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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Our tutors have indicated that to solve this problem you will need to apply the The Colligative Properties concept. You can view video lessons to learn The Colligative Properties. Or if you need more The Colligative Properties practice, you can also practice The Colligative Properties practice problems.

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