SILVER CHLORIDE
SILVER CHLORIDE
Silver chloride is a chemical compound with the chemical formula AgCl.
This white crystalline solid, Silver chloride, is well known for its low solubility in water and its sensitivity to light.
Silver chloride occurs naturally as the mineral chlorargyrite.
CAS Number: 7783-90-6
EC Number: 232-033-3
Chemical Formula: AgCl
Molar Mass: 143.32 g/mol
Synonyms: Silver(I) chloride, Cerargyrite, Chlorargyrite, Horn silver, Argentous chloride, Silver chloride, 7783-90-6, chlorosilver, AgCl, Silver monochloride, Mark II, Caswell No. 735A, EINECS 232-033-3, UNII-MWB0804EO7, EPA Pesticide Chemical Code 072506, MWB0804EO7, EC 232-033-3, Silver chloride (AgCl), Silver chloride(AgCl), Silver( centn)Chloride, Silver monochloride Mark II, Silver(I) chloride, Premion, Sanitizer Hand and Skin Care, Silver(I) chloride, ultra dry, DTXCID2015251, HKZLPVFGJNLROG-UHFFFAOYSA-M, Silver chloride, p.a., 99.6%, Silver chloride, purum, >=99.5%, AKOS024438107, Silver chloride, ReagentPlus(R), 99%, CS-0031738, FT-0693927, Silver chloride, 99.999% trace metals basis, Silver chloride, SAJ special grade, >=99.5%, Q216918, Silver chloride, anhydrous, beads, -10 mesh, 99.998% trace metals basis, AgCl, ver(I) ChL, Chlorosilver, Silver chlorid, Silver chloride, Silve (Ⅰ)Chloride, silvermonochloride, SILVER (I) CHLORIDE, Silver monochloride, Silver chloride 99+,
Silver chloride is an inorganic salt.
Silver chloride is a chemical compound with the chemical formula AgCl.
Silver chloride is a white crystalline chemical compound with the formula AgCl.
Silver chloride in the test tube quickly turns purplish, especially in a sunny laboratory because the Silver chloride is split up into silver and chlorine.
Silver chloride is prepared when sodium chloride is added to silver nitrate solution a white precipitate of Silver chloride occurs.
Silver chloride is an example of a well-known salt stain used to impart an amber colour to the glass.
Silver chloride is a chemical compound with the chemical formula AgCl.
This white crystalline solid, Silver chloride, is well known for its low solubility in water and its sensitivity to light.
Upon illumination or heating, Silver chloride converts to silver (and chlorine), which is signaled by grey to black or purplish coloration in some samples.
Silver chloride occurs naturally as a mineral chlorargyrite.
Silver chloride is produced by a metathesis reaction for use in photography and in pH meters as electrodes.
Silver chloride is a chloride of silver that occurs naturally as the mineral chlorargyrite.
Silver is a metallic element with the chemical symbol Ag and atomic number 47.
Silver chloride occurs naturally in its pure, free form, as an alloy with gold and other metals, and in minerals such as argentite and chlorargyrite.
Silver chloride is a white crystalline solid which is well known for its low solubility in water.
Silver chloride occurs naturally as the mineral chlorargyrite.
Silver chloride converts to silver and chlorine, when subjected to sunlight or heating.
Silver chloride adopts the fcc NaCl structure, in which Ag+ ions are surrounded by octahedrons of six chloride ligands.
Silver chloride is a white, curdy, crystalline solid compound.
In the lab, Silver chloride is prepared from a solution of AgNO3 by precipitation with NaCl solution.
Silver chloride is roughly 75% silver by weight.
Silver chloride melts at a temperature of 455° C and boils at 1550° C.
Silver chloride is one of the few chloride compounds known to be very insoluble in water.
Only PbCl2 and Hg2CL2 share this unique property, with PbCl2 being soluble in hot water.
Thus, selective precipitation of silver from a mixed metal ion solution is an ideal method.
Upon precipitating, Silver chloride tends to agglomerate into larger and larger masses.
This is enhanced by mild agitation.
For improving solid settling rates and obtaining clear resultant filtrate solutions from liquid/solid separations, this agglomeration enhancement principle is important.
Electrochemically, Silver chloride is quite noble.
The standard potential relative to hydrogen is 0.2223 V for the following reaction.
AgCl (S) + e- → Ag° + Cl
As such, Silver chloride may be reduced by redox couples with many less noble materials.
This knowledge has been adapted by the battery industry.
A prime example of this is the use of AgCl-Mg batteries for submarine torpedoes.
Here the redox couple and the resultant electrical energy necessary to drive the propeller is started by immersion in seawater, an excellent electrolyte.
Also, because of limited solubility and favorable electrochemical properties, Silver chloride finds use as a material in the fabrication of electrochemical reference electrodes.
Compared to the calomel or hydrogen electrode, Silver chloride is the preferred choice for most reference electrode applications.
Perhaps the greatest use of Silver chloride exploits its photochemical properties.
This is directly related to the ability of light energy to readily reduce Silver chloride to silver metal.
When exposed to light, Silver chloride turns violet at first and finally black; Silver chloride is decomposed to its elements.
This is represented as:
2AgCl (S) + light → 2Ag° + Cl2
As such, the Silver chlorides, bromides and iodides present in film form the basis for photography.
Silver chloride is a white granular powder or cubic crystals.
Silver chloride is refractive index 2.071.
Silver chloride darkens on exposure to light.
Silver chloride is density 5.56 g/cm3.
Silver chloride is Moh’s hardness 2.5.
Silver chloride is melts at 455°C.
Silver chloride is vaporizes at 1,547°C.
Silver chloride is vapor pressure 1 and 5 torr at 912 and 1,019°C.
Silver chloride is insoluble in water, alcohol and dilute acids.
Silver chloride is soluble in ammonia solution and concentrated sulfuric acid, alkali cyanide, ammonium carbonate.
Silver chloride is also soluble in potassium bromide and sodium thiosulfate solutions.
Silver chloride is a chloride of silver that occurs naturally as the mineral chlorargyrite.
Silver chloride is used to make photographic paper and pottery glazes.
Silver chloride is also found in stained glass colorants, bandages, and other wound healing products, and may be used as an antidote to mercury poisoning.
Silver is a metallic element with the chemical symbol Ag and atomic number 47.
Silver chloride occurs naturally in its pure, free form, as an alloy with gold and other metals, and in minerals such as argentite and chlorargyrite.
This white crystalline solid, Silver chloride, is well known for its low solubility in water (this behavior being reminiscent of the chlorides of Tl+ and Pb2+).
Silver chloride is described as a white crystalline chemical compound having the formula AgCl.
Silver chloride, present in the test tube, turns purplish quickly, especially in the case of a sunny laboratory due to the Silver chloride being split up into both chlorine and silver.
Silver chloride can be prepared when the sodium chloride compound is added to the silver nitrate solution; there occurs a white precipitate of Silver chloride.
Silver chloride is also an example of a well-known salt stain, which is used to impart an amber colour to the glass.
Chloro silver is the other name of Silver chloride.
Silver chloride, abbreviated as AgCl, is a chemical compound.
This white crystalline substance, Silver chloride, is well recognised for its inability to dissolve in water.
Natural sources of Silver chloride include the mineral chlorargyrite.
Because the Silver chloride is divided up into silver and chlorine, the Silver chloride in the test tube quickly turns purplish, especially in a sunny environment.
When sodium chloride is added to a silver nitrate solution, a white Silver chloride precipitate appears.
Silver chloride is a well-known salt stain used to provide amber colour to the glass.
The Silver chloride formula is a crystalline solid white.
Silver chloride is insoluble in water, alcohol, and dilute acids.
Silver chloride dissolves easily in ammonia, sulfuric acid, alkali cyanide, hydrochloric acid, and potassium bromide solution.
Silver chloride occurs naturally as a mineral, such as chlorargyrite.
Silver chloride may be made commercially by homogenising aqueous solutions of sodium chloride and silver nitrate.
Silver chloride is an inorganic photosensitive substance that is commonly used in photography.
Silver chloride has a molecular weight of 143.32 grams/mol and is a crystalline white solid.
Silver chloride has a density of 5.56 gm/cm3.
Silver chloride has a melting point of 455 °C.
Silver chloride has a boiling point of 1547 °C.
Silver chloride is a prime example of a salt that cannot dissolve in water.
Silver chloride also cannot be dissolved in dilute acids or alcohols.
Ammonia, alkali cyanides, potassium bromide, sulfuric acid, and hydrochloric acid are used to render Silver chloride soluble.
Silver chloride is a white cubic crystalline solid.
Silver chloride is nearly insoluble in water but is soluble in a water solution of ammonia, potassium cyanide, or sodium thiosulfate (“hypo”).
On exposure to light Silver chloride becomes a deep grayish blue due to its decomposition into metallic silver and atomic chlorine.
Silver chloride is a useful material for deep IR applications where sensitivity to moisture is a problem.
This soft crystal deforms under heat and pressure and can be forged in polished dies to create IR windows and lenses.
A major use for Silver chloride is in the manufacture of small disposable cell windows for spectroscopy, known as mini-cells.
These windows have a depression of controlled thickness pressed into the surface.
The inherent cost of Silver chloride material is offset against ease of manufacture.
The functioning process of Silver chloride is intricate, but Silver chloride can be simplified into several fundamental stages.
Upon exposure to an aqueous solution, silver ions within Silver chloride interact with chloride ions, resulting in the formation of Silver chloride.
This reaction is reversible, allowing Silver chloride to disintegrate into silver and chloride ions when subjected to an acidic or basic environment.
Additionally, Silver chloride has the ability to bind to proteins and other molecules within the body, leading to modifications in their structure and function.
Furthermore, upon absorption into the body, Silver chloride can engage with cells and induce alterations in their metabolism.
Silver chloride, Granular, Reagent is a chemical compound of silver and chlorine, with a molecular formula AgCl.
Silver chloride is a chemical compound with the chemical formula AgCl.
This white crystalline solid, Silver chloride, is well known for its low solubility in water.
Upon illumination or heating, Silver chloride converts to silver, which is signaled by grey to black or purplish coloration to some samples.
Silver chloride and NaCl seem to be similar, the Ag ion’s effective nuclear charge is much more compared to the Na+ ion.
Thus, according to the Fajan law, Silver chloride polarizes chloride anion and forms the bond between them more covalently (in NaCl, Na holds an overall positive charge, and chloride holds a negative charge.
Hence, there is no electron present between Cl and Na, and thus Silver chloride is not covalent.
Whereas in Cl and Ag, as polarization occurs, the electron residing on Cl- gets towards the Ag+ ion.
Therefore, some amount of electric charge comes between Cl- and Ag+ ion and this forms a covalent bond.
Uses of Silver chloride:
Silver chloride is used to make photographic paper and pottery glazes.
Silver chloride is also found in stained glass colorants, bandages, and other wound healing products, and may be used as an antidote to mercury poisoning.
Other photographic uses include making photographic paper, since Silver chloride reacts with photons to form latent images via photoreduction; and in photochromic lenses, taking advantage of its reversible conversion to Ag metal.
Unlike photography, where the photoreduction is irreversible, the glass prevents the electron from being ‘trapped’.
These photochromic lenses are used primarily in sunglasses.
Silver chloride’s low solubility makes it a useful addition to pottery glazes for the production of “Inglaze lustre”.
Silver chloride has been used as an antidote for mercury poisoning, assisting in the elimination of mercury.
Other uses of Silver chloride include:
Silver chloride is used in bandages and wound healing products, to create yellow, amber, and brown shades in stained glass manufacture, as an infrared transmissive optical component, as Silver chloride can be hot-pressed into window and lens shapes, and as an antimicrobial agent.
The most effective form of water-activated battery uses magnesium as the anode and Silver chloride as the positive electrode.
Silver chloride is used in electroplating and polishing mirrors and in making alloys.
Silver chloride is used as an antidote that reacts with the poison to produce a harmless chemical compound.
Silver chloride is used in medicines and silver salts are used in photographic films.
The most efficient type of water-activated battery employs magnesium as an anode and Silver chloride as a positive electrode.
Silver chloride’s used in mirror electroplating and polishing, as well as alloy manufacturing.
As an antidote, Silver chloride interacts with the poison to form an innocuous chemical molecule.
Silver salts are utilised in photographic films and are used in pharmaceuticals.
Because of its limited solubility, Silver chloride is a helpful additive to ceramic glazes for the development of “Inglaze lustre.”
Because Silver chloride reacts with photons to form a latent picture via photoreduction, Silver chloride is used to make photographic paper.
Silver chloride has a variety of applications, including: Photography, Electronics, Medicine, and Chemicals
Silver chloride is a compound made up of silver and chlorine.
Silver chloride is a white solid that is often used in photography.
Silver chloride is also used in some types of batteries.
Silver chloride is used in silver plating and to obtain pure silver.
Silver chloride also finds applications in photography and optics; in photochromic glass; and in electrodes and batteries.
Silver chloride is used to make antiseptic silver solution.
Silver chloride occurs as the mineral cerargyrite.
Silver chloride is used in photographic films, to coat and silver glass, as an antiseptic, and to absorb infrared light in lenses.
Silver chloride is used employed in Silver plating.
Owing to its characteristic of reversible reduction to silver metal, Silver chloride is used in photochromic lenses.
Silver chloride is used as a cathode in sea water activated batteries.
In electrochemistry, Silver chloride electrode is used for potentiometric measurements.
Silver chlorideserves as an antidote for mercury poisoning, and eliminates mercury from body.
Silver chloride is used in glass manufacturing industry.
Silver chloride is useful in the production of bandages, wound healing products and inglaze lustre, personal deodorant products, as well as for long term preservation of drinking water in water tanks; its pharmaceutical composition finds use as an antibacterial agent.
Silver chloride is very important as a linear polarizer in the infrared region (λ: 2–23 mm).
The refractive index is almost constant in the infrared region and the polarization angle is almost independent of wavelength.
The polarization angles are 63°43′ (3 mm), 63°20′ (10 mm), and 63°33′ (20 mm), showing the difference of angle below 18 for λ: 2–23 mm.
The polariscope is fabricated typically by arranging the six sheets of plates with the thickness of 0.5 mm in the shape of roof type.
Bakelite or plastic is good for the material of the holder case.
Silver chloride is used in silver plating, in making antiseptic silver preparations.
Silver chloride is found in nature as horn silver, this white powder is made by the combination of a soluble chloride and silver nitrate.
Silver bromide could also be formed by exposing metallic silver to the fumes of bromine as in the daguerreotype process.
Silver chloride is soluble in sodium thiosulfate, potassium bromide solutions, and strong ammonia.
This silver halide was the first to be observed to darken spontaneously by exposure to light.
Silver chloride formed the basis of the photogenic drawing, salted paper print, albumen print, collodion-chloride POP, gelatin chloride POP, and gaslight paper.
Silver chloride is used in photography,photometry and optics, batteries, photochromic glass,silver plating,production of pure silver, and as an antiseptic.
Single crystals are used for infrared absorption cells and lens elements and as a lab reagent.
Silver chloride has been used as an antidote for mercury poisoning, assisting in mercury elimination.
Silver chloride is used as a cathode in sea water activated batteries. In electrochemistry, Silver chloride electrode is used for potentiometric measurements.
Silver chloride is used to make a photographic paper because Silver chloride reacts with photons to produce a latent image via photoreduction.
Silver chloride is used in the photochromic lenses, again taking advantage of its reversible conversion to Ag metal.
Silver chloride is used wound healing products and in bandages.
Silver chloride is used to create amber, brown, and yellow shades in the manufacturing of stained glass.
Silver chloride is used as an infrared transmissive optical component since Silver chloride can be hot-pressed into lens shapes and window.
Silver chloride is used as an Antimicrobial Agent: For the long-term preservation of drinking water in water tanks, and In a few personal deodorant products.
There are many applications for Silver chloride, including those in electrochemistry, infra-red technology, photochromic lenses, photographic paper, as well as bandages.
Silver chloride is an analytical reagent used in some laboratory tests to determine the purity of other products and whether they can be graded pure enough for use in cosmetics, personal care, pharmaceutical or food and beverages.
This light-sensitive behavior is the basis of photographic processes.
Since silver bromide, AgBr, and silver iodide, Silver chloride, react similarly, all three of these silver halide salts are used in making photographic films and plates.
Both the bromide and iodide are less soluble in water and more sensitive to light than the chloride.
The bromide forms light yellow cubic crystals; the iodide forms yellow hexagonal or yellow-orange cubic crystals, depending on the temperature.
Besides use in photography, Silver chloride is used in silver plating, and silver iodide is used for seeding clouds.
The chloride, bromide, and iodide occur naturally as the minerals cerargyrite, bromyrite, and iodyrite, respectively.
Silver fluoride, AgF, forms colorless cubic crystals; Silver chloride is much more soluble in water than the other silver halides.
Use of Silver chloride as Electrode Material:
The brightness of a light emitting diode (LED) determined by the forward voltage (Vf) needed to make the LED light up.
The higher the Vf, the brighter the LED.
Therefore Silver chloride has a high Vf of 2.5 volts, which makes Silver chloride a good choice for an electrode material in an LED.
Photography Uses:
Silver chloride and silver nitrate have been used in photography since Silver chloride began, and are well known for their light sensitivity.
Silver chloride was also a vital part of the Daguerreotype sensitization where silver plates were fumed with chlorine to produce a thin layer of Silver chloride.
Another famous process that used Silver chloride was the gelatin silver process where embedded Silver chloride crystals in gelatin were used to produce images.
However, with advances in color photography, these methods of black-and-white photography have dwindled.
Even though color photography uses Silver chloride, it only works as a mediator for transforming light into organic image dyes.
Electrode Uses:
Silver chloride is a constituent of the Silver chloride electrode which is a common reference electrode in electrochemistry.
The electrode functions as a reversible redox electrode and the equilibrium is between the solid silver metal and Silver chloride in a chloride solution of a given concentration.
Silver chloride is usually the internal reference electrode in pH meters and Silver chloride is often used as a reference in reduction potential measurements.
As an example of the latter, the Silver chloride electrode is the most commonly used reference electrode for testing cathodic protection corrosion control systems in seawater environments.
Silver chloride is considered a convenient option to be used as a reference electrode.
In electrochemistry, the industry uses two types of electrodes to make potential measurements.
One type of electrode is called the indicator electrode which has a particular characteristic that allows the electrode to selectively respond to changes in activity of the analyte being measured.
On the other end, a reference electrode is needed in the system that possesses a characteristic which allows Silver chloride to remain stable to the changes in the activity of the analyte being measured.
In order for potential measurements to have context, the reference electrode needs to be composed in a manner that Silver chloride remains stable over time to potential changes being measured whereas the indicator electrode responds reactively.
The Silver chloride reference electrode is made up of a silver wire coated with a layer of solid Silver chloride submerged in a solution saturated with potassium chloride and Silver chloride.
Electrolyte:
Silver chloride is considered a strong electrolyte.
Silver chloride is one of the few insoluble ionic compounds that are strong electrolytes.
There is virtually no undissociated form of the Silver chloride compound in the solution as even if small amounts dissolve in water, they do so as ions only.
Get Silver chloride From Sodium Chloride:
In a double displacement reaction between aqueous silver nitrate solution and aqueous sodium chloride solution, Silver chloride and sodium nitrate are formed.
Silver nitrate solution and sodium chloride solution are both colourless solutions.
These solutions upon reaction with each other produce a white precipitate and a colourless solution.
The resultant precipitate is Silver chloride.
Then resulting compounds, Silver chloride and sodium nitrate do not react with each other.
Silver chloride can be separated from sodium nitrate by adding water to the solution to dissolve sodium nitrate because Silver chloride is soluble in water whereas the Silver chloride precipitate is not soluble in water.
Hence, Silver chloride can be obtained through separation and filtration.
Properties of Silver chloride:
Silver chloride comes in the form of a white powder.
Silver chloride has no odour.
The vapour pressure of Silver chloride is 670/1Pa.
Silver chloride’s not soluble in water.
Chemical Properties:
Silver chloride is a white,granular powder that darkens on exposure to light,finally turning black.
Silver chloride exists in several modifications differing in behavior toward light and solubility in various solvents.
Silver chloride is soluble in ammonium hydroxide, concentrated sulfuric acid, and sodium thiosulfate and potassium bromide solutions, very slightly soluble in water, can be melted, cast, and fabricated like a metal.
Silver chloride is derived by heating a silver nitrate solution and adding hydrochloric acid or salt solution.
The whole is boiled, then filtered.
This must take place in the dark or under a ruby-red light.
Silver chloride is used in photography, photometry and optics, batteries, photochromic glass,silver plating,production of pure silver, and as an antiseptic.
Single crystals are used for infrared absorption cells and lens elements and as a lab reagent
Silver chloride undergos decomposition reaction in the presence of sunlight to form silver and chlorine.
The chemical reaction is as follows.
2AgCl → 2Ag + Cl2
Silver chloride reacts with bases like ammonia forming a complex compound called Silver diammonium ion and chloride ion.
AgCl + 2NH3 → [Ag(NH3)2]+ + Cl–
Silver chloride undergoes a decomposition reaction in the presence of sunlight to produce chlorine and silver.
The chemical reaction for the same can be given as follows:
AgCl → Ag + Cl
Silver chloride reacts with a base same as ammonia, forming a complex compound known as chloride ion and Silver diammo ion.
The chemical reaction for the same can be given as follows:
AgCl + 2NH3 → [Ag(NH3)2]+ + Cl–
Purification Methods of Silver chloride:
Recrystallise Silver chloride from the conc NH3 solution by acidifying with HCl, filtering off the solid, washing Silver chloride with H2O and drying it in a vacuum.
Silver chloride is soluble in NH3 and should be kept in the dark.
Crystal System of Silver chloride:
The space lattice of Silver chloride belongs to the cubic system, and its rock salt structure has a lattice constant of a=0.554 nm, Ag–Cl=0.277 nm.
Cleavage does not occur.
Preparation of Silver chloride:
Silver chloride is prepared by slowly adding an alkali metal chloride solution to a hot solution of silver nitrate.
The solution mixture is boiled:
Ag+ (aq) + Cl¯ (aq) → AgCl (s)
The precipitate is washed with hot water.
Silver chloride is purified by dissolving in ammonia solution, filtering out any insoluble residues, and then adding hydrochloric acid to reprecipitate Silver chloride.
Preparation should be carried out in the dark in ruby red light.
Silver chloride is unusual in that, unlike most chloride salts, Silver chloride has very low solubility.
Silver chloride is easily synthesized by metathesis: combining an aqueous solution of silver nitrate (which is soluble) with a soluble chloride salt, such as sodium chloride (which is used industrially as a method of producing Silver chloride), or cobalt(II) chloride.
The Silver chloride that forms will precipitate immediately.
AgNO3+NaCl⟶AgCl↓+NaNO3
2AgNO3+CoCl2⟶2AgCl↓+Co(NO3)2
Silver chloride can also be produced by the reaction of silver metal and aqua regia; however, the insolubility of Silver chloride decelerates the reaction.
Silver chloride is also a by-product of the Miller process, where silver metal is reacted with chlorine gas at elevated temperatures.
Silver chloride is given as unusual, where in that, unlike most of the chloride salts, Silver chloride contains very low solubility.
Silver chloride can be synthesized easily by the process of metathesis, which is combining an aqueous solution of silver nitrate (soluble) with a soluble chloride salt, like cobalt(II) chloride or sodium chloride.
The formed Silver chloride will precipitate immediately.
In electrochemistry, the Silver chloride electrode is described as a common reference electrode.
Silver chloride’s low solubility makes it a useful addition to pottery glazes for the formation of “Inglaze lustre”.
History of Silver chloride:
Silver chloride has been known since ancient times.
Ancient Egyptians produced Silver chloride as a method of refining silver, which was done by roasting silver ores with salt to produce Silver chloride, which was subsequently decomposed to silver and chlorine.
However, Silver chloride was later identified as a distinct compound of silver in 1566 by Georg Fabricius.
Silver chloride, historically known as luna cornea which could be translated as “horn silver” as the moon was an alchemic codename for silver, has also been an intermediate in other historical silver refining processes.
One such example is the Augustin process developed in 1843, where copper ore containing small amounts of silver is roasted in chloridizing conditions and the Silver chloride produced is leached by brine, where Silver chloride is more soluble.
Silver-based photographic films were first made in 1727 by Johann Heinrich Schulze with silver nitrate.
However, he was not successful in making permanent images, as they faded away.
Later in 1816, the use of Silver chloride was introduced into photography by Nicéphore Niépce.
Structure of Silver chloride:
The solid adopts the fcc NaCl structure, in which each Ag+ ion is surrounded by an octahedron of six chloride ligands.
Similarly, AgBr and AGF crystallize.
However, the crystallography depends on the condition of crystallization, primarily free silver ion concentration, as is shown in the pictures left (greyish tint and metallic lustre are due to partly reduced silver).
Above 7.5 GPa, Silver chloride transitions into a monoclinic KOH phase.
Then at 11 GPa, Silver chloride undergoes another phase change to an orthorhombic TlI phase.
Reactions of Silver chloride:
Silver chloride dissolves in solutions containing ligands such as chloride, cyanide, triphenylphosphine, thiosulfate, thiocyanate and ammonia.
Silver chloride reacts with these ligands according to the following illustrative equations:
AgCl(s)+Cl−(aq)⟶AgCl2−(aq)
AgCl(s)+2S2O32−(aq)⟶(Ag(S2O3)2)3−(aq)+Cl−(aq)
AgCl(s)+2NH3(aq)⟶Ag(NH3)2+(aq)+Cl−(aq)
These reactions are used to leach Silver chloride from silver ores, cyanidation is the most commonly used, which are later converted to silver metal.
Silver chloride does not react with nitric acid, but instead reacts with sulfuric acid to produce silver sulfate.
Then the sulfate is protonated in the presence of sulfuric acid to bisulfate, which can be reversed by dilution.
This reaction is used to separate silver from other platinum group metals.
Most complexes derived from Silver chloride are two-, three-, and, in rare cases, four-coordinate, adopting linear, trigonal planar, and tetrahedral coordination geometries, respectively.
3AgCl(s)+Na3AsO3(aq)⟶Ag3AsO3(s)+3NaCl(aq)
These two reactions are particularly important in the qualitative analysis of Silver chloride in labs as Silver chloride is white, which changes to
Ag3AsO3 which is yellow, or Ag3AsO4 which is reddish brown.
Chemistry of Silver chloride:
In one of the most famous reactions in chemistry, the addition of colorless aqueous silver nitrate to an equally colorless solution of sodium chloride produces an opaque white precipitate of Silver chloride:
Ag+(aq)+Cl−(aq)⟶AgCl(s)
This conversion is a common test for the presence of chloride in solution.
Due to its conspicuousness, Silver chloride is easily used in titration, which gives the typical case of argentometry.
The solubility product, Ksp, for Silver chloride in water is 1.77×10−10 at room temperature, which indicates that only 1.9 mg (that is, 1.77×10−10 mol of Silver chloride will dissolve per liter of water.
The chloride content of an aqueous solution can be determined quantitatively by weighing the precipitated Silver chloride, which conveniently is non-hygroscopic since Silver chloride is one of the few transition metal chlorides that are unreactive toward water.
Interfering ions for this test are bromide and iodide, as well as a variety of ligands.
For AgBr and AgI, the Ksp values are 5.2 x 10−13 and 8.3 x 10−17, respectively.
Silver bromide (slightly yellowish white) and silver iodide (bright yellow) are also significantly more photosensitive than is Silver chloride.
Silver chloride quickly darkens on exposure to light by disintegrating into elemental chlorine and metallic silver.
This reaction is used in photography and film and is the following:
Cl− + hν → Cl + e− (excitation of the chloride ion, which gives up its extra electron into the conduction band)
Ag+ + e− → Ag (liberation of a silver ion, which gains an electron to become a silver atom)
The process is not reversible because the silver atom liberated is typically found at a crystal defect or an impurity site so that the electron’s energy is lowered enough that Silver chloride is “trapped”.
Natural Occurence of Silver chloride:
Silver chloride occurs naturally as chlorargyrite in the arid and oxidized zones in silver deposits.
If some of the chloride ions are replaced by bromide or iodide ions, the words bromian and iodian are added before the name, respectively.
Silver chloride is a source of silver and is leached by cyanidation, where it will produce the soluble [Ag(CN)2]– complex.
Nature of Silver chloride:
According to its chemical name, Silver chloride is very corrosive to many metals located above silver in the electrochemical series.
Silver chloride is also harmful to the environment.
When Silver chloride comes into contact with the skin, eyes, or respiratory system, Silver chloride produces irritation.
Silver chloride is also light sensitive and is utilised in the development of photographic films.
Separate Silver chloride From Water:
As Silver chloride is a white solid compound which is not soluble in water, the two can be easily separated through the filtration technique if the mixture is passed through a filter paper.
The white precipitate stuck on the filter paper as residue is Silver chloride.
The filtrate collected in the beaker at the bottom of the filter paper is water.
This water can be distilled to achieve purity.
Distillation to purify water is a process that relies on evaporation and condensation.
Contaminated water is heated to form steam, whereas molecular compounds like Silver chloride do not get evaporated and are left behind.
Then, the steam cools down to condense in the form of pure water droplets collected separately.
Handling And Storage of Silver chloride:
Conditions for safe storage, including any incompatibilities:
Storage conditions:
No metal containers.
Handle and store under inert gas.
Light sensitive.
Moisture sensitive.
Storage class:
Storage class (TRGS 510): 8B: Non-combustible,
Stability And Reactivity
Chemical stability:
Silver chloride is chemically stable under standard ambient conditions (room temperature).
First Aid Measures of Silver chloride:
General advice:
Show Silver chloride safety data sheet to the doctor in attendance.
If inhaled:
After inhalation:
Rresh 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.
Remove contact lenses.
If swallowed:
After swallowing:
Make victim drink water (two glasses at most).
Consult doctor if feeling unwell.
Indication of any immediate medical attention and special treatment needed:
No data available
Fire Fighting Measures of Silver chloride:
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.
Accidental Release Measures of Silver 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.
Exposure Controls/Personal Protection of Silver chloride:
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 P1
Control of environmental exposure:
Do not let product enter drains.
Identifiers of Silver chloride:
CAS number: 7783-90-6
EC number: 232-033-3
Hill Formula: AgCl
Chemical formula: AgCl
Molar Mass: 143.32 g/mol
HS Code: 2843 29 00
Density: 5.560 g/cm3
Melting Point: 455 °C
Vapor pressure: 1 hPa (912 °C)
Solubilit: 0.00188 g/l
Melting point: 455 °C (lit.)
Boiling point: 1550 °C
Density: 5.56
vapor pressure: 1 mm Hg ( 912 °C)
refractive index: 2.071
Flash point: 1550°C
storage temp.: Store at +5°C to +30°C.
solubility: 0.00188g/l
form: beads
color: Yellow
Specific Gravity: 5.56
Water Solubility: 1.93 mg/L (25 ºC)
Sensitive: Light Sensitive
Merck: 14,8509
Solubility Product Constant (Ksp): pKsp: 9.75
Stability: Stable, but discolours in light.
InChIKey: HKZLPVFGJNLROG-UHFFFAOYSA-M
CAS DataBase Reference: 7783-90-6(CAS DataBase Reference)
Indirect Additives used in Food Contact Substances: Silver chloride
EWG’s Food Scores: 2
FDA UNII: MWB0804EO7
NIST Chemistry Reference: Silver chloride(7783-90-6)
EPA Substance Registry System: Silver chloride (7783-90-6)
Pesticides Freedom of Information Act (FOIA): Silver chloride
Compound Formula: ClAg
Molecular Weight: 143.32
Appearance: White Powder
Melting Point: 480° C (860° F)
Boiling Point: 1,547° C (2,817° F)
Density: 5.6 g/cm3
Solubility in H2O: 520 μg/100 g (50 °C)
Properties of Silver chloride:
Chemical formula: AgCl
Molar mass: 143.32 g·mol−1
Appearance: White Solid
Density: 5.56 g cm−3
Melting point: 455 °C (851 °F; 728 K)
Boiling point: 1,547 °C (2,817 °F; 1,820 K)
Solubility in water: 520 μg/100 g at 50 °C
Solubility product (Ksp): 1.77×10−10[1]
Solubility: soluble in NH3, conc. HCl, conc.
H2SO4, alkali cyanide, (NH4)2CO3, KBr, Na2S2O3;
insoluble in alcohol, dilute acids.
Magnetic susceptibility (χ): −49.0·10−6 cm3/mol
Refractive index (nD): 2.071
Molecular Weight: 143.32 g/mol
Hydrogen Bond Donor Count: 0
Hydrogen Bond Acceptor Count: 0
Rotatable Bond Count: 0
Exact Mass: 141.87394 g/mol
Monoisotopic Mass: 141.87394 g/mol
Topological Polar Surface Area: 0 Ų
Heavy Atom Count: 2
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
AgCl: Silver chloride
Density: 5.56 g/cm³
Molecular weight/ Molar mass: 143.32 g/mol
Boiling point: 1,547 °C
Melting point: 455 °C
Chemical formula: AgCl
Odour: No odour
Appearance: White powder
Complexity: 2
Vapour pressure: 670/1Pa
Covalently-bonded Unit: 1
Solubility: Insoluble in water
Physical state: solid
Color: white
Odor: odorless
Melting point/freezing point:
Melting point/range: 455 °C – lit.
Initial boiling point and boiling range: 1.554 °C at 1.013 hPa
Flammability (solid, gas): Silver chloride 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: No data available
Viscosity
Viscosity, kinematic: No data available
Viscosity, dynamic: No data available
Water solubility: 0,00188 g/l at 25 °C
Partition coefficient: n-octanol/water:
Not applicable for inorganic substances
Vapor pressure: 1 hPa at 912 °C
Density: 5,560 g/cm3
Relative density: No data available
Relative vapor density: No data available
Particle characteristics: No data available
Refractive Index: 2
Crystal Phase / Structure: Halite
Poisson’s Ratio: 0.4
Specific Heat: 360 J/kg-K
Thermal Conductivity: 1.2 W/m-K
Thermal Expansion: 31 µm/m-K
Young’s Modulus: 20 GPa
Exact Mass: 141.874 g/mol
Monoisotopic Mass: 141.873947 Da
Chemical Formula: AgCl
Molar Mass: 143.32 g/mol
Appearance: white solid
Density: 5.5 g/cm3
Melting Point: 961 °C
Boiling Point: 1413 °C