200 ml 0.6 N `H_(2)SO_(4)` and 100 ml of 0.3 N HCl are mixed together. Acidic normality of the resultant solution is

Options

A. 0.5 N
B. 0.9 N
C. 0.3 N
D. 0.6 N

Explanation

To find the acidic normality of the resultant solution when mixing 200 ml of 0.6 N H₂SO₄ and 100 ml of 0.3 N HCl, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Normality and Volume of Each Acid:**
- For H₂SO₄:
- Normality (N₁) = 0.6 N
- Volume (V₁) = 200 ml
- For HCl:
- Normality (N₂) = 0.3 N
- Volume (V₂) = 100 ml

2. **Calculate the Number of Milliequivalents for Each Acid:**
- The formula for milliequivalents is:
\[ \text{Milliequivalents} = \text{Normality} \times \text{Volume (ml)} \]
- For H₂SO₄:
\[ \text{Milliequivalents of H₂SO₄} = N₁ \times V₁ = 0.6 \, \text{N} \times 200 \, \text{ml} = 120 \, \text{meq} \]
- For HCl:
\[ \text{Milliequivalents of HCl} = N₂ \times V₂ = 0.3 \, \text{N} \times 100 \, \text{ml} = 30 \, \text{meq} \]

3. **Calculate the Total Milliequivalents:**
- Total milliequivalents in the resultant solution:
\[ \text{Total milliequivalents} = \text{Milliequivalents of H₂SO₄} + \text{Milliequivalents of HCl} = 120 \, \text{meq} + 30 \, \text{meq} = 150 \, \text{meq} \]

4. **Calculate the Total Volume of the Resultant Solution:**
- Total volume (V) = Volume of H₂SO₄ + Volume of HCl:
\[ V = V₁ + V₂ = 200 \, \text{ml} + 100 \, \text{ml} = 300 \, \text{ml} \]

5. **Calculate the Acidic Normality of the Resultant Solution:**
- Normality (N) of the resultant solution is given by:
\[ N = \frac{\text{Total milliequivalents}}{\text{Total volume (ml)}} \]
- Substituting the values:
\[ N = \frac{150 \, \text{meq}}{300 \, \text{ml}} = 0.5 \, \text{N} \]

### Conclusion:
The acidic normality of the resultant solution is **0.5 N**.