If 100 mL of `1NH_(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 what happens when 100 mL of 1 N H₂SO₄ is mixed with 100 mL of 1 M NaOH, we will follow these steps:

### Step 1: Understand the Normality and Molarity
- Given:
- H₂SO₄ is a diprotic acid, meaning it can donate 2 protons (H⁺ ions).
- The normality (N) of H₂SO₄ is given as 1 N.

### Step 2: Convert Normality to Molarity
- The relationship between normality and molarity for acids is given by:
\[ \text{Normality (N)} = \text{Molarity (M)} \times n \]
where \( n \) is the number of protons that can be donated.
- For H₂SO₄, \( n = 2 \):
\[ 1 \, \text{N} = \text{Molarity (M)} \times 2 \implies \text{Molarity (M)} = \frac{1}{2} = 0.5 \, \text{M} \]

### Step 3: Calculate Moles of H₂SO₄ and NaOH
- Volume of H₂SO₄ = 100 mL = 0.1 L
- Molarity of H₂SO₄ = 0.5 M
- Moles of H₂SO₄:
\[ \text{Moles of H₂SO₄} = \text{Molarity} \times \text{Volume} = 0.5 \, \text{mol/L} \times 0.1 \, \text{L} = 0.05 \, \text{mol} \]

- Volume of NaOH = 100 mL = 0.1 L
- Molarity of NaOH = 1 M
- Moles of NaOH:
\[ \text{Moles of NaOH} = \text{Molarity} \times \text{Volume} = 1 \, \text{mol/L} \times 0.1 \, \text{L} = 0.1 \, \text{mol} \]

### Step 4: Determine the Reaction
- The balanced chemical reaction between H₂SO₄ and NaOH is:
\[ H₂SO₄ + 2 \, NaOH \rightarrow Na₂SO₄ + 2 \, H₂O \]
- From the reaction, we see that 1 mole of H₂SO₄ reacts with 2 moles of NaOH.

### Step 5: Determine Limiting Reactant
- We have 0.05 moles of H₂SO₄ and 0.1 moles of NaOH.
- According to the stoichiometry:
- 0.05 moles of H₂SO₄ would require \( 2 \times 0.05 = 0.1 \) moles of NaOH.
- Since we have exactly 0.1 moles of NaOH, both reactants will completely react.

### Step 6: Analyze the Resulting Solution
- After the reaction, we will have:
- Products: Na₂SO₄ (salt) and water.
- The resulting solution will contain only the salt (Na₂SO₄) and water, which is neutral.

### Conclusion
- The resulting solution will be neutral.

### Final Answer
The resulting solution will be **Neutral**.

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