Kjeldahl's method was used for the estimation | vedclass

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(D) The reaction for the neutralization of ammonia by sulfuric acid is: $2NH_3 + H_2SO_4 \rightarrow (NH_4)_2SO_4$.Number of milliequivalents $(meq)$

Vedclass · Accepted Answer

$64$

Vedclass · Answer

(D) The reaction for the neutralization of ammonia by sulfuric acid is: $2NH_3 + H_2SO_4 ightarrow (NH_4)_2SO_4$.Number of milliequivalents $(meq)$ of $H_2SO_4$ used = $Molarity 	imes Volume 	imes n	ext{-factor} = 1 \ M 	imes 12.5 \ mL 	imes 2 = 25 \ meq$.Since $1 \ meq$ of $NH_3$ reacts with $1 \ meq$ of $H_2SO_4$,the $meq$ of $NH_3$ evolved = $25 \ meq$.Mass of nitrogen = $\frac{meq 	imes 14}{1000} = \frac{25 	imes 14}{1000} = 0.35 \ g$.Percentage of nitrogen = $\frac{	ext{Mass of nitrogen}}{	ext{Mass of compound}} 	imes 100 = \frac{0.35}{0.55} 	imes 100 = 63.63\%$.Rounding to the nearest integer,we get $64\%$.

Kjeldahl's method was used for the estimation of nitrogen in an organic compound. The ammonia evolved from $0.55 \ g$ of the compound neutralized $12.5 \ mL$ of $1 \ M \ H_2SO_4$ solution. The percentage of nitrogen in the compound is $.....$ (Nearest integer).

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Fill in the blanks:
$(1)$ .......... gas is produced in Kjeldahl's method and absorbed in ...........
$(2)$ The excess $H_2SO_4$ is added in Kjeldahl's method and then the remaining $H_2SO_4$ is titrated with a calculated ..........

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