Consider the titration of a 24.0 mL sample of 0.110 mol/L CH3COOH (Ka=1.8×10⁻⁵) with 0.125 mol/L NaOH. What volume of NaOH is required to reach the equivalence point?

A student titrated a 100 mL sample of 0.100 M acetic acid with 0.050 M NaOH. (For acetic acid, Ka = 1.8 × 10^-5 at room temperature.) Calculate the pH after 50.0 mL of NaOH has been added.

Consider the titration of 100.0 mL of 0.016 M HOCl (Ka=3.5×10⁻⁸) with 0.0400 M NaOH. Calculate the pH after the addition of 10.0 mL of 0.0400 M NaOH.

Consider the titration of 25.00 mL of 0.150 M hydrazoic acid (Ka = 1.90 × 10^-5) with 0.200 M NaOH. What is the pH of the solution after the addition of 15.00 mL of NaOH solution?

Consider the titration of 25.00 mL of 0.150 M hydrazoic acid (Ka = 1.90 x 10^-5) with 0.200 M NaOH. What is the pH of the solution at the equivalence point of the titration?

Determine the pH at the equivalence point for the titration of a 40.0 mL sample of 0.100 M HNO2 by 0.200 M KOH. (The pKa of nitrous acid is 3.34.)

In a titration of a weak acid with a strong base, what determines the pH at the equivalence point?

For a titration of 1.0 M benzoic acid (C6H5COOH, Ka = 6.5×10^-5) with 1.0 M NaOH, what is the pH at the equivalence point?

Suppose 40.0 mL of an acetic acid solution of unknown concentration is titrated with 0.100 M NaOH. After 20.0 mL of the base solution has been added, the pH in the titration flask is 5.10. What was the concentration of the original acetic acid solution?