Calculate the boiling point of the solution.
whats you do for the next step then
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?
3 answers
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.
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.
Identify the percent by volume of ethylene glycol in a solution that freezes at -10.°C.
4 answers