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

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Quizplus · Accepted Answer

The boiling point elevation and freezing point depression are colligative properties that depend on the concentration of solute particles in a solution, not on the nature of the solute particles. The boiling point elevation (ΔT_b) is given by the equation ΔT_b = K_bm, where K_b is the boiling point elevation constant for the solvent and m is the molality of the solution. The freezing point depression (ΔT_f) is given by the equation ΔT_f = K_fm, where K_f is the freezing point depression constant for the solvent and m is the molality of the solution.In this problem, we are given that the boiling point of the aqueous solution is 102.5^$\circ$C. We can use the boiling point elevation equation to calculate the molality of the solution:ΔT_b = K_bm102.5^$\circ$C - 100.0^$\circ$C = 0.52^$\circ$C/m * m2.5^$\circ$C = 0.52^$\circ$C/m * mm = 4.81 mol/kgNow that we know the molality of the solution, we can use the freezing point depression equation to calculate the freezing point of the solution:ΔT_f = K_fmΔT_f = 1.86^$\circ$C/m * 4.81 mol/kgΔT_f = 8.94^$\circ$CThe freezing point of the solution is therefore 100.0^$\circ$C - 8.94^$\circ$C = -8.94^$\circ$C.

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