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 - Salts of Strong Bases and Weak Acids - Page 745: 74

Answer

$K_b ({N_3}^-)= 5.3\times 10^{- 10}$

Work Step by Step

1. Since ${N_3}^-$ is the conjugate base of $HN_3$ , we can calculate its kb by using this equation: $K_a * K_b = K_w = 1.0 \times 10^{-14}$ $ 1.9\times 10^{- 5} * K_b = 1.0 \times 10^{-14}$ $K_b = \frac{1.0 \times 10^{-14}}{ 1.9\times 10^{- 5}}$ $K_b = 5.3\times 10^{- 10}$
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