Answer
This is an acidic cation.
$N{H_4}^+(aq) + H_2O(l) \lt -- \gt NH_3(aq) + H_3O^+(aq)$
Work Step by Step
$N{H_4}^+$ is the conjugate acid of a very common weak base: $NH_3$, therefore, it is a weak acid.
- The formula: $BH^+$ can help us when identifying this type of acidic cation, where "$B$" is a base, so:
1. Remove one proton from the cation,
$N{H_4}^+ -- \gt NH_3$
2. Identify if that compound is a base.
- The $K_b$ table can help this process.
$NH_3$ is a weak base, so $NH_4^+$ is a weak acid.
