For the diprotic weak acid H2A, Kal = 3.5 × 10-6 and K22 = 7.7 × 10-9. What is the pH of a 0.0400 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 H2A, Kal = 3.5 × 10-6 and K22 = 7.7 × 10-9. What is the pH of a 0.0400 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

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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Question

For the diprotic weak acid H2A, Kal
3.5 x 10-6 and K22 = 7.7 x 10-9.
What is the pH of a 0.0400 M solution of H, A?
pH
What are the equilibrium concentrations of H,A and A2-
this solution?
[H,A] =
M
[A?-] =
M

Expert Solution

Step 1

The pH is used to determine the alkalinity or acidity of a solution.

the pH is determined as the negative logarithm of hydrogen ion concentration.

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