But I am willing to make an attempt at introduction. #"Colligative properties"#, by definition, depend on the NUMBER of solute particles in solution, AND NOT on the identity of the solute particles themselves. And thus ionic solutes, which speciate in solution to give equivalent quantities of anions and cations, thus exhibit greater colligative properties than non-ionic solutes, which are presumed to give only the ONE equiv of solute in solution.
And, as chemists, traditionally we are concerned with 3 colligative properties:
#1.# #"Boiling point elevation"#, in which the boiling point of a solution is raised proportional to the amount of solute in the solution.
#2.# #"Freezing point depression"#, in which the melting point of a solution is DECREASED proportional to the amount of solute in the solution.
#3.# #"Osmotic pressure"#, in which the vapour pressure of a solution is DECREASED proportional to the amount of solute in the solution.
Sometimes these colligative properties allow the determination of the molecular weight of a chemical species in SOLUTION; and this is something that neither X-ray crystallography nor mass spectroscopy can do.
Anyway, I urge you to read the relevant chapter in your text. Of course, if there is a specific problem, post away, and someone will help you.