`100ml` of `0.2 M H_(2)SO_(4)` is added to `100 ml` of `0.2 M NaOH`. The resulting solution will be

Options

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

Answer

To solve the problem of mixing 100 mL of 0.2 M H₂SO₄ with 100 mL of 0.2 M NaOH, we will calculate the milli-equivalents of both the acid and the base and determine the nature of the resulting solution.

### Step-by-Step Solution:

1. **Calculate the milli-equivalents of H₂SO₄:**
- Molarity (M) of H₂SO₄ = 0.2 M
- Volume (V) of H₂SO₄ = 100 mL
- n-factor of H₂SO₄ = 2 (because it dissociates into 2 H⁺ ions)
- Formula for milli-equivalents (meq) = Molarity × Volume (in mL) × n-factor

\[ \text{meq of H₂SO₄} = 0.2 \, \text{M} \times 100 \, \text{mL} \times 2 = 40 \, \text{meq} \]

2. **Calculate the milli-equivalents of NaOH:**
- Molarity (M) of NaOH = 0.2 M
- Volume (V) of NaOH = 100 mL
- n-factor of NaOH = 1 (because it dissociates into 1 OH⁻ ion)
- Using the same formula for milli-equivalents:

\[ \text{meq of NaOH} = 0.2 \, \text{M} \times 100 \, \text{mL} \times 1 = 20 \, \text{meq} \]

3. **Compare the milli-equivalents:**
- Milli-equivalents of H₂SO₄ = 40 meq
- Milli-equivalents of NaOH = 20 meq

Since the milli-equivalents of H₂SO₄ (40 meq) are greater than those of NaOH (20 meq), we conclude that H₂SO₄ is in excess.

4. **Determine the nature of the resulting solution:**
- Since H₂SO₄ is in excess, the resulting solution will be acidic.

### Final Answer:
The resulting solution will be acidic.

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