Chemistry 10th Edition

Published by Brooks/Cole Publishing Co.
ISBN 10: 1133610668
ISBN 13: 978-1-13361-066-3

Chapter 18 - Ionic Equilibria I: Acids and Bases - Exercises - The Autoionization of Water - Page 743: 10

Answer

(a) $$ H_2O(l) + H_2O(l) \leftrightharpoons H_3O^+(aq) + OH^-(aq)$$ (b) $$K = [H_3O^+][OH^-]$$ (c) $K_w$ is the special symbol for this specific constant. (d) At room temperature, $K_w = 1.0 \times 10^{-14}$, so: $$1.0 \times 10^{-14} = [H_3O^+][OH^-]$$ At pure water: $$[H_3O^+] = [OH^-] = 1.0 \times 10^{-7} M$$ (e) The definition of acidic and basic is directly related to the relation between the concentrations of $H_3O^+$ and $OH^-$, if $[H_3O^+] > [OH^-]$, the solution is acidic, if $[OH^-] > [H_3O^+]$, the solution is basic.
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