Question

Disproportionate reaction of perxenate ion

Answer 1

This is the problem I am trying to balance for redox:

HXeO4⟶XeO64−+Xe+O2

It is supposed to be in a basic solution. However, my answer does not contain OH− on either side:

4HXeO4⟶XeO64−+3Xe+4O2+2H2O

I am wondering if I had made a mistake or if it's ok for the reaction to not contain OH− ions.

Answer 2

Explanation:

disproportionation reaction is when a multiatomic species whose pertinent element has a specific oxidation state gets oxidized and reduced in two separate half-reactions, yielding two other products containing the same pertinent element. EXAMPLE: MANGANESE OXIDES. A convenient example is Mn2O3 becoming Mn2+ and MnO2.