A what is the ph of the solution whennbsp750nbspml of 0100

Question

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?

(c) What is the pH after 110.0 mL of NaOH has been added?