Chemistry and Chemical Reactivity (9th Edition)

Published by Cengage Learning
ISBN 10: 1133949649
ISBN 13: 978-1-13394-964-0

Chapter 17 Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria - Study Questions - Page 677a: 21


$V=68.7\ mL$

Work Step by Step

By the Henderson-Hasselbach Equation: $pH=pKa+\log([A^-]/[HA])$ $[A^-]=[OH^-]=1.00\ M\times V/(V+250.0)$ $[HA]\approx0.5\ M\times 250.0\ mL/(V+250.0)\ mL$ $4.5=4.76+\log(V/125)$ $V=68.7\ mL$
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.