Which of the acids in the table above has the strongest conjugate base? Your answer Acidities of Substituted Benzoic and Acetic Acids pks at 25°C Y Y Y CH₂COOT meta H 4.75 4.19 CN 2.47 3.64 OCH, 3.57 4.09 What is the structure of the strongest acid in the table above? Your answer CH₂COOH para 4.19 3.55 4.46

Which of the acids in the table above has the strongest conjugate base? Your answer Acidities of Substituted Benzoic and Acetic Acids pks at 25°C Y Y Y CH₂COOT meta H 4.75 4.19 CN 2.47 3.64 OCH, 3.57 4.09 What is the structure of the strongest acid in the table above? Your answer CH₂COOH para 4.19 3.55 4.46

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 48E: You may need Table 13-2 to answer the following questions. a. Which is the stronger base, Cl or H2O?...

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Several acids and their respective equilibrium constants are: Which is the strongest acid? Which is the weakest acid? Which acid has the weakest conjugate base? Which acid has the strongest conjugate base?
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Define or illustrate the meaning of the following terms: a. Ka reaction b. Ka equilibrium constant c. Kb reaction d. Kb equilibrium constant e. conjugate acidbase pair
In each of the following acid-base reactions, identify the Brnsted acid and base on the left and their conjugate partners on the right. (a) C2H5N(aq) + CH3CO2H(aq) C5H5NH+(aq) + CH3CO2(aq) (b) N2H4(aq) + HSO4(aq) N2H5+(aq) + SO42(aq) (c) [Al(H2O)6]3+ (aq) + OH(aq) [Al(H2O)5OH]2+ (aq) + H2O+()
Consider the following four biological solutions: (1) bile, pH 8.0, (2) blood, pH 7.4, (3) urine, pH 6.0, and (4) gastric juice, pH 1.6. a. Which solution has the lowest [H3O+]? b. Which solution has the lowest [OH]? c. List the solutions in order of decreasing acidity. d. List the solutions in order of increasing basicity.
Place the species in each of the following groups in order of increasing acid strength. a. H2O, H2S, H2Se (bond energies: HO, 467 kJ/mol; HS, 363 kJ/mol; HSe, 276 kJ/mol) b. CH3CO2H, FCH2CO2H, F2CHCO2H, F3CCO2H c. NH4+, HONH3+ d. NH4+, PH4+ (bond energies: NH, 391 kJ/mol; PH, 322 kJ/mol) Give reasons for the orders you chose.
Predict the position of equilibrium for this acid-base reaction.
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Acid-Base Equilibria Many factors contribute to the acidity of organic compounds. Electronegativity, resonance, induction, hybridization, aromaticity, and atomic size, all play a role. In the following comparisons, you are asked to identify the factor(s) that would be most important to analyze when predicting relative acidity, and then to predict the trend in acidity and pKa values. For each of the following pairs of compounds answer the following two multiple-choice questions. 1. What factor(s) are the most important to consider when predicting the relative acidity of the two compounds? a. Electronegativity of the atom possessing the hydrogen. b. Resonance stabilization of the anionic conjugate base. c. Inductive stabilization of the anionic conjugate base. d. Hybridization of the atom possessing the hydrogen. e. The atomic size of the atom possessing the hydrogen.
You may need Table 13-2 to answer the following questions. a. Which is the stronger base, Cl or H2O? b. Which is the stronger base, H2O or NO2? c. Which is the stronger base, CNor OC6H5?