Question

A scientist measures the freezing point depression of a 0.1m sodium nitrate solution. He uses the ideal van't hoff factor for the calculation of the ideal freezing point depression. the observed freezing point depression is.

Answer 1

A. not measurable, because the solution did not freeze.
B. lower than the theoretical.
C. less than the change in the boiling point.
D. higher than the theoretical.

Answer 2

first and foremost, let's assume that if we have some electrolyte XY in solution. I'm guessing that our van hoff factor i shows us how many moles of ions were produced by that solution. but what it assumes to my knowledge is that there isn't any interaction between molecules. you see i though that interactions between the ions might possibly explain why the van hoff factor measured experimentally would be lower than your ideal one.

\[XY --> X ^{+} + Y ^{-}\]