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Calculate the pH-value of a solution that does not contain water

  1. Nov 13, 2005 #1
    Hi,

    How do one calculate the pH-value of a solution that does not contain water, pH being equal to -log([H3O+])?

    I need to calculate the pH-value of a solution where BaCO3 and SrCO3 is dissolved in acetic acid (4 M). The only information I am given is, that half of the acetic acid is consumed in the reaction. Any hints?
     
  2. jcsd
  3. Nov 13, 2005 #2

    mrjeffy321

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    Science Advisor

    You are given that the acetic acid is 4 Molar solution, and more likely than not, it is dissolve in water.
     
  4. Nov 14, 2005 #3
    Ok, I see. The reaction is this (right?):

    CO3^2- + CH3COOH -> HCO3^- CH3COO^-​

    How can I determine pH? All I know is that half of the CH3COOH is used up in this reaction.
     
    Last edited: Nov 14, 2005
  5. Nov 14, 2005 #4

    Astronuc

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    Staff: Mentor

  6. Nov 14, 2005 #5
    Thanks, man! :-)
     
  7. Nov 14, 2005 #6

    Astronuc

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  8. Nov 14, 2005 #7

    Borek

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    Staff: Mentor

    Carbonates will decompose in acetic acid. You will be left with acetic buffer.

    Although in so concentrated solution ionic strength is too high for any serious calculations.
     
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