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Assuming 100% dissociation, calculate the freezing point and boiling point of 1.85 m Na2SO4(aq). Constants may be found here. Constants for freezing-point depression and boiling-point elevation calculations at 1 atm: Solvent Formula Kf value* (°C/m) Normal freezing point (°C) Kb value (°C/m) Normal boiling point (°C) water H2O 1.86 0.00 0.512 100.00 benzene C6H6 5.12 5.49 2.53 80.1 cyclohexane C6H12 20.8 6.59 2.92 80.7 ethanol C2H6O 1.99 -117.3 1.22 78.4 carbon tetrachloride CCl4 29.8 -22.9 5.03 76.8 camphor C10H16O 37.8 176 *When using positive Kf values, assume that ?Tf is the absolute value of the change in temperature. If you would prefer to define ?Tf as "final minus initial" temperature, then ?Tf will be negative and so you must use negative Kf values. Either way, the freezing point of the solution should be lower than that of the pure solvent. Assuming 100% dissociation, Find the freezing and boiling points of 1.85 m Na2SO4(aq).

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