Silver chlorate
 | |
| Names | |
|---|---|
| Other names
chloric acid silver salt | |
| Identifiers | |
7783-92-8  | |
| 3D model (Jmol) | Interactive image |
| ChemSpider | 7991255  |
| ECHA InfoCard | 100.029.122 |
| EC Number | 232-034-9 |
| PubChem | 9815505 |
| |
| |
| Properties | |
| AgClO3 | |
| Molar mass | 191.319 g/mol |
| Appearance | white crystals |
| Density | 4.443 g/cm3, solid |
| Melting point | 230 °C (446 °F; 503 K) |
| Boiling point | 250 °C (482 °F; 523 K) (decomposes) |
| slightly soluble | |
| Solubility | soluble in water and ethanol alcohol |
| Structure | |
| tetragonal | |
| Hazards | |
| NFPA 704 | |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| verify (what is ?) | |
| Infobox references | |
Silver chlorate (AgClO3) forms white, tetragonal crystals.[1][2] Like all chlorates, it is water-soluble and an oxidizing agent. As a simple metal salt, it is a common chemical in basic inorganic chemistry experiments. It is light-sensitive, so it must be stored in tightly closed dark-coloured containers.
The substance exhibits blasting properties, therefore it is sometimes use as a primary explosive.
Silver(I) means silver is in its normal +1 oxidation state.
Production
Silver chlorate is produced by the reaction of silver nitrate with sodium chlorate to produce both silver chlorate and sodium nitrate.
Alternatively, it may be produced by the transmission of chlorine through a suspension of silver oxide.
See also
References
- ↑ Náray-Szabó, St. v.; Pócza, J. (January 1942). "Die Struktur des Silberchlorats AgClO3". Zeitschrift für Kristallographie - Crystalline Materials (in German). 104 (1). doi:10.1524/zkri.1942.104.1.28.
- ↑ Deshpande, Vilas; Suryanarayana, S V; Frantz, C (December 1982). "Tetragonal to cubic phase transition in silver chlorate". Bulletin of Materials Science. 4 (5): 563–568. doi:10.1007/BF02824963.
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