Calculate the normality and molarity of `H_2SO_4` solution containing 4.9 g of `H_2SO_4` per litre of the solution.

Answer

To calculate the normality and molarity of a `H2SO4` solution containing 4.9 g of `H2SO4` per liter, we will follow these steps:

### Step 1: Calculate the Molar Mass of `H2SO4`
The molar mass of sulfuric acid (`H2SO4`) can be calculated as follows:
- Hydrogen (H): 1 g/mol × 2 = 2 g/mol
- Sulfur (S): 32 g/mol × 1 = 32 g/mol
- Oxygen (O): 16 g/mol × 4 = 64 g/mol

Adding these together:
\[ \text{Molar mass of } H2SO4 = 2 + 32 + 64 = 98 \text{ g/mol} \]

### Step 2: Calculate the Number of Moles of `H2SO4`
Using the formula for moles:
\[ \text{Moles of } H2SO4 = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}} \]

Substituting the values:
\[ \text{Moles of } H2SO4 = \frac{4.9 \text{ g}}{98 \text{ g/mol}} = 0.05 \text{ moles} \]

### Step 3: Calculate the Molarity of the Solution
Molarity (M) is defined as the number of moles of solute per liter of solution:
\[ \text{Molarity} = \frac{\text{moles of solute}}{\text{volume of solution (L)}} \]

Substituting the values:
\[ \text{Molarity} = \frac{0.05 \text{ moles}}{1 \text{ L}} = 0.05 \text{ M} \]

### Step 4: Calculate the Normality of the Solution
Normality (N) is defined as the number of equivalents of solute per liter of solution. For acids, it is calculated as:
\[ \text{Normality} = \text{Basicity} \times \text{Molarity} \]

For sulfuric acid (`H2SO4`), the basicity is 2 (since it can donate 2 protons). Therefore:
\[ \text{Normality} = 2 \times 0.05 \text{ M} = 0.1 \text{ N} \]

### Final Results
- Molarity of the `H2SO4` solution = 0.05 M
- Normality of the `H2SO4` solution = 0.1 N

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