🤓 Based on our data, we think this question is relevant for Professor Brewer's class at UARK.

We’re being asked to **rank the given solutions** in order of **increasing vapor pressure**.

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.

We’re given the mass of solute and the volume of solvent (water).

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

$\overline{){\mathbf{Osmolarity}}{\mathbf{=}}{\mathbf{i}}{\mathbf{\times}}\frac{\mathbf{moles}\mathbf{}\mathbf{of}\mathbf{}\mathbf{solute}}{\mathbf{Liters}\mathbf{}\mathbf{of}\mathbf{}\mathbf{solution}}}$

where **i = van’t Hoff factor**.

Note that all the given volumes are in mL so we need to *convert mL to L*.

Rank the following solutions from lowest to highest vapor pressure. To rank items as equivalent, overlap them.

(1) 10.0 g of potassium acetate KC _{2}H_{3}O_{2} in 100.0 mL of water

(2) 20.0 g of sucrose (C_{12}H_{22}O_{11}) in 100.0 mL of water

(3) 20.0 g of glucose (C _{6}H_{12}O_{6}) in 100.0 mL of water