State whether each of the following statements is true or false. Justify your answer in each case.
(c) Although sulfuric acid is a strong electrolyte, an aqueous solution of H₂SO₄ contains more HSO₄^- ions than SO₄^2- ions.

Verified step by step guidance

1. Identify the nature of sulfuric acid (H2SO4) in aqueous solution. Sulfuric acid is a strong acid and a strong electrolyte, meaning it dissociates completely in water.
2. Understand the dissociation process of H2SO4 in water. Initially, H2SO4 dissociates into H+ and HSO4- ions.
3. Recognize that HSO4- can further dissociate into H+ and SO4^2- ions. However, HSO4- is a weaker acid compared to H2SO4.
4. Consider the relative strengths of the acids involved. Since H2SO4 is a stronger acid than HSO4-, the first dissociation step is more complete than the second. This results in a higher concentration of HSO4- ions compared to SO4^2- ions in the solution.
5. Conclude that the statement is true. In an aqueous solution of sulfuric acid, there are indeed more HSO4- ions than SO4^2- ions due to the complete and preferential first dissociation of H2SO4 and the partial second dissociation of HSO4-.

Key Concepts

Strong Electrolytes

Strong electrolytes are substances that completely dissociate into ions when dissolved in water. This means that they conduct electricity very well due to the presence of free-moving ions. Sulfuric acid (H2SO4) is classified as a strong electrolyte because it ionizes completely in aqueous solution, producing H+ ions and sulfate ions.

Dissociation of Sulfuric Acid

Sulfuric acid dissociates in two steps: first, it ionizes to form H+ and HSO4- ions, and then HSO4- can further dissociate into H+ and SO4^2- ions. The first dissociation is strong and produces a significant amount of HSO4-, while the second dissociation is weaker, resulting in fewer SO4^2- ions compared to HSO4- ions in solution.

Ion Concentration in Aqueous Solutions

In an aqueous solution of sulfuric acid, the concentration of HSO4- ions is greater than that of SO4^2- ions due to the predominance of the first dissociation step. This means that, at equilibrium, there will be more HSO4- ions present than SO4^2- ions, which supports the statement in the question.