Final answer:
Colligative properties of solutions depend on the number of dissolved solute particles, not their chemical nature, affecting factors like vapor pressure, boiling and freezing points, and osmotic pressure.
Step-by-step explanation:
The physical properties of solutions that depend on the number of solute particles, and not on their specific type, are known as colligative properties. These properties include factors like vapor pressure depression, boiling point elevation, freezing point depression, and osmotic pressure. These changes occur due to the presence of solute particles rather than their chemical nature. For instance, when solute is added to a solvent, the resulting solution will have a lower vapor pressure compared to the pure solvent because the solute particles hinder the escape of solvent particles into the gaseous phase, following Raoult's law. Similarly, the solution will exhibit a higher boiling point (boiling point elevation) and a lower freezing point (freezing point depression) than the pure solvent. The amount of boiling point elevation and freezing point depression is directly proportional to the molality of the solute. Osmotic pressure is another colligative property, which is the pressure required to prevent solvent movement through a semipermeable membrane into the solution.