Choose the true statement concerning the relative acid strengths of H₂SO₄ and H₂SO_3. A) H₂SO₄ is a stronger acid than H₂SO₃ because the S in H₂SO₄ has a more positive oxidation state than the S in H₂SO₃ which influences the polarity of the O-H bonds. B) H₂SO₄ is a weaker acid than H₂SO₃ because the S in H₂SO₄ has a more positive oxidation state than the S in H₂SO₃ which influences the polarity of the O-H bonds. C) H₂SO₄ is a stronger acid than H₂SO₃ because the S in H₂SO₄ has a less positive oxidation state than the S in H₂SO₃ which influences the polarity of the O-H bonds. D) H₂SO₄ is a weaker acid than H₂SO₃ because the S in H₂SO₄ has a more negative oxidation state than the S in H₂SO₃ which influences the polarity of the O-H bonds.

Question

Quizplus · Accepted Answer

The oxidation state of sulfur (S) affects the acidity of the compound. A higher oxidation state of sulfur increases the compound's ability to stabilize the negative charge on the conjugate base after deprotonation, making H₂SO₄ (with sulfur in a higher oxidation state) a stronger acid than H₂SO₃.

Choose the True Statement Concerning the Relative Acid Strengths of H2SO4

Choose the True Statement Concerning the Relative Acid Strengths of H₂SO₄