[Review Topics][References]Use the References to access important values if needed for this questionIdentify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this net ionic equation.H,SO3 (aq)HSHSO,H,S (aq)Bronsted-LowryBronsted-LowryBrønsted-LowryBrønsted-LowryIn this reaction:The formula for the conjugateMof H,SO3 isThe formula for the conjugateof HS isSubmit AnswerRetry Entire Group9 more group attempts remainingCengage Learning Cengage Technical Support98°F Rain coming

The reaction given is, => H2SO3 (aq) + HS- (aq) ⇔HSO3- (aq) + HS (aq)

Answered: Identify whether each species functions…

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter18: Acids And Bases

Section: Chapter Questions

Problem 105A

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Define each of the following: a. Arrhenius acid b. BronstedLowry acid c. Lewis acid Which of the definitions is most general? Write reactions to justify your answer.
a Write a net ionic equation to show that hypochlorous acid behaves as a Brnsted-Lowry acid in water. b The substance triethanolamine is a weak nitrogen-containing base, like ammonia. Write a net ionic equation to show that triethanolamine, C6H15O3N, behaves as a Brnsted-Lowry base in water.
In the following net ionic reaction, identify each species as either a Brnsted-Lowry acid or a Brnsted -Lowry base: CH3COO(aq)+HS(aq)CH3COOH(aq)+S2(aq). Identify the conjugate of each reactant and state whether it is a conjugate acid or a conjugate base.
Define each of the following: a. Arrhenius acid b. BronstedLowry acid c. Lewis acid Which of the definitions is most general? Write reactions to justify your answer.
The sec-butyl cation can react as both a Brnsted-Lowry acid (a proton donor) and a Lewis acid (an electron pair acceptor) in the presence of a watersulfuric acid mixture. In each case, however, the product is different. The two reactions are as follows: (a) In which reaction(s) does this cation react as a Lewis acid? In which reaction(s) does it react as a Brnsted-Lowry acid? (b) Write Lewis structures for reactants and products and show by the use of curved arrows how each reaction occurs.
Identify and label the Bronsted-Lowry acid, its conjugate base, the Bronsted—Lowry base, and its conjugate acid in each of the following equations: (a) HNO3+H2OH3O++NO3 (b) CN+H2OHCN+OH (c) H2SO4+CIHCI+HSO4 (d) HSO4+OHSO42+H2O (e) O2+H2O2OH (f) [Cu( H 2 O)3(OH)]++[Al( H 2 O)6]3+[Cu( H 2 O)4]2++[Al( H 2 O)5(OH)]2+ (g) H2S+NH2HS+NH3
. The following are representations of acid-base reactions: a. Label each of the species in both equations as an acid or base, and explain. b. For those species that are acids, which labels apply: Arrhenius acid, Brønsted-Lowry acid? What about the bases?
When perchloric acid ionizes, it makes the perchlorate ion, ClO4. Draw the Lewis electron dot symbol for the perchlorate ion.
Write a brief description of the relationships among each of the following groups of terms or phrases. Answers to the Concept-Linking Exercises are given at the end of the chapter. Terms from optional sections 17.1 and 17.3 are in italics. Exercise 11 covers terms related to logarithms, and it is also optional. Arrhenius acid, Brnsted-Lowry acid, Lewis acid
. 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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