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An aqueous solution of urea containing $18 \mathrm{~g}$ urea in $1500 \mathrm{~cm}^{3}$ of the solution has a density equal to $1.052$. If the molecular weight of urea is 60, the molality of the solution is
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The correct answer is:
$0.192$
$$
1500 \mathrm{cc} \text { . solution }=1500 \times 1.052 \mathrm{~g}
$$
$\quad=1578 \mathrm{~g}$
Weight of solvent $=1560 \mathrm{~g}$
$\quad$ Weight of solute $=18 \mathrm{~g}$
Molality $=\frac{\text { weight of solute }}{\text { molecular weight of solute } \times}$
weight of solvent in $\mathrm{kg}$
$=\frac{18 \times 1000}{60 \times 1560}$
$=0.192 \mathrm{~m}$
1500 \mathrm{cc} \text { . solution }=1500 \times 1.052 \mathrm{~g}
$$
$\quad=1578 \mathrm{~g}$
Weight of solvent $=1560 \mathrm{~g}$
$\quad$ Weight of solute $=18 \mathrm{~g}$
Molality $=\frac{\text { weight of solute }}{\text { molecular weight of solute } \times}$
weight of solvent in $\mathrm{kg}$
$=\frac{18 \times 1000}{60 \times 1560}$
$=0.192 \mathrm{~m}$
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