Solutions Flashcards
Intensive properties
Properties which do not depend upon the quantity of matter present in the system are called intensive properties
E.g. temperature, density, concentration
Extensive properties
Properties which depend upon the quantity of matter present in the system are called extensive properties
E.g. no. of moles, mass, volume, enthalpy
Colligative properties
Properties of solutions which depend upon the number of solute particles (molecules or ions) present in a definite amount of solvent but not on the chemical nature of solute are called colligative properties
Name 4 colligative properties
- Lowering of vapour pressure
- Elevation of boiling point
- Depression of freezing point
- Osmotic pressure
Henry’s Law
At a constant temperature, solubility of a gas in a liquid is directly proportional to pressure of the gas
Partial pressure of the gas in vapour phase is directly proportional to the mole fraction of the gas in solution (Dalton’s Law)
p= Kₕ ⋅ Χ
where KH= Henry’s Law constant
Factors affecting solutbility of a solid in a liquid
- Nature of solute and solvent: (Non-)polar solutes dissolve readily in (non-)polar solvents but not non-(polar) solvents
-
Temperature:
* When a substance dissolves with the evolution of heat (exothermic) solubility decreases with rise in temperature
* When a substance dissolves with absorption of hear (endothermic) solubility increases with rise in termperature
Factors affecting V.P. of a liquid
-
Nature of the liquid:
Weak intermolecular forces- more VP
Strong intermolecular forces- less VP -
Temperature
VP of a liquid increases with increase in temperature
Addition of non-volatile solute lowers VP
GRW addition of non-volatile solute to volatile solvent leads to lowering of VP
- Pure solvent has only liquid particles on the surface
- In a solution with non-volatile solite, solid particles also occupy space of the liquid surface
- Area of surface containing liquids decreases
- Escaping tendency of molecules decreases
- VP decreases
GRW addition of non-volatile solute to volatile solvent leads to lowering of VP
- Pure solvent has only liquid particles on the surface
- In a solution with non-volatile solite, solid particles also occupy space of the liquid surface
- Area of surface containing liquids decreases
- Escaping tendency of molecules decreases
- VP decreases
Raoult’s Law: Both statements
- For a solution of volatile liquids, the partial VP of each component in soln is directly propotional to its mole fraction
Po - P / Po = Xsolute - For a soln of volatile liquids, the partial VP of each component in the soln at a particular remperature is equal to the product of VP of the component in the pure state and its mole fraction in solution
Pₛₒₗᵤₜᵢₒₙ= Pₛₒₗᵥₑₙₜ ⋅ Χ
Ideal solution
A solution of two or more completely miscible liquids that obeys Raoult’s Law at all concentrations and temperatures
Non-ideal solutions
Solutions which do not follow Raoult’s Law
Positively deviated non-ideal solution
Theoretical VP < Observed VP
E.g.
Water + methanol
Water + ethanol
Acetone + benzene
Negatively deviated non-ideal solution
Theoretical VP > Observed VP
E.g.
HCl + water
Chloroform + benzene
Water + nitric acid
Azeotropic mixture
The solution of completely miscible liquids, which boils at a constant temperature like a pure liquid and distils over without any change in composition is called an azeotropic mixture