If 100 mL of `1 N H_(2)SO_(4)` is mixed with 100 mL of 1 M NaOH solution. The resulting solution will be

Options

A. Highly acidic
B. Neutral
C. Highly basic
D. Slightly acidic

Answer

To solve the problem of mixing 100 mL of 1 N H₂SO₄ with 100 mL of 1 M NaOH, we will follow these steps:

### Step 1: Determine the moles of H₂SO₄
1. **Calculate the normality and convert it to molarity**:
- Given: Normality (N) of H₂SO₄ = 1 N
- H₂SO₄ can donate 2 protons (H⁺), so its n-factor = 2.
- Molarity (M) = Normality (N) / n-factor = 1 N / 2 = 0.5 M.

2. **Calculate the volume in liters**:
- Volume of H₂SO₄ = 100 mL = 100 / 1000 = 0.1 L.

3. **Calculate moles of H₂SO₄**:
- Moles of H₂SO₄ = Molarity × Volume = 0.5 M × 0.1 L = 0.05 moles.

### Step 2: Determine the moles of NaOH
1. **Given**: Molarity (M) of NaOH = 1 M.
2. **Calculate the volume in liters**:
- Volume of NaOH = 100 mL = 100 / 1000 = 0.1 L.

3. **Calculate moles of NaOH**:
- Moles of NaOH = Molarity × Volume = 1 M × 0.1 L = 0.1 moles.

### Step 3: Write the balanced chemical equation
- The reaction between H₂SO₄ and NaOH is:
\[ H₂SO₄ + 2 NaOH \rightarrow Na₂SO₄ + 2 H₂O \]
- From the equation, 1 mole of H₂SO₄ reacts with 2 moles of NaOH.

### Step 4: Determine the limiting reactant
1. **Calculate the required moles of NaOH for the available moles of H₂SO₄**:
- For 0.05 moles of H₂SO₄, the required moles of NaOH = 0.05 moles H₂SO₄ × 2 = 0.1 moles NaOH.

2. **Compare with available moles of NaOH**:
- Available moles of NaOH = 0.1 moles.
- Since both the required and available moles of NaOH are equal, both reactants are completely consumed.

### Step 5: Determine the nature of the resulting solution
- Since both the acid (H₂SO₄) and the base (NaOH) are completely neutralized, the resulting solution will be neutral.
- The pH of a neutral solution is 7.

### Conclusion
The resulting solution after mixing 100 mL of 1 N H₂SO₄ with 100 mL of 1 M NaOH is **neutral**.

---