# Disproportionation Reaction [closed]

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

$$\ce{HXeO4 -> XeO6^{4-} + Xe + O2}$$

It is supposed to be in a basic solution. However, my answer does not contain $\ce{OH-}$ on either side:

$$\ce{4HXeO4 -> XeO6^{4-} + 3Xe + 4O2 + 2H2O}$$

I am wondering if I had made a mistake or if it's ok for the reaction to not contain $\ce{OH-}$ ions.

• The reaction is not balanced. When there are charges you have to balance them too. Try adding hydroxide ions ("basic solution") to the reactants and use them to balance the charges. You'll need to rebalance the elements of course. – Oscar Lanzi Sep 10 '17 at 2:31
• I thought this thing looked weird. The answer confirms that there is no neutral $\ce{HXeO4}$. – Jan Sep 10 '17 at 15:15

$$\ce{2 HXeO4^− + 2 OH^− → XeO6^{4−} + Xe + O2 + 2 H2O}$$