Balance each redox reaction occurring in acidic aqueous solution. a. PbO₂(s) + I^–(aq) → Pb²⁺(aq) + I₂(s) b. SO₃^2–(aq) + MnO₄^–(aq) → SO₄^2–(aq) + Mn²⁺(aq) c. S₂O₃^2–(aq) + Cl₂(g) → SO₄^2–(aq) + Cl^–(aq)

Verified step by step guidance

1. Step 1: Identify the oxidation and reduction half-reactions for each given redox reaction. For example, in reaction (a), determine which species is oxidized and which is reduced.
2. Step 2: Balance each half-reaction for atoms other than oxygen and hydrogen. For instance, in reaction (a), balance the lead and iodine atoms in their respective half-reactions.
3. Step 3: Balance oxygen atoms by adding H2O molecules to the side that needs oxygen. Then, balance hydrogen atoms by adding H+ ions to the side that needs hydrogen.
4. Step 4: Balance the charge of each half-reaction by adding electrons. Ensure that the number of electrons lost in the oxidation half-reaction equals the number gained in the reduction half-reaction.
5. Step 5: Combine the balanced half-reactions, ensuring that electrons cancel out, and verify that both mass and charge are balanced in the final equation.