Which aqueous solution has the lowest freezing point: 0.5 m glucose, 0.5 m NaCl, or 0.5 m CaCl2

step 1 So one might look at these solutions and knowing that the freezing point depression depends on t

Which aqueous solution has the lowest freezing point: 0.5 m...

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Key Concepts

Colligative Properties

These are properties of solutions that depend solely on the number of solute particles in a given amount of solvent rather than on the properties of the individual solute species. Examples include freezing point depression, boiling point elevation, and vapor pressure lowering, all of which reflect changes caused by adding a solute to a solvent.

Freezing Point Depression

This phenomenon describes the lowering of a solvent's freezing point when a solute is dissolved in it. The magnitude of the freezing point depression is directly proportional to the concentration of solute particles present in the solution. This is typically quantified by the equation ?Tƒ = i · Kƒ · m, where ?Tƒ is the freezing point change, Kƒ is the cryoscopic constant of the solvent, m is the molality of the solution, and i is the van't Hoff factor.

Van't Hoff Factor

The van't Hoff factor (i) represents the number of particles into which a solute dissociates in solution. It is crucial in calculating colligative properties such as freezing point depression because it adjusts the effective concentration of particles that influence these properties. For instance, electrolytes that dissociate into multiple ions have a higher van't Hoff factor than non-electrolytes.

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