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needchemhelp
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So we did an experiment of freezing point depression and my calculated molar mass values were larger than actual...
First, the freezing point of the pure solvent had to be determined and so if some of the solvent was on the walls of the test tube opposed to in the solution how would this affect results?
As far as I've gotten is that it would result in a greater actual molality than observed, but how would this then effect temperature change and molar mass?
hope this is enough, please help
First, the freezing point of the pure solvent had to be determined and so if some of the solvent was on the walls of the test tube opposed to in the solution how would this affect results?
As far as I've gotten is that it would result in a greater actual molality than observed, but how would this then effect temperature change and molar mass?
hope this is enough, please help