Difference between revisions of "Caesium bromate"
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| OtherAnions = [[Caesium chlorate]]<br/>[[Caesium iodate]] | | OtherAnions = [[Caesium chlorate]]<br/>[[Caesium iodate]] | ||
| OtherCations = [[Lithium bromate]]<br/>[[Sodium bromate]]<br/>[[Potassium bromate]]<br/>[[Rubidium bromate]] | | OtherCations = [[Lithium bromate]]<br/>[[Sodium bromate]]<br/>[[Potassium bromate]]<br/>[[Rubidium bromate]] | ||
| − | | OtherCpds = [[Caesium bromide]] | + | | OtherCpds = [[Caesium bromide]]<br/>[[Caesium perbromate]] |
}} | }} | ||
}} | }} | ||
Latest revision as of 06:31, 5 January 2011
| Caesium bromate | |
|---|---|
| IUPAC name | Caesium bromate |
| Other names | Caesium bromate(V) |
| Identifiers | |
| InChI | InChI=1/BrHO3.Cs/c2-1(3)4;/h(H,2,3,4);/q;+1/p-1 |
| InChIKey | LCIQMVZXQUMARP-REWHXWOFAF |
| Standard InChI | InChI=1S/BrHO3.Cs/c2-1(3)4;/h(H,2,3,4);/q;+1/p-1 |
| Standard InChIKey | LCIQMVZXQUMARP-UHFFFAOYSA-M |
| CAS number | [] |
| ChemSpider | |
| Properties[1] | |
| Chemical formula | CsBrO3 |
| Molar mass | 260.81 g mol−1 |
| Appearance | white crystalline solid |
| Density | 4.109 g cm−3 |
| Melting point |
420 °C decomp. |
| Solubility in water | 3.66 g/100 g (25 °C) 5.32 g/100 g (35 °C) |
| Related compounds | |
| Other anions | Caesium chlorate Caesium iodate |
| Other cations | Lithium bromate Sodium bromate Potassium bromate Rubidium bromate |
| Other compounds | Caesium bromide Caesium perbromate |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
Caesium bromate, CsBrO3, is the caesium salt of bromic acid.
Preparation
Caesium bromate is usually prepared by the electrolysis of caesium bromide solution at 65–70 °C, in the presence of dichromate and using anodes of lead dioxide or iron and cathodes of stainless steel or copper.[2] The caesium bromate can be crystallized by cooling the electrolyte, and any unoxidized bromide recycled.[3]
Caesium bromate can also be prepared by reacting bromine with caesium hydroxide solution at 50–90 °C.[4]
- 3 Br2 + 3 OH− ⇌ BrO−3 + 5 Br− + 3 H+
Notes and references
Notes
References
- ↑ CRC Handbook of Chemistry and Physics, 62nd ed.; Weast, Robert C., Ed.; CRC Press: Boca Raton, FL, 1981; p B-91. ISBN 0-8493-0462-8.
- ↑ Osuga, Takasi; Sugino, Kiichiro Electrolytic Production of Bromates. J. Electrochem. Soc. 1957, 104 (7), 448–51. DOI: 10.1149/1.2428623.
- ↑ Ukeles, S. D.; Freiberg, M. Bromine, Inorganic Compounds. In Kirk-Othmer Encyclopedia of Chemical Technology; John Wiley: New York, 2002. DOI: 10.1002/0471238961.021815131001031.
- ↑ Prager, Aavi; Smilovitch, Shaul; Freiberg, Mira, et al. (Bromine Compounds Ltd.) Alkali and alkaline earth metal bromide and bromate solid mixtures and process for preparation thereof. IL Patent 84830, published 24 January 1995.
Further reading
- McCrosky, C. R.; Buell, Harold D. The Preparation and Study of the Rarer Alkali Bromates. Cesium Bromate. J. Am. Chem. Soc. 1920, 42 (9), 1786–89. DOI: 10.1021/ja01454a005.
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