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Super stuck on Titration problem

  1. Oct 18, 2009 #1
    A 10.00 mL solution of 0.2500 M CH3COONa is titrated with 0.1300 M HCl to the equivalence point.
    CH3COO− + H+ → CH3COOH
    volume of HCl required=19.23 mL

    Calculate the pH of the solution at the equivalence point.

    I've tried this a million ways and still keep getting it wrong. Also, my chemistry prof doesn't respond or have office hours so I'm kind of on my own :( Thank you in advance for your help :).
     
  2. jcsd
  3. Oct 18, 2009 #2

    symbolipoint

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    You need the dissociation constant for acetic acid. It is a weak acid, and therefore the equivalence point pH will be greater than 7.
     
  4. Oct 19, 2009 #3

    Borek

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  5. Oct 20, 2009 #4
    Dissociation constant for CH3COOH
    Ka = 1.8 x 10^-5
     
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