Silver(I) oxide
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| Silver oxide | |
|---|---|
| Image:Silver(I) oxide.jpg | |
| General | |
| Systematic name | Silver oxide |
| Other names | Silver rust |
| Molecular formula | Ag2O |
| Molar mass | 231.7148 g/mol |
| Appearance | black/brown solid |
| CAS number | 20667-12-3 |
| Properties | |
| Density and phase | 7.2 g/cm3, solid |
| Solubility in water | 0.0013 g/100 ml (20°C) |
| Solubility Product (of AgOH) | Ksp = 1.52 × 10-8 (20°C) |
| Melting point | 200°C, decomposition |
| Structure | |
| Molecular shape | ? |
| Coordination geometry |
? |
| Crystal structure | cubic |
| Dipole moment | ? D |
| Hazards | |
| MSDS | External MSDS |
| Main hazards | ? |
| NFPA 704 | |
| Flash point | ? °C |
| R/S statement | R: ? S: ? |
| RTECS number | ? |
| Supplementary data page | |
| Structure and properties |
n, εr, etc. |
| Thermodynamic data |
Phase behaviour Solid, liquid, gas |
| Spectral data | UV, IR, NMR, MS |
| Related compounds | |
| Other anions | ? |
| Other cations | ? |
| Related compounds | silver(II) oxide, AgO |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references |
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Silver oxide, also known as silver rust and argentous oxide, is a chemical compound with formula Ag2O and CAS number 20667-12-3. It is used in a silver-oxide battery.
Silver oxide is prepared by precipitating it from an aqueous solution of silver nitrate by the action of an alkali hydroxide.[1] It is poorly soluble in water (1 part in 40,000), but dissolves in nitric acid solution and ammonium hydroxide solution, and is slightly soluble in aqueous solutions of alkali hydroxides. It is insoluble in alcohol and nonpolar solvents.[2] Solution in alkali hydroxide solutions is due to the formation of the ion, Ag(OH)2–.[3] Silver oxide dissolved in neutral aqueous solution exists as an ionized hydroxide (Ag+ OH–).[1]
Silver oxide reacts with solutions of HF, HCl, HBr, or HI to form the respective silver halides. It will also react with solutions of alkali chlorides to precipitate silver chloride, leaving a solution of the corresponding alkali hydroxide.[1][3]
Like many silver compounds, silver oxide decomposes on exposure to light into its constituents. It also decomposes at temperatures above 200°C.[2]
[edit] References
- ^ a b c General Chemistry by Linus Pauling, 1970 Dover ed. p703-704
- ^ a b Merck Index of Chemicals and Drugs, 9th ed. monograph 8265
- ^ a b Advanced Inorganic Chemistry by Cotton and Wilkinson, 2nd ed. p1042
[edit] External links
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