`H_(3)BO_(3)` is :

Options

A. Monobasic and weak Lewis acid
B. Monobasic and weak Bronsted acid
C. Tribasic and weak Bronsted acid
D. Monobasic and strong Lewis acid

Explanation

To determine the nature of H₃BO₃ (boric acid), we can analyze its properties step by step.

### Step 1: Identify the Chemical Structure
H₃BO₃ can be represented as B(OH)₃, indicating that it has three hydroxyl (OH) groups attached to a boron atom.

**Hint:** Look at the molecular formula and structure to understand how the atoms are arranged.

### Step 2: Determine the Basicity
Basicity refers to the number of hydrogen ions (H⁺) that an acid can donate. In the case of boric acid, although it has three hydrogen atoms, it does not release any of them as H⁺ ions in solution. Instead, it acts as a Lewis acid.

**Hint:** Remember that basicity is defined by the number of H⁺ ions an acid can donate.

### Step 3: Understand the Lewis Acid Concept
Boric acid can accept a lone pair of electrons from a hydroxide ion (OH⁻) to form a complex ion (B(OH)₄⁻). This behavior is characteristic of Lewis acids, which are defined as substances that accept electron pairs.

**Hint:** Recall that Lewis acids accept electrons, while Lewis bases donate electrons.

### Step 4: Analyze the Bronsted Acid Concept
According to the Bronsted-Lowry theory, an acid is a substance that donates protons (H⁺). Since boric acid does not donate H⁺ ions but rather accepts OH⁻, it does not fit the definition of a Bronsted acid.

**Hint:** Differentiate between Lewis and Bronsted definitions of acids.

### Step 5: Conclusion on Acid Strength
Boric acid is classified as a weak acid because it does not completely dissociate in solution. It is also monobasic because it can accept only one hydroxide ion to form the complex ion.

**Hint:** Consider the strength of an acid based on its ability to dissociate in solution.

### Final Answer
Based on the analysis, H₃BO₃ (boric acid) is a **monobasic and weak Lewis acid**. Therefore, the correct option is:

**Option 1: Monobasic and weak Lewis acid.**