Question

Part A: At equal concentrations, would a nonelectrolyte ( glucose) or electrolyte (NaCl) containing solution have a lower freezing point? Why?

Part B: Arrange the following in increasing freezing point order (lowest to highest): pure H20, aqueous NaF (0.31m), aqueous glucose (0.60m), aqueous sucrose (0.50m), aqueous Mgl2 (0.22m)

Answer 1

A ) ) deltaTf = To-Tf= i xKf x( M2/ solute molar mass) x (1000/ M1 )     

i increase deltaTf increase but Tf of the solution decrease

electrolyte freezing point less compared to non electrolyte freezing point with same concentrations. it is due to i value (vanthoff factor) . depession in freezing point increase with number of ions so freezing point decrease.

     Glucose freezing point > NaCl freezing point

        B)    Mgl2 (0.22m) < NaF (0.31m) <pure H20 <glucose (0.60m)<sucrose (0.50m)

Answer 2

十2 2丁 -0.66ド, F.P