In Kjeldahl's method for the estimation of nitrogen,$3.88 \ mg$ of an organic compound produces ammonia which requires $5.73 \ mL$ of $0.011 \ N$ $HCl$ for neutralization. Calculate the percentage of nitrogen in the compound.

(N/A) The formula for the percentage of nitrogen in Kjeldahl's method is: $\% \ N = \frac{1.4 \times N \times V}{W}$,where $N$ is the normality of $HCl$,$V$ is the volume of $HCl$ in $mL$,and $W$ is the weight of the compound in $mg$.
Substituting the given values: $\% \ N = \frac{1.4 \times 0.011 \times 5.73}{3.88}$.
$\% \ N = \frac{0.088242}{3.88} \approx 2.274 \%$.
Note: The provided solution $22.74 \%$ appears to be a calculation error by a factor of $10$. The correct calculated value is $2.274 \%$.