Silver chloride

Silver chloride is a chemical compound with the chemical formula AgCl. This white crystalline solid is well known for its low solubility in water (this behavior being reminiscent of the chlorides of Tl⁺ and Pb²⁺). Upon illumination or heating, silver chloride converts to silver (and chlorine), which is signaled by grey to black or purplish coloration to some samples. AgCl occurs naturally as a mineral chlorargyrite.

Silver chloride

Names
IUPAC name Silver chloride
Other names cerargyrite chlorargyrite horn silver
Identifiers
CAS Number	7783-90-6^Y
3D model (JSmol)	Interactive image
ChEBI	CHEBI:30341^Y
ChemSpider	22967^Y
ECHA InfoCard	100.029.121
PubChem CID	24561
RTECS number	VW3563000
UNII	MWB0804EO7^Y
CompTox Dashboard (EPA)	DTXSID4035251
InChI InChI=1S/Ag.ClH/h;1H/q+1;/p-1^Y Key: HKZLPVFGJNLROG-UHFFFAOYSA-M^Y InChI=1S/Ag.ClH/h;1H/q+1;/p-1 Key: HKZLPVFGJNLROG-UHFFFAOYSA-M
SMILES Cl[Ag]
Properties
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	soluble in NH3, conc. HCl, conc. H2SO4, alkali cyanide, NH4CO3^?, KBr, Na2S2O3; insoluble in alcohol, dilute acids.
Magnetic susceptibility (χ)	−49.0·10^−6 cm^3/mol
Refractive index (nD)	2.071
Structure
Crystal structure	halite
Thermochemistry
Std molar entropy (S^o298)	96 J·mol^−1·K^−1[1]
Std enthalpy of formation (ΔfH^⦵298)	−127 kJ·mol^−1[1]
Hazards
Safety data sheet	Fischer Scientific, Salt Lake Metals
NFPA 704 (fire diamond)	0 2 0
Related compounds
Other anions	silver(I) fluoride, silver bromide, silver iodide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is ^YN ?)
Infobox references

Preparation

Silver chloride is easily synthesized by combining aqueous solutions of silver nitrate and sodium chloride.

${\displaystyle {\ce {AgNO3 + NaCl -> AgCl(v) + NaNO3}}}$

It can also be produced by reacting silver nitrate with cobalt(II) chloride. This precipitation is general for silver nitrate's reaction with soluble chloride salts and is not unique simply to cobalt.

${\displaystyle {\ce {2 AgNO3 + CoCl2 -> 2 AgCl(v) + Co(NO3)2}}}$

Structure and reactions

Silver chloride crystals

Pyramidal crystals of AgCl

The solid adopts the fcc NaCl structure, in which each Ag⁺ ion is surrounded by an octahedron of six chloride ligands. AgF and AgBr crystallize similarly.[2] However, the crystallography depends on the condition of crystallization, primarily free silver ion concentration, as is shown on the pictures left (greyish tint and metallic lustre are due to partly reduced silver). AgCl 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:

${\displaystyle {\ce {AgCl (s) + Cl^- (aq) -> AgCl2^- (aq)}}}$

${\displaystyle {\ce {AgCl (s) + 2 S2O3^2- (aq) ->(Ag(S2O3)2)^3- (aq) + Cl^- (aq)}}}$

${\displaystyle {\ce {AgCl (s) + 2 NH3(aq) -> Ag(NH3)2+ (aq) + Cl^- (aq)}}}$

Silver chloride does not react with nitric acid. Most complexes derived from AgCl are two-, three-, and, in rare cases, four-coordinate, adopting linear, trigonal planar, and tetrahedral coordination geometries, respectively.

${\displaystyle {\ce {3AgCl(s) + Na3AsO3(aq) -> Ag3AsO3(s) + 3NaCl(aq)}}}$

${\displaystyle {\ce {3AgCl(s) +Na3AsO4(aq) -> Ag3AsO4(s) + 3NaCl(aq)}}}$

Above 2 reactions are particularly important in qualitative analysis of AgCl in labs as AgCl is white in colour , which changes to ${\displaystyle {\ce {Ag3AsO3}}}$ (silver arsenite) which is yellow in colour or ${\displaystyle {\ce {Ag3AsO4}}}$(Silver arsenate) which is reddish brown in colour.

Chemistry

Silver chloride decomposes over time with exposure to UV light

In one of the most famous reactions in chemistry, addition of colorless aqueous silver nitrate to an equally colorless solution of sodium chloride produces an opaque white precipitate of AgCl:[3]

${\displaystyle {\ce {Ag+ (aq) + Cl^- (aq) -> AgCl (s)}}}$

This conversion is a common test for the presence of chloride in solution. Due to its conspicuousness it is easily used in titration, which gives the typical case of argentometry.

The solubility product, K_sp, for AgCl in water is 1.77×10⁻¹⁰ at room temperature, which indicates that only 1.9 mg (that is, ${\displaystyle {\sqrt {1.77\times 10^{-10}}}\ \mathrm {mol} }$) of AgCl will dissolve per liter of water. The chloride content of an aqueous solution can be determined quantitatively by weighing the precipitated AgCl, which conveniently is non-hygroscopic, since AgCl is one of the few transition metal chlorides that is unreactive toward water. Interfering ions for this test are bromide and iodide, as well as a variety of ligands (see silver halide). For AgBr and AgI, the K_sp 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 AgCl.

AgCl quickly darkens on exposure to light by disintegrating into elemental chlorine and metallic silver. This reaction is used in photography and film.

Uses

• The silver chloride electrode is a common reference electrode in electrochemistry.
• 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.
• Silver chloride is used:
  • to make photographic paper since it reacts with photons to form latent image and via photoreduction
  • in photochromic lenses, again taking advantage of its reversible conversion to Ag metal
  • in bandages and wound healing products
  • to create yellow, amber, and brown shades in stained glass manufacture
  • as an infrared transmissive optical component as it can be hot-pressed into window and lens shapes[4]
  • as an antimicrobial agent:
    • in some personal deodorant products
    • for long-term preservation of drinking water in water tanks

See also

• Photosensitive glass

References

1. Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23. ISBN 978-0-618-94690-7.
2. Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
3. More info on Chlorine test Archived December 3, 2007, at the Wayback Machine
4. "Silver Chloride (AgCl) Optical Material". www.crystran.co.uk. Archived from the original on September 5, 2012. Retrieved 2019-12-04.