Chemistry: The Molecular Science (5th Edition)

Published by Cengage Learning
ISBN 10: 1285199049
ISBN 13: 978-1-28519-904-7

Chapter 14 - Acids and Bases - Questions for Review and Thought - Topical Questions - Page 652b: 27

Answer

pH = 12.40 pOH = 1.60

Work Step by Step

- NaOH is a strong base, therefore: $[OH^-] = [NaOH] = 0.025M$ 1. Calculate the hydronium concentration: $[OH^-] * [H_3O^+] = Kw = 10^{-14}$ $ 2.5 \times 10^{- 2} * [H_3O^+] = 10^{-14}$ $[H_3O^+] = \frac{10^{-14}}{ 2.5 \times 10^{- 2}}$ $[H_3O^+] = 4 \times 10^{- 13}$ 2. Calculate the pH Value $pH = -log[H_3O^+]$ $pH = -log( 4 \times 10^{- 13})$ $pH = 12.40$ 3. Use this value to calculate the pOH: $pH + pOH = 14$ $12.40 + pOH = 14$ $pOH = 14 - 12.40 = 1.60$
Update this answer!

You can help us out by revising, improving and updating this answer.

Update this answer

After you claim an answer you’ll have 24 hours to send in a draft. An editor will review the submission and either publish your submission or provide feedback.