   Chapter 10, Problem 90E Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
ISBN: 9781305079243

Solutions

Chapter
Section Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
ISBN: 9781305079243
Textbook Problem

A 0.500-g sample of a compound is dissolved in enough water to form 100.0 mL of solution. This solution has an osmotic pressure of 2.50 atm at 25°C. If each molecule of the solute dissociates into two particles (in this solvent), what is the molar mass of this solute?

Interpretation Introduction

Interpretation: The molar mass of a solute has to be calculated.

Concept Introduction:

Molar mass of a compound can be given by mass of a substance to the amount of the substance. It can be given by expression

Molarmass=MassofasubstanceAmountofsubstance

Explanation

Record the given data

Mass of sample = 0.500g

Volume of solution = 100.0mL

Osmotic pressure = 2.50atm

Temperature = 25°C

To calculate the molarity of solution

Number of moles of solute = 2

Gas law constant = 0.08206Latm

Temperature = 298K

The molarity of solution can be calculated from the osmotic pressure equation,

Π=iMRTM=ΠiRT

Molarity = 2.50atm0.08206LatmKmol×298K

= 5.11×10-2molL-1

Molarity of solute = 5

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