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The identity of the solute(s) has no First Order importance in the consideration of colligative properties, and the degree to which their manifestation can be observed and measured is effected only by the number of solute particles in the solution. However, the identity of solute may effect the number of effective molecules in solution; for example, Hydrogen Bonding . These types of considerations are approximate however, since in general, colligative models make assumptions of ideality wherein Molecular Interactions are neglected.

The four colligative properties are:
  • s.

  • (i) of the solute multiplied by its Molality (m) multiplied by the freezing point depression constant of the solvent (Kf): ΔT=iKfm. Alternatively, it can be calculated as the total molality of all solutes in solution times the depression constant: ΔT=Kf∑m.

  • (i) of the solute multiplied by its Molality multiplied by the boiling point elevation constant of the solvent (Kb): ΔT=iKbm. ΔT can also be calculated using the sum of all molalities: ΔT=Kf∑m.

  • , T is the Absolute Temperature in Kelvin s, and V is the volume: π=(nRTi)/V



''In (1), the two columns of pure solvent (blue) under the same pressure. When solute (green) is added to the right column (2), osmotic pressure is exerted and solvent flows through the permeable membrane (red) to the right side.''