Calculate the molality of $1 \ L$ solution of $93 \%$ $H_2SO_4$ by $w/V$ $[d = 1.84 \ g/cc]$.

$A$ sample of drinking water was found to be severely contaminated with chloroform,$CHCl_{3}$,supposed to be 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.

When $1.04 \ g$ of $BaCl_2$ is dissolved in $10^5 \ g$ of water,what will be the concentration of the solution in $ppm$?

What is the molarity of a solution of $HCl$ which contains $49\%$ by weight of solute and whose specific gravity is $1.41$ (in $M$)?

For the solution formed by dissolving a solid in water,choose the correct option regarding the following statements: Statement-$1$: $A$ $1$ molal aqueous glucose solution contains $180 \ g$ of glucose in $1000 \ g$ of water. Statement-$2$: $A$ solution containing $1$ mole of solute in $1000 \ g$ of water is called a $1$ molal solution.

The mole fraction of glucose $(C_{6}H_{12}O_{6})$ in an aqueous binary solution is $0.1$. The mass percentage of water in it,to the nearest integer,is $....$.