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For the diprotic weak acid H,A, Kal = 2.4 x 10-6 and K2 = 6.9 × 10-9. What is the pH of a 0.0500 M solution of H, A? pH What are the equilibrium concentrations of H,A and A²- in this solution? [H,A] = M [A?-] = M

For the diprotic weak acid H,A, Kal = 2.4 x 10-6 and K2 = 6.9 × 10-9. What is the pH of a 0.0500 M solution of H, A? pH What are the equilibrium concentrations of H,A and A²- in this solution? [H,A] = M [A?-] = M

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Diprotic Weak Acid Equilibrium** For the diprotic weak acid \( \text{H}_2\text{A} \), the ionization constants are given as \( K_{a1} = 2.4 \times 10^{-6} \) and \( K_{a2} = 6.9 \times 10^{-9} \). **Problem 1: Calculating the pH** What is the pH of a 0.0500 M solution of \( \text{H}_2\text{A} \)? \[ \text{pH} = \] \[ \_\_\_\_\_\_ \] **Problem 2: Equilibrium Concentrations** What are the equilibrium concentrations of \( \text{H}_2\text{A} \) and \( \text{A}^{2-} \) in this solution? \[ [\text{H}_2\text{A}] = \] \[ \_\_\_\_\_\_ \] \(\text{M}\) \[ [\text{A}^{2-}] = \] \[ \_\_\_\_\_\_ \] \(\text{M}\)
Transcribed Image Text:**Diprotic Weak Acid Equilibrium** For the diprotic weak acid \( \text{H}_2\text{A} \), the ionization constants are given as \( K_{a1} = 2.4 \times 10^{-6} \) and \( K_{a2} = 6.9 \times 10^{-9} \). **Problem 1: Calculating the pH** What is the pH of a 0.0500 M solution of \( \text{H}_2\text{A} \)? \[ \text{pH} = \] \[ \_\_\_\_\_\_ \] **Problem 2: Equilibrium Concentrations** What are the equilibrium concentrations of \( \text{H}_2\text{A} \) and \( \text{A}^{2-} \) in this solution? \[ [\text{H}_2\text{A}] = \] \[ \_\_\_\_\_\_ \] \(\text{M}\) \[ [\text{A}^{2-}] = \] \[ \_\_\_\_\_\_ \] \(\text{M}\)
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