   Chapter 13, Problem 39PS

Chapter
Section
Textbook Problem

An aqueous solution containing 1.00 g of bovine insulin (a protein, not ionized) per liter has an osmotic pressure of 3.1 mm Hg at 25 °C. Calculate the molar mass of bovine insulin.

Interpretation Introduction

Interpretation: The molar mass of bovine insulin has to be determined if the solution has an osmotic pressure of 3.1mmHg at 25°C.

Concept introduction:

Colligative properties: Properties of solutions which having influence on the concentration of the solute in it. Colligative properties are,

• Decrease in the vapor pressure
• Increase in the boiling point
• Decline in the freezing point
• Osmotic pressure

Osmotic pressure is calculated by using the equation,

π=cRT

where,

c is the molar concentration

The number of moles of any substance can be determined using the equation

Numberofmole=GivenmassofthesubstanceMolarmass

Explanation

Given,

R=0.082057L.atm K1mol1T=250C=(25+273.2)K=298.2K

Mass of the bovine insulin is 1.00g

Osmotic pressure,π=3.1mmHg

The osmotic pressure of the solution is,

π=cRT

Hence,

The concentration is calculated by,

Concentration,c=πRT=(3.1mmHg)(1atm760mmHg)(0.082057L.atmK1mol1)(298.2K)=1.6669×104mol/L

The amount of bovine insulin dissolved in one liter of water is,

1

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