In each row check off the boxes that apply to the highlighted reactant. reaction .2+ *(aq) + 6 NH3(aq) → Ni (NH3)2+(aq) 6 The highlighted reactant acts as a... (check all that apply) Brønsted-Lowry acid Brønsted-Lowry base HNO2(aq) + C2H3NH2(aq) → NO(aq) + C₂H₂NH(aq) N2(g) + 3 H2(g) → 2 NH3(9) Lewis acid Lewis base Brønsted-Lowry acid Brønsted-Lowry base Lewis acid Lewis base Brønsted-Lowry acid Brønsted-Lowry base Lewis acid Lewis base

In each row check off the boxes that apply to the highlighted reactant. reaction .2+ *(aq) + 6 NH3(aq) → Ni (NH3)2+(aq) 6 The highlighted reactant acts as a... (check all that apply) Brønsted-Lowry acid Brønsted-Lowry base HNO2(aq) + C2H3NH2(aq) → NO(aq) + C₂H₂NH(aq) N2(g) + 3 H2(g) → 2 NH3(9) Lewis acid Lewis base Brønsted-Lowry acid Brønsted-Lowry base Lewis acid Lewis base Brønsted-Lowry acid Brønsted-Lowry base Lewis acid Lewis base

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 88AP: . The following are representations of acid-base reactions: a. Label each of the species in both...

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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.
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?
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.
In each of the following acid-base reactions, identify the Brnsted acid and base on the left and their conjugate partners on the right. (a) HCO2H(aq) + H2O() HCO2(aq) + H3O+(aq) (b) NH3(aq) + H2S(aq) NH4+(aq) + HS(aq) (c) HSO4(aq) + OH(aq) SO42(aq) + H2O+()
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.
Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
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.
Figure 14.3 shows the pH of some common solutions. How many times more acidic or basic is each of these compared with a neutral solution? (a) Black coffee (b) Household ammonia (c) Baking soda (d) Vinegar
. 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.
In each of the following acid-base reactions, identify the Brnsted acid and base on the left and their conjugate partners on the right. (a) C2H5N(aq) + CH3CO2H(aq) C5H5NH+(aq) + CH3CO2(aq) (b) N2H4(aq) + HSO4(aq) N2H5+(aq) + SO42(aq) (c) [Al(H2O)6]3+ (aq) + OH(aq) [Al(H2O)5OH]2+ (aq) + H2O+()
What is meant by the presence of a common ion? How does the presence of a common ion affect an equilibrium such as HNO2(aq) H+(aq) + NO2-(aq) What is an acidbase solution called that contains a common ion?