Difference between revisions of "Barium bromate"
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{{chembox | {{chembox | ||
| IUPACName = Barium bromate | | IUPACName = 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 | ||
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}} | }} | ||
| Section2 = {{Chembox Properties | | Section2 = {{Chembox Properties | ||
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| Appearance = white crystalline solid | | Appearance = white crystalline solid | ||
| MeltingPt = 270 °C ''decomp.'' | | MeltingPt = 270 °C ''decomp.'' | ||
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}} | }} | ||
| Section8 = {{Chembox Related | | Section8 = {{Chembox Related | ||
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}} | }} | ||
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| + | {{chembox | ||
| + | | Name = Barium bromate monohydrate | ||
| + | | IUPACName = Barium bromate — water (1/1) | ||
| + | | Section1 = {{Chembox Identifiers | ||
| + | | StdInChI=1S/Ba.2BrHO3.H2O/c;2*2-1(3)4;/h;2*(H,2,3,4);1H2/q+2;;;/p-2 | ||
| + | | StdInChIKey = SRLAISWMODXCQE-UHFFFAOYSA-L | ||
| + | | CASNo = 10326-26-8 | ||
| + | }} | ||
| + | | Section2 = {{Chembox Properties | ||
| + | | Reference = <ref name="Kirk-Othmer"/> | ||
| + | | Formula = Ba(BrO<sub>3</sub>)<sub>2</sub>·H<sub>2</sub>O | ||
| + | | MolarMass = 411.15 g mol<sup>−1</sup> | ||
| + | | Appearance = white crystalline solid | ||
| + | | MeltingPt = 180–200 °C ''dehydr.'' | ||
| + | | Density = 4.0 g cm<sup>−3</sup> | ||
| + | }} | ||
| + | }} | ||
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'''Barium bromate''', Ba(BrO<sub>3</sub>)<sub>2</sub>, is the [[barium]] [[salt]] of [[bromic acid]]. It is used as a corrosion inhibitor.<ref name="Kirk-Othmer"/> | '''Barium bromate''', Ba(BrO<sub>3</sub>)<sub>2</sub>, is the [[barium]] [[salt]] of [[bromic acid]]. It is used as a corrosion inhibitor.<ref name="Kirk-Othmer"/> | ||
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Barium bromate is usually prepared by the electrolysis of [[sodium 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 sodium bromate can be crystallized by cooling the electrolyte, and any unoxidized bromide recycled.<ref name="Kirk-Othmer"/> | Barium bromate is usually prepared by the electrolysis of [[sodium 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 sodium 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 [[sodium hydroxide]] solution at 50–90 °C.<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 | + | Barium bromate can also be prepared by reacting [[bromine]] with [[sodium 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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| + | ==Decomposition== | ||
| + | Anhydrous barium bromate decomposes at about 270 °C to give [[barium bromide]] and [[oxygen]]:<ref name="Kirk-Othmer"/> | ||
| + | :Ba(BrO<sub>3</sub>)<sub>2</sub> → BaBr<sub>2</sub> + 3 O<sub>2</sub> | ||
| + | Controlled decomposition in vacuo at 250 °C gives [[barium bromite]]:<ref>{{citation | first1 = A. J. | last1 = Downs | first2 = C. J. | last2 = Adams | editor1-first = J. C., Jr. | editor1-last = Bailar | editor2-first = H. J. | editor2-last = Emeleus | editor3-first = R. | editor3-last = Nyholm | editor4-first = A. F. | editor4-last = Trotman-Dickenson | title = Comprehensive Inorganic Chemistry | volume = 2 | publisher = Pergamon | location = Oxford | year = 1973 | pages = 1419–20}}.</ref> | ||
| + | :Ba(BrO<sub>3</sub>)<sub>2</sub> → Ba(BrO<sub>2</sub>)<sub>2</sub> + O<sub>2</sub> | ||
==Notes and references== | ==Notes and references== | ||
Revision as of 09:00, 4 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]
Preparation
Barium bromate is usually prepared by the electrolysis of sodium 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 sodium bromate can be crystallized by cooling the electrolyte, and any unoxidized bromide recycled.[1]
Barium bromate can also be prepared by reacting bromine with sodium hydroxide solution at 50–90 °C.[1][3]
- 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:[4]
- 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.
- ↑ 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.
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