Perbromic acid

Structural formula
General
Surname	Perbromic acid
other names	Bromine (VII) acid
Molecular formula	HBrO 4
External identifiers / databases
PubChem	192513
ChemSpider	167074
Wikidata	Q421233
properties
Molar mass	144.91 g mol −1
solubility	soluble in water
safety instructions
GHS hazard labeling ; no classification available
GHS hazard labeling ; no classification available
	As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions .

As perbromic is oxygen acid of bromine in the oxidation state +7, with molecular formula HBrO ₄ , respectively. Their salts are called perbromates .

presentation

The first time perbromic acid was produced by the radioactive decay of a selenate salt with radioactive ⁸³ Se:

{\ displaystyle \ mathrm {^ {83} SeO_ {4} ^ {2 -} \ {\ xrightarrow {\ beta ^ {-}}} \ ^ {83} BrO_ {4} ^ {-} \ {\ xrightarrow { \ beta ^ {-}}} \ ^ {83} Kr + 2 \ O_ {2}}}

The through β-decay resulting ⁸³ BrO ₄^- disintegrates in this case, in a further β-decay to krypton and oxygen .

In contrast to perchloric acid , perbromic acid cannot be obtained by thermal disproportionation of bromic acid . It can only be produced from solutions containing bromate using very strong oxidizing agents , such as molecular fluorine or xenon difluoride , and also using anodic oxidation.

{\ displaystyle \ mathrm {BrO_ {3} ^ {-} + \ F_ {2} +2 \ OH ^ {-} \ longrightarrow \ BrO_ {4} ^ {-} + 2 \ F ^ {-} + 2 \ H_ {2} O}}

properties

Perbromic acid can be concentrated without decomposition up to a concentration of 6 mol / l, but higher concentrations can also be produced. Perbromic acid is a very strong (standard potential for perbromate → bromate in acid: +1.853 V), but in dilute solution it is quite inert oxidizing agent . In dilute solutions, for example, chlorides and bromides are oxidized very slowly, while their three-molar solution oxidizes stainless steel quickly.

Perbromic acid is stable up to a concentration of 6 mol / l even at 100 ° C. However, more concentrated solutions quickly decompose into bromic acid and oxygen .

use

By reaction with sodium hydroxide can Natriumperbromat be won.

Individual evidence

^ ^A ^b ^c ^d A. F. Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 101st edition. Walter de Gruyter, Berlin 1995, ISBN 3-11-012641-9 .
↑ This substance has either not yet been classified with regard to its hazardousness or a reliable and citable source has not yet been found.
↑ Kurt H. Stern: High Temperature Properties and Thermal Decomposition of Inorganic Salts with Oxyanions . CRC Press, 2000, ISBN 978-1-4200-4234-4 , pp. 224 ( limited preview in Google Book search).

[Holleman-Wiberg-1] A ^b ^c ^d A. F. Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 101st edition. Walter de Gruyter, Berlin 1995, ISBN 3-11-012641-9 .

[NV-2] This substance has either not yet been classified with regard to its hazardousness or a reliable and citable source has not yet been found.

[Kurt_H._Stern-3] Kurt H. Stern: High Temperature Properties and Thermal Decomposition of Inorganic Salts with Oxyanions . CRC Press, 2000, ISBN 978-1-4200-4234-4 , pp. 224 ( limited preview in Google Book search).