(D) $1$. Molar mass of urea $(NH_2CONH_2) = 2(14) + 4(1) + 12 + 16 = 60 \text{ g mol}^{-1}$.$2$. For $100 \text{ g}$ of solution, mass of urea $= 10 \

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(D) $1$. Molar mass of urea $(NH_2CONH_2) = 2(14) + 4(1) + 12 + 16 = 60 \text{ g mol}^{-1}$.$2$. For $100 \text{ g}$ of solution, mass of urea $= 10 \text{ g}$, mass of water $= 90 \text{ g}$.$3$. Moles of urea $= 10 / 60 = 1/6 \approx 0.1667 \text{ mol}$.$4$. Moles of water $= 90 / 18 = 5 \text{ mol}$.$5$. Mole fraction of water $(x_{H_2O}) = \frac{n_{H_2O}}{n_{H_2O} + n_{urea}} = \frac{5}{5 + 0.1667} = \frac{5}{5.1667} \approx 0.967$.

Class 12 Chemistry Solutions Method of expressing concentration of solution

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What is the mole fraction of water in $10\%$ by weight $(w/w)$ of aqueous urea solution? [Given: Molar mass of $H, O, C$ and $N$ are $1, 16, 12$ and $14 \text{ g mol}^{-1}$ respectively.]

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A
$0.825$
B
$0.032$
C
$0.867$
D
$0.967$

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What is the mole fraction of water in $10\%$ by weight $(w/w)$ of aqueous urea solution? [Given: Molar mass of $H, O, C$ and $N$ are $1, 16, 12$ and $14 \text{ g mol}^{-1}$ respectively.]

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If the molarity and molality of an aqueous solution of $H_2SO_4$ are $1.56 \ M$ and $1.8 \ m$ respectively,what is the density of the solution in $g/mL$?

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