A solution containing ethylene glycol and water has a vapor pressure of 7.88 torr at 10°C. Pure water has a vapor pressure of 9.21 torr at 10°C. What is the mole fraction of ethylene glycol in the solution?

A solution is prepared from 4.5701 g of magnesium chloride and 43.238 g of water. The vapor pressure of water above this solution is 0.3624 atm at 348.0 K. The vapor pressure of pure water at this temperature is 0.3804 atm. What is the value of the van’t Hoff factor (i) for magnesium chloride in this solution?

Use the result of the previous problem to calculate the mole fraction of chloroform in the vapor above a solution obtained by three successive separations and condensations of the vapors above the original solution of carbon tetrachloride and chloroform. Show how this result explains the use of distillation as a separation method.

A KCl solution is prepared by dissolving 40.0 g KCl in 250.0 g of water at 25°C. What is the vapor pressure of the solution if the vapor pressure of pure water at 25°C is 23.76 mm Hg?

A solution contains naphthalene (C10H8) dissolved in hexane (C6H14) at a concentration of 16.65% naphthalene by mass. Calculate the vapor pressure at 25°C of hexane above the solution. The vapor pressure of pure hexane at 25°C is 151 torr. What is the vapor pressure of hexane above the solution?

A solution is prepared by dissolving 40.0 g of sucrose, C12H22O11, in 250. g of water at 25°C. What is the vapor pressure of the solution if the vapor pressure of pure water at 25°C is 23.76 mm Hg?

A solution is prepared by dissolving 0.5 mol of a non-volatile solute in 1.0 mol of water. Calculate the vapor pressure of water above this solution at 338 K, given that the vapor pressure of pure water at this temperature is 0.2467 atm.

Using Raoult's Law, calculate the vapor pressure of water at 50.0°C if the pure vapor pressure of water at this temperature is 12.3 kPa and a non-volatile solute is added to form a solution with a mole fraction of water of 0.8.