What is the boiling point of a 4.00 m aqueous solution of a nonvolatile nonelectrolyte? (The boiling point elevation constant for water is 0.512^° C/m) A)100.^° C B)102^° C C)98.0^° C D)2.05^° C

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Quizplus · Accepted Answer

The boiling point elevation can be calculated using the formula ΔTb = Kb x m, where ΔTb is the boiling point elevation, Kb is the boiling point elevation constant, and m is the molality of the solution. Since the solute is nonvolatile and nonelectrolyte, its van't Hoff factor is 1 and we can assume that the molality is equal to the molarity of the solution, which is 4.00 mol/L. Therefore, ΔTb = 0.512 °C/m x 4.00 m = 2.05 °C. The boiling point of the solution is higher than that of pure water by ΔTb, which is 100 °C + 2.05 °C = 102.05 °C. The nearest answer choice is B.

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