Chemistry and Chemical Reactivity (9th Edition)

Published by Cengage Learning
ISBN 10: 1133949649
ISBN 13: 978-1-13394-964-0

Chapter 16 Principles of Chemical Reactivity: The Chemistry of Acids and Bases - Study Questions: 34

Answer

$K_b = 8.913\times 10^{- 11}$

Work Step by Step

1. Calculate the Ka value: $K_a = 10^{-pKa}$ $K_a = 10^{- 3.95}$ $K_a = 1.122 \times 10^{- 4}$ 2. Since $[Cr{(H_2O)_5OH}]^{2+}$ is the conjugate base of $[Cr{(H_2O)_6}]^{3+}$ , we can calculate its kb by using this equation: $K_a * K_b = K_w = 10^{-14}$ $ 1.122\times 10^{- 4} * K_b = 10^{-14}$ $K_b = \frac{10^{-14}}{ 1.122\times 10^{- 4}}$ $K_b = 8.913\times 10^{- 11}$
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.