Asked by Drew
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.
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.
Answers
Answered by
DrBob222
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.
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.
Answered by
Anonymous
PartB.No,at this concentration,clustering of ions will cause the actual (f.p) depression to be less than expected.
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