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: 17.14b


The concentration of $B(aq)$ will increase.

Work Step by Step

This is the equation for that equilibrium. $B(aq) + H_2O(l) \lt -- \gt HB^+(aq) + OH^-(aq)$ According to the Le Chatelier's principle, if we add $HB^+$ ions to the solution in equilibrium, it will try to consume these ions by shifting the equilibrium to the left. Which means that a larger quantity of $HB^+$ will be consumed, and a greater quantity of $B$ will be produced.
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.