   # You wish to prepare an aqueous solution of glycerol, C 3 H 5 (OH) 3 , in which the mole fraction of the solute is 0.093. What mass of glycerol must you add to 425 g of water to make this solution? What is the molality of the solution? ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 13, Problem 7PS
Textbook Problem
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## You wish to prepare an aqueous solution of glycerol, C3H5(OH)3, in which the mole fraction of the solute is 0.093. What mass of glycerol must you add to 425 g of water to make this solution? What is the molality of the solution?

Interpretation Introduction

Interpretation: The mass and molality of glycerol to be identified.

Concept introduction:

Mole fraction: Amount of that component divided by the total amount of all of the components of the mixture ( nA +  nB +  n...).

Mole fraction of A (χA)= nA nA +  nB +  n...

Molality: The amount of solute (mol) per kilogram of solvent.

Concentration (C, mol/kg) =  molality of solute = Amount of solute (mol)Mass of solvent (Kg)

Weight percent: The mass of one component divided by the total mass of the mixture, multiplied by 100%

weight % A = Mass of A Mass of A + Mass of B + Mass of C + ...×100%

### Explanation of Solution

Given:

Molefractionofglycerol(solute ,χglycerol)= 0.093Mass ofglycerol = ?Massofwater=425g

Number of moles of water can be calculated using mass of water:

no.of moles (water) = 425 g 18.0158 g/mol = 23.60 mol

Mole fraction is the amount of that component divided by the total amount of all of the components of the mixture ( nA +  nB +  n...).

Mole fraction of A (χA)= nA nA +  nB +  n...

χglycerol = nglycerol nglycerol +  nWater 0.093=nglycerol nglycerol +  23

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