Which of the following is the correct balanced equation for the reaction: MnO4^-(aq) + Br^-(aq) → MnO2(s) + BrO3^-(aq)?

• A. MnO4^-(aq) + Br^-(aq) → MnO2(s) + BrO3^-(aq)
• B. 2 MnO4^-(aq) + 6 Br^-(aq) + 4 H2O(l) → 2 MnO2(s) + 3 BrO3^-(aq) + 8 OH^-(aq)
• C. 2 MnO4^-(aq) + 3 Br^-(aq) + 4 H2O(l) → 2 MnO2(s) + 3 BrO3^-(aq) + 8 OH^-(aq)
• D. MnO4^-(aq) + 6 Br^-(aq) + 4 H2O(l) → MnO2(s) + 3 BrO3^-(aq) + 8 OH^-(aq)

Answer: (B)

Verified step by step guidance

1. Identify that this is a redox reaction occurring in a basic solution, involving permanganate ion (MnO4^-), bromide ion (Br^-), manganese dioxide (MnO2), and bromate ion (BrO3^-).
2. Write the half-reactions separately: the reduction half-reaction for MnO4^- to MnO2, and the oxidation half-reaction for Br^- to BrO3^-.
3. Balance each half-reaction for atoms other than O and H first, then balance oxygen atoms by adding H2O, and hydrogen atoms by adding OH^- (since the solution is basic).
4. Balance the charges in each half-reaction by adding electrons (e^-), ensuring that the total charge is the same on both sides of each half-reaction.
5. Multiply the half-reactions by appropriate coefficients so that the number of electrons lost in oxidation equals the number gained in reduction, then add the half-reactions together and simplify to get the balanced overall equation.