What are the mole fraction of water and the total number of moles in a solution formed by dissolving $1$ mole of urea in $1000 \ g$ of pure water,respectively?

If the mole fraction of ethanol in a solution made by mixing $x \ g$ of water and $69 \ g$ of ethanol is $0.6$,then $x = \dots \dots \dots \dots$

The formula weight of $H_2SO_4$ is $98$. The weight of the acid in $400 \ mL$ of $0.1 \ M$ solution is ........... $g$.

Calculate the molality of $1 \ L$ solution of $93 \ \%$ $H_2SO_4$ (weight/volume). The density of the solution is $1.84 \ g/mL$.

Mole fraction $(X)$ of any solution is equal to

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