Open Question
The viscosity of liquid sulfur increases sharply at about 160 °C and then decreases again above 200 °C. Explain.
Ch.22 - The Main Group Elements
Chapter 22, Problem 138a
Account for each of the following observations.
(a) H2SO4 is a stronger acid than H2SO3.
Verified step by step guidance1
Understand the concept of acid strength: Acid strength is determined by the ability of an acid to donate protons (H+ ions) in solution. A stronger acid will dissociate more completely in water, releasing more H+ ions.
Compare the structures of H2SO4 and H2SO3: H2SO4 (sulfuric acid) has two hydroxyl groups (OH) and two double-bonded oxygens, while H2SO3 (sulfurous acid) has two hydroxyl groups and one double-bonded oxygen.
Consider the role of electronegativity and resonance: The presence of more electronegative oxygen atoms in H2SO4 allows for greater stabilization of the negative charge on the conjugate base (HSO4-) through resonance, compared to H2SO3.
Evaluate the stability of the conjugate bases: The conjugate base of H2SO4 (HSO4-) is more stable than the conjugate base of H2SO3 (HSO3-) due to the additional resonance stabilization provided by the extra oxygen atom in H2SO4.
Conclude based on the stability of conjugate bases: Since H2SO4 has a more stable conjugate base than H2SO3, it is a stronger acid, as the stability of the conjugate base is a key factor in determining acid strength.
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Open Question
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