According to the Bronsted-Lowry acid-base theory, what are the conjugate acid and conjugate base of the amphiprotic hydrogen sulfate ion (HSO4-)?
Answer and explanation
Correct answer: C. Conjugate acid: H2SO4; Conjugate base: SO4(2-)
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Therefore, the conjugate acid of is sulfuric acid ().
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Therefore, the conjugate base of is the sulfate ion ().
Therefore, the conjugate acid of is sulfuric acid ().
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Therefore, the conjugate base of is the sulfate ion ().
- Step 1: A conjugate acid is formed when a Bronsted base accepts a single proton ():
- Step 2: A conjugate base is formed when a Bronsted acid donates a single proton ():
Answer
Conjugate acid: H2SO4; Conjugate base: SO4(2-)
Why not the others: 'Conjugate acid: SO4(2-)...' reverses the conjugate acid and base definitions; 'Conjugate acid: H3O+...' lists water conjugates; 'Conjugate acid: H2SO3...' involves sulfurous acid with an incorrect oxidation state.
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