🤓 Based on our data, we think this question is relevant for Professor Evans' class at QC CUNY .
Solution: An aqueous solution is 10.% glucose by mass (d = 1.039 g/mL at 20°C). Calculate its freezing point, boiling point at 1 atm, and osmotic pressure.
Problem
An aqueous solution is 10.% glucose by mass (d = 1.039 g/mL at 20°C). Calculate its freezing point, boiling point at 1 atm, and osmotic pressure.
Solution
The mass percent of a solution is given by:
In a 10% by mass glucose (C6H12O6) solution, this means there are 10 g of glucose for every 100 g solution. From this, we can calculate the mass of water (the solvent):
We need to find the molality of the solution since we'll use it to calculate the freezing point depression and boiling point elevation. Recall that molality is:
The molar mass of glucose is 6(12.01 g/mol C) + 12(1.01 g/mol H) + 6(16.00 g/mol O) = 180.18 g/mol. Calculating the molality of the glucose solution:
View Complete Written SolutionAdditional Practice Problems
Freezing Point Depression
Freezing Point Depression
Q. What is the minimum mass of glycerol (C3H8O3) that must be dissolved in 11.0 mg of water to prevent the solution from freezing at −15°C? (Assume ideal...
Freezing Point Depression
Q. The freezing point of benzene is 5.5°C. What is the freezing point of a solution of 5.00 g of naphthalene (C10H8) in 444 g of benzene (Kf of benzene =...
Freezing Point Depression