Normality of `2M H_2 SO_4` is

Options

A. 4 N
B. 6 N
C. `N/4`
D. `N/6`

Answer

To find the normality of a 2M solution of \( H_2SO_4 \), we can follow these steps:

### Step 1: Understand the Definition of Normality
Normality (N) is defined as the number of equivalents of solute per liter of solution. It is related to molarity (M) by the formula:
\[ \text{Normality} = \text{Molarity} \times \text{Valence Factor} \]

### Step 2: Determine the Valence Factor
The valence factor for an acid is determined by the number of hydrogen ions (\( H^+ \)) it can donate. For sulfuric acid (\( H_2SO_4 \)), when it dissociates in solution, it produces:
\[ H_2SO_4 \rightarrow 2H^+ + SO_4^{2-} \]
This means that one molecule of \( H_2SO_4 \) can donate 2 \( H^+ \) ions. Therefore, the valence factor for \( H_2SO_4 \) is 2.

### Step 3: Calculate Normality
Now that we have the molarity and the valence factor, we can calculate the normality:
\[ \text{Normality} = \text{Molarity} \times \text{Valence Factor} = 2M \times 2 = 4N \]

### Step 4: Conclusion
Thus, the normality of a 2M solution of \( H_2SO_4 \) is 4N.

### Final Answer
The normality of \( 2M H_2SO_4 \) is **4N**.

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