unknown Substance Benzoic Aud 122.1239 /mol REPORT SHEET Freezing Point Depressi
ID: 530504 • Letter: U
Question
unknown Substance Benzoic Aud 122.1239 /mol REPORT SHEET Freezing Point Depression A. Preparation of experimental apparatus and freezing point determination of lauri acid 1. Mass of freezing point depression apparatus 2. Mass of freezing point depression apparatus with lauric acid 3. Mass of lauric acid used OO B. Freezing point determination of a lauric acid solution 4. Designation of unknown 5. Mass of added unknown, Exp. 3 6. Mass of added unknown, Exp. 4 Freezing point of lauric acid from Part A,Exp. 1 (Mol3) Freezing point of lauric acid from Part A, Exp.2 Average freezing point of lauric acid Freezing point of lauric acid and unknown from Part B, Exp 3 (Plato) 42. OO Freezing point oflauric acid and unknown from Part B, Exp 4 (tlalo) Exp 4 AT T solution molality (show calculations) Exp 3 170 M Exp 4 KF Moles of unknown (show calculation) Exp.3 Exp 4 Mol Molar mass of unknown (show calculation) Exp 3 Exp. 4 M m I 009 1.80 x 10 mo Average molar mass molar mass of unknown. Show your calculations for the solution molality, mole of unknown, and Hand in your cooling curves with your report sheet. SSS S 122.12 Achal- Theo x 100 en GalExplanation / Answer
The major sources of error in this experiment have to relate to measurements. Either temperature, weighting masses, etc. Also, a source of error could be the actual calculations that were made.
As for the molarity, it depends... If it was a consistent error in the thermometer, then the difference of temperatures to calculate the molality would not have changed ( 4-3 = 1, as well as 2.6 - 1.6= 1).
If the error was not consistent, the molality would have decreased if the error was in the pure-substance temperature; but increased if the error was in the mixed-substance temperature. As the molality changes, the molarity would change likewise.
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