The problem shows two soulutions of NaCl in water, one iscompletely dissolved, t
ID: 690910 • Letter: T
Question
The problem shows two soulutions of NaCl in water, one iscompletely dissolved, the other with solid salt at thebottom. It asks which one will have the higher vapor pressureand to explain. I believe that this will be due to Raoultslaw, stating that a solution with solute dissolved in it will haveonly a fraction of the vapor pressure that the pure substance wouldhave. Am I to understand that the less solute a solution hasrelative to another, the higher its respective vapor pressure wouldbe?The next part of the question states that one of these solutionswill have a constant vapor pressure, even as water evaporates fromit. I would pick the solution with a completely aqueoussolution because it is a homogeneous solution, completelymixed. Is this relating to it being an ideal solution, wherevapor pressure is enriched in the more volatile component relativeto the solution? Im not sure if this directly applies and Iwould like to be as specific as possible here.
The third part of the problem asks which solution will have thehigher boiling point. I already stated that the solution withsolid NaCl AND dissolved NaCl would likely have the lower vaporpressure, so I believe it must also have the higher boiling pointdue to there being MORE solute in the solution.
Thank you very much I would greatly appreciate an answer as soon aspossible as i am a little bit CRAMming for a chemistrymidterm. The time given is about 5 minutes before I beginwriting so hurrry please. :D
Explanation / Answer
In the first part what you are think is the correct. In the socond part also your assumption is right. In this case we are not consider the vapour pressure .Whenheat is supplied to the system containing the solid present at thebottom in the the solution , first the solid will absorb heatto dissolve in the solution & then the total solution iscomes to the vapour state.So it will have more boiling point.Related Questions
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