H₂SO₄

Definition

H₂SO₄, also known as sulfuric acid, is a strong, corrosive, and highly reactive chemical compound that plays a crucial role in the context of Brønsted-Lowry acid-base theory. It is a diprotic acid, meaning it can donate two protons (H⁺) in aqueous solutions.

5 Must Know Facts For Your Next Test

1. Sulfuric acid, H₂SO₄, is a strong, diprotic acid that completely dissociates in water, producing two hydrogen ions (H⁺) per molecule.
2. The first and second acid dissociation constants (Ka1 and Ka2) of sulfuric acid are 1.0 × 10⁻³ and 1.2 × 10⁻¹⁷, respectively, indicating its high acidity.
3. Sulfuric acid is a versatile industrial chemical, used in the production of fertilizers, explosives, and various other products.
4. The high acidity of sulfuric acid makes it a powerful proton donor, allowing it to readily participate in Brønsted-Lowry acid-base reactions.
5. Sulfuric acid is a key component in the lead-acid batteries used in many vehicles, where it helps facilitate the electrochemical reactions that generate electricity.

Review Questions

• Explain how the diprotic nature of sulfuric acid (H₂SO₄) affects its behavior as a Brønsted-Lowry acid.
  • As a diprotic acid, sulfuric acid (H₂SO₄) can donate two protons (H⁺) in aqueous solutions, forming two separate acid-base equilibria. The first dissociation step produces the bisulfate ion (HSO₄⁻), which can then further dissociate to produce the sulfate ion (SO₄²⁻) in the second step. This ability to donate multiple protons makes sulfuric acid a stronger Brønsted-Lowry acid compared to monoprotic acids, allowing it to readily participate in acid-base reactions and influence the pH of solutions.
• Describe the relationship between the acid dissociation constants (Ka) of sulfuric acid and its strength as a Brønsted-Lowry acid.
  • The acid dissociation constants (Ka) of sulfuric acid, specifically Ka1 and Ka2, provide a measure of its strength as a Brønsted-Lowry acid. The first acid dissociation constant (Ka1) of sulfuric acid is 1.0 × 10⁻³, while the second constant (Ka2) is 1.2 × 10⁻¹⁷. These high Ka values indicate that sulfuric acid is a strong acid, meaning it readily dissociates in water to produce a high concentration of hydrogen ions (H⁺). The large magnitude of the Ka values reflects the strong tendency of sulfuric acid to donate protons, which is a key characteristic of a Brønsted-Lowry acid.
• Analyze the role of sulfuric acid (H₂SO₄) in the context of Brønsted-Lowry acid-base theory and its practical applications.
  • In the context of Brønsted-Lowry acid-base theory, sulfuric acid (H₂SO₄) is a powerful proton donor due to its diprotic nature and high acid dissociation constants. This allows it to readily participate in acid-base reactions, where it can donate protons to other substances, acting as a Brønsted-Lowry acid. The strong acidity of sulfuric acid makes it a versatile industrial chemical, with applications ranging from the production of fertilizers and explosives to its use in lead-acid batteries. Additionally, the ability of sulfuric acid to influence the pH of solutions through its proton-donating behavior is crucial in various chemical and biological processes, underscoring its importance in the context of Brønsted-Lowry acid-base theory.

Related terms

Brønsted-Lowry Acid: A Brønsted-Lowry acid is a substance that can donate a proton (H⁺) to another substance, thereby acting as a proton donor.

Diprotic Acid: A diprotic acid is a polyprotic acid that can donate two protons (H⁺) in aqueous solutions, forming two separate acid-base equilibria.

Acid Dissociation Constant (Ka): The acid dissociation constant (Ka) is a measure of the strength of an acid, indicating the extent to which it dissociates in an aqueous solution.