Calculate the volume (mL) of 0.500 M NaOH required to reach the equivalence point in the titration of 25.0 mL of 0.650 M HF. K_a for HF = 3.5 × 10⁻⁴.

You are given a solution of HCOOH (formic acid) with an approximate concentration of 0.20 M and you will titrate this with a 0.1105 M NaOH. If you add 20.00 mL of HCOOH to the beaker before titrating, approximately what volume of NaOH will be required to reach the equivalence point?

In a titration of a weak acid with a strong base, how is the pH determined before reaching the equivalence point?

What is the pH at the equivalence point for a titration involving 25 mL of 0.1 M acetic acid and 0.2 M KOH, given that the acid dissociation constant (Ka) for acetic acid is 1.8 × 10^-5?

During the titration of a weak acid with a strong base, which of the following statements is true regarding the pH at the equivalence point?

For a titration of a weak acid with a strong base, the pH at the equivalence point ________.

20.0 mL of 0.500 M HC₂H₃O₂ is titrated with 0.350 M KOH. Determine the pH after 15.0 mL of the base has been added. K_a for HC₂H₃O₂ = 1.8 × 10⁻⁵.

20.0 mL of 0.500 M HC₂H₃O₂ is titrated with 0.350 M KOH. Determine the pH after 15.0 mL of the base has been added. K_a for HC₂H₃O₂ = 1.8 × 10⁻⁵.

Determine the pH when 5.00 mL of excess KOH (beyond the equivalence point) has been added to the titration of 20.0 mL of 0.500 M HC₂H₃O₂ with 0.350 M KOH.