Silver carbonate
Silver carbonate | |
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Other names none | |
Identifiers | |
CAS number | 534-16-7 |
PubChem | 92796 |
ChemSpider | 83768 |
EC number | 208-590-3 |
MeSH | silver+carbonate |
Jmol-3D images | {{#if:[Ag]OC(=O)O[Ag]|Image 1 |
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Properties | |
Molecular formula | Ag 2CO 3 |
Molar mass | 275.7453 g mol-1 |
Appearance | Pale yellow crystals |
Density | 6.077 g cm-3 |
Melting point | 210 °C; 410 °F; 483 K (decomposes) |
Solubility in water | 0.0032 g/100 mL |
Thermochemistry | |
Std enthalpy of formation ΔfH |
-506 kJ/mol |
Specific heat capacity, C | 112.5 J/mol K |
Hazards | |
MSDS | External MSDS from Salt Lake Metals |
NFPA 704 |
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(verify) (what is: / ?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa) | |
Infobox references | |
Silver carbonate is the chemical compound with the formula Ag2CO3. Silver carbonate is yellow but typical samples are grayish due to the presence of elemental silver. It is poorly soluble in water, like most transition metal carbonates. Silver carbonate is used as a reagent in organic synthesis such as the Koenigs-Knorr reaction. In the Fétizon oxidation, silver carbonate on celite acts as an oxidising agent to form lactones from diols. It is also employed to convert alkyl bromides into alcohols.[1]
Preparation
Silver carbonate can be easily prepared by combining aqueous solutions of sodium carbonate and silver nitrate.
References
- ↑ McCloskey C. M.; Coleman, G. H. (1955), "β-d-Glucose-2,3,4,6-Tetraacetate", Org. Synth.; Coll. Vol. 3: 434
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