What will be normality of the resultant solution when 500 ml `1 N H_2SO_4`, 300 ml `HCl` and 200 ml `5N HNO_3` are mixed together and then volume was made 2000 ml by adding some water ?

Options

A. 0.9 N
B. 2 N
C. 1.9 N
D. 4 N

Answer

To find the normality of the resultant solution when mixing different solutions, we can follow these steps:

### Step 1: Calculate the equivalent molarity for each solution.

1. **For H₂SO₄:**
- Normality (N) = 1 N
- Volume (V) = 500 ml = 0.5 L
- Equivalent Molarity = Normality × Volume = 1 N × 0.5 L = 0.5 equivalents

2. **For HCl:**
- Normality (N) = 1 N (since it's a strong acid, we assume 1 N)
- Volume (V) = 300 ml = 0.3 L
- Equivalent Molarity = Normality × Volume = 1 N × 0.3 L = 0.3 equivalents

3. **For HNO₃:**
- Normality (N) = 5 N
- Volume (V) = 200 ml = 0.2 L
- Equivalent Molarity = Normality × Volume = 5 N × 0.2 L = 1.0 equivalents

### Step 2: Sum the equivalent molarities.

- Total Equivalent Molarity = Equivalent Molarity of H₂SO₄ + Equivalent Molarity of HCl + Equivalent Molarity of HNO₃
- Total Equivalent Molarity = 0.5 + 0.3 + 1.0 = 1.8 equivalents

### Step 3: Calculate the total volume of the resultant solution.

- Total Volume = 2000 ml = 2 L

### Step 4: Calculate the normality of the resultant solution.

Using the formula:
\[ \text{Normality} = \frac{\text{Total Equivalent Molarity}}{\text{Total Volume}} \]

Substituting the values:
\[ \text{Normality} = \frac{1.8 \text{ equivalents}}{2 \text{ L}} = 0.9 \text{ N} \]

### Final Answer:
The normality of the resultant solution is **0.9 N**.

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