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For the diprotic weak acid H_2A, K_a1 = 3.6 times 10^-6 and K_a2 = 8.8 times 10^-9. What is the pH of a 0.0650 M solution of H_2A? What are the equilibrium concentrations of H_2A and A^2- in this solution? pH = [H_2 A] = [A^2-] =
For the diprotic weak acid H_2A, K_a1 = 3.6 times 10^-6 and K_a2 = 8.8 times 10^-9. What is the pH of a 0.0650 M solution of H_2A? What are the equilibrium concentrations of H_2A and A^2- in this solution? pH = [H_2 A] = [A^2-] =
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