A sample of `Na_(2)CO_(3).H_(2)O` weighing `0.62` g is added to 10 ml of `0.1 N H_(2)SO_(4)` solution . The resulting solution will be

Options

A. Acidic
B. Neutral
C. Basic
D. None of these

Answer

To solve the problem, we need to determine the nature of the resulting solution when a sample of sodium carbonate hydrate (Na₂CO₃·H₂O) is added to a sulfuric acid (H₂SO₄) solution. Here’s a step-by-step breakdown of the solution:

### Step 1: Calculate the number of milliequivalents of H₂SO₄
Given:
- Volume of H₂SO₄ = 10 mL
- Normality of H₂SO₄ = 0.1 N

To find the milliequivalents of H₂SO₄, we use the formula:
\[ \text{Milliequivalents} = \text{Volume (mL)} \times \text{Normality} \]
\[ \text{Milliequivalents of H₂SO₄} = 10 \, \text{mL} \times 0.1 \, \text{N} = 1 \, \text{milliequivalent} \]

### Step 2: Calculate the molecular mass of Na₂CO₃·H₂O
- Molar mass of Na = 23 g/mol (2 Na = 46 g)
- Molar mass of C = 12 g/mol (1 C = 12 g)
- Molar mass of O = 16 g/mol (3 O = 48 g)
- Molar mass of H₂O = 18 g/mol (2 H + 1 O = 18 g)

Calculating the total molecular mass:
\[ \text{Molecular mass of Na₂CO₃·H₂O} = 46 + 12 + 48 + 18 = 124 \, \text{g/mol} \]

### Step 3: Calculate the equivalent weight of Na₂CO₃·H₂O
The n-factor for Na₂CO₃ is 2 (it can donate 2 moles of OH⁻ ions). The equivalent weight is given by:
\[ \text{Equivalent weight} = \frac{\text{Molecular weight}}{\text{n-factor}} = \frac{124 \, \text{g/mol}}{2} = 62 \, \text{g/equiv} \]

### Step 4: Calculate the number of equivalents of Na₂CO₃·H₂O
Given mass of Na₂CO₃·H₂O = 0.62 g
\[ \text{Number of equivalents} = \frac{\text{mass}}{\text{equivalent weight}} = \frac{0.62 \, \text{g}}{62 \, \text{g/equiv}} = 0.01 \, \text{equivalents} \]

### Step 5: Calculate the milliequivalents of Na₂CO₃·H₂O
To convert equivalents to milliequivalents:
\[ \text{Milliequivalents of Na₂CO₃·H₂O} = 0.01 \, \text{equivalents} \times 1000 = 10 \, \text{milliequivalents} \]

### Step 6: Compare the milliequivalents of acid and base
- Milliequivalents of H₂SO₄ = 1
- Milliequivalents of Na₂CO₃·H₂O = 10

### Step 7: Determine the nature of the resulting solution
Since the milliequivalents of Na₂CO₃·H₂O (10) are greater than those of H₂SO₄ (1), the resulting solution will be basic.

### Conclusion
The resulting solution will be **basic** in nature.

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