Question

Consider the following reaction: Pb(OH)42- (aq) + ClO- (aq)  PbO2 (s) + Cl- (aq) in basic solution.

Determine the element being oxidized. What is its oxidation number as a reactant and as a product?

Determine the element being reduced. What is its oxidation number as a reactant and as a product?

Write and balance the oxidation half-reaction in basic solution.

Write and balance the reduction half-reaction in basic solution.

Write the overall balanced net ionic equation in basic solution for this reaction

What is the reducing agent in this reaction?