Here are the essential concepts you must grasp in order to answer the question correctly.
Acid Strength
Acid strength refers to the ability of an acid to donate protons (H⁺ ions) in a solution. Stronger acids dissociate more completely in water, leading to a higher concentration of H⁺ ions. The strength of an acid is influenced by its molecular structure, including the stability of its conjugate base after proton donation.
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Conjugate Base Stability
The stability of a conjugate base is crucial in determining the strength of its corresponding acid. A more stable conjugate base results from factors such as resonance, electronegativity, and size of the atoms involved. In the case of H₂SO₄ and H₂SO₃, the conjugate base of H₂SO₄ (HSO₄⁻) is more stable than that of H₂SO₃ (HSO₃⁻), making H₂SO₄ a stronger acid.
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Strength of Conjugate Acids and Bases
Oxidation State and Acidic Behavior
The oxidation state of the central atom in an acid can influence its acidic behavior. In H₂SO₄, sulfur is in a higher oxidation state (+6) compared to H₂SO₃ (+4). Higher oxidation states typically lead to stronger acids due to increased positive charge on the central atom, which stabilizes the negative charge on the conjugate base after proton donation.
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