We can look up the $K_b$ for methylamine, which is given as $4.4 \times 10^{-4}$. The $K_a$ for the conjugate acid, methylammonium ion ($\mathrm{CH}_3\mathrm{NH}_3^+$), can be found using the relationship $K_a = \frac{K_w}{K_b}$, where $K_w$ is the ion product of
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