## Chemistry and Chemical Reactivity (9th Edition)

Published by Cengage Learning

# Chapter 16 Principles of Chemical Reactivity: The Chemistry of Acids and Bases - Study Questions - Page 629b: 31

#### Answer

$K_b = 7.092\times 10^{- 12}$

#### Work Step by Step

1. Since $ClCH_2{CO_2}^-$ is the conjugate base of $ClCH_2CO_2H$ , we can calculate its Kb by using this equation: $K_a * K_b = K_w = 10^{-14}$ $1.41\times 10^{- 3} * K_b = 10^{-14}$ $K_b = \frac{10^{-14}}{ 1.41\times 10^{- 3}}$ $K_b = 7.092\times 10^{- 12}$

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