What is the balanced equation for the redox reaction occurring in a basic solution: Cr(OH)4⁻(aq) + ClO⁻(aq) → CrO4²⁻(aq) + Cl⁻(aq)?

• A. Cr(OH)4⁻ + 2ClO⁻ + 2OH⁻ → CrO4²⁻ + 2Cl⁻ + 2H2O
• B. Cr(OH)4⁻ + 4ClO⁻ + 4OH⁻ → CrO4²⁻ + 4Cl⁻ + 4H2O
• C. Cr(OH)4⁻ + ClO⁻ + OH⁻ → CrO4²⁻ + Cl⁻ + H2O
• D. Cr(OH)4⁻ + 3ClO⁻ + 2OH⁻ → CrO4²⁻ + 3Cl⁻ + 4H2O

Answer: (D)

Verified step by step guidance

1. Identify the oxidation and reduction half-reactions. In this case, Cr(OH)4⁻ is oxidized to CrO4²⁻, and ClO⁻ is reduced to Cl⁻.
2. Write the oxidation half-reaction: Cr(OH)4⁻ → CrO4²⁻. Balance the chromium atoms and then balance the oxygen atoms by adding H2O molecules.
3. Write the reduction half-reaction: ClO⁻ → Cl⁻. Balance the chlorine atoms and then balance the oxygen atoms by adding H2O molecules.
4. Balance the hydrogen atoms in both half-reactions by adding OH⁻ ions, since the reaction occurs in a basic solution.
5. Combine the balanced half-reactions, ensuring that the electrons lost in the oxidation half-reaction equal the electrons gained in the reduction half-reaction. Simplify the equation by canceling out common species on both sides.