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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![**Title: Osmosis Experiment: Glucose Solution in Dialysis Tubing**
**Experiment Objective:**
For an experiment on osmosis, some dialysis tubing (a semi-permeable membrane) is filled with 750 mL of a glucose (C6H12O6, non-electrolyte) solution (glucose cannot pass through the membrane). If the reaction is carried out at 36.5°C and creates an osmotic pressure of 1.75 atm, what would be the concentration of the glucose solution?
**Key Calculations and Formulas:**
1. **Formula for Osmotic Pressure (π):**
\[\pi = MRT\]
Where,
- \(\pi\) = osmotic pressure (in atm)
- \(M\) = molarity of the solution (in mol/L)
- \(R\) = gas constant (0.0821 L·atm/(K·mol))
- \(T\) = temperature (in Kelvin)
2. **Converting Celsius to Kelvin:**
\[
T(K) = T(°C) + 273
\]
For 36.5°C:
\[
36.5 + 273 = 309.5 \, K
\]
3. **Rearranging the Osmotic Pressure Formula to Solve for Molarity (M):**
\[
M = \frac{\pi}{RT}
\]
**Given Data:**
- Osmotic Pressure (π) = 1.75 atm
- Gas Constant (R) = 0.0821 L·atm/(K·mol)
- Temperature (T) = 36.5°C = 309.5 K
**Calculation Steps:**
1. Substitute the values into the rearranged formula:
\[
M = \frac{1.75 \, \text{atm}}{0.0821 \, \text{L·atm/(K·mol)} \times 309.5 \, \text{K}}
\]
2. Perform the calculation:
\[
M = \frac{1.75}{0.0821 \times 309.5}
\]
3. Simplify the calculation to find the molarity (M):
\[
M = 0.0686 \, \text{mol/L}
\]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff2609b9a-bccc-4ea0-ab3c-7cfd8cf7907c%2Fb2b7c46f-b527-4467-87f7-2d88b186e79d%2Fxzxlxtc_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Title: Osmosis Experiment: Glucose Solution in Dialysis Tubing**
**Experiment Objective:**
For an experiment on osmosis, some dialysis tubing (a semi-permeable membrane) is filled with 750 mL of a glucose (C6H12O6, non-electrolyte) solution (glucose cannot pass through the membrane). If the reaction is carried out at 36.5°C and creates an osmotic pressure of 1.75 atm, what would be the concentration of the glucose solution?
**Key Calculations and Formulas:**
1. **Formula for Osmotic Pressure (π):**
\[\pi = MRT\]
Where,
- \(\pi\) = osmotic pressure (in atm)
- \(M\) = molarity of the solution (in mol/L)
- \(R\) = gas constant (0.0821 L·atm/(K·mol))
- \(T\) = temperature (in Kelvin)
2. **Converting Celsius to Kelvin:**
\[
T(K) = T(°C) + 273
\]
For 36.5°C:
\[
36.5 + 273 = 309.5 \, K
\]
3. **Rearranging the Osmotic Pressure Formula to Solve for Molarity (M):**
\[
M = \frac{\pi}{RT}
\]
**Given Data:**
- Osmotic Pressure (π) = 1.75 atm
- Gas Constant (R) = 0.0821 L·atm/(K·mol)
- Temperature (T) = 36.5°C = 309.5 K
**Calculation Steps:**
1. Substitute the values into the rearranged formula:
\[
M = \frac{1.75 \, \text{atm}}{0.0821 \, \text{L·atm/(K·mol)} \times 309.5 \, \text{K}}
\]
2. Perform the calculation:
\[
M = \frac{1.75}{0.0821 \times 309.5}
\]
3. Simplify the calculation to find the molarity (M):
\[
M = 0.0686 \, \text{mol/L}
\]
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