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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.

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  1. Photon336
    • one year ago
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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.

  2. Photon336
    • one year ago
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    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. \[XY --> X ^{+} + Y ^{-}\]

  3. Photon336
    • one year ago
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    |dw:1438971657651:dw|

  4. Photon336
    • one year ago
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    \[iK _{b}\Delta T\]

  5. Photon336
    • one year ago
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    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

  6. Photon336
    • one year ago
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    Said B. but it's wrong

  7. Rushwr
    • one year ago
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    is it A?/

  8. Rushwr
    • one year ago
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    @Photon336 I haven't tried all this neither learnt in school . But was trying with what I knew !

  9. abb0t
    • one year ago
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    Freezing point depression is teh process when u add a solute to a solvent to decreases the freezing point of the solvent.

  10. abb0t
    • one year ago
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    I would have guessed D.

  11. Photon336
    • one year ago
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    @abb0t that's the correct answer

  12. Photon336
    • one year ago
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    @Rushwr the answer is D.

  13. Rushwr
    • one year ago
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    @Photon336 I have no idea LOL! SOrry for that

  14. Photon336
    • one year ago
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    So i would guess that since i is lower the van hoff factor, it doesn't freeze at a lower temperature as it should

  15. Photon336
    • one year ago
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    so the temperature would be higher than the theoretical

  16. Photon336
    • one year ago
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    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.

  17. Photon336
    • one year ago
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    any thoughts are welcome

  18. abb0t
    • one year ago
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    Nice. And yes, it is based on colligative properties.

  19. Photon336
    • one year ago
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    will post another. question guys

  20. Rushwr
    • one year ago
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    okaaai

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