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pH of Weak Bases

17. Acid and Base Equilibrium / pH of Weak Bases / Problem 4

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

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