   # A solid mixture contains MgCl 2 and NaCl. When 0.5000 g of this solid is dissolved in enough water to form 1.000 L of solution, the osmotic pressure at 25.0°C is observed to be 0.3950 atm. What is the mass percent of MgCl 2 in the solid? (Assume ideal behavior for the solution.) ### Chemistry: An Atoms First Approach

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

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 10, Problem 126CP
Textbook Problem
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## A solid mixture contains MgCl2 and NaCl. When 0.5000 g of this solid is dissolved in enough water to form 1.000 L of solution, the osmotic pressure at 25.0°C is observed to be 0.3950 atm. What is the mass percent of MgCl2 in the solid? (Assume ideal behavior for the solution.)

Interpretation Introduction

Interpretation: The mass percent of Magnesium chloride in solid.

Concept Introduction:

The mass percentage of a compound is ratio of calculated mass of compound to the total mass whole multiplied by 100. The mass percentage of compound can be given by the equation.

Masspercentage(%)=Calculatedmass(ing)Totalmass(ing)×100

### Explanation of Solution

Record the given info

Mass of solid      = 0.5000g

Osmotic pressure = 0.3950atmat25°C

Volume of solution = 1.000L

To calculate the total ion concentration

From osmotic pressure equation,

iM=πRT=0.3950atm0.08206LatmKmol×298.2K=0.01614mol/L

The total ion concentration is 0.01614mol/L

0.01614molL-1=MMg2++MNa++MCl-;MCl-=2MMg2++MNa+(chargebalance)Combining, we get0.01614=3MMg++2MNa+

To calculate the mass of Magnesium chloride

Let x = Mass of Magnesium chloride

y = Mass of Sodium chloride

Then, x+y=0.5000g

MMg2+=x95

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