Boric acid is weak monobasic acid and acts as Lewis acid

Options

A. By donating `H^(oplus)`
B. By accepting `overset (Ө) O H`
C. By donating line pair of electrons
D. By accepting lone pair of electrons

Explanation

### Step-by-Step Solution:

1. **Understanding Boric Acid**:
- Boric acid (H₃BO₃) is a compound of boron that is often represented in its ortho form. It is known to be a weak acid.

2. **Weak Monobasic Acid**:
- A monobasic acid is one that can donate one proton (H⁺) per molecule. In the case of boric acid, it does not dissociate completely in water, which is why it is classified as a weak acid.
- When boric acid is dissolved in water, it interacts with water molecules.

3. **Formation of the Complex**:
- The boron atom in boric acid has an incomplete octet, meaning it has an empty p-orbital. This is crucial for its behavior as an acid.
- When boric acid is mixed with water, the oxygen atom in the water molecule has a lone pair of electrons. This lone pair can be donated to the empty p-orbital of boron.

4. **Proton Donation**:
- As the water molecule donates its lone pair to boron, a coordinate bond is formed between the oxygen of water and boron.
- This interaction leads to the cleavage of a bond in boric acid, resulting in the release of a hydrogen ion (H⁺) into the solution.

5. **Conclusion**:
- Since boric acid can donate one H⁺ ion, it is classified as a monobasic acid.
- Additionally, because it can accept a lone pair of electrons from water, it acts as a Lewis acid.

### Final Statement:
Thus, boric acid is a weak monobasic acid and acts as a Lewis acid due to its ability to accept lone pairs from water and donate protons.

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