   # How would you prepare 1.0 L of an aqueous solution of sodium chloride having an osmotic pressure of 15 atm at 22°C? Assume sodium chloride exists as Na + and Cl − ions in 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 78E
Textbook Problem
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## How would you prepare 1.0 L of an aqueous solution of sodium chloride having an osmotic pressure of 15 atm at 22°C? Assume sodium chloride exists as Na+ and Cl− ions in solution.

Interpretation Introduction

Interpretation: The amount of Sodium chloride required to prepare 1.0L aqueous solution of Sodium chloride has to be calculated.

Concept Introduction:

When a semi-permeable membrane, separates a solution and pure solvent. The solvent molecules are passed through the semi permeable membrane. There is gradual increase in the volume of solution with a decrease in volume of the solvent with respect to time. The flow of solvent through a semi-permeable membrane into the solution is called as osmosis. By the time system reaches equilibrium, the changes in the liquid level stops. There is a higher hydrostatic pressure on the solution than compared to that of the pure solvent because there is variation in the liquid levels at this point. The excess pressure on the solution is called osmotic pressure.

The osmotic pressure of solution is calculated by using,

π=MRT

Here,

π=osmoticpressure(in atm)

M=molarityofsolution(inM)

R=GasLawconstant Latm

T=Temperature(inK)

### Explanation of Solution

Record the given info

Osmoticpressure=15atmTemperature=22°CVolumeofaqueoussolution=1.0L

To calculate the molarity of solution

π=MRTM=πRT=15atm0.08206LatmKmol×295K=0.62M

Molarity of solution = 0

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