Answer
$V=68.7\ mL$
Work Step by Step
By the Henderson-Hasselbach Equation:
$pH=pKa+\log([A^-]/[HA])$
$[A^-]=[OH^-]=1.00\ M\times V/(V+250.0)$
$[HA]\approx0.5\ M\times 250.0\ mL/(V+250.0)\ mL$
$4.5=4.76+\log(V/125)$
$V=68.7\ mL$
Chemistry and Chemical Reactivity (9th Edition)
by Kotz, John C.; Treichel, Paul M.; Townsend, John R.; Treichel, David A.
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
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