pH at equivalence point (Matthew's Workshop Week 2 #5)

[Aliya 1H]

Can someone please help w this!! I can't get it

5. (15 min) Acetic acid (CH 3COOH) is a common weak acid that gives vinegar its sour taste. At
25℃, its pK a
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? Hint: The equivalence point in a titration is where the
moles of acid = the moles of base.

[Chem_Mod]

In future posts, please provide the steps you have already taken and more specific questions you have about the problem.

Here I would start with finding out how many moles of acid you have, which is also how many moles of base you added since moles acid= moles base at equivalence point. From there you can find the volume of base added since you have the molarity. This will give you the volume to use when calculating molarity at equilibrium. At equivalence point, all the moles of acid have reacted with base, so you now have only conjugate base. Do an ICE box with the reaction of conjugate base with water, find [OH-] and use that to find pH