Considering the protons highlighted in red in the two compounds shown below, which compound is more acidic. но I II O l is the stronger acid because its conjugate base is better stabilized by solvation. O lis the stronger acid because its conjugate base is stabilized by resonance. O lis the stronger acid because its conjugate base is better stabilized by solvation. O Il is the stronger acid because its conjugate base is better stabilized by inductive effects.
Considering the protons highlighted in red in the two compounds shown below, which compound is more acidic. но I II O l is the stronger acid because its conjugate base is better stabilized by solvation. O lis the stronger acid because its conjugate base is stabilized by resonance. O lis the stronger acid because its conjugate base is better stabilized by solvation. O Il is the stronger acid because its conjugate base is better stabilized by inductive effects.
General Chemistry - Standalone book (MindTap Course List)
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Chapter15: Acids And Bases
Section: Chapter Questions
Problem 15.101QP
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Transcribed Image Text:3.4 Bronsted-Lowry Acidity: Factors Affecting the Stability of Anions
Considering the protons highlighted in red in the two compounds shown below, which compound is more acidic.
HO
II
O Il is the stronger acid because its conjugate base is better stabilized by solvation.
O lis the stronger acid because its conjugate base is stabilized by resonance.
O l is the stronger acid because its conjugate base is better stabilized by solvation.
O Il is the stronger acid because its conjugate base is better stabilized by induc
e effects.
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