The ionisation of acetic acid in `H_(2)SO_(4)` compared to in water, is :

Options

A. Weak
B. Strong
C. Medium
D. 1

Explanation

To analyze the ionization of acetic acid (CH₃COOH) in sulfuric acid (H₂SO₄) compared to water, we can follow these steps:

### Step 1: Understand the Ionization of Acetic Acid
Acetic acid is a weak acid that partially ionizes in water according to the following equilibrium reaction:
\[ \text{CH}_3\text{COOH} \rightleftharpoons \text{CH}_3\text{COO}^- + \text{H}^+ \]

### Step 2: Ionization in Water
In pure water, acetic acid ionizes to produce acetate ions (CH₃COO⁻) and hydrogen ions (H⁺). However, since it is a weak acid, the degree of ionization is limited, and the equilibrium lies to the left.

### Step 3: Ionization in Sulfuric Acid
When acetic acid is placed in a solution of sulfuric acid, which is a strong acid, the concentration of hydrogen ions (H⁺) is significantly increased due to the complete ionization of sulfuric acid:
\[ \text{H}_2\text{SO}_4 \rightarrow 2\text{H}^+ + \text{SO}_4^{2-} \]

### Step 4: Effect of Increased H⁺ Concentration
The increased concentration of H⁺ ions from sulfuric acid will shift the equilibrium of acetic acid to the left according to Le Chatelier's principle. This is because the presence of additional H⁺ ions suppresses the ionization of acetic acid.

### Step 5: Conclusion
As a result, the ionization of acetic acid in sulfuric acid is weaker compared to its ionization in water. Therefore, the ionization of acetic acid in H₂SO₄ compared to in water is **weaker**.

### Final Answer
The ionization of acetic acid in H₂SO₄ compared to in water is **weaker**.

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