For a 2.50 M NaClO solution, what would be the concentration of the species present at equilibrium?

• A. [Na⁺] = 2.50 M; [ClO^–] = 2.39 M; [HClO] = 2.98×10^–4 M; [OH^–] = 2.98×10^–4 M; [H₃O⁺] = 8.10×10^–11 M
• B. [Na⁺] = 1.25 M; [ClO^–] = 1.25 M; [HClO] = 6.57×10^–4 M; [OH^–] = 6.57×10^–4 M; [H₃O⁺] = 1.52×10^–11 M
• C. [Na⁺] = 2.50 M; [ClO^–] = 2.50 M; [HClO] = 9.28×10^–4 M; [OH^–] = 9.28×10^–4 M; [H₃O⁺] = 1.08×10^–11 M
• D. [Na⁺] = 1.25 M; [ClO^–] = 1.25 M; [HClO] = 6.57×10^–4 M; [OH^–] = 1.52×10^–11 M; [H₃O⁺] = 6.57×10^–4 M

Answer: (C)