An aqueous fructose solution having a density of 1.049 g/cm³ is found to have an osmotic pressure of 17.0 atm at 25°C.Find the temperature at which this solution freezes.[Given: for water K_f = 1.86 °C/m; molecular mass of fructose = 180.16 g/mol] A)-1.30°C B)-1.41°C C)-1.52°C D)-1.57°C E)-1.69°C

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Quizplus · Accepted Answer

The osmotic pressure (π) can be used to find the molarity (M) of the solution using the formula π = MRT, where R is the gas constant (0.0821 L·atm/mol·K) and T is the temperature in Kelvin. Solving for M gives M = π / (RT). Substituting the given values, M = 17.0 atm / (0.0821 L·atm/mol·K × 298 K) = 0.693 mol/L. The molality (m) can be calculated using the density of the solution and the molarity. The freezing point depression ΔTf = Kf × m. Using the calculated molality and Kf = 1.86 °C/m, ΔTf is approximately 1.41°C. Therefore, the solution freezes at -1.41°C.

An Aqueous Fructose Solution Having a Density of 1