The solution of strong acid and weak base `NH_(4)Cl` is

Options

A. Acidic
B. Basic
C. Neutral
D. None of the above

Answer

To determine the nature of the solution of the salt \( NH_4Cl \) (ammonium chloride), we can follow these steps:

### Step 1: Identify the components of the salt
The salt \( NH_4Cl \) is composed of ammonium ions \( NH_4^+ \) and chloride ions \( Cl^- \).

### Step 2: Determine the nature of the ions
- **Chloride ion \( Cl^- \)**: This ion comes from hydrochloric acid \( HCl \), which is a strong acid. Therefore, \( Cl^- \) does not affect the pH of the solution significantly and is considered neutral.
- **Ammonium ion \( NH_4^+ \)**: This ion comes from ammonia \( NH_3 \), which is a weak base. When \( NH_4^+ \) is in solution, it can donate protons (H⁺) to water, forming \( NH_3 \) and \( H_3O^+ \), thus making the solution acidic.

### Step 3: Analyze the overall effect on pH
Since \( NH_4^+ \) is the conjugate acid of a weak base, it will hydrolyze in water:
\[ NH_4^+ + H_2O \rightleftharpoons NH_3 + H_3O^+ \]
This reaction produces \( H_3O^+ \) ions, which increases the acidity of the solution.

### Step 4: Conclude the nature of the solution
Given that \( NH_4^+ \) produces \( H_3O^+ \) ions and \( Cl^- \) does not contribute to the acidity, the solution of \( NH_4Cl \) is acidic.

### Final Answer:
The solution of \( NH_4Cl \) is acidic.

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