Problem: When the following aqueous solutions are ranked in order of INCREASING vapor pressure, which solution is fourth on the list (lowest vapor pressure)?a. 0.2 m KNO3b. 0.2 m urea, (NH2)2COc. 0.1 m CaCl2d. 0.1 m glucose, (C6H12O6)

We’re being asked to rank the given solutions in order of increasing vapor pressure and determine the 4th on the list

The vapor pressure of a solution is related to the intermolecular forces: a stronger IMF leads to lower vapor pressure. This means the solution with the lowest vapor pressure has the strongest IMF, and vice-versa. 

Recall that a solution with higher solute concentration will have a stronger IMF, resulting in lower vapor pressure. Therefore, we need to calculate the osmolality of each solution, which is given by:

$\boxed{\mathbf{Osmolality}\mathbf{=}\mathbf{i}\mathbf{\times }\frac{\mathbf{moles}\mathbf{ }\mathbf{of}\mathbf{ }\mathbf{solute}}{\mathbf{Liters}\mathbf{ }\mathbf{of}\mathbf{ }\mathbf{solution}}}$

where i = van’t Hoff factor.