Answer:
They all have about the same vapor pressure.
Explanation:
The elevation of the vapor pressure is related to the elevation of the boiling point: for higher vapor pressure, the liquid will boils at a low temperature.
When a nonvolatile compound is added to the liquid, the boiling temperature increases, in an effect called ebullioscopy, and that difference of temperature can be calculated by:
ΔT = K*W*i
Where K is a constant for the liquid, W is the molality, and i is the van't Hoff factor, which depends on the dissociation of the compound.
i = dissociated particles/total particles
For the molecules compounds given, the ideal van't Hoff factor is 1.
The molality can be calculated by:
W = n1/m2
Where n1 is the number of moles of the solute and m2 is the mass of the solvent. In this case, all the solutes have the same number of moles for the same volume of the solution because they have the same concentration, so the change in temperature is the same for all of them.
Then, they all have about the same vapor pressure.
