Chapter 13, Problem 35PS

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

# You dissolve 15.0 g of sucrose, C12H22O11, in a cup of water (225 g). What is the freezing point of the solution?

Interpretation Introduction

Interpretation: The freezing point of solution has to be identified.

Concept introduction:

Freezing point elevation: The freezing point of the solution varies with the solute concentration.

Depression in Freezing point = ΔTfp= Kfp. msolute,where,Kfpismolal boiling point elevation constant,msoluteis molality of solute

Explanation

Given data:

Massâ€‰ofâ€‰â€‰sucroseâ€‰(solute)Â =â€‰15â€‰gMassÂ ofÂ WaterÂ =Â 0.225Â kgÂ Freezingâ€‰pointâ€‰ofâ€‰solutionâ€‰â€‰=Â ?

Numberâ€‰ofâ€‰moleâ€‰â€‰=â€‰â€‰â€‹Massâ€‰â€‰ofâ€‰â€‰â€‰theâ€‰â€‰substanceâ€‰â€‰inâ€‰â€‰gramMolarâ€‰â€‰massâ€‰

MoleÂ ofÂ soluteÂ =Â 15g342.3â€‰g/molâ€‰=â€‰0.044mol

FreezingÂ pointÂ ofÂ waterÂ =Â 0oCKfpofâ€‰Water=â€‰-1.86oC/m

CalculateÂ theÂ molalityÂ ofÂ soluteÂ Â inÂ solution(m):_molalityÂ =Â MolesÂ ofÂ soluteÂ (mol)AmountÂ ofÂ solvent(inÂ kg)Â =Â (0.044Â mol)0

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