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A sample of 0.50 g of an organic compoun...

A sample of 0.50 g of an organic compound was treated according to Kjeldahl's method. The ammonia evolved was absorbed in 50 mL of 0.5 M `H_(2)SO_(4)`. The residual acid required 60 mL of 0.5 M solution of NaOH for neutralisation. What would be the percentage composition of nitrogen in the compound?

A

50

B

60

C

56

D

44

Text Solution

Verified by Experts

The correct Answer is:
C
Given:
Mass of compound taken=0.50g
Vol. of `H_(2)SO_(4)=50`mL
Molarity of `H_(2)SO_(4)=0.5M`
Vol. of NaOH required=60mL
Molarity of NaOH requried=0.5M
Method adopted Kjeldahl's method
Formula used: % of N`=(1.4xxMxx2[V-(V_(1))/(2)])/(m)` . . (i)
by substituting the vlaues in the formula, we get
`%` of `N=(1.4xx0.5xx2(50-60//2))/(0.5)=56`
`therefore` % of N in the given compound=56%
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A sample of 0.50 g of an organic compound was treated according to Kjeldahl's method. The ammonia evolved was absorbed in 50 mL of 0.5 M H_(2)SO_(4) . The residual acid required 60 mL of 0.5 M solution of NaOH for neutralization. Find the percentage composition of nitrogen in the compound. Strategy: Step 1 . Convert molarity into normality using the relation Normality (N) = n xx Molarity (M) where n factor is either the acidity of base or basicity of acid. Step 2 . Calculate the milliequivalents of NaOH which is equal to the milliequivalents of unreacted H_(2)SO_(4) . Step 3 . Calculate the milliequivalents of total H_(2)SO_(4) and subtract the milliequivalents of unreacted H_(2)SO_(4) to get the milliequivalents of NH_(3) evolved. Step 4 . Calculate the equivalents of NH_(3) , moles of NH_(3) , and moles of N . Step 5 . Calculate the mass of N in the organic compound. Step 6 . Finally, calculate % of N or directly apply Eq. (13.8) or (13.9) to get the % of N in the organic compound.

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