The mole fractions of glucose $(C_6H_{12}O_6)$ and water $(H_2O)$ in an aqueous glucose solution are $0.0244$ and $0.9756$ respectively. What is the weight percentage $(w/w)$ of glucose in this solution?

The mole fraction of urea in an aqueous urea solution containing $900 \text{ g}$ of water is $0.05$. If the density of the solution is $1.2 \text{ g cm}^{-3}$,the molarity of the urea solution is . . . . . (Given data: Molar masses of urea and water are $60 \text{ g mol}^{-1}$ and $18 \text{ g mol}^{-1}$,respectively)

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 $g/mL$?

$450 \ mg$ of glucose is dissolved in $100 \ g$ of solvent. What is the molality of the solution (in $m$)?

Calculate the mass of urea $(NH_2CONH_2)$ required in making $2.5 \, kg$ of $0.25 \, \text{molal}$ aqueous solution.

The density of '$x$' $M$ solution ('$x$' molar) of $NaOH$ is $1.12 \ g \ mL^{-1}$. While in molality,the concentration of the solution is $3 \ m$ $(3 \ molal)$. Then '$x$' is.
(Given: Molar mass of $NaOH$ is $40 \ g \ mol^{-1}$)