Chemistry: The Molecular Nature of Matter and Change 7th Edition

Published by McGraw-Hill Education
ISBN 10: 007351117X
ISBN 13: 978-0-07351-117-7

Chapter 19 - Problems: 19.15

Answer

pH of buffer = 3.89

Work Step by Step

1 (A) Given : 1. [conjugate base] = [HCOO-] = 0.63 M 2. [acid] = [HCOOH] = 0.45 M 3. pKa of acid (HCOOH) = 3.74 2 (B) Formulae : 1. Henderson - Hasselbalch equation of a buffer : pH = pKa + log [conjugate base] / [acid] 3 (C) Solution : pH = pKa + log [conjugate base] / [acid] So, pH = 3.74 + log (0.63 / 0.45) 3.74 + 0.15 = 3.89 Hence, pH of the buffer is 3.89. 4 (D) Answer : pH of buffer = 3.89
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