10 Questions
Explain the relationship between the solubility of a gas in a liquid and the partial pressure of the gas according to Henry's law.
Solubility of a gas in a liquid is directly proportional to the partial pressure of the gas at a given temperature.
Define ideal solutions and mention one property that characterizes them.
Ideal solutions obey Raoult's law over the entire range of concentration. One property that characterizes ideal solutions is that they show no deviation from Raoult's law.
What is the condition for the reversal of the osmosis process?
The reversal of osmosis can occur if a pressure higher than the osmotic pressure is applied to the solution.
What is the relationship between the lowering of vapor pressure and the concentration of solute particles according to Raoult's law?
The lowering of vapor pressure depends only on the concentration of the solute particles and is independent of their identity.
How is the relative lowering of vapor pressure defined in a solution?
The relative lowering of vapor pressure is equal to the mole fraction of the solute in the solution.
Explain how the equation for the reduction in vapor pressure simplifies in a solution with multiple non-volatile solutes.
In a solution with multiple non-volatile solutes, the reduction in vapor pressure is the sum of the mole fractions of all the solutes.
What causes positive deviation from Raoult's law?
When A-B interactions are weaker than A-A or B-B interactions.
How does positive deviation affect vapor pressure in solutions?
It increases the vapor pressure.
Why do mixtures of ethanol and acetone show positive deviation from Raoult's law?
The addition of acetone weakens hydrogen bonding interactions in ethanol.
What type of interactions make a solution show positive deviation from Raoult's law?
When dipolar interactions between solute-solvent molecules are weaker.
Study Notes
Henry's Law and Gas Solubility
- The solubility of a gas in a liquid is directly proportional to the partial pressure of the gas, as stated by Henry's Law.
- The law can be expressed mathematically as: C = k * P, where C is the concentration of the gas in the liquid, k is Henry's Law constant, and P is the partial pressure of the gas.
Ideal Solutions
- Ideal solutions are mixtures of two or more components that behave ideally, meaning they follow Raoult's Law and Henry's Law.
- One characteristic property of ideal solutions is that the vapor pressure of the solution is directly proportional to the mole fraction of each component.
Osmosis Reversal
- The reversal of the osmosis process occurs when the osmotic pressure of the more concentrated solution is greater than the external pressure applied to the system.
Raoult's Law and Vapor Pressure
- Raoult's Law states that the vapor pressure of a solution is proportional to the mole fraction of the solvent.
- The law can be expressed mathematically as: P = P° * x, where P is the vapor pressure of the solution, P° is the vapor pressure of the pure solvent, and x is the mole fraction of the solvent.
Relative Lowering of Vapor Pressure
- The relative lowering of vapor pressure is defined as the ratio of the vapor pressure of the solution to the vapor pressure of the pure solvent.
- Mathematically, it can be expressed as: ΔP/P° = (P° - P) / P°.
Multiple Non-Volatile Solutes
- In a solution with multiple non-volatile solutes, the equation for the reduction in vapor pressure simplifies to: P = P° * x, where x is the mole fraction of the solvent.
Positive Deviation from Raoult's Law
- Positive deviation from Raoult's Law occurs when the intermolecular forces between the solute and solvent molecules are weaker than the forces between the solvent molecules.
- Positive deviation causes the vapor pressure of the solution to be greater than predicted by Raoult's Law.
- Mixtures of ethanol and acetone show positive deviation from Raoult's Law due to the weak hydrogen bonding between the molecules.
- Positive deviation is caused by the presence of weak intermolecular forces, such as London dispersion forces or weak hydrogen bonding, between the solute and solvent molecules.
Test your knowledge on the principles of Henry’s Law and Raoult’s Law, which govern the dissolution of gases in liquids and the lowering of vapor pressure in solutions. Understand the relationships between gas solubility, partial pressure, and solute concentration in solutions.
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