Answer
$CH_2N{H_3}^+$ is a weak acid.
$CH_2N{H_3}^+(aq) + H_2O(l) \lt -- \gt CH_2N{H_2}(aq) + H_3O^+(aq)$
Work Step by Step
$CH_2N{H_3}^+$ is the conjugate acid of a very common weak base: $CH_2N{H_2}$, 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,
$CH_2N{H_3}^+ -- \gt CH_2N{H_2}$
2. Identify if that compound is a base.
- The $K_b$ table can help this process.
$CH_2N{H_2}$ is a weak base, so $CH_2N{H_3}^+$ is a weak acid.
Therefore, when reacting with water, $CH_2N{H_3}^+$ donates one proton to the $H_2O$ molecule, producing hydronium ion.
