100 c.c. of 0.5 N NaOH Solution is added to 10 c.c. opf 3N `H_(2)SO_(4)` solution and 20 c.c. of 1N HCl solution. The solution will be -

Options

A. Strongly acids
B. Alkaline
C. Neutral
D. Fairly acidic

Answer

To solve the problem, we need to determine the total milliequivalents of the base (NaOH) and the total milliequivalents of the acids (H₂SO₄ and HCl) in the given solutions. Then we will compare these values to see if they neutralize each other.

### Step-by-Step Solution:

1. **Calculate the milliequivalents of NaOH:**
- Given:
- Volume of NaOH solution = 100 c.c. = 100 ml
- Normality of NaOH = 0.5 N
- Formula for milliequivalents:
\[ \text{Milliequivalents} = \text{Normality} \times \text{Volume (ml)} \]
- Calculation:
\[ \text{Milliequivalents of NaOH} = 0.5 \, \text{N} \times 100 \, \text{ml} = 50 \, \text{milliequivalents} \]

2. **Calculate the milliequivalents of H₂SO₄:**
- Given:
- Volume of H₂SO₄ solution = 10 c.c. = 10 ml
- Normality of H₂SO₄ = 3 N
- Calculation:
\[ \text{Milliequivalents of H₂SO₄} = 3 \, \text{N} \times 10 \, \text{ml} = 30 \, \text{milliequivalents} \]

3. **Calculate the milliequivalents of HCl:**
- Given:
- Volume of HCl solution = 20 c.c. = 20 ml
- Normality of HCl = 1 N
- Calculation:
\[ \text{Milliequivalents of HCl} = 1 \, \text{N} \times 20 \, \text{ml} = 20 \, \text{milliequivalents} \]

4. **Total milliequivalents of acids:**
- Combine the milliequivalents of H₂SO₄ and HCl:
\[ \text{Total milliequivalents of acids} = 30 + 20 = 50 \, \text{milliequivalents} \]

5. **Compare the milliequivalents of acids and bases:**
- Milliequivalents of NaOH (base) = 50
- Total milliequivalents of acids (H₂SO₄ + HCl) = 50
- Since the milliequivalents of the base are equal to the milliequivalents of the acids, they will completely neutralize each other.

6. **Conclusion:**
- The solution will be neutral since the amount of acid equals the amount of base.

### Final Answer:
The solution will be neutral.