If 50.0 mL of a 0.1 solution of HOAc (Ka = 1.8 x 10^-5) has been titrated to the equivalence point with 0.1 M NaOH solution, what is the pH of the resulting solution? Please explain the math. Thanks.
For this question, you must get familiar with what I call ICE tables. Whenever you have titrations, you need to talk about moles as well. As for the equivalence point, you need moles of acid to equal moles of base.
M x volume = moles for each component
0.050 L x 0.1 M = 0.005 moles of HOAc, which means that I need 0.005 moles of NaOH, so I will need 50 mL of the 0.1 M ...
This solution calculates the level of pH acidity, given the equivalence point parameter.