Which of these salts will given acidic solution ?

Options

A. `NaCO_(3)`
B. `NaCI`
C. `NH_(4)CI`
D. COONa

Explanation

To determine which of the given salts will produce an acidic solution, we need to analyze the salts based on their constituent acids and bases. Here’s a step-by-step solution:

### Step 1: Understand the nature of salts
Salts are formed from the neutralization reaction between an acid and a base. The nature of the salt (acidic, basic, or neutral) depends on the strength of the acid and base from which it is formed.

### Step 2: Identify the salts
Let's consider the salts mentioned:
1. NaCl (Sodium Chloride)
2. Na2CO3 (Sodium Carbonate)
3. NH4Cl (Ammonium Chloride)
4. HClO (Hypochlorous Acid)

### Step 3: Analyze each salt for hydrolysis
1. **NaCl**:
- Formed from NaOH (strong base) and HCl (strong acid).
- Hydrolysis: NaCl → Na⁺ + Cl⁻
- Result: Neutral solution (no acidic or basic properties).

2. **Na2CO3**:
- Formed from NaOH (strong base) and H2CO3 (weak acid).
- Hydrolysis: Na2CO3 → 2Na⁺ + CO3²⁻
- Result: Basic solution (since CO3²⁻ can accept protons).

3. **NH4Cl**:
- Formed from NH4OH (weak base) and HCl (strong acid).
- Hydrolysis: NH4Cl → NH4⁺ + Cl⁻
- Result: Acidic solution (NH4⁺ can donate protons).

4. **HClO**:
- This is a weak acid itself and does not form a salt in the context of this question.
- Result: Weakly acidic solution.

### Step 4: Conclusion
Among the salts analyzed, **NH4Cl** is the only salt that will produce an acidic solution due to the presence of the ammonium ion (NH4⁺), which can donate protons in solution.

### Final Answer
**NH4Cl** will give an acidic solution.

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