In regards to freezing point depression: The original experiment calls for 3 grams lauric acid and .4 g benzoic acid to be melted and then observed to crystalize to demonstrate freezing point depression. A student misreads the directions and adds 4.0 g of benzoic acid instead of 0.4 g. What do you expect to happen? Would the experiment still be valid? Explain your reasoning. I think that since the amount of lauric acid (3g) doesnt change that the solution may be too oversaturated with benzoic acid. I'm not sure if this would still demonstrate freezing point depression since it is a colligative property based on amount of solute....
In regards to freezing point depression: The original experiment calls for 3 grams lauric acid and .4 g benzoic acid to be melted and then observed to crystalize to demonstrate freezing point depression. A student misreads the directions and adds 4.0 g of benzoic acid instead of 0.4 g. What do you expect to happen? Would the experiment still be valid? Explain your reasoning. I think that since the amount of lauric acid (3g) doesnt change that the solution may be too oversaturated with benzoic acid. I'm not sure if this would still demonstrate freezing point depression since it is a colligative property based on amount of solute....
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter10: Properties Of Solutions
Section: Chapter Questions
Problem 7RQ
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In regards to freezing point depression:
The original experiment calls for 3 grams lauric acid and .4 g benzoic acid to be melted and then observed to crystalize to demonstrate freezing point depression.
- A student misreads the directions and adds 4.0 g of benzoic acid instead of 0.4 g. What do you expect to happen? Would the experiment still be valid? Explain your reasoning.
I think that since the amount of lauric acid (3g) doesnt change that the solution may be too oversaturated with benzoic acid. I'm not sure if this would still demonstrate freezing point depression since it is a colligative property based on amount of solute....
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