Choose the aqueous solution below with the highest freezing point.These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable. A)0.200 m Ca(ClO₄)₂ B)0.200 m K₃PO₃ C)0.200 m HOCH₂CH₂OH D)0.200 m Ba(NO₃)₂ E)These all have the same freezing point.

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The freezing point depression of a solution is proportional to the molality of the solute particles (ΔTf = Kf * molality), where Kf is the freezing point depression constant for the solvent. The solute in option C, HOCH2CH2OH, is a molecular compound that dissociates into two particles in solution (since it has a hydroxyl group that ionizes slightly). The other options contain ionic compounds that dissociate into more than two particles in solution, which will result in larger freezing point depressions. Therefore, option C, which has the smallest van't Hoff factor, will have the highest freezing point.

Choose the Aqueous Solution Below with the Highest Freezing Point