(Answered) Consider the titration of 1000 ml of 0100 m acetic acid

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Consider the titration of 100.0 mL of 0.100 M acetic acid with 0.100 M NaOH.

CH₃CO₂H(aq) + OH^-(aq) →

CH₃CO₂^-(aq) + H₂O(l)

K_a for acetic acid = 1.8×10^-5

K_b for acetate ion = 5.6×10^-10

(a) What is the pH of the solution when 75.0 mL of 0.100 M NaOH has been added to 100.0 mL 0.100 M acetic acid?

(b) What is the pH at the equivalence point?

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