Deck 17: Acidbase Proton Transferreactions

Question 1

Consider the following image which depicts the reactants in an acid-base reaction.Atoms other than H are labeled with the element symbol.
The products of this reaction are shown below.
Which of the following is a correct interpretation of this reaction?

A)1 is a Brønsted-Lowry acid.
B)2 is a Brønsted-Lowry base.
C)The reaction is an acid-base neutralization.
D)1 is also an Arrhenius acid.
E)All of the above are correct interpretations of this reaction.

Answer 1

All of the above are correct interpretations of this reaction.

Question 2

Which of the following is a Brønsted-Lowry base but not an Arrhenius base?

A)HSO₃^-(aq)
B)NaOH(s)
C)NH₄⁺(aq)
D)Al(OH)₃(s)
E)NH₄OH(aq)

Answer 2

HSO₃^-(aq)

Question 3

Which of the following is a Lewis acid but not a Brønsted-Lowry acid?

A)OH^-
B)HPO₄^2-
C)HCl
D)NH₄⁺
E)Fe³⁺

Answer 3

Fe³⁺

Question 4

Consider the following generalized reaction. For this reaction,which of the following is correct?

A)A is proton source.
B)B is a proton remover.
C)A is an electron pair donor.
D)B is an electron pair acceptor.
E)This a Lewis acid-base reaction.

Question 5

A Brønsted-Lowry acid is defined as a(n):

A)proton remover
B)electron source
C)proton source
D)electron pair remover
E)electron pair source

Question 6

What is the conjugate acid of HPO₄^2-(aq)?

A)H₃PO₄(aq)
B)HPO₄^2-(aq)
C)H₂PO₄^-(aq)
D)PO₄^3-(aq)
E)H₃O⁺(aq)

Question 7

Which of the following properties is traditionally associated with Arrhenius bases?

A)They cause blue litmus indicator to turn red
B)They form precipitates with solutions of most metals
C)They react with carbonates to release CO₂
D)They release hydrogen when zinc is added
E)They contain hydronium ions

Question 8

What is a Brønsted-Lowry base?

A)An electron pair source
B)A hydroxide ion source
C)A metal ion
D)A proton source
E)A proton remover

Question 9

Which pair below cannot have a Brønsted-Lowry acid base reaction between them?

A)OH^- and NH
B)PO₄^3- and ClO^-
C)HCO₃^- and SO₃^2-
D)HClO₄ and HNO₂
E)HSO₄^- and HCl

Question 10

Identify the conjugate acid base pairs in the reaction H₂SO₄ + HNO₃ → H₂NO₃⁺ + HSO₄^-.

A)H₂SO₄/HSO₄^- and H₂NO₃⁺/HNO₃
B)H₂SO₄/HNO₃ and H₂NO₃⁺/HSO₄^-
C)HNO₃/HSO₄^- and H₂SO₄/H₂NO₃⁺
D)HNO₃/NO₃^- and HSO₄^-/SO₄^2-
E)HNO₃/H₂SO₄ and H₂NO₃⁺/HSO₄^-

Question 11

Which of the following conforms to the Arrhenius definition of an acid?

A)H₂O( )
B)HBrO₃(aq)
C)HCO₃^-(aq)
D)Al³⁺(aq)
E)Mg(OH)₂(s)

Question 12

Which of the following is not capable of acting like a Brønsted-Lowry base?

A)H₂O( )
B)NH₄⁺ ion
C)Cl^- ion
D)HNO₃(aq)
E)H₂PO₄^-(aq)

Question 13

According to Arrhenius theory,what is an acid?

A)A substance that contains a high concentration of hydrogen ions in solutions with water
B)A substance that will lower the hydrogen ion concentration when placed in water
C)A substance that has an H in its formula
D)An electron pair donor
E)An electron pair acceptor

Question 14

Which of the following is a characteristic property traditionally associated with an Arrhenius acid?

A)Turns litmus indicator blue
B)Feels slippery
C)Tastes bitter
D)Sour taste
E)Contain OH^- ions

Question 15

Which of these statements is true?

A)All Brønsted-Lowry acids and bases are also Arrhenius acids and bases
B)All Lewis acids are Brønsted-Lowry acids
C)All Brønsted-Lowry acids and bases are stronger than Arrhenius acids and bases
D)All Arrhenius acids and bases are also Brønsted-Lowry acids and bases
E)There is no relationship between Brønsted-Lowry acids and bases and Lewis acids and bases

Question 16

Consider the following image which depicts the reactants in an acid-base reaction.Atoms other than H are labeled with the element symbol. The products of this reaction are shown below. Which of the following is a correct interpretation of this reaction?

A)1 and 2 are a conjugate acid-base pair.
B)3 and 4are a conjugate acid-base pair.
C)1 and 4 are a conjugate acid-base pair.
D)2 and 4 are a conjugate acid-base pair.
E)1 and 3 are a conjugate acid-base pair.

Question 17

Which of the following cannot act as a Brønsted-Lowry acid?

A)HCO₃^-(aq)
B)HOH( )
C)NH₃(g)
D)CO₃^2-(aq)
E)CH₃OH( )

Question 18

What is the conjugate base of water?

A)HCl(aq)
B)H₃O⁺(aq)
C)OH^-(aq)
D)H⁺ ion
E)H₂O( )

Question 19

Which of the following substances is amphoteric?

A)H₂O( )
B)CO₃^2- ion
C)NH₄⁺ ion
D)H₃PO₄
E)NaOH(aq)

Question 20

A substance that can act as both a proton source and a proton remover is called:

A)a Brønsted-Lowry acid
B)a Lewis acid
C)amphibious
D)amphoteric
E)neither an acid nor a base

Question 21

Given the following acid strengths: HF > H₂S > HCN,which of the following reactions is predicted to occur from left to right as written?

A)HCN(aq) + H₂S(aq) → H₃S(aq) + CN^-(aq)
B)HCN(aq) + F^-(aq) → HF(aq) + CN^-(aq)
C)HF(aq) + CN^-(aq) → HCN(aq) + F^-(aq)
D)H₂S(aq) + F^-(aq) → HF(aq) + HS^-(aq)
E)H₂S(aq) + HF(aq) → H₂F⁺(aq) + HS^-(aq)

Question 22

Consider a general comparison between acid-base and redox reactions.Which of the following is correct?

A)The acid-base analog of a reducing agent is an acid.
B)The acid-base analog of an oxidizing agent is a base.
C)The acid-base analog of electrons are protons.
D)All of the above represent correct comparisons.

Question 23

What are the [H⁺] and [OH^-] of a solution made by dissolving 0.0001 mole of HI in sufficient water to make 1.00 liter of solution?

A)[H⁺] = 4 M [OH^-] = 10 M
B)[H⁺] = 1 × 10^-14 M [OH^-] = 1 × 10^-4 M
C)[H⁺] = 1 × 10^-10 M [OH^-] = 1 × 10^-4 M
D)[H⁺] = 1 × 10^-4 M [OH^-] = 1 × 10^-14 M
E)[H⁺] = 1 × 10^-4 M [OH^-] = 1 × 10^-10 M

Question 24

A water solution is considered acidic when what is true?

A)[H⁺] = [OH^-]
B)[H⁺] < [OH^-]
C)[OH^- ] > [H⁺]
D)[H⁺] > [OH^-]
E)[H⁺] = K_w

Question 25

What is the conjugate base of ammonia?

A)NH₃(g)
B)NH₄⁺(aq)
C)NH₄OH(aq)
D)NH₂^-(aq)
E)OH^-(aq)

Question 26

The hydroxide ion concentration of a solution is 0.00001 moles per liter.What is the hydrogen ion concentration,and is the solution acidic or basic?

A)10^-10, acidic
B)10^-9, acidic
C)10^-5, acidic
D)10^-5, basic
E)10^-9, basic

Question 27

A solution is made by dissolving 0.0010 mole KOH in enough water to make 1.00 liter of solution.What are the pH and the pOH of the solution?

A)pH = 3, pOH = 11
B)pH = 3, pOH = 3
C)pH = -11, pOH = -3
D)pH = 11, pOH = 3
E)pH = 10^-11, pOH = 10^-3

Question 28

A solution has a hydroxide ion concentration of 1 × 10^-11 M.What is the pH of the solution,and is it acidic or basic?

A)pH = 11, basic
B)pH = 3, basic
C)pH = 3, acidic
D)pH = -11 acidic
E)pH = -11, basic

Question 29

What is the conjugate base of H₃C₆H₅O₇?

A)C₆H₅O₇^3-
B)H₂C₆H₅O₇^-
C)H₃C₆H₅O₇^-
D)H₄C₆H₅O₇⁺
E)H₃C₆H₅O₇(OH)^-

Question 30

Which of the following solutions is most acidic?

A)[H⁺] = 1 × 10^-4
B)[H⁺] = 1 × 10^-14
C)[OH^-] = 1 × 10^-3
D)pH = 10
E)pOH = 12

Question 31

Which is the correct net ionic equation for the reaction between HC₂O₄^- and HPO₄^2-? (Note:
H₂C₂O₄ is a stronger acid than H₂PO₄^-.)

A)HC₂O₄^- + HPO₄^2- H⁺ + H₂O₄^2- + HPO₄^2-
B)HC₂O₄^- + HPO₄^2- H⁺ + HC₂O₄^- + PO₄^3-
C)HC₂O₄^- + HPO₄^2- C₂O₄^2- + H₂PO₄^-
D)HC₂O₄^- + HPO₄^2- H₂C₂O₄ + PO₄^3-
E)HC₂O₄^- + HPO₄^2- H₂ + C₂O₄^2- + PO₄^3-

Question 32

A pH meter is used to test the pH of a solution.See the figure below. How is the solution classified?

A)neutral
B)acidic
C)basic

Question 33

The hydrogen ion concentration of a solution is 1 × 10^-4 M.What is the pH of the solution,and is it acidic or basic?

A)pH = 10, acidic
B)pH = 10, basic
C)pH =13, basic
D)pH = -4, basic
E)pH = 4, acidic

Question 34

Which of the following statements is incorrect ?
i.K_w = [H⁺][OH^-] = 1.0 × 10^-14 at 25°C.
ii.Water or water solutions in which [H⁺] = [OH^-] = 10^-7 M are neutral solutions,neither acidic nor basic.
iii.A solution in which [H⁺] > [OH^-] is basic
iv.A solution in which [OH^- ] > [H⁺] is acidic

A)i and ii
B)iii and iv
C)ii, iii, and iv
D)All statements are correct
E)All statements are incorrect

Question 35

Given the following relative acid strengths,starting with the weakest: HCO₃^- < HNO₃ < HBr,what is the relative strength of each conjugate base,starting with the weakest?

A)CO₃^2- < NO₃^- < Br^-
B)Br^- < CO₃^2- < NO₃^-
C)NO₃^- < Br^- < CO₃^2-
D)Br^- < NO₃^-< CO₃^2-
E)CO₃^2- < Br^- < NO₃^-

Question 36

What is the hydroxide ion concentration in a solution with pH = 3?

A)10^-3 M
B)11 M
C)10^-11 M
D)3 M
E)10¹¹ M

Question 37

Given the following relative base strengths,starting with the weakest:
HSO₃^- < F^- < C₂H₃O₂^-,what is the relative strength of each conjugate acid,starting with the weakest?

A)HC₂H₃O₂ < HF < H₂SO₃
B)HC₂H₃O₂ < H₂SO₃ < HF
C)H₂SO₃ < HF < HC₂H₃O₂
D)H₂SO₃ < HC₂H₃O₂ < HF
E)HF < H₂SO₃ < HC₂H₃O₂

Question 38

Which of the following statements is incorrect?

A)Acid-base reactions involve a transfer of protons; redox reactions, a transfer of electrons
B)In both redox and acid-base reactions, the reactants are given special names to indicate their roles in the transfer process
C)Just as certain species can either donate or accept protons and thereby behave as an acid in one reaction and a base in another, certain species can either accept or donate electrons, acting as an oxidizing agent in one reaction and a reducing agent in another
D)Just as acids and bases may be classified as "strong" or "weak" depending on how readily they donate or accept protons, the strengths of oxidizing and reducing agents may be compared according to their tendencies to attract or release electrons
E)Unlike most acid-base reactions in solution, which reach a state of equilibrium, most aqueous redox reactions do not reach a state of equilibrium and proceed entirely either in the forward or reverse direction

Question 39

Which of the following is the correct net ionic equation for the reaction between nitrous acid and hydrogen sulfide ion?

A)HNO₂ + HS^- H₂NO₂⁺ + S^2-
B)HNO₂ + HS^- NO₂^- + H₂S
C)HNO₂ + HSO₄^- H₂NO₂⁺ + SO₄^2-
D)HNO₂ + HSO₄^- NO₂^- + H₂SO₄
E)HNO₃ + HSO₄^- NO₃^- + H₂SO₄

Question 40

In Brønsted-Lowry acid-base reactions,which of the following species are favored at equilibrium?

A)The weaker acid and the weaker base
B)The weaker acid and the stronger base
C)The stronger acid and the weaker base
D)The stronger acid and the stronger base
E)At equilibrium, neither side is favored

Question 41

Consider the following image. Based on the reading,what is the hydrogen ion concentration in this solution?

A)0.100 M
B)0.00010 M
C)1.0 × 10^-10 M
D)zero
E)10.00 M

Question 42

What is the pH of a solution if [H⁺] = 3.1 × 10^-4 molar?

A)pH = 4.31
B)pH = 10.49
C)pH = -9.69
D)pH = -3.51
E)pH = 3.51

Question 43

A solution is made by dissolving 12.50 g of NaOH,a strong base,in water to produce 2.0 liters of solution.What is the pH of this solution?

A)13.50
B)13.19
C)11.74
D)0.81
E)0.31

Question 44

The pH of a solution is 5.330.Find [OH^-].

A)[OH^-] = 2.14 × 10^-9 molar
B)[OH^-] = 4.70 × 10^-11 molar
C)[OH^-] = 5.33 × 10^-7 molar
D)[OH^-] = 4.70 × 10^-6 molar
E)[OH^-] = 5.33 molar

Question 45

What is the hydrogen ion concentration in a solution with pH = 11.27? Is the solution acidic or basic?

A)5.4 × 10^-12 M basic
B)1.86 × 10^-3 M basic
C)5.37 × 10^-12 M acidic
D)1.86 × 10^-3 M acidic
E)2.73 M acidic