For the diprotic weak acid H₂A, Kal = 3.7 x 10-6 and Ka2 = 6.1 x 10-⁹. What is the pH of a 0.0800 M solution of H₂A? pH = What are the equilibrium concentrations of H₂A and A²- in this solution? 2- [H₂A] = [A²-] = M M
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![For the diprotic weak acid \( \text{H}_2\text{A} \), \( K_{\text{a}_1} = 3.7 \times 10^{-6} \) and \( K_{\text{a}_2} = 6.1 \times 10^{-9} \).
What is the pH of a 0.0800 M solution of \( \text{H}_2\text{A} \)?
\[ \text{pH} = \underline{\hspace{3cm}} \]
What are the equilibrium concentrations of \( \text{H}_2\text{A} \) and \( \text{A}^{2-} \) in this solution?
\[ [\text{H}_2\text{A}] = \underline{\hspace{4cm}} \, \text{M} \]
\[ [\text{A}^{2-}] = \underline{\hspace{4cm}} \, \text{M} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0ee67c44-0754-41fd-9006-bdc882dbaccb%2F4fcf3312-4e0a-48be-a10d-d1d4e4caacd7%2Ftwu81of_processed.jpeg&w=3840&q=75)
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