For the diprotic weak acid H2A, Kal = 2.1 x 10-6 and K2 = 6.1 x 10-9. What is the pH of a 0.0600 M solution of H, A? pH = What are the equilibrium concentrations of H, A and A2- in this solution? [H,A] = M [A?-] = M
Ionic Equilibrium
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![For the diprotic weak acid H2A, Ka1 = 2.1 × 10-6 and K2 = 6.1 × 10-9.
What is the pH of a 0.0600 M solution of H, A?
pH =
What are the equilibrium concentrations of H,A and A2- in this solution?
[H, A] =
M
[A?-] =
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F06a257f2-cd9d-41ad-abbb-e1cba0ed0454%2F0ec5644c-a7e9-4849-ad10-1de1beca4465%2Fdo5t0rb1u_processed.png&w=3840&q=75)
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