Which statement is true regarding the calculation of colligative properties?

Colligative properties are properties of solutions that depend on the number of solute particles in a given amount of solvent, rather than the identity of the solute itself. This means that both ionic and molecular solutes can affect properties such as vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.

With ionic solutes, they dissociate into multiple particles in solution. For example, sodium chloride (NaCl) dissociates into two ions: Na⁺ and Cl⁻. Thus, an ionic solute influences colligative properties based on the total number of ions present in the solution. Molecular solutes, which do not dissociate into ions, influence these properties based solely on the number of molecules added to the solution.

The fundamental principle of colligative properties ensures that they are applicable and significant for both types of solutes, making this statement accurate. The calculations are indeed reliant on the concentration of solute particles, which is typically measured in terms of molality or molarity, not grams. Thus, the correct assertion reflects the broad applicability of colligative properties to various types of solutes.