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owlet

  • one year ago

Strong, weak, or nonelectrolyte? how will I know? propyl amine, potassium iodide and carbonic acid, what kind of electrolyte are they?

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  1. owlet
    • one year ago
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    @aaronq @Vocaloid

  2. owlet
    • one year ago
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    @Photon336 @Shalante

  3. Jhannybean
    • one year ago
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    write these all out as chemical compounds first

  4. owlet
    • one year ago
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    ok.. propyl amine: \(CH_3CH_2CH_2NH_2\) potassium iodide: KI and carbonic acid: \(H_2CO_3\)

  5. owlet
    • one year ago
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    then..?

  6. owlet
    • one year ago
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    I think KI is a strong electrolyte.. because of K+ and I-

  7. Photon336
    • one year ago
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    @owlet electrolytes usually produce ions in solution

  8. Jhannybean
    • one year ago
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    Im not too sure about propyl amine, but if you look at it's structure you know that \(\sf CH_3CH_2CH_2\mathbf{NH_2}\) have hydrogen bonds, and hydrogen bonds take a lot of energy to break. You are right about \(\sf KI\), therefore it's a strong electrolyte because it has an ionic bond, and ionic bonds are soluble in water. for Carbonic Acid, \(\sf H_2CO_3\), ask yourself whether it's a strong acid, if it's a strong acid, then it's a strong electrolyte

  9. Photon336
    • one year ago
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    I think acids are also considered electrolytes. and their strength depends on how many H+ ions are produced.

  10. Jhannybean
    • one year ago
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    for acids and bases, the strength of their electrolytes depends on whether theyre a strong acid, or a strong base

  11. owlet
    • one year ago
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    okay.. just wanted to confirm.. if a substance is a strong acid/base then they are strong electrolytes?

  12. Photon336
    • one year ago
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    yeah, because that means more ions are produced

  13. Jhannybean
    • one year ago
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    Acetate, \(\sf HC_2H_3O_2\) is a weak electrolyte compared to let's say... nitric acid, \(\sf HNO_3\)

  14. owlet
    • one year ago
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    what about organic compounds, like glucose? they have H bonds also..?

  15. Photon336
    • one year ago
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    |dw:1443922500887:dw| @owlet question to you is that compound above hexane would that be considered an electrolyte?

  16. Photon336
    • one year ago
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    and why?

  17. owlet
    • one year ago
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    i think it is nonelectrolyte because.. it doesn't ionize in water..?

  18. Photon336
    • one year ago
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    yep @owlet another one, which one is a better electrolyte and why? |dw:1443922689755:dw|

  19. owlet
    • one year ago
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    I'm not sure about that one

  20. owlet
    • one year ago
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    both of them will ionize, aren't they?

  21. Photon336
    • one year ago
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    =]

  22. owlet
    • one year ago
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    acetic acid is a strong acid, so it should be the one i think

  23. Photon336
    • one year ago
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    what does acidic strength mean? and how does this relate to electrolyte strength?

  24. owlet
    • one year ago
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    hmm acidic strength has something to do with loosing H+ ? it is related to electrolyte strength because i think.. if the acid is strong, it will ionize completely(loose all H+) .. i don't know anymore

  25. owlet
    • one year ago
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    but acetic acid and sulfuric acid are both strong acids though??

  26. Photon336
    • one year ago
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    yep strong acid will produce more H+

  27. Photon336
    • one year ago
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    @owlet acetic acid is a weak acid, sulfuric acid is a strong acid

  28. Photon336
    • one year ago
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    so based off of this which would be the better electrolyte?

  29. owlet
    • one year ago
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    ohh so it is sulfuric acid? quick question.... i know this may sound dumb.. but why is acetic acid a weak one?

  30. Photon336
    • one year ago
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    yep =]

  31. Photon336
    • one year ago
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    well because it loses some of it's protons, not all. have you heard of something called Ka, acid dissociation constant. NOT pKA \[HA --> H ^{+} + A ^{-} | Ka = \frac{ [H ^{+}][A ^{-}] }{ [KA] } \]

  32. owlet
    • one year ago
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    yeah I remember doing that. I completely forgot everything, that's why I'm revising everything :3

  33. Photon336
    • one year ago
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    so @owlet would a strong acid have a High Ka or low, and how could you tell this from looking at the equation?

  34. owlet
    • one year ago
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    They should have a high Ka. The larger the Ka, the larger the [H+] ?

  35. owlet
    • one year ago
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    If [H+] is high, then it means the acid can donate more?

  36. Photon336
    • one year ago
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    =] yep

  37. Photon336
    • one year ago
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    like unfortunately, I was told in my chem classes to just memorize that H2SO4 is a strong acid, I don't like that but that's what I was told lol. but it's a strong acid b/c it's Ka is high. which means it's pKA meaning -log[Ka] will be small.

  38. owlet
    • one year ago
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    yes! ok i think i'm getting it now.. yeah same thing, we have to like memorize a table of strong & weak acids and bases before doing the solving part. Probably that's the reason why forgot everything lol let me try another substance.. carbonic acid... will it be weak?

  39. Photon336
    • one year ago
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    In my classes they taught me that well yeah, These are your strong acids H2SO4 HNO3 HCL HBr HI H3PO4 i think i'm missing one. everything else is weak

  40. owlet
    • one year ago
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    how about HF?

  41. Photon336
    • one year ago
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    that's a weak acid

  42. owlet
    • one year ago
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    oh yeah one more thing, before i closed this question.. how about alcohols also?

  43. Photon336
    • one year ago
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    F- i think is very unstable and it's going to react readily

  44. Photon336
    • one year ago
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    I'm not too sure about alcohols but I think they would be weak electrolytes

  45. Photon336
    • one year ago
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    at least in water though could be different

  46. owlet
    • one year ago
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    F is super negative so it will attach to H+ more than the other group 17 i think, so probably it is weak.. hmm okay, i will try to read more to find out about alcohols. Thanks a lot for the help! :)

  47. Photon336
    • one year ago
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    no problem

  48. Jhannybean
    • one year ago
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    \(\color{#0cbb34}{\text{Originally Posted by}}\) @Photon336 In my classes they taught me that well yeah, These are your strong acids H2SO4 HNO3 HCL HBr HI H3PO4 i think i'm missing one. everything else is weak \(\color{#0cbb34}{\text{End of Quote}}\) You were pissing perchloric acid i believe, \(\sf HClO_4\)

  49. Jhannybean
    • one year ago
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    \(\sf H_3PO_4\) is a weak acid :P

  50. Photon336
    • one year ago
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    this is what happens when you just memorize stuff, I always forget one of them BTW how do you quote lol? @Jhannybean

  51. Jhannybean
    • one year ago
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    Ohh Jaynator has a script you add to chrome for OS that allows you quote, and post images in the drawing tool as well as use different colors when drawing things as well. I'll have to find the link to the script, or you can ask Nnesha :P

  52. Photon336
    • one year ago
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    if you find it please send that to me!

  53. Jhannybean
    • one year ago
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    sure thing!

  54. owlet
    • one year ago
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    since you guys are still here.... HNO2 vs.HNO3, which is a stronger one? HNO3 right?

  55. owlet
    • one year ago
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    nvm, got it

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