Calculate the Kb given that the boiling point of the 6.2 m solution is 50.3℃ and the normal boiling point of the solvent is 46.2℃. The solute is KCl.

13.5 g of nonvolatile solute (79.1 g/mol) is added to 229.9 g of solvent (35.70 g/mol) at 23ºC to form a solution. What is the vapor pressure of the solution in units of atm? The equilibrium vapor pressure of the pure solvent at this temperature is 0.800 atm

A solution containing 0.10 mol of naphthalene (nonvolatile) and 0.90 mol of benzene is cooled until some solid benzene freezes out. The solution is then decanted off from the solid and the decanted solution is warmed to 80°C, at which temperature the vapor pressure above the solution is found to be 670 torr. The normal freezing and boiling points of pure benzene are 5.5 °C and 80°C, respectively and the molar enthalpy of fusion of benzene ∆fus?=10.67 kJ/mol Assume the solution is ideal. a) Calculate the temperature to which the solution was cooled originally. b) Calculate the number of moles of benzene that froze out.

when 7.94 g of xylene was added to 132.5 g of cyclohexane, the freezing point of the solution was -4.9 C. what is the molar mass of xylene?

We mixed some ethylene glycol with 346 g water to reduce the equilibrium vapor pressure of water from 23.76 Hg to 22.5 Hg at 25°C. The molar masses of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol, respectively. Assume ideal behavior for the solution. What is the boiling point of this solution? (Hint: find the molality first, and for water, kb = .510 m/°C; boiling point of water: 100.0°C.)

Calculate the molality of a sulfuric acid solution containing 0.10 mole of sulfuric acid in 198 g of water. The molar mass of sulfuric acid is 98.09 g. Molality = Moles solute/ Kg of Solvent O 0.51 O 1.51 O 1.0 123.0

A 30.0 mL sample of this aqueous HX solution freezes at – 0.186 oC. What is the molar mass of HX?