Silver carbonate

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Silver carbonate
Names
IUPAC name
Silver carbonate
Other names
Disilver carbonate
Silver(I) carbonate
Properties
Ag2CO3
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
0.031 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
Thermochemistry
167.4 J·mol-1·K-1
−505.8 kJ/mol
Hazards
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.

Properties

Chemical

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.

Physical

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.

Availability

Silver carbonate is sold by various suppliers, but it's not cheap.

Preparation

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

Projects

  • Make silver fulminate
  • Make silver mirror
  • Catalyst in Koenigs–Knorr reaction
  • Oxidizer in Fétizon oxidation

Handling

Safety

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.

Storage

In closed opaque plastic or dark amber glass bottles, in a dark place, away from light.

Disposal

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

References

Relevant Sciencemadness threads