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?

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?

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?

What is the approximate pH at the equivalence point of a titration between formic acid (HCOOH) and sodium hydroxide (NaOH), given that 25 mL of formic acid is titrated with 29.80 mL of 0.1567 mol L⁻¹ NaOH? The acid dissociation constant (Ka) for formic acid is 1.8 × 10⁻⁴.