products, such as mounts and isolators, the Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination may be used to enhance the properties of rubber components.

The vulcanization process improves the durability and performance of Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD).
Rubber compounds with the Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination may find applications in medical and healthcare products.
For example, rubber components in medical devices, gloves, or healthcare equipment may undergo vulcanization to ensure reliability and safety.

Rubber components used in rail transportation, such as seals and gaskets, may undergo vulcanization with accelerators like Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD).
This ensures the durability and reliability of rubber parts in the challenging conditions of rail applications.
Rubber components used in water treatment equipment, such as seals and gaskets, may benefit from the Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination during vulcanization.

This enhances the chemical resistance and durability of rubber parts in water treatment applications.
Seals and gaskets in various industrial equipment, including pumps, valves, and machinery, may undergo vulcanization using the Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination.
This enhances the sealing properties and longevity of these rubber components.

Rubber products used in the mining industry, such as conveyor belts and seals, may undergo vulcanization with accelerators like Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD).
This ensures the durability and reliability of rubber components in mining applications.
Rubber components used in the electronics industry, such as gaskets and seals for electronic devices, may undergo vulcanization using the Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination.

This contributes to the reliability and protection of electronic components.
Rubberized fabrics and components used in the textile industry may undergo vulcanization with the Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination.
This ensures the durability and performance of rubberized materials in textile applications.

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination is often used in research and development efforts within the rubber industry.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) serves as a reference or benchmark accelerator in studies aimed at developing new rubber formulations or exploring alternative accelerators.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is used as fungicide; bacteriostat; pesticide; rubber vulcanization accelerator; scabicide; seed disinfectant; animal repellent; insecticide; lube-oil additive; wood preservative; in antiseptic sprays; in the blending of lubrieant oils; used against Botrytis, rusts and downy mildews; seed dressing against "damping off' and verticillium wilt; ethanol antagonist and deterrent in mixtures of the methyl, ethyl, propyl, and butyl derivatives; antioxidant in polyolefin plastics; peptizing agent in polysulphide elastomers; in soaps and rodent repellents; nut, fruit, and mushroom disinfectant.

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is used in agriculture to prevent fungal diseases in seed and crops.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) has other applications ranging from use as a topical bactericide to animal repellent.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is used as a fungicide to prevent crop damage in the field and to prevent crops from deterioration in storage or transport.

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is also used as a seed, nut, fruit, and mushroom disinfectant from a variety of fungal diseases.
In addition, Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is used as an animal repellent to protect fruit trees and ornamentals from damage by rabbits, rodents, and deer.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) has been used in the treatment of human scabies, as a sun screen, and as a bactericide applied directly to the skin or incorporated into soap.

Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is used as a rubber accelerator and vulcanizer and as a bacteriostat for edible oils and fats.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) is also used as a rodent repellent, wood preservative, and may be used in the blending of lubricant oils.
The tetramethyl derivative, known as Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD), is a widely used fungicide.

The tetraethyl derivative, known as Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD), is commonly used to treat chronic alcoholism.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) produces an acute sensitivity to alcohol ingestion by blocking metabolism of acetaldehyde by acetaldehyde dehydrogenase, leading to a higher concentration of the aldehyde in the blood, which in turn produces symptoms of a severe hangover.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination is widely used in the production of tires.

Vulcanization accelerators play a key role in ensuring that tires have the necessary strength, elasticity, and heat resistance for safe and reliable performance on vehicles.
Various industrial rubber products, including belts, hoses, seals, gaskets, and other molded rubber components, utilize the Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination during vulcanization.
This enhances the mechanical properties of these goods, making them suitable for diverse industrial applications.

Rubber components in automobiles, such as engine mounts, seals, and gaskets, often undergo vulcanization with accelerators like Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD).
This ensures the durability and performance of these rubber parts in the challenging conditions of automotive use.

Rubber used for insulation in wires and cables can benefit from the Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) during vulcanization.
The process enhances the electrical insulation properties and mechanical strength of rubber, making it suitable for use in various electrical applications.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) may be employed in the vulcanization of rubber soles and components used in the footwear industry.

This ensures the production of durable and resilient shoe soles.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination can be used to modify the curing characteristics and improve the adhesive properties.
This is important in applications where strong and durable bonds are required.

Rubberized materials used in construction, such as seals, gaskets, and other components, may undergo vulcanization with accelerators like Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD).
This enhances the durability and performance of rubber products in construction applications.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination is employed in the formulation of specialty rubber compounds where specific curing characteristics and properties are required.

In the manufacturing of foam rubber products, such as cushions and padding, the Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) may be used as accelerators in the vulcanization process to impart the necessary properties for comfort and resilience.
Rubber components in various consumer goods, such as toys, sporting equipment, and household items, may undergo vulcanization using the Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) combination to ensure the desired properties and durability.

Safety Profile:
Poison by ingestion and intraperitoneal routes.
Questionable carcinogen with experimental tumorigenic and teratogenic data.
Other experimental reproductive effects.

Mutation data reported, Affects human pulmonary system.
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) a rmld allergen and irritant.
Acute poisoning in experimental animals produced liver, hdney, and brain damage.

Health Hazard:
Inhalation of dust may cause respiratory irritation.
Liquid irritates eyes and skin and may cause allergic eczema in sensitive individuals.
Ingestion causes nausea, vomiting, and diarrhea, all of which may be persistent; paralysis may develop.

Fire Hazard:
Special Hazards of Combustion Products: Toxic and irritating oxides of sulfur are formed.
Carbon disulfide may be formed from unburned material.

Toxicity evaluation:
Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) appears to result from its potential to disrupt cellular defense mechanisms against oxidative stress.
In cultured human skin fibroblast, Combination of Tetramethylthiuram disulfide/Tetraethylthiuram Disulfide (TM/ETD) results in an increase in oxidative markers such as lipid peroxidation and oxidation of reduced glutathione and decrease in other endogenous antioxidant.

Toxic effects of thiram have been described in humans and animal model systems ranging from liver injury, testicular toxicity, ophthalmological changes, and development of micronuclei in bone marrow.
However, the mechanisms of these effects are not characterized and inconsistent across various studies.

Synonyms:
thiram
Tetramethylthiuram disulfide
137-26-8
Thiuram
Rezifilm
TMTD
Pomarsol
Thirame
Arasan
Fernasan
Nobecutan
Thioscabin
Thirasan
Aapirol
Tersan
Tetrathiuram disulfide
Tetramethylthiuram
Falitiram
Formalsol
Hexathir
Kregasan
Mercuram
Normersan
Sadoplon
Spotrete
Tetrasipton
Thillate
Thiramad
Aatiram
Atiram
Fermide
Fernide
Hermal
Pomasol
Puralin
Thiosan
Thiotox
Thiulin
Thiulix
Heryl
Pomarsol forte
Methyl tuads
Accelerator T
Methyl Thiram
Fernasan A
Tetramethylthiuram disulphide
Nocceler TT
Arasan-M
Bis(dimethylthiocarbamoyl) disulfide
Thiram B
Arasan-SF
Cyuram DS
Ekagom TB
Hermat TMT
Tetramethylenethiuram disulfide
Accel TMT
Accelerator thiuram
Aceto TETD
Radothiram
Royal TMTD
Tetramethyl-thiram disulfid
Fernacol
Sadoplon 75
Tetramethylthiuram bisulfide
Tetrapom
Thioknock
Thirampa
Thiramum
Anles
Arasan-SF-X
Aules
Thimer
Panoram 75
Tetramethylthiouram disulfide
Tetramethylthiurane disulfide
Arasan 70
Arasan 75
Tersan 75
Thiram 75
Thiram 80
Spotrete-F
TMTDS
Arasan 70-S Red
Tetramethylthioperoxydicarbonic diamide
Methylthiuram disulfide
N,N-Tetramethylthiuram disulfide
Metiurac
Micropearls
Nomersan
Thianosan
Cunitex
Delsan
Thimar
Teramethylthiuram disulfide
Tersantetramethyldiurane sulfide
Pol-Thiuram
Arasan 42-S
Tetramethylthiurum disulfide
Disulfure de tetramethylthiourame
Tetrathiuram disulphide
Sranan-sf-X
Hy-Vic
SQ 1489
Chipco thiram 75
Bis(dimethyl-thiocarbamoyl)-disulfid
Orac TMTD
Tetramethylthioramdisulfide
Tetramethyldiurane sulphite
Thiotox (fungicide)
Disulfide, bis(dimethylthiocarbamoyl)
Bis((dimethylamino)carbonothioyl) disulfide
Fermide 850
Tetramethyl thiuramdisulfide
Tetramethylthiocarbamoyldisulphide
Thiuramyl
Thylate
Methyl thiuramdisulfide
Bis(dimethylthiocarbamyl) disulfide
Tetramethyl thiurane disulfide
Bis(dimethyl thiocarbamoyl)disulfide
Thirame [INN-French]
Thiramum [INN-Latin]
Thiuram D
Disolfuro di tetrametiltiourame
Tetramethyl thiurane disulphide
Tetramethylenethiuram disulphide
N,N'-(Dithiodicarbonothioyl)bis(N-methylmethanamine)
RCRA waste number U244
Flo Pro T Seed Protectant
Tetramethylthiuram bisulphide
Tetramethylthiuran disulphide
Tetramethylthiurum disulphide
NSC-1771
Tetramethyl thiuram disulfide
alpha,alpha'-Dithiobis(dimethylthio)formamide
Thiotex
Thiurad
Tirampa
Tiuramyl
Trametan
Tridipam
Tripomol
Tyradin
Tuads
Tutan
Vulkacit mtic
N,N,N',N'-Tetramethylthiuram disulfide
N,N-Tetramethylthiuram disulphide
Vulkacit thiuram
Thioperoxydicarbonic diamide, tetramethyl-
Thiuram M
Vulkacit TH
Tetramethylthioramdisulfide [Dutch]
Vulcafor TMT
Vulcafor TMTD
Bis((dimethylamino)carbonothioyl) disulphide
FMC 2070
Bis(dimethylthiocarbamoyl) disulphide
Tetramethyl-thiram disulfid [German]
Formamide, 1,1'-dithiobis(N,N-dimethylthio-
Zaprawa Nasienna T
[Me2NC(S)S]2
Vancida tm-95
Disulfuro di tetrametiltiourame
Arasan 42S
TUEX
Disolfuro di tetrametiltiourame [Italian]
Disulfuro di tetrametiltiourame [Italian]
DTXSID5021332
Disulfure de tetramethylthiourame [French]
NSC1771
dimethylcarbamothioylsulfanyl N,N-dimethylcarbamodithioate
Bis(dimethyl-thiocarbamoyl)-disulfid [German]
VUAgT-I-4
NSC-49512
Thioperoxydicarbonic diamide ([(H2N)C(S)]2S2), tetramethyl-
NSC-622696
[disulfanediylbis(carbonothioylnitrilo)]tetramethane
Thiuram M rubber accelerator
MLS000069752
MLS002702972
0D771IS0FH
CHEBI:9495
Thiuram disulfide, tetramethyl-
Thiuram-M
Thioperoxydicarbonic diamide (((H2N)C(S))2S2), tetramethyl-
NSC49512
CCG-35460
NSC-59637
NSC622696
TNTD
SQ-1489
NCGC00091563-01
SMR000059023
Thioperoxydicarbonic diamide ((H2N)C(S))2S2, tetramethyl-
[dithiobis(carbonothioylnitrilo)]tetramethane
.alpha.,.alpha.'-Dithiobis(dimethylthio)formamide
DTXCID401332
Caswell No. 856
Granuflo
N,N-dimethyl[(dimethylcarbamothioyl)disulfanyl]carbothioamide
Thiuramin
N,N',N'-Tetramethylthiuram disulfide
Thioperoxydicarbonic diamide (((H2N)C(S))2S2), N,N,N',N'-tetramethyl-
CAS-137-26-8
Formamide,1'-dithiobis(N,N-dimethylthio-
Bis[(dimethylamino)carbonothioyl] disulfide
Attack [Antifungal]
Thiram [ISO]
NSC59637
CCRIS 1282
HSDB 863
ENT 987
WLN: 1N1 & YUS & SSYUS & N1 & 1
NSC 1771
EINECS 205-286-2
NSC 49512
NSC 59637
RCRA waste no. U244
EPA Pesticide Chemical Code 079801
NSC 622696
BRN 1725821
tiramo
UNII-0D771IS0FH
Basultra
Betoxin
Tiradin
Accelerant T
AI3-00987
Ziram metabolite
Arasan m
Vulkazam S
Thioperoxydicarbonic diamide ([(H2N)C(S)]2S2), N,N,N',N'-tetramethyl-
Vanguard GF
Vancide TM
Akrochem TMTD
Perkacit TMTD
Vulkacit DTMT
Robac TMT
Rezifilm (TN)
Arasan 50 red
Spotrete WP 75
MFCD00008325
Vancide TM-95
Naftocit thiuram 16
Spectrum_001687
Thiram (USAN/INN)
Agrichem flowable thiram
THIRAM [HSDB]
THIRAM [IARC]
THIRAM [INCI]
THIRAM [USAN]
THIRAM [INN]
Spectrum2_001554
Spectrum3_001592
Spectrum4_000860
Spectrum5_001653
THIRAM [WHO-DD]
THIRAM [MI]
THIRAM [MART.]
bmse000928
EC 205-286-2
NCIMech_000272
cid_5455
NCIOpen2_007854
SCHEMBL21144
BSPBio_003184
KBioGR_001499
KBioSS_002167
4-04-00-00242 (Beilstein Handbook Reference)
BIDD:ER0359
DivK1c_000741
SPECTRUM1503322
SPBio_001428
CHEMBL120563
Thiram [USAN:INN:BSI:ISO]
BDBM43362
HMS502F03
KBio1_000741
KBio2_002167
KBio2_004735
KBio2_007303
KBio3_002684
KUAZQDVKQLNFPE-UHFFFAOYSA-
ENT-987
NINDS_000741
HMS1922A12
HMS2093E03
HMS2234B08
HMS3374C05
Pharmakon1600-01503322
Tetramethylthiuram disulfide, 97%
Tox21_111150
Tox21_201569
Tox21_301102
NSC758454
s2431
(dimethylamino){[(dimethylamino)thioxomethyl]disulfanyl}methane-1-thione
AKOS000120200
bis (dimethyl thiocarbamoyl) disulfide
Bis(dimethylaminothiocarbonyl)disulfide
Tox21_111150_1
bis(dimethylaminothiocarbonyl) disulfide
DB13245
KS-5354
NSC-758454
IDI1_000741
QTL1_000082
NCGC00091563-02
NCGC00091563-03
NCGC00091563-04
NCGC00091563-05
NCGC00091563-06
NCGC00091563-07
NCGC00091563-08
NCGC00091563-09
NCGC00091563-10
NCGC00091563-12
NCGC00255002-01
NCGC00259118-01
NCI60_001477
NCI60_006736
SBI-0051813.P002
Thiram, PESTANAL(R), analytical standard
B0486
CS-0012858
FT-0631799
EN300-16677
D06114
D97716
AB00052345_10
Q416572
SR-01000736911
J-006992
J-524968
SR-01000736911-2
Thiram, certified reference material, TraceCERT(R)
BRD-K29254801-001-06-3
Z56754480
F0001-0468
TETRAMETHYLTHIOPEROXYDICARBONIC ACID [(H2N)C(S)]2S2
N,N-Dimethyl[(dimethylcarbamothioyl)-disulfanyl]carbothioamide
1-(dimethylthiocarbamoyldisulfanyl)-N,N-dimethyl-methanethioamide
N,N-dimethylcarbamodithioic acid (dimethylthiocarbamoylthio) ester
InChI=1/C6H12N2S4/c1-7(2)5(9)11-12-6(10)8(3)4/h1-4H3
N(1),N(1),N(3),N(3)-tetramethyl-2-dithioperoxy-1,3-dithiodicarbonic diamide
N,N-dimethylcarbamodithioic acid [[dimethylamino(sulfanylidene)methyl]thio] ester
TETRAMETHYLTHIOPEROXYDICARBONIC DIAMIDE ((((CH(SUB 3))(SUB 2)N)C(S))(SUB 2)S(SUB 2))

Concentrated sulfuric acid is an inorganic acid composed of the elements chromium, oxygen, and hydrogen.
Concentrated sulfuric acid is a dark, purplish red, odorless, sand-like solid powder.
When dissolved in water, Concentrated sulfuric acid is a strong acid.

CAS Number: 7738-94-5
EC Number: 231-801-5
Chemical Formula: H2CrO4
Molecular Weight: 118.010 g/mol

Synonyms: CHROMIC ACID, Chromic(VI) acid, 7738-94-5, dihydroxy(dioxo)chromium, Acide chromique, Caswell No. 221, Chromic acid (H2CrO4), tetraoxochromic acid, CCRIS 8994, HSDB 6769, UNII-SA8VOV0V7Q, SA8VOV0V7Q, EINECS 231-801-5, EPA Pesticide Chemical Code 021101, AI3-51760, dihydroxidodioxidochromium, dihydrogen(tetraaoxidochromate), DTXSID8034455, CHEBI:33143, J34.508C, CHROMIUM HYDROXIDE OXIDE (CR(OH)2O2), (CrO2(OH)2), [CrO2(OH)2], Acide chromique [French], Chromium hydrogen oxide, Pesticide Code: 021101, DTXCID6014455, KRVSOGSZCMJSLX-UHFFFAOYSA-L, AMY22327, AKOS025243247, Q422642, Chromic acid [Wiki], 231-801-5 [EINECS], 7738-94-5 [RN], chromic acid (H2CrO4), Chromium, dihydroxydioxo- [ACD/Index Name], Dihydroxy(dioxo)chrom [German] [ACD/IUPAC Name], Dihydroxy(dioxo)chrome [French] [ACD/IUPAC Name], Dihydroxy(dioxo)chromium [ACD/IUPAC Name], SA8VOV0V7Q, [CrO2(OH)2], 11115-74-5 [RN], 1333-82-0 [RN], 13530-68-2 [RN], 13765-19-0 [RN], 199384-58-2 [RN], 237391-94-5 [RN], 24934-60-9 [RN], 9044-10-4 [RN], Acide chromique [French], chromate [Wiki], Chromatite syn, CHROMIC ACID|DIOXOCHROMIUMDIOL, CHROMIC ANHYDRIDE, chromic(VI) acid, Chromium hydroxide oxide, Chromium trioxide [Wiki], dihydrogen(tetraaoxidochromate), dihydrogen(tetraaoxidochromate); dihydroxidodioxidochromium, dihydroxidodioxidochromium, dihydroxy-dioxochromium, dihydroxy-dioxo-chromium, Gelbin, H2CrO4, SOLID CHROMIC ACID, tetraoxochromic acid, UNII:SA8VOV0V7Q, UNII-SA8VOV0V7Q, Yellow ultramarine, 铬酸 [Chinese],

Concentrated sulfuric acid is a very weak acid and Concentrated sulfuric acid salts can be dissociated event by acetic acid.
Concentrated sulfuric acid has a strong oxidising action and is itself reduced to CrO3; because of this, Concentrated sulfuric acid should never be used in combination with alcohol or formalin.

Concentrated sulfuric acid is an inorganic acid composed of the elements chromium, oxygen, and hydrogen.
Concentrated sulfuric acid is a dark, purplish red, odorless, sand-like solid powder.
When dissolved in water, Concentrated sulfuric acid is a strong acid.

There are 2 types of Concentrated sulfuric acid: molecular Concentrated sulfuric acid with the formula H2CrO4 and diConcentrated sulfuric acid with the formula H2Cr2O7.

The term Concentrated sulfuric acid is usually used for a mixture made by adding Chromic acid to a dichromate, which may contain a variety of compounds, including solid chromium trioxide.
This kind of Concentrated sulfuric acid may be used as a cleaning mixture for glass.

Concentrated sulfuric acid may also refer to the molecular species, H2CrO4 of which the trioxide is the anhydride.
Concentrated sulfuric acid features chromium in an oxidation state of +6 (or VI).
Concentrated sulfuric acid is a strong and corrosive oxidising agent and a moderate carcinogen.

Concentrated sulfuric acid is formed when chromium trioxide reacts with water.
Chromium trioxide is crystalline, light red or brown in color and is deliquescent and fully soluble in water.

In a number of fixing fluids, however, Concentrated sulfuric acid is used together with formalin–the reducing action being slow, the fixation is completed before the acid is fully reduced.
Concentrated sulfuric acid is a strong precipitant of protein but Berg (1927) found Concentrated sulfuric acid to be a very weak precipitant of nuclein.

The dissociation of Concentrated sulfuric acid in water may result in H+ and HCrO4− or 2H+ and CrO4− ions.
According to Berg (1927), protein undergoes denaturation and precipitation by the primary action of Concentrated sulfuric acid, and the secondary action results in hardening.

He holds that the ion HCrO4− is responsible for the secondary action.
Chemical reaction probably occurs between protein and Concentrated sulfuric acid, but the exact steps are not precisely known.

However, the principal affinity of chromium is for the carboxyl and hydroxyl groups.
Green (1953) suggested that coordinates with –OH and –NH2 are formed after reaction with carboxyl groups.

Proteins, acted upon by Concentrated sulfuric acid, are resistant to the action of pepsin and trypsin.
Concentrated sulfuric acid penetrates the tissues slowly and the hardening induced by this acid makes the tissue resistant to hardening by ethanol in subsequent processing.
Concentrated sulfuric acid does not cause excessive shrinkage of the tissue.

Materials fixed in this acid require thorough washing in water, at least overnight, otherwise the deposition of chromic crystals not only hinders staining but also hampers the observation of chromosomes.
Because of Concentrated sulfuric acid slight hardening action Concentrated sulfuric acid is difficult to use this fluid as a fixative for squash preparations, unless softened by some strong acid, which may hamper staining.

Concentrated sulfuric acid should never be used alone, as then heavy precipitates are formed causing shrinkage of nucleus and cytoplasm.
Materials treated in Concentrated sulfuric acid should not be kept in strong sunlight due to the chance of breakdown of proteins.
Basic dyes adhere closely to tissue fixed in Concentrated sulfuric acid.

In general, Concentrated sulfuric acid is considered an essential ingredient of several fixing mixtures.
Concentrated sulfuric acid imparts a better consistency to the tissue and aids staining better than osmium tetroxide.

Synonymous with Chromic acid, the term Concentrated sulfuric acid refers to a mixture formed by adding Chromic acid to a dichromate solution that contains a variety of compounds, including solid chromium trioxide.
Concentrated sulfuric acid is possible to use this type of Concentrated sulfuric acid to clean glass with a cleaning solution.

Concentrated sulfuric acid is an inorganic compound with the chemical formula H2CrO4 and is a compound compound.
Tetraoxo Concentrated sulfuric acid, also known as Chromic(VI) acid, is another name for Concentrated sulfuric acid.

This article discusses the structure, preparation, properties, and various applications of Concentrated sulfuric acid.
Concentrated sulfuric acid has a +6 (or VI) chromium oxidation state, which is also known as the hexavalent chromium oxidation state.

Chromium can exist in a number of different oxidation states, with +6 being the most extreme.
Concentrated sulfuric acid is used to oxidise a wide range of organic compounds, the most common of which are alcohols.

Concentrated sulfuric acid is a powerful oxidising agent that is effective against a wide range of organic compounds.
Using Concentrated sulfuric acid as an oxidant, there are two basic principles that can be applied to any alcohol.

The oxidation of any alcohol containing approximately one alpha hydrogen occurs in the presence of Concentrated sulfuric acid, which means that tertiary alcohols do not undergo oxidation in the presence of the acid.
The oxidation of any organic product formed, whose molecule contains at least one hydrogen atom bound to the carbonyl carbon, is further enhanced by Concentrated sulfuric acid.

Concentrated sulfuric acid is also called TetraoxoConcentrated sulfuric acid or Chromic(VI) acid.
Concentrated sulfuric acid is usually a mixture made by adding concentrated sulphuric acid (H2SO4) to a dichromate which consists of a variety of compounds and solid chromium trioxide.

The term Concentrated sulfuric acid is generally used for a mixture made by the addition of Chromic acid in a dichromate that may contain various compounds, including solid chromium trioxide.
This type of Concentrated sulfuric acid can be used as a cleaning mixture for glass.

Concentrated sulfuric acid can also be related to a molecular species, H2CrO4, which is the trioxide anhydride.
Concentrated sulfuric acid contains chromium in the +6 (or VI) oxidation state.
Concentrated sulfuric acid is a strong and corrosive oxidizing agent.

The anhydride of Concentrated sulfuric acid is chromium trioxide (CrO3).
Therefore, when Concentrated sulfuric acid is mentioned, CrO3 comes to mind.

Here chromium has (6+) valency.
Concentrated sulfuric acid is an unstable compound and turns into di(bi) chromatic acid (H2Cr2O7) by reacting with itself.

Concentrated sulfuric acid anhydride (CrO3) is a red-pink crystal and Concentrated sulfuric acid specific gravity is between 2.67 and 2.82 g/cm3.
Concentrated sulfuric acid melts at 197°C and slowly decomposes after melting.

Concentrated sulfuric acid draws moisture from the air.
Concentrated sulfuric acid is very soluble in water and organic solvents such as acetic acid, pyridine and ether.

Crude CrO3 is separated by precipitation from a mixture of saturated sulfate acid and saturated sodium bichromate.
This precipitate is purified by crystallization or melting.

Concentrated sulfuric acid is a strong acid and is also a strong oxidizing agent.
Concentrated sulfuric acid is highly destructive to plant and animal cells.
If Concentrated sulfuric acid is brought into contact with an organic compound or by reduction, a serious explosion may occur.

Concentrated sulfuric acid is a chromium oxoacid.
Concentrated sulfuric acid has a role as an oxidising agent.
Concentrated sulfuric acid is a conjugate acid of a hydrogenchromate.

Concentrated sulfuric acid generally refers to a collection of compounds generated by the acidification of solutions containing chromate and dichromate anions or the dissolving of chromium trioxide in sulfuric acid.
Concentrated sulfuric acid contains hexavalent chromium.

Hexavalent chromium refers to chromium in the +6 oxidation state, and is more toxic than other oxidation states of the chromium atom because of Concentrated sulfuric acid greater ability to enter cells and a higher redox potential.
Molecular Concentrated sulfuric acid, H2CrO4, has much in common with sulfuric acid, H2SO4 as both are classified as strong acids.

Concentrated sulfuric acid was widely used in the instrument repair industry, due to Concentrated sulfuric acid ability to "brighten" raw brass.
A Concentrated sulfuric acid dip leaves behind a bright yellow patina on the brass.

Due to growing health and environmental concerns, many have discontinued use of this chemical in their repair shops.
Most Concentrated sulfuric acid sold or available as a 10% aqueous solution.

Also known as Tetraoxochromic or Chromic (VI) acid, Concentrated sulfuric acid is a dark red purplish solid with Concentrated sulfuric acid solution being corrosive to tissue and metals.
Concentrated sulfuric acid is a naturally occurring oxide but can also be made by adding concentrated sulphuric acid to a dichromate which may contain a mixture of compounds such as the solid chromium trioxide.

Concentrated sulfuric acid usually refers to a collection of compounds formed via the dissolution of Chromium Trioxide in Sulfuric Acid, or via the acidification of Chromate/Dichromate solutions.
Concentrated sulfuric acid is a dark red, strongly corrosive liquid.

Since Concentrated sulfuric acid contains chromium in Concentrated sulfuric acid +6 oxidation state, Concentrated sulfuric acid has strong oxidizing properties and a high redox potential.
Hence, Concentrated sulfuric acid has been used as a cleaning reagent for lab glassware, textiles, and metals, and an oxidizing agent in organic chemistry reactions.

For a time, Concentrated sulfuric acid was commonly used in musical instrument repair to brighten brass, and as a bleach in photograph development.
The properties that lend this compound to these applications also increase Concentrated sulfuric acid toxicity due to Concentrated sulfuric acid increased ability to enter cells, so some industries have phased in out in favor of alternatives.
Concentrated sulfuric acid is generally available in relatively dilute solutions.

Concentrated sulfuric acid solution is a type of acid that consists of a mixture of Chromic acid with dichromate and can contain many different compounds such as solid chromium trioxide.
Concentrated sulfuric acid is a very good cleaner for windows.

Concentrated sulfuric acid can also refer to the molecular species H2CrO4 where the trioxide is anhydride.

Concentrated sulfuric acid contains chromium in the +6-valent oxidation state, which is a strong and corrosive oxidizing agent.
Since Concentrated sulfuric acid is not a stable compound, Concentrated sulfuric acid reacts with itself and turns into dichromatic acid.

Concentrated sulfuric acid has a melting point of 197 degrees and due to Concentrated sulfuric acid chemical properties, Concentrated sulfuric acid absorbs moisture from the air and decomposes slowly when Concentrated sulfuric acid melts.
Concentrated sulfuric acid is very soluble in organic solvents such as Concentrated sulfuric acid, pyridine, ether, acetic acid and water.

Concentrated sulfuric acid is a strong acid solution that can also be used for oxidation.
Concentrated sulfuric acid can be corrosive and harmful to living species such as animals and plants.
There is a possibility of creating a massive explosion if Concentrated sulfuric acid comes into contact with an organic compound or through reduction.

Concentrated sulfuric acid should be stored in a dry and cool environment.
Concentrated sulfuric acid should be protected from heat and direct sunlight.

Concentrated sulfuric acid generally refers to a collection of compounds generated by the acidification of solutions containing chromate and dichromate anions or the dissolving of chromium trioxide in sulfuric acid.
Concentrated sulfuric acid contains hexavalent chromium.

Hexavalent chromium refers to chromium in the +6 oxidation state, and is more toxic than other oxidation states of the chromium atom because of Concentrated sulfuric acid greater ability to enter cells and a higher redox potential.
Molecular Concentrated sulfuric acid, H2CrO4, has much in common with sulfuric acid, H2SO4 as both are classified as strong acids.

Concentrated sulfuric acid was widely used in the instrument repair industry, due to Concentrated sulfuric acid ability to "brighten" raw brass.
A Concentrated sulfuric acid dip leaves behind a bright yellow patina on the brass.

Due to growing health and environmental concerns, many have discontinued use of this chemical in their repair shops.
Most Concentrated sulfuric acid sold or available as a 10% aqueous solution.

DiConcentrated sulfuric acid:
DiConcentrated sulfuric acid, H2Cr2O7 is the fully protonated form of the dichromate ion and also can be seen as Concentrated sulfuric acid of adding chromium trioxide to molecular Concentrated sulfuric acid.
DiConcentrated sulfuric acid will behave the same exact way when reacting with a primary or secondary alcohol.
The caveat to this statement is that a secondary alcohol will be oxidized no further than a ketone, whereas a primary alcohol will be oxidized to a aldehyde for the first step of the mechanism and then oxidized again to a carboxylic acid, contingent on no significant steric hindrance impeding this reaction.

DiConcentrated sulfuric acid undergoes the following reaction:
[Cr2O7]2− + 2H+ ⇌ H2Cr2O7 ⇌ H2CrO4 + CrO3

Concentrated sulfuric acid is probably present in Concentrated sulfuric acid cleaning mixtures along with the mixed chromosulfuric acid H2CrSO7.

Molecular Concentrated sulfuric acid:
Molecular Concentrated sulfuric acid, H2CrO4, has much in common with sulfuric acid, H2SO4.
Only sulfuric acid can be classified as part of the 7 strong acids list.

Due to the laws pertinent to the concept of "first order ionization energy", the first proton is lost most easily.
Concentrated sulfuric acid behaves extremely similarly to sulfuric acid deprotonation.
Since the process of polyvalent acid-base titrations have more than one proton (especially when the acid is starting substance and the base is the titrant), protons can only leave an acid one at a time.

Hence the first step is as follows:
H2CrO4 ⇌ [HCrO4]− + H+

The pKa for the equilibrium is not well characterized.
Reported values vary between about −0.8 to 1.6.
The value at zero ionic strength is difficult to determine because half dissociation only occurs in very acidic solution, at about pH 0, that is, with an acid concentration of about 1 mol dm−3.

A further complication is that the ion [HCrO4]− has a marked tendency to dimerize, with the loss of a water molecule, to form the dichromate ion, [Cr2O7]2−:
2 [HCrO4]− ⇌ [Cr2O7]2− + H2O log KD = 2.05.

Furthermore, the dichromate can be protonated:
[HCr2O7]− ⇌ [Cr2O7]2− + H+ pK = 1.8

The pK value for this reaction shows that Concentrated sulfuric acid can be ignored at pH > 4.

Loss of the second proton occurs in the pH range 4–8, making the ion [HCrO4]− a weak acid.

Molecular Concentrated sulfuric acid could in principle be made by adding chromium trioxide to water (cf. manufacture of sulfuric acid).

CrO3 + H2O ⇌ H2CrO4

But in practice the reverse reaction occurs when molecular Concentrated sulfuric acid is dehydrated.


This is what happens when concentrated sulfuric acid is added to a dichromate solution.

At first the colour changes from orange (dichromate) to red (Concentrated sulfuric acid) and then deep red crystals of chromium trioxide precipitate from the mixture, without further colour change.
The colours are due to LMCT transitions.

Chromium trioxide is the anhydride of molecular Concentrated sulfuric acid.
Concentrated sulfuric acid is a Lewis acid and can react with a Lewis base, such as pyridine in a non-aqueous medium such as dichloromethane (Collins reagent).

Concentrated sulfuric acid is a strong oxidizing agent.
Concentrated sulfuric acid is formed when chromium trioxide reacts with water.

Concentrated sulfuric acid chemical formula is H2CrO4.
Concentrated sulfuric acid is used to oxidize many classes of organic compounds.

Concentrated sulfuric acid is an intermediate in chromium plating.
Concentrated sulfuric acid generally refers to a collection of compounds generated by the acidification of solutions containing chromate and dichromate anions.

Concentrated sulfuric acid forms dark purplish red crystals.
Concentrated sulfuric acid and Concentrated sulfuric acid salts are used in electroplating.

Applications of Concentrated sulfuric acid:
In chemistry trade, Concentrated sulfuric acid is used in chromate, which is salt of Concentrated sulfuric acid, production.
A large portion of Concentrated sulfuric acid’s production is used for chrome coating.

Concentrated sulfuric acid is used as burner in medical fields due to Concentrated sulfuric acid being a good oxidizing agent.
Concentrated sulfuric acid is also efficient in cleaning organic filth from glasses in labs but this method is not preferred because of Concentrated sulfuric acid harm to environment.

Concentrated sulfuric acid is also used as rubber pigment in carving processes, salt glaze making, colorizing glasses, cleaning metals, ink and dye productions.
Concentrated sulfuric acid is acquired from adding additive chemicals to chrome trioxide’s aquenous solution.
Chrome trioxde is generally produced by putting 2,4 mol sodium dichromate and 2,8 mol sulphuric acid.

Concentrated sulfuric acid is an intermediate in chromium plating and is also used in ceramic glazes, and colored glass.
Concentrated sulfuric acid can be used to clean laboratory glass ware, particularly of otherwise insoluble organic residues

Concentrated sulfuric acid has also been widely used in the band instrument repair industry, due to Concentrated sulfuric acid ability to “brighten” raw brass.
Concentrated sulfuric acid is used as wood preservative

Concentrated sulfuric acid is a strong oxidizing agent finding application in organic synthesis.
Concentrated sulfuric acid is used for preparation of other chrome chemicals of analytical grades.

Concentrated sulfuric acid is used in chemicals (chromates, oxidizing agents, catalysts), chrome plating, intermediates, pharmaceuticals (caustic), process engraving, anodizing, ceramic glazes, colored glass, metal cleaning, inks, tanning, dyes, textile mordant and plastics.
Concentrated sulfuric acid is used in coating agents, surface treatment agents and surfactants.

Uses of Concentrated sulfuric acid:
Concentrated sulfuric acid is an intermediate in chromium plating, and is also used in ceramic glazes, and colored glass.
Because a solution of Concentrated sulfuric acid in sulfuric acid (also known as a sulfochromic mixture or chromosulfuric acid) is a powerful oxidizing agent, Concentrated sulfuric acid can be used to clean laboratory glassware, particularly of otherwise insoluble organic residues.

This application has declined due to environmental concerns.
Furthermore, the acid leaves trace amounts of paramagnetic chromic ions (Cr3+) that can interfere with certain applications, such as NMR spectroscopy.

This is especially the case for NMR tubes.
Piranha solution can be used for the same task, without leaving metallic residues behind.

Concentrated sulfuric acid was widely used in the musical instrument repair industry, due to Concentrated sulfuric acid ability to "brighten" raw brass.
A Concentrated sulfuric acid dip leaves behind a bright yellow patina on the brass.
Due to growing health and environmental concerns, many have discontinued use of this chemical in their repair shops.

Concentrated sulfuric acid was used in hair dye in the 1940s, under the name Melereon.

Concentrated sulfuric acid is used as a bleach in black and white photographic reversal processing.

Concentrated sulfuric acid is used in electroplating, metal cleaning, leather tanning, and photography.
Concentrated sulfuric acid is an intermediate in chromium plating, and is also used in ceramic glazes, and colored glass.

Concentrated sulfuric acid is used in ceramic glazes.
Concentrated sulfuric acid is used as a photographic chemical.

Concentrated sulfuric acid is used as an oxidizing agent.
Concentrated sulfuric acid is used as a cleaner in the laboratory.

Concentrated sulfuric acid is used in the metal finishing industry.
Concentrated sulfuric acid is used in the leather tanning, electroplating, and anticorrosive metal treatment industries.

Concentrated sulfuric acid acts as an intermediate in chromium plating.
Concentrated sulfuric acid is used in ceramic glazes and coloured glass.

Chromosulfuric acid or sulfochromic mixture is a strong oxidizing agent that is used to clean laboratory glassware.
Concentrated sulfuric acid has the ability to brighten raw brass and therefore Concentrated sulfuric acid is used in the instrument repair industry.
In the year 1940, Concentrated sulfuric acid was used in hair dye.

The completely protonated form of the dichromate ion is diConcentrated sulfuric acid, H2Cr2O7 and can also be seen as the result of adding chromium trioxide to molecular Concentrated sulfuric acid.
When reacting with an aldehyde or ketone, diConcentrated sulfuric acid exactly the same way.

In organic chemistry, the Concentrated sulfuric acid solution can oxidize primary alcohols to aldehyde and secondary alcohol to a ketone.
But the tertiary alcohols and ketones are unaffected.
During oxidation, the colour of Concentrated sulfuric acid changes from orange to brownish green.

Concentrated sulfuric acid is capable of oxidising many forms of organic compounds, and many variants have been created for this reagent.
Concentrated sulfuric acid is referred to as the Jones reagent in aqueous sulfuric acid and acetone, which oxidises primary and secondary alcohols into carboxylic acids and ketones, respectively, though rarely affecting unsaturated bonds.

Cromyl chloride which is used to test the presence of chloride ions in inorganic chemistry, is derived from Concentrated sulfuric acid.
Chromium trioxide and pyridinium chloride produce pyridinium chlorochromate.

Concentrated sulfuric acid converts to the corresponding aldehydes (R-CHO) primary alcohols.
Concentrated sulfuric acid was used to repair musical instruments due to Concentrated sulfuric acid ability to “brighten” raw brass.

Concentrated sulfuric acid is used in to manufacture metal and plastic coatings to produce a strong, tarnish-resistant, chrome finish.
Concentrated sulfuric acid finds applications in many industries including in the manufacture of appliances and automobiles.

Concentrated sulfuric acid is also used as a wood preservative for marine pilings, telephone poles, landscape timbers and other industrial wood applications.
Being a strong oxidizing agent, Concentrated sulfuric acid also finds applications in organic synthesis and for preparation of other chrome chemicals of analytical grades.

Usage areas:
Concentrated sulfuric acid is used in the chemical industry to manufacture chromates, which are salts of Concentrated sulfuric acid.
Most Concentrated sulfuric acid is produced for use in chrome plating.

Concentrated sulfuric acid is used as a caustic in medicine,
Concentrated sulfuric acid is used in carving processes,

Concentrated sulfuric acid is used in making ceramic glaze,
Concentrated sulfuric acid is used in tinting windows,

Concentrated sulfuric acid is used in cleaning metals,
Concentrated sulfuric acid is used in ink and paint manufacturing
Concentrated sulfuric acid is used as rubber pigment.

In the chemical industry, Concentrated sulfuric acid is used for the manufacture of chromates, the salt form of Concentrated sulfuric acid.
The area where Concentrated sulfuric acid is used most in the market is the chrome plating process.

Concentrated sulfuric acid is used as a caustic agent in the medical industry.
Concentrated sulfuric acid is used during the glazing process during the production stages of handicrafts such as carving and ceramics.

Concentrated sulfuric acid is used in the coloring phase of the glass production process.
Concentrated sulfuric acid is used in the cleaning of metals.

Concentrated sulfuric acid is used in paint and ink production.
Concentrated sulfuric acid is used as a pigment in the production of rubber material.

Industrial Processes with risk of exposure:
Acid and Alkali Cleaning of Metals
Electroplating
Leather Tanning and Processing
Photographic Processing
Textiles (Printing, Dyeing, or Finishing)

Activities with risk of exposure:
Textile arts

General Properties of Concentrated sulfuric acid:
Concentrated sulfuric acid generally refers to a mixture produced by adding concentrated sulphuric acid to a dichromate.
Dichromate may contain several other compounds such as solid chromium trioxide.

Concentrated sulfuric acid is a very good chemical for glass cleaning.
Anhydrous form of trioxide(H2CrO4) can also be called Concentrated sulfuric acid.

Concentrated sulfuric acid is a strong and abrasive oxidizing agent.
Chemically, Concentrated sulfuric acid bear may remeblance to sulphuric acid and acts simlarly when yielding hydrogen.
Only sulphuric acid yields first proton much easier than Concentrated sulfuric acid.

Additionally, Concentrated sulfuric acid slowly disintigrates while reaching boiling point and, in proper environments, Concentrated sulfuric acid becomes dessicant.

Formula of Concentrated sulfuric acid:
Hydrogen is a chemical element with the symbol H and Concentrated sulfuric acid atomic number is 1 and Concentrated sulfuric acid electron configuration is 1s.
Concentrated sulfuric acid is the lightest element.

Concentrated sulfuric acid is colorless, odorless, tasteless, non-toxic, and highly combustible.
Concentrated sulfuric acid is an extremely flammable gas, Concentrated sulfuric acid burns in the air and oxygen to produce water.

Concentrated sulfuric acid is used in the synthesis of Ammonia and the manufacturing of Nitrogenous fertilizers.
Concentrated sulfuric acid is used as rocket fuel and is used in the production of hydrochloric acid.

Chromium is a chemical element with the symbol Cr.
Concentrated sulfuric acid atomic number is 24 and Concentrated sulfuric acid electronic configuration is [Ar]3d5 4s.

Concentrated sulfuric acid is a steely gray, lustrous, hard, and brittle transition metal.
Concentrated sulfuric acid is not found as a free element in nature but is found in the form of ores.
The main ore of chromium is Chromite.

Oxygen is a chemical element with the symbol O and the atomic number is 8.
Concentrated sulfuric acid is a colorless, odorless, tasteless gas essential to living organisms.

Concentrated sulfuric acid is a reactive element that is found in water, in most rocks and minerals, and in numerous organic compounds.
Concentrated sulfuric acid is the most abundant element in the earth’s crust.
Concentrated sulfuric acid is life-supporting gas and highly combustible.

Structure of Concentrated sulfuric acid:
Concentrated sulfuric acid is a strong oxidizing agent.
Concentrated sulfuric acid is an acid so Concentrated sulfuric acid begins with H.

Next, we look at the name there is no prefix in front of the Concentrated sulfuric acid.
Acids all contain hydrogen.

In this structure hydrogen bonded with chromate.
The structure of Concentrated sulfuric acid starts with four oxygen atoms bonded to chromium.

Two of them have double bonds, and two have single bonds.
They singly bonded oxygen atoms each have a hydrogen bonded to them.

Reactions of Concentrated sulfuric acid:
Concentrated sulfuric acid is capable of oxidizing many kinds of organic compounds and many variations on this reagent have been developed:
Concentrated sulfuric acid in aqueous sulfuric acid and acetone is known as the Jones reagent, which will oxidize primary and secondary alcohols to carboxylic acids and ketones respectively, while rarely affecting unsaturated bonds.

Pyridinium chlorochromate is generated from chromium trioxide and pyridinium chloride.
This reagent converts primary alcohols to the corresponding aldehydes (R–CHO).

Collins reagent is an adduct of chromium trioxide and pyridine used for diverse oxidations.

Chromyl chloride, CrO2Cl2 is a well-defined molecular compound that is generated from Concentrated sulfuric acid.

Illustrative transformations:
Oxidation of methylbenzenes to benzoic acids.
Oxidative scission of indene to homophthalic acid.
Oxidation of secondary alcohol to ketone (cyclooctanone) and nortricyclanone.

Use in qualitative organic analysis:
In organic chemistry, dilute solutions of Concentrated sulfuric acid can be used to oxidize primary or secondary alcohols to the corresponding aldehydes and ketones.
Similarly, Concentrated sulfuric acid can also be used to oxidize an aldehyde to Concentrated sulfuric acid corresponding carboxylic acid.

Tertiary alcohols and ketones are unaffected.
Because the oxidation is signaled by a color change from orange to brownish green (indicating chromium being reduced from oxidation state +6 to +3), Concentrated sulfuric acid is commonly used as a lab reagent in high school or undergraduate college chemistry as a qualitative analytical test for the presence of primary or secondary alcohols, or aldehydes.[9]

Alternative reagents:
In oxidations of alcohols or aldehydes into carboxylic acids, Concentrated sulfuric acid is one of several reagents, including several that are catalytic.
For example, nickel(II) salts catalyze oxidations by bleach (hypochlorite).

Aldehydes are relatively easily oxidised to carboxylic acids, and mild oxidising agents are sufficient.
Silver(I) compounds have been used for this purpose.

Each oxidant offers advantages and disadvantages.
Instead of using chemical oxidants, electrochemical oxidation is often possible.

Handling and Storage of Concentrated sulfuric acid:
Store containers upright & tightly closed in a dry and well-ventilated place.
Containers holding Concentrated sulfuric acid and dichromates need to be stored below eye level.

Each container’s label should include a skull-and-crossbones pictogram, the word “Danger”, and identify Concentrated sulfuric acid as both acutely toxic and carcinogenic.
Containers of Concentrated sulfuric acid and dichromate salts must be stored in leak-proof secondary containment within a Designated Area.
The secondary container’s label should include a skull-and-crossbones pictogram, the word “Danger”, and identify Concentrated sulfuric acid as both acutely toxic and carcinogenic.

Incompatibles: acids, bases, powdered metals, hydrazine, phosphorous, and all organic chemicals.

Storage Conditions:
Storage site should be as close as practical to lab in which carcinogens are to be used, so that only small quantities required for expt need to be carried.
Carcinogens should be kept in only one section of cupboard, an explosion-proof refrigerator or freezer (depending on chemicophysical properties) that bears appropriate label.

An inventory should be kept, showing quantity of carcinogen & date Concentrated sulfuric acid was acquired.
Facilities for dispensing should be contiguous to storage area.

Reactivity Profile of Concentrated sulfuric acid:
Concentrated sulfuric acid reacts rapidly with many materials including common combustibles, often causing ignition.
Mixing with reducing reagents can cause explosions.

Dangerously reactive with acetone, alcohols, alkali metals (sodium, potassium), ammonia, arsenic, dimethylformamide, hydrogen sulfide, phosphorus, peroxyformic acid, pyridine, selenium, sulfur, and many other chemicals.
Often mixed with sulfuric acid and used to clean glass ("cleaning solution").
Closed containers for used cleaning solution may explode from the internal pressure of carbon dioxide generated by oxidation of carbon compounds removed from the glass.

Safety of Concentrated sulfuric acid:
Hexavalent chromium compounds (including chromium trioxide, Concentrated sulfuric acids, chromates, chlorochromates) are toxic and carcinogenic.
For this reason, Concentrated sulfuric acid oxidation is not used on an industrial scale except in the aerospace industry.

Chromium trioxide and Concentrated sulfuric acids are strong oxidisers and may react violently if mixed with easily oxidisable organic substances.
Fires or explosions may result.

Concentrated sulfuric acid burns are treated with a dilute sodium thiosulfate solution.

First Aid Measures of Concentrated sulfuric acid:
Call 911 or emergency medical service.
Ensure that medical personnel are aware of Concentrated sulfuric acid(s) involved and take precautions to protect themselves.

Move victim to fresh air if Concentrated sulfuric acid can be done safely.
Give artificial respiration if victim is not breathing.

Do not perform mouth-to-mouth resuscitation if victim ingested or inhaled Concentrated sulfuric acid; wash face and mouth before giving artificial respiration.
Use a pocket mask equipped with a one-way valve or other proper respiratory medical device.

Administer oxygen if breathing is difficult.
Remove and isolate contaminated clothing and shoes.

In case of contact with substance, immediately flush skin or eyes with running water for at least 20 minutes.
For minor skin contact, avoid spreading material on unaffected skin.

Keep victim calm and warm.
Effects of exposure (inhalation, ingestion or skin contact) to substance may be delayed.

Skin Contact:
Immediately remove contaminated clothing and accessories; flush the skin with water for at least 15 minutes.
Seek medical attention immediately.

Eye Contact:
Check for and remove contact lenses.
Immediately flush eyes with water for at least 15 minutes.
Seek medical attention immediately.

Inhalation:
Move affected individual(s) into fresh air.
Seek medical attention immediately.

Ingestion:
Do not induce vomiting or give anything by mouth to an unconscious person.
Rinse mouth with water.
Seek medical attention.

Isolation and Evacuation:

IMMEDIATE PRECAUTIONARY MEASURE:
Isolate spill or leak area in all directions for at least 50 meters (150 feet) for liquids and at least 25 meters (75 feet) for solids.

SPILL:
Increase the immediate precautionary measure distance, in the downwind direction, as necessary.

FIRE:
If tank, rail car or tank truck is involved in a fire, ISOLATE for 800 meters (1/2 mile) in all directions; also, consider initial evacuation for 800 meters (1/2 mile) in all directions. (ERG, 2020)

Firefighting Measures of Concentrated sulfuric acid:

SMALL FIRE:
Dry chemical, CO2 or water spray.

LARGE FIRE:
Dry chemical, CO2, alcohol-resistant foam or water spray.
If Concentrated sulfuric acid can be done safely, move undamaged containers away from the area around the fire.
Dike runoff from fire control for later disposal.

FIRE INVOLVING TANKS OR CAR/TRAILER LOADS:
Fight fire from maximum distance or use unmanned master stream devices or monitor nozzles.
Do not get water inside containers.

Cool containers with flooding quantities of water until well after fire is out.
Withdraw immediately in case of rising sound from venting safety devices or discoloration of tank.
ALWAYS stay away from tanks engulfed in fire.

Non-Fire Response:
ELIMINATE all ignition sources (no smoking, flares, sparks or flames) from immediate area.
Do not touch damaged containers or spilled material unless wearing appropriate protective clothing.

Stop leak if you can do Concentrated sulfuric acid without risk.
Prevent entry into waterways, sewers, basements or confined areas.

Absorb or cover with dry earth, sand or other non-combustible material and transfer to containers.
DO NOT GET WATER INSIDE CONTAINERS.

Protective Clothing:
Wear positive pressure self-contained breathing apparatus (SCBA).
Wear chemical protective clothing that is specifically recommended by the manufacturer when there is NO RISK OF FIRE.
Structural firefighters' protective clothing provides thermal protection but only limited chemical protection.

Disposal Methods of Concentrated sulfuric acid:
Generators of waste (equal to or greater than 100 kg/mo) containing this contaminant, EPA hazardous waste number D007, must conform with USEPA regulations in storage, transportation, treatment and disposal of waste.

The following wastewater treatment technologies have been investigated for Concentrated sulfuric acid:
Concentration process: Reverse Osmosis.

SRP: Wastewater from contaminant suppression, cleaning of protective clothing/equipment, or contaminated sites should be contained and evaluated for subject chemical or decomposition product concentrations.
Concentrations shall be lower than applicable environmental discharge or disposal criteria.

Alternatively, pretreatment and/or discharge to a permitted wastewater treatment facility is acceptable only after review by the governing authority and assurance that "pass through" violations will not occur.
Due consideration shall be given to remediation worker exposure (inhalation, dermal and ingestion) as well as fate during treatment, transfer and disposal.
If Concentrated sulfuric acid is not practicable to manage the chemical in this fashion, Concentrated sulfuric acid must be evaluated in accordance with EPA 40 CFR Part 261, specifically Subpart B, in order to determine the appropriate local, state and federal requirements for disposal.

PRECAUTIONS FOR "CARCINOGENS": There is no universal method of disposal that has been proved satisfactory for all carcinogenic compounds & specific methods of chem destruction published have not been tested on all kinds of carcinogen-containing waste.

Preventive Measures of Concentrated sulfuric acid:
If employees' clothing may have become contaminated with solids or liquids containing Concentrated sulfuric acid or chromates, employees should change into uncontaminated clothing before leaving the work premises.
Clothing contaminated with Concentrated sulfuric acid or chromates should be placed in closed containers for storage until Concentrated sulfuric acid can be discarded or until provision is made for the removal of substance from the clothing. If the clothing is to be laundered or otherwise cleaned to remove the Concentrated sulfuric acid or chromates, the person performing the operation should be informed of Concentrated sulfuric acid or chromates hazardous properties.

Where there is any possibility of exposure of an employee's body to solids or liquids containing Concentrated sulfuric acid or chromates, facilities for quick drenching of the body should be provided within the immediate work area for emergency use.
Non-impervious clothing which becomes contaminated with Concentrated sulfuric acid or chromates should be removed immediately and not reworn until Concentrated sulfuric acid is removed from the clothing.

Identifiers of Concentrated sulfuric acid:
CAS Number: 7738-94-5
ChEBI: CHEBI:33143
ChemSpider: 22834
ECHA InfoCard: 100.028.910
EC Number: 231-801-5
Gmelin Reference: 25982
PubChem CID: 24425
UNII: SA8VOV0V7Q
UN number: 1755 1463
CompTox Dashboard (EPA): DTXSID8034455
InChI: InChI=1S/Cr.2H2O.2O/h;2*1H2;;/q+2;;;;/p-2
Key: KRVSOGSZCMJSLX-UHFFFAOYSA-L check
InChI=1/Cr.2H2O.2O/h;2*1H2;;/q+2;;;;/p-2/rCrH2O4/c2-1(3,4)5/h2-3H
Key: KRVSOGSZCMJSLX-OOUCQFSRAZ

SMILES:
O[Cr](O)(=O)=O
O=[Cr](=O)(O)O

Properties of Concentrated sulfuric acid:
Chemical formula: Chromic acid: H2CrO4
Dichromic acid: H2Cr2O7
Appearance: Dark red crystals
Density: 1.201 g cm−3
Melting point: 197 °C (387 °F; 470 K)
Boiling point: 250 °C (482 °F; 523 K) (decomposes)
Solubility in water: 169 g/100 mL
Acidity (pKa): -0.8 to 1.6
Conjugate base: Chromate and dichromate

Molecular Weight: 118.010 g/mol
Hydrogen Bond Donor Count: 2
Hydrogen Bond Acceptor Count: 4
Rotatable Bond Count: 0
Exact Mass: 117.935813 g/mol
Monoisotopic Mass: 117.935813 g/mol
Topological Polar Surface Area: 74.6Ų
Heavy Atom Count: 5
Complexity: 81.3
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: 1
Compound Is Canonicalized: Yes

Related Products of Concentrated sulfuric acid:
Diphenyltin Dichloride
Dipotassium Hydrogen Phosphite
1,​1'-​Diisooctyl Ester 2,​2'-​[(Dioctylstannylene)​bis(thio)​]​bis-acetic Acid (Technical Grade)
Diphenylsilane-D2
4-ethynyl-α,α-diphenyl-Benzenemethanol

Names of Concentrated sulfuric acid:

IUPAC names:
Chromic acid
Dichromic acid

Systematic IUPAC name:
Dihydroxidodioxidochromium

Other names:
Chromic(VI) acid
Tetraoxochromic acid

DESCRIPTION:
Condicare PQ-7 PF, in this version, is paraben-free.
Condicare PQ-7 PF is a highly charged cationic co-polymer that provides clarity and compatibility to anionic systems.
Condicare PQ-7 PF is highly water soluble and is ideal for use in hair and skin care applications.



CHEMICAL AND PHYSICAL PROPERTIES OF CONDICARE PQ-7:
Appearance: Clear, colorless viscous liquid
Odor: Slight, characteristic odor
Color: APHA 50 Maximum
Total Solids, % 8-10
pH (as supplied): 6.0 – 7.5
Viscosity, cps@25°C:
Brookfield LV Spindle #4@ 10rpm :7500 – 15000

APPLICATIONS OF CONDICARE PQ-7:
Condicare PQ-7 is an aqueous solution.
Use levels are recommended at approximately 0.2-5.0%.
Add co-polymer to aqueous phase under agitation.

Order of addition can be adjusted to help achieve optimum clarity.
Condicare PQ-7 contains 0.1% methyl paraben and 0.02% propyl paraben as preservatives.
A paraben-free version of Condicare PQ-7 is also available.


PERFORMANCE BENEFITS OF CONDICARE PQ-7:
Hair Care Products:
Hair Dyes and Bleaches, Permanent Waves and Relaxers, Shampoos, Conditioners, and Styling Products
• Improved wet and dry combability
• Reduced static and flyaway
• Contributes shine and a soft silky feel
• Provides rich, creamy lather with improved foam stability
Skin Care Products:
Creams & Lotions, Liquid Soaps and Bath Products, Shaving Products, AP/DO
• Provides excellent moisturization
• Smooth silky feel with good spreadability
• Soft non-greasy feel after drying
• Thick, rich foam with improved foam stability

CONDICARE PQ-7 is a highly charged cationic co-polymer that provides clarity and compatibility to anionic systems.
Condicare PQ7 is highly water-soluble and is ideal for use in hair and skincare applications.
Condicare PQ7 acts as a cationic conditioner for transparent skin and hair formulations.

Condicare PQ7 is paraben-free and leaves soft and silky feeling on skin.
Condicare PQ7 protects hair against damaging effects of processing.
Condicare PQ7 reduces build-up in hair and static flyaway.

A type of polymer, Condicare PQ7 is one of the most stable, safe, and widely used cationic conditioning ingredients in skin and hair care products, for its incredible moisturising and film-forming abilities.
The colourless, smooth and viscous liquid has strong antistatic properties which are ideal for application in anhydrous (water-free) products, where it provides rich, creamy foam to products like shampoos and shower gels for exceptional lubricity and softness.

Condicare PQ7 is a water-soluble emollient, making it a great hydrating addition to skincare products.
Compatible with most surfactant systems.

USAGE OF CONDICARE PQ7:
Condicare PQ7 is Used in a wide variety of hair care, skincare, and personal products like shampoo, conditioners, hairsprays, soaps, lubricants, make-up & make-up removers, fragrances and shaving creams.
Condicare PQ7 Gives skin and hair a silky, smooth feel when used in products.
Condicare PQ7 is also used as a thickener in many cosmetic formulations to improve the consistency and stability of the product.

0.2–5% Condicare PQ7 may be added in the cool-down phase.
Condicare PQ7 May be used in higher concentrations for products like hair gels and mousses.


BENEFITS OF CONDICARE PQ7:
Condicare PQ7 Leaves skin and hair feeling moisturised without a hint of greasiness
Condicare PQ7 Forms a thin coating on the hair shaft, inhibiting it from absorbing moisture and thus reducing frizz
Condicare PQ7 Helps detangle wet and dry hair for increased manageability
Condicare PQ7 Thickens cosmetic formulations
Condicare PQ7 is non-toxic and may be easily dissolved in water.



SAFETY INFORMATION ABOUT CONDICARE PQ-7:

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.

Conditioneze 22 polymer is a highly charged, cationic conditioning copolymer of dimethyl diallyl ammonium chloride and acrylic acid.
Furthermore, Conditioneze 22 is ampholytic and demonstrated excellent stability at extreme pH ranges (2-12).
Conditioneze 22 is ideally suited for use as a conditioning polymer in shampoos, conditioners and colorant products.

Cas Number: 53694-17-0
Molecular Formula: (C8H16ClN)n.(C3H5NO)m
Molecular Weight: 233.73



APPLICATIONS


Conditioneze 22 polymer is a highly charged, cationic conditioning copolymer of dimethyl diallyl ammonium chloride and acrylic acid.
Moreover, Conditioneze 22 is ampholytic.

Conditioneze 22 polymer is an aqueous copolymer that demonstrates ampholytic characteristics. Besides, Conditioneze 22 polymer has excellent stability in extreme pH applications making it ideally suited for use in products for dry or chemically treated hair.
Conditioneze 22 polymer is also recommended for ethnic hair care as well as skin care applications.

Conditioneze 22 polymer acts as a conditioning agent.
In addition, Conditioneze 22 is a highly charged, cationic copolymer of dimethyl diallyl ammonium chloride and acrylic acid.

This water-soluble copolymer is ampholytic and demonstrated excellent stability at extreme pH ranges (2-12).
Conditioneze 22 is compatible with a wide range of anionic, non-ionic and cationic surfactants.

Conditioneze 22 provides excellent conditioning and emulsion stabilization.
More to that, Conditioneze 22 efficiently builds viscosity at low usage levels even at low pH levels.

Conditioneze 22 polymer is used in shampoos, conditioners, styling lotions, gels, mousses, hair colorants, novelty stylers, body care, face and body washes and facial care applications.
Further to that, Conditioneze 22 is a hair conditioning agent that provides excellent conditioning and leaves hair feeling soft and silky and contributes to luster.


Features and Benefits of Conditioneze 22:

Highly charged
Cationic conditioning copolymer
Compatible with a wide range of anionic, nonionic and cationic surfactants
Stable over a wide pH range (pH 2-12)
Provides excellent conditioning, wet and dry compatibility
Leaves hair feeling soft and silky and contributes to luster
Leaves a smooth and silky feel in skin care products
Water soluble
Ampholytic
Vegan suitable


Applications of Conditioneze 22:

Ideal for shampoos
Conditioners formulated especially for damaged and treated hair
Colorant products
Ethnic hair care products


Some uses of Conditioneze 22:

Relaxant
Dyestuff
Shampoo
Conditioner
Moisturizing lotion
Emulsion
Bath liquid



DESCRIPTION


The high pH tolerance of Conditioneze 22 makes it ideal for permanent wave and relaxer products.
Conditioneze 22 is compatible with a wide range of anionic, nonionic and cationic surfactants.

Conditioneze 22 polymer is a highly charged, cationic conditioning copolymer of dimethyl diallyl ammonium chloride and acrylic acid.
This water-soluble copolymer is ampholytic and demonstrated excellent stability at extreme pH ranges (2-12).

Conditioneze 22 is ideally suited for use as a conditioning polymer in shampoos, conditioners and colorant products.
The high pH tolerance of Conditioneze 22 makes it ideal for permanent wave and relaxer products.

Conditioneze 22 is compatible with a wide range of anionic, nonionic and cationic surfactants.
Additionally, Conditioneze 22 is a copolymer of vinylpyrrolidone and methacrylamidopropyl trimethylammonium chloride, supplied as a 20% viscous solution in water.

The copolymer delivers excellent wet and dry combability, builds creamy rich lather, imparts body and manageability and does not lead to build-up on hair.
Conditioneze 22 is applied as a conditioning additive for shampoo.
Furthermore, Conditioneze 22 permits cold processing during formulation.



PROPERTIES


Appearance: viscous
Odour: No data available
Odour Threshold: No data available
pH: 4,2 - 5,3
Melting point/range: No data available
Boiling point/boiling range: 100 °C
Flash point: Not applicable
Evaporation rate: No data available
Flammability (solid, gas): No data available
Upper explosion limit: No data available
Lower explosion limit: No data available
Vapour pressure: 32 hPa (25 °C)
Relative vapour density: No data available
Relative density: No data available
Density: 1 g/cm3 (20 °C)
Solubility(ies):
Water solubility: No data available
Solubility in other solvents: No data available
Partition coefficient (n-octanol/water): No data available
Thermal decomposition: No data available
Viscosity:
Viscosity, dynamic: 4.500 mPa.s
Viscosity, kinematic: No data available
Oxidizing properties: No data available
Molecular Weight: 233.73
Hydrogen Bond Donor Count: 1
Hydrogen Bond Acceptor Count: 3
Rotatable Bond Count: 5
Exact Mass: 233.1182566
Monoisotopic Mass: 233.1182566
Topological Polar Surface Area: 37.3 Ų
Heavy Atom Count: 15
Formal Charge: 0
Complexity: 147
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: 3
Compound Is Canonicalized: Yes



FIRST AID


General advice:

No hazards which require special first aid measures.


If inhaled:

If breathed in, move person into fresh air.
If unconscious place in recovery position and seek medical advice.
If symptoms persist, call a physician.


In case of skin contact:

First aid is not normally required.
However, it is recommended that exposed areas be cleaned by washing with soap and water.


In case of eye contact:

Remove contact lenses.
Protect unharmed eye.


If swallowed:

Do not give milk or alcoholic beverages.
Never give anything by mouth to an unconscious person.
If symptoms persist, call a physician.


Most important symptoms and effects, both acute and delayed:

Symptoms:

Signs and symptoms of exposure to this material through breathing, swallowing, and/or passage of the material through the skin may include:

Stomach or intestinal upset (nausea, vomiting, diarrhea)



HANDLING AND STORAGE


Precautions for safe handling:

Advice on safe handling:

Smoking, eating and drinking should be prohibited in the application area.


Advice on protection against fire and explosion:

Normal measures for preventive fire protection.


Hygiene measures:

General industrial hygiene practice.


Conditions for safe storage, including any incompatibilities:

Requirements for storage areas and containers:

Electrical installations / working materials must comply with the technological safety standards.


Further information on storage conditions:

Protect from frost.


Advice on common storage:

No materials to be especially mentioned.


Other data:

No decomposition if stored and applied as directed.


Specific end use(s):

No data available



SYNONYMS


Dimethyldiallylammonium chloride acrylic acid polymer
N,N-Dimethyl-N-2-propenyl-2-propen-1-aminium chloride polymer with 2-propenoic acid
Acrylic acid-dimethyldiallylammonium chloride copolymer
2-Propenoic acid, polymer with N,N-dimethyl-N-2-propenyl-2-propen-1-aminium chloride (9CI)
2-Propen-1-aminium, N,N-dimethyl-N-2-propen-1-yl-, chloride (1:1), polymer with 2-propenoic acid
2-Propen-1-aminium, N,N-dimethyl-N-2-propenyl-, chloride
polymer with 2-propenoic acid (9CI)
Floc Aid 34
Diallyldimethylammonium chloride-acrylic acid copolymer
Merquat 280SD
Conditioneze 22
Acrylic acid-diallyldimethylammonium chloride copolymer
N,N-Diallyl-N,N-dimethylammonium chloride-acrylic acid copolymer
Acrylic acid-diallyldimethylammonium chloride polymer
Dimethyldiallylammonium chloride-acrylic acid copolymer
Merquat 295
Merquat 281
Merquat 280
Merquat 280 Dry
OF 280
Acrylic acid-DADMAC copolymer
Merquat 295 Dry
conditioneze 22 polymer
merquat 280 polymer
merquat 280SD polymer
merquat 281 polymer
merquat 295 polymer
2-propenaminium
N,N-dimethyl-N-(2-propenyl)-
chloride
polymer with 2-propenoic acid
Polyquaternium-22
53694-17-0
SCHEMBL1356182
dimethyl-bis(prop-2-enyl)azanium;prop-2-enoic acid;chloride

DESCRIPTION:

Conditioneze 22 polymer is a highly charged, cationic conditioning copolymer of dimethyl diallyl ammonium chloride and acrylic acid.
This water-soluble copolymer is ampholytic and demonstrated excellent stability at extreme pH ranges (2-12).
Conditioneze 22 polymer is ideally suited for use as a conditioning polymer in shampoos, conditioners and colorant products.


CAS Number(s): 53694-17-0
INCI/chemical name: Polyquaternium-22

SYNONYMS OF CONDITIONEZE 22 POLYMER

2-Propenaminium, N,N-dimethyl-N-(2-propenyl)-, chloride, polymer with 2-propenoic acid


Its high pH tolerance makes Conditioneze 22 polymer ideal for permanent wave and relaxer products.
Conditioneze 22 polymer is compatible with a wide range of anionic, nonionic and cationic surfactants.

Polyquaternium-22. Conditioneze 22 polymer by Ashland acts as a conditioning agent.
Conditioneze 22 polymer is a highly charged, cationic copolymer of dimethyl diallyl ammonium chloride and acrylic acid.
Conditioneze 22 polymer is ampholytic and demonstrated excellent stability at extreme pH ranges (2-12).

Conditioneze 22 polymer is compatible with a wide range of anionic, non-ionic and cationic surfactants.
Conditioneze 22 polymer Provides excellent conditioning and emulsion stabilization.
Conditioneze 22 polymer efficiently builds viscosity at low usage levels even at low pH levels.
Conditioneze 22 polymer is used in shampoos, conditioners, styling lotions, gels, mousses, hair colorants, novelty stylers, body care, face and body washes and facial care applications.


Conditioneze 22 polymer is a highly charged, cationic conditioning copolymer of dimethyl diallyl ammonium chloride and acrylic acid.
This water-soluble copolymer is ampholytic and demonstrated excellent stability at extreme pH ranges (2-12).

Conditioneze 22 polymer is ideally suited for use as a conditioning polymer in shampoos, conditioners and colorant products.
Its high pH tolerance makes it ideal for permanent wave and relaxer products.
Conditioneze 22 polymer is compatible with a wide range of anionic, nonionic and cationic surfactants.



BENEFITS OF CONDITIONEZE 22 POLYMER:
Conditioneze 22 polymer has Great conditioning and moisturizing properties
Conditioneze 22 polymer is Easily removable and great stiffness
Conditioneze 22 polymer Improves dry and wet combability


Conditioneze 22 polymer Works well with dry, ethnic and treated hair
Conditioneze 22 polymer is Readily available at cosmetic ingredient supplier for manufacturers

Hair care products:
Hair dyes and colors, permanent waves and relaxers, shampoos, conditioners, and styling products:
Conditioneze 22 polymer Provides excellent conditioning for products with pH ranges from 3-12
Conditioneze 22 polymer Contributes shine and a soft, lubricious feel

Conditioneze 22 polymer Improves wet and dry comb
Conditioneze 22 polymer Aids in curl retention
Conditioneze 22 polymer is Compatible with most anionic and amphoteric surfactants

Skincare products:
Creams and lotions, liquid soaps and bath products, shaving products, AP/DO:
Conditioneze 22 polymer Provides excellent moisturization
Conditioneze 22 polymer Smooth silky feel with good spreadability

Conditioneze 22 polymer has Soft non-tacky feel after drying
Conditioneze 22 polymer is Thick, rich foam with improved foam stability.



Conditioneze 22 polymer is copolymer of acrylic acid and diallyldimethylammonium chloride.
Conditioneze 22 polymer is Known for excellent conditioning qualities and ability to provide stiff hold in hair styling products.


Conditioneze 22 polymer is a highly charged cationic co-polymer that is capable of demonstrating both anionic and cationic characteristics.
Conditioneze 22 polymer demonstrates excellent pH stability and is ideal for use as a conditioning polymer in hair and skin care applications.
Conditioneze 22 polymer is a viscous clear to slightly hazy liquid with a mild aldehyde odor.



Conditioneze 22 polymer is a highly charged cationic co-polymer that is capable of demonstrating both anionic and cationic characteristics.
Conditioneze 22 polymer demonstrates excellent pH stability and is ideal for using as conditioning polymers in hair and skin care applications.


FUNCTIONS OF CONDITIONEZE 22 POLYMER:
Conditioneze 22 polymer is Moisturizer
Conditioneze 22 polymer is Sensory Modifier
Conditioneze 22 polymer is Foam stabilizer


Conditioneze 22 polymer is Antistatic
Conditioneze 22 polymer is Film-forming agent


CHEMICAL AND PHYSICAL PROPERTIES OF CONDITIONEZE 22 POLYMER
INCI NamePolyquaternium-22
Chemical Name2-Propenaminium, N,N-dimethyl-N-(2-propenyl)-, chloride, polymer with 2-propenoic acid
HS Code3906.90
CAS Number53694-17-0
Product FormLiquid
Region of OriginAsia Pacific
ReachYes
Product GroupPolyquaterniums


SAFETY INFORMATION ABOUT CONDITIONEZE 22 POLYMER
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.

CONTRAM ST1/50 is also known as N-(2-Hydroxyethyl) Morpholine, and it contains a five-membered morpholine ring and an amino group.
CONTRAM ST1/50 has been widely used in various fields of research and industry due to its unique properties, which make it suitable for a wide range of applications.
CONTRAM ST1/50 is an organic compound with the chemical formula C7H14N2O2.

CAS: 5625-90-1
MF: C9H18N2O2
MW: 186.25
EINECS: 227-062-3

CONTRAM ST1/50 is a highly concentrated industrial bactericide based on tetrahydrooxazines. Owing to CONTRAM ST1/50's good solubility this preserving agent is suitable for oily as well as aqueous systems.
CONTRAM ST1/50 is effective against gram-negative and gram positive bacterias.
CONTRAM ST1/50 is a chemical compound that has two nitrogen atoms and one oxygen atom.
CONTRAM ST1/50 is colorless, odorless, and soluble in organic solvents.
CONTRAM ST1/50 has been shown to have strong antibacterial activity against Gram-positive bacteria such as Staphylococcus aureus and some Gram-negative bacteria such as Pseudomonas aeruginosa.
The biocidal action of CONTRAM ST1/50 is due to its ability to inhibit the growth of microorganisms by disrupting the cell membrane or by inhibiting protein synthesis.
CONTRAM ST1/50 also has been used as an additive in bronchial reactivity tests on animals.

CONTRAM ST1/50 Chemical Properties
Boiling point: 122-124°C 12mm
Density: 1,04 g/cm3
Refractive index: 1.4790 (estimate)
Storage temp.: 2-8°C
pka: 6.91±0.10(Predicted)
Water Solubility: Soluble in water.
InChIKey: MIFZZKZNMWTHJK-UHFFFAOYSA-N
CAS DataBase Reference: 5625-90-1(CAS DataBase Reference)
EPA Substance Registry System: CONTRAM ST1/50 (5625-90-1)

CONTRAM ST1/50 is a colorless to pale yellow liquid with a faint odor.
CONTRAM ST1/50 has a molecular weight of 158.2 g/mol and a boiling point of 205-208°C at normal pressure.
CONTRAM ST1/50 is highly soluble in water and polar organic solvents such as ethanol, methanol, and acetone.
CONTRAM ST1/50 is stable under standard conditions and is not highly reactive towards acids, bases, or oxidizing agents.
However, CONTRAM ST1/50 can react with strong reducing agents and halogens, leading to the formation of toxic compounds (Bulger et al., 2006).

Uses
CONTRAM ST1/50 is employed as intermediate for pharmaceutical.
CONTRAM ST1/50 is successfully applied for the preservation, mineral oil containing, water miscible coolants.
Compared to hexahydrotriazines and oxazolidines, CONTRAM ST1/50 is more stable in metalworking concentrates.
CONTRAM ST1/50 should be used at an addition level of 2 – 6% in a concentrate and at 0.3% in finished cutting fluid user dilutions, in order to have a concentration of 1,000 to 1,500 ppm of the active.

Synonyms
5625-90-1
Dimorpholinomethane
N,N'-Dimorpholinomethane
4,4'-Methylenedimorpholine
4-(morpholin-4-ylmethyl)morpholine
4,4-Methylenedimorpholine
Morpholine, 4,4'-methylenebis-
N,N'-Methylenebismorpholine
bis(4-morpholinyl)methane
MORPHOLINE, 4,4'-METHYLENEDI-
MFCD00023369
4-[(morpholin-4-yl)methyl]morpholine
4,4'-Methylenebismorpholine
7O79DZW79Z
Bismorpholino methane
Dimorpholinomethone
n,n'-methylene-bis-morpholine
Bis(morpholino-)methan [German]
Bis(morpholino-)methan
EINECS 227-062-3
BRN 0111886
4,4-methylenebis-Morpholine
UNII-7O79DZW79Z
AI3-62944
bismorpholinomethane
Contram ST-1
methylenebismorpholine
bis(morpholino)methane
4,4-methylene-bismorpholine
Oprea1_332757
4,4'-methanediyldimorpholine
4-27-00-00203 (Beilstein Handbook Reference)
SCHEMBL536772
DTXSID8052859
AKOS002314380
4,4'-METHYLENEBIS(MORPHOLINE)
FS-4049
AC-12628
SY032818
CS-0236719
FT-0629594
EN300-172423
Q865946
W-110051
F2163-0188
Morpholine, 4,4'-methylenedi- (6CI,7CI,8CI); 4,4'-Methylenebis[morpholine]; Bis(morpholino)methane; Dimorpholinomethane; Methylenebismorpholine; N,N'-Methylenebismorpholine

CONTRAM ST-1 is a highly concentrated and purified industrial bactericide based on N,N-Methylenebismorpholine.
CONTRAM ST-1 is effective against both gram-negative and gram-positive bacteria.
Since CONTRAM ST-1 has limited efficacy against fungi, the product should be used in combination with a fungicide.

CAS: 5625-90-1
MF: C9H18N2O2
MW: 186.25
EINECS: 227-062-3

To inhibit the growth of bacteria in soluble oil and semi-synthetic metalworking fluids, the recommended addition level for CONTRAM ST-1 is 3% in concentrates designed for 20:1 dilution.
At a 3% treat level, this results in a 1500ppm concentration in the diluted metalworking fluid.
CONTRAM ST-1 might be added to the oil phase prior to addition of water when preparing a semi-synthetic formulation in order to maximize product efficacy and ensure long lasting performance.
CONTRAM ST-1 is a chemical compound that has two nitrogen atoms and one oxygen atom.
CONTRAM ST-1 is colorless, odorless, and soluble in organic solvents.
CONTRAM ST-1 has been shown to have strong antibacterial activity against Gram-positive bacteria such as Staphylococcus aureus and some Gram-negative bacteria such as Pseudomonas aeruginosa.
The biocidal action of CONTRAM ST-1 is due to its ability to inhibit the growth of microorganisms by disrupting the cell membrane or by inhibiting protein synthesis.
CONTRAM ST-1 also has been used as an additive in bronchial reactivity tests on animals.

CONTRAM ST-1, also known as dimethylformamide (DMF), is an organic compound belonging to the class of amides, and is one of the most widely used solvents in the world.
CONTRAM ST-1 is a colorless, volatile liquid with a characteristic odor and a relatively low boiling point.
CONTRAM ST-1 is an important industrial solvent and is used in a variety of industries, including pharmaceuticals, chemicals, plastics, and adhesives.
CONTRAM ST-1 is also used in the synthesis of a variety of organic compounds, including pharmaceuticals and agrochemicals.

CONTRAM ST-1 is an organic compound with the chemical formula C7H14N2O2.
CONTRAM ST-1 is also known as N-(2-Hydroxyethyl) Morpholine, and it contains a five-membered morpholine ring and an amino group.
CONTRAM ST-1 has been widely used in various fields of research and industry due to its unique properties, which make it suitable for a wide range of applications.

CONTRAM ST-1 is a well-known morpholine derivative that has been extensively studied for its biological and chemical properties for over 30 years.
CONTRAM ST-1 was first synthesized in 1923 and has been used as a solvent, ion-pairing reagent, buffering agent, and catalyst in various chemical reactions.
CONTRAM ST-1 has also been utilized for its unique properties such as solubility, stability, and reactivity, which make it an attractive compound for use in various fields of research and industry.

CONTRAM ST-1 Chemical Properties
Boiling point: 122-124°C 12mm
Density: 1,04 g/cm3
Refractive index: 1.4790 (estimate)
Storage temp.: 2-8°C
pka: 6.91±0.10(Predicted)
Water Solubility: Soluble in water.
InChIKey: MIFZZKZNMWTHJK-UHFFFAOYSA-N
CAS DataBase Reference: 5625-90-1(CAS DataBase Reference)
EPA Substance Registry System: CONTRAM ST-1 (5625-90-1)

CONTRAM ST-1 is a colorless to pale yellow liquid with a faint odor.
CONTRAM ST-1 has a molecular weight of 158.2 g/mol and a boiling point of 205-208°C at normal pressure.
CONTRAM ST-1 is highly soluble in water and polar organic solvents such as ethanol, methanol, and acetone.
CONTRAM ST-1 is stable under standard conditions and is not highly reactive towards acids, bases, or oxidizing agents.
However, CONTRAM ST-1 can react with strong reducing agents and halogens, leading to the formation of toxic compounds.

Uses
CONTRAM ST-1 is employed as intermediate for pharmaceutical.
CONTRAM ST-1 is successfully applied for the preservation, mineral oil containing, water miscible coolants.
Compared to hexahydrotriazines and oxazolidines, CONTRAM ST-1 is more stable in metalworking concentrates.
CONTRAM ST-1 should be used at an addition level of 2 – 6% in a concentrate and at 0.3% in finished cutting fluid user dilutions, in order to have a concentration of 1,000 to 1,500 ppm of the active.

CONTRAM ST-1 has been used in various applications in scientific experiments such as solvent, buffer, stabilizer, and reaction medium.
CONTRAM ST-1 has also been used as a catalyst for various chemical reactions such as esterification, alkylation, and isomerization.
CONTRAM ST-1 has also been utilized as an ion-pairing reagent in HPLC and as a hydrazine scavenger in water treatment.

Synthesis Method
CONTRAM ST-1 is synthesized through a variety of methods, including the reaction of dimethyl sulfate with ammonium hydroxide, the reaction of formaldehyde with dimethyl sulfate, and the reaction of dimethyl sulfoxide with formaldehyde.
CONTRAM ST-1 can also be synthesized through the reaction of dimethyl sulfoxide with ammonia, and through the reaction of dimethyl sulfoxide with formic acid.

CONTRAM ST-1 can be synthesized by reacting morpholine with formaldehyde in the presence of a catalyst such as para-toluenesulfonic acid or p-dodecylbenzenesulfonic acid.
The reaction yields a mixture of mono- and dimethylated products, which can be separated by distillation or chromatography.
The analytical methods used to characterize the compound include NMR spectroscopy, FTIR spectroscopy, and mass spectrometry.
These techniques provide information about the molecular structure, purity, and stability of the compound.

Synonyms
5625-90-1
Dimorpholinomethane
N,N'-Dimorpholinomethane
4,4'-Methylenedimorpholine
4-(morpholin-4-ylmethyl)morpholine
4,4-Methylenedimorpholine
Morpholine, 4,4'-methylenebis-
N,N'-Methylenebismorpholine
bis(4-morpholinyl)methane
MORPHOLINE, 4,4'-METHYLENEDI-
MFCD00023369
4-[(morpholin-4-yl)methyl]morpholine
4,4'-Methylenebismorpholine
7O79DZW79Z
Bismorpholino methane
Dimorpholinomethone
n,n'-methylene-bis-morpholine
Bis(morpholino-)methan [German]
Bis(morpholino-)methan
EINECS 227-062-3
BRN 0111886
4,4-methylenebis-Morpholine
UNII-7O79DZW79Z
AI3-62944
bismorpholinomethane
Contram ST-1
methylenebismorpholine
bis(morpholino)methane
4,4-methylene-bismorpholine
Oprea1_332757
4,4'-methanediyldimorpholine
4-27-00-00203 (Beilstein Handbook Reference)
SCHEMBL536772
DTXSID8052859
AKOS002314380
4,4'-METHYLENEBIS(MORPHOLINE)
FS-4049
AC-12628
SY032818
CS-0236719
FT-0629594
EN300-172423
Q865946
W-110051
F2163-0188
Morpholine, 4,4'-methylenedi- (6CI,7CI,8CI); 4,4'-Methylenebis[morpholine]; Bis(morpholino)methane; Dimorpholinomethane; Methylenebismorpholine; N,N'-Methylenebismorpholine

Contram ST-1 is a highly concentrated and purified industrial bactericide based on N, N-Methylenebismorpholine (CAS#: 5625-90-1).
Contram ST-1 is a highly concentrated industrial bactericide based on N, N - Methylenebismorpholine, an extremely effective anti-bacterial compound for use in aqueous metalworking fluids.
Contram ST-1 is effective against both gram-negative and gram-positive bacteria.


CAS Number: 5625-90-1
EC Number: 227-062-3
MDL Number: MFCD00023369
Molecular Formula: C9H18N2O2


Contram ST-1 provides a unique balance of oil and water solubility allowing for longer fluid stability and it is proven to be highly effective against a wide variety of bacteria.
Contram ST-1, also known as dimethylformamide (DMF), is an organic compound belonging to the class of amides, and is one of the most widely used solvents in the world.


Contram ST-1 is soluble in water.
Contram ST-1 is a highly concentrated industrial bactericide based on tetrahydrooxazines.
Owing to its good solubility Contram ST-1 is suitable for oily as well as aqueous systems.


Contram ST-1 has demonstrated efficacy against a wide variety of bacteria and limited efficacy against fungi, including the following typical metalworking fluid spoilage organisms:
*Acremonium spec.
*Candida albicans
*Escherichia coli
*Fusarium spec.
*Klebsiella aerogenes
*Legionella pneumophila
*Mycobacterium immunogenum
*Pseudomonas aeruginosa
*Pseudomonas fluorescens
*Pseudomonas putida
*Staphylococcus aureus



USES and APPLICATIONS of CONTRAM ST-1:
Since Contram ST-1 has limited efficacy against fungi, the product should be used in combination with a fungicide.
To inhibit the growth of bacteria in soluble oil and semi-synthetic metalworking fluids, the recommended addition level for Contram ST-1 is 3% in concentrates designed for 20:1 dilution.


At a 3% treat level, this results in a 1500ppm concentration in the diluted metalworking fluid.
Contram ST-1 might be added to the oil phase prior to addition of water when preparing a semi-synthetic formulation in order to maximize product efficacy and ensure long lasting performance.
Contram ST-1 is widely used as a low toxicity broad spectrum fungicide for water-based metalworking fluid.


With the benefits of low skin irritation, mild odor, low toxicity; formulation compatibility, lasting bactericidal, this biocide Contram ST-1 is well-known in the MWFs additives.
Contram ST-1 is employed as intermediate for pharmaceutical.


Contram ST-1 is an important industrial solvent and is used in a variety of industries, including pharmaceuticals, chemicals, plastics, and adhesives.
Contram ST-1 is also used in the synthesis of a variety of organic compounds, including pharmaceuticals and agrochemicals.


Contram ST-1 is also used in the synthesis of pharmaceuticals and agrochemicals, and as a solvent for the extraction of natural products.
In addition, Contram ST-1 is used in the preparation of catalysts, in the synthesis of polymers, and in the preparation of functionalized materials.
Contram ST-1 is employed as intermediate for pharmaceutical.



FEATURES OF CONTRAM ST-1:
Contram ST-1 is very stable and purified bactericide for metalworking concentrates with balanced oil and water solubility
In the EU this biocidal substance is already authorized under the Biocidal Products Regulation (BPR) for use in PT6 and PT13, and this Biocidal Product Contram ST-1 is in the authorization process as a biocidal Product for use in PT13 for concentrate and tank side.
Contram ST-1 is also registered in the United States under the Federal Insecticide, Fungicide and Rodenticide Act (FIFRA) for use in metalworking concentrates.
The Environmental Protection Agency (EPA) registration number is 52484-3.
Metal working fluid concentrates containing Contram ST-1 are therefore allowed for Import into the US.



ENHANCED PERFORMANCE OF CONTRAM ST-1:
*Long-lasting, persistent bacteria control for extended fluid life with minimal tank side supplements
*Exceptional stability in metalworking fluid concentrates
*Unique solubility properties in both oil and water
*Safe and effective when applied and handled properly – not classified as a skin sensitizer
*Extensive history of successful use – millions of liters of diluted metalworking fluid have been protected with Contram ST-1.



OTHER REMARKABLE FEATURES OF CONTRAM ST-1:
*Low odour
*Low formaldehyde content
*Helps in the corrosion protection
*Very stable molecule
*Good compatibility and solubility
*Very good performance
*It can be used in fluids with pH of 3 to 12.



BENEFITS OF CONTRAM ST-1:
1. a low toxicity broad spectrum fungicide for water-based metalworking fluid
2. anti-Bacteria and fungi effectively
3. fully meet with the requirements of water-based metalworking fluid: low skin irritation, mild odor, low toxicity; formulation compatibility, lasting bactericidal.
At higher concentrations, fungi and molds also have better inhibition.
Recommended addition amount (mass ratio): Recipe 2-3%, the working liquid 1-2‰;



SYNTHESIS METHOD OF CONTRAM ST-1:
Contram ST-1 is synthesized through a variety of methods, including the reaction of dimethyl sulfate with ammonium hydroxide, the reaction of formaldehyde with dimethyl sulfate, and the reaction of dimethyl sulfoxide with formaldehyde.
Contram ST-1 can also be synthesized through the reaction of dimethyl sulfoxide with ammonia, and through the reaction of dimethyl sulfoxide with formic acid.



SCIENTIFIC RESEARCH APPLICATION OF CONTRAM ST-1:
Contram ST-1 has a wide range of applications in scientific research, including as a solvent for organic synthesis, as a reagent for the synthesis of organic compounds, and as a medium for chromatography.



MECHANISM OF ACTION OF CONTRAM ST-1:
Contram ST-1 is a polar aprotic solvent, meaning that it has a low dielectric constant and a low boiling point.
This makes it an ideal solvent for many organic reactions, as Contram ST-1 has a low solubility for most organic compounds.
As a result, Contram ST-1 can facilitate the reaction of different molecules by allowing them to interact with each other more easily.
In addition, Contram ST-1 can act as a proton acceptor, allowing the formation of hydrogen bonds between molecules.



BIOCHEMICAL AND PHYSIOLOGICAL EFFECTS OF CONTRAM ST-1:
Contram ST-1 is a volatile, colorless liquid with a characteristic odor.



ADVANTAGES AND LIMITATIONS FOR LAB EXPERIMENTS OF CONTRAM ST-1:
Contram ST-1 has several advantages for laboratory experiments.
Contram ST-1 is a relatively inexpensive solvent, and is widely available.
Contram ST-1 is also a relatively non-toxic solvent, and can be used in a variety of reactions.



FUTURE DIRECTIONS OF CONTRAM ST-1:
There are a number of potential future directions for the use of Contram ST-1.
One potential direction is the development of new methods for the synthesis of organic compounds, as dimorphoContram ST-1 linomethane can facilitate the reaction of different molecules by allowing them to interact with each other more easily.
Another potential direction is the development of new catalysts and functionalized materials, as Contram ST-1 can act as a proton acceptor and facilitate the formation of hydrogen bonds between molecules.
Finally, further research into the use of Contram ST-1 as a solvent for the extraction of natural products could help to identify potential applications in the pharmaceutical and agrochemical industries.



PHYSICAL and CHEMICAL PROPERTIES of CONTRAM ST-1:
Aspect (visual): Clear low viscous liquid
Colour (visual): Colourless to slightly yellowish
Odour: Mild, nil in dilution
Density (g/cm3) @ 20°C (DIN 51 757): typ. 1.06
pH (10 g/l in water) typ.:10.2
Active content (%) typ. 50%
Refraction index @ 20°C typ.: 1.416
Viscosity (20°C, mm2/s): typ. 16
Solubility: Water soluble
Flash Point: Not applicable.
Upper Flammable: Limit Not Determined.
Lower Flammable: Limit Not Determined.
Autoignition Point: Not Determined.
Explosion Data: Material does not have explosive properties.
Vapour Pressure: Not Determined.
pH 10

Specific Gravity: 1.07 (20 °C)
Bulk Density: Not Determined.
Water Solubility: Soluble.
Percent Solid: Not Determined.
Percent Volatile: Unknown.
Volatile Organic: Compound Not Determined.
Vapour Density: Not Determined.
Evaporation Rate: Not Determined.
Odour: Amine
Appearance: Clear liquid.
Viscosity: Unknown.
Odour Threshold: Unknown.
Boiling Point: Not Determined.
Pour Point Temperature: Not Determined.
Melting / Freezing Point: Not Determined.



FIRST AID MEASURES of CONTRAM ST-1:
*Ingestion:
Rinse mouth.
*Eyes:
Rinse cautiously with water for several minutes.
Remove contact lenses, if present and easy to do.
Continue rinsing.
*Skin Wash with soap and water.
Remove contaminated clothing.
Launder contaminated clothing before reuse.
*Additional Information:
Note to physician:
Treat symptomatically.



ACCIDENTAL RELEASE MEASURES of CONTRAM ST-1:
*Spill Procedures:
Ventilate area if spilled in confined space or other poorly ventilated areas.
Do not dispose in landfill.
Pick up free liquid for recycle and/or disposal.
Residual liquid can be absorbed on inert material.



FIRE FIGHTING MEASURES of CONTRAM ST-1:
*Flash Point:
Not applicable.
*Extinguishing Media:
CO2, dry chemical, foam, water spray, water fog.



EXPOSURE CONTROLS/PERSONAL PROTECTION of CONTRAM ST-1:
-Other Exposure Limits:
None known.
-Engineering Controls:
Use material in well ventilated area only.
*Hand Protection:
If contact with the material may occur wear chemically protective gloves.
*Eye Protection:
Safety glasses.



HANDLING and STORAGE of CONTRAM ST-1:
*Pumping Temperature:
Not Determined.
Maximum Handling
Temperature:
Not Determined.
*Handling Procedures:
Keep containers closed when not in use.
Do not discharge into drains or the environment, dispose to an authorized waste collection point.
Use appropriate containment to avoid environmental contamination.
Wash thoroughly after handling.
Do not eat, drink or smoke when using this product.
*Maximum Storage:
Temperature:
Not Determined.
Storage Procedures:
No special storage precautions required.
Loading Temperature:
Not Determined.



STABILITY and REACTIVITY of CONTRAM ST-1:
*Stability:
Material is normally stable at moderately elevated temperatures and pressures.
*Decomposition Temperature:
Not Determined.
*Polymerization:
Will not occur.
*Thermal Decomposition:
Thermal decomposition and combustion are not expected to occur except under extreme conditions.

Contram ST-1/50 is a highly concentrated industrial bactericide based on tetrahydrooxazines.
Owing to its good solubility Contram ST-1/50 is suitable for oily as well as aqueous systems.
Contram ST-1/50 is soluble in water.


CAS Number: 5625-90-1
EC Number: 227-062-3
MDL Number: MFCD00023369
Molecular Formula: C9H18N2O2


Contram ST-1/50 is effective against gram-negative and gram positive bacterias.
Contram ST-1/50, also known as dimethylformamide (DMF), is an organic compound belonging to the class of amides, and is one of the most widely used solvents in the world.
Contram ST-1/50 is a colorless, volatile liquid with a characteristic odor and a relatively low boiling point.



USES and APPLICATIONS of CONTRAM ST-1/50:
Contram ST-1/50 is successfully applied for the preservation, mineral oil containing, water-miscible coolants.
Compared to hexahydrotriazines and oxazolidines, Contram ST-1/50 is more stable in metalworking concentrates.
Contram ST-1/50 should be used at an addition level of 2 – 6% in a concentrate and at 0.3% in finished cutting fluid user dilutions, in order to have a concentration of 1,000 to 1,500 ppm of the active.


Contram ST-1/50 is widely used as a low toxicity broad spectrum fungicide for water-based metalworking fluid.
With the benefits of low skin irritation, mild odor, low toxicity; formulation compatibility, lasting bactericidal, this biocide Contram ST-1/50 is well-known in the MWFs additives.
Contram ST-1/50 is employed as intermediate for pharmaceutical.


Contram ST-1/50 is an important industrial solvent and is used in a variety of industries, including pharmaceuticals, chemicals, plastics, and adhesives.
Contram ST-1/50 is also used in the synthesis of a variety of organic compounds, including pharmaceuticals and agrochemicals.
Contram ST-1/50 is employed as intermediate for pharmaceutical.
Contram ST-1/50 is employed as intermediate for pharmaceutical.


Contram ST-1/50 is also used in the synthesis of pharmaceuticals and agrochemicals, and as a solvent for the extraction of natural products.
In addition, Contram ST-1/50 is used in the preparation of catalysts, in the synthesis of polymers, and in the preparation of functionalized materials.
In addition, Contram ST-1/50 is used in the preparation of catalysts, in the synthesis of polymers, and in the preparation of functionalized materials.


Contram ST-1/50 is widely used as a low toxicity broad spectrum fungicide for water-based metalworking fluid.
With the benefits of low skin irritation, mild odor, low toxicity; formulation compatibility, lasting bactericidal, this biocide Contram ST-1/50 is well-known in the MWFs additives.
Contram ST-1/50 is employed as intermediate for pharmaceutical.


Contram ST-1/50 is an important industrial solvent and is used in a variety of industries, including pharmaceuticals, chemicals, plastics, and adhesives.
Contram ST-1/50 is also used in the synthesis of a variety of organic compounds, including pharmaceuticals and agrochemicals.
Contram ST-1/50 is also used in the synthesis of pharmaceuticals and agrochemicals, and as a solvent for the extraction of natural products.



OTHER REMARKABLE FEATURES OF CONTRAM ST-1/50:
*Low odour
*Low formaldehyde content
*Helps in the corrosion protection
*Very stable molecule
*Good compatibility and solubility
*Very good performance
*It can be used in fluids with pH of 3 to 12.



BENEFITS OF CONTRAM ST-1/50:
1, a low toxicity broad spectrum fungicide for water-based metalworking fluid
2, anti-Bacteria and fungi effectively
3, fully meet with the requirements of water-based metalworking fluid: low skin irritation, mild odor, low toxicity; formulation compatibility, lasting bactericidal.
At higher concentrations, fungi and molds also have better inhibition.
Recommended addition amount (mass ratio): Recipe 2-3%, the working liquid 1-2‰;



SYNTHESIS METHOD OF CONTRAM ST-1/50:
Contram ST-1/50 is synthesized through a variety of methods, including the reaction of dimethyl sulfate with ammonium hydroxide, the reaction of formaldehyde with dimethyl sulfate, and the reaction of dimethyl sulfoxide with formaldehyde.
Contram ST-1/50 can also be synthesized through the reaction of dimethyl sulfoxide with ammonia, and through the reaction of dimethyl sulfoxide with formic acid.



SCIENTIFIC RESEARCH APPLICATION OF CONTRAM ST-1/50:
Contram ST-1/50 has a wide range of applications in scientific research, including as a solvent for organic synthesis, as a reagent for the synthesis of organic compounds, and as a medium for chromatography.



MECHANISM OF ACTION OF CONTRAM ST-1/50:
Contram ST-1/50 is a polar aprotic solvent, meaning that it has a low dielectric constant and a low boiling point.
This makes it an ideal solvent for many organic reactions, as Contram ST-1/50 has a low solubility for most organic compounds.
As a result, Contram ST-1/50 can facilitate the reaction of different molecules by allowing them to interact with each other more easily.
In addition, Contram ST-1/50 can act as a proton acceptor, allowing the formation of hydrogen bonds between molecules.



BIOCHEMICAL AND PHYSIOLOGICAL EFFECTS OF CONTRAM ST-1/50:
Contram ST-1/50 is a volatile, colorless liquid with a characteristic odor.



ADVANTAGES AND LIMITATIONS FOR LAB EXPERIMENTS OF CONTRAM ST-1/50:
Contram ST-1/50 has several advantages for laboratory experiments.
Contram ST-1/50 is a relatively inexpensive solvent, and is widely available.
Contram ST-1/50 is also a relatively non-toxic solvent, and can be used in a variety of reactions.



FUTURE DIRECTIONS OF CONTRAM ST-1/50:
There are a number of potential future directions for the use of Contram ST-1/50.
One potential direction is the development of new methods for the synthesis of organic compounds, as dimorphoContram ST-1/50 linomethane can facilitate the reaction of different molecules by allowing them to interact with each other more easily.
Another potential direction is the development of new catalysts and functionalized materials, as Contram ST-1/50 can act as a proton acceptor and facilitate the formation of hydrogen bonds between molecules.
Finally, further research into the use of Contram ST-1/50 as a solvent for the extraction of natural products could help to identify potential applications in the pharmaceutical and agrochemical industries.



PHYSICAL and CHEMICAL PROPERTIES of CONTRAM ST-1/50:
Flash Point: Not applicable.
Upper Flammable: Limit Not Determined.
Lower Flammable: Limit Not Determined.
Autoignition Point: Not Determined.
Explosion Data: Material does not have explosive properties.
Vapour Pressure: Not Determined.
pH 10
Specific Gravity: 1.07 (20 °C)
Bulk Density: Not Determined.
Water Solubility: Soluble.
Percent Solid: Not Determined.
Percent Volatile: Unknown.
Volatile Organic: Compound Not Determined.
Vapour Density: Not Determined.
Evaporation Rate: Not Determined.

Odour: Amine
Appearance: Clear liquid.
Viscosity: Unknown.
Odour Threshold: Unknown.
Boiling Point: Not Determined.
Pour Point Temperature: Not Determined.
Melting / Freezing Point: Not Determined.
Aspect (visual): Clear low viscous liquid
Colour (visual): Colourless to slightly yellowish
Odour: Mild, nil in dilution
Density (g/cm3) @ 20°C (DIN 51 757): typ. 1.06
pH (10 g/l in water) typ.:10.2
Active content (%) typ. 50%
Refraction index @ 20°C typ.: 1.416
Viscosity (20°C, mm2/s): typ. 16
Solubility: Water soluble



FIRST AID MEASURES of CONTRAM ST-1/50:
*Ingestion:
Rinse mouth.
*Eyes:
Rinse cautiously with water for several minutes.
Remove contact lenses, if present and easy to do.
Continue rinsing.
*Skin Wash with soap and water.
Remove contaminated clothing.
Launder contaminated clothing before reuse.
*Additional Information:
Note to physician:
Treat symptomatically.



ACCIDENTAL RELEASE MEASURES of CONTRAM ST-1/50:
*Spill Procedures:
Ventilate area if spilled in confined space or other poorly ventilated areas.
Do not dispose in landfill.
Pick up free liquid for recycle and/or disposal.
Residual liquid can be absorbed on inert material.



FIRE FIGHTING MEASURES of CONTRAM ST-1/50:
*Flash Point:
Not applicable.
*Extinguishing Media:
CO2, dry chemical, foam, water spray, water fog.



EXPOSURE CONTROLS/PERSONAL PROTECTION of CONTRAM ST-1/50:
-Other Exposure Limits:
None known.
-Engineering Controls:
Use material in well ventilated area only.
*Hand Protection:
If contact with the material may occur wear chemically protective gloves.
*Eye Protection:
Safety glasses.



HANDLING and STORAGE of CONTRAM ST-1/50:
*Pumping Temperature:
Not Determined.
Maximum Handling
Temperature:
Not Determined.
*Handling Procedures:
Keep containers closed when not in use.
Do not discharge into drains or the environment, dispose to an authorized waste collection point.
Use appropriate containment to avoid environmental contamination.
Wash thoroughly after handling.
Do not eat, drink or smoke when using this product.
*Maximum Storage:
Temperature:
Not Determined.
Storage Procedures:
No special storage precautions required.
Loading Temperature:
Not Determined.



STABILITY and REACTIVITY of CONTRAM ST-1/50:
*Stability:
Material is normally stable at moderately elevated temperatures and pressures.
*Decomposition Temperature:
Not Determined.
*Polymerization:
Will not occur.
*Thermal Decomposition:
Thermal decomposition and combustion are not expected to occur except under extreme conditions.

Contram ST-1/50 is a colorless, volatile liquid with a characteristic odor and a relatively low boiling point.
Contram ST-1/50 is a highly concentrated industrial bactericide based on tetrahydrooxazines.
Contram ST-1/50, also known as dimethylformamide (DMF), is an organic compound belonging to the class of amides, and is one of the most widely used solvents in the world.


CAS Number: 5625-90-1
EC Number: 227-062-3
MDL Number: MFCD00023369
Molecular Formula: C9H18N2O2


Contram ST-1/50 is a highly concentrated industrial bactericide based on tetrahydrooxazines.
Owing to its good solubility Contram ST-1/50 is suitable for oily as well as aqueous systems.
Contram ST-1/50 is soluble in water.


Contram ST-1/50 is effective against gram-negative and gram positive bacterias.
Contram ST-1/50, also known as dimethylformamide (DMF), is an organic compound belonging to the class of amides, and is one of the most widely used solvents in the world.
Contram ST-1/50 is a colorless, volatile liquid with a characteristic odor and a relatively low boiling point.


Contram ST-1/50 is effective against gram-negative and grampositive bacteria.
Contram ST-1/50 is a highly concentrated industrial bactericide based on tetra hydro oxazines.
Due to Contram ST-1/50's good solubility, this preserving agent is suitable for oilbased and water-based systems.


The recommended addition level for Contram ST-1/50
is 1 - 3% in the concentrate and 0.15% in the end use dilution.
Contram ST-1/50 is not compatible with acids and oxidizing agents.



USES and APPLICATIONS of CONTRAM ST-1/50:
Contram ST-1/50 is successfully applied for the preservation, mineral oil containing, water-miscible coolants.
Contram ST-1/50 is also used in the synthesis of a variety of organic compounds, including pharmaceuticals and agrochemicals.
Compared to hexahydrotriazines and oxazolidines, Contram ST-1/50 is more stable in metalworking concentrates.


Contram ST-1/50 is employed as intermediate for pharmaceutical.
Contram ST-1/50 should be used at an addition level of 2 – 6% in a concentrate and at 0.3% in finished cutting fluid user dilutions, in order to have a concentration of 1,000 to 1,500 ppm of the active.


Compared to hexahydrotriazines and oxazolidines, Contram ST-1/50 is more stable in metalworking concentrates.
In addition, Contram ST-1/50 is used in the preparation of catalysts, in the synthesis of polymers, and in the preparation of functionalized materials.
Contram ST-1/50 is widely used as a low toxicity broad spectrum fungicide for water-based metalworking fluid.


With the benefits of low skin irritation, mild odor, low toxicity; formulation compatibility, lasting bactericidal, this biocide Contram ST-1/50 is well-known in the MWFs additives.
Contram ST-1/50 is employed as intermediate for pharmaceutical.
Contram ST-1/50 is widely used as a low toxicity broad spectrum fungicide for water-based metalworking fluid.


With the benefits of low skin irritation, mild odor, low toxicity; formulation compatibility, lasting bactericidal, this biocide Contram ST-1/50 is well-known in the MWFs additives.
Contram ST-1/50 has been used successfully to preserve oil-based and water-based metalworking fluids.
Contram ST-1/50 is employed as intermediate for pharmaceutical.


Contram ST-1/50 is an important industrial solvent and is used in a variety of industries, including pharmaceuticals, chemicals, plastics, and adhesives.
Contram ST-1/50 is also used in the synthesis of pharmaceuticals and agrochemicals, and as a solvent for the extraction of natural products.
Contram ST-1/50 is an important industrial solvent and is used in a variety of industries, including pharmaceuticals, chemicals, plastics, and adhesives.


Contram ST-1/50 is also used in the synthesis of a variety of organic compounds, including pharmaceuticals and agrochemicals.
Contram ST-1/50 is employed as intermediate for pharmaceutical.
Contram ST-1/50 is also used in the synthesis of pharmaceuticals and agrochemicals, and as a solvent for the extraction of natural products.
In addition, Contram ST-1/50 is used in the preparation of catalysts, in the synthesis of polymers, and in the preparation of functionalized materials.



BENEFITS OF CONTRAM ST-1/50:
1, a low toxicity broad spectrum fungicide for water-based metalworking fluid
2, anti-Bacteria and fungi effectively
3, fully meet with the requirements of water-based metalworking fluid: low skin irritation, mild odor, low toxicity; formulation compatibility, lasting bactericidal.
At higher concentrations, fungi and molds also have better inhibition.
Recommended addition amount (mass ratio): Recipe 2-3%, the working liquid 1-2‰;



MECHANISM OF ACTION OF CONTRAM ST-1/50:
Contram ST-1/50 is a polar aprotic solvent, meaning that it has a low dielectric constant and a low boiling point.
This makes it an ideal solvent for many organic reactions, as Contram ST-1/50 has a low solubility for most organic compounds.
As a result, Contram ST-1/50 can facilitate the reaction of different molecules by allowing them to interact with each other more easily.
In addition, Contram ST-1/50 can act as a proton acceptor, allowing the formation of hydrogen bonds between molecules.



OTHER REMARKABLE FEATURES OF CONTRAM ST-1/50:
*Low odour
*Low formaldehyde content
*Helps in the corrosion protection
*Very stable molecule
*Good compatibility and solubility
*Very good performance
*It can be used in fluids with pH of 3 to 12.



SYNTHESIS METHOD OF CONTRAM ST-1/50:
Contram ST-1/50 is synthesized through a variety of methods, including the reaction of dimethyl sulfate with ammonium hydroxide, the reaction of formaldehyde with dimethyl sulfate, and the reaction of dimethyl sulfoxide with formaldehyde.
Contram ST-1/50 can also be synthesized through the reaction of dimethyl sulfoxide with ammonia, and through the reaction of dimethyl sulfoxide with formic acid.



FUTURE DIRECTIONS OF CONTRAM ST-1/50:
There are a number of potential future directions for the use of Contram ST-1/50.
One potential direction is the development of new methods for the synthesis of organic compounds, as dimorphoContram ST-1/50 linomethane can facilitate the reaction of different molecules by allowing them to interact with each other more easily.
Another potential direction is the development of new catalysts and functionalized materials, as Contram ST-1/50 can act as a proton acceptor and facilitate the formation of hydrogen bonds between molecules.
Finally, further research into the use of Contram ST-1/50 as a solvent for the extraction of natural products could help to identify potential applications in the pharmaceutical and agrochemical industries.



BIOCHEMICAL AND PHYSIOLOGICAL EFFECTS OF CONTRAM ST-1/50:
Contram ST-1/50 is a volatile, colorless liquid with a characteristic odor.



SCIENTIFIC RESEARCH APPLICATION OF CONTRAM ST-1/50:
Contram ST-1/50 has a wide range of applications in scientific research, including as a solvent for organic synthesis, as a reagent for the synthesis of organic compounds, and as a medium for chromatography.



ADVANTAGES AND LIMITATIONS FOR LAB EXPERIMENTS OF CONTRAM ST-1/50:
Contram ST-1/50 has several advantages for laboratory experiments.
Contram ST-1/50 is a relatively inexpensive solvent, and is widely available.
Contram ST-1/50 is also a relatively non-toxic solvent, and can be used in a variety of reactions.



PHYSICAL and CHEMICAL PROPERTIES of CONTRAM ST-1/50:
Odour: Amine
Appearance: Clear liquid.
Viscosity: Unknown.
Odour Threshold: Unknown.
Boiling Point: Not Determined.
Pour Point Temperature: Not Determined.
Melting / Freezing Point: Not Determined.
Aspect (visual): Clear low viscous liquid
Colour (visual): Colourless to slightly yellowish
Odour: Mild, nil in dilution
Density (g/cm3) @ 20°C (DIN 51 757): typ. 1.06
pH (10 g/l in water) typ.:10.2
Active content (%) typ. 50%
Refraction index @ 20°C typ.: 1.416
Viscosity (20°C, mm2/s): typ. 16
Solubility: Water soluble
Flash Point: Not applicable.
Upper Flammable: Limit Not Determined.
Lower Flammable: Limit Not Determined.
Autoignition Point: Not Determined.
Explosion Data: Material does not have explosive properties.
Vapour Pressure: Not Determined.

pH: 10
Specific Gravity: 1.07 (20 °C)
Bulk Density: Not Determined.
Water Solubility: Soluble.
Percent Solid: Not Determined.
Percent Volatile: Unknown.
Volatile Organic: Compound Not Determined.
Vapour Density: Not Determined.
Evaporation Rate: Not Determined.
Appearance at Room Temperature: Clear Low Viscous Liquid
Appearance below 18ºC: Solid
Colour Colourless to Light: Yellow
Odour: Mild
Density: at 20°C g/cm3 1.06
pH-value (10 g/l in water): 10
Activity: % 92
Refractive Index: at 20°C 1.47
Viscosity: at 20ºC mm2/s 20
Water content: % 8
Solubility: Soluble in oil
Miscible with water



FIRST AID MEASURES of CONTRAM ST-1/50:
*Ingestion:
Rinse mouth.
*Eyes:
Rinse cautiously with water for several minutes.
Remove contact lenses, if present and easy to do.
Continue rinsing.
*Skin Wash with soap and water.
Remove contaminated clothing.
Launder contaminated clothing before reuse.
*Additional Information:
Note to physician:
Treat symptomatically.



ACCIDENTAL RELEASE MEASURES of CONTRAM ST-1/50:
*Spill Procedures:
Ventilate area if spilled in confined space or other poorly ventilated areas.
Do not dispose in landfill.
Pick up free liquid for recycle and/or disposal.
Residual liquid can be absorbed on inert material.



FIRE FIGHTING MEASURES of CONTRAM ST-1/50:
*Flash Point:
Not applicable.
*Extinguishing Media:
CO2, dry chemical, foam, water spray, water fog.



EXPOSURE CONTROLS/PERSONAL PROTECTION of CONTRAM ST-1/50:
-Other Exposure Limits:
None known.
-Engineering Controls:
Use material in well ventilated area only.
*Hand Protection:
If contact with the material may occur wear chemically protective gloves.
*Eye Protection:
Safety glasses.



HANDLING and STORAGE of CONTRAM ST-1/50:
*Pumping Temperature:
Not Determined.
Maximum Handling
Temperature:
Not Determined.
*Handling Procedures:
Keep containers closed when not in use.
Do not discharge into drains or the environment, dispose to an authorized waste collection point.
Use appropriate containment to avoid environmental contamination.
Wash thoroughly after handling.
Do not eat, drink or smoke when using this product.
*Maximum Storage:
Temperature:
Not Determined.
Storage Procedures:
No special storage precautions required.
Loading Temperature:
Not Determined.



STABILITY and REACTIVITY of CONTRAM ST-1/50:
*Stability:
Material is normally stable at moderately elevated temperatures and pressures.
*Decomposition Temperature:
Not Determined.
*Polymerization:
Will not occur.
*Thermal Decomposition:
Thermal decomposition and combustion are not expected to occur except under extreme conditions.




SYNONYM:
5625-90-1
Dimorpholinomethane
N,N'-Dimorpholinomethane
4,4'-Methylenedimorpholine
4,4-Methylenedimorpholine
4-(morpholin-4-ylmethyl)morpholine
N,N'-Methylenebismorpholine
Morpholine, 4,4'-methylenebis-
bis(4-morpholinyl)methane
n,n'-methylene-bis-morpholine
MORPHOLINE, 4,4'-METHYLENEDI-
MFCD00023369
4,4'-Methylenebismorpholine
7O79DZW79Z
4-[(morpholin-4-yl)methyl]morpholine
Bismorpholino methane
Dimorpholinomethone
Bis(morpholino-)methan
EINECS 227-062-3
BRN 0111886
UNII-7O79DZW79Z
AI3-62944
bismorpholinomethane
Contram ST-1
methylenebismorpholine
bis(morpholino)methane
N,N\'-Dimorpholinomethane
4,4-methylene-bismorpholine
Oprea1_332757
4,4'-methanediyldimorpholine
N,N'-Methylene bismorpholine
4-27-00-00203 (Beilstein Handbook Reference)
SCHEMBL536772
DTXSID8052859
Bis(4-morpholinyl)methane, 98%
ZINC19324145
AKOS002314380
4,4'-METHYLENEBIS(MORPHOLINE)
FS-4049
AC-12628
SY032818
DB-052882
CS-0236719
FT-0629594
EN300-172423
Q865946
W-110051
F2163-0188
N,N'-DIMORPHOLINOMETHANE
4,4'-methylenedi-morpholin
4,4'-methylenedimorpholine
bis(morpholino-)methan
bismorpholinomethane
N,N'-Methylenebismorpholine
DIMORPHOLINOMETHANE
DIMORPHOLINOMETHONE
N,N'-DIMORPHOLINOMETHANE
4,4’-methylenedi-morpholin
4,4’-methylenedimorpholine
bis(morpholino-)methan
bismorpholinomethane
N,N’-Methylenebismorpholine
DIMORPHOLINOMETHANE
DIMORPHOLINOMETHONE
N,N'-Dimorpholinomethane
N,N´-Methylene bismorpholine
Bis (morpholino-) methan
Bismorpholino methane
4,4-Methylenedimorpholine
Morpholine, 4,4-methylenedi-
DIMORPHOLINOMETHONE
DIMORPHOLINOMETHANE
N,N-Dimorpholinomethane
MORPHOLINE44METHYLENEDI
BIS-(MORPHOLINE-)METHANE
44METHYLENEBISMORPHOLINE
Bis(4-morpholinyl)methane
N,N'-Methylenebismorpholine
4,4-methylenebis-Morpholine
N,N'-Methylenebismorpholine
Morpholine,4,4-Methylenebis-
4,4'-methanediyldimorpholine
Morpholine,4,4-methylenebis-
N,N'-Methylene-bis-morpholine
Methylene-bis-morpholine,N,N'-
N,N-Dimorpholinomethane
Morpholine,4,4-methylenebis-
Bis(4-morpholinyl)methane
N,N'-Methylenebismorpholine
4,4'-methanediyldimorpholine
4,4-methylenebis-Morpholine
N,N-Methylene-bis-morpholine
N,N-Dimorpholinomethane
Morpholine,4,4-methylenebis-
Bis(4-morpholinyl)methane
N,N'-Methylenebismorpholine
4,4'-methanediyldimorpholine
-bis-morpholine
4,4′-Methylenebis[morpholine]
4,4′-Methylenedimorpholine
4,4'-Dimorpholinylmethane
4,4'-Methylenebismorpholine
44METHYLENEBISMORPHOLINE
BIS-(MORPHOLINE-)METHANE
Bis(morpholino)methane
DIMORPHOLINOMETHANE
DIMORPHOLINOMETHONE
Methylenebismorpholine
Methylene-bis-morpholine,N,N'-
Morpholine, 4,4′-methylenebis-
Morpholine, 4,4′-methylenedi-
Morpholine,4,4-Methylenebis-
MORPHOLINE44METHYLENEDI
N,N′-Methylenebismorpholine;
N,N′-methylenebismorpholine
formaldehyde released from N,N′-methylenebismorpholine
N,N′-methylenebismorpholine
formaldehyde released by N,N′-methylenebismorpholine / MBM
DIMORPHOLINOMETHANE
N,N'-DIMORPHOLINOMETHANE
4,4’-methylenedi-morpholin
4,4’-methylenedimorpholine
bis(morpholino-)methan
bismorpholinomethane
N,N’-Methylenebismorpholine
DIMORPHOLINOMETHONE
Morpholine,4,4-Methylenebis-
Methylene-bis-morpholine,N,N'-
MORPHOLINE44METHYLENEDI
44METHYLENEBISMORPHOLINE
BIS-(MORPHOLINE-)METHANE
DIMORPHOLINOMETHONE
DIMORPHOLINOMETHANE
N,N-Dimorpholinomethane
MORPHOLINE44METHYLENEDI
BIS-(MORPHOLINE-)METHANE
44METHYLENEBISMORPHOLINE
Bis(4-morpholinyl)methane
N,N'-Methylenebismorpholine
4,4-methylenebis-Morpholine
N,N'-Methylenebismorpholine
Morpholine,4,4-Methylenebis-
4,4'-methanediyldimorpholine
Morpholine,4,4-methylenebis-
N,N'-Methylene-bis-morpholine
Methylene-bis-morpholine,N,N'-

Contram ST-2 is a highly concentrated industrial bactericide based on tetrahydrooxazines.
Owing to its good solubility Contram ST-2 is suitable for oily as well as aqueous systems.
Contram ST-2 is soluble in water.


Contram ST-2 is effective against gram-negative and gram positive bacterias.
Contram ST-2, also known as dimethylformamide (DMF), is an organic compound belonging to the class of amides, and is one of the most widely used solvents in the world.
Contram ST-2 is a colorless, volatile liquid with a characteristic odor and a relatively low boiling point.



USES and APPLICATIONS of CONTRAM ST-2:
Contram ST-2 has been used successfully to preserve oil-based and water-based metalworking fluids.
Contram ST-2 is successfully applied for the preservation, mineral oil containing, water-miscible coolants.
Contram ST-2 is also used in the synthesis of a variety of organic compounds, including pharmaceuticals and agrochemicals.


Compared to hexahydrotriazines and oxazolidines, Contram ST-2 is more stable in metalworking concentrates.
Compared to hexahydrotriazines and oxazolidines, Contram ST-2 is more stable in metalworking concentrates.
Contram ST-2 is employed as intermediate for pharmaceutical.


Contram ST-2 should be used at an addition level of 2 – 6% in a concentrate and at 0.3% in finished cutting fluid user dilutions, in order to have a concentration of 1,000 to 1,500 ppm of the active.
In addition, Contram ST-2 is used in the preparation of catalysts, in the synthesis of polymers, and in the preparation of functionalized materials.


Contram ST-2 is widely used as a low toxicity broad spectrum fungicide for water-based metalworking fluid.
With the benefits of low skin irritation, mild odor, low toxicity; formulation compatibility, lasting bactericidal, this biocide Contram ST-2 is well-known in the MWFs additives.


Contram ST-2 is employed as intermediate for pharmaceutical.
Contram ST-2 is widely used as a low toxicity broad spectrum fungicide for water-based metalworking fluid.
With the benefits of low skin irritation, mild odor, low toxicity; formulation compatibility, lasting bactericidal, this biocide Contram ST-2 is well-known in the MWFs additives.


Contram ST-2 is employed as intermediate for pharmaceutical.
Contram ST-2 is an important industrial solvent and is used in a variety of industries, including pharmaceuticals, chemicals, plastics, and adhesives.
Contram ST-2 is also used in the synthesis of pharmaceuticals and agrochemicals, and as a solvent for the extraction of natural products.
Contram ST-2 is an important industrial solvent and is used in a variety of industries, including pharmaceuticals, chemicals, plastics, and adhesives.


Contram ST-2 is also used in the synthesis of a variety of organic compounds, including pharmaceuticals and agrochemicals.
Contram ST-2 is employed as intermediate for pharmaceutical.
Contram ST-2 is also used in the synthesis of pharmaceuticals and agrochemicals, and as a solvent for the extraction of natural products.
In addition, Contram ST-2 is used in the preparation of catalysts, in the synthesis of polymers, and in the preparation of functionalized materials.



BENEFITS OF CONTRAM ST-2:
1, a low toxicity broad spectrum fungicide for water-based metalworking fluid
2, anti-Bacteria and fungi effectively
3, fully meet with the requirements of water-based metalworking fluid: low skin irritation, mild odor, low toxicity; formulation compatibility, lasting bactericidal.
At higher concentrations, fungi and molds also have better inhibition.
Recommended addition amount (mass ratio): Recipe 2-3%, the working liquid 1-2‰;



MECHANISM OF ACTION OF CONTRAM ST-2:
Contram ST-2 is a polar aprotic solvent, meaning that it has a low dielectric constant and a low boiling point.
This makes it an ideal solvent for many organic reactions, as Contram ST-2 has a low solubility for most organic compounds.
As a result, Contram ST-2 can facilitate the reaction of different molecules by allowing them to interact with each other more easily.
In addition, Contram ST-2 can act as a proton acceptor, allowing the formation of hydrogen bonds between molecules.



OTHER REMARKABLE FEATURES OF CONTRAM ST-1/50:
*Low odour
*Low formaldehyde content
*Helps in the corrosion protection
*Very stable molecule
*Good compatibility and solubility
*Very good performance
*It can be used in fluids with pH of 3 to 12.



SYNTHESIS METHOD OF CONTRAM ST-2:
Contram ST-2 is synthesized through a variety of methods, including the reaction of dimethyl sulfate with ammonium hydroxide, the reaction of formaldehyde with dimethyl sulfate, and the reaction of dimethyl sulfoxide with formaldehyde.
Contram ST-2 can also be synthesized through the reaction of dimethyl sulfoxide with ammonia, and through the reaction of dimethyl sulfoxide with formic acid.



FUTURE DIRECTIONS OF CONTRAM ST-2:
There are a number of potential future directions for the use of Contram ST-2.
One potential direction is the development of new methods for the synthesis of organic compounds, as dimorphoContram ST-2 linomethane can facilitate the reaction of different molecules by allowing them to interact with each other more easily.
Another potential direction is the development of new catalysts and functionalized materials, as Contram ST-2 can act as a proton acceptor and facilitate the formation of hydrogen bonds between molecules.
Finally, further research into the use of Contram ST-2 as a solvent for the extraction of natural products could help to identify potential applications in the pharmaceutical and agrochemical industries.



BIOCHEMICAL AND PHYSIOLOGICAL EFFECTS OF CONTRAM ST-2:
Contram ST-2 is a volatile, colorless liquid with a characteristic odor.



SCIENTIFIC RESEARCH APPLICATION OF CONTRAM ST-2:
Contram ST-2 has a wide range of applications in scientific research, including as a solvent for organic synthesis, as a reagent for the synthesis of organic compounds, and as a medium for chromatography.



ADVANTAGES AND LIMITATIONS FOR LAB EXPERIMENTS OF CONTRAM ST-2:
Contram ST-2 has several advantages for laboratory experiments.
Contram ST-2 is a relatively inexpensive solvent, and is widely available.
Contram ST-2 is also a relatively non-toxic solvent, and can be used in a variety of reactions.



PHYSICAL and CHEMICAL PROPERTIES of CONTRAM ST-2:
Appearance at Room Temperature: Clear Low Viscous Liquid
Appearance below 18ºC: Solid
Colour Colourless to Light: Yellow
Odour: Mild
Density: at 20°C g/cm3 1.06
pH-value (10 g/l in water): 10
Activity: % 92
Refractive Index: at 20°C 1.47
Viscosity: at 20ºC mm2/s 20
Water content: % 8
Solubility: Soluble in oil
Miscible with water
Odour: Amine
Appearance: Clear liquid.
Viscosity: Unknown.
Odour Threshold: Unknown.
Boiling Point: Not Determined.
Pour Point Temperature: Not Determined.
Melting / Freezing Point: Not Determined.
Aspect (visual): Clear low viscous liquid

Colour (visual): Colourless to slightly yellowish
Odour: Mild, nil in dilution
Density (g/cm3) @ 20°C (DIN 51 757): typ. 1.06
pH (10 g/l in water) typ.:10.2
Active content (%) typ. 50%
Refraction index @ 20°C typ.: 1.416
Viscosity (20°C, mm2/s): typ. 16
Solubility: Water soluble
Flash Point: Not applicable.
Upper Flammable: Limit Not Determined.
Lower Flammable: Limit Not Determined.
Autoignition Point: Not Determined.
Explosion Data: Material does not have explosive properties.
Vapour Pressure: Not Determined.
pH: 10
Specific Gravity: 1.07 (20 °C)
Bulk Density: Not Determined.
Water Solubility: Soluble.
Percent Solid: Not Determined.
Percent Volatile: Unknown.
Volatile Organic: Compound Not Determined.
Vapour Density: Not Determined.
Evaporation Rate: Not Determined.



FIRST AID MEASURES of CONTRAM ST-2:
*Ingestion:
Rinse mouth.
*Eyes:
Rinse cautiously with water for several minutes.
Remove contact lenses, if present and easy to do.
Continue rinsing.
*Skin Wash with soap and water.
Remove contaminated clothing.
Launder contaminated clothing before reuse.
*Additional Information:
Note to physician:
Treat symptomatically.



ACCIDENTAL RELEASE MEASURES of CONTRAM ST-2:
*Spill Procedures:
Ventilate area if spilled in confined space or other poorly ventilated areas.
Do not dispose in landfill.
Pick up free liquid for recycle and/or disposal.
Residual liquid can be absorbed on inert material.



FIRE FIGHTING MEASURES of CONTRAM ST-2:
*Flash Point:
Not applicable.
*Extinguishing Media:
CO2, dry chemical, foam, water spray, water fog.



EXPOSURE CONTROLS/PERSONAL PROTECTION of CONTRAM ST-2:
-Other Exposure Limits:
None known.
-Engineering Controls:
Use material in well ventilated area only.
*Hand Protection:
If contact with the material may occur wear chemically protective gloves.
*Eye Protection:
Safety glasses.



HANDLING and STORAGE of CONTRAM ST-2:
*Pumping Temperature:
Not Determined.
Maximum Handling
Temperature:
Not Determined.
*Handling Procedures:
Keep containers closed when not in use.
Do not discharge into drains or the environment, dispose to an authorized waste collection point.
Use appropriate containment to avoid environmental contamination.
Wash thoroughly after handling.
Do not eat, drink or smoke when using this product.
*Maximum Storage:
Temperature:
Not Determined.
Storage Procedures:
No special storage precautions required.
Loading Temperature:
Not Determined.



STABILITY and REACTIVITY of CONTRAM ST-2:
*Stability:
Material is normally stable at moderately elevated temperatures and pressures.
*Decomposition Temperature:
Not Determined.
*Polymerization:
Will not occur.
*Thermal Decomposition:
Thermal decomposition and combustion are not expected to occur except under extreme conditions.



SYNONYMS:
5625-90-1
Dimorpholinomethane
N,N'-Dimorpholinomethane
4,4'-Methylenedimorpholine
4,4-Methylenedimorpholine
4-(morpholin-4-ylmethyl)morpholine
N,N'-Methylenebismorpholine
Morpholine, 4,4'-methylenebis-
bis(4-morpholinyl)methane
n,n'-methylene-bis-morpholine
MORPHOLINE, 4,4'-METHYLENEDI-
MFCD00023369
4,4'-Methylenebismorpholine
7O79DZW79Z
4-[(morpholin-4-yl)methyl]morpholine
Bismorpholino methane
Dimorpholinomethone
Bis(morpholino-)methan
EINECS 227-062-3
BRN 0111886
UNII-7O79DZW79Z
AI3-62944
bismorpholinomethane
Contram ST-1
methylenebismorpholine
bis(morpholino)methane
N,N\'-Dimorpholinomethane
4,4-methylene-bismorpholine
Oprea1_332757
4,4'-methanediyldimorpholine
N,N'-Methylene bismorpholine
4-27-00-00203 (Beilstein Handbook Reference)
SCHEMBL536772
DTXSID8052859
Bis(4-morpholinyl)methane, 98%
ZINC19324145
AKOS002314380
4,4'-METHYLENEBIS(MORPHOLINE)
FS-4049
AC-12628
SY032818
DB-052882
CS-0236719
FT-0629594
EN300-172423
Q865946
W-110051
F2163-0188
N,N'-DIMORPHOLINOMETHANE
4,4'-methylenedi-morpholin
4,4'-methylenedimorpholine
bis(morpholino-)methan
bismorpholinomethane
N,N'-Methylenebismorpholine
DIMORPHOLINOMETHANE
DIMORPHOLINOMETHONE
N,N'-DIMORPHOLINOMETHANE
4,4’-methylenedi-morpholin
4,4’-methylenedimorpholine
bis(morpholino-)methan
bismorpholinomethane
N,N’-Methylenebismorpholine
DIMORPHOLINOMETHANE
DIMORPHOLINOMETHONE
N,N'-Dimorpholinomethane
N,N´-Methylene bismorpholine
Bis (morpholino-) methan
Bismorpholino methane
4,4-Methylenedimorpholine
Morpholine, 4,4-methylenedi-
DIMORPHOLINOMETHONE
DIMORPHOLINOMETHANE
N,N-Dimorpholinomethane
MORPHOLINE44METHYLENEDI
BIS-(MORPHOLINE-)METHANE
44METHYLENEBISMORPHOLINE
Bis(4-morpholinyl)methane
N,N'-Methylenebismorpholine
4,4-methylenebis-Morpholine
N,N'-Methylenebismorpholine
Morpholine,4,4-Methylenebis-
4,4'-methanediyldimorpholine
Morpholine,4,4-methylenebis-
N,N'-Methylene-bis-morpholine
Methylene-bis-morpholine,N,N'-
N,N-Dimorpholinomethane
Morpholine,4,4-methylenebis-
Bis(4-morpholinyl)methane
N,N'-Methylenebismorpholine
4,4'-methanediyldimorpholine
4,4-methylenebis-Morpholine
N,N-Methylene-bis-morpholine
N,N-Dimorpholinomethane
Morpholine,4,4-methylenebis-
Bis(4-morpholinyl)methane
N,N'-Methylenebismorpholine
4,4'-methanediyldimorpholine
-bis-morpholine
4,4′-Methylenebis[morpholine]
4,4′-Methylenedimorpholine
4,4'-Dimorpholinylmethane
4,4'-Methylenebismorpholine
44METHYLENEBISMORPHOLINE
BIS-(MORPHOLINE-)METHANE
Bis(morpholino)methane
DIMORPHOLINOMETHANE
DIMORPHOLINOMETHONE
Methylenebismorpholine
Methylene-bis-morpholine,N,N'-
Morpholine, 4,4′-methylenebis-
Morpholine, 4,4′-methylenedi-
Morpholine,4,4-Methylenebis-
MORPHOLINE44METHYLENEDI
N,N′-Methylenebismorpholine;
N,N′-methylenebismorpholine
formaldehyde released from N,N′-methylenebismorpholine
N,N′-methylenebismorpholine
formaldehyde released by N,N′-methylenebismorpholine / MBM
DIMORPHOLINOMETHANE
N,N'-DIMORPHOLINOMETHANE
4,4’-methylenedi-morpholin
4,4’-methylenedimorpholine
bis(morpholino-)methan
bismorpholinomethane
N,N’-Methylenebismorpholine
DIMORPHOLINOMETHONE
Morpholine,4,4-Methylenebis-
Methylene-bis-morpholine,N,N'-
MORPHOLINE44METHYLENEDI
44METHYLENEBISMORPHOLINE
BIS-(MORPHOLINE-)METHANE
DIMORPHOLINOMETHONE
DIMORPHOLINOMETHANE
N,N-Dimorpholinomethane
MORPHOLINE44METHYLENEDI
BIS-(MORPHOLINE-)METHANE
44METHYLENEBISMORPHOLINE
Bis(4-morpholinyl)methane
N,N'-Methylenebismorpholine
4,4-methylenebis-Morpholine
N,N'-Methylenebismorpholine
Morpholine,4,4-Methylenebis-
4,4'-methanediyldimorpholine
Morpholine,4,4-methylenebis-
N,N'-Methylene-bis-morpholine
Methylene-bis-morpholine,N,N'-

Copper Dinitrate; Cupric Nitrate; cupric nitrate, n-hydrate; Nitric Acid, Copper (2+) salt; Kupferdinitrat; Dinitrato de cobre; Dinitrate de cuivre CAS NO:10031-43-3 (Trihydrate)

DESCRIPTION:
Copolyvidone used as dry binder in tablets, as matrix formers for amorphous solid dispersions
Copolyvidone is a white or slightly yellowish, free-flowing powder with a faint characteristic odor and practically no taste.
Copolyvidone readily dissolves in all hydrophilic solvents.


Solutions of more than 10 % concentration can be prepared in water, ethanol, isopropanol, methylene chloride, glycerol and propylene glycol.
Copolyvidone is less soluble in ether, cyclic, aliphatic and alicyclic hydrocarbons.


BENEFITS OF COPOLYVIDONE:
Copolyvidone provides erodible instant release matrix
Copolyvidone is a solubilizer, dispersant, crystallization inhibitor and matrix former
For direct compression, roller compaction and wet granulation, suitable for markets with higher humidity exposure

Copolyvidone has excellent stability throughout the extrusion process
A coarse powder provides a dust free handling, good flowability and faster extruder feeding
Recently obtained GRAS/SA status (Generally Recognized As Safe/Self-Affirmed) by the U.S. Food & Drug Administration (FDA) for use in food and nutritional supplements e.g. vitamin and mineral tablets

Copolyvidone is a vinylpyrrolidone-vinyl acetate copolymer that is soluble both in water and in alcohol.
Copolyvidone is used as a dry binder in tabletting, as a granulating auxiliary and as a film-forming agent in the pharmaceutical industry.



SAFETY INFORMATION ABOUT COPOLYVIDONE:
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

DESCRIPTION:
Copovidone is co-polymer made by N-vinyl-2- pyrolidone and vinyl acetate.
Copovidone is used for coating agent or binder.
Copovidone is insoluble in water, so dimethyl formamide (DMF) was used as the eluent.


CAS Number: 25086-89-9



SYNONYMS OF COPOVIDONE:
Poly(1-vinylpyrrolidone-co-vinyl acetate), Copovidone K25-31,Copovidone K26-29,Copovidone K28,D9C330MD8B,Plasdone-S630,Acetic Acid Ethenyl Ester Polymer with 1-Ethenyl-2-Pyrrolidone,COPOLYMER OF 1-VINYL-2-PYRROLIDONE AND VINYL ACETATE IN THE MASS PROPORTION OF 3:2 (MW=40000),COPOVIDONE (EP IMPURITY),COPOVIDONE (EP MONOGRAPH),COPOVIDONE (MART.),COPOVIDONE (PLASDONE-S630),COPOVIDONE (USP-RS),NSC-114023,NSC-114024,NSC-114025,NSC-114026,POLYVINYLPYRROLIDONE/VINYL ACETATE COPOLYMER,POVIDONE/VINYL ACETATE COPOLYMER,VP/VA COPOLYMER, Copovidone; Copolyvidone; Vinylpyrrolidone-vinyl acetate copolymer; Copolymer of 1-vinyl-2-pyrrolidone and vinyl acetate in a ratio of 3:2 by mass; Copolyvidone; Poly (1-vinylpyrrolidone-co-vinyl acetate); Polyvinylpyrrolidone-vinyl Acetate Copolymer; PVP/VA; PVP/VA Copolymer; Kollidon VA 64; Plasdone® Crospovidone,Copovidone [BAN:NF],D9C330MD8B,25086-89-9,Acetic acid ethenyl ester, polymer with 1-ethenyl-2-pyrrolidinone,Copovidone,Vinyl acetate N-vinyl-pyrrolidone polymer,Poly(vinylpyrrolidone-co-vinyl-acetate),UNII-D9C330MD8B,Ethenyl acetate, polymer with 1-ethenyl-2-pyrrolidinone,GAF-S 630,Ganex E 535,Vinyl acetate-N-vinylpyrrolidone copolymer,Vinyl acetate-N-vinyl-2-pyrrolidone copolymer,Vinyl acetate-vinylpyrrolidone polymer,Vinyl acetate-N-vinylpyrrolidone polymer,Vinyl acetate-vinylpyrrolidone copolymer,Gantron S 630,Gantron S 860,Gantron PVP,Luviskol VA 28I,Luviskol VA 37E,Luviskol VA 37I,Luviskol VA 55E,Luviskol VA 55I,Luviskol VA 64,Luviskol VA 73E,NSC 114023,Polectron 845,PVP-VA,PVP-VA-E 735,Kolima 10,Kolima 35,Kolima 75,Kollidon VA 64,Vinyl acetate-1-vinyl-2-pyrrolidinone polymer,Vinyl acetate-N-vinyl-2-pyrrolidinone copolymer,Vinyl acetate-vinylpyrrolidinone polymer,Vinyl acetate-N-vinylpyrrolidinone polymer,Vinylpyrrolidinone-vinyl acetate copolymer,Vinylpyrrolidinone-vinyl acetate polymer,Vinylpyrrolidone-vinyl acetate copolymer,1-Vinyl-2-pyrrolidone-vinyl acetate copolymer,Vinylpyrrolidone-vinyl acetate polymer,N-Vinylpyrrolidone-vinyl acetate polymer,PVP/VA-S 630,PVP/VA copolymer,2-Pyrrolidinone, 1-ethenyl-, polymer with ethenyl acetate,Vinyl acetate-vinylpyrrolidinone copolymer,Vinyl acetate-N-vinylpyrrolidinone copolymer,I 635,I 735,S 630,Acetic acid vinyl ester, polymer with 1-vinyl-2-pyrrolidinone,Copolyvidon,E 335,E 535,I 535,Acetic acid, ethenyl ester, polymer with 1-ethenyl-2-pyrrolidinone,1-Ethenyl-2-pyrrolidinone, polymer with acetic acid ethenyl ester,1-Ethenyl-2-pyrrolidinone, polymer with ethenyl acetate,Polyvinylpyrrolidone - vinyl acetate copolymer,NSC 114024


Copovidone is used as a binder, hardener, a film-former, and as part of a proprietary blend used in controlled-release formulations of tablets and other products.
In tableting, copovidone can be used as a binder for direct compression of tablets, increasing their hardness and as a binder in wet granulation of tablets.

Copovidone is often added to coating solutions as a film-forming agent.
Copovidone provides good adhesion, elasticity, and hardness, and can be used as a moisture barrier.


Copovidone can be used as an excipient, such as Film formers, adhesives, etc.
Pharmaceutical excipients, or pharmaceutical auxiliaries, refer to other chemical substances used in the pharmaceutical process other than pharmaceutical ingredients.

Pharmaceutical excipients generally refer to inactive ingredients in pharmaceutical preparations, which can improve the stability, solubility and processability of pharmaceutical preparations.
Pharmaceutical excipients also affect the absorption, distribution, metabolism, and elimination (ADME) processes of co-administered drugs.



In this application, Even though DMF is used as the eluent, adding lithium bromide into the eluent is effective.
Lithium bromide was added for analyzing copovidone.

Copovidone, an analog of povidone, is used as a tablet binder, a film-former, and as part of the matrix material used in controlled-release formulations.

In tableting, copovidone can be used as a binder for direct compression and as a binder in wet granulation.
Copovidone is often added to coating solutions as a film-forming agent.
Copovidone provides good adhesion, elasticity, and hardness, and can be used as a moisture barrier.


Copovidone has better plasticity than povidone as a tablet binder, is less hygroscopic, more elastic, and better for film-forming applications than povidone.
Copovidone is also used in cosmetics as a thickener, dispersant, lubricant, film-forming agent and binder.
Copovidone is widely used in the food, cosmetic and pharmaceutical industry.


Copovidone is generally regarded as nontoxic. However, oral consumption of excessive quantities may produce stomach upset.

Copovidone has not been shown to be sensitizing to the skin.
Animal studies in rats and dogs do not show significant toxicity with high dietary levels.
The average molecular weight of copovidone is usually expressed as a K-value and it ranges between 45 and 70.




BENEFITS OF COPOVIDONE:
Copovidone has Diverse range of low to high molecular weight povidones
Copovidone Includes highly effective water soluble binders resulting in coarse and strong granules
Copovidone Consists of standard and micronized grade super-disintegrants and dissolution enhancers to address solubilization challenges


Copovidone has Instant release and sustained release profiles
Copovidone has Versatile processing options including direct compression, roller compaction, and wet granulation
Copovidone is Suitable for a broad range of applications


Copovidone has Low sensitivity to lubricant
Copovidone has High Plasticity, makes robust tablets
Copovidone has Low Hygroscopicity

APPLICATIONS OF COPOVIDONE IN PHARMACEUTICAL FORMULATIONS OR TECHNOLOGY:
Copovidone was developed as an improvement over Povidone (binder).
Its favourable technical properties, namely better flowability, lower hygroscopicity, spherical particle shape, plasticity, lower glass-transition temperature, and hydrophobic–hydrophilic balance, rendered Copovidone highly advantageous in direct compression and roller-compaction tabletting operations.

While Copovidone is still used as a dry binder (for direct compression and roller compression), its main utility is as a matrix former for the development of solid dispersions, film former (especially in the formulation of moisture-barrier coatings), and as a matrice former for sustained-release solid dosage forms.

1). Binder in Tablets :
Copovidone performs superbly as a dry binder for direct compression applications.
It is particularly preferred for formulations susceptible to capping due to its plasticity.

Finer grades have demonstrated superior binding performance compared with either Povidone and Cellulose-based polymers.
Formulations developed with Copovidone show a direct relationship between tablet hardness, friability, porosity and disintegration with the applied compaction force.


2). Binder in Wet Granulation:
The high solubility of Copovidone in water and standard granulation liquids makes it as an ideal binder in wet granulation operations.
It may be added either as a solution or in the form of a dry powder followed by the addition of the granulating solvent or a combination of both.

Copovidone, owing to its low hygroscopicity, allows greater predictable granulation endpoints and its granules have a much less propensity to stick to tooling, even when conducted under less favourable conditions.


3). Roller Compression:
Copovidone has been shown to be particularly well-suited for use in roller compaction.
It is an excipient of choice when particle size distribution and particle shape considerations are critical during roller compression process design.

Owing to its spherical shape and fine size Copovidone gives better surface coverage and develops multiple bridges that lead to hard tablets with a reduced friability.

4). Film-Coating Film Former:
Copovidone is a film former and it soluble membranes whose solubility is independent of pH.
Copovidone films are also less hygroscopic, but more flexible compared with those formed by Povidone.

For best results, it’s used in combination with other film-forming polymers that are less hygroscopic.
Due to its flexibility, a plasticizer is not required.


5). Polymer for Amorphous Solid Dispersions:
Copovidone is a suitable polymer for developing amorphous solid dispersions that are both kinetically and thermodynamically stable.
Both spray-drying and hot melt extrusion approaches can be reliably used.

6). Other Uses:
Inhibition of crystallisation of APIs in liquid soft-gel formulations
Sugar coating applications (to improve adhesion)
Subcoating of tablets (film coating)






CHEMICAL AND PHYSICAL PROPERTIES OF COPOVIDONE:
Chemical Name, Acetic acid ethenyl ester, polymer with 1-etheny1-2 pyrrolidinone
CAS Registry Number, [25086-89-9]
Empirical Formula, (C6H9NO)n (C4H6O2)m (111.1)n + (86.1)mThe ratio of n to m is approximately n = 1.2m
Molecular Weight, Molecular weights of 45,000-70,000 have been determined for Koliidon VA 64. The average molecular weight of Copovidone is usually expressed as a K-value.The K-value of Kollidon VA 64 is nominally 28, with a range of 25.2-30.8. The K-value of Plasdone® S 630 is specified between 25.4 and 34.2. K-values are calculated from the kinematic viscosity of a 1% aqueous. Molecular weight can be calculated with the formulaM = 22.22 (K + 0.075K2)1.65The Ph.Eur and USP-NF describe Copovidone as a copolymer of 1-ethenylpyrrolidin-2-one and ethenyl acetate in the ratio (by mass) of 3:2

EINECS Number, 607-540-1
FDA UNII Code, D9C330MD8B
Physical form, Solid, powder
Appearance, White, cream to yellowish finely divided powder
pH value, 3.0-7.0
pKa, -1.4 (Computed)
Log P, -1.1
Bulk density, Standard grades: 0.20-0.30 g/mlFine grades: 0.08-0.15 g/ml
Tapped density, Standard grades: 0.30-0.45 g/ml
Density (true), 1.1 g/ml
Flashpoint, 215 0C
Flowability, Poorly flowing to relatively free-flowing powder
Glass transition temperature, 100 – 110 0C
Hygroscopicity, Absorbs <10% weight at 50% RH
K-value -630, Dependent on the supplier/grade. For Plasdone®, K value = 25 – 35
Melting point, 140 0C
Solubility, Soluble in water (179g/l). Soluble in ethanol, isopropyl alcohol, propylene glycol and glycerol (a 10% w/w solution can be easily prepared)
Viscosity (Brookfield), Viscosity of aqueous solutions varies with concentration and molecular weight of the polymer. A 5% w/v solution has a viscosity of 4-5 mPas (25 oC)


SAFETY INFORMATION ABOUT COPOVIDONE:
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

(2S)-2-[[(2S)-2-[[(2S)-2-[[(2-methylpropan-2-yl)oxy-oxomethyl]amino]-1-oxopropyl]amino]-1-oxopropyl]amino]-3-[4-(2-oxiranylmethoxy)phenyl]propanoic acid ethyl ester; bis(1-hydroxy-1h-pyridine-2-thionato-o,s)copper 2(; Bis(1-hydroxy-1H-pyridine-2-thionato-O,S)copper; Copper omadine; Omadine Copper; Copper Pyritione; Copper Pyrithione(CuPT); Copper 2-pyridinethio-1-oxide CAS NO:14915-37-8

Copper Carbonate is an inorganic compound having the chemical formula CuCO3.
The chemical name of Copper Carbonate is copper(II) carbonate hydroxide, and it is an alkaline compound.


CAS Number: 12069-69-1
EC Number: 235-113-6
Chemical formula: CuCO3


Copper Carbonate is a powdery green solid.
Copper Carbonate is insoluble in water, alcohol and organic solvents while it decomposes in the presence of diluted acids.
Copper Carbonate is an inorganic compound having the chemical formula CuCO3.


The chemical name of Copper Carbonate is copper(II) carbonate hydroxide, and it is an alkaline compound.
Copper Carbonate exists as a green colour crystalline solid substance in nature.
Copper Carbonate occurs as the malachite mineral compound.


Due to its colour, Copper Carbonate is important mainly as a pigment for colour formation.
When a copper atom loses one or two of its electrons it forms positively charged ions known as Cu+1 and Cu+2.
Whilst ordinary copper carbonate contains cupric ion (or Cu+2), it may sometimes contain a chemically similar alkaline component.


Copper Carbonate can actually serve a number of applications around industry and life in general; you probably haven’t realized how many purposes it is utilized in today.
Copper Carbonate is a water insoluble chemical created when copper loses the electrons in its outermost shell.


Also known as copper (II) carbonate, carbonic acid, and copper monocarbonate, Copper Carbonate converts quickly to copper salts.
Most commonly, the term of Copper Carbonate or cupric carbonate is referred to as a basic copper carbonate like Cu2(OH)2CO3.
This occurs in nature in the form of the mineral malachite or Cu3(OH)2(CO3)2 which is azurite.


It is because of this reason that the qualifier neutral can be utilized in place of basic which refers particularly to Copper Carbonate.
As with other metallic colouring carbonates, Copper Carbonate is green in colour and bulkier than the oxide form, thus it tends to disperse better to give more even results.


Copper Carbonate is also more reactive chemically and thus melts better.
As such, Copper Carbonate is ideal for use in brush work where minimal speck is required.
However Copper Carbonate produces gases as it decomposes and these can cause pinholes or blisters in glazes.


Also the carbonate form contains less copper per gram, therefore colours are less intense than the oxide form.
Copper Carbonate is a powdery green solid.
Copper Carbonate is insoluble in water, alcohol and organic solvents while it decomposes in the presence of diluted acids.


Copper Carbonate and cupric carbonate basic are actually not presented.
The addition of sodium carbonate to the dilute copper sulfate solution, or the introduction of carbon dioxide into the suspension of copper hydroxide can both give the precipitate of cupric carbonate basic.


Cupric carbonate basic can be seen as consisting of the copper hydroxide and Copper Carbonate.
Actually there are two types of copper hydroxides with both combination with one Copper Carbonate and two copper carbonates.
Copper Carbonate is a chemical compound, more properly called copper(II) carbonate hydroxide.


Copper Carbonate is an ionic compound (a salt) consisting of the ions copper(II) Cu2+, carbonate CO2−3, and hydroxide OH−.
The name most commonly refers to Copper Carbonate with formula Cu2CO3(OH)2.
Copper Carbonate is a green crystalline solid that occurs in nature as the mineral malachite.


Both malachite and azurite can be found in the verdigris patina that is found on weathered brass, bronze, and copper.
The composition of the patina can vary, in a maritime environment depending on the environment a basic chloride may be present, in an urban environment basic sulfates may be present.


Copper Carbonate is often improperly called (even in chemistry articles) copper carbonate, cupric carbonate, and similar names.
The true (neutral) copper(II) carbonate CuCO3 is not known to occur naturally.
Copper Carbonate is decomposed by water or moisture from the air, and was synthesized only in 1973 by high temperature and very high pressures.


Copper Carbonate is the common name for the green crystalline cupric carbonate, in which copper has valence +2.
Copper Carbonate is soluble in water and decomposes at 200 C.
Normal cupric carbonate is not commonly available and the abbreviated term ‘Copper Carbonate’ is widely used to describe either of the two basic copper carbonates, the green malachite (CuCO3.Cu(OH)2), the blue azurite (2CuCO3.CU(OH)2), or a mixture of the two.


Copper Carbonate is the green malachite variety and is supplied as a fine powder.
Copper Carbonate (CuCO3) is formed after copper loses its electrons.
Copper Carbonate typically contains Cu + 2, known as the cupric ion.


However, at times Copper Carbonate may have an alkaline component as the content.
Copper carbonate is a water-insoluble chemical compound.
Copper Carbonate can be converted into other copper compounds by different methods such as calcination, where on the application of heat, the chemical compound gives oxide.


Copper Carbonate is a neutral compound with the chemical formula CuCO3.
Therefore, Copper Carbonate is also known as Cupric Carbonate.
The Copper ions in the compound are available in a +2 Oxidation state which allows it to be reactive to water or moisture.


Therefore, the mixture is easily convertible to other compounds on heat, also referred to as Calcination.
The preparation is difficult and is a reaction between Sodium Carbonate and Copper Sulfate.
In the preparation method, the Copper Carbonate is heated in a Carbon Dioxide Atmosphere to give a grey powder as the output, which is the Copper Carbonate.


The final product is very stable due to the partial pressure created by the Carbon Dioxide in the environment.
The stability can be maintained for months in a dry atmosphere.
Once Copper Carbonate starts to decompose, it gives Copper Oxide one of the significant products.


Copper Carbonate is found in blue and green coloured crystalline forms known as Azurite and Malachite.
Copper Carbonate contains Copper ions and carbonate anions and has the formula CuCO3.
Copper Carbonate is derived in powder form in grey color.


Copper Carbonate can be derived in two different colors: blue and green.
Copper (Cu) is one of the elements that was never discovered.
They have been a part of every stage in the evolution of civilization.


The metal has been utilized for so long that it can be found isolated as a pure element.
One may be tunneling in a mine and come find pure copper in a variety of forms.
It is the 29th element in the periodic table, denoted by the symbol ‘Cu’ from the Latin term ‘cuprum.’


Copper is a soft but strong metal.
It combines easily with other metals to make alloys such as bronze and bronze.
Bronze is a tin-copper alloy, whereas brass is a zinc-copper alloy.


Copper and brass can be recycled quickly.
Perhaps 70% of the copper that is now in use has been recycled at least once.
Copper has a density of 8.96 and an atomic number of 29.


Copper has been an important element of human culture for thousands of years.
Silver, gold, copper, and iron have all been used in some way.
Copper Carbonate is another name for Copper II Carbonate.


Furthermore, Copper Carbonate is a chemical substance.
Copper Carbonate is also an ionic solid compound composed of copper (II) cations Cu2+ and carbonate anions CO2-3.



USES and APPLICATIONS of COPPER CARBONATE:
Copper Carbonate can be used as a dietary ingredient and as a nutrient.
Copper aids in the absorption of iron, in the formation of red blood cells and the proper bone formation and maintenance.
Copper Carbonate is used in pyrotechnics, pesticides, pigments, feed, fungicides, antiseptics and other industries and the manufacture of copper compounds


Copper Carbonate is used as analytical reagent and insecticide
Copper Carbonate is used in industries such as catalysts, pyrotechnics, pesticides, pigments, feeds, fungicides, electroplating, anticorrosion, and the manufacture of copper compounds.


Copper Carbonate is a green solid completely insoluble in water, alcohol and organic solvents.
Copper Carbonate decomposes if placed in contact with diluted acids.
Also known as green malachite, Copper Carbonate was used as a fungicide since the beginning of the nineteenth century, although it has now been replaced by other copper compounds.


Copper Carbonate is used as raw material in the electroplating and agricultural industries.
Copper Carbonate is also used for the production of pigments and as raw material used in wood protective formulations.
Copper Carbonate is used as seed treatment fungicide; in pyrotechnics; as paint and varnish pigment; in animal and poultry feeds; in sweetening of petrol sour crude stock; in manufacture of other Cu salts.


The term Copper Carbonate or cupric carbonate is most usually used to refer to a Copper Carbonate such as CuCO3.
This can be found in nature in the form of the mineral malachite or the azurite mineral Cu3(OH)2(CO3)2.
As a result, the qualifier neutral can be used in place of basic, which specifically refers to Copper Carbonate.


Copper Carbonate is used as a blue flame colorant in low temperature class compositions of the potassium (per)chlorate base or in compositons of the ammonium perchlorate base.
Copper Carbonate helps with the creation of many products, as well as helping along the scientific process.


Laboratories: Copper Carbonate catalyzes copper chromite, which breaks down fatty methyl esters in the production of fatty alcohols.
Paints: In artist’s palettes, Copper Carbonate creates the sought-after colors verditer and mountain green.
Petroleum: Adding nitric acid to Copper Carbonate produces copper chloride, important in the process of “oil sweetening”, or purifying oil of its sulfur components.


Pyrotechnics: Companies manufacturing fireworks use Copper Carbonate for a stellar blue sparkle to pyrotechnic displays.
Copper Carbonate is used in paint and varnish pigments, pyrotechnics and animal and poultry feeds.
Copper Carbonate is also used as a fungicide.


Pigment for paints and ceramics - Copper Carbonate is used in pigments under the names mountain green, mineral green or verdeazzuro (green azure).
While Copper Carbonate is not routinely used in modern bulk paints, it is still desired for restoration and artists’ paints.
Ceramics and pottery applications call for Copper Carbonate in slips (2-8%) and glazes (<5%, if more than 5% is added, glazes often change to a metallic pewter).


The pigment will normally give a green colour when fired, but alkaline glazes will create a turquoise, and reds are achievable with a reduction kiln.
Copper Carbonate is not suitable for soluble glazes that will come into contact with food or drink as the copper can leach out.
Pyrotechnic flame colourant - Copper Carbonate is often used as a blue flame colourant, sometimes written in formulations as Basic Copper Carbonate.


Copper carbonate is added to arsenic to produce acetoarsenite, which is popularly known as Paris green.
Copper Carbonate is used as a wood preservative.
Copper carbonate is actively used as an ingredient in animal feeds and is demanded continuously in animal fodder.


Fertilizer is the other product where the demand for copper carbonate is very high.
Copper Carbonate is used to create different pesticides, insecticides, and fungicides.
Acetoarsenite is used as an insecticide.


Besides agriculture, aquaculture is also one of the major application areas.
Copper Carbonate is used in controlling the unnecessary spreading of weeds.
Copper Chromite is very active for the hydrogenation of aldehydes and ketones to their corresponding alcohols, as well as nitro-compounds to the primary amines.


Some applicators use Copper Oxide Black instead of Copper Carbonate to reduce reaction rate and control synthesis in the reactor.
Copper carbonate is commercially used for veterinary applications.
While high concentration can be toxic to humans, in minimal quantities, it is used in cosmetics.


From the food industry to pharmaceutical products, copper carbonate is used in a wide variety of applications.
Copper Carbonate is used in the timber industry as a wood preservative and other products.
Copper Carbonate is also used in making pigments and feed additives.


Copper Carbonate is primarily used in paints as pigments for its varied color.
Copper Carbonate is also used in gemstones.
Copper carbonate is used in several applications.


Copper Carbonate is subjected to different refining processes as pigments in paint.
Copper Carbonate can be developed by combining Sodium Carbonate and Copper Sulphate in an aqueous form.
The other way of deriving Copper Carbonate is using Copper Sulfate with Sodium Bicarbonate.


Copper Carbonate has many applications owing to its vibrant colors.
Copper Carbonate is also used in copper chrome catalyst manufacturing.
Both malachite and azurite, as well as synthetic Copper Carbonate have been used as pigments.


One example of the use of both azurite and Copper Carbonate's artificial form blue verditer is the portrait of the family of Balthasar Gerbier by Peter Paul Rubens.
The green skirt of Deborah Kip is painted in azurite, smalt, blue verditer (artificial form of azurite), yellow ochre, lead-tin-yellow and yellow lake.


The green color is achieved by mixing blue and yellow pigments.
Copper Carbonate has also been used in some types of make-up, like lipstick, although it can also be toxic to humans.
Copper Carbonate also has been used for many years as an effective algaecide.


In organic salt industry, Copper Carbonate is used for preparation of various copper compound; in organic industry.
Copper Carbonate is used as catalyst of organic synthesis.
In electroplating industry, Copper Carbonate is used as copper additive.


In recent years, Copper Carbonate has been widely applied in wood preservation field.
Copper Carbonate has been used since antiquity as a pigment, and it is still used as such in artist paints, sometimes called verditer, green bice, or mountain green.


Sometimes the name is used for Cu3(CO3)2(OH)2, a blue crystalline solid also known as the mineral azurite.
Copper Carbonate too has been used as pigment, sometimes under the name mountain blue or blue verditer.


-Aesthetic and Practical uses of Copper Carbonate:
Copper Carbonate has a number of aesthetic purposes, most notably in jewellery.
Copper Carbonate can also be converted into the metal version of copper, which is highly valuable and serves a number of its own applications.
This is achieved through a process of pulverization, sizing, conversion and electrolysis.


-Copper Salts uses of Copper Carbonate:
Copper Carbonate can be converted into copper salts by mixing it with a stronger acid.
The resulting salt, Copper Carbonate is complemented with water and carbon dioxide gas.
Mixing the carbonate with acetic acid (otherwise known as vinegar) will produce cupric acid, water and carbon dioxide.


-Pigments and Colorants uses of Copper Carbonate:
Copper Carbonate, when pure, should have a mint green colour.
When alkaline components have been added, a tinge of blue will be added to the colour.
Copper Carbonate is often added to paints, varnishes, pottery glazes and even fireworks to impart some of the colour.


-Miscellaneous uses of Copper Carbonate:
Small amounts of copper carbonates are used in a variety of animal feeds and fertilizers.
Copper Carbonate also plays a major role in the creation of pesticides and fungicides.

Copper Carbonate can also be used to control the growth and spread of aquatic weeds.
Copper Carbonate is also a common ingredient in the ammonia compounds that are used to treat timber.
As you can see, copper carbonate has a number of uses across a wide variety of industries and products.


-Agriculture uses of Copper Carbonate:
Copper Carbonate is used frequently in fertilizer as well as in fungicides, insecticides, pesticides — where it acts as an anti-pathogenic — and in aquaculture where it controls unwanted foliage.

Rather than adding copper carbonate to fertilizer, manufacturers may add this important nutrient, Copper Carbonate, to the seeds as they are packaged.
The cost of Copper Carbonate at this point is significantly lower than adding it to soil, reducing overall expenses.
Animal feed, specifically poultry and ruminant feed, often has added Copper Carbonate since these animals rely on copper as a supplemental nutrient.


-Woodworking and Ceramics uses of Copper Carbonate:
Micronized copper wood treatment consists of tiny Copper Carbonate particles suspended in a final treatment solution (often containing ammonia) for preserving wood and timber.
Copper Carbonate also helps with ceramic products.

Before ceramics are fired, a glaze is often added to retain color and give a finished look to the product.
Adding Copper Carbonate to the glaze creates a seafoam sheen to the ceramic.
Applying Copper Carbonate plus an alkaline generates a bluer hue.


-Agriculture and aquaculture uses of Copper Carbonate:
Copper carbonate is used across a wide range of applications.
Copper Carbonate is commonly used to develop compounds for the treatment of timber.


-Drilling Fluids uses of Copper Carbonate:
A compound, Copper Carbonate, that was used as a sulfide scavenger for water-base muds.
However, Copper Carbonate was found to be corrosive due to spontaneous plating of metallic copper onto metal surfaces, causing pitting corrosion; it has largely been replaced by zinc compounds.



PHYSICAL PROPERTIES OF COPPER CARBONATE:
Copper Carbonate is a powdery blue-green compound that is insoluble in water.
Copper Carbonate's color can be different shades of blue or green depending on the purity and the presence of other basic copper carbonates, which are usually present in any technical grade samples.



CHEMICAL PROPERTIES OF COPPER CARBONATE:
Copper Carbonate, like copper(II) hydroxide, is used as a source of copper(II) ions.
Most salts of copper can be produced by reacting this chemical with the desired acid.
Copper Carbonate keeps well, so it is often kept in larger amounts, and not just made when needed.
This is very unlike iron(III) carbonate and iron(II) carbonate, which decompose to iron oxides and carbon dioxide.
Heating of copper(II) carbonate yields copper(II) oxide (CuO) and carbon dioxide.



CHEMICAL PROPERTIES AND PHYSICAL PROPERTIES OF COPPER CARBONATE:
The stability of dry Copper Carbonate is dependent significantly on the partial pressure of carbon dioxide (pCO2).
Copper Carbonate can remain stable for months in dry air but will decompose slowly into CuO and CO2 if pCO2 is less than 0.11 atm.

In the company of water or moist air at 25 °C, Copper Carbonate is constant only for pCO2 above 4.57 atmospheres and pH between about 4 and 8.
Further, below that partial pressure, Copper Carbonate reacts with water to make a very basic carbonate (azurite, Cu3(CO3)2(OH)2).

3 CuCO3 + H2O → Cu3(CO3)2(OH)2 + CO2
In highly basic solutions, the complex anion Cu(CO3)22− is formed as an alternative.



PREPARATION OF COPPER CARBONATE:
Sodium Carbonate and Copper Sulfate combination give Copper Carbonate.
For Copper Carbonate, heat is applied to Copper Carbonate in the Carbon Dioxide Atmosphere.



COPPER CHROMITE CATALYSTS MANUFACTURING, COPPER CARBONATE:
Copper Carbonate is used in manufacturing Copper Chromite catalysts.
The largest field (industrial scale) of applying copper chromite catalysts is the hydrogenolysis of fatty methyl esters in fatty alcohol production.



AVAILABILITY OF COPPER CARBONATE:
Pottery stores that sell various oxides and carbonates usually sell Copper Carbonate.
It is almost always a mix of Copper Carbonates in various states of hydration.
This is generally not an issue for chemistry but may interfere with stoichiometry calculations.



PROPERTIES OF COPPER CARBONATE:
Copper Carbonate is in peafowl green color.
And Copper Carbonate is fine particle powder; density: 3.85; melting point: 200°C; insoluble in cold water, alcohol; soluble in acid,
cyanide, sodium hydroxide, ammonium salt.



DIFFERENCE BETWEEN COPPER CARBONATE AND BASIC COPPER CARBONATE:
Copper carbonate and basic copper carbonate are important ionic compounds.
The key difference between copper carbonate and basic copper carbonate is that copper carbonate is a neutral chemical compound, whereas basic copper carbonate is an alkaline chemical compound.
Moreover, copper carbonate is a grey powder, whereas basic copper carbonate is a blue-green powder.
In addition, copper carbonate is made of copper ions and carbonate anions, while basic copper carbonate is made of copper ions, hydroxide ions, and carbonate ions.



PREPARATION OF COPPER CARBONATE:
Copper Carbonate is prepared by combining aqueous solutions of copper(II) sulfate and sodium carbonate at ambient temperature and pressure.
Copper Carbonate precipitates from the solution, with release of carbon dioxide CO2:

2 CuSO4 + 2 Na2CO3 + H2O → Cu2(OH)2CO3 + 2 Na2SO4 + CO2
Copper Carbonate can also be prepared by reacting aqueous solutions of copper(II) sulfate and sodium bicarbonate at ambient conditions.
Copper Carbonate precipitates from the solution, again with release of carbon dioxide:

2 CuSO4 + 4 NaHCO3 → Cu2(OH)2CO3 + 2 Na2SO4 + 3 CO2 + H2O
Copper(II) sulfate may also be substituted with Copper(II) chloride, creating Sodium chloride (NaCl) as a byproduct instead of Sodium sulfate (Na2SO4), both of which are soluble in water.



REACTIONS OF COPPER CARBONATE:
Copper Carbonate is decomposed by acids, such as solutions of hydrochloric acid HCl, into the copper(II) salt and carbon dioxide.
In 1794 the French chemist Joseph Louis Proust (1754–1826) thermally decomposed Copper Carbonate to CO2 and CuO, cupric oxide.
The Copper Carbonates, malachite, and azurite, both decompose forming H2O, CO2, and CuO, cupric oxide.



PREPARATION OF COPPER CARBONATE:
Copper Carbonate can be made by reacting copper(II) salts with a carbonate or bicarbonate salt.
This is most easily done by mixing saturated solutions of copper(II) sulfate and either sodium carbonate or sodium bicarbonate.
Carbonates are preferred because they do not emit carbon dioxide when added to solution.
This process yields Copper Carbonate, which is blue and includes additional hydroxide ions.
Copper Carbonate is also produced when copper(II) hydroxide reacts with carbon dioxide in the air.



SYNTHESIS OF COPPER CARBONATE:
Method 1:
Dissolve a soluble copper compound (Copper acetate, Copper (II) chloride, or Copper sulfate for example) in as little distilled water as possible.
Make a seperate solution of Sodium carbonate or Sodium bicarbonate in as little distilled water as possible.

Mix these two solutions slowly and Copper Carbonate will precipitate out.
(if you are using Sodium bicarbonate there will be a lot of fizzing) Filter, wash with distilled water, and allow to dry without heating Copper Carbonate. (sunlight is OK)


Method 2:
Add Copper hydroxide to Carbonic acid (tonic water) and Copper Carbonate will precipitate out.
Filter, wash with distilled water, and allow to dry without heating Copper Carbonate. (sunlight is OK)



WHAT IS THE DIFFERENCE BETWEEN COPPER CARBONATE AND BASIC COPPER CARBONATE:
The key difference between copper carbonate and basic copper carbonate is that copper carbonate is a neutral chemical compound, whereas basic copper carbonate is an alkaline chemical compound.
Copper carbonate and basic copper carbonate are important ionic compounds.
Copper carbonate is an inorganic chemical compound having the chemical formula CuCO3, while basic copper carbonate is an inorganic compound having the chemical formula Cu2(OH)2CO3.



PREPARATION OF COPPER CARBONATE:
It is generally expected of reactions like mixing solutions of Copper II sulfate CuSO4 and sodium carbonate Na2CO3 in ambient conditions to produce Copper Carbonate, but instead, it produces a basic carbonate and CO2 because of the great attraction of the Cu2+ ion for the hydroxide anion HO−
When the basic carbonate thermally decomposes at atmospheric pressure, it produces Copper (II) oxide CuO instead of the carbonate.
W. F. T. Pistorius in the year, 1960, claimed synthesis.

He did so when he heated Copper Carbonate at 180 °C in an atmosphere containing carbon dioxide, CO 2(450 atm) and water (50 atm) up to 36 hours.
The majority of these products came out to be well-crystallized malachite Cu2CO3(OH)2, however, there was also a small quantity of the rhombohedral substance in the result which was claimed as Copper Carbonate.

But, it is important to note that this synthesis was actually not reproduced.
If we look at the origin, we will see that the reliable synthesis of true Copper (II) carbonate was testified for the first time in 1973 by Hartmut Ehrhardt and others.

Thus, Copper Carbonate was acquired in the form of gray powder.
It was after they heated Copper Carbonate in an atmosphere containing carbon dioxide (which we produce by decomposing silver oxalate Ag 2C2O 4) at 500 °C and 2 GPa (20,000 atm).
Copper Carbonate was said to have a monoclinic structure.



METALS AND SALT CONVERSIONS OF COPPER CARBONATE:
Copper carbonate is very commonly used to convert the compound into copper salts.
In the process, the mixture is first treated with a more vital acid.
In the next step, water along with the carbon dioxide gas is added.

Vinegar, known as acetic acid, is mixed with carbonate to produce water, cupric acid, and carbon dioxide.
Copper Carbonate is also used for various aesthetics and practical purposes.
One of the prominent application areas of Copper Carbonate is jewelry.

The metal conversion of Copper Carbonate is highly sought after in the industry.
Copper Carbonate is precious and has numerous applications.
Several processes are used to obtain the desired result, such as pulverization, conversion, sizing, and electrolysis.



COLORING PIGMENT, COPPER CARBONATE:
Owing to the specific color of different compounds, they are used as colorants and pigments.
In pure form, the combination is of mint green color.
A tinge of blue is obtained after the addition of alkaline components. These colors act as great coloring agents.

They are used as a pigment in products, paints, and varnishes.
Copper carbonate is used in artist paints to obtain desired colors for which it is also known with different names such as verditer and mountain green.
Copper carbonate is highly demanded in fireworks and pottery glazes as pigment and colorant.



METHODS OF MANUFACTURING OF COPPER CARBONATE:
*Copper sulfate method:
Reaction equation: 2CuSO4+4NaHCO3→CuCO3·Cu(OH)2+2Na2SO4+3CO2↑+H2O Operation method: mix baking soda into a solution with a relative density of 1.05, add it to the reactor first, and add it under stirring at 50℃ Refined copper sulfate solution, the reaction temperature is controlled at 70 ~ 80 ℃, the reaction changes from precipitation to malachite green, the pH value is maintained at 8, after the reaction is allowed to stand and settle, use 70 ~ 80 ℃ water or deionized water Wash until the washing liquid is free of SO2-4, and then centrifugal separation and drying to obtain the finished Copper Carbonate.

*Copper nitrate method:
Reaction equation: Cu+4HNO3→Cu(NO3)2+2NO2↑+2H2O2Cu(NO3)2+2Na2CO3+H2O→CuCO3·Cu(OH)2+4NaNO3+CO2↑ 2Cu(NO3)2+4NaHCO3→CuCO3·Cu( OH)2+4NaNO3+3CO2↑+H2O

*Operation method:
After the electrolytic copper reacts with concentrated nitric acid to produce copper acid, then it reacts with the mixture of sodium carbonate and sodium bicarbonate to produce Copper Carbonate.

The precipitate is washed, separated and dehydrated.
After drying, the finished Copper Carbonate is obtained.



PHYSICAL and CHEMICAL PROPERTIES of COPPER CARBONATE:
Chemical formula: Cu2(OH)2CO3
Molar mass: 221.114 g/mol
Appearance: green powder
Density: 4 g/cm3
Melting point: 200 °C (392 °F; 473 K)
Boiling point: 290 °C (554 °F; 563 K) decomposes
Solubility in water: insoluble
Solubility product (Ksp): 7.08·10−9
Thermochemistry:
Std molar entropy (S⦵298): 88 J/mol·K
Std enthalpy of formation (ΔfH⦵298): −595 kJ/mol
Physical state: solid
Color: No data available

Odor: odorless
Melting point/freezing point:
Melting point/range: > 400 °C
Initial boiling point and boiling range: Not applicable
Flammability (solid, gas): The product is not flammable.
Upper/lower flammability or explosive limits: No data available
Flash point: does not flash
Autoignition temperature: No data available
Decomposition temperature: 200 °C
pH: 8 - 9 at 50 g/l at 20 °C (slurry)
Viscosity
Viscosity, kinematic: No data available
Viscosity, dynamic: No data available
Water solubility: 0,002 g/l at 20 °C

Partition coefficient: n-octanol/water:
Not applicable for inorganic substances
Vapor pressure: No data available
Density: 3,9 - 4,0 g/cm3 at 25 °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
Chemical Name: Copper oxide (electroplate grade)
CAS NO.: 12069-69-1
Molecular formula: CuCO3·Cu(OH)2·XH2O
Molecular weight: 221.11(anhydride)

Colour: Pale green
Melting point: 200°C
Boiling point: Decomposes at 290°C to copper(II)oxide and carbon dioxide.
Solvent: Acetic acid, insoluble in water.
Formula: CuCO3.Cu(OH)2
Molecular Weight： 221.11
Exact Mass： 219.84900
EC Number： 235-113-6
HScode： 28369911
PSA： 103.65000
XLogP3：-2.80560
Appearance： green Solid
Density： 4

Melting Point： 200 °C (decomp)
Boiling Point： 333.6ºC at 760 mmHg
Flash Point： 169.8ºC
Water Solubility： Insoluble
Storage Conditions： Store in a tightly closed container.
Store in a cool, dry, well-ventilated area away from incompatible substances.
Flammability characteristics： Non-combustible
Chemical Formula: CuCO3· Cu(OH)2
CAS Number: 12069-69-1
Molecular Weight: 221.11
Use: Pharmaceuticals
Description: Blue-Green/Dark Green, odorless granules
Storage: Store in a clean, dry warehouse in the original unopened containers.



FIRST AID MEASURES of COPPER CARBONATE:
-Description of first-aid measures:
*General advice:
Show this material safety data sheet to the doctor in attendance.
*If inhaled:
After inhalation:
Fresh air.
Immediately call in physician.
*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 COPPER CARBONATE:
-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 COPPER CARBONATE:
-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 COPPER CARBONATE:
-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: 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 COPPER CARBONATE:
-Precautions for safe handling:
*Advice on safe handling:
Work under hood.
*Hygiene measures:
Change contaminated clothing.
Preventive skin protection recommended.
Wash hands after working with substance
-Conditions for safe storage, including any incompatibilities:
*Storage conditions:
Tightly closed.
Dry.
*Storage class:
Storage class (TRGS 510): 13:
Non Combustible Solids



STABILITY and REACTIVITY of COPPER CARBONATE:
-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



SYNONYMS:
Dicopper carbonate dihydroxide
copper carbonate hydroxide
cupric carbonate
copper carbonate, Greenium
Cupric carbonate basic
12069-69-1
CUPRIC CARBONATE, BASIC
Copper,[μ-[carbonato(2-)-κO:κO′]]dihydroxydi-
Copper carbonate hydroxide (Cu2(OH)2CO3)
Copper,(carbonato)dihydroxydi-
Copper,[μ-[carbonato(2-)-O:O′]]dihydroxydi-
Carbonic acid,copper complex
[μ-[Carbonato(2-)-κO:κO′]]dihydroxydicopper
Cheshunt compound
Dicopper dihydroxycarbonate
Copper basic carbonate
Copper hydroxide carbonate (Cu2(OH)2CO3)
Basic cupric carbonate
Basic copper carbonate
Copper carbonate hydroxide [CuCO3.Cu(OH)2]
Cupric carbonate,basic
Cupric carbonate hydroxide (CuCO3.Cu(OH)2)
Basic copper(II) carbonate
Cupric carbonate (CuCO3.Cu(OH)2)
Basic copper carbonate (Cu2(OH)2CO3)
Basic copper carbonate (Cu2(CO3)(OH)2)
Carbonic acid,copper(2+) salt (1:1),basic
Dicopper(2+) carbonate dihydroxide
Carbonatodihydroxodicopper
Copper dihydroxide carbonate
Copper carbonate hydroxide (Cu2(CO3)(OH)2)
[Carbonato(2-)]copper-dihydroxycopper (1:1)
Copper(II) hydroxycarbonate
1344-66-7
37396-60-4
39361-73-4
138210-92-1
866114-86-5
1036286-41-5
1821514-05-9
2108065-66-1
2130903-30-7
Cupric carbonate basic, malachite
COPPER CARBONATE
Copper oxycarbonate
copper(2+) carbonate
Copper (II) carbonate
Copper carbonate (CuCo3)
CARBONICACID,COPPER(II)SALT
Copper(Ⅱ)carbonate monohydrate
Malachite, Cupric Carbonate, Basic
Malachite green
copper(II) carbonate
copper carbonate
Malachite green
copper(II) carbonate
copper carbonate
cupric carbonate

DESCRIPTION:
Copper carbonate is a chemical compound of copper.
Copper carbonate is used as a pigment, in some types of make-up, as an algaecide, and for bronze plating.
Copper is a chemical element with the symbol Cu and atomic number 29.

CAS: 1184-64-1
European Community (EC) Number:. 231-325-8
Molecular Formula: CuCO3


SYNONYMS OF COPPER CARBONATE:
copper carbonate;copper carbonate, x-Cu(II) salt;CUPRIC CARBONATE;Copper carbonate;1184-64-1;Copper(II) carbonate,copper;carbonate,Copper monocarbonate,Copper carbonate (1:1),Carbonic acid, copper(2+) salt (1:1),9AOA5F11GJ,7492-68-4,Carbonic acid, copper salt,Cupromaag,MFCD00051038,Cupric carbonate (1:1),Copper carbonate (CuCO3),HSDB 258,EINECS 214-671-4,UNII-9AOA5F11GJ,CUPRICCARBONATE,Copper (II) carbonate,Carbonic acid,copper salt,cupric carbonate, AldrichCPR,SCHEMBL29678,COPPER (AS CARBONATE),DTXSID6034471,COPPER(II) CARBONATE [HSDB],SY347833,DB-208425,NS00078651,D78271,Q409630

Copper is an essential elements in plants and animals as it is required for the normal functioning of more than 30 enzymes.
Copper carbonate occurs naturally throughout the environment in rocks, soil, water, and air. (L277, L278, L298)



Copper(II) carbonate or cupric carbonate is a chemical compound with formula CuCO3.
At ambient temperatures, it is an ionic solid (a salt) consisting of copper(II) cations Cu2+
and carbonate anions CO2−3.

Copper carbonate is rarely encountered because it is difficult to prepare[2] and readily reacts with water moisture from the air.

The terms "copper carbonate", "copper(II) carbonate", and "cupric carbonate" almost always refer (even in chemistry texts) to a basic copper carbonate (or copper(II) carbonate hydroxide), such as Cu2(OH)2CO3 (which occurs naturally as the mineral malachite) or Cu3(OH)2(CO3)2 (azurite).
For this reason, the qualifier neutral may be used instead of "basic" to refer specifically to CuCO
3.

PREPARATION OF COPPER CARBONATE:
Reactions that may be expected to yield CuCO3, such as mixing solutions of copper(II) sulfate CuSO4 and sodium carbonate Na2CO3 in ambient conditions, yield instead a basic carbonate and CO2, due to the great affinity of the Cu2+ ion for the hydroxide anion HO−.[5]

Thermal decomposition of the basic carbonate at atmospheric pressure yields copper(II) oxide CuO rather than the carbonate.
In 1960, C. W. F. T. Pistorius claimed synthesis by heating basic copper carbonate at 180 °C in an atmosphere of carbon dioxide CO2 (450 atm) and water (50 atm) for 36 hours.


The bulk of the products was well-crystallized malachite Cu2CO3(OH)2, but a small yield of a rhombohedral substance was also obtained, claimed to be CuCO3.[6]
However, this synthesis was apparently not reproduced.[2]
Reliable synthesis of true copper(II) carbonate was reported for the first time in 1973 by Hartmut Ehrhardt and others.

The compound was obtained as a gray powder, by heating basic copper carbonate in an atmosphere of carbon dioxide (produced by the decomposition of silver oxalate Ag2C2O4) at 500 °C and 2 GPa (20,000 atm).
The compound was determined to have a monoclinic structure.[7]

CHEMICAL AND PHYSICAL PROPERTIES OF COPPER CARBONATE:
The stability of dry CuCO3 depends critically on the partial pressure of carbon dioxide (pCO2).
It is stable for months in dry air, but decomposes slowly into CuO and CO2 if pCO2 is less than 0.11 atm.[3]

In the presence of water or moist air at 25 °C, CuCO3 is stable only for pCO2 above 4.57 atmospheres and pH between about 4 and 8.[8]
Below that partial pressure, it reacts with water to form a basic carbonate (azurite, Cu3(CO3)2(OH)2).[3]
3 CuCO3 + H2O → Cu3(CO3)2(OH)2 + CO2
In highly basic solutions, the complex anion Cu(CO3)2−2 is formed instead.

The solubility product of the true copper(II) carbonate was measured by Reiterer and others as pKso = 11.45 ± 0.10 at 25 °C.


STRUCTURE OF COPPER CARBONATE:
In the crystal structure of CuCO3, copper adopts a distorted square pyramidal coordination environment with coordination number 5.
Each carbonate ion bonds to 5 copper centres.

Finer than copper oxide, disperses better in the glaze.

In oxidizing firing develops green-yellow and turquoise hues in alkaline glaze.

And the famous "copper" reds in reduction*.

*In this form it allows a greater division of the oxide, copper is used to give reds called "copper" with a very reducing firing (colloidal coloring)




Copper salt of very fine grain, insoluble in cold water which decomposes in hot water.

Copper carbonate is soluble in ammonium hydroxide and in most acids.

Normally Copper carbonate is green in color and is very toxic.

Its dispersion in glazes is better than that of oxide because of its granulometry, although the green color obtained is less intense than with copper oxide.


When added to lead glazes or frits, the action of copper increases their solubility considerably and the green glazes thus obtained cannot be used for food articles and generally for any container that may be in contact with food.
A less powerful colouring stain than copper oxide but is able to disperse through a glaze more uniformly and is used where the slight speckle of the oxide is not desired. 3-7%


Copper carbonate comes in various shades of green, reflecting various degrees of hydration.
Pure copper carbonate (CuCO3) is about 64% CuO, whereas the basic carbonate (CuCO3 Cu(OH)2) is nearly 72% CuO.
The basic carbonate is (in theory) easier to disperse in glazes due to its greater affinity for water. Prepared from Malachite (CuCO3 Cu(OH)2) and Azurite (2CuCO3 Cu(OH)2) or by chemical processes.


Copper carbonate (Cu2CO3(OH)2) is a water insoluble chemical created when copper loses the electrons in its outermost shell.
Also known as copper (II) carbonate, carbonic acid, and copper monocarbonate, copper carbonate converts quickly to copper salts.
USP ingredient supplier Bell Chem’s customers use copper carbonate in jewelry metallurgy, wood preservation, pesticides, and more.



Agriculture:
Copper carbonate is used frequently in fertilizer as well as in fungicides, insecticides, pesticides — where it acts as an anti-pathogenic — and in aquaculture where it controls unwanted foliage.
Rather than adding copper carbonate to fertilizer, manufacturers may add this important nutrient to the seeds as they are packaged.

The cost of copper carbonate at this point is significantly lower than adding it to soil, reducing overall expenses.
Animal feed, specifically poultry and ruminant feed, often has added copper carbonate since these animals rely on copper as a supplemental nutrient.


Woodworking and Ceramics:
Micronized copper wood treatment consists of tiny copper carbonate particles suspended in a final treatment solution (often containing ammonia) for preserving wood and timber.
Copper carbonate also helps with ceramic products.
Before ceramics are fired, a glaze is often added to retain color and give a finished look to the product.

Adding copper carbonate to the glaze creates a seafoam sheen to the ceramic.
Applying copper carbonate plus an alkaline generates a bluer hue.


Other Uses of Copper Carbonate:
Copper carbonate helps with the creation of many products, as well as helping along the scientific process. Here are a few more examples of its range of uses:
Laboratories: Copper carbonate catalyzes copper chromite, which breaks down fatty methyl esters in the production of fatty alcohols.

Paints: In artist’s palettes, copper carbonate creates the sought-after colors verditer and mountain green.
Petroleum: Adding nitric acid to copper carbonate produces copper chloride, important in the process of “oil sweetening”, or purifying oil of its sulfur components.
Pyrotechnics: Companies manufacturing fireworks use copper carbonate for a stellar blue sparkle to pyrotechnic displays.



CHEMICAL AND PHYSICAL PROPERTIES OF COPPER CARBONATE:

Molecular Weight
123.55 g/mol
Computed by PubChem 2.2 (PubChem release 2021.10.14)
Hydrogen Bond Donor Count
0
Computed by Cactvs 3.4.8.18 (PubChem release 2021.10.14)
Hydrogen Bond Acceptor Count
3
Computed by Cactvs 3.4.8.18 (PubChem release 2021.10.14)
Rotatable Bond Count
0
Computed by Cactvs 3.4.8.18 (PubChem release 2021.10.14)
Exact Mass
122.914341 g/mol
Computed by PubChem 2.2 (PubChem release 2021.10.14)
Monoisotopic Mass
122.914341 g/mol
Computed by PubChem 2.2 (PubChem release 2021.10.14)
Topological Polar Surface Area
63.2Ų
Computed by Cactvs 3.4.8.18 (PubChem release 2021.10.14)
Heavy Atom Count
5
Computed by PubChem
Formal Charge
0
Computed by PubChem
Complexity
18.8
Computed by Cactvs 3.4.8.18 (PubChem release 2021.10.14)
Isotope Atom Count
0
Computed by PubChem
Defined Atom Stereocenter Count
0
Computed by PubChem
Undefined Atom Stereocenter Count
0
Computed by PubChem
Defined Bond Stereocenter Count
0
Computed by PubChem
Undefined Bond Stereocenter Count
0
Computed by PubChem
Covalently-Bonded Unit Count
2
Computed by PubChem
Compound Is Canonicalized
Yes
CAS Number
1184-64-1 check[ECHA]
3D model (JSmol)
Interactive image
ChemSpider
13799
ECHA InfoCard 100.013.338 Edit this at Wikidata
EC Number
214-671-4
PubChem CID
14452
UNII
9AOA5F11GJ check
CompTox Dashboard (EPA)
DTXSID6034471 Edit this at Wikidata
InChI
SMILES
Properties
Chemical formula CuCO3
Molar mass 123.5549
Appearance green or blue Powder[1]
Solubility in water insoluble in water [clarification needed]
Solubility product (Ksp) 10−11.45 ± 0.10 at 25 °C.[2][3][4]
Structure
Space group Pa-C2s (7) [1]
Lattice constant
a = 6.092 Å, b = 4.493 Å, c = 7.030 Å
α = 90°, β = 101,34°°, γ = 90°
Coordination geometry 5 [1



SAFETY INFORMATION ABOUT COPPER CARBONATE:
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.

Copper Chloride, commonly called cuprous chloride, is the lower chloride of copper, with the formula CuCl.
Copper Chloride is a white solid sparingly soluble in water, but very soluble in concentrated hydrochloric acid.
Impure samples appear green due to the presence of copper(II) chloride (CuCl2).


CAS Number: 7758-89-6
EC Number: 231-842-9
Molecular Formula: CuCl / ClCu


Copper Chloride is an inorganic chloride of copper in which the metal is in the +1 oxidation state.
Copper Chloride has a role as a molluscicide and an agrochemical.
Copper Chloride is an inorganic chloride and a copper molecular entity.


Copper Chloride contains a copper(1+).
Copper Chloride is a chloride of copper that occurs naturally as the rare mineral nantokite.
The main use of Copper Chloride is as a precursor to the fungicide copper oxychloride.


Copper Chloride is also used in organic and polymer chemistry.
Copper is a chemical element with the symbol Cu and atomic number 29.
Copper is an essential elements in plants and animals as it is required for the normal functioning of more than 30 enzymes.


It occurs naturally throughout the environment in rocks, soil, water, and air.
Copper Chloride is a yellowish-brown powder (the anhydrous form) or a green crystalline solid (the dihydrate).
Copper Chloride is noncombustible but hydrogen chloride gas may form when heated in a fire.


Copper Chloride is used to manufacture other chemicals, in dyeing, in printing, in fungicides, as a wood preservative.
Copper Chloride is registered under the REACH Regulation and is manufactured in and / or imported to the European Economic Area, at ≥ 1 000 tonnes per annum.


Copper Chloride, commonly called cuprous chloride, is the lower chloride of copper, with the formula CuCl.
Copper Chloride is a white solid sparingly soluble in water, but very soluble in concentrated hydrochloric acid.
Impure samples appear green due to the presence of copper(II) chloride (CuCl2).


Copper Chloride is white or pale grey powder
Copper Chloride is a brownish-yellow powder.
Copper Chloride is an inorganic chloride of copper in which the metal is in the +1 oxidation state.


The structure of Copper Chloride is similar to zinc-blende crystal at room temperature; the structure is wurtzite at 407 °C and at higher temperatures it forms Copper Chloride vapor as per mass spectroscopy.
Copper Chloride refers to an inorganic chloride of copper.


Furthermore, Copper Chloride is commonly known as cuprous chloride and it happens to be a lower chloride of copper.
Copper Chloride is a white solid and is somewhat soluble in water.
Moreover, the impure samples of Copper Chloride have a greenish appearance because of the copper II chloride.



USES and APPLICATIONS of COPPER CHLORIDE:
Copper Chloride is used by consumers, in articles, by professional workers (widespread uses), in formulation or re-packing, at industrial sites and in manufacturing.
Copper Chloride is used in the following products: fertilisers, textile treatment products and dyes and cosmetics and personal care products.


Other release to the environment of Copper 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 as reactive substance 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 Copper Chloridecan occur from industrial use: industrial abrasion processing with low release rate (e.g. cutting of textile, cutting, machining or grinding of metal).
Copper Chloride is used for the manufacture of: chemicals.


Other release to the environment of Copper Chloride is likely to occur from: 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).


Copper Chloride is used in the following products: fertilisers and laboratory chemicals.
Copper Chloride is used in the following areas: agriculture, forestry and fishing, formulation of mixtures and/or re-packaging and scientific research and development.


Release to the environment of Copper Chloride can occur from industrial use: formulation of mixtures, in the production of articles and as an intermediate step in further manufacturing of another substance (use of intermediates).
Copper Chloride can be found in products with material based on: fabrics, textiles and apparel (e.g. clothing, mattress, curtains or carpets, textile toys).


Other release to the environment of Copper Chloride is likely to occur from: indoor use as reactive substance, outdoor use as reactive substance and outdoor use in close systems with minimal release (e.g. hydraulic liquids in automotive suspension, lubricants in motor oil and break fluids).
Copper Chloride is used in the following products: adsorbents, metals, fertilisers, pH regulators and water treatment products, laboratory chemicals, polymers, textile treatment products and dyes and cosmetics and personal care products.


Release to the environment of Copper Chloride can occur from industrial use: formulation of mixtures, in the production of articles, as an intermediate step in further manufacturing of another substance (use of intermediates), formulation in materials, manufacturing of the substance, in processing aids at industrial sites and as processing aid.


Copper Chloride is used in the following products: adsorbents, pH regulators and water treatment products, laboratory chemicals, metals, fertilisers, polymers, textile treatment products and dyes and cosmetics and personal care products.
Copper Chloride has an industrial use resulting in manufacture of another substance (use of intermediates).


Copper Chloride has an industrial use resulting in manufacture of another substance (use of intermediates).
Copper Chloride is used in the following areas: formulation of mixtures and/or re-packaging, scientific research and development and agriculture, forestry and fishing.


Release to the environment of Copper Chloride can occur from industrial use: as an intermediate step in further manufacturing of another substance (use of intermediates), in the production of articles, as processing aid, in processing aids at industrial sites and formulation of mixtures.
Copper Chloride is used for the manufacture of: chemicals, metals, and textile, leather or fur.


Release to the environment of Copper Chloride can occur from industrial use: manufacturing of the substance, formulation of mixtures, 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) and as processing aid.


The major use of Copper Chloride is as a precursor to fungicide copper oxychloride.
To achieve this, the generation of aqueous Copper Chloride takes place by comproportionation and then air-oxidization:
Cu+CuCl2→2CuCl
4CuCl+O2+2H2O→Cu3Cl2(OH)4+CuCl2


Copper Chloride catalyzes a variety of reactions that are organic in nature.
Copper Chloride has an affinity for carbon monoxide in the presence of aluminium chloride.
Moreover, there is an exploitation of this affinity of Copper Chloride in the process of COPureSM.


Copper Chloride has important usage with carbon monoxide, hydrogen chloride, and aluminium chloride, in the Gatterman-Koch reaction to result in the formation of benzaldehyde.
In the Sandmeyer reaction, an arenediazonium salt’s treatment with Copper Chloride leads to an aryl chloride.


Moreover, this reaction usually results in good yields and has a massive scope.
An observation was made by early investigators that copper I halides catalyze 1,4-addition of Grignard reagents to alpha ketones that are beta-unsaturated.
This observation led to the development of organocuprate reagents that are important in organic synthesis.


Also, Copper Chloride has usage as a molluscicide and an agrochemical.
Copper Chloride is an initiator of radical reactions
Copper Chloride is an initiator of radical reactions, such as the hydrostannation of α,β-unsaturated ketones.


Copper Chloride has many applications.
The main use of Copper Chloride is as a precursor to the fungicide copper oxychloride.
In organic synthesis, Copper Chloride is used as an initiator of radical reactions such as the hydrostannation of a,b-unsaturated ketones.


Copper chloride is also known as cupric chloride, this substance was made by treating copper carbonate with hydrochloric acid.
The greenish-blue crystals of Copper Chloride are soluble in water, alcohol, and ether.
This halide, Copper Chloride, was added to printing-out and silver bromide emulsions for increased contrast.


Copper Chloride is a white powder used as an absorbing agent for carbon dioxide gas in enclosed breathing areas such as space vehicles.
Copper Chloride is used as catalyst for organic reactions; catalyst, decolorizer and desulfuring agent in petroleum industry.
Copper Chloride is used in denitration of cellulose; as condensing agent for soaps, fats and oils.


Copper Chloride is used in gas analysis to absorb carbon monoxide.
Copper Chloride shows unique character as an initiator of radical reactions such as the hydrostannation of α,β-unsaturated ketones.
Copper Chloride is used for absorption of carbon monoxide in gas analysis.


The main use of Copper Chloride is as a precursor to the fungicide copper oxychloride.
For this purpose aqueous Copper Chloride is generated by comproportionation and then air-oxidized:
Cu + CuCl2 → 2 CuCl
4 CuCl + O2 + 2 H2O → Cu3Cl2(OH)4 + CuCl2


Copper Chloride catalyzes a variety of organic reactions, as discussed above.
Copper Chloride's affinity for carbon monoxide in the presence of aluminium chloride is exploited in the COPureSM process.


-Niche uses of Copper Chloride:
Copper Chloride is used as a catalyst in atom transfer radical polymerization (ATRP).
Copper Chloride is also used in pyrotechnics as a blue/green coloring agent.
In a flame test, copper chloride, like all copper compounds, emit green-blue.



PREPARATION OF COPPER CHLORIDE:
Copper Chloride can be prepared by reduction of copper(II) ions in presence of chloride ions.
CuCl2 → CuCl + Cl-
Possible methods include bubbling sulfur dioxide through an aqueous solution of copper(II) chloride, or heating a solution of copper sulfate, sodium chloride and ascorbic acid.

CuCl2 + SO2 + 2 H2O → 2 CuCl + H2SO4 + 2 HCl
2 CuCl2 + C6H8O6 → 2 CuCl + 2HCl + C6H6O6
Copper Chloride can also be produced by boiling copper(II) chloride and copper metal in hydrochloric acid.

CuCl2 + Cu → 2 CuCl
Originally, Copper Chloride was first made by reducing mercury(II) chloride with copper metal:

HgCl2 + 2 Cu → 2 CuCl + Hg
Industrially Copper Chloride is made by direct combination of copper metal and chlorine at 450–900 °C:
2 Cu + Cl2 → 2 CuCl



HISTORY OF COPPER CHLORIDE:
Copper Chloride was first prepared by Robert Boyle in the mid-seventeenth century from mercury(II) chloride ("Venetian sublimate") and copper metal:
HgCl2 + 2 Cu → 2 CuCl + Hg
In 1799, J.L. Proust characterized the two different chlorides of copper.

He prepared Copper Chloride by heating CuCl2 at red heat in the absence of air, causing it to lose half of its combined chlorine followed by removing residual CuCl2 by washing with water.

An acidic solution of Copper Chloride was formerly used to analyze carbon monoxide content in gases, for example in Hempel's gas apparatus where the Copper Chloride absorbs the carbon monoxide.
This application was significant during the nineteenth and early twentieth centuries when coal gas was widely used for heating and lighting.



SYNTHESIS OF COPPER CHLORIDE:
Copper Chloride is produced industrially by the direct combination of copper metal and chlorine at 450–900 °C:
2 Cu + Cl2 → 2 CuCl
Copper Chloride can also be prepared by reducing copper(II) chloride with sulfur dioxide, or with ascorbic acid (vitamin C) that acts as a reducing sugar:

2 CuCl2 + SO2 + 2 H2O → 2 CuCl + H2SO4 + 2 HCl
2 CuCl2 + C6H8O6 → 2CuCl + 2HCl + C6H6O6
Many other reducing agents can be used



PROPERTIES OF COPPER CHLORIDE:
Copper Chloridehas the cubic zincblende crystal structure at ambient conditions.
Upon heating to 408 °C the structure changes to hexagonal.
Several other crystalline forms of CuCl appear at high pressures (several GPa).

Copper Chloride is a Lewis acid.
Copper Chloride is classified as soft according to the hard-soft acid-base concept.
Thus, Copper Chloride forms a series of complexes with soft Lewis bases such as triphenylphosphine:

CuCl + 1 P(C6H5)3 → 1/4 {CuCl[P(C6H5)3]}4
CuCl + 2 P(C6H5)3 → CuCl[P(C6H5)3)]2
CuCl + 3 P(C6H5)3 → CuCl[P(C6H5)3)]3

Copper Chloride also forms complexes with halides.
For example H3O+ CuCl2− forms in concentrated hydrochloric acid.
Chloride is displaced by CN− and S2O32−.

Solutions of Copper Chloride in HCl absorb carbon monoxide to form colourless complexes such as the chloride-bridged dimer [CuCl(CO)]2.
The same hydrochloric acid solutions also react with acetylene gas to form [CuCl(C2H2)].
Ammoniacal solutions of Copper Chloride react with acetylenes to form the explosive copper(I) acetylide, Cu2C2.

Alkene complexes of Copper Chloride can be prepared by reduction of CuCl2 by sulfur dioxide in the presence of the alkene in alcohol solution. Complexes with dienes such as 1,5-cyclooctadiene are particularly stable:



CHEMICAL PROPERTIES OF COPPER CHLORIDE:
Copper Chloride is almost completely insoluble in water.
Copper Chloride does however form complexes and dissolve in concentrated hydrochloric acid and ammonium hydroxide (aq. ammonia), as well as in cyanide and thiosulfate solutions.



PHYSICAL PROPERTIES OF COPPER CHLORIDE:
Pure samples of Copper Chloride appear as white, dense, cubical crystals.
As Copper Chloride is slowly oxidized in air, older samples may appear dirty green or brown.



STRUCTURE OF COD COMPLEX OF COPPER CHLORIDE:
Upon contact with water, Copper Chloride slowly undergoes disproportionation:
2 CuCl → Cu + CuCl2
In part for this reason, samples in air assume a green coloration.



PREPARATION OF COPPER CHLORIDE:
Copper Chloride is prepared by reduction of copper(II) chloride in solution: 2CuCl2 + H2 2CuCl + 2HCl
Alternatively, Copper Chloride can be prepared by boiling an acidic solution of copper(II) chloride with copper metal, which on dilution yields white CuCl: Cu + CuCl2 2CuCl

Copper Chloride dissolved in concentrated HCl absorbs carbon monoxide under pressure forming an adduct, CuCl(CO).
The complex decomposes on heating releasing CO.
Copper Chloride is slightly soluble in water.

However, in the presence of Cl- ion, it forms soluble complexes of discrete halogeno anions such as, CuCl2-, CuCl3 2-, and CuCl4 3-.
Formation of complexes and organocopper derivatives as outlined below are not confined only to Copper Chloride, but typify Cu+ in general.
Reaction with ethylenediamine (en) in aqueous potassium chloride solution forms Cu(II)-ethylenediamine complex, while Cu+ ion is reduced to its metallic state: 2CuCl + 2en → [Cuen2]2+ + 2Cl- + Cu°

It dissolves in acetonitrile, CH3CN forming tetrahedral complex ion [Cu(CH3CN)4]+ which can be precipitated with large anions such as ClO4 - or PF6- .
Reactions with alkoxides of alkali metals produce yellow copper(I) alkoxides.
For example, reaction with sodium ethoxide yield copper(I) ethoxide, a yellow compound that can be sublimed from the product mixture: CuCl + NaOC2H5 → CuOC2H5 + NaCl

Copper Chloride forms complexes with ethylene and other alkenes in solutions that may have compositions such as [Cu(C2H4)(H2O)2]+ or [Cu(C2H4)(bipy)]+. (bipy = bipyridyl)
Reactions with lithium or Grignard reagent yield alkyl or aryl copper(I) derivatives, respectively.
Such organocopper compounds containing Cu-Cu bonds are formed only by Cu+ and not Cu2+ ions.



IN ORGANIC SYNTHESIS OF COPPER CHLORIDE:
Copper Chloride is used as a co-catalyst with carbon monoxide, aluminium chloride, and hydrogen chloride in the Gatterman-Koch reaction to form benzaldehydes.

In the Sandmeyer reaction, the treatment of an arenediazonium salt with Copper Chloride leads to an aryl chloride.
For example: (Example Sandmeyer reaction using CuCl)

The reaction has a wide scope and usually gives good yields.
Early investigators observed that copper(I) halides catalyse 1,4-addition of Grignard reagents to alpha,beta-unsaturated ketones led to the development of organocuprate reagents that are widely used today in organic synthesis:

(Addition of RMgX to C=C-C=O mediated by CuCl)
This finding led to the development of organocopper chemistry.
For example, Copper Chloride reacts with methyllithium (CH3Li) to form "Gilman reagents" such as (CH3)2CuLi, which find use in organic synthesis.

Grignard reagents form similar organocopper compounds.
Although other copper(I) compounds such as copper(I) iodide are now more often used for these types of reactions, copper(I) chloride is still recommended in some cases:
(Alkylation of sorbate ester at 4-position mediated by CuCl)



NATURAL OCCURRENCE OF COPPER CHLORIDE:
Natural form of Copper Chloride is the rare mineral nantokite.



FORMULA OF COPPER CHLORIDE:
Derivation of Copper I Chloride Formula
Copper Chloride is certainly a lower copper chloride where copper is in the oxidation state +1.

The chemical formula of Copper Chloride happens to be CuCl.
The production of Copper Chloride takes place by the direct combination of copper and chlorine at a temperature of 450–900 °C:
2Cu + Cl2→2CuCl



PROPERTIES OF COPPER CHLORIDE:
Copper Chloride has the crystal structure of cubic zincblende at conditions that are ambient.
Upon heating Copper Chloride to 408 °C, a change of structure takes place to hexagonal.
Moreover, at high pressures, there is the appearance of several other crystalline forms of Copper Chloride.

Copper Chloride happens to be a Lewis acid.
Moreover, the classification of Copper Chloride is as soft, in accordance with the Hard-Soft Acid-Base concept.
Therefore, there is a formation of stable complexes with soft Lewis bases such as triphenylphosphine.

Copper Chloride can dissolve in aqueous solutions containing appropriate donor molecules.
With halide ions, Copper Chloride forms complexes, for example, the formation of H3O+CuCl−2 with concentrated hydrochloric acid.
Furthermore, CN−, S2O2−3, and NH3 attack Copper Chloride to give the corresponding complexes.

Solutions of Copper Chloride in HCl or NH3 absorb carbon monoxide to result in the formation of complexes that are colorless.
Moreover, one of these complexes is the chloride-bridged dimer.
Furthermore, a reaction also takes place between the same hydrochloric acid solutions and acetylene gas to result in the formation of [CuCl(C2H2)].

Ammoniacal solutions of Copper Chloride react with acetylenes to result in the formation of the explosive copper I acetylide, Cu2C2.
Preparation of complexes of Copper Chloride with alkenes can take place by reduction of CuCl2 by sulfur dioxide with the availability of alkene in an alcohol solution.
Complexes with dienes like the 1,5-cyclooctadiene are stable.



PURIFICATION METHODS OF COPPER CHLORIDE:
Wash the solid with ethanol and diethyl ether, then dry Copper Chloride and store it in a vacuum desiccator.
Alternatively, an aqueous solution of CuCl2.2H2O is added, with stirring, an aqueous solution of anhydrous sodium sulfite.
The colorless Copper Chloride is dried at 80o for 30 minutes and stored under N2.
Cu2Cl2 can be purified by zone-refining.



INCOMPATIBILITIES OF COPPER CHLORIDE:
Contact with Copper Chloride strong acids forms monovalent copper salts and toxic hydrogen chloride gas.
Copper Chloride forms shock-sensitive and explosive compounds with potassium, sodium, sodium hypobromite, nitromethane, acetylene.
Keep away from moisture and alkali metals.
Copper Chloride attacks metals in the presence of moisture.

Copper Chloride reacts with moist air to form cupric chloride dihydrate.
Copper Chloride may attack some metals, paints, and coatings.
Copper Chloride may be able to ignite combustible materials.



PHYSICAL PROPERTIES OF COPPER CHLORIDE:
Copper Chloride is white cubic crystal which turns blue when heated at 178°C; density 4.14 g/cm3; the mineral nantokite (CuCl) has density 4.14 g/cm3, hardness 2.5 (Mohs), refractive index 1.930; melts at 430°C becoming a deep, green liquid; vaporizes around 1,400°C; vapor pressure 5 torr at 645°C and 400 torr at 1,250°C; low solubility in water (decomposes partially); Ksp 1.72x10-7; insoluble in ethanol and acetone; soluble in concentrated HCl and ammonium hydroxide.



PHYSICAL and CHEMICAL PROPERTIES of COPPER CHLORIDE:
Chemical formula: CuCl
Molar mass: 98.999 g/mol
Appearance: white powder, slightly green from oxidized impurities
Density: 4.14 g/cm3
Melting point: 423 °C (793 °F; 696 K)
Boiling point: 1,490 °C (2,710 °F; 1,760 K) (decomposes)
Solubility in water: 0.047 g/L (20 °C)
Solubility product (Ksp): 1.72×10−7
Solubility: insoluble in ethanol,
acetone;soluble in concentrated HCl, NH4OH
Band gap: 3.25 eV (300 K, direct)
Magnetic susceptibility (χ): -40.0·10−6 cm3/mol
Refractive index (nD): 1.930
Structure:
Crystal structure: Zincblende, cF20
Space group: F43m, No. 216
Lattice constant:
a = 0.54202 nm
Lattice volume (V): 0.1592 nm3
Formula units (Z): 4

Molecular Weight: 99.00 g/mol
Hydrogen Bond Donor Count: 0
Hydrogen Bond Acceptor Count: 0
Rotatable Bond Count: 0
Exact Mass: 97.898450 g/mol
Monoisotopic Mass: 97.898450 g/mol
Topological Polar Surface Area: 0 Ų
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: 1
Compound Is Canonicalized: Yes
Physical state: granules
Color: beige

Odor: odorless
Melting point/freezing point:
Melting point/range: 430 °C - lit.
Initial boiling point and boiling range: 1.490 °C - lit.
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: 5 at 50 g/l at 20 °C
Viscosity
Viscosity, kinematic: No data available
Viscosity, dynamic: No data available
Water solubility: 0,047 g/l at 20 °C - slightly soluble
Partition coefficient: n-octanol/water:
Not applicable for inorganic substances
Vapor pressure: 1,7 hPa at 546 °C
Density: 4,140 g/cm3 at 25 °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

Chemical formula: CuCl
Molar mass: 98.999 g/mol
Appearance: White solid
Density: 4.14 g/cm3
Melting point: 423 °C (793 °F; 696 K)
Boiling point: 1,490 °C (2,710 °F; 1,760 K) (decomposes)
Solubility in water: 0.47 g/100 ml (20 °C)
Solubility: Soluble in aq. ammonia, conc. HCl
Insoluble in acetone, ethanol
Vapor pressure: ~0 mmHg
CAS number: 7758-89-6
EC index number: 029-001-00-4
EC number: 231-842-9
Grade: ACS
Hill Formula: ClCu
Chemical formula: CuCl
Molar Mass: 98.99 g/mol
HS Code: 2827 39 85
Boiling point: 1367 °C (1013 hPa)
Density: 4.140 g/cm3 (25 °C)
Melting Point: 430 °C
pH value: 5 (50 g/l, H₂O, 20 °C) (slurry)
Vapor pressure: 1.7 hPa (546 °C)
Bulk density: 1600 - 1800 kg/m3
Melting point: 430 °C (lit.)
Boiling point: 1490 °C (lit.)

Density: 1.15 g/mL at 20 °C
vapor pressure: 1.3 mm Hg ( 546 °C)
refractive index: 1.93
Flash point: 1490°C
storage temp.: Store at +5°C to +30°C.
solubility: 0.06 g/L (25°C)
form: beads
color: Slightly greenish-gray
Specific Gravity: 4.14
PH: 5 (50g/l, H2O, 20℃)(slurry)
Water Solubility: 0.06 g/L (25 ºC)
Sensitive: Air & Moisture Sensitive
Crystal Structure: Hexagonal, Wurtzite (Zincite) Structure - Space Group P 63mc
Merck: 14,2660
Solubility Product Constant (Ksp):
pKsp: 6.76
Exposure limits ACGIH: TWA 1 mg/m3
NIOSH: IDLH 100 mg/m3; TWA 1 mg/m3
Stability: Stable.
FDA 21 CFR: 582.80
CAS DataBase Reference: 7758-89-6(CAS DataBase Reference)
EWG's Food Scores: 2
FDA UNII: C955P95064
NIST Chemistry Reference: Cuprous monochloride(7758-89-6)
EPA Substance Registry System: Cuprous chloride (7758-89-6)



FIRST AID MEASURES of COPPER 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.
Immediately 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 COPPER 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 COPPER 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 COPPER CHLORIDE:
-Control parameters:
--Ingredients with workplace control parameters:
-Exposure controls:
--Personal protective equipment:
*Eye/face protection:
Use equipment for eye protection.
Tightly fitting safety goggles
*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 COPPER CHLORIDE:
-Conditions for safe storage, including any incompatibilities:
*Storage conditions
Tightly closed.
Dry.
Air, light, and moisture sensitive.
*Storage class:
Storage class (TRGS 510): 8B:
Non-combustible



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



SYNONYMS:
Cuprous chloride
COPPER(I) CHLORIDE
7758-89-6
Dicopper dichloride
Copper monochloride
Chlorocopper
Copper (I) chloride
Copper(1+) chloride
Copper chloride (CuCl)
CuCl
MFCD00010971
copper [I] chloride
Chlorid medny [Czech]
Chlorid medny
EINECS 231-842-9
Cuproid
Cu-lyt
copper(I) cloride
UNII-C955P95064
copper (I)chloride
copper(I)-chloride
copper (1)chloride
copper(1) chloride
copper-(I) chloride
copper-(I)-chloride
copper (1) chloride
copper chloride dihydride
Copper( centn) chloride
EC 231-842-9
Copper(I) Chloride ACS reagent
CHEBI:53472
OXBLHERUFWYNTN-UHFFFAOYSA-M
Copper(I) chloride, LR, >=96%
EINECS 215-704-5
UN2802
AKOS030228591
Copper(I) chloride, p.a., 97.0%
DB15535
BP-11474
Copper chloride [UN2802]
Copper(I) chloride, reagent grade, 97%
Copper(I) chloride, ACS reagent, >=90%
FT-0624053
Copper(I) chloride, purum, >=97.0% (RT)
D78100
Q423879
Copper(I) chloride, >=99.995% trace metals basis
Copper(I) chloride, JIS special grade, >=95.0%
Copper(I) chloride, ReagentPlus(R), purified, >=99%
(2Z)-(2,4-DIOXO-1,3-THIAZOLIDIN-5-YLIDENE)ACETICACID
Copper (I) chloride, 99.99% trace metals basis glass ampoules
Copper(I) chloride, anhydrous, beads, >=99.99% trace metals basis
Copper(I) chloride, puriss. p.a., ACS reagent, >=97.0% (RT)
Cuprous monochloride
Copper(I) chloride
Copper monochloride
Cuprous chloride
Copper Chloride (CuCl)
Copper Chloride (Cu2Cl2)
Copper Monochloride
Copper(1+) Chloride
Cuprous Chloride
Cuprous Chloride (Cu2Cl2)
Cuprous Chloride (CuCl)
Dicopper Dichloride
CuCl
Cu-lyt
Cuproid
Nantokite
chloridmedny
COPPER CHLORIDE
Chlorocopper(I)
cooper chloride
CUPROUS CHLORIDE
cuprousdichloride
CuCl
COPPER CHLORIDE
CUPROUS CHLORIDE
COPPER(L) CHLORIDE
cooper chloride
Copper(Ⅰ)chloride
CUPROUS CHLORIDE
REAGENT (ACS)CUPROUS CHLORIDE
REAGENT (ACS)CUPROUS CHLORIDE
REAGENT (ACS)CUPROUS CHLORIDE, REAGENT (ACS)
Cu-lyt
Cuproid
Nantokite