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: 22


$V=231.97\ mL$

Work Step by Step

By the Henderson-Hasselbach Equation: $pH=pKa+\log([HPO_4^{2-}]/[H_2PO_4^-])$ $[HPO_4^{2-}]=0.5\ M\times 750.0\ mL/(V+750.0)\ mL-[H_2PO_4]$ $[H_2PO_4^-]=[HCl]=1.00\ M\times V/(V+750.0)$ $7.00=7.21+\log((375-V)/V)$ $V=231.97\ mL$
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