Colligative properties of a dilute solution depend on:

By definition, colligative properties (relative lowering of vapour pressure, boiling-point elevation, freezing-point depression, osmotic pressure) depend on how many solute particles are dissolved, not what those particles are. One mole of glucose and one mole of urea cause the same boiling-point elevation in 1 kg of water. With electrolytes like NaCl that dissociate into 2 ions, the effective particle count is multiplied by the van't Hoff factor $i$ (close to 2 for NaCl in dilute solution).