Question

An ethylene glycol solution contains 26.2g of ethylene glycol (C2H6O2) in 81.4mL of water. Calculate the freezing point of the solution. (Assume a density of 1.00 g/mL for water.)

how do I set this up?

Answer 1

Calculate the boiling point of the solution.

whats you do for the next step then

Answer 2

mols ethylene glycol = grams/molar mass = ?
81.4 mL at density of 1.00 g/mL = 81.4g
Convert 81.4 g to kg.
molality = mols eth gly/kg solvent, then
delta T = Kf*m
You know Kf is 1.86 and you know m from above. Solve for delta T and subtract from 0 to find new freezing point.

For the boiling point, Kb is 0.512, m is same as above, solve for delta T = K*m and add to normal boiling point to find new boiling point.
Post your work if you get stuck.

Answer 3

Identify the percent by volume of ethylene glycol in a solution that freezes at -10.°C.