A 0.166 g sample of an organic compound was digested with conc. H2SO4 and then distilled with NaOH. The ammonia gas evolved was passed through 50.0 mL of 0.5 N H2SO4. The used acid required 30.0 mL of 0.25 N NaOH for complete neutralization. The mass percentage of nitrogen in the organic compound is ____________.
Answer (integer)
63
Solution
Millimoles of used acid $=\frac{30 \times 0.25}{2}$
<br/><br/>
Millimoles of $\mathrm{NH}_{3}=30 \times 0.25=7.5$
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Mass $\%$ of nitrogen $=\frac{7.5}{0.166} \times 10^{-3} \times 14 \times 100 \simeq 63 \%$
About this question
Subject: Chemistry · Chapter: Some Basic Concepts of Chemistry · Topic: Mole Concept
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