If `100mL` of `1N` sulphuric acid were mixed with 100mL of 1N sodium hydroxide, the solution will be

Options

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

Explanation

To solve the problem of mixing 100 mL of 1N sulfuric acid (H₂SO₄) with 100 mL of 1N sodium hydroxide (NaOH), we can follow these steps:

### Step 1: Understand the Reaction
Sulfuric acid (H₂SO₄) is a strong acid, and sodium hydroxide (NaOH) is a strong base. When they are mixed, they undergo a neutralization reaction:
\[ \text{H}_2\text{SO}_4 + 2 \text{NaOH} \rightarrow \text{Na}_2\text{SO}_4 + 2 \text{H}_2\text{O} \]

### Step 2: Calculate Moles of Reactants
1. **Moles of H₂SO₄:**
- Normality (N) = 1N means 1 equivalent of H₂SO₄ per liter.
- Volume of H₂SO₄ = 100 mL = 0.1 L
- Moles of H₂SO₄ = Normality × Volume = 1 × 0.1 = 0.1 equivalents

2. **Moles of NaOH:**
- Normality (N) = 1N means 1 equivalent of NaOH per liter.
- Volume of NaOH = 100 mL = 0.1 L
- Moles of NaOH = Normality × Volume = 1 × 0.1 = 0.1 equivalents

### Step 3: Determine the Stoichiometry of the Reaction
From the reaction equation, we see that 1 mole of H₂SO₄ reacts with 2 moles of NaOH. Therefore, to completely neutralize 0.1 equivalents of H₂SO₄, we need:
\[ 0.1 \text{ equivalents of H}_2\text{SO}_4 \times 2 = 0.2 \text{ equivalents of NaOH} \]

### Step 4: Compare Available Equivalents
- We have 0.1 equivalents of H₂SO₄ and 0.1 equivalents of NaOH.
- Since we need 0.2 equivalents of NaOH to completely neutralize 0.1 equivalents of H₂SO₄, we do not have enough NaOH to neutralize all the H₂SO₄.

### Step 5: Determine the Resulting Solution
Since there is excess H₂SO₄ (0.1 equivalents of H₂SO₄ and only 0.1 equivalents of NaOH), the solution will be acidic.

### Conclusion
The resulting solution after mixing 100 mL of 1N sulfuric acid with 100 mL of 1N sodium hydroxide will be **acidic**.

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