`0.5g` of an organic compound on `Kjeldahl's` analysis gave enough ammonia to just neutralize `10 cm^(3)` of `1 M H_(2)SO_(4)`. The percentage of nitrogen in the compound is

Answer

To find the percentage of nitrogen in the organic compound using Kjeldahl's analysis, we can follow these steps:

### Step-by-Step Solution:

1. **Understand the given data**:
- Mass of the organic compound = 0.5 g
- Volume of H₂SO₄ = 10 cm³
- Molarity of H₂SO₄ = 1 M

2. **Convert volume from cm³ to mL**:
- Since 1 cm³ = 1 mL, we have:
\[ \text{Volume} = 10 \text{ mL} \]

3. **Determine the basicity of H₂SO₄**:
- The basicity of H₂SO₄ (number of ionizable H⁺ ions) = 2 (because it can donate two protons).

4. **Use the formula for percentage of nitrogen**:
- The formula for calculating the percentage of nitrogen (N) in the compound is:
\[ \text{Percentage of N} = \frac{1.4 \times M \times V \times \text{Basicity}}{\text{Mass of compound}} \]
- Where:
- M = molarity of H₂SO₄ = 1 M
- V = volume of H₂SO₄ in mL = 10 mL
- Basicity = 2
- Mass of compound = 0.5 g

5. **Substitute the values into the formula**:
\[ \text{Percentage of N} = \frac{1.4 \times 1 \times 10 \times 2}{0.5} \]

6. **Calculate**:
- First, calculate the numerator:
\[ 1.4 \times 1 \times 10 \times 2 = 28 \]
- Now, divide by the mass of the compound:
\[ \text{Percentage of N} = \frac{28}{0.5} = 56 \]

7. **Final answer**:
- The percentage of nitrogen in the compound is **56%**.