Question

Explain the Van’t Hoff rule.

Answer 1

Hint : In order to answer this question, we must know about the changes in molar mass and various colligative properties caused due to dissociation and association in solution. The concept of colligative properties and molar mass can help to solve this question

Complete step-by-step solution:
We all know molar mass is known to us as the mass of a sample of that compound divided by the amount of substance in that substance (measured in mole). Colligative properties are known as those properties of a solution that rely upon the proportion of the number of solute particles to the number of dissolvable particles in an answer, and not on the idea of the substance species present. As the Scientist Van’t Hoff know osmotic pressure increments by around $\dfrac{1}{273}$ for every level of temperature increment, he concludes that the osmotic pressure $\pi$of a solution having $n$a number of moles of the solute particle in a volume$V$of the solution is given–
$\pi =\dfrac{nRT}{V}$
Where$R$= gas constant ($0.0821$L atm$mo{{l}^{-1}}{{K}^{-1}}$)
$T$= is the absolute temperature
Rather than the need to utilize solute molality to ascertain the impacts of a non-unpredictable solute on changes in the freezing and boiling point of the solution.

Note: With the help of the theory of Van’t Hoff we can discover the modern theory of chemical equilibrium, chemical affinity, chemical thermodynamics, and chemical kinetics. The higher degree of Van’t Hoff factor is responsible for higher degree of dissociation.