What is the freezing point of an aqueous solution of a nonvolatile solute that has a boiling point of 102.5°C? For water K_f = 1.86°C/m and K_b = 0.52°C/m. A)8.94°C B)0.99°C C)-0.99°C D)-8.94°C E)-366°C

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The correct answer is D because the boiling point elevation and freezing point depression are colligative properties that depend on the concentration of the solute particles in the solution, not on the nature of the solute. The freezing point depression is given by the equation ΔT_f = K_fm, where ΔT_f is the change in freezing point, K_f is the freezing point depression constant for the solvent, and m is the molality of the solution. The boiling point elevation is given by the equation ΔT_b = K_bm, where ΔT_b is the change in boiling point, K_b is the boiling point elevation constant for the solvent, and m is the molality of the solution. In this problem, we are given the boiling point elevation (ΔT_b = 102.5°C - 100°C = 2.5°C) and the freezing point depression constant for water (K_f = 1.86°C/m). We can use the relationship between ΔT_b and ΔT_f to find the freezing point depression:ΔT_f = ΔT_b * (K_f/K_b) = 2.5°C * (1.86°C/m / 0.52°C/m) = 8.94°CTherefore, the freezing point of the solution is 100°C - 8.94°C = -8.94°C.

What Is the Freezing Point of an Aqueous Solution of a Nonvolatile