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 pH and pOH Scales - Page 743: 23

Answer

$[H_3O^+] = 0.0548M$ $[OH^-] = 1.825 \times 10^{-13}M $ $pH = 1.261$ $pOH = 12.739$

Work Step by Step

1. HCl is a strong acid, so : $[HCl] = [H_3O^+] = 0.0548M:$ 2. Now, find the pH and pOH: $pH = -log[H_3O^+]$ $pH = -log( 0.0548)$ $pH = 1.261$ $pOH + pH = 14$ $pOH = 14 - pH = 14 - 1.261$ $pOH = 12.739$ 3. And the $[OH^-]$: $[H_3O^+] * [OH^-] = Kw = 10^{-14}$ $ 5.48 \times 10^{- 2} * [OH^-] = 10^{-14}$ $[OH^-] = \frac{10^{-14}}{ 5.48 \times 10^{- 2}}$ $[OH^-] = 1.825 \times 10^{- 13}M$
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