| IUPAC name
| Other names
|Molar mass||143.32 g/mol|
|Melting point||455 °C (851 °F; 728 K)|
|Boiling point||1,547 °C (2,817 °F; 1,820 K)|
|0.00052 g/100 ml (50 °C)|
|Solubility||Soluble in NH3, conc. HCl, conc. H2SO4, alkali cyanide|
|Vapor pressure||~0 mmHg|
Std enthalpy of
|Safety data sheet||Sigma-Aldrich|
|Lethal dose or concentration (LD, LC):|
LD50 (Median dose)
|5,000 mg/kg (rat, oral)|
| Silver(I) fluoride|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Silver chloride is an inorganic chemical compound with the chemical formula AgCl. The compound is known for its extremely low water solubility.
- 2 AgCl → 2 Ag + Cl2
Silver chloride is an insoluble white solid, which slowly decomposes when exposed to light.
Silver chloride is sold by chemical suppliers. Since it's a silver compound, it's not very cheap.
AgCl occurs naturally as a mineral chlorargyrite.
Silver chloride is extremely easy to prepare by metathesis reaction: a soluble chloride salt, like NaCl is added as solution to a solution of a soluble silver salt, such as silver nitrate. Due to its extremely low solubility, silver chloride will precipitate out of the solution, and can be filtered from the resulting suspension, washed and then dried.
- AgNO3 + NaCl → NaNO3 + AgCl
- Make photographic paper (photography)
- Silver chloride electrode (common reference electrode in electrochemistry)
- Pottery glazes ("Inglaze lustre")
- Antidote for mercury poisoning
- Compound collecting
Silver chloride may be harmful if ingested in large amounts, but usually it doesn't pose a serious health risk. May cause silver stains though.
In closed amber glass or plastic bottles, away from light and reducing agents.
Since silver is expensive, AgCl should be recycled. This can be done by reducing the compound to Ag metal, which is then collected and stored for further uses.