Question
An ethylene glycol solution contains 20.9 g of ethylene glycol (C2H6O2) in 85.0 mL of water. Compute the freezing point and boiling point of the solution. (Assume a density of 1.00 g/mL for water.)
freezing point
°C
boiling point
°C
How would I set this up?
thanks
freezing point
°C
boiling point
°C
How would I set this up?
thanks
Answers
moles ethylene clycol = grams/molar mass. Solve for mole.
molality = moles/kg solvent
Solve for molality
delta T = Kf*m and convert to freezing point.
delta T = Kb*m and add to 100 C to convert to boiling point.
molality = moles/kg solvent
Solve for molality
delta T = Kf*m and convert to freezing point.
delta T = Kb*m and add to 100 C to convert to boiling point.
Thanks
Related Questions
An aqueous antifreeze is 40.0% ethylene glycol (C2H6O2) by mass. The density of the solution is 1.05...
Calculate the vapor pressure of water over each of the following ethylene glycol C2H6O2 solutions at...
A 13.03 g sample contains only ethylene glycol (C2H6O2) and propylene glycol (C3H8O2). When the samp...
A chemist has two ethylene glycol and water solutions: one that contains 11.98% ethylene glycol an...