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Colligative Properties of Solutions

Colligative Properties of Solutions. Jacobus Henricus van 't Hoff (1852-1911). (Colligative Properties have been excluded from the AP Chemistry curriculum). Colligative Properties.

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Colligative Properties of Solutions

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  1. Colligative Properties of Solutions Jacobus Henricus van 't Hoff (1852-1911) (Colligative Properties have been excluded from the AP Chemistry curriculum)

  2. Colligative Properties Colligative properties are those that depend on the concentration of particles in a solution, not upon the identity of those particles. • Boiling Point Elevation • Freezing Point Depression • Osmotic Pressure

  3. Freezing Point Depression Each mole of solute particles lowers the freezing point of 1 kilogram of water by 1.86 degrees Celsius. Kf = 1.86 C  kilogram/mol m = molality of the solution i= van’t Hofffactor

  4. Boiling Point Elevation Each mole of solute particles raises the boiling point of 1 kilogram of water by 0.51 degrees Celsius. Kb= 0.51 C  kilogram/mol m= molality of the solution i=van’t Hofffactor

  5. Freezing Point Depression and Boiling Point Elevation Constants, C/m

  6. The van’t Hoff Factor, i Electrolytes may have two, three or more times the effect on boiling point, freezing point, and osmotic pressure, depending on its dissociation.

  7. Dissociation Equations and the Determination of i i = 2 NaCl(s)  Na+(aq) + Cl-(aq) i = 2 AgNO3(s)  Ag+(aq) + NO3-(aq) i = 3 MgCl2(s)  Mg2+(aq) + 2 Cl-(aq) i = 3 Na2SO4(s)  2 Na+(aq) + SO42-(aq) AlCl3(s)  Al3+(aq) + 3 Cl-(aq) i = 4

  8. Ideal vs. Real van’t Hoff Factor The ideal van’t Hoff Factor is only achieved in VERY DILUTE solution.

  9. Osmotic Pressure The minimum pressure that stops the osmosis is equal to the osmotic pressure of the solution

  10. Osmotic Pressure Calculations  = Osmotic pressure i = van’t Hoff Factor M = Molarity of the solution R = Gas Constant = 0.08206 Latm/molK

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