STATEMENT-1: `0.1 MH_(3)PO_(3)`(aq) solution has normality equal to 0.3 N when completely reacted with NaOH.
STATEMENT-2 : `H_(3)PO_(3)` is a dibasic acid.

Options

A. If both the statement are TRUE and STATEMENT -2 is the correct explanation of STATEMENT-1
B. If both the statement are TRUE but STATEMENT-2 is NOT the correct explanation of STATEMENT-1
C. If STATEMENT- is 1 TRUE and STATEMENT-2 is FALSE
D. If STATEMENT-1 is FALSE and STATEMENT-2 is TRUE

Answer

To solve the problem, we need to analyze both statements regarding the acid \( H_3PO_3 \) (phosphorous acid) and its properties in relation to normality and basicity.

### Step-by-Step Solution:

1. **Understanding Normality and Molarity**:
- Normality (N) is related to molarity (M) by the equation:
\[ \text{Normality} = \text{Molarity} \times n \]
where \( n \) is the number of equivalents of the acid or base.

2. **Identifying the Molarity**:
- The problem states that the molarity of the \( H_3PO_3 \) solution is \( 0.1 \, M \).

3. **Determining the n Factor**:
- The n factor for an acid is determined by the number of \( H^+ \) ions it can donate.
- For \( H_3PO_3 \), it can donate a maximum of 2 \( H^+ \) ions, which means its n factor is 2.

4. **Calculating Normality**:
- Using the values we have:
\[ \text{Normality} = 0.1 \, M \times 2 = 0.2 \, N \]
- This means that the normality of the \( H_3PO_3 \) solution is \( 0.2 \, N \).

5. **Evaluating Statement 1**:
- Statement 1 claims that the normality is \( 0.3 \, N \). Since we calculated it to be \( 0.2 \, N \), this statement is **incorrect**.

6. **Evaluating Statement 2**:
- Statement 2 claims that \( H_3PO_3 \) is a dibasic acid. Since it can donate 2 \( H^+ \) ions, this statement is **correct**.

### Conclusion:
- **Statement 1 is false** and **Statement 2 is true**.

### Final Answer:
- The correct option is that Statement 1 is false and Statement 2 is true.

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