Deck 15: Acids and Bases

Question 1

In the reaction
CuO(s)+ CO₂(g)→ CuCO₃(s),

A)O^2- acts as a Lewis base and CO₂ acts as a Lewis acid.
B)O^2- acts as a Lewis base and Cu²⁺ acts as a Lewis acid.
C)CuO is the Lewis acid and CuCO₃ is its conjugate base.
D)CO₂ is the Lewis acid and CuCO₃ is its conjugate base.
E)Cu²⁺ acts as a Lewis acid and CO₃^2- acts as a Lewis base.

Answer 1

O^2- acts as a Lewis base and CO₂ acts as a Lewis acid.

Question 2

Which of the following statements is correct concerning the neutralization of sulfurous acid by a strong base?
2OH^-(aq)+ H₂SO₃(aq)→ SO₃^2-(aq)+ 2H₂O(l)

A)H₂SO₃ is both an Arrhenius acid and a Brønsted-Lowry acid.
B)H₂SO₃ is a Brønsted-Lowry acid,but not an Arrhenius acid.
C)H₂SO₃ is neither an Arrhenius acid nor a Brønsted-Lowry acid.
D)H₂SO₃ is an Arrhenius acid,but not a Brønsted-Lowry acid.
E)H₂SO₃ is a Lewis base.

Answer 2

H₂SO₃ is both an Arrhenius acid and a Brønsted-Lowry acid.

Question 3

Which of the following species is not capable of acting as an Arrhenius acid in aqueous solution?

A)ClO₄^-
B)HClO₃
C)H₂SO₃
D)H₃PO₄
E)HSO₄^-

Answer 3

ClO₄^-

Question 4

Which acid has the strongest conjugate base in aqueous solution?

A)HF
B)HNO₃
C)HClO₄
D)HI
E)H₂SO₄

Question 5

Which of the following species cannot act as a Lewis base?

A)NH₃
B)NH₄⁺
C)N^3-
D)NH₂^-
E)NH^2-

Question 6

What is a conjugate acid-base pair for the following equilibrium?
H₂O(l)+ NH₄⁺(aq)
NH₃(aq)+ H₃O⁺(aq)

A)H₂O is an acid and NH₃ is its conjugate base.
B)H₂O is an acid and H₃O⁺ is its conjugate base.
C)NH₄⁺ is an acid and NH₃ is its conjugate base.
D)H₂O is a base and NH₃ is its conjugate acid.
E)H₂O is a base and NH₄⁺ is its conjugate acid.

Question 7

Which are the Brønsted-Lowry bases in the following equilibrium?
HCOO^-(aq)+ H₂O(l)
HCOOH(aq)+ OH^-(aq)

A)HCOO^- and OH^-
B)H₂O and OH^-
C)H₂O,HCOOH,and OH^-
D)HCOO^- and HCOOH
E)H₂O and HCOOH

Question 8

Which of the following species cannot act as a Lewis base?

A)H₂O₂
B)OH^-
C)O^2-
D)H₂O
E)Be²⁺

Question 9

Which of the following species is not capable of acting as an Arrhenius acid in aqueous solution?

A)CH₄
B)​HSO₃^-
C)H₂SO₃
D)H₃O⁺
E)HCl

Question 10

Which of the following pairs of species is not a conjugate acid-base pair?

A)HOCl,OCl^-
B)HNO₂,NO₂⁺
C)O^2-,OH^-
D)HSO₄^-,SO₄^2-
E)H₂CO₃,HCO₃^-

Question 11

Which of the following is not an example of an acid-base reaction?

A)Al(OH)₃(s)+ 3H⁺(aq)→→ Al³⁺(aq)+ 3H₂O(l)
B)C₂H₆(g)→ →→→→→C₂H₄(g)+ H₂(g)
C)MgO(s)+ CO₂(g)→→ MgCO₃(s)
D)Al(OH)₃(s)+ OH^-(aq)→→→→→ Al(OH)₄^-(aq)
E)CN^-(aq)+ H₂O(l) HCN(aq)+ OH^-(aq)

Question 12

Consider the following reaction:
AgBr(s)+ 2CN^-(aq)→ Ag(CN)₂^-(aq)+ Br^-(aq)
The species that are acting as a Lewis acid and Lewis base,respectively,are

A)Br^- and CN^-.
B)Ag⁺ and CN^-.
C)AgBr and Ag(CN)₂^-.
D)Ag(CN)₂^- and Ag⁺.
E)Ag⁺ and Br^-.

Question 13

What is a conjugate acid-base pair for the following equilibrium?
H₂O(l)+ HPO₄^2-(aq)
H₂PO₄^-(aq)+ OH^-(aq)

A)H₂O is an acid and HPO₄^2- is its conjugate base.
B)HPO₄^2- is an acid and OH^- is its conjugate base.
C)H₂O is an acid and OH^- is its conjugate base.
D)HPO₄^2- is an acid and H₂PO₄^- is its conjugate base.
E)HPO₄^2- is an acid and H₂O is its conjugate base.

Question 14

What is the conjugate base of H₂PO₄^-(aq)?

A)PO₄^3-
B)H₃O⁺
C)HPO₄^2-
D)H₃P
E)H₃PO₄

Question 15

Which of the following species is amphiprotic in aqueous solution?

A)CH₃NH₂
B)H₃O⁺
C)NH₄⁺
D)F−
E)HSO₄-

Question 16

Which of the following species cannot act as a Lewis acid?

A)H⁺
B)H^-
C)K⁺
D)Mg²⁺
E)Al³⁺

Question 17

Which of the following species cannot act as a Lewis acid?

A)BeCl₂
B)H⁺
C)Ag⁺
D)BF₃
E)NH₄⁺

Question 18

Which of the following reactions is not readily explained by the Arrhenius concept of acids and bases?

A)HCl(g)+ NH₃(g)→ NH₄Cl(s)
B)HCl(aq)+ NaOH(aq)→ NaCl(aq)+ H₂O(l)
C)HClO₄(aq)+ H₂O(l)→ H₃O⁺(aq)+ ClO₄−(aq)
D)HC₂H₃O₂(aq)+ H₂O(l) H₃O⁺(aq)+ C₂H₃O₂−(aq)
E)H₃O⁺(aq)+ OH−(aq)→ 2H₂O(l)

Question 19

Which of the following statements does not describe a characteristic of an Arrhenius acid?

A)An Arrhenius acid reacts with an Arrhenius base to produce a salt.
B)An Arrhenius acid turns red litmus blue.
C)An Arrhenius acid is an electrolyte.
D)An Arrhenius acid reacts with CaCO₃ to produce CO₂.
E)An Arrhenius acid tastes sour.

Question 20

Which of the following species cannot act as a Lewis base?

A)H₂S
B)S^2-
C)Al³⁺
D)SH^-
E)H₂O

Question 21

What is the equilibrium concentration of amide ion (NH₂^-)in liquid ammonia at 25°C? ("am" = dissolved in ammonia)
2NH₃(l)
NH₄⁺(am)+ NH₂^-(am); K_c = 1.8 × 10^-24 at 25°C

A)2.6 × 10^-12 M
B)3.6 × 10^-24 M
C)1.3 × 10^-12 M
D)1.8 × 10^-24 M
E)9.0 × 10^-25 M

Question 22

Given equal concentrations of the following acids,which exhibits the greatest amount of ionization in water?

A)acetic acid
B)sulfurous acid
C)citric acid
D)perchloric acid
E)hypochlorous acid

Question 23

Which solution has the highest pH?

A)0.10 M HBr(aq)
B)0.10 M HI(aq)
C)0.10 M HF(aq)
D)0.10 M HCl(aq)
E)0.10 M HClO₄(aq)

Question 24

Which of the following statements is true concerning an aqueous solution of the weak base NH₃?

A)OH^- is a stronger base than NH₃.
B)OH^- is a stronger acid than NH₄⁺.
C)NH₄⁺ is a stronger acid than H₃O⁺.
D)NH₃ is a weaker base than H₂O.
E)H₂O is a stronger acid than H₃O⁺.

Question 25

Which of the following is the strongest acid?

A)HClO₂
B)HCl
C)HClO₄
D)HClO
E)HClO₃

Question 26

Which of the following is the strongest acid in aqueous solution?

A)H₃AsO₄
B)H₃PO₄
C)H₃PO₃
D)H₃SbO₄
E)H₃AsO₃

Question 27

Rank the following in order of decreasing acid strength in aqueous solution: HBr,HOCl,HOBr,HOI.

A)HBr > HClO > HBrO > HIO
B)HIO > HBrO > HClO > HBr
C)HBr > HIO > HBrO > HClO
D)HClO > HBr > HBrO > HIO
E)HClO > HBrO > HBr > HIO

Question 28

Rank H₃PO₄,H₂PO₄^-,and HPO₄^2- in order of increasing acid strength.

A)HPO₄^2- < H₂PO₄^- < H₃PO₄
B)H₂PO₄^- < HPO₄^2- < H₃PO₄
C)H₂PO₄^- < H₃PO₄ < HPO₄^2-
D)HPO₄^2- < H₃PO₄ < H₂PO₄^-
E)H₃PO₄ < H₂PO₄^- < HPO₄^2-

Question 29

Which of the following acids has the weakest conjugate base in aqueous solution?

A)CH₃COOH
B)HOCl
C)HF
D)HNO₂
E)HNO₃

Question 30

Which of the following statements is true concerning an aqueous solution of the strong acid HBr?

A)Br^- is a stronger acid than H₂O.
B)Br^- is a stronger base than OH^-.
C)H₃O⁺ is a stronger acid than HBr.
D)H₂O is a stronger acid than HBr.
E)H₂O is a stronger base than Br^-.

Question 31

The autoionization of water,as represented by the equation below,is known to be endothermic.Which of the following correctly states what occurs as the temperature of water is raised?
H₂O(l)+ H₂O(l)
H₃O⁺(aq)+ OH^-(aq)

A)The pH of the water decreases,and the water becomes more acidic.
B)The pH of the water decreases,and the water remains neutral.
C)The pH of the water increases,and the water remains neutral.
D)The pH of the water does not change,and the water remains neutral.
E)The pH of the water increases,and the water becomes more acidic.

Question 32

Which of the following reactions is not product-favored?

A)NaOH(aq)→ Na⁺(aq)+ OH^-(aq)
B)NH₃(aq)+ H₂O(l)→ NH₄⁺(aq)+ OH^-(aq)
C)HClO₄(aq)+ H₂O(l)→ H₃O⁺(aq)+ ClO₄^-(aq)
D)HCl(aq)+ H₂O(l)→ H₃O⁺(aq)+ Cl^-(aq)
E)H₂SO₄(aq)+ H₂O(l)→ H₃O⁺(aq)+ HSO₄^-(aq)

Question 33

Which of the following acids has the strongest conjugate base?

A)HClO
B)HClO₄
C)HClO₂
D)HClO₃
E)HCl

Question 34

The ionization constant of water at a temperature above 25°C is 3.5 × 10^-14.What is the pH of pure water at this temperature?
2H₂O(l)
H₃O⁺(aq)+ OH^-(aq)

A)7.73
B)5.53
C)6.73
D)13.49
E)7.00

Question 35

What is the leveling effect?

A)All bases are 100% ionized in water.
B)All acids are 100% ionized in solvents other than water.
C)All strong acids are 100% ionized in water.
D)An acid with a higher concentration in water has a lower pH than an acid with a lower concentration in water.
E)A base with a higher concentration in water has a lower pH than a base with a lower concentration in water.

Question 36

Rank the following in order of decreasing acid strength: H₂O,H₂S,H₂Se,H₂Te

A)H₂Te > H₂Se > H₂S > H₂O
B)H₂O > H₂S > H₂Se > H₂Te
C)H₂Se > H₂Te > H₂S > H₂O
D)H₂S > H₂Te > H₂Se > H₂O
E)H₂Se > H₂S > H₂Te > H₂O

Question 37

Which of the following solutes,dissolved in 1.0 kg of water,would be expected to provide the fewest particles and to freeze at the highest temperature?

A)0.10 mol HClO
B)0.10 mol HClO₃
C)0.10 mol HClO₂
D)0.10 mol HClO₄
E)0.10 mol HCl

Question 38

The equilibrium constant for the autonionization of water (shown below)increases with increasing temperature,from 1.01 x10^-14 at 25°C to 5.31 x10^-14 at 50°C.
H₂O(l)+ H₂O(l)
H₃O⁺(aq)+ OH^-(aq)
Which of the following statements is consistent with this behaviour?

A)The autoionization of water is an endothermic reaction.
B)The autoionization of water is an exothermic reaction.
C)The hydronium ion concentration at equilibrium increases with increasing temperature.
D)The hydronium ion concentration at equilibrium decreases with increasing temperature.
E)Both A and C.

Question 39

Which of the following statements is incorrect?

A)One reason why HCl is a stronger acid than HF is that the H-Cl bond is weaker than the H-F bond.
B)F^- is a stronger base than Cl^-.
C)One reason why HCl is a stronger acid than HF is that Cl is more electronegative than F.
D)The acids HBr and HI both appear equally strong in water.
E)One reason why HCl is a stronger acid than HF is that Cl has a larger atomic radius than F.

Question 40

The acid strength decreases in the series HBr > HSO₄^- > CH₃COOH > HCN > HCO₃^-.Which of the following is the strongest base?

A)SO₄^2-
B)CO₃^2-
C)CH₃COO^-
D)Br^-
E)CN^-

Question 41

What is the pH of a 0.072 M HClO₄ solution?

A)15.14
B)2.63
C)12.86
D)1.14
E)11.37

Question 42

The concentration of H₃O⁺ in a solution is 6 × 10^-4 M at 25°C.What is its hydroxide-ion concentration?

A)6 × 10^-4 M
B)1 × 10^-10 M
C)2 × 10^-10 M
D)3 × 10^-10 M
E)2 × 10^-11 M

Question 43

What is the pOH of a 0.011 M HI solution?

A)4.51
B)12.04
C)9.49
D)15.96
E)1.96

Question 44

What is the pH of the final solution when 25 mL of 0.023 M HCl has been added to 35 mL of 0.040 M HCl at 25°C?

A)3.22
B)1.81
C)1.48
D)2.70
E)3.41

Question 45

At 10°C,the ion-product constant of water,K_w,is 6.88 × 10^-15.What is the pH of pure water at 10°C?

A)7.000
B)6.684
C)7.364
D)7.264
E)none of these

Question 46

What is the hydronium-ion concentration of a 0.0041 M LiOH solution?

A)2.4 × 10^-12 M
B)4.1 × 10^-3 M
C)1.0 × 10^-14 M
D)1.0 × 10^-7 M
E)4.1 × 10^-17 M

Question 47

What is the hydronium-ion concentration of a 0.0017 M Ba(OH)₂ solution?

A)3.4 × 10^-3 M
B)1.7 × 10^-3 M
C)2.9 × 10^-12 M
D)5.9 × 10^-12 M
E)1.0 × 10^-7 M

Question 48

What is the hydronium-ion concentration in a solution formed by combining 450 mL of 0.10 M NaOH with 150 mL of 0.30 M HCl?
NaOH(aq)+ HCl(aq)→ NaCl(aq)+ H₂O(l)

A)0.045 M
B)1.7 × 10^-13 M
C)1.0 × 10^-7 M
D)0.30 M
E)0.10 M

Question 49

At 25°C a solution has a hydroxide-ion concentration of 8.22 × 10^-5 M.What is its hydronium-ion concentration?

A)8.22 × 10^-19 M
B)1.00 × 10^-7 M
C)1.00 × 10^-14 M
D)8.22 × 10^-5 M
E)1.22 × 10^-10 M

Question 50

What pH should a solution have if its pH is about the same as that of vinegar?

A)about 8
B)about 11
C)about 1
D)about 6
E)about 3

Question 51

A solution has a pH value of 3.66.What is the pOH for this solution?

A)7.00
B)3.83
C)3.66
D)2.19
E)10.34

Question 52

Which aqueous solution has the lowest pH?

A)0.30 M HCl
B)0.30 M NaOH
C)0.30 M NH₃
D)0.30 M Ba(OH)₂
E)0.30 M H₂SO₄

Question 53

A solution in which the pH is 1.5 would be described as

A)neutral.
B)very acidic.
C)slightly basic.
D)slightly acidic.
E)very basic.

Question 54

At 25°C,what is the pH of a 10.0 M HNO₃ solution?

A)1.000
B)0.000
C)10.000
D)-1.000
E)14.000

Question 55

The hydronium-ion concentration of a solution is 8.2 × 10^-6 M.What is the pH of the solution?

A)6.30
B)3.26
C)2.00
D)5.09
E)9.41

Question 56

Which solution has the highest pH?

A)0.1 M Ba(OH)₂
B)0.1 M CH₃COOH
C)0.1 M HCl
D)0.1 M NH₃
E)0.1 M NaOH

Question 57

Which of the following expressions is not equivalent to pH?

A)-log [H⁺(aq)]
B)
C)14.0 - pOH
D)
E)-log K_w

Question 58

The pOH of a solution is 5.15.What is the pH of the solution?

A)5.15
B)8.85
C)7.08
D)7.00
E)2.72

Question 59

What is the pH of a 0.0072 M hydrochloric acid solution?

A)4.93
B)11.86
C)7.00
D)9.07
E)2.14

Question 60

A solution has a hydroxide-ion concentration of 0.0040 M.What is the pOH of the solution?

A)11.60
B)2.40
C)7.00
D)8.48
E)5.52

Question 61

What is the pOH of a 0.0027 M Ba(OH)₂ solution?

A)8.78
B)11.43
C)11.73
D)2.27
E)2.57

Question 62

In Arrhenius theory,a(n)_____ is a substance that completely ionizes in aqueous solution to give H₃O⁺(aq)and an anion.

A)​strong acid
B)​strong base
C)​weak acid
D)​alkali
E)​weak base

Question 63

In Arrhenius theory,a _____ completely ionizes in aqueous solution to give OH^- and a cation.

A)​strong acid
B)​strong base
C)​weak acid
D)​carborane
E)​weak base

Question 64

What is the pOH of a 0.033 M HNO₃ solution?

A)12.52
B)10.59
C)15.48
D)1.48
E)3.41

Question 65

What is the pOH of a 0.0032 M CsOH solution?

A)2.49
B)16.49
C)8.26
D)5.74
E)11.51

Question 66

What is the pOH of a solution prepared by dissolving 0.951L of HCl(g),measured at STP,in enough water such that the total volume of the solution is 8.50 L? (R = 0.0821 L · atm/(K · mol))

A)12.628
B)7.000
C)1.372
D)11.698
E)2.302

Question 67

Which of the following solutions has the highest hydroxide-ion concentration?

A)0.1 M HCl
B)a solution with pH = 5
C)0.1 M H₂SO₄
D)pure water
E)a solution with pOH = 12

Question 68

What is the pOH of a solution prepared by dissolving 0.591 g of KOH(s)in 7.50 L of water?

A)11.148
B)2.852
C)1.977
D)12.023
E)7.000

Question 69

What is the pH of a 0.0052 M CaOH solution?

A)8.74
B)11.72
C)2.28
D)5.26
E)16.28

Question 70

A solution has a hydronium-ion concentration of 0.0029 M.What is its pOH?

A)2.54
B)16.54
C)8.16
D)​5.84
E)11.46

Question 71

A solution has a hydroxide-ion concentration of 0.078 M.What is its pH?

A)15.11
B)12.89
C)16.55
D)7.00
E)1.11

Question 72

What is the pH of a 0.0025 M Ba(OH)₂ solution?

A)8.70
B)11.40
C)2.60
D)11.70
E)2.30

Question 73

Which solution would cause blue litmus to turn red?

A)a solution of pH 10
B)a solution of 0.01 M NH₃
C)a solution of pOH 4
D)a solution of 0.005 M CH₃COOH
E)a solution of 0.10 M NaOH

Question 74

The pOH of a solution is 5.72 .What is its hydronium-ion concentration?

A)5.2 × 10⁵ M
B)5.2 × 10^-9 M
C)1.9 × 10^-6 M
D)5.72 M
E)3.3 × 10^-3 M

Question 75

The pH of a solution of a strong base is 10.32 at 25°C.What is its hydronium-ion concentration?

A)3.1 × 10^-3 M
B)2.1 × 10^-4 M
C)1.6 × 10^-4 M
D)4.8 × 10^-11 M
E)1.4 × 10^-2 M

Question 76

What is the pH of a solution prepared by dissolving 0.195 g of NaOH(s)in 9.00 L of water?

A)2.312
B)11.688
C)7.000
D)10.734
E)3.266

Question 77

What is the pH of a solution prepared by dissolving 0.241 L of HCl(g),measured at STP,in enough water such that the total volume of the solution is 2.00 L? (R = 0.0821 L · atm/(K · mol))

A)2.270
B)11.730
C)1.968
D)7.000
E)12.032

Question 78

A solution has a pOH of 5.20.What is its hydroxide-ion concentration?

A)1.5 × 10^-4 M
B)5.2 M
C)1.6 × 10^-9 M
D)6.3 × 10^-6 M
E)5.5 × 10^-3 M

Question 79

A solution has a pH of 10.20 at 25°C.What is the hydroxide-ion concentration at 25°C?

A)3.8 M
B)2.2 × 10^-2 M
C)1.6 × 10^-4 M
D)6.3 × 10^-11 M
E)1.0 × 10^-7 M

Question 80

What is the hydroxide-ion concentration in a solution formed by combining 200.mL of 0.16 M HCl with 300.mL of 0.091 M NaOH at 25°C?
HCl(aq)+ NaOH(aq)→ NaCl(aq)+ H₂O(l)

A)1.6 × 10^-13 M
B)0.091 M
C)1.1 × 10^-12 M
D)0.055 M
E)1.0 × 10^-7 M