Difference between revisions of "Rubidium bromate"
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| OtherAnions = [[Rubidium chlorate]]<br/>[[Rubidium iodate]] | | OtherAnions = [[Rubidium chlorate]]<br/>[[Rubidium iodate]] | ||
| − | | OtherCations = [[Sodium bromate]]<br/>[[Potassium bromate]]<br/>[[Caesium bromate]] | + | | OtherCations = [[Lithium bromate]]<br/>[[Sodium bromate]]<br/>[[Potassium bromate]]<br/>[[Caesium bromate]] |
| − | | OtherCpds = [[Rubidium bromide]] | + | | OtherCpds = [[Rubidium bromide]]<br/>[[Rubidium perbromate]] |
}} | }} | ||
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Latest revision as of 06:31, 5 January 2011
| Rubidium bromate | |
|---|---|
| IUPAC name | Rubidium bromate |
| Other names | Rubidium bromate(V) |
| Identifiers | |
| InChI | InChI=1/BrHO3.Rb/c2-1(3)4;/h(H,2,3,4);/q;+1/p-1 |
| InChIKey | LACSDIAFVPRAER-REWHXWOFAI |
| Standard InChI | InChI=1S/BrHO3.Rb/c2-1(3)4;/h(H,2,3,4);/q;+1/p-1 |
| Standard InChIKey | LACSDIAFVPRAER-UHFFFAOYSA-M |
| CAS number | [] |
| ChemSpider | |
| Properties[1] | |
| Chemical formula | RbBrO3 |
| Molar mass | 213.37 g mol−1 |
| Appearance | white crystalline solid |
| Density | 3.68 g cm−3 |
| Melting point |
430 °C |
| Solubility in water | 2.93 g/100 g (25 °C) 5.08 g/100 g (40 °C) |
| Related compounds | |
| Other anions | Rubidium chlorate Rubidium iodate |
| Other cations | Lithium bromate Sodium bromate Potassium bromate Caesium bromate |
| Other compounds | Rubidium bromide Rubidium perbromate |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
Rubidium bromate, RbBrO3, is the rubidium salt of bromic acid.
Preparation
Rubidium bromate is usually prepared by the electrolysis of rubidium 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 rubidium bromate can be crystallized by cooling the electrolyte, and any unoxidized bromide recycled.[3]
Rubidium bromate can also be prepared by reacting bromine with rubidium 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-139. 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
- Buell, Harold D.; McCrosky, C. R. The Preparation and Study of the Rarer Alkali Bromates. Rubidium Bromate. J. Am. Chem. Soc. 1921, 43 (9), 2031–34. DOI: 10.1021/ja01442a006.
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