Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this net ionic equation. H2CO3 (aq) HS HCO3 H2S (aq) Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry acid v acid v acid v base v In this reaction: The formula for the conjugate base of H2CO3 is HCO; The formula for the conjugate acid v of HS is H,S

Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this net ionic equation. H2CO3 (aq) HS HCO3 H2S (aq) Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry acid v acid v acid v base v In this reaction: The formula for the conjugate base of H2CO3 is HCO; The formula for the conjugate acid v of HS is H,S

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 12E

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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.
Classify each of the following as a property of an Arrhenius acid or the property of an Arrhenius base. a. changes the color of blue litmus paper to red b. changes the color of red litmus paper to blue
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
Classify each of the following as a property of an Arrhenius acid or the property of an Arrhenius base. a. H as a sour taste b. H as a bitter taste
. 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)
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.
Mark each of the following statements True or False: a. The conjugate base of a strong acid is always a weak base. b. The conjugate acid of a strong base is always a weak acid. c. The stronger the acid, the weaker its conjugate base, and vice versa.
Write a formula for the conjugate base formed when each of the following behaves as a Brnsted acid: a. HSO4 b. CH3NH3+ c. HClO4 d. NH4+ e. HCl