Titrations and salts

[William_Hora_2H]

Acetic acid (CH3COOH) is a common weak acid that gives vinegar its sour taste. At 25℃, its pKa is 4.76. Suppose you titrate 100. mL of a 7.410 x 10-3 M solution of acetic acid with an appropriate volume of 1.482 x 10-2 M NaOH to the equivalence point at 25℃. What is the pH of the solution at the equivalence point?

My question is: Why do we assume that the mol acetate = mol acetic acid?

[SarahOMalley1D]

At an equivalence point, the moles of proton donors and proton acceptors will be equal. That is why the equivalence point of a strong acid/base titrated with a strong base/acid will have a pH of 7. Even though this is not a strong acid/base, the moles of proton donors and acceptors will still need to be equal at the equivalence point.