Consider two acids: HCO,H (formic acid, pKa = 3.8) and pivalic acid [(CH3)3CCO2H, pKa = 5.0]. (a) Which acid has the larger K,? (b) Which acid is the stronger acid? (c) Which acid forms the stronger conjugate base? (d) When each acid is dissolved in water, for which acid does the equilibrium lie further to the right?

Consider two acids: HCO,H (formic acid, pKa = 3.8) and pivalic acid [(CH3)3CCO2H, pKa = 5.0]. (a) Which acid has the larger K,? (b) Which acid is the stronger acid? (c) Which acid forms the stronger conjugate base? (d) When each acid is dissolved in water, for which acid does the equilibrium lie further to the right?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 38QAP: Consider these acids (a) Arrange the acids in order of increasing acid strength from weakest to...

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The following reactions illustrate Brnsted acid-base behavior. Complete each equation. a.HI(aq)+?H3O+(aq)+I(aq) b.NH3(l)+?NH4++NH2 c.H2C2O4(aq)+H2O(l)?+HC2O4(aq) d.H2N2O2(aq)+H2O(l)H3O+(aq)+? e.?+H2O(l)H3O+(aq)+CO32(aq)
1. Which of the following can act as a Lewis acid? (Hint : In each case, draw the Lewis electron dot structure of the molecule or ion. Are there lone pairs of electrons on the central atom? If so, it can be a Lewis base. Does the central atom lack an electron pair? If so, it can behave as a Lewis acid.) PH3 BCl3 H2S HS−
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
How do the components of a conjugate acid—base pair differ from one another4? Give an example of a conjugate acid—base pair to illustrate your answer.
Trimethylamine, (CH3)3N, reacts readily with diborane, B2H6. The diborane dissociates to two BH3 fragments, each of which can react with trimethylamine to form a complex, (CH3)3N:BH3. Write an equation for this reaction and interpret it in terms of Lewis acid-base theory.
Gastric juice, the digestive ?uid produced in the stomach, contains hydrochloric acid, HCl, Milk of Magnesia, a suspension of solid Mg(OH)2 in an aqueous medium, is sometimes used to neutralize-excess stomach acid. Write a complete balanced equation for the neutralization reaction, and identify the conjugate acid—base pairs.
Following is a structural formula for imidazole, a building block of the essential amino acid histidine (Chapter 27). It is also a building block of histamine, a compound all too familiar to people with allergies and takers of antihistamines. When imidazole is dissolved in water, proton transfer to it gives a cation. Is this cation better represented by structure A or B? Explain.
Which of the following compounds or ions has the weakest conjugate base? Briefly explain your choice. a) HCN b) HClO c) NH4+
Consider these acids (a) Arrange the acids in order of increasing acid strength from weakest to strongest. (b) Which acid has the smallest pKa value?
Hypofluorous acid, HOF, is known, but fluorous acid, HOFO, is not. Which acid would you expect to be stronger?
Pure liquid ammonia ionizes in a manner similar to that of water. (a) Write the equilibrium for the autoionization of liquid ammonia. (b) Identify the conjugate acid form and the base form of the solvent. (c) Is NaNH2 an acid or a base in this solvent? (d) Is ammonium bromide an acid or a base in this solvent?
Coal and other fossil fuels usually contain sulfur compounds that produce sulfur dioxide, SO2, when burned. One possible way to remove the sulfur dioxide is to pass the combustion gases into a tower packed with calcium oxide, CaO. Write the equation for the reaction. Identify each reactant as either a Lewis acid or a Lewis base. Explain how you arrived at your answer.

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