Key Concepts and Formulas:
Types of Solutions
- Solute: The component present in a smaller quantity.
- Solvent: The component present in a larger quantity.
- Solute: The component present in a smaller quantity.
- Solvent: The component present in a larger quantity.
Concentration of Solutions
- Molarity (M): Moles of solute per liter of solution.
- Molality (m): Moles of solute per kilogram of solvent.
- Mole fraction (χ): Moles of a component divided by the total moles in the solution.
- Mass percentage (%w/w): Mass of solute divided by mass of solution (in grams) multiplied by 100.
- Molarity (M): Moles of solute per liter of solution.
- Molality (m): Moles of solute per kilogram of solvent.
- Mole fraction (χ): Moles of a component divided by the total moles in the solution.
- Mass percentage (%w/w): Mass of solute divided by mass of solution (in grams) multiplied by 100.
Raoult's Law
- For an ideal solution, the partial vapor pressure of a component is proportional to its mole fraction in the solution.
- Vapor pressure lowering: The vapor pressure of a solution is lower than that of the pure solvent due to the presence of solute
- For an ideal solution, the partial vapor pressure of a component is proportional to its mole fraction in the solution.
- Vapor pressure lowering: The vapor pressure of a solution is lower than that of the pure solvent due to the presence of solute
particles.
Colligative Properties
- Properties that depend on the number of solute particles, not on the nature of the solute.
- Relative lowering of vapor pressure: The decrease in vapor pressure of a solution compared to the pure solvent.
- Elevation of boiling point: The increase in boiling point of a solution compared to the pure solvent.
- Depression of freezing point: The decrease in freezing point of a solution compared to the pure solvent.
- Osmotic pressure: The pressure required to prevent the flow of solvent across a semipermeable membrane.
Formulas:
- Molarity (M): M = moles of solute / volume of solution (L)
- Molality (m): m = moles of solute / mass of solvent (kg)
- Mole fraction (χ): χA = moles of A / total moles
- Mass percentage (%w/w): %w/w = (mass of solute / mass of solution) × 100
- Raoult's Law: PA = χA × PA°
- Relative lowering of vapor pressure: ΔP = PA° - PA
- Elevation of boiling point: ΔTb = Kb × m
- Depression of freezing point: ΔTf = Kf × m
- Osmotic pressure (π): π = CRT (where C is molarity, R is the gas constant, and T is temperature)
Important Points:
- Ideal solutions: Solutions that obey Raoult's Law at all concentrations.
- Non-ideal solutions: Solutions that deviate from Raoult's Law, usually due to intermolecular forces between solute and solvent particles.
- Colligative properties can be used to determine the molar mass of a solute.
- Osmotic pressure is used in dialysis and reverse osmosis.
Revision Tips:
- Understand the concepts of concentration and colligative properties.
- Practice numerical problems to apply the formulas.
- Learn the relationships between the different colligative properties.
- Remember the key points about ideal and non-ideal solutions.
- Review the applications of colligative properties in various fields.
Additional Resources:
- Properties that depend on the number of solute particles, not on the nature of the solute.
- Relative lowering of vapor pressure: The decrease in vapor pressure of a solution compared to the pure solvent.
- Elevation of boiling point: The increase in boiling point of a solution compared to the pure solvent.
- Depression of freezing point: The decrease in freezing point of a solution compared to the pure solvent.
- Osmotic pressure: The pressure required to prevent the flow of solvent across a semipermeable membrane.
Formulas:
- Molarity (M): M = moles of solute / volume of solution (L)
- Molality (m): m = moles of solute / mass of solvent (kg)
- Mole fraction (χ): χA = moles of A / total moles
- Mass percentage (%w/w): %w/w = (mass of solute / mass of solution) × 100
- Raoult's Law: PA = χA × PA°
- Relative lowering of vapor pressure: ΔP = PA° - PA
- Elevation of boiling point: ΔTb = Kb × m
- Depression of freezing point: ΔTf = Kf × m
- Osmotic pressure (π): π = CRT (where C is molarity, R is the gas constant, and T is temperature)
Important Points:
- Ideal solutions: Solutions that obey Raoult's Law at all concentrations.
- Non-ideal solutions: Solutions that deviate from Raoult's Law, usually due to intermolecular forces between solute and solvent particles.
- Colligative properties can be used to determine the molar mass of a solute.
- Osmotic pressure is used in dialysis and reverse osmosis.
Revision Tips:
- Understand the concepts of concentration and colligative properties.
- Practice numerical problems to apply the formulas.
- Learn the relationships between the different colligative properties.
- Remember the key points about ideal and non-ideal solutions.
- Review the applications of colligative properties in various fields.
Additional Resources:
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