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What are some problems with the use of water as a solvent for determining the molecular mass of an unknown using the freezing point depression method?
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∙ 12y ago
i dont know this answer but know is mad and donkey
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∙ 12y ago
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What is freezing point elevation?
This is not a common phenomenon. Usually it is boiling points that are elevated, and freezing points are depressed. It is possible that a freezing point could be raised (elevated) due to the presence of an impurity with a much higher freezing point.Changes in boiling and freezing points are typically due to impurities in compound.See the Related Questions to the left for more information about freezing point depression and boiling point elevation problems.
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What is freezing point depression?
For the definition and description of freezing point lower or freezing point depression[http://www.answers.com/freezing+point+depression?cat=technology&gwp=13Click here for the answer from Answers.com]For how to solve a freezing point depression problem with step-by-step instructions click on this question:[http://wiki.answers.com/Q/How_do_you_solve_freezing_point_depression_problemsHow do you solve freezing point depression problems?]
How do you solve freezing point depression problems when given only the molarity?
Calculating the freezing point depression of a solvent requires three pieces of information: 1) the molal freezing point depression of that solvent; 2) the molality of the solution; 3) the number of distinct entities produced in solution per molecular formula unit of solute. Hopefully you meant molality instead of molarity (if the solvent is water and it's a dilute solution, assuming that molality = molarity isn't a bad approximation). I suspect you've been told what 1 and 3 are (or been given enough information to figure them out) but simply didn't mention it; otherwise you're pretty much boned.
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