What is the mole fraction of water in a spirit sample containing $92 \%$ ethyl alcohol by weight?

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 $40 \ g \ mol^{-1}$)

$V_1 \ \text{c.c.}$ of a solution having molarity $M_1$ is diluted to have molarity $M_2$. The volume of water required to be added will be $:-$

Which concentrations can be calculated if the mole fraction and density of an aqueous solution of $HCl$ are known? $1.$ Molality $2.$ Molarity $3.$ Percentage by mass

State whether the following sentences are true $(T)$ or false $(F)$.
$(a)$ Concentration of pure water is $1.0 \ mol \ L^{-1}$.
$(b)$ Concentration of pure water is $55.5 \ mol \ L^{-1}$.

If $100 \ g$ of a $0.2 \ m$ aqueous solution is diluted by adding $200 \ g$ of water,what will be the molality of the resulting solution?