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Questions and Answers
Which of the following is NOT a colligative property?
Which of the following is NOT a colligative property?
- Boiling point elevation
- Color change (correct)
- Freezing point depression
- Vapour pressure lowering
What are colligative properties dependent on?
What are colligative properties dependent on?
The number of dissolved non-volatile solute species.
Osmotic pressure is of primary significance to pharmacists.
Osmotic pressure is of primary significance to pharmacists.
True (A)
What is Raoult's law related to?
What is Raoult's law related to?
The vapour pressure, P1, of a solvent over a dilute solution is equal to the vapour pressure of the pure solvent multiplied by the __________ of solvent in the solution.
The vapour pressure, P1, of a solvent over a dilute solution is equal to the vapour pressure of the pure solvent multiplied by the __________ of solvent in the solution.
What are colligative properties of solutions?
What are colligative properties of solutions?
What happens to the entropy of the solvent when a solute is dissolved?
What happens to the entropy of the solvent when a solute is dissolved?
Which of the following are colligative properties? (Select all that apply)
Which of the following are colligative properties? (Select all that apply)
Osmotic pressure is significant to pharmacists.
Osmotic pressure is significant to pharmacists.
What occurs when a solute is dissolved in a solvent?
What occurs when a solute is dissolved in a solvent?
According to Raoult’s law, P1 = X1______
According to Raoult’s law, P1 = X1______
Match the terms with their definitions:
Match the terms with their definitions:
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Study Notes
Learning Outcomes
- Ability to identify and discuss colligative properties of solutions.
- Understanding of iso-osmoticity versus isotonicity.
- Recognition of the importance of isotonicity in pharmaceutical preparations.
- Skill to perform calculations related to tonicity in pharmaceuticals.
Colligative Properties
- Defined as physical properties of solutions dependent on the number of dissolved non-volatile solute species.
- Key types of colligative properties include:
- Vapour pressure lowering
- Boiling point elevation
- Freezing point depression
- Osmotic pressure
- Osmotic pressure is particularly significant in pharmacy practices.
Vapour Pressure Lowering
- Non-volatile solutes decrease the vapour pressure of a solvent.
- Vapour pressure of the solution is lower than that of the pure solvent due to increased disorder (entropy).
- Reduction in vapour pressure is proportional to the relative number of solute molecules in the solution.
- Raoult’s law explains the relationship:
- Vapour pressure of a solvent over a dilute solution (P1) equals the pure solvent vapour pressure (𝜌𝜌1o) multiplied by the mole fraction of the solvent (X1).
- Representation: P1 = X1𝜌𝜌1o
- Vapour pressure lowering can be quantified as:
- ΔP = X2 𝜌𝜌1o (where X2 is the mole fraction of solute).
Elevation of Boiling Point
- The boiling point is defined as the temperature where the liquid's vapour pressure equals atmospheric pressure.
- Elevation of boiling point occurs when a solute is added, requiring a higher temperature for the vapour pressure to equal the atmospheric pressure.
Importance of Entropy
- Dissolving a solute increases the disorder of solvent molecules, leading to higher entropy (S).
- Increase in entropy results in lower free energy (G), described by the equation ΔG = ΔH – TΔS.
Learning Outcomes
- Ability to identify and discuss colligative properties of solutions.
- Understanding of iso-osmoticity versus isotonicity.
- Recognition of the importance of isotonicity in pharmaceutical preparations.
- Skill to perform calculations related to tonicity in pharmaceuticals.
Colligative Properties
- Defined as physical properties of solutions dependent on the number of dissolved non-volatile solute species.
- Key types of colligative properties include:
- Vapour pressure lowering
- Boiling point elevation
- Freezing point depression
- Osmotic pressure
- Osmotic pressure is particularly significant in pharmacy practices.
Vapour Pressure Lowering
- Non-volatile solutes decrease the vapour pressure of a solvent.
- Vapour pressure of the solution is lower than that of the pure solvent due to increased disorder (entropy).
- Reduction in vapour pressure is proportional to the relative number of solute molecules in the solution.
- Raoult’s law explains the relationship:
- Vapour pressure of a solvent over a dilute solution (P1) equals the pure solvent vapour pressure (𝜌𝜌1o) multiplied by the mole fraction of the solvent (X1).
- Representation: P1 = X1𝜌𝜌1o
- Vapour pressure lowering can be quantified as:
- ΔP = X2 𝜌𝜌1o (where X2 is the mole fraction of solute).
Elevation of Boiling Point
- The boiling point is defined as the temperature where the liquid's vapour pressure equals atmospheric pressure.
- Elevation of boiling point occurs when a solute is added, requiring a higher temperature for the vapour pressure to equal the atmospheric pressure.
Importance of Entropy
- Dissolving a solute increases the disorder of solvent molecules, leading to higher entropy (S).
- Increase in entropy results in lower free energy (G), described by the equation ΔG = ΔH – TΔS.
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