Calculate the freezing point of a solution of 500.0 g of ethylene glycol dissovled in 500g water. Kf = 1.86 degrees C/m and Kb (which my instructor said was just extraneous info that is not used here) is 0.512 degrees C/m.

= -29.96 °C

Explanation: A solution has a lower freezing point compared to the pure solvent, due to the solute lowering the vapor pressure of the solvent.

The "new" freezing point is calculated as:

is the molal freezing-point depression constant

m is molality concentration, i.e., moles of solute per kilogram of solvent

Before calculating freezing point, let's find moles of ethylene glycol () in the solution:

Molar mass = 62.08 g/mol

For 500 g:

n = 8.05 moles

The molality concentration for 0.5kg of water:

m =

m = 16.11

The freezing point will be:

Freezing point of a solution of Ethylene Glycol and Water is -29.96°C