The statement "although sulfuric acid is a strong electrolyte, an aqueous solution of h2so4 contains more hso4− ions than so42− ions" is the statement "although sulfuric acid is a strong electrolyte, an aqueous solution of h 2 s o 4 contains more h s o 4 − ions than s o 4 2 − ions" is blank. this is best explained by the fact that h 2 s o 4 blank.. this is best explained by the fact that h2so4 the statement "although sulfuric acid is a strong electrolyte, an aqueous solution of h 2 s o 4 contains more h s o 4 − ions than s o 4 2 − ions" is blank. this is best explained by the fact that h 2 s o 4 blank..

The statement "Although sulfuric acid is a strong electrolyte, an aqueous solution of H₂SO₄ contains more HSO₄⁻ ions than SO₄²⁻ ions is True. This is best explained by the fact that H₂SO₄ is a diprotic acid where only the first hydrogen completely ionizes.

Why?

H₂SO₄ is a diprotic acid. That means that it has two hydrogen ions to give to the solution. The two dissociation reactions are shown below:

H₂SO₄ + H₂O → HSO₄⁻ + H₃O⁺

HSO₄⁻ + H₂O ⇄ SO₄²⁻ + H₃O⁺

As the arrows show, the first dissociation is complete, meaning that all the sulfuric acid that is present initially is dissociated into HSO₄⁻ and H₃O⁺. However, the second dissociation is incomplete, and it's actually an equilibrium with an acid constant  (Ka)of 1.2×10⁻².

That means that if the initial concentration of H₂SO₄ was 1M, the concentration of HSO₄⁻ is going to be 1M as well, but the concentration of SO₄²⁻ is going to be much less than 1M, according to the dissociation constant.

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aquifers are bounded above and below by impermeable rock. the driving force of groundwater movement in confined aquifers is pressure, rather than gravity.