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March 28, 2017

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Consider a weak acid-strong base titration in which 25.0 mL of 0.100 M acetic acid is titrated with 0.100 M NaOH.

a) Calculate the pH after the addition of 3.00mL of NaOH.

b) What is the pH of the solution before the addition of NaOH (pKa of acetic acid=4.75)

I got pH= 3.88 for part A

  • Chemistry - ,

    I agree with your answer of 3.88 for part A (but I don't know that you worked it correctly since you didn't show any work). Part B is done this way.
    HAc = CH3COOH = acetic acid.

    .................HAc ==> H^+ + Ac^-
    initial...........0.1M... .0......0
    change............-x......+x......+x
    final............0.1-x.....x.......x

    Ka = (H^+)(Ac^-)/(HAc)
    Plug into Ka expession from the ICE chart I constructed above and solve for (H^+), then convert to pH.

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