Aqueous solution of aluminium sulphate would show

Options

A. `H^(+)` ions
B. `H_(2)^(+)` ions
C. `H_(3)O^(+)` ions
D. `H_(4)O^(+)` ions

Explanation

To solve the question regarding the behavior of an aqueous solution of aluminium sulphate, we need to analyze the hydrolysis process of aluminium ions in the solution. Here’s a step-by-step breakdown of the solution:

### Step 1: Identify the Compound
The compound in question is aluminium sulphate, which has the chemical formula \( \text{Al}_2(\text{SO}_4)_3 \).

### Step 2: Dissociation in Water
When aluminium sulphate is dissolved in water, it dissociates into aluminium ions (\( \text{Al}^{3+} \)) and sulphate ions (\( \text{SO}_4^{2-} \)):
\[ \text{Al}_2(\text{SO}_4)_3 \rightarrow 2 \text{Al}^{3+} + 3 \text{SO}_4^{2-} \]

### Step 3: Analyze the Ions
- **Sulphate Ion (\( \text{SO}_4^{2-} \))**: This ion comes from a strong acid (sulphuric acid) and does not undergo hydrolysis in water.
- **Aluminium Ion (\( \text{Al}^{3+} \))**: This ion is a cation that can undergo hydrolysis because it is derived from a weak base (aluminium hydroxide).

### Step 4: Hydrolysis of Aluminium Ion
The hydrolysis of the aluminium ion can be represented as follows:
\[ \text{Al}^{3+} + 3 \text{H}_2\text{O} \rightleftharpoons \text{Al(OH)}_3 + 3 \text{H}^+ \]
In this reaction, aluminium ions react with water to form aluminium hydroxide and release hydrogen ions (\( \text{H}^+ \)) into the solution.

### Step 5: Conclusion
The presence of \( \text{H}^+ \) ions in the solution indicates that the solution is acidic. Therefore, an aqueous solution of aluminium sulphate will show acidic properties due to the hydrolysis of aluminium ions.

### Final Answer
An aqueous solution of aluminium sulphate would show an acidic nature due to the hydrolysis of \( \text{Al}^{3+} \) ions, resulting in the formation of \( \text{H}^+ \) ions.

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