Question

Use the half-reaction method to balance each redox reaction occurring in acidic aqueous solution. SO32−(aq)+MnO4−(aq)→SO42−(aq)+Mn2+(aq) Express your answer as a chemical equation. Identify all of the phases in your answer.

Answer 1

The redox reaction between SO32-(aq) and MnO4-(aq) in acidic solution is balanced by using the half-reaction method, resulting in the balanced equation: 3 SO32-(aq) + 2 MnO4-(aq) + 2 H+(aq) → 3 SO42-(aq) + 2 Mn2+(aq) + 4H2O(l).

Step-by-step explanation:

To balance the redox reaction SO32-(aq) + MnO4-(aq) → SO42-(aq) + Mn2+(aq) in an acidic solution using the half-reaction method, we can follow these steps:

1. Write the oxidation and reduction half-reactions:
   
   Oxidation: SO32-(aq) → SO42-(aq)
   
   Reduction: MnO4-(aq) → Mn2+(aq)
2. Balance all elements other than oxygen and hydrogen in each half-reaction.
3. Balance oxygen by adding water (H2O) to the side lacking oxygen.
4. Balance hydrogen by adding hydrogen ions (H+) to the side lacking hydrogen.
5. Balance the charges by adding electrons (e-).
6. Multiply each half-reaction by an appropriate factor so the number of electrons gained in the reduction equals the number of electrons lost in the oxidation.
7. Add the two half-reactions together and cancel out anything that appears on both sides of the reaction.

The balanced equation for the overall reaction is:

3 SO32-(aq) + 2 MnO4-(aq) + 2 H+(aq) → 3 SO42-(aq) + 2 Mn2+(aq) + 4H2O(l)