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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.
3D model (JSmol)
CompTox Dashboard (EPA)
|Molar mass||143.32 g·mol−1|
|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)|
|520 μg/100 g at 50 °C|
Solubility product (Ksp)
|Solubility||soluble in NH3, conc. HCl, conc. H2SO4, alkali cyanide, (NH4)2CO3, KBr, Na2S2O3;|
Refractive index (nD)
Std enthalpy of
|Safety data sheet||Fischer Scientific, Salt Lake Metals|
|NFPA 704 (fire diamond)|
|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).
|what is ?)(|
Silver chloride is unusual in that, unlike most chloride salts, it has very low solubility. It is easily synthesized by metathesis: combining an aqueous solution of silver nitrate (which is soluble) with a soluble chloride salt, such as sodium chloride or cobalt(II) chloride. The silver chloride that forms will precipitate immediately.
Structure and reactionsEdit
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. 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:
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.
Above 2 reactions are particularly important in qualitative analysis of AgCl in labs as AgCl is white in colour , which changes to (silver arsenite) which is yellow in colour or (Silver arsenate) which is reddish brown in colour.
The solubility product, Ksp, for AgCl in water is 1.77×10−10 at room temperature, which indicates that only 1.9 mg (that is, ) 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 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 AgCl.
- 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
- as an antimicrobial agent:
- in some personal deodorant products
- for long-term preservation of drinking water in water tanks
- John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–189. ISBN 1138561630.
- Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23. ISBN 978-0-618-94690-7.
- Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
- More info on Chlorine test Archived December 3, 2007, at the Wayback Machine
- "Silver Chloride (AgCl) Optical Material". www.crystran.co.uk. Archived from the original on September 5, 2012. Retrieved 2019-12-04.