For the diprotic weak acid H2A, Ka1 = 3.0 × 10-6 and Ka2 = 7.1 x 10-9. What is the pH of a 0.0700 M solution of H,A? pH = 3.33 What are the equilibrium concentrations of H, A and A²- in this solution? [H,A] = | 0.0095 M Incorrect [A?-] = 0.0000018 M
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![For the diprotic weak acid H2A, Ka1 = 3.0 × 10-6 and K2 = 7.1 x 10-9.
What is the pH of a 0.0700 M solution of H, A?
pH = 3.33
What are the equilibrium concentrations of H, A and A²- in this solution?
[H,A] = 0.0095
M
Incorrect
[A?-] = 0.0000018
M
Incorrect](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F88270d99-f085-4c3e-be91-1bddcbccdb85%2F2a8236f0-0a2b-491f-be01-0f5652f0751c%2Fm6dufee_processed.png&w=3840&q=75)
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