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Urea is a common fertilizer with the formula CO(NH2)2 that is sometimes used as a chemical deicer for icy road surfaces in the winter months. Adding a solute to a solvent causes the freezing point to be lowered and allows the solvent to remain liquid at lower temperatures.
The value of Kf for water is 1.86°C/m, and its normal freezing point is 0.00°C, Urea is a nonvolatile nonelectrolyte solute.
What molality of urea is required to lower the freezing point of ice water by 2.63°C?
Using your answer from Part 1, calculate the mass of urea that must be added to 427 mL of water (density 1.00 g/mL) to lower the freezing point by 2.63°C.
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Our tutors have indicated that to solve this problem you will need to apply the Freezing Point Depression concept. If you need more Freezing Point Depression practice, you can also practice Freezing Point Depression practice problems.
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Based on our data, we think this problem is relevant for Professor Ekanayake's class at KENT.