delta T = i*Kf*m
i = van't Hoff factor, which for KNO3 is 2.
So -0.744.
b. Have you had anything about the Debye-Huckel theory/law. That says the 0.2 m is not quite 0.2 and as the concn increases there is more attraction between solvent/solute molecules. The net result is the same as the explanation you gave.
a. Calculate the expected freezing-point depression of a 0.200 m KNO3 solution.
b. Will the value you calculated match the actual freezing-point depression for this solution?
Why or why not?
a). -0.372 degrees Celsius
b). Possibly because not all of the substance ionizes 100% of the time? Not really sure.
2 answers
PartB.No,at this concentration,clustering of ions will cause the actual (f.p) depression to be less than expected.
1 answer