Chemistry (4th Edition)

Published by McGraw-Hill Publishing Company
ISBN 10: 0078021529
ISBN 13: 978-0-07802-152-7

Chapter 17 - Questions and Problems - Page 824: 17.1


According to Le Chatelier's principle, when we increase the concentration of a compound that participates in the reaction, the equilibrium will move. Therefore, if we add the conjugate base in an acid dissociation, the $[H_3O^+]$ will change, affecting the pH.

Work Step by Step

Considering the generic acid dissociation: $HA(aq) + H_2O(l) \lt -- \gt A^-(aq) + H_3O^+(aq)$ If we add $A^-$ to the solution, the equilibrium will try to favor the reactants; therefore, the reactants size will be favored. Since $H_3O^+$ is on the products side, it will be more consumed, changing the pH.
Update this answer!

You can help us out by revising, improving and updating this answer.

Update this answer

After you claim an answer you’ll have 24 hours to send in a draft. An editor will review the submission and either publish your submission or provide feedback.