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Photon336
 one year ago
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.
Photon336
 one year ago
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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Photon336
 one year ago
Best ResponseYou've already chosen the best response.0A. 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.

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0first 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. \[XY > X ^{+} + Y ^{}\]

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0dw:1438971657651:dw

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0I 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

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0Said B. but it's wrong

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.0@Photon336 I haven't tried all this neither learnt in school . But was trying with what I knew !

abb0t
 one year ago
Best ResponseYou've already chosen the best response.2Freezing point depression is teh process when u add a solute to a solvent to decreases the freezing point of the solvent.

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0@abb0t that's the correct answer

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0@Rushwr the answer is D.

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.0@Photon336 I have no idea LOL! SOrry for that

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0So i would guess that since i is lower the van hoff factor, it doesn't freeze at a lower temperature as it should

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0so the temperature would be higher than the theoretical

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0Because 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.

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0any thoughts are welcome

abb0t
 one year ago
Best ResponseYou've already chosen the best response.2Nice. And yes, it is based on colligative properties.

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0will post another. question guys
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