Dissolving $120 \ g$ of a compound (mol. wt $= 60$) in $1000 \ g$ of water gave a solution of density $1.12 \ g \ mL^{-1}$. The molarity of the solution is: (in $M$)

An $X$ molal solution of a compound in benzene has a mole fraction of solute equal to $0.2$. The value of $X$ is

Mole fraction of solute in its $2$ molal aqueous solution is

An aqueous solution of $98\% (w/w)$ $H_2SO_4$ has a density of $1.84 \ g/mL$. The molality of the solution is: (in $m$)

$A$ sample of drinking water is severely contaminated with chloroform $(CHCl_3)$. $CHCl_3$ is considered carcinogenic in nature. The level of contamination was $15 \ ppm$ (by mass).
$(i)$ Express this in percent by mass.
$(ii)$ Determine the molality of chloroform in the water sample.

$3.0\, g$ of oxalic acid $[(CO_2H)_2 \cdot 2H_2O]$ is dissolved in a solvent to prepare a $250\, mL$ solution. The density of the solution is $1.9\, g/mL$. The molality and normality of the solution,respectively,are closest to