   # A 4.7 × 10 −2 mg sample of a protein is dissolved in water to make 0.25 mL of solution. The osmotic pressure of the solution is 0.56 torr at 25°C. What is the molar mass of the protein? ### 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 116CWP
Textbook Problem
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## A 4.7 × 10−2 mg sample of a protein is dissolved in water to make 0.25 mL of solution. The osmotic pressure of the solution is 0.56 torr at 25°C. What is the molar mass of the protein?

Interpretation Introduction

Interpretation: The molar mass of Protein 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=MassofsubstanceAmountofsubstance

### Explanation of Solution

Record the given info

Mass of Protein sample = 4.7×10-2mg

Volume of solution = 0.25mL

Osmotic pressure = 0.56torr at25°C

To calculate the molarity of solution

Temperature = 298K

Gas Law constant = 0.08206Latm

From the osmotic pressure equation,

π=MRTπ=0.56torr×1atm760torr=M×0.08206LatmKmol×298KM=3.0×10-5M

Molarity of solution = 3.0×10-5M

To calculate the moles of Protein

Volume of solution = 0.25mL

Molarity of solution = 3

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