Chemistry 12th Edition

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

Chapter 15 - Acids and Bases - Questions & Problems - Page 711: 15.39


Higher Ka value: Stronger acid. Lower Ka value: Weaker acid.

Work Step by Step

Let's take a look at the Ka formula: $K_a = \frac{[H^+][A^-]}{[HA]}$ The Ka value increases when the $[H^+]$ and $[A^-]$ increases and decreases when the value of $[HA]$ increases. Strong acids have more $[H^+]$ and $[A^-]$, because the molecules ionized more than weak acids molecules; therefore, the value of $K_a$ is also higher.
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