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The statement 'Although sulfuric acid is a strong electrolyte, an aqueous solution of H2S04 contains more HSO4 ions than SO42 ions is

a. H2SO4 reacts with H20 by hydrolysis
b. HSO4 ions undergo disproportionation
c. SO42 ions are preferentially attracted to the cathode
d. SO42 ions form insoluble complexes in the solution

User Comonadd
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Final answer:

An aqueous solution of sulfuric acid contains predominantly HSO4- ions over SO42- ions because sulfuric acid ionizes in two stages and the second stage of ionization is not as complete as the first.

Step-by-step explanation:

The statement 'Although sulfuric acid is a strong electrolyte, an aqueous solution of H2SO4 contains more HSO4- ions than SO42- ions' can be understood by examining the ionization stages of sulfuric acid. Sulfuric acid is a strong diprotic acid that ionizes in water in two stages. The first stage of ionization is nearly complete, where H2SO4 loses one proton to form HSO4-. This first dissociation is strong, resulting in a high concentration of HSO4- ions. The second stage, where HSO4- loses another proton to form SO42-, is not as complete, making HSO4- a moderately strong acid but not fully ionized like the first stage. The given dissociation constants (Ka) indicate that in a solution predominantly HSO4- ions are present compared to SO42- ions.

User Dibs
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