a student collecting data in a freezing point depression lab calculates the mola

Question

a student collecting data in a freezing point depression lab calculates the molar mass of a solid by seeing how much it lowers the freezing point of a solvent. However, she finds the molar mass is 15% higher than the true molar mass of the solid. The student then debates with the other students about where the error could come from. They all identify the following possible mistakes: (1) solid didnt completely dissolve in the solvent. (2) the student pipetted more solvent into the solution than she realized (3) the solid actually dissociated slightly into two particles as it dissolved. (4) some solid remained on the weighing paper. (5) the container holding the solution was rinsed with solvent and not dried before the experiment. WHICH mistake(s) could account for this error? and please explin why

Explanation / Answer

the student did not take the vant hoff factor into consideration which is
=i-1/n-1

so the solid did not dissociate completely and the student pipetted more liquid.

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