Problem: Which one solution would have the highest vapor pressure at a given temperature? a. Li2SO4 b. C6H12O6 c. NaC2H3O2 d. KCl

FREE Expert Solution

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 highest vapor pressure has the weakest 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 osmolarity of each solution, which is given by:

Assuming that each solution has the same concentration:

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Problem Details

Which one solution would have the highest vapor pressure at a given temperature? 

a. Li2SO4 

b. C6H12O6 

c. NaC2H3O2 

d. KCl

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