Balance the reaction of plumbate ions and hydrochlorite ions:

Question

Pb(OH)42-(aq) + ClO-(aq) → PbO2(s) + Cl-

I put:
Pb(OH)3-(aq) + ClO-(aq) → PbO2(s) + Cl-(aq) + H2O(l) + OH-(aq)

It said: The reaction described in your answer is not balanced. One or more of your reactants appear to have an improper oxidation state. One or more of your products contains an improper oxidation state.

Oxidizing agent: Pb(OH)4^2-
It said: Your answer contains an improper oxidation state. Your answer contains an incorrect or incomplete chemical formula.

Reducing agent: ClO-
Your answer differs too much from the expected answer to provide useful feedback.

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What did I do wrong?

Answer 1

The plumbate ions I know are of the hydrated form Pb(OH)₆^2-

That stuck out at me, but it was in the problem. How did you get to Pb(OH)₃^-1

So I cant help you with the grader on this, I don't know what the problem is.