Q.
The colligative properties of electrolytes require a slightly diferent approach than the one used for the colligative properties of non- electrolytes. The electrolytes dissociate
into ions in solution. It is the number of solute particles that determine the colligative properties of a solution. The electrolyte solutions, therefore show abnormal colligative properties. To account for this effect we define a quantity; called the van't Hoff factor which is given by [solution]
$i= \frac{\text{Actual number of particles in solution after dissociation}}{\text{ Number of formula units initially dissolved in solution }}$
$i =1$ (for non - electrolytes);
$i >1$ (for electrolytes, undergoing dissociation)
$i < 1$ (for solute, undergoing association)
For a solution of a non electrolyte in water, the van't Hoff factor is
Solutions
Solution: