The vapor pressure of water at 20.0 ºC is 17.5 torr. At that temperature, what would be the vapor pressure of a solution made by dissolving 43.0 g of NaCl in 0.300 kg of water? (Assume complete dissociation of the solute and an ideal solution.)

Calculate the vapor pressure above a solution prepared by dissolving 2.00 g of aspirin (C9H8O4) in 50.0 g of methanol (CH3OH) at 21.2 °C. Pure methanol has a vapor pressure of 101 torr at 21.2 °C.

If 100 mL of a 0.15 M Mg(NO3)2(aq) solution has a density of 1.09 g/mL, which of the following statements is false? The mass of the water in this solution is 109 g The mass of Mg(NO3)2 in this solution can be determined from this information. If the solution density was not given, it is usually reasonable to assume 1.00 g/mL It is possible to determine the mole fraction of water in this solution.

How many grams of pentane, CH3(CH2)3CH3, must be mixed with 64.18 g of hexane, CH3(CH2)4CH3, at 25.00 °C to produce a solution with a vapor pressure above the solution of 273.5 torr? The vapor pressures of pure pentane and hexane at 25.00 °C are 511.0 torr and 150.0 torr, respectively. These compounds form nearly ideal solutions when mixed together.

Biphenyl, C,,H10, is a nonvolatile, nonionizing solute that is soluble in benzene, C,H,. At 25 °C, the vapor pressure of pure benzene is 100.84 Torr. What is the vapor pressure of a solution made from dissolving 14.4 g of biphenyl in 29.2 g of benzene? Psolution = Torr

At a particular temperature, the solubility of CO₂ in water is 0.13 M when the partial pressure is 1.5 atm. What partial pressure (in atm) of CO₂ would give a solubility of 0.078 M?

A solution is composed of 1.40 mol cyclohexane (P∘cy=97.6 torrPcy∘=97.6 torr) and 2.50 molmol acetone (P∘ac=229.5 torr). What is the total vapor pressure Ptotal above this solution?

Benzene is a common industrial solvent (molar mass: 78.11 g/mol). Its normal freezing point is 5.50 °C and its freezing point depression constant is Kf = -5.12 °C/m. Determine the freezing point (in °C with 3 significant figures) for the solution prepared by mixing 3.82 g of anthracene (C14H10; molar mass = 178.23 g/mol) and 51.4 g of benzene.

A nonvolatile solute is dissolved in benzene and the resulting solution has a vapor pressure of 18.7 torr. What is the mole fraction of the solute? (P° of benzene is 26.5 torr).

Calculate the molar mass (MM) of an unknown solid when 1.0 g was dissolved in 225 mL (225 g) water. The freezing point of the solution was determined to be 6.18oC.