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Q1. Calculate the freezing point of a 1.7 m aqueous ethylene glycol solution.

Recall

Molality: ((moles of solute (mol))/(mass of solvent (kg))→m)

Freezing Point Depression: (ΔT_f=m×K_f )

• Where K_f is freezing point depression constant and is a property of the solvent. Assume that for water, the constant is −1.86 (°C)/m
• Actually freezing point is 0 C° − ΔT_f

Note: When a liquid is cooled below the temperature at which it freezes (T_f) it will undergo a transition from the liquid state to the solid state. When a nonvolatile solute is added to a liquid solvent, the freezing point of the solvent is lowered by an amount that is proportional to the molal concentration of the solute. This lowering (depression) of the freezing point of the solvent can be represented using the following equation

Q2. Calculate the freezing point of a 2.6 m aqueous sucrose solution.

The units of the answer are correct. The magnitude seems about right. The expected range for freezing points of an aqueous solution is anywhere from −10 °C to just below 0 °C. Any answers out of this range would be suspect.