You know that an unlabeled water bottle contains at least some water. You measure the freezing point of the unknown substance and find that it freezes at a temperature lower than 0 degrees Celsius at 1 atmosphere pressure. Which of the following can you conclude?
A. The substance is pure water.
B. The substance will have a boiling point that is less than 100 degrees Celsius.
C. The substance will have a vapor pressure that is greater than that of pure water.
D. The substance is an aqueous solution.
Thanks in Advance

Question

You know that an unlabeled water bottle contains at least some water. You measure the freezing point of the unknown substance and find that it freezes at a temperature lower than 0 degrees Celsius at 1 atmosphere pressure. Which of the following can you conclude?
A.   The substance is pure water. 
B.   The substance will have a boiling point that is less than 100 degrees Celsius. 
C.   The substance will have a vapor pressure that is greater than that of pure water. 
D.   The substance is an aqueous solution. 
Thanks in Advance

australopithecus · Answer

When water has a solute in it and you sequester some of that water as vapor, or ice the concentration of solute is going to increase. 

As solvent decreases, solute concentration increases leading to a more ordered solution, this is not entropically favourable

australopithecus · Answer

Does that help you with your question?

australopithecus · Answer

Also you probably already know this but 0 Celsius is the freezing point of water, and 100 Celsius is the boiling point

australopithecus · Answer

at 1 atm

australopithecus · Answer

I would also assume that the solute is a solid for this question

anonymous · Answer

thanks for the help, i was on another tab :) thanks a bunch though

australopithecus · Answer

No problem