| IUPAC name
| Other names
|Appearance||Pale yellow solid|
|Melting point||218 °C (424 °F; 491 K) (decomposition begins around 120 °C)|
| 0.031 g/L (15 °C)|
0.032 g/L (25 °C)
0.5 g/L (100 °C)
|Solubility|| Reacts with acids|
Insoluble in acetone, liq. ammonia, chloroform, ethanol, ethyl acetate, methanol, toluene, xylene
Std enthalpy of
|Safety data sheet||Sigma-Aldrich|
|Lethal dose or concentration (LD, LC):|
LD50 (Median dose)
|3,730 mg/kg (mice, oral)|
| Silver nitrate|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Silver carbonate is a silver chemical compound with the formula Ag2CO3.
Like all other carbonates, silver carbonate will react with acids to give their respective silver salts and give off carbon dioxide.
- Ag2CO3 + 2 HNO3 → 2 AgNO3 + H2O + CO2
- 4 Ag2CO3 + 4 NH3 → 4 AgCNO + 6 H2O + 4 Ag + O2
No conditions are given for this reaction.
Silver carbonate is colorless solid which quickly turns yellow upon exposure to light and finally brown if kept too much in light. It is poorly soluble in water and organic solvents. Silver carbonate will decompose if heated above the boiling point of water.
Silver carbonate is sold by various suppliers, but it's not cheap.
Silver carbonate can be prepared by reacting a mixture of silver nitrate with another of sodium carbonate. Since silver carbonate is less soluble, it will precipitate, while sodium nitrate will remain in solution.
- 2 AgNO3 + Na2CO3 → Ag2CO3 + 2 NaNO3
- Make silver fulminate
- Make silver mirror
- Catalyst in Koenigs–Knorr reaction
- Oxidizer in Fétizon oxidation
Silver carbonate is light-sensitive, decomposition begins in seconds after synthesis under light and tends to stain. Wear proper protection when handling the compound. Ingestion of the compound may lead to argyria.
In closed opaque plastic or dark amber glass bottles, in a dark place, away from light.