Erythrocytes are red blood cells containing hemoglobin. In a saline solution they shrivel when the salt concentration is high and swell when the salt concentration is low. In a 25°C aqueous solution of NaCl, whose freezing point is −0.406°C, erythrocytes neither swell nor shrink. If we want to calculate the osmotic pressure of the solution inside the erythrocytes under these conditions, what do we need to assume? Why? Estimate how good (or poor) of an assumption this is. Make this assumption and calculate the osmotic pressure of the solution inside the erythrocytes.

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Interpretation Introduction Interpretation: The osmotic pressure of the solution inside the erythrocytes has to be explained. 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 = osmotic pressure(in atm) M=molarity of solution(in M) R= Gas Law constant L atm T=Temperature(in K) Explanation Record the given info Freezing point =-0 .406°C Temperature =25°C To calculate the molarity of solution m= ΔT K f = 0

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Chemistry: An Atoms First Approach

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Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

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Chemistry: An Atoms First Approach

2nd Edition

Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

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Interpretation Introduction

Interpretation: The osmotic pressure of the solution inside the erythrocytes has to be explained.

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= osmotic pressure(in atm)

M=molarity of solution(in M)

R= Gas Law constant L atm

T=Temperature(in K)

Explanation of Solution

Record the given info

Freezing point =-0.406°CTemperature =25°C

To calculate the molarity of solution

m=ΔTKf=0

Chemistry: An Atoms First Approach

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Chemistry: An Atoms First Approach

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