The density of NH_4OH solution is found to be | vedclass

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(D) Given: Density $(d)$ = $0.6 \, g/mL$,Mass percentage = $35 \%$,Molar mass of $NH_4OH$ = $35 \, g/mol$.Since $NH_4OH$ is a monoacidic base,its equi

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$6$

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(D) Given: Density $(d)$ = $0.6 \, g/mL$,Mass percentage = $35 \%$,Molar mass of $NH_4OH$ = $35 \, g/mol$.Since $NH_4OH$ is a monoacidic base,its equivalent mass $(E)$ is equal to its molar mass,$E = 35 \, g/eq$.Consider $100 \, g$ of the solution. The mass of $NH_4OH$ $(W)$ = $35 \, g$.The volume of the solution $(V)$ = $\frac{	ext{mass}}{	ext{density}} = \frac{100 \, g}{0.6 \, g/mL} = \frac{100}{0.6} \, mL = \frac{100}{0.6 	imes 1000} \, L$.Normality $(N)$ = $\frac{W}{E 	imes V(L)} = \frac{35}{35 	imes (100 / (0.6 	imes 1000))} = \frac{0.6 	imes 1000}{100} = 6 \, N$.

The density of $NH_4OH$ solution is found to be $0.6 \, g/mL$. It contains $35 \%$ by mass of $NH_4OH$. The normality of the solution is ......... $N$.

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