$A$ $1$ molal solution is defined as $1$ mole of solute dissolved in:

If $5.85 \ g$ of $NaCl$ (molecular weight $58.5$) is dissolved in water and the solution is made up to $0.5 \ L$,the molarity of the solution will be (in $M$)

When $6 \ g$ of urea is dissolved in $180 \ g$ of $H_2O$,the mole fraction of urea is:

$8 \ g$ of $NaOH$ is dissolved in $18 \ g$ of $H_2O$. Mole fraction of $NaOH$ in solution and molality (in $mol \ kg^{-1}$) of the solution respectively are

The mass of urea required to make $2.5 \ kg$ of $0.25 \ molal$ aqueous solution is (in $g$)

If the density of a $1 \, m$ aqueous solution of $NaCl$ is $1.21 \, g/mL$,then the molarity of the solution is .......... (in $, M$)