Basicity of `H_3 BO_3` is

Options

A. 1
B. 2
C. 3
D. 0

Answer

To determine the basicity of boric acid, \( H_3BO_3 \), we can follow these steps:

### Step 1: Understand the Structure of Boric Acid
Boric acid, \( H_3BO_3 \), has a structure where a boron atom is bonded to three hydroxyl groups (–OH). This structure is crucial for understanding its acidic behavior.

**Hint:** Recall that the presence of hydroxyl groups in an acid can influence its ability to donate protons (H⁺ ions).

### Step 2: Reaction with Water
When boric acid reacts with water, it can donate a proton (H⁺) to form the tetrahydroxyborate ion \( B(OH)_4^- \) and release one H⁺ ion into the solution:

\[ H_3BO_3 + H_2O \rightarrow B(OH)_4^- + H^+ \]

**Hint:** Identify how many protons (H⁺) are released when boric acid interacts with water.

### Step 3: Determine the Number of H⁺ Ions Released
From the reaction, we observe that boric acid releases one H⁺ ion per molecule when it reacts with water. This indicates that it can only donate one proton.

**Hint:** Count the number of H⁺ ions produced in the reaction to determine the basicity.

### Step 4: Define Basicity
Basicity refers to the number of protons (H⁺ ions) an acid can donate. Since boric acid donates only one proton, it is classified as a monobasic acid.

**Hint:** Remember that monobasic acids release one H⁺ ion, dibasic acids release two, and so on.

### Conclusion
Therefore, the basicity of \( H_3BO_3 \) is 1, indicating that it is a monobasic acid.

**Final Answer:** The basicity of \( H_3BO_3 \) is 1.

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