Answer
This solution will be basic.
Work Step by Step
1. Analyze each type of ion in this salt, and determine which is stronger.
- $N{H_4}^+$:
- Weak bases have weak acids as conjugate pair.
- $N{H_4}^{+}$ is the conjugate acid of $NH_3$, which is a weak base.
- $N{H_4}^{+}$: Weak acid.
- $ClO^-$
- Weak acids have Weak bases as conjugate pair.
- $ClO^-$ is the conjugate base of $HClO$, which is a weak acid.
- $ClO^-$: Weak base.
Therefore, we will have to compare their constants values:
- We don't have these values, but, we have the one for their conjugate pairs:
$NH_3$ $K_b = 1.8 \times 10^{-5}$
$HClO$ $K_a = 2.9 \times 10^{-8}$
- $NH_3$ is the stronger conjugate pair.
- Knowing the $Ka-Kb$ relation: $N{H_4}^+$ is the weaker electrolyte.
** The stronger the base, the weaker its conjugate acid, and vice versa.
- Therefore, $ClO^-$ is the stronger ion, and since it is a base, the solution will be basic.
