Explain can't hoof factors

The van’t Hoff factor is a relation between the ideal value of a solution’s colligative properties and the observed colligative properties such as relative lowering of vapour pressure, elevation of boiling point, depression of freezing point and osmotic pressure.In other words, the van 't Hoff factor is the ratio between the actual concentration of particles produced when the substance is dissolved, and the concentration of a substance as calculated from its mass

For strong electrolytes, Van 't Hoff factor equals the number of ions per formula unit of the ionic compound.The experimentally measured Van 't Hoff factors are generally less than theoretically predicted ones for a given solute due to pairing of ions in the solution.For example: in aqueous MgSO₄ solution, i _theor = 2 whereas in 0.50M MgSO₄, i _expt = 1.07 and in 0.005M MgSO₄, i _expt = 1.72.For nonelectrolytes such as ethanol, benzene etc., Van 't Hoff factor is 1.0.For a weak electrolyte such as acetic acid, Van 't Hoff factor is greater than 1 but less than the total number of ions available for dissociation.