Difference between revisions of "Barium bromate"

Barium bromate monohydrate
IUPAC name	Barium bromate — water (1/1)
Identifiers
Standard InChI	InChI=1S/Ba.2BrHO3.H2O/c;22-1(3)4;/h;2(H,2,3,4);1H2/q+2;;;/p-2
Standard InChIKey	SRLAISWMODXCQE-UHFFFAOYSA-L
CAS number	[10326-26-8]
Properties
Chemical formula	Ba(BrO3)2·H2O
Molar mass	411.15 g mol−1
Appearance	white crystalline solid
Density	3.99 g cm−3 (18 °C)
Melting point	180–200 °C dehydr.
Solubility in water	0.3 g/100 g (0 °C); 5.67 g/100 g (100 °C)
	Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)

Barium bromate
IUPAC name	Barium bromate
Other names	Barium bromate(V)
Identifiers
InChI	InChI=1/Ba.2BrHO3/c;22-1(3)4/h;2(H,2,3,4)/q+2;;/p-2
InChIKey	VEASZGAADGZARC-NUQVWONBAI
Standard InChI	InChI=1S/Ba.2BrHO3/c;22-1(3)4/h;2(H,2,3,4)/q+2;;/p-2
Standard InChIKey	VEASZGAADGZARC-UHFFFAOYSA-L
ChemSpider	55607
Properties
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)

Revision as of 10:16, 4 January 2011

Barium bromate, Ba(BrO₃)₂, is the barium salt of bromic acid. It is used as a corrosion inhibitor.^[1]

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.^[3] 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]^[4]

3 Br₂ + 3 OH⁻ ⇌ BrO−3 + 5 Br⁻ + 3 H⁺

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:^[5]

Ba(BrO₃)₂ → Ba(BrO₂)₂ + O₂

↑ ^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.
↑ 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.

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    }}
 | Section2 = {{Chembox Properties
-|   Reference = <ref name="Kirk-Othmer"/>
+|   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
 |   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>
+|   Density = 3.99 g cm<sup>−3</sup> (18&nbsp;°C)
+|   Solubility = 0.3 g/100 g (0&nbsp;°C)<br/>5.67 g/100 g (100&nbsp;°C)
    }}
 }}