A solution is a homogeneous mixture of two or more substances.
Solutions are classified as:
The concentration of a solution in terms of mole fraction, molarity, molality and in percentages.
Henry’s Law: The dissolution of a gas is governed by Henry’s Law which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas.
Raoult’s Law: This law states that the relative lowering of vapour pressure of the solvent over a solution is equal to the mole fraction of a non-volatile solute present in the solution.
Solutions which obey Raoult’s law over the entire range of concentration are called ideal solutions.
Two types of deviations from Raoult’s law, called positive and negative deviations, are observed. Azeotropes arise due to very large deviations from Raoult’s law.
Colligative properties: The properties of solutions which depend on the number of solute particles and are independent of their chemical identity are called colligative properties. These include:
Lowering of vapour pressure
Elevation of boiling point
Depression of freezing point
The process of osmosis can be reversed if a pressure higher than the osmotic pressure is applied to the solution.
Colligative properties have been used to determine the molar mass of solutes. Solutes which dissociate in solution exhibit molar mass lower than the actual molar mass and those which associate show higher molar mass than their actual values.
The extent to which a solute is dissociated or associated can be expressed by van’t Hoff factor i. This factor has been defined as ratio of normal molar mass to experimentally determined molar mass as the ratio of observed colligative property to the calculated colligative property.