## Chemistry and Chemical Reactivity (9th Edition)

$K_b = 6.31\times 10^{- 5}$
1. Calculate the Ka value: $K_a = 10^{-pKa}$ $K_a = 10^{- 9.8}$ $K_a = 1.585 \times 10^{- 10}$ 2. Since $(CH_3)_3N$ is the conjugate base of $(CH_3)_3NH^+$ , we can calculate its kb by using this equation: $K_a * K_b = K_w = 10^{-14}$ $1.585\times 10^{- 10} * K_b = 10^{-14}$ $K_b = \frac{10^{-14}}{ 1.585\times 10^{- 10}}$ $K_b = 6.31\times 10^{- 5}$