If one mole of `H_(2)SO_(4)` reacts with one mole of NaOH, equivalent weight of `H_(2)SO_(4)` will be :

Options

A. 98
B. 49
C. 96
D. 48

Answer

To find the equivalent weight of sulfuric acid (H₂SO₄) when it reacts with sodium hydroxide (NaOH), we can follow these steps:

### Step 1: Understand the reaction
When sulfuric acid (H₂SO₄) reacts with sodium hydroxide (NaOH), it can donate hydrogen ions (H⁺) to form water and sodium sulfate (Na₂SO₄). The balanced reaction is:
\[ H_2SO_4 + 2 NaOH \rightarrow Na_2SO_4 + 2 H_2O \]

### Step 2: Determine the molecular weight of H₂SO₄
The molecular weight of H₂SO₄ can be calculated using the atomic weights of its constituent elements:
- Hydrogen (H): 1 g/mol (2 H atoms contribute 2 g/mol)
- Sulfur (S): 32 g/mol (1 S atom contributes 32 g/mol)
- Oxygen (O): 16 g/mol (4 O atoms contribute 64 g/mol)

Thus, the molecular weight of H₂SO₄ is:
\[ 2 + 32 + 64 = 98 \, \text{g/mol} \]

### Step 3: Identify the number of replaceable hydrogen atoms
In the reaction, H₂SO₄ can release two hydrogen ions (H⁺) in total, but since it reacts with one mole of NaOH, we consider only one of the hydrogen ions being replaced in this scenario. Therefore, the number of replaceable hydrogen atoms is 1.

### Step 4: Calculate the equivalent weight
The equivalent weight of an acid is calculated using the formula:
\[ \text{Equivalent Weight} = \frac{\text{Molecular Weight}}{\text{Number of Replaceable Hydrogen Atoms}} \]

Substituting the values we have:
\[ \text{Equivalent Weight of H₂SO₄} = \frac{98 \, \text{g/mol}}{1} = 98 \, \text{g/equiv} \]

### Conclusion
The equivalent weight of H₂SO₄ is 98 g/equiv.

### Final Answer
The correct option is **98**.

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