Acid-dissociation constants of two acids are listed in the table above. A 20. mL

Question

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? (A) Solution I has a higher pH at the equivalence point because CH_3CO_2H is the stronger acid. (B) Solution 1 has a higher pH at the equivalence point because CH_3CO_2H has the stronger conjugate base. (C) Solution 1 has a lower pH at the equivalence point because CH_3CO_2H is the stronger acid.

Explanation / Answer

answer : B )

explanation:

A ) this option is wrong because CH3CO2H is the stronger acid its pH should be lesser

B) this is correct . if its conjugate base is stroges it should give OH- in the solution so its pH higher

   CH3COO- + H2O -----------------> CH3COOH + OH-

   conjugate base

C) CH3COOH is not strong acid

D) this is completely wrong from my second statement B

note : you missed to give tables and acids but my answer is correct

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