Chemistry 12th Edition

Published by McGraw-Hill Education
ISBN 10: 0078021510
ISBN 13: 978-0-07802-151-0

Chapter 16 - Acid-Base Equilibria and Solubility Equilibria - Questions & Problems - Page 764: 16.4


Please see the work below.

Work Step by Step

As we know, $pK_a= -log(K_a)$. The strength of an acid depends on $K_a$ which means that the higher the value of $K_a$, the stronger the acid will be, and thus the value of $pK_a$ will be lower. From the given data, we conclude that $H_A$ is a stronger acid because it has a lower value of $pK_a.$
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