Problem: A solution is prepared by dissolving 456 g of sucrose (C12H22O11, molar mass 342 g/mol) in 764 g of water (18.02 g/mol; density 1.00 g/mL) calculate: b) The boiling point of the solution. (Kb = 0.52 °C/m).

FREE Expert Solution

We’re being asked to calculate the boiling point of the solution. 


Recall that the boiling point of a solution is higher than that of the pure solvent and the change in boiling point (ΔT­b) is given by:


ΔTb=Tb, solution-Tb, pure solvent


The change in boiling point is also related to the molality of the solution:


ΔTb=imKb


where: 

i = van’t Hoff factor

m = molality of the solution (in m or mol/kg)

Kb = boiling point elevation constant (in ˚C/m) of the solvent


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Problem Details

A solution is prepared by dissolving 456 g of sucrose (C12H22O11, molar mass 342 g/mol) in 764 g of water (18.02 g/mol; density 1.00 g/mL) calculate: 

b) The boiling point of the solution. (Kb = 0.52 °C/m).

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the The Colligative Properties concept. You can view video lessons to learn The Colligative Properties. Or if you need more The Colligative Properties practice, you can also practice The Colligative Properties practice problems.