One molar solution of sulphuric acid is equal to

Options

A. Normal solution
B. `(N)/(2)` solution
C. 2N solution
D. 4 N solution

Answer

To determine the normality of a one molar solution of sulfuric acid (H₂SO₄), we will follow these steps:

### Step 1: Understand Molarity and Normality
- Molarity (M) is defined as the number of moles of solute per liter of solution.
- Normality (N) is defined as the number of gram equivalents of solute per liter of solution.

### Step 2: Relate Normality to Molarity
- The relationship between normality and molarity can be expressed as:
\[ \text{Normality} = \text{Molarity} \times n \text{ factor} \]
where the n factor is the number of equivalents of the solute.

### Step 3: Determine the n Factor for Sulfuric Acid
- For sulfuric acid (H₂SO₄), the n factor is determined by its basicity, which is the number of replaceable hydrogen ions (H⁺) in the acid.
- H₂SO₄ can donate two protons (H⁺) in a reaction, so its n factor is 2.

### Step 4: Calculate Normality
- Given that the molarity of the solution is 1 M, we can substitute the values into the formula:
\[ \text{Normality} = 1 \, \text{M} \times 2 = 2 \, \text{N} \]

### Step 5: Conclusion
- Therefore, a one molar solution of sulfuric acid is equal to 2 normal solutions.

### Final Answer:
The correct answer is **2 normal solution (2 N)**.

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