The aqueous solution of which one of the following salts will be acidic?

Options

A. `NaHCO_(3)`
B. NaCl
C. `NH_(4)Cl`
D. `CH_(3)COONa`

Answer

To determine which aqueous solution of the given salts will be acidic, we can analyze the hydrolysis of each salt. Here’s a step-by-step solution:

### Step 1: Identify the salts
The salts provided in the question are:
1. Sodium Bicarbonate (NaHCO3)
2. Sodium Fluoride (NaF)
3. Ammonium Fluoride (NH4F)
4. Sodium Acetate (NaC2H3O2)

### Step 2: Analyze the hydrolysis of each salt

**1. Sodium Bicarbonate (NaHCO3):**
- When NaHCO3 is dissolved in water, it dissociates into Na⁺ and HCO3⁻ ions.
- HCO3⁻ can react with water to form H2CO3 (carbonic acid) and OH⁻ (hydroxide ions).
- Since NaOH is a strong base and H2CO3 is a weak acid, the solution will be basic.

**2. Sodium Fluoride (NaF):**
- NaF dissociates into Na⁺ and F⁻ ions in water.
- F⁻ can react with water to form HF (hydrofluoric acid) and OH⁻.
- HF is a weak acid, and NaOH is a strong base, making the solution basic.

**3. Ammonium Fluoride (NH4F):**
- NH4F dissociates into NH4⁺ and F⁻ ions.
- NH4⁺ can react with water to form NH4OH (ammonium hydroxide) and H⁺ ions.
- Since NH4OH is a weak base and HCl is a strong acid, the resulting solution will be acidic.

**4. Sodium Acetate (NaC2H3O2):**
- Sodium acetate dissociates into Na⁺ and C2H3O2⁻ ions.
- C2H3O2⁻ can react with water to form acetic acid (CH3COOH) and OH⁻.
- Acetic acid is a weak acid, and NaOH is a strong base, resulting in a basic solution.

### Step 3: Conclusion
After analyzing all four salts, we find that:
- Sodium Bicarbonate (NaHCO3) → Basic
- Sodium Fluoride (NaF) → Basic
- Ammonium Fluoride (NH4F) → Acidic
- Sodium Acetate (NaC2H3O2) → Basic

Thus, the aqueous solution of **Ammonium Fluoride (NH4F)** will be acidic.

### Final Answer:
The aqueous solution of Ammonium Fluoride (NH4F) will be acidic.

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