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.

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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.

Chemistry
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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.
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. \[XY --> X ^{+} + Y ^{-}\]
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\[iK _{b}\Delta T\]
I thought it would be lower but I believe that was wrong. I thought maybe if the ions interact somehow maybe that would lower the i and lower the delta T. not sure. your thoughts are welcome
Said B. but it's wrong
is it A?/
@Photon336 I haven't tried all this neither learnt in school . But was trying with what I knew !
Freezing point depression is teh process when u add a solute to a solvent to decreases the freezing point of the solvent.
I would have guessed D.
@abb0t that's the correct answer
@Rushwr the answer is D.
@Photon336 I have no idea LOL! SOrry for that
So i would guess that since i is lower the van hoff factor, it doesn't freeze at a lower temperature as it should
so the temperature would be higher than the theoretical
Because of two reasons i guess it's like colligative properties; the first thing that i guess because the ions pair in solution, I think of it as there being fewer solute molecules in solution, so the freezing point would be higher than what's expected.
any thoughts are welcome
Nice. And yes, it is based on colligative properties.
will post another. question guys
okaaai

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