**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.

Given : Osmotic pressure = 1.47 mm Hg Mass of dextran = 0.589 g Volume of solution = 106 mL = 0.106…

Answered: An aqueous solution contains 0.589 g of…

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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Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

**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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