If a substance $A$ dissolves in a solution of a mixture of $B$ and $C$ with their respective number of moles as $n_A, n_B$ and $n_C$,the mole fraction of $C$ in the solution is:

If the mole fraction of $H_2SO_4$ in an aqueous solution of $H_2SO_4$ is $0.1$,then the molality of the solution will be ......... $m$.

Some amount of dichloromethane $(CH_2Cl_2)$ is added to $671.141 \ mL$ of chloroform $(CHCl_3)$ to prepare a $2.6 \times 10^{-3} \ M$ solution of $CH_2Cl_2$ $(DCM)$. The concentration of $DCM$ is $......... \ ppm$ (by mass). Given: Atomic mass: $C = 12, H = 1, Cl = 35.5$; density of $CHCl_3 = 1.49 \ g \ cm^{-3}$.

Which of the following methods of expressing concentration does not change with temperature?

If the molality of an aqueous solution is $m$ and the mole fraction of the solute is $y$,which of the following relations is correct?

How are $0.50 \, mol$ $Na_{2}CO_{3}$ and $0.50 \, M$ $Na_{2}CO_{3}$ different?