The colligative properties of electrolytes require a slightly different
Channel: Doubtnut
Date: 2020-03-29

The colligative properties of electrolytes require a slightly different approach than the one used for the colligative properties of non-electrolytes. The electrolytes dissociate into ions in a solution. It is the number fo solute particles that determines 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, given by : `i=(\"Actual number of particles in solution after dissociation\")/(\"NUmber of formula units initially dissolved in solution\")` `i=1` (for non-electrolytes) , `i gt 1` (for electrolytes, undergoing dissociation) `i lt 1` (for solutes, undergoing association). The molare mass of the solute sodium hydroxide obtained from the measurement of the osmotic pressure of its aqueous solution at `27^(@)C` is `25 \"g mol\"^(-1)`. Therefore, its dissociation percentage in this solution is :