Difference between revisions of "Barium bromate"

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(Created page with "{{chembox | IUPACName = Barium bromate | OtherNames = Barium bromate(V) | Section1 = {{Chembox Identifiers | ChemSpiderID = 55607 | InChI=1/Ba.2BrHO3/c;2*2-1(3)4/h;2*(H,2,3,4...")
 
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{{chembox
 
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| 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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|  CASNo = 10326-26-8
 
 
   }}
 
   }}
 
| 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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|  Density = 4.0 g cm<sup>−3</sup>
 
 
   }}
 
   }}
 
| Section8 = {{Chembox Related
 
| Section8 = {{Chembox Related
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   }}
 
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{{chembox
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| Name = Barium bromate monohydrate
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| IUPACName = Barium bromate — water (1/1)
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| Section1 = {{Chembox Identifiers
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|  StdInChI=1S/Ba.2BrHO3.H2O/c;2*2-1(3)4;/h;2*(H,2,3,4);1H2/q+2;;;/p-2
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|  StdInChIKey = SRLAISWMODXCQE-UHFFFAOYSA-L
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|  CASNo = 10326-26-8
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  }}
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| Section2 = {{Chembox Properties
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|  Reference = <ref name="Kirk-Othmer"/>
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|  Formula = Ba(BrO<sub>3</sub>)<sub>2</sub>·H<sub>2</sub>O
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|  MolarMass = 411.15 g mol<sup>−1</sup>
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|  Appearance = white crystalline solid
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|  MeltingPt = 180–200 °C ''dehydr.''
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|  Density = 4.0 g cm<sup>−3</sup>
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  }}
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}}
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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&nbsp;°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&nbsp;°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"/>
  
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Barium bromate can also be prepared by reacting [[bromine]] with [[sodium hydroxide]] solution at 50–90&nbsp;°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><ref name="Kirk-Othmer"/>
+
Barium bromate can also be prepared by reacting [[bromine]] with [[sodium hydroxide]] solution at 50–90&nbsp;°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==
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Anhydrous barium bromate decomposes at about 270&nbsp;°C to give [[barium bromide]] and [[oxygen]]:<ref name="Kirk-Othmer"/>
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:Ba(BrO<sub>3</sub>)<sub>2</sub> &rarr; BaBr<sub>2</sub> + 3 O<sub>2</sub>
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Controlled decomposition in vacuo at 250&nbsp;°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> &rarr; Ba(BrO<sub>2</sub>)<sub>2</sub> + O<sub>2</sub>
  
 
==Notes and references==
 
==Notes and references==

Revision as of 10:00, 4 January 2011

Barium bromate
IUPAC name Barium bromate
Other names Barium bromate(V)
Identifiers
InChI InChI=1/Ba.2BrHO3/c;2*2-1(3)4/h;2*(H,2,3,4)/q+2;;/p-2
InChIKey VEASZGAADGZARC-NUQVWONBAI
Standard InChI InChI=1S/Ba.2BrHO3/c;2*2-1(3)4/h;2*(H,2,3,4)/q+2;;/p-2
Standard InChIKey VEASZGAADGZARC-UHFFFAOYSA-L
ChemSpider 55607
Properties[1]
Chemical formula Ba(BrO3)2
Molar mass 393.13 g mol−1
Appearance white crystalline solid
Melting point

270 °C decomp.

Related compounds
Other anions Barium chlorate
Barium iodate
Other cations Calcium bromate
Strontium bromate
Other compounds Barium bromide
Barium hypobromite
Barium bromite
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Barium bromate monohydrate
IUPAC name Barium bromate — water (1/1)
Identifiers
Standard InChI InChI=1S/Ba.2BrHO3.H2O/c;2*2-1(3)4;/h;2*(H,2,3,4);1H2/q+2;;;/p-2
Standard InChIKey SRLAISWMODXCQE-UHFFFAOYSA-L
CAS number [10326-26-8]
Properties[1]
Chemical formula Ba(BrO3)2·H2O
Molar mass 411.15 g mol−1
Appearance white crystalline solid
Density 4.0 g cm−3
Melting point

180–200 °C dehydr.

Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)

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. ↑ 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. ↑ Osuga, Takasi; Sugino, Kiichiro Electrolytic Production of Bromates. J. Electrochem. Soc. 1957, 104 (7), 448–51. DOI: 10.1149/1.2428623.
  3. ↑ 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.
  4. ↑ 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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