Chemistry: Molecular Approach (4th Edition)

Published by Pearson
ISBN 10: 0134112830
ISBN 13: 978-0-13411-283-1

Chapter 16 - Exercises - Page 771: 14


The $[OH^-]$ of a solution decreases when the $[H_3O^+]$ is increased, and increases when the $[H_3O^+]$ is decreased.

Work Step by Step

According to the expression of the ion product constant for water: $$K_w = [H_3O^+][OH^-]$$ - Dividing both sides by $[H_3O^+]$: $$\frac{K_w}{[H_3O^+]} = [OH^-]$$ - $K_w$ is a constant, assuming constant temperature; therefore, $[OH^-]$ is inversely proportional to $[H_3O^+]$. $$\frac{1}{[H_3O^+]} \propto [OH^-]$$ When $[H_3O^+]$ increases, $[OH^-]$ decreases and vice versa.
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