Which of the following is the correct balanced chemical equation for the reaction between aluminum and permanganate ion in aqueous solution to produce manganese dioxide and aluminum hydroxide?

• A. 2 Al(s) + 3 MnO4^-(aq) + 6 H2O(l) → 3 MnO2(s) + 2 Al(OH)4^-(aq) + 2 OH^-(aq)
• B. Al(s) + MnO4^-(aq) + 2 H2O(l) → MnO2(s) + Al(OH)4^-(aq)
• C. 2 Al(s) + 3 MnO4^-(aq) + 4 H2O(l) → 3 MnO2(s) + 2 Al(OH)4^-(aq) + 2 OH^-(aq)
• D. 3 Al(s) + 4 MnO4^-(aq) + 10 H2O(l) → 4 MnO2(s) + 3 Al(OH)4^-(aq) + 2 OH^-(aq)

Answer: (C)

Verified step by step guidance

1. Identify the species involved in the redox reaction: aluminum (Al) is oxidized, and permanganate ion (MnO4^-) is reduced to manganese dioxide (MnO2). Aluminum hydroxide species (Al(OH)4^-) and hydroxide ions (OH^-) are formed in the basic aqueous solution.
2. Write the half-reactions separately: the oxidation half-reaction for aluminum going to Al(OH)4^- and the reduction half-reaction for MnO4^- going to MnO2. Balance atoms other than O and H first, then balance oxygen by adding H2O, and hydrogen by adding OH^- (since the solution is basic).
3. Balance the charges in each half-reaction by adding electrons (e^-). The number of electrons lost in the oxidation half-reaction must equal the number gained in the reduction half-reaction.
4. Multiply each half-reaction by appropriate coefficients so that the electrons cancel out when the half-reactions are added together. Then add the half-reactions to get the overall balanced equation.
5. Verify that the number of atoms of each element and the total charge are balanced on both sides of the equation. This confirms the correct stoichiometric coefficients and the correct balanced chemical equation.