🤓 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:
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 2H3O2 in 100.0 mL of water
(2) 20.0 g of sucrose (C12H22O11) in 100.0 mL of water
(3) 20.0 g of glucose (C 6H12O6) in 100.0 mL of water