An unknown alcohol is analyzed by freezing point depression. The unknown is either methanol (CH3OH), ethanol (C2H5OH), or propanol, (C3H7OH). A solution made by adding 10.423 g of the unknown to 100.0mL of water freezes at -4.2 degrees C [water kFP= -1.853 degrees C.kg/mol, assume d(water)= 1g/mL]. Explain how you used the data to identify the alcohol.
mass of unknown = 10.423 g
mass of water = 100 g
delta Tf = Kf x m
0 - (- 4.2) = 1.853 x m
m = 2.266
molality = 2.266 m
molality = moles of solute / mass of solvent
2.266 = moles / 0.1
moles = 0.2266
moles = mass / molar mass
0.2266 = 10.423 / molar mass
molar mass = 45.985 g/mol
corresponding alcohol is Ethanol. because its molar mass - 46 g/mol
An unknown alcohol is analyzed by freezing point depression. The unknown is either methanol (CH3OH), ethanol...
1. What is the freezing point depression for the unknown solution for each trial? 2. How do you determine the van't Hoff factor for each trial, and what is the average van't Hoff factor? Trial 1: 18mL of 0.200 m unknown, ionic compound solution initial temp: 17.90 degrees C. observed freezing point of solution: -1.55 degrees C. Observed freezing point of water: -0.84 degrees C. Trial 2: 20 mL of 0.200 m unknown, ionic compound solution initial temp: 17.66 degrees...
A freezing point depression experiment was conducted using tert-butyl alcohol as the solvent instead of water The freezing point of pure tert-butyl alcohol is 27C and Kf=9.1C/mol. To 25g of tert-butyl alcohol was added 0.70 g of a non-electrolyte solute (i.e. sugar). The solution was cooled and the new freezing point was determined to be 20C. 1. What is the molar mass of the unknown non-electrolyte solute? 2. In a similar experiment, MgCl2 (MW= 95.2 g/mol) solute was added to...
Chemistry:
Molar mass determination and freezing point depression.
If your unknown solute sample weighed 0.634 grams, but some of it stuck to the test tube wall when you were pouring it in and did not dissolve in the t-butyl alcohol, what sort of error will this cause in the calculated molar mass of your unknown solute? Explain. What would be the freezing point of an aqueous solution that contains 10.3 grams of ethylene glycol [(C_2H_4(OH)_2] in 100 mL of water?
Freezing Point Depression: Determination of the Molar Mass of an Unknown Substance Laboratory Record Unknown Identifier #4 (All unknowns are nonelectrolytes, soi-1) Determination of the freezing point of pure l-butyl alcohol: (Record time-temperature data on the next page) 29.62 1. Mass of empty test tube 2. Mass of test tube and t-butyl alcohol after determination of freezing point of pure t-butyl alcohol 50.25 20.71 3. Mass of t-butyl alcohol Determination of the molar mass of an unknown: (Record time-temperature data...
1a. Please review Data Table #2 and check the information that
has been filled in for accuracy/fill in the remaining information
that has not been completed.
1b. Based on your temperature measurements, which molecule seems
to have the strongest intermolecular forces? What is/are the
force(s) in that particular molecule? Use your data to explain your
reasoning.
1c. Which seems to have the weakest intermolecular forces? What
is/are the force(s) in that particular molecule? Use your data to
explain your reasoning....