Sketch the titration curve for the titration of 100.0 mL of 0.500 M KOH with 0.500 M HBr. Calculate the volume of HBr required to reach the equivalence point, and show the following pH in the sketch:
a) Before addition of HBr
b) At the equivalence point
c) After addition of excess HBr

For the titration of 0.15 M solutions of HClO₄ and NaOH, what is the pH at the equivalence point? Choose a suitable indicator from the table below.

After the addition of 5.0 mL of base beyond the equivalence point, what is the pH of the solution of 15.0 mL of 0.126 M nitric acid titrated with 0.145 M NaOH?

A 0.150 M NaOH solution is used to titrate two separate acid solutions: A 25.00 mL 0.124 M HI solution and a 20.00 mL 0.184 M CH₃COOH solution. Which of the two titration curves will have a higher pH at the start?

What will be pH at the equivalence point when a 25 mL sample of 0.115 M LiOH is titrated against a 0.0750 M solution of HI?

Consider these two 25.0 mL basic solutions: 0.450 M NaOH and 0.450 M C₆H₅NH₂. These two solutions are titrated with 0.150 M HCl. Calculate the volume of acid that should be added to reach the equivalence point for each titration.