Is sulfuric acid a strong acid, strong base, weak acid, or weak base
The Correct Answer and Explanation is:
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Sulfuric acid (H₂SO₄) is classified as a strong acid. This is because it dissociates completely in aqueous solution, meaning that it releases all of its hydrogen ions (H⁺) into the solution. The dissociation process occurs in two steps:
- First dissociation: H₂SO₄ → H⁺ + HSO₄⁻. In this first step, sulfuric acid dissociates completely, releasing a proton (H⁺) and forming the hydrogen sulfate ion (HSO₄⁻). This step is virtually complete in dilute solutions, making sulfuric acid a strong acid in this regard.
- Second dissociation: HSO₄⁻ → H⁺ + SO₄²⁻. The second dissociation step is not as complete as the first, but it still contributes to the acidic nature of the solution. The hydrogen sulfate ion (HSO₄⁻) can further dissociate to release another proton, forming the sulfate ion (SO₄²⁻). However, this second dissociation is only partial, and the extent depends on the concentration of sulfuric acid.
Despite the partial dissociation in the second step, the complete dissociation in the first step is enough to categorize sulfuric acid as a strong acid in practical applications.
Sulfuric acid also plays a key role in many industrial processes, such as the production of fertilizers, petroleum refining, and as a catalyst in chemical reactions. Its ability to fully ionize in water is what makes it a strong acid, able to lower the pH of a solution dramatically.
In summary, sulfuric acid is considered a strong acid because it dissociates fully in its first step and nearly completely in the second, contributing significantly to its acidic properties.
