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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?

Respuesta :

Answer:

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-

Answer:

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

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