Aqueous solution of two compounds `M_(1) - O - H and M_(2) - O - H` are prepared in two different beakers . If electronegativity of `M_(1) = 3.4, M_(2) = 1.2, 0 = 3.5 and H = 2.1`, then the nature of two solution will be respectively

Options

A. Acidic,acidic
B. acidic,basic
C. basic,basic
D. basic,acidic.

Explanation

To determine the nature of the aqueous solutions of the compounds \( M_1OH \) and \( M_2OH \), we will analyze the electronegativity values of the elements involved and how they influence the character of the bonds in each compound.

### Step-by-Step Solution:

1. **Identify Electronegativity Values**:
- \( M_1 \) has an electronegativity of 3.4.
- \( M_2 \) has an electronegativity of 1.2.
- Oxygen (O) has an electronegativity of 3.5.
- Hydrogen (H) has an electronegativity of 2.1.

2. **Analyze Compound \( M_1OH \)**:
- Calculate the electronegativity difference between \( M_1 \) and O:
\[ \text{Difference} = |3.4 - 3.5| = 0.1 \]
- Calculate the electronegativity difference between O and H:
\[ \text{Difference} = |3.5 - 2.1| = 1.4 \]
- Since the difference between \( M_1 \) and O is small (0.1), the bond between \( M_1 \) and O is more covalent in nature. However, the bond between O and H has a larger difference (1.4), indicating it is more ionic.

3. **Determine the Nature of \( M_1OH \)**:
- The bond between O and H is more ionic, leading to the release of \( H^+ \) ions in solution. Therefore, \( M_1OH \) is **acidic** in nature.

4. **Analyze Compound \( M_2OH \)**:
- Calculate the electronegativity difference between \( M_2 \) and O:
\[ \text{Difference} = |1.2 - 3.5| = 2.3 \]
- Calculate the electronegativity difference between O and H:
\[ \text{Difference} = |3.5 - 2.1| = 1.4 \]
- The difference between \( M_2 \) and O is large (2.3), indicating a more ionic character for the bond between \( M_2 \) and O. The bond between O and H remains more ionic.

5. **Determine the Nature of \( M_2OH \)**:
- The bond between \( M_2 \) and O is more ionic, leading to the release of \( OH^- \) ions in solution. Therefore, \( M_2OH \) is **basic** in nature.

### Conclusion:
The nature of the two solutions is:
- \( M_1OH \): Acidic
- \( M_2OH \): Basic

Thus, the final answer is **acidic and basic** respectively.