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    Calculate the pH in titration of 25mL of 0.1M CH3COOH by NaOH after the addition to the acid solution of :
    a) 10mL of 0.1M NaOH
    b) 25mL of 0.1M NaOH
    c) 35mL of 0.1M NaOH

    so far i only got (a) by using Henderson-Hasselbalch equation. For (b) i don't know how to solve since the number of moles of CH3COOH and NAOH are the exact same, wouldn't they just cancel out? Doesn't that mean the pH of the solution would just be -log(Ka) + log(1mol/1mol) = pKa = 4.74 ??

    Meanwhile for (c) i just lost it. i don't know how to do it.

    I would really appreciate some help solving these question.
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Updated: May 16, 2015


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