Difference between revisions of "Sodium hypobromite"
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| − | | Name = Sodium | + | | Name = Sodium hypobromite pentahydrate |
| IUPACName = Sodium hypobromite — water (1/5) | | IUPACName = Sodium hypobromite — water (1/5) | ||
| OtherNames = Sodium bromate(I) | | OtherNames = Sodium bromate(I) | ||
| Section1 = {{Chembox Identifiers | | Section1 = {{Chembox Identifiers | ||
| InChI=1/BrO.Na.5H2O/c1-2;;;;;;/h;;5*1H2/q-1;+1;;;;; | | InChI=1/BrO.Na.5H2O/c1-2;;;;;;/h;;5*1H2/q-1;+1;;;;; | ||
| + | | StdInChI=1S/BrO.Na.5H2O/c1-2;;;;;;/h;;5*1H2/q-1;+1;;;;; | ||
| + | | StdInChIKey = NPFXHYUPZMEVOH-UHFFFAOYSA-N | ||
| CASNo = 13824-96-9 | | CASNo = 13824-96-9 | ||
| EINECS = 237-520-4 | | EINECS = 237-520-4 | ||
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| Section8 = {{Chembox Related | | Section8 = {{Chembox Related | ||
| OtherAnions = [[Sodium hypochlorite]] | | OtherAnions = [[Sodium hypochlorite]] | ||
| − | | OtherCations = [[Potassium hypobromite]] | + | | OtherCations = [[Lithium hypobromite]]<br/>[[Potassium hypobromite]] |
| + | | OtherCpds = [[Sodium bromide]]<br/>[[Sodium bromite]]<br/>[[Sodium bromate]]<br/>[[Sodium perbromate]] | ||
}} | }} | ||
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| − | '''Sodium hypobromite''' is the [[sodium]] [[salt]] of [[hypobromous acid]]. It can be prepared by the reaction of [[bromine]] with aqueous [[sodium hydroxide]] solution at 0 °C or lower.<ref name="C&W">{{Cotton&Wilkinson5th|pages=563–67}}.</ref><ref name="isol">{{citation | first1 = R. | last1 = Scholder | first2 = K. | last2 = Krauss | title = Über Kristallisierte Alkalihypobromite | journal = Z. Anorg. Allg. Chem. | volume = 268 | issue = 4–6 | pages = 279–90 | year = 1952 | doi = 10.1002/zaac.19522680410}}.</ref> It has long been known as a strong [[oxidizing agent]] in solution,<ref>{{citation | first = Erik | last = Troell | title = The use of Sodium Hypobromite for the Oxidation of Organic Matter in the Mechanical Analysis of Soils | journal = J. Agric. Sci. | year = 1931 | volume = 21 | pages = 476–83 | doi = 10.1017/S002185960008847X}}.</ref> but the solid pentahydrate was not isolated until | + | '''Sodium hypobromite''', NaBrO, is the [[sodium]] [[salt]] of [[hypobromous acid]]. It can be prepared by the reaction of [[bromine]] with aqueous [[sodium hydroxide]] solution at 0 °C or lower.<ref name="C&W">{{Cotton&Wilkinson5th|pages=563–67}}.</ref><ref name="isol">{{citation | first1 = R. | last1 = Scholder | first2 = K. | last2 = Krauss | title = Über Kristallisierte Alkalihypobromite | journal = Z. Anorg. Allg. Chem. | volume = 268 | issue = 4–6 | pages = 279–90 | year = 1952 | doi = 10.1002/zaac.19522680410}}.</ref> It has long been known as a strong [[oxidizing agent]] in solution,<ref>{{citation | first = Erik | last = Troell | title = The use of Sodium Hypobromite for the Oxidation of Organic Matter in the Mechanical Analysis of Soils | journal = J. Agric. Sci. | year = 1931 | volume = 21 | pages = 476–83 | doi = 10.1017/S002185960008847X}}.</ref><ref>{{citation | title = Volumetric Determinations in Strongly Alkaline Solutions. III. The Titration of Thallium and Cerium with Hypobromite | first1 = O. | last1 = Tomíček | first2 = M. | last2 = Jašek | journal = J. Am. Chem. Soc. | year = 1935 | volume = 57 | issue = 12 | pages = 2409–11 | doi = 10.1021/ja01315a026}}.</ref><ref>{{citation | title = The Oxidation of Amino Acids with Sodium Hypobromite | first1 = Alvin H. | last1 = Friedman | first2 = Sergius | last2 = Morgulis | journal = J. Am. Chem. Soc. | year = 1936 | volume = 58 | issue = 6 | pages = 909–13 | doi = 10.1021/ja01297a017}}.</ref> but the solid pentahydrate was not isolated until 1952.<ref name="isol"/> |
==Notes and references== | ==Notes and references== | ||
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===References=== | ===References=== | ||
{{reflist}} | {{reflist}} | ||
| + | |||
| + | ==External links== | ||
| + | *{{OrgSynth preps|id=34509|name=sodium hypobromite}} | ||
[[Category:Sodium compounds]] | [[Category:Sodium compounds]] | ||
Latest revision as of 08:29, 7 January 2011
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Sodium hypobromite, NaBrO, is the sodium salt of hypobromous acid. It can be prepared by the reaction of bromine with aqueous sodium hydroxide solution at 0 °C or lower.[1][2] It has long been known as a strong oxidizing agent in solution,[3][4][5] but the solid pentahydrate was not isolated until 1952.[2]
Notes and references
Notes
References
- ↑ Cotton, F. Albert; Wilkinson, Geoffrey Advanced Inorganic Chemistry, 5th ed.; Wiley-Interscience: New York, 1988; pp 563–67. ISBN 0-471-84997-9.
- ↑ 2.0 2.1 Scholder, R.; Krauss, K. Über Kristallisierte Alkalihypobromite. Z. Anorg. Allg. Chem. 1952, 268 (4–6), 279–90. DOI: 10.1002/zaac.19522680410.
- ↑ Troell, Erik The use of Sodium Hypobromite for the Oxidation of Organic Matter in the Mechanical Analysis of Soils. J. Agric. Sci. 1931, 21, 476–83. DOI: 10.1017/S002185960008847X.
- ↑ Tomíček, O.; Jašek, M. Volumetric Determinations in Strongly Alkaline Solutions. III. The Titration of Thallium and Cerium with Hypobromite. J. Am. Chem. Soc. 1935, 57 (12), 2409–11. DOI: 10.1021/ja01315a026.
- ↑ Friedman, Alvin H.; Morgulis, Sergius The Oxidation of Amino Acids with Sodium Hypobromite. J. Am. Chem. Soc. 1936, 58 (6), 909–13. DOI: 10.1021/ja01297a017.
External links
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