Perbromic acid

Solution

Soluble in water

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Perbromic acid as the oxygen of the bromine in the 7 oxidation state is designated by the empirical formula HBrO4. Its salts are called Perbromates.

Representation

The first time was perbromic produced by the radioactive decay of a radioactive 83Se Selenatsalzes:

The resulting by β -decay 83BrO4 - decays in this case in another β -decay to Krypton and oxygen.

In contrast to the perchloric acid is perbromic can not be obtained by the thermal disproportionation of hydrobromic acid. They can only be very strong oxidizing agents, such as molecular fluorine or xenon difluoride, are made from solutions containing bromate, as well as by means of anodic oxidation.

Properties

Up to a concentration of 6 mol / l perbromic can be concentrated without decomposition, but it can also be made higher concentrations. Perbromic is a very strong ( standard potential for perbromate → bromate in acidic medium: 1.853 V ), but in dilute solution rather sluggish oxidant. Thus, in dilute solution as chlorides and bromides are only very slowly oxidized, while their dreimolare solution stainless steel oxidizes rapidly.

Perbromic is stable up to a concentration of 6 mol / L even at 100 ° C. However, highly concentrated solutions decompose rapidly to bromo acid and oxygen.