None a.6. Within each pair of compounds, determine which is the appropriately stronger acid or base. Explain.don't give Aigenerated solutionStronger acid:a.HN-H orΝHStronger base:b.or

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Answered: a. 6. Within each pair of compounds,…

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter20: Acidity And Pka Of Phenols

Section: Chapter Questions

Problem 14E

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The following are equivalent ways of asking about the acidity of an H atom: • What is the most acidic H on the molecule? • Which H is associated with the published pKa value? • Which H on the molecule is easiest to remove? • Which H on the molecule takes the least energy to remove? • Which bond to an H is most polarized? • For which H atom is removal least uphill in energy? • Which bond to an H atom, when broken, results in the lowest PE conjugate base? We will often find the last of these questions is easiest to answer. To do this, find all the different Hatoms on the molecule, and draw all possible conjugate bases.Only the lowest-energy one is the “real” conjugate base. Identify this structure, and you have found the most acidic H. Use this strategy to find the most acidic H on each of the following molecules. Note: Each structure hasat least three different kinds of H’s, so draw at least three unique conjugate bases for each.
Summarize the relationship between pKa and base strength by completing the followingsentences: a. For a given base, the higher the pKa of its conjugate acid, the stronger or weaker the base. b. For a given base, the lower the pKa of its conjugate acid, the stronger or weaker the base.
Phenol (shown below) has a pKa10 . a. Based on pKa data, is phenol a stronger or weaker acid than an ordinaryalcohol (e.g.. CH3OH ) or water? b. Draw the conjugate base of phenol (called phenoxide) including allimportant resonance structures. c. Construct an explanation for why phenol is a stronger acid than anordinary alcohol. (You may want to consider first why phenoxide is lowerin PE than methoxide (RO) or hydroxide (HO) .
For the previous four questions, label each molecule that appears in the question or your answer asstrong acid, strong base, weak acid, or weak base.
Would delocalization be the best explanation possible for this compound being more acidic? I was able to choose between electronegativity, inductive effect, and Resonance ( delocalization). I choose resonance because the conjugate base could share the charge on the first compound better is this the best choice. The first compound is given to be more acidic
please explain why. .......
Arrange the follwoing in order of decreasing basicity. OH-, CH3COOH, CH3CH2-, NH2-, NH3, Cl- How would I solve this question? what concepts should I look into when comparing bascity? Thank You!!
1. In the following acid-base reactions, the mechanism of reaction is shown. (i) Label the reactants as acid and base. (ii) Draw structures of the products in the appropriate boxes for conjugate acid and conjugate base. a. b. NH₂ 0:0: 1 Conjugate acid Conjugate acid + Conjugate base Conjugate base
Compare compounds I and Il and choose the best statement from the list below. Vs. column I compound II a. The basicity of the compounds I and Il cannot be compared. b. Compound I is MORE basic than the compound II. c. Compound Il is MORE basic than the compound I. d. Both compounds have the same basicity ZI
I find the solution way too brief and unsatisfactory as it does not clearly explain the solution provided in the problem.
Which compound would be the weakest acid?
Classify each compound as a Lewis base, a Brønsted–Lowry base, both,or neither. (See in Attachment)

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a. 6. Within each pair of compounds, determine which is the appropriately stronger acid or base. Explain. don't give Ai generated solution Stronger acid: a. H N-H or Ν H Stronger base: b. or