www que predominan son In equilibrium the predominant species are 요 CH3COH Acetic acid PK 4.76 + HCO3 Bicarbonate ion A. ácido acético e ión bicarbonato acetic acid and bicarbonate ion B. ión acetato y ácido acético acetate ion and acetic acid OC. ión acetato y ácido carbónico acetate ion and carbonic acid OD. ácido carbónico e ión bicarbonato carbonic acid and bicarbonate ion - CH3CO + Acetate ion H₂CO3 Carbonic acid pK, 6.36

www que predominan son In equilibrium the predominant species are 요 CH3COH Acetic acid PK 4.76 + HCO3 Bicarbonate ion A. ácido acético e ión bicarbonato acetic acid and bicarbonate ion B. ión acetato y ácido acético acetate ion and acetic acid OC. ión acetato y ácido carbónico acetate ion and carbonic acid OD. ácido carbónico e ión bicarbonato carbonic acid and bicarbonate ion - CH3CO + Acetate ion H₂CO3 Carbonic acid pK, 6.36

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.65PAE

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8-87 The pKavalue of barbituric acid is 5.0. If the H3O+ and barbiturate ion concentrations are each 0.0030 M, what is the concentration of the undissociated barbituric acid?
For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)
. The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in aqueous solutions, water is the solvent and is intimately involved in the equilibria). However, the Brønsted-Lowry acid-base theory can be extended easily to other solvents. One such solvent that has been investigated in depth is liquid ammonia. NH3. a. Write a chemical equation indicating how HCl behaves as an acid in liquid ammonia. b. Write a chemical equation indicating how OH- behaves as a base in liquid ammonia.
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For each of the following reactions, predict whether the equilibrium lies predominantly to the left or to the right. Explain your predictions briefly. (a) H2S(aq) + CO32(aq) HS(aq) + HCO3(aq) (b) HCN(aq) + SO42(aq) CN(aq) + HSO4(aq) (c) SO42(aq) + CH3CO2H(aq) HSO4(aq) + CH3CO2(aq)
What are the products of each of the following acid-base reactions? Indicate the acid and its conjugate base and the base and its conjugate acid. HC1O4+ H2O — NH/ + H2O -» HCOr + OH" —
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
Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?