Which of the following is true about colligative properties?

Colligative properties are characteristics of solutions that depend primarily on the number of solute particles in a given amount of solvent, rather than the identity or type of solute particles. Examples of colligative properties include boiling point elevation, freezing point depression, vapor pressure lowering, and osmotic pressure.

These properties arise because the presence of solute particles disrupts the interactions between solvent molecules. As more solute particles are added, the extent of these disruptions increases, leading to measurable changes in the physical properties of the solvent.

The notion that the identity of the solute matters is not relevant to colligative properties; rather, it is the concentration (or number) of particles that influences the observed effects. This is why the correct understanding highlights the dependence on the number of solute particles present in the solution.