A 250 mL solution of sulfuric acid (H₂SO₄) is prepared by dissolving 2.45 grams of H₂SO₄ in water. What is the normality of the solution?

To find the normality (N) of the sulfuric acid (H₂SO₄) solution, we need to follow these steps:

### Step 1: Calculate the molar mass of H₂SO₄
The molar mass of H₂SO₄ is calculated by summing the atomic masses of its components:
- Hydrogen (H): 1.008 g/mol × 2 = 2.016 g/mol
- Sulfur (S): 32.06 g/mol
- Oxygen (O): 16.00 g/mol × 4 = 64.00 g/mol

So, the molar mass of H₂SO₄ = 2.016 + 32.06 + 64.00 = **98.08 g/mol**

### Step 2: Calculate the number of moles of H₂SO₄
We can now find the number of moles of H₂SO₄ using the mass and molar mass:

\[
\text{Moles of H₂SO₄} = \frac{\text{mass of H₂SO₄}}{\text{molar mass of H₂SO₄}} = \frac{2.45 \, \text{g}}{98.08 \, \text{g/mol}} = 0.0250 \, \text{mol}
\]

### Step 3: Determine the equivalent factor of H₂SO₄
Sulfuric acid (H₂SO₄) is a diprotic acid, meaning it can donate 2 protons (H⁺ ions). Therefore, the equivalent factor is 2.

### Step 4: Calculate the normality (N)
Normality is calculated using the formula:

\[
\text{Normality (N)} = \frac{\text{equivalents of solute}}{\text{volume of solution in liters}}
\]

The equivalents of solute are calculated as:

\[
\text{Equivalents of solute} = \text{moles of H₂SO₄} \times \text{equivalent factor} = 0.0250 \, \text{mol} \times 2 = 0.0500 \, \text{equivalents}
\]

The volume of the solution is 250 mL, which is 0.250 L. Now, we can calculate the normality:

\[
\text{Normality (N)} = \frac{0.0500 \, \text{equivalents}}{0.250 \, \text{L}} = 0.200 \, \text{N}
\]

### Conclusion:
The normality of the H₂SO₄ solution is **0.200 N**.

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Would you like further details or have any questions?

### Related Questions:
1. How is normality different from molarity?
2. Can the normality of a diprotic acid change depending on the reaction?
3. How do you calculate normality for a base like NaOH?
4. What is the significance of normality in titration calculations?
5. How do you calculate the normality if the volume of the solution is increased?

**Tip**: When dealing with acids and bases, remember that normality takes into account the number of ions that react, which can differ from molarity.

Learn how to calculate the normality of a sulfuric acid (H₂SO₄) solution with a detailed step-by-step explanation. This example involves dissolving 2.45 grams of H₂SO₄ in 250 mL of water and covers key concepts like stoichiometry, molarity, and acid-base chemistry. Ideal for students in Grades 11-12.

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