Calculate the pH of 0.10 M solution of `NH_(4)Cl`. The dissociation constant `(K_(b))` of `NH_(3)` is `1.6xx10^(-5)`.

Explanation

To calculate the pH of a 0.10 M solution of \( NH_4Cl \), we need to follow these steps:

### Step 1: Identify the nature of \( NH_4Cl \)
- \( NH_4Cl \) is a salt formed from the weak base \( NH_3 \) (ammonia) and the strong acid \( HCl \). When dissolved in water, it dissociates into \( NH_4^+ \) and \( Cl^- \) ions. The \( NH_4^+ \) ion can act as a weak acid.

### Step 2: Write the dissociation reaction of \( NH_4^+ \)
- The dissociation of \( NH_4^+ \) in water can be represented as:
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