After 50.0 mL of a 0.100 M solution of NaOH is added to 50.0 mL of a 0.100 M solution of an unknown acid, the equilibrium pH is basic. What may be concluded about the identity of the acid?

Question

Quizplus · Accepted Answer

Since the addition of NaOH causes the equilibrium pH to be basic, we know that the acid must be weak. The fact that it could be either monoprotic, diprotic, or polyprotic is due to the fact that there are many weak acids with different numbers of acidic hydrogen ions that could fit this description. Therefore, the best choice is D.

After 500 ML of a 0