Difference between revisions of "Barium bromate"
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| Appearance = white crystalline solid | | Appearance = white crystalline solid | ||
| MeltingPt = 270 °C ''decomp.'' | | MeltingPt = 270 °C ''decomp.'' | ||
| + | }} | ||
| + | | Section7 = {{Chembox Hazards | ||
| + | | Reference = <ref name="CLP">{{CLP Regulation|index=056-002-00-7|page=438}}</ref><ref name="PEL">{{29CFR1910.1000Z1|entry=Barium, soluble compounds (as Ba)}}.</ref> | ||
| + | | EUIndex = 056-002-00-7 | ||
| + | | GHSPictograms = {{GHS07|Acute Tox. 4 (oral, inhal.)}} | ||
| + | | GHSSignalWord = WARNING | ||
| + | | HPhrases = {{H-phrases|302|332}} | ||
| + | | PPhrases = {{P-phrases|261|264|270|271|301+312|304+340|330|501}} | ||
| + | | PEL = 0.5 mg m<sup>−3</sup> TWA (as Ba) | ||
}} | }} | ||
| Section8 = {{Chembox Related | | Section8 = {{Chembox Related | ||
| OtherAnions = [[Barium chlorate]]<br/>[[Barium iodate]] | | OtherAnions = [[Barium chlorate]]<br/>[[Barium iodate]] | ||
| − | | OtherCations = [[Calcium bromate]]<br/>[[Strontium bromate]] | + | | OtherCations = [[Magnesium bromate]]<br/>[[Calcium bromate]]<br/>[[Strontium bromate]] |
| OtherCpds = [[Barium bromide]]<br/>[[Barium hypobromite]]<br/>[[Barium bromite]] | | OtherCpds = [[Barium bromide]]<br/>[[Barium hypobromite]]<br/>[[Barium bromite]] | ||
}} | }} | ||
| Line 43: | Line 52: | ||
| Density = 3.99 g cm<sup>−3</sup> (18 °C) | | Density = 3.99 g cm<sup>−3</sup> (18 °C) | ||
| Solubility = 0.3 g/100 g (0 °C)<br/>5.67 g/100 g (100 °C) | | Solubility = 0.3 g/100 g (0 °C)<br/>5.67 g/100 g (100 °C) | ||
| + | }} | ||
| + | | Section7 = {{Chembox Hazards | ||
| + | | Reference = <ref name="CLP"/><ref name="PEL"/> | ||
| + | | EUIndex = 056-002-00-7 | ||
| + | | GHSPictograms = {{GHS07|Acute Tox. 4 (oral, inhal.)}} | ||
| + | | GHSSignalWord = WARNING | ||
| + | | HPhrases = {{H-phrases|302|332}} | ||
| + | | PPhrases = {{P-phrases|261|264|270|271|301+312|304+340|330|501}} | ||
| + | | PEL = 0.5 mg m<sup>−3</sup> TWA (as Ba) | ||
}} | }} | ||
}} | }} | ||
| Line 66: | Line 84: | ||
===References=== | ===References=== | ||
{{reflist}} | {{reflist}} | ||
| + | |||
| + | ==External links== | ||
| + | *{{EHC|107|name=Barium}} | ||
| + | *{{HSG|046|name=Barium}} | ||
[[Category:Barium compounds]] | [[Category:Barium compounds]] | ||
Latest revision as of 11:51, 8 January 2011
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Barium bromate, Ba(BrO3)2, is the barium salt of bromic acid. It is used as a corrosion inhibitor.[1]
Contents
Preparation
Barium bromate is usually prepared by the electrolysis of barium 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.[5] The barium bromate can be crystallized by cooling the electrolyte, and any unoxidized bromide recycled.[1]
Barium bromate can also be prepared by reacting bromine with barium hydroxide solution at 50–90 °C.[1][6]
- 3 Br2 + 3 OH− ⇌ BrO−3 + 5 Br− + 3 H+
Decomposition
Anhydrous barium bromate decomposes at about 270 °C to give barium bromide and oxygen:[1]
- Ba(BrO3)2 → BaBr2 + 3 O2
Controlled decomposition in vacuo at 250 °C gives barium bromite:[7]
- Ba(BrO3)2 → Ba(BrO2)2 + O2
Notes and references
Notes
References
- ↑ 1.0 1.1 1.2 1.3 1.4 1.5 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.
- ↑ 2.0 2.1 Index no. 056-002-00-7 of Annex VI, Part 3, to Regulation (EC) No 1272/2008 of the European Parliament and of the Council of 16 December 2008 on classification, labelling and packaging of substances and mixtures, amending and repealing Directives 67/548/EEC and 1999/45/EC, and amending Regulation (EC) No 1907/2006. OJEU L353, 31.12.2008, pp 1–1355 at p 438.
- ↑ 3.0 3.1 "Barium, soluble compounds (as Ba)" in 29 C.F.R. § 1910.1000 Table Z-1, 54 FR 36767, September 5, 1989, as amended.
- ↑ CRC Handbook of Chemistry and Physics, 62nd ed.; Weast, Robert C., Ed.; CRC Press: Boca Raton, FL, 1981; p B-80. 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.
- ↑ 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.
- ↑ Downs, A. J.; Adams, C. J. In Comprehensive Inorganic Chemistry; Bailar, J. C., Jr.; Emeleus, H. J.; Nyholm, R., et al., Eds.; Pergamon: Oxford, 1973; Vol. 2, pp 1419–20.
External links
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