Which will undergo cationic hydrolysis ?

Options

A. NaCI
B. `CH_3COONa`
C. `(NH_4)_2SO_4`
D. `Na_2CO_3`

Answer

To determine which compound will undergo cationic hydrolysis, we need to analyze the nature of the cations present in each of the given compounds. Cationic hydrolysis occurs when the cation is derived from a weak base. Here’s a step-by-step solution:

### Step 1: Identify the Compounds
The given options are:
1. NaCl
2. CH3COONa
3. NH4(SO4)2
4. Na2CO3

### Step 2: Analyze Each Compound
- **NaCl**: Sodium (Na⁺) is derived from NaOH, which is a strong base. Chloride (Cl⁻) comes from HCl, which is a strong acid. Therefore, NaCl does not undergo hydrolysis.

- **CH3COONa**: Sodium (Na⁺) is from NaOH (strong base), and acetate (CH3COO⁻) is from acetic acid (weak acid). The cation Na⁺ does not undergo hydrolysis, but the anion CH3COO⁻ can undergo hydrolysis. However, we are focusing on cationic hydrolysis, so this does not qualify.

- **NH4(SO4)2**: The ammonium ion (NH4⁺) is derived from ammonia (NH3), which is a weak base. Therefore, NH4⁺ can undergo hydrolysis, making this compound capable of cationic hydrolysis.

- **Na2CO3**: Sodium (Na⁺) is from NaOH (strong base), and carbonate (CO3²⁻) is from carbonic acid (H2CO3), which is a weak acid. The cation Na⁺ does not undergo hydrolysis.

### Step 3: Conclusion
From the analysis, the only compound that contains a cation derived from a weak base and can undergo cationic hydrolysis is **NH4(SO4)2**.

### Final Answer
**C. NH4(SO4)2** will undergo cationic hydrolysis.

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