Silver carbonate

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Silver carbonate
IUPAC name
Silver carbonate
Other names
Disilver carbonate
Silver(I) carbonate
Molar mass 275.75 g/mol
Appearance Pale yellow solid
Odor Odorless
Density 6.077 g/cm3
Melting point 218 °C (424 °F; 491 K) (decomposition begins around 120 °C)
Boiling point Decomposes
0.0031 g/100 ml (15 °C)
0.0032 g/100 ml (25 °C)
0.05 g/100 ml (100 °C)
Solubility Reacts with acids
Insoluble in acetone, liq. ammonia, chloroform, ethanol, ethyl acetate, methanol, toluene, xylene
Vapor pressure ~0 mmHg
167.4 J·mol-1·K-1
−505.8 kJ/mol
Safety data sheet Sigma-Aldrich
Lethal dose or concentration (LD, LC):
3,730 mg/kg (mice, oral)
Related compounds
Related compounds
Silver nitrate
Silver perchlorate
Silver sulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

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

Silver carbonate reacts with ammonia to give the explosive silver fulminate.

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 practically insoluble in water, it will precipitate out of the solution, 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.


Adding a reducing agent, such as formaldehyde or ascorbic acid will cause it to decompose to metallic silver which can be recycled.


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