Which amongst the following has the highest normality ?

Options

A. 16.0 g of NaOH in 200 mL of water
B. 1 N oxalic acid
C. 2 M sulphuric acid
D. 1.5 N hydrochloric acid

Answer

To determine which solution has the highest normality, we will analyze each option step by step.

### Step 1: Understanding Normality
Normality (N) is defined as the number of gram equivalents of solute per liter of solution. For acids, normality can be calculated as:
\[ \text{Normality} = \text{Molarity} \times \text{Basicity} \]
For bases, it is:
\[ \text{Normality} = \text{Molarity} \times \text{Acidity} \]

### Step 2: Analyzing Each Option

#### Option 1: 16.0 grams of NaOH in 1200 mL of water
1. **Calculate moles of NaOH**:
\[ \text{Moles of NaOH} = \frac{\text{mass}}{\text{molar mass}} = \frac{16 \text{ g}}{40 \text{ g/mol}} = 0.4 \text{ moles} \]

2. **Convert volume to liters**:
\[ 1200 \text{ mL} = 1.2 \text{ L} \]

3. **Calculate molarity**:
\[ \text{Molarity} = \frac{\text{moles of solute}}{\text{volume of solution in L}} = \frac{0.4 \text{ moles}}{1.2 \text{ L}} = \frac{0.4}{1.2} = 0.333 \text{ M} \]

4. **Calculate normality**:
Since NaOH has one replaceable OH group (acidity = 1):
\[ \text{Normality} = \text{Molarity} \times \text{Acidity} = 0.333 \text{ M} \times 1 = 0.333 \text{ N} \]

#### Option 2: 1 Normal Oxalic Acid
- The concentration is already given as 1 Normal (1 N).

#### Option 3: 2 Molar Sulfuric Acid
1. **Calculate normality**:
Sulfuric acid (H₂SO₄) has two replaceable hydrogens (basicity = 2):
\[ \text{Normality} = \text{Molarity} \times \text{Basicity} = 2 \text{ M} \times 2 = 4 \text{ N} \]

#### Option 4: 1.5 Normal Hydrochloric Acid
- The concentration is already given as 1.5 Normal (1.5 N).

### Step 3: Comparing Normalities
- Option 1: 0.333 N (NaOH)
- Option 2: 1 N (Oxalic Acid)
- Option 3: 4 N (Sulfuric Acid)
- Option 4: 1.5 N (Hydrochloric Acid)

### Conclusion
The solution with the highest normality is from Option 3: **2 Molar Sulfuric Acid**, which is **4 Normal**.