$25 \ g$ of a solute of molar mass $250 \ g \ mol^{-1}$ is dissolved in $100 \ mL$ of water to obtain a solution whose density is $1.25 \ g \ mL^{-1}$. The molarity and molality of the solution are respectively

The number of moles of $KCl$ in $1000 \ mL$ of $3 \ M$ solution is

The molality of $90\%$ ${H_2SO_4}$ solution is [density $= 1.8 \ g/mL$].

The approximate molarity of a solution in $mol \ L^{-1}$ that contains $13.50 \ g$ of $NaCl$ dissolved in $452 \ mL$ of water is

Calculate the mass percentage of benzene $(C_{6}H_{6})$ and carbon tetrachloride $(CCl_{4})$ if $22 \ g$ of benzene is dissolved in $122 \ g$ of carbon tetrachloride.

The mole fraction of urea in an aqueous urea solution containing $900 \text{ g}$ of water is $0.05$. If the density of the solution is $1.2 \text{ g cm}^{-3}$,the molarity of the urea solution is . . . . . (Given data: Molar masses of urea and water are $60 \text{ g mol}^{-1}$ and $18 \text{ g mol}^{-1}$,respectively)