Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this net ionic equation. HCN (aq) HCO3 H2CO3 (aq) CN- Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry In this reaction: The formula for the conjugate v of CN is | The formula for the conjugate v of H2CO3 is

Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this net ionic equation. HCN (aq) HCO3 H2CO3 (aq) CN- Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry In this reaction: The formula for the conjugate v of CN is | The formula for the conjugate v of H2CO3 is

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter17: Acid-base(proton Transfer) Reactions

Section: Chapter Questions

Problem 17.2TC

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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) NO2+H2OHNO2+OH (b) HBR+H2OH3O++Br (c) HS-+H2OH2S+OH (d) H2PO4+OHHPO42+H2O (e) H2PO4+HClH3PO4+Cl (f) [Fe( H 2 O)5(OH)]2++[Al( H 2 O)6]3+[Fe( H 2 O)6]3++[Al( H 2 O)5(OH)]2+ (g) CH3OH+HCH3O+H2
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.
Classify each of the following statements as true or false: aAll Brnsted-Lowry acids are Arrhenius acids. bAll Arrhenius bases are Brnsted-Lowry bases, but not all Brnsted-Lowry bases are Arrhenius bases. c HCO3 is capable of being amphoteric. d HS is the conjugate base of S2. eIf the species on the right side of an ionization equilibrium are present in greater abundance than those on the left, the equilibrium is favored in the forward direction. f NH4+ cannot act as a Lewis base. gWeak bases have a weak attraction for protons. hThe stronger acid and the stronger base are always on the same side of a proton transfer reaction equation. iA proton transfer reaction is always favored in the direction that yields the stronger acid. jA solution with pH=9 is more acidic than one with pH=4. kA solution with pH=3 is twice as acidic as one with pH=6. lA pOH of 4.65 expresses the hydroxide ion concentration of a solution in three significant figures.
. a. Write the conjugate acid for each of the following Brønsted-Lowry bases. NO3.HSO4,ClO4,NH3,HCO3b. Write the conjugate base for each of the following Brønsted- Lowry acids. HCI,H2SO4,NH3,NH4,HCO3
Write the acid ionization constant expression for the ionization of each of the following monoprotic acids. a. HF (hydrofluoric acid) b. HC2H3O2 (acetic 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.
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.
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.
. In each of the following chemical equations, identify the conjugate acid-base pairs. a. NH3(aq)+H2O(l)NH4+(aq)+OH(aq) b. PO43(aq)+H2O(1)HPO42(aq)+OH(aq) c. C2H3O2(aq)+H2O(l)HC2H3O2(aq)+OH(aq)