We’re being asked to rank the given solutions in order of increasing vapor pressure and give 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.
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 osmolality 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.
When the following aqueous solutions are ranked in order of INCREASING vapor pressure, which solution is fourth on the list?
0.2 m KNO3
0.2 m urea, (NH2)2CO
0.1 m CaCl2
0.1 m glucose, (C6H12O6)
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