An aqueous solution contains 0.589 g of dextran in 106 mL of solution at 21°C. It has an osmotic pressure of 1.47 mmHg. What is the average molecular weight of the dextran?
An aqueous solution contains 0.589 g of dextran in 106 mL of solution at 21°C. It has an osmotic pressure of 1.47 mmHg. What is the average molecular weight of the dextran?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Problem Statement:**
An aqueous solution contains **0.589 g** of dextran in **106 mL** of solution at **21°C**. It has an osmotic pressure of **1.47 mmHg**. What is the average molecular weight of the dextran?
**Calculation Required:**
You need to calculate the molecular weight of dextran in atomic mass units (amu).
**Input Box:**
- Molecular weight = [Input Field]
- Unit: amu
**Explanation:**
To find the molecular weight, you can use the formula for osmotic pressure:
\[
\Pi = \frac{nRT}{V}
\]
Where:
- \(\Pi\) is the osmotic pressure.
- \(n\) is the number of moles of solute.
- \(R\) is the ideal gas constant.
- \(T\) is the temperature in Kelvin.
- \(V\) is the volume of the solution in liters.
Convert the given information into the proper units, and use this relationship to solve for the molecular weight.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc57e455c-e356-45e8-9424-9ece1c8d9714%2F6319e38e-d1f4-4a92-976e-873f080e6cde%2Fw8l1wqe_processed.png&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
An aqueous solution contains **0.589 g** of dextran in **106 mL** of solution at **21°C**. It has an osmotic pressure of **1.47 mmHg**. What is the average molecular weight of the dextran?
**Calculation Required:**
You need to calculate the molecular weight of dextran in atomic mass units (amu).
**Input Box:**
- Molecular weight = [Input Field]
- Unit: amu
**Explanation:**
To find the molecular weight, you can use the formula for osmotic pressure:
\[
\Pi = \frac{nRT}{V}
\]
Where:
- \(\Pi\) is the osmotic pressure.
- \(n\) is the number of moles of solute.
- \(R\) is the ideal gas constant.
- \(T\) is the temperature in Kelvin.
- \(V\) is the volume of the solution in liters.
Convert the given information into the proper units, and use this relationship to solve for the molecular weight.
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