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Topic: Freezing Points of varying molal solutions  (Read 6094 times)

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Offline soccer05

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Freezing Points of varying molal solutions
« on: December 10, 2006, 11:37:59 AM »
How could you arrange the following aqueous solutions in order of increasing freezing points?

0.10 m glucose, 0.10 m BaCl2, 0.20 m NaCl and 0.20 m Na2SO4
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Offline Borek

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Re: Freezing Points of varying molal solutions
« Reply #1 on: December 10, 2006, 12:09:09 PM »
What lowers freezing point?
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Offline soccer05

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Re: Freezing Points of varying molal solutions
« Reply #2 on: December 10, 2006, 06:25:33 PM »
the molality lowers freezing point. does molar mass have anything to do with this?
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Offline Borek

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Re: Freezing Points of varying molal solutions
« Reply #3 on: December 10, 2006, 06:56:27 PM »
Quote from: soccer05 on December 10, 2006, 06:25:33 PM
the molality lowers freezing point

Just molality? What if the substance dissociates?
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Offline sdekivit

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Re: Freezing Points of varying molal solutions
« Reply #4 on: December 11, 2006, 06:46:42 AM »
remember the formula for freezing point depression: delta Tf = Kf * m * a

--> m = molality and a is amount of dissociation.
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Offline soccer05

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Re: Freezing Points of varying molal solutions
« Reply #5 on: December 12, 2006, 03:27:32 PM »
ohh! thanks. my teacher never taught me about the amount of dissociation part.
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