Difference between revisions of "Barium bromate"
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| StdInChI=1S/Ba.2BrHO3/c;2*2-1(3)4/h;2*(H,2,3,4)/q+2;;/p-2 | | StdInChI=1S/Ba.2BrHO3/c;2*2-1(3)4/h;2*(H,2,3,4)/q+2;;/p-2 | ||
| StdInChIKey = VEASZGAADGZARC-UHFFFAOYSA-L | | StdInChIKey = VEASZGAADGZARC-UHFFFAOYSA-L | ||
| + | | CASNo = 13967-90-3 | ||
| + | | EINECS = 237-750-5 | ||
}} | }} | ||
| Section2 = {{Chembox Properties | | Section2 = {{Chembox Properties | ||
| Line 16: | Line 18: | ||
| 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]] | ||
}} | }} | ||
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| StdInChIKey = SRLAISWMODXCQE-UHFFFAOYSA-L | | StdInChIKey = SRLAISWMODXCQE-UHFFFAOYSA-L | ||
| CASNo = 10326-26-8 | | CASNo = 10326-26-8 | ||
| + | | EINECS = 237-750-5 | ||
}} | }} | ||
| Section2 = {{Chembox Properties | | Section2 = {{Chembox Properties | ||
| − | | Reference = <ref name="Kirk-Othmer"/><ref>{{RubberBible62nd|page=B-80}}</ref> | + | | Reference = <ref name="Kirk-Othmer"/><ref>{{RubberBible62nd|page=B-80}}.</ref> |
| Formula = Ba(BrO<sub>3</sub>)<sub>2</sub>·H<sub>2</sub>O | | Formula = Ba(BrO<sub>3</sub>)<sub>2</sub>·H<sub>2</sub>O | ||
| MolarMass = 411.15 g mol<sup>−1</sup> | | MolarMass = 411.15 g mol<sup>−1</sup> | ||
| Line 40: | 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 46: | Line 67: | ||
==Preparation== | ==Preparation== | ||
| − | Barium bromate is usually prepared by the electrolysis of [[ | + | Barium bromate is usually prepared by the electrolysis of [[barium bromide]] solution at 65–70 °C, in the presence of [[dichromate]] and using [[anode]]s of [[lead dioxide]] or [[iron]] and [[cathode]]s of [[stainless steel]] or [[copper]].<ref>{{citation | first1 = Takasi | last1 = Osuga | first2 = Kiichiro | last2 = Sugino | title = Electrolytic Production of Bromates | journal = J. Electrochem. Soc. | volume = 104 | issue = 7 | pages = 448–51 | year = 1957 | doi = 10.1149/1.2428623}}.</ref> The barium bromate can be crystallized by cooling the electrolyte, and any unoxidized bromide recycled.<ref name="Kirk-Othmer"/> |
| − | Barium bromate can also be prepared by reacting [[bromine]] with [[ | + | Barium bromate can also be prepared by reacting [[bromine]] with [[barium hydroxide]] solution at 50–90 °C.<ref name="Kirk-Othmer"/><ref name="IL84830">{{citation | inventor1-first = Aavi | inventor1-last = Prager | inventor2-first = Shaul | inventor2-last = Smilovitch | inventor3-first = Mira | inventor3-last = Freiberg | inventor4-first = Haim | inventor4-last = Hariton | assignee = Bromine Compounds Ltd. | title = Alkali and alkaline earth metal bromide and bromate solid mixtures and process for preparation thereof | country-code = IL | patent-number = 84830 | publication-date = 1995-01-24}}.</ref> |
:3 Br<sub>2</sub> + 3 OH<sup>−</sup> {{eqm}} BrO{{su|b=3|p=−}} + 5 Br<sup>−</sup> + 3 H<sup>+</sup> | :3 Br<sub>2</sub> + 3 OH<sup>−</sup> {{eqm}} BrO{{su|b=3|p=−}} + 5 Br<sup>−</sup> + 3 H<sup>+</sup> | ||
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===References=== | ===References=== | ||
{{reflist}} | {{reflist}} | ||
| + | |||
| + | ==External links== | ||
| + | *{{EHC|107|name=Barium}} | ||
| + | *{{HSG|046|name=Barium}} | ||
[[Category:Barium compounds]] | [[Category:Barium compounds]] | ||
Latest revision as of 12:51, 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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