A solution is prepared by dissolving 2.5g of a non-volatile solute in 100g of water. The vapor pressure of the solution is found to be 22.87 Torr at $25^\circ C$. If the vapor pressure of pure water is 23.76 Torr at the same temperature, what is the molar mass of the solute (in g/mol)?

What is the molality of a solution where the mole fraction of the solute is 0.02 and the solvent is water?

A solution is prepared by dissolving 20g of a non-volatile solute in 180g of water. If the vapor pressure of pure water at this temperature is 23.76 mmHg and the solution exhibits a vapor pressure of 23.52 mmHg, what is the molar mass of the solute? (Molar mass of water = 18 g/mol)

A mixture of two volatile liquids A and B follows Raoult's law. At a certain temperature, the partial pressures of A and B above the solution are 200 mmHg and 300 mmHg respectively. If the mole fraction of A in the liquid phase is 0.4, what is the vapor pressure of pure A at this temperature?

In a solution containing 0.1 moles of a solute and 5 moles of solvent, what is the mole fraction of the solvent?

100g of a liquid A (molar mass 140 g/mol) and 100g of liquid B (molar mass 70 g/mol) form an ideal solution. What is the mole fraction of B in the vapor phase? (Assume $P^0_A = 70$ mmHg and $P^0_B = 140$ mmHg)

A solution is prepared by dissolving 10 g of sucrose ($C_{12}H_{22}O_{11}$) in 200 g of water. What is the mole fraction of sucrose?

What is the mole fraction of the solute in a 1.00 m aqueous solution of glucose?

A 0.5 molal aqueous solution of urea ($CON_2H_4$) is prepared. What is the mole fraction of urea?

Henry's law constant for CO$_2$ in water at 298K is 1.67 x 10$^8$ Pa. Calculate the mass of CO$_2$ dissolved in 500 mL of soda water when packed under 2.5 atm CO$_2$ pressure at 298K. (1 atm = 1.013 x 10$^5$ Pa, molar mass of CO$_2$ = 44 g/mol)