Determine the freezing point of a solution that contains 0.31 mol of sucrose in 175 g of water. K_f = 1.86°C/m A)3.3°C B)1.1°C C)0.0°C D)−1.1°C E)−3.3°C

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The freezing point depression can be calculated using the formula ΔTf = i * Kf * m, where i is the van't Hoff factor (1 for sucrose, a non-electrolyte), Kf is the freezing point depression constant (1.86°C/m), and m is the molality of the solution. Molality (m) = moles of solute / kg of solvent = 0.31 mol / 0.175 kg = 1.7714 m. ΔTf = 1 * 1.86°C/m * 1.7714 m = 3.3°C. The freezing point of pure water is 0°C, so the freezing point of the solution is 0°C - 3.3°C = -3.3°C.

Determine the Freezing Point of a Solution That Contains 0