Chemistry: The Central Science (13th Edition)

Published by Prentice Hall
ISBN 10: 0321910419
ISBN 13: 978-0-32191-041-7

Chapter 17 - Additional Aspects of Aqueous Equilibria - Exercises - Page 768: 17.14c


The pH of the solution will decrease.

Work Step by Step

Since $HB^+$ is an acid, it makes sense that it will raise the $[H_3O^+]$ of the solution, reducing the pH. -------------------- As we discussed on the last exercise (17.14b), after the addition of $HB^+$, the equilibrium is shifted to the left side of the equation: $B(aq) + H_2O(l) \lt -- \gt HB^+(aq) + OH^-(aq)$ Which implies a greater consumption of $OH^-$. When $[OH^-]$ decreases, the hydronium ion concentration $[H_3O^+]$ increases, which will cause the decrease of the pH.
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