Final answer:
Colligative properties rely on the number of solute particles in a solution affecting its vapor pressure, boiling point, freezing point, and osmotic pressure, irrespective of the chemical nature of the solute.
Step-by-step explanation:
Colligative properties of a solution depend on the number of dissolved particles present in the solution, which directly affects the solution's characteristics regardless of the particles' chemical identity. Colligative properties include important factors such as vapor pressure depression, boiling point elevation, freezing point depression, and osmotic pressure. They are called 'colligative' because these properties are collectively determined by the number of particles in a solution rather than their nature. Notably, the presence of a nonvolatile solute lowers the solvent's vapor pressure according to Raoult's law and changes the boiling and freezing points of the solution proportionally to the solute's molality. These changes are especially crucial when dealing with electrolytes, as their dissociation or ionization increases the number of solute particles and intensifies the colligative effects.