Solutions
A solution is the mixture in which the substances are intermixed so intimately that they cannot be observed as distinct components. The dispersed phase or the substance which is to be dissolved is called as solute, while dispersion medium in which the solute is dispersed to obtain a homogenous mixture is called as solvent.
Solubility
The Solubility of a substance can be defined as the amount of the solute dissolved in 100gms of the solvent to form a saturated solution at the given temperature. A saturated solution is the solution which contains at the given temperature as much solute as it can hold in the presence of dissolving solvent. Any solution can contain less solute than it would be necessary to saturate it. Such type of solution is known as unsaturated solution. When solution contains more solute than would be necessary to saturate it then it is called as supersaturated solution.
Colligative properties
The certain properties of the dilute solutions containing the non-volatile solute does not depend upon the nature of the solute which is dissolved but depend only upon the concentration that is the number of particles of the solute present in the solution. Such properties are termed as colligative properties. The four well known examples of colligative properties are,
(1) The lowering of vapour pressure of solvent.
(2) Osmotic pressure of solution.
(3) The elevation in the boiling point of solvent.
(4) The depression in freezing point of solvent.
As colligative properties depend on the number of solute particles present in the solution, simple case will be that when the solute is the non-electrolyte in nature. In case the solute is an electrolyte, it might split into a number of ions each of which acts as the particle and hence will affect the value of the colligative property.
Each of the colligative property is exactly related to other; Relative lowering of the vapour pressure, elevation in the boiling point and depression in the freezing point are directly proportional to the osmotic pressure.
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