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Calculate the molarities of CH3COOH and CH3COO-

  1. Feb 19, 2004 #1
    Can someone help me how to calculate the molarities of CH3COOH and CH3COO- in a buffer solution containing 40.00 ml of 0.100M acetic acid, 10.00 ml of distilled water and 30.00ml of 0.100M NaOH?
     
  2. jcsd
  3. Feb 19, 2004 #2

    GCT

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    What will happen after sodium hydroxide, which dissociates completely in water, is added? The hydroxide will alter the equilibrium of the acetic acid by reacting with _______?

    You need to find the new concentrations after the equilibrium.
     
    Last edited: Feb 19, 2004
  4. Feb 19, 2004 #3
    Still dont get it. Chemistry is a nightmare for me.Can someone explain in detail.:frown:
     
  5. Feb 20, 2004 #4

    GCT

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    Thus the first thing to do is to find the initial concentrations of both OH and acetic acid.

    The base, OH- (which dissociates completely), will react with the acetic acid directly. So subtract the original concentration of acetic acid by the concentration of hydroxide anion. Using this concentration substitute into the equilibrium equation and find the rest of the concentrations.

    Hope this answers your question.
     
  6. Feb 20, 2004 #5

    GCT

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    don't forget to add the concentration value of OH- to the conjugate base concentration of the acetic acid.
     
  7. Feb 26, 2004 #6
    thanks a lot
     
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