What is the nature of the resulting solution prepared from 100ml to `0.2M` `H_2SO_4` added to 100ml of `0.2 M` `NaOH`.

Options

A. Neutral
B. Acidic
C. Basic
D. Slightly basic

Answer

To determine the nature of the resulting solution when 100 mL of 0.2 M H₂SO₄ is mixed with 100 mL of 0.2 M NaOH, we can follow these steps:

### Step-by-Step Solution:

1. **Calculate the moles of H₂SO₄:**
- The concentration of H₂SO₄ is 0.2 M, and the volume is 100 mL (which is 0.1 L).
- Moles of H₂SO₄ = Concentration × Volume = 0.2 mol/L × 0.1 L = 0.02 moles.

2. **Determine the moles of H⁺ ions from H₂SO₄:**
- H₂SO₄ is a strong acid that dissociates completely in water to give 2 H⁺ ions per molecule.
- Therefore, moles of H⁺ = 2 × moles of H₂SO₄ = 2 × 0.02 = 0.04 moles of H⁺.

3. **Calculate the moles of NaOH:**
- The concentration of NaOH is also 0.2 M, and the volume is 100 mL (0.1 L).
- Moles of NaOH = Concentration × Volume = 0.2 mol/L × 0.1 L = 0.02 moles.

4. **Determine the moles of OH⁻ ions from NaOH:**
- NaOH is a strong base that dissociates completely in water to give 1 OH⁻ ion per molecule.
- Therefore, moles of OH⁻ = moles of NaOH = 0.02 moles.

5. **Neutralization Reaction:**
- The reaction between H⁺ and OH⁻ can be represented as:
\[ H^+ + OH^- \rightarrow H_2O \]
- Since we have 0.04 moles of H⁺ and 0.02 moles of OH⁻, they will react in a 1:1 ratio.
- After neutralization, the remaining moles of H⁺ will be:
\[ \text{Remaining H}^+ = 0.04 - 0.02 = 0.02 \text{ moles} \]

6. **Calculate the total volume of the solution:**
- The total volume after mixing is 100 mL + 100 mL = 200 mL (0.2 L).

7. **Calculate the concentration of H⁺ in the resulting solution:**
- Concentration of H⁺ = Remaining moles of H⁺ / Total volume = 0.02 moles / 0.2 L = 0.1 M.

8. **Determine the pH of the solution:**
- pH = -log[H⁺] = -log(0.1) = 1.

### Conclusion:
Since the pH of the resulting solution is 1, it indicates that the solution is acidic.