The molarity of a $70 \%$ (mass/mass) aqueous solution of a monobasic acid $(X)$ is $........... \ M$ (Nearest integer). Given: Density of aqueous solution of $(X)$ is $1.25 \ g \ mL^{-1}$,Molar mass of the acid is $70 \ g \ mol^{-1}$.

The mole fraction of a solute in a solution is $0.1$. At $298 \ K$,molarity of the solution is the same as its molality. The density of this solution at $298 \ K$ is $2.0 \ g \ cm^{-3}$. The ratio of the molecular weights of the solute and solvent,$\left(\frac{MW_{solute}}{MW_{solvent}}\right)$,is

What is the mole fraction of the solute in a $1 \, m$ (molal) aqueous solution?

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

$x \ g$ of water is mixed in $69 \ g$ of ethanol. The mole fraction of ethanol in the resultant solution is $0.6$. What is the value of $x$ in grams?

$3.65 \ g$ of $HCl$ is dissolved in $16.2 \ g$ of water. The mole fraction of $HCl$ in the resulting solution is ......