What volume of NH_3 gas at STP would be neede | vedclass

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(C) $1$. $2.5 \ m$ $NH_4OH$ means $2.5 \ moles$ of $NH_3$ are dissolved in $1000 \ g$ of solvent $(H_2O)$.$2$. Assuming the density of the solution is

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$5.6$

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(C) $1$. $2.5 \ m$ $NH_4OH$ means $2.5 \ moles$ of $NH_3$ are dissolved in $1000 \ g$ of solvent $(H_2O)$.$2$. Assuming the density of the solution is approximately $1 \ g/mL$,the mass of $1000 \ mL$ of solution is $1000 \ g$.$3$. Since $1000 \ g$ of solution contains $2.5 \ moles$ of $NH_3$,then $100 \ mL$ of solution will contain $0.25 \ moles$ of $NH_3$.$4$. At $STP$,$1 \ mole$ of any gas occupies $22.4 \ L$.$5$. Therefore,the volume of $NH_3$ required is $0.25 \ mol 	imes 22.4 \ L/mol = 5.6 \ L$.

What volume of $NH_3$ gas at $STP$ would be needed to prepare $100 \ mL$ of $2.5$ molal $(2.5 \ m)$ ammonium hydroxide solution? (Assume the density of the solution is $1 \ g/mL$)

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