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NaHCO3 as an acid as a base

  1. Mar 31, 2009 #1
    1. The problem statement, all variables and given/known data

    Write two equations that illustrate that an aqeous solution of NaHCO3 can act either as an acid or a base. In pure water show quantitatively which of the two reactions predominate. ka1= 4.2x10-7, Ka2=4.8x10-11


    3. The attempt at a solution
    as an acid:

    NaHCO3(aq) + H2O(l)---> H3O+(aq) + NaCO3-(aq)

    Base:

    NaHCO3(aq) + H2O(l) ------> OH-(aq) + NaH2CO3+(aq)

    The second part is where I am having some trouble. I am not sure if I am doing this correctly so i will try to show and explain what I think will happen as best I can. I think Ka1 will predominate the reason being that kb1= (1x10^-14)/(4.2x10^-7)=2.38x10^-8
    so Ka1>Kb1 therefore this reaction will proceed. Meaning most of the sodium bicarbonate will act as an acid and release protons. whereas Kb2=(1x10^-14)/(4.8x10^11)=2.08x10^-4.
    so Kb2>>Ka2 so releasing a 2nd proton is not very favorable the species is much more likely to pick up another proton then it is to release another proton.
     
    Last edited: Mar 31, 2009
  2. jcsd
  3. Mar 31, 2009 #2
    I guess if I am correct then the fact that Ka1 is quantitatively greater then kb1 is the proof that ka1 will predominate.
     
  4. Mar 31, 2009 #3

    symbolipoint

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    Your written reactions are good. For which dissocation of bicarbonate is more favorable, check the Na2CO3 hydrolysis steps on the way towards H2CO3, or check the dissocation steps of H2CO3 toward Na2CO3. You know how to find Ka from corresponding Kb, right?
     
  5. Mar 31, 2009 #4
    How does NaHCO3 become Na2CO3? I am not sure exactly what you mean by checking the Na2CO3 hydrolysis steps on the way towards H2CO3.
     
  6. Mar 31, 2009 #5

    symbolipoint

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    Synergix, maybe I was sloppy with my terminology or notation. You were on a good track with your idea of comparing the acidic dissociation constant for bicarbonate to the equilibrium constant for HCO3- + H20 <===> H2CO3 + OH-
    Are you studying weak acid-base equilibria right now? If so, you will soon know how to evaluate those constants.
     
  7. Mar 31, 2009 #6
    Ya we have covered that already as part of the last section. I will look at it again maybe I can figure it out thanks.
     
  8. Apr 1, 2009 #7

    Borek

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    pH of amphiprotic salt

    I am not sure you can say which of the reactions dominate. If you will read through the lecture you will find that ratio [H2CO3]/[CO32-] is close to 1, that means both reactions proceed to the same degree.
     
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