18. Aqueous Equilibrium

Consider the titration of a 23.0 mL sample of 0.120 M RbOH with 0.100 M HCl. Determine the pH after adding 4.3 mL of acid beyond the equivalence point.

Consider the titration of a 25.0 mL sample of 0.115 M RbOH with 0.100 M HCl. Determine the pH at 5.0 mL of added acid.

In the titration of a 35.0 mL sample of 0.175 M HBr with 0.210 M KOH, what is the pH after adding 5.0 mL of base beyond the equivalence point?

Determine the pH at the equivalence point for a titration of 50 mL of 0.1 M KOH with 0.1 M HClO4.

Suppose you are titrating an acid solution with a base solution of known concentration. To calculate the concentration of the acid solution, which of the following steps should you perform after finding the number of moles of base used?

The titration of a 20.0 mL sample of an H2SO4 solution of unknown concentration requires 22.51 mL of a 0.154 M KOH solution to reach the equivalence point. What is the concentration of the unknown H2SO4 solution? Express your answer to three significant figures.

Two 20.0-mL samples, one 0.200 M KOH and the other 0.200 M unknown base, are titrated with 0.100 M HI. What is the volume of added acid at the equivalence point for each titration?