The `pH` an aqueous solution of `Al^(3+)` is likely to be.

Options

A. Neutral
B. Acidic
C. Slightly basic
D. Highly basic

Explanation

To determine the pH of an aqueous solution of \( \text{Al}^{3+} \), we can follow these steps:

### Step 1: Understand the nature of \( \text{Al}^{3+} \) in solution
When aluminum ions \( \text{Al}^{3+} \) are dissolved in water, they interact with water molecules.

### Step 2: Formation of Hydroxo Complex
The \( \text{Al}^{3+} \) ions can react with water to form aluminum hydroxide complexes:
\[ \text{Al}^{3+} + 3 \text{H}_2\text{O} \rightarrow \text{Al(OH)}_3 + 3 \text{H}^+ \]
This reaction indicates that aluminum ions can hydrolyze in water.

### Step 3: Release of \( \text{H}^+ \) Ions
During this hydrolysis, \( \text{H}^+ \) ions are released into the solution. The presence of these \( \text{H}^+ \) ions is crucial because they determine the acidity of the solution.

### Step 4: Determine the pH
The release of \( \text{H}^+ \) ions means that the solution will have an increased concentration of hydrogen ions, leading to a decrease in pH. Therefore, the solution will be acidic.

### Conclusion
Based on the hydrolysis of \( \text{Al}^{3+} \) and the release of \( \text{H}^+ \) ions, we conclude that the pH of the aqueous solution of \( \text{Al}^{3+} \) is likely to be acidic.

### Final Answer
The pH of an aqueous solution of \( \text{Al}^{3+} \) is likely to be **acidic**.

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