Question

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

• A. Always equal to 2
• B. Always equal to 0
• C. $>1$ but $<2$
• D. $\le 1$

Answer 1

Answer: (D)

Correct answer is (d) $\le 1$