Answer
$Pb(OH)_{4}^{2-} (aq) + ClO^{-} (aq) → PbO_{2}(s) + Cl^{-} (aq) + 2OH^{-} (aq) + H_{2}O (l)$
Oxidizing Agent: $ClO^{-}$
Reducing Agent: $Pb(OH)_{4}^{2-}$
Work Step by Step
We add water and OH- on right side to balance the equation as it is in basic medium. Oxidation state of Pb is changed from +2 to +4, hence it is oxidized and state of Cl is changed from +1 to -1, hence it is reduced.
