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Colligative Properties

Learn about the colligative properties of solutions, specifically boiling point elevation and freezing point depression, and how they depend on solute concentration. Explore examples and calculations to determine molar mass and solute mass.

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Colligative Properties

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  1. Colligative Properties

  2. Definition • Properties that depend on the concentration of a solution no matter what the solute’s identity is

  3. Boiling Point Elevation • A solute lowers the vapor pressure, therefore a solution must be heated to a higher temperature in order to boil • ΔT = KBm • ΔT – amount of elevation • KB – constant for a given solvent • m – molality

  4. Example • A solution consisting of 18.00 g of glucose in 150.0 g of water elevates the boiling point to 100.34ºC. What is the molar mass of glucose?

  5. Freezing Point Depression • A solute lowers the vapor pressure of the solvent • At lower vapor pressure, the rate of melting is higher than the rate of crystallization • ΔT = KFm

  6. Example • What mass of ethylene glycol (C2H6O2), the main component of antifreeze, must be added to 10.0L of water to produce a solution in the car’s radiator that freezes at –23.3ºC?

  7. Example • A chemist is trying to identify a human hormone by determining it’s molar mass. A sample weighing .546 g was dissolved in 15.0 g of benzene, and the freezing point depression was determined to be .240ºC. What is it’s molar mass?

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