Is this similar to solving for the volume of the titrated solution! Help! how to do this?

Question

The following question refers to the titration of 25.00 mL of 0.131 M HCl with 0.143 M Ba(OH)2. The reaction proceeds according to the following stoichiometry:

2HCl + Ba(OH)2 BaCl2 + 2H2O

What will be the pH of the titrated solution at the equivalence point?

Answer 1

Barium Hydroxide (Ba(OH)2) is a strong base, meaning it will disassociate completely into ions in solution.
Hydrochloric acid (HCl) is a strong acid, it too will disassociate completely in solution.

In a strong acid - strong base titration, the equivalence point is neutral, pH = 7, when the acid / base reacts together in the proper stoichiometric ratio (neither are in excess).