Acid-dissociation constants of two acids are listed in the table above. A 20. mL sample of a 0.10 M solution of each acid is titrated to the equivalence point with 20. mL of 0.10 M NaOH. Which of the following is a true statement about the pH of the solutions at the equivalence point?

Solution 1 has a higher pH at the equivalence point because CH3CO2H has the stronger conjugate base.

Explanation:

Since according to the chemical reaction shown below, if the conjugated base is stroboscopic, the product of the reaction would be an OH- so that its pH is higher:

CH3COO- + H2O  = CH3COOH+ OH-

Refer below for the explanation.

Explanation:

CH₃CO₂H has a higher conjugate base because Solution 1 has a bigger pH at the similar point.

Solution

1 CH₃CO₂H 1.75 x 10⁻⁵

2 CF₃CO₂H 1.0 x 10⁰

water and alcohols have similar properties because water molecules contain hydroxyl groups that can form hydrogen bonds with other water molecules and with alcohol molecules, and likewise alcohol molecules can form hydrogen bonds with other alcohol molecules as well as with water.