An aqueous solution of boric acid is found to be weakly acidic in nature. This acidic character arises due to the following reasons.

Options

A. It is a protic acid which donates protons in aqueous solution.
B. It is a Lewis acid which abstracts `OH^(-)` from water and leaves `H^(+)` to make to solution acidic
C. It gives metaboric acid when dissolved in water.
D. It is prepared by reaction of borax with sulphuric acid hence it behaves as an acid.

Explanation

### Step-by-Step Solution:

1. **Understanding Boric Acid**:
- Boric acid (H₃BO₃) can be represented as B(OH)₃. It is a weak acid when dissolved in water.

2. **Reaction with Water**:
- When boric acid is added to water, it undergoes a reaction:
\[ \text{B(OH)}_3 + \text{H}_2\text{O} \rightleftharpoons \text{B(OH)}_4^- + \text{H}_3\text{O}^+ \]
- This reaction shows that boric acid accepts a hydroxide ion (OH⁻) from water, leading to the formation of the tetrahydroxyborate ion (B(OH)₄⁻) and hydronium ions (H₃O⁺).

3. **Acidic Nature**:
- The presence of H₃O⁺ ions in the solution is what gives the solution its acidic character. An acid is defined as a substance that can donate protons (H⁺ ions) in an aqueous solution.

4. **Lewis Acid Behavior**:
- Boron in boric acid has an incomplete octet (only six electrons around it). It can accept a pair of electrons, making it a Lewis acid.
- The hydroxide ion (OH⁻) acts as a Lewis base by donating a pair of electrons to boron, allowing it to complete its octet.

5. **Conclusion**:
- The weakly acidic nature of boric acid in aqueous solution is primarily due to its ability to accept hydroxide ions and produce hydronium ions, thus acting as a weak acid.

### Final Answer:
The acidic character of boric acid arises because it acts as a Lewis acid, accepting OH⁻ ions from water and generating H₃O⁺ ions.

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