Flask 1: 2 g Nacl, 200 g H20 flask 2: 2 g KCl, 200 g H20. MW of NaCl = 58.4 MW of KCl = 74.5 Why is this a false statement: the solution in flask 2 has a higher vapor pressure than the solution in flask #2. Wouldn't NaCl have the lower BP because it has the lower mass, thus, there should be more NaCl in the flask. Edit: wait: the BP proportional to mass has to do with pure liquids/solids, right? So, I guess we should approach this problem differently. So, then because there are more solute in flask 1, it would have a higher BP, because BP elevation = Kim. Then higher bp= lower vapor pressure. Right?