Chemistry: The Molecular Science (5th Edition)

Published by Cengage Learning
ISBN 10: 1285199049
ISBN 13: 978-1-28519-904-7

Chapter 15 - Additional Aqueous Equilibria - Questions for Review and Thought - Applying Concepts - Page 693f: 109g


$E. pH = pK_a$

Work Step by Step

- Analyzing the Henderson-Hasselbalch equation: $pH = pK_a + log(\frac{[Base]}{[Acid]})$ If $[Base] = [Acid]$, then: $\frac{[Base]}{[Acid]} = 1$ $pH = pK_a + log(1)$ $pH = pK_a + 0$ $pH = pK_a$
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.