We know that $K_a \times K_b = K_w$, where $K_w$ is the ion product of water, $1.0 \times 10^{-14}$ at 25°C. Given that the $K_b$ for ethylamine is $5.6 \times 10^{-4}$, we can calculate $K_a$ as follows:
\[K_a = \frac{K_w}{K_b} = \frac{1.0 \times 10^{-14}}{5.6
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