Answer
We can deduce that, the stronger the acid, the weaker the conjugate base will be.
Work Step by Step
If we have 2 values multiplying to form a constant, these 2 values will be inversely porportional:
$K_a * K_b = 10^{-14}$
$K_a = \frac{10^{-14}}{K_b}$
or
$K_b = \frac{10^{-14}}{K_a}$
- When Ka increases, Kb decreases, and vice versa.
Since the $K_a$ and the $K_b$ are directly related to their acids/bases strengths, the weaker the base, the stronger the conjugate acid will be, and vice versa.
