Explain below the effect of adding a non-volatile solute to a volatile solution would have on vapor pressure and boiling point. Why is this specific to non-volatile substances? Use math to support your answer.
Explain below the effect of adding a non-volatile solute to a volatile solution would have on vapor pressure and boiling point. Why is this specific to non-volatile substances? Use math to support your answer.
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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![**Effect of Adding a Non-volatile Solute to a Volatile Solution on Vapor Pressure and Boiling Point**
When a non-volatile solute is added to a volatile solvent, the overall vapor pressure of the solution decreases. This reduction in vapor pressure occurs because the solute particles occupy space at the liquid's surface, preventing some solvent molecules from escaping into the vapor phase.
**Vapor Pressure:**
The relationship can be explained by Raoult’s Law, which states that the vapor pressure of a solvent over a solution (\(P\)) is equal to the vapor pressure of the pure solvent (\(P^0\)) times the mole fraction of the solvent (\(X_{\text{solvent}}\)) in the solution:
\[ P = P^0 \times X_{\text{solvent}} \]
As the mole fraction of the solvent decreases with the addition of solute, the vapor pressure \(P\) also decreases.
**Boiling Point:**
The boiling point of the solution increases due to the decrease in vapor pressure. A solution boils when its vapor pressure equals the atmospheric pressure. Since the vapor pressure is lower, a higher temperature is required to reach the boiling point, leading to what is called boiling point elevation.
**Boiling Point Elevation Formula:**
\[ \Delta T_b = i \cdot K_b \cdot m \]
Where:
- \(\Delta T_b\) is the boiling point elevation.
- \(i\) is the van 't Hoff factor (number of particles the solute splits into).
- \(K_b\) is the ebullioscopic constant of the solvent.
- \(m\) is the molality of the solution.
This effect is specific to non-volatile solutes because they do not contribute to the vapor phase, thereby primarily impacting the solvent’s escaping tendency, altering both vapor pressure and boiling point significantly.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fee47860b-51bf-4c58-a4ad-6a29df2141ce%2F5e90a435-c013-4645-bd56-b71ed2cbf27c%2Faudskjn_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Effect of Adding a Non-volatile Solute to a Volatile Solution on Vapor Pressure and Boiling Point**
When a non-volatile solute is added to a volatile solvent, the overall vapor pressure of the solution decreases. This reduction in vapor pressure occurs because the solute particles occupy space at the liquid's surface, preventing some solvent molecules from escaping into the vapor phase.
**Vapor Pressure:**
The relationship can be explained by Raoult’s Law, which states that the vapor pressure of a solvent over a solution (\(P\)) is equal to the vapor pressure of the pure solvent (\(P^0\)) times the mole fraction of the solvent (\(X_{\text{solvent}}\)) in the solution:
\[ P = P^0 \times X_{\text{solvent}} \]
As the mole fraction of the solvent decreases with the addition of solute, the vapor pressure \(P\) also decreases.
**Boiling Point:**
The boiling point of the solution increases due to the decrease in vapor pressure. A solution boils when its vapor pressure equals the atmospheric pressure. Since the vapor pressure is lower, a higher temperature is required to reach the boiling point, leading to what is called boiling point elevation.
**Boiling Point Elevation Formula:**
\[ \Delta T_b = i \cdot K_b \cdot m \]
Where:
- \(\Delta T_b\) is the boiling point elevation.
- \(i\) is the van 't Hoff factor (number of particles the solute splits into).
- \(K_b\) is the ebullioscopic constant of the solvent.
- \(m\) is the molality of the solution.
This effect is specific to non-volatile solutes because they do not contribute to the vapor phase, thereby primarily impacting the solvent’s escaping tendency, altering both vapor pressure and boiling point significantly.
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