Question

For the diprotic weak acid H2A, Ka1 = 3.6 × 10^(-6) and Ka2 = 7.1 × 10^(-9). What is the pH of a 0.0450 M solution of H2A? pH = What are the equilibrium concentrations of H2A and A^2- in this solution? [H2A] = [A^2-] =

Name: for the diprotic weak acid h2a ka136106 and ka271109 what is the ph of a 00450 m solution of h2a ph what are the equilibrium concentrations of h2a and a2 in this solution h2a a2 13127
Uploaded: 2023-04-16T13:41:33-08:00
Duration: 2 min 39 s
Channel: Madhur L
Description: for the diprotic weak acid h2a ka136106 and ka271109 what is the ph of a 00450 m solution of h2a ph what are the equilibrium concentrations of h2a and a2 in this solution h2a a2 13127

          For the diprotic weak acid H2A, Ka1 = 3.6 × 10^(-6) and Ka2 = 7.1 × 10^(-9).
What is the pH of a 0.0450 M solution of H2A?
pH =
What are the equilibrium concentrations of H2A and A^2- in this solution?
[H2A] =
[A^2-] =

Added by Pedro A.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Madhur L

04/16/2023

Step 1

For the first ionization, we have the equilibrium expression: $K_{a1} = \frac{[H_3O^+][HA^-]}{[H_2A]}$ Let x be the concentration of H3O+ ions after the first ionization. Then, we have: $3.6 \times 10^{-6} = \frac{x^2}{0.0450 - x}$ Solving for x, we get: $x Show more…

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For the diprotic weak acid H2A, Ka1 = 3.6 × 10^(-6) and Ka2 = 7.1 × 10^(-9). What is the pH of a 0.0450 M solution of H2A? pH = What are the equilibrium concentrations of H2A and A^2- in this solution? [H2A] = [A^2-] =