Chemistry: The Molecular Science (5th Edition)

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

Chapter 14 - Acids and Bases - Questions for Review and Thought - Topical Questions - Page 652c: 45b


$0.10M$ $KHSO_4$ is more acidic.

Work Step by Step

** You can find the $K_a$ values on table: 14.2 (Page 624) Since both solutions have the same concentration, we just have to determine which compound is more acidic: -$HF$: $HF$ is an acid with $K_a = 6.8 \times 10^{-4}$ - $KHSO_4$: It is a salt formed by $K^+$ and ${HSO_4}^-$. $K^+$ has negligible acidity, so, we don't need to consider it. ${HSO_4}^-$ is an acid with $K_a = 1.1 \times 10^{-2}$ $HS{O_4}^-$ has a greater $K_a$ value, therefore, it is more acidic. So, $0.10M$ $KHS{O_4}$ is more acidic.
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