   Chapter 12.4, Problem 12.11E General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343

Solutions

Chapter
Section General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343
Textbook Problem

An aqueous solution is 2.00 M urea. The density of the solution is 1.029 g/mL. What is the molal concentration of urea in the solution?

Interpretation Introduction

Interpretation:

Molal concentration of aqueous solution of urea has to be calculated.

Concept Introduction:

Molality is one of the many parameters that is used to express concentration of a solution.  It is expressed as,

Molality = number of moles of solutemass of solvent in kg

Molarity is one of the many parameters that is used to express concentration of a solution.  It is expressed as,

Molarity = number of moles of solutevolume of solution in L

Explanation

To determine the molal concentration of urea, we need to know the volume of the solution.  Volume of the solution is equivalent to mass of the solution divided by density of the solution since density = massvolume .  Mass of the solution is equivalent to sum of the mass of solute urea and mass of the solvent water.  Hence we first need to calculate the mass of the solution.

Given:

The molar concentration of aqueous solution of urea is 2.00 M .

no. of moles of urea = mass of ureamolar mass of urea

mass of urea in 2.00 M aqueous solution = no. of moles of urea × molar mass of urea                                                                = 2.00 mol × 60.06 g/mol= 120.12 g

Considering one liter of solution,

Mass of the solution = density of solution × volume of solution                                  = 1

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