Deck 10: Acids and Bases

Question 1

The base forms a new ________ bond in a Brønsted-Lowry acid-base reaction.

A)covalent
B)aquo
C)hydrogen
D)ionic
E)metallic

Answer 1

covalent

Question 2

A Brønsted-Lowry base is a substance which

A)produces hydrogen ions in aqueous solution.
B)produces hydroxide ions in aqueous solution.
C)donates protons to other substances.
D)accepts protons from other substances.
E)accepts hydronium ions from other substances.

Answer 2

accepts protons from other substances.

Question 3

Which of the following compounds is a salt?

A)HBr
B)KNO₃
C)H₂SO₄
D)NaOH
E)C₆H₁₂O₆

Answer 3

KNO₃

Question 4

What is the conjugate base of HSO₄^-?

A)SO₄^2-
B)H₂SO₄
C)H₃O⁺
D)OH^-
E)H₂SO₃

Question 5

Consider the following reaction: NO₂^- + HCO₃^-
CO₃^-2 + HNO₂
Identify the acid,base,conjugate acid and conjugate base.

Question 6

When acids and bases react the product other than water is a

A)hydrogen ion.
B)hydroxide ion.
C)hydronium ion.
D)metal.
E)salt.

Question 7

Which of the following cannot act as a Brønsted base?

A)HCO₃^-
B)CO₃^2-
C)NH₃
D)NH₂^-
E)NH₄⁺

Question 8

Which of the following is a diprotic acid?

A)acetic acid
B)hydrochloric acid
C)phosphoric acid
D)sulfuric acid
E)nitric acid

Question 9

C₅H₅N + H₂CO₃
C₅H₆ N⁺ + HCO₃^-
In the reaction shown,the conjugate acid of C₅H₅N is ________.

A)C₅H₅N
B)H₂CO₃
C)C₅H₆N⁺
D)HCO₃^-
E)H₃O⁺

Question 10

Which statement concerning Arrhenius acid-base theory is not correct?

A)An Arrhenius acid produces hydrogen ions in water solution.
B)An Arrhenius base produces hydroxide ions in water solution.
C)A neutralization reaction produces water plus a salt.
D)Acid-base reactions must take place in aqueous solution.
E)none of the above

Question 11

In the following equation,which of the following is acting as the Bronsted acid?
HClO₄ + H₂O --> ClO₄^- + H₃O⁺

A)HClO₄
B)H₂O
C)ClO₄^-
D)H₃O⁺

Question 12

According to Brønsted-Lowry theory,acid-base reactions can be described as ________ reactions.

A)electrolytic
B)electron transfer
C)gas phase
D)nuclear transfer
E)proton transfer

Question 13

Which compound is manufactured in larger quantities in the U.S.than any other industrial chemical?

A)HCl
B)HNO₃
C)H₃PO₄
D)H₂SO₄
E)NaOH

Question 14

Which pair of compounds is used in the manufacture of fertilizers?

A)HCl and NaOH
B)HCl and H₃PO₄
C)HNO₃ and HCl
D)H₂SO₄ and H₃PO₄
E)HNO₃ and NaOH

Question 15

Consider the reaction: H₂SO₃ + HCO₃^-
H₂CO₃ + HSO₃^-
a)Identify the acid,base,conjugate acid and conjugate base
b)Identify two substances from the reaction which could be used to prepare a buffer.

Question 16

A Brønsted-Lowry acid is a substance which

A)produces hydrogen ions in aqueous solution.
B)produces hydroxide ions in aqueous solution.
C)donates protons to other substances.
D)accepts protons from other substances.
E)accepts hydronium ions from other substances.

Question 17

Which of the following compounds is a salt?

A)CH₃CO₂H
B)NH₃
C)NH₄NO₃
D)Al(OH)₃
E)C₆H₆

Question 18

CH₃NH₂ + HCl
CH₃NH₃⁺ + Cl^-
A conjugate acid-base pair in the reaction shown is ________ and ________.

A)CH₃NH₂ and HCl
B)CH₃NH₂ and Cl^-
C)CH₃NH₃⁺ and Cl^-
D)HCl and Cl^-
E)HCl and H₃O⁺

Question 19

The H₃O⁺ ion is called the ________ ion.

A)hydroxide
B)hydronium
C)hydrogen
D)protium
E)water

Question 20

A necessary requirement for a Brønsted base is

A)the presence of water as a reaction medium.
B)the presence of hydroxide in its formula.
C)a lone pair of electrons in its Lewis dot structure.
D)the production of hydronium ion upon reaction with water.
E)the presence of a metal ion in its formula.

Question 21

Which solution is basic?

A)[H₃O⁺] = 1.0 × 10^-4
B)[H₃O⁺] = 1.0 × 10^-7
C)[H₃O⁺] = 1.0 × 10^-10
D)[OH^-] = 1.0 × 10^-7
E)[OH^-] = 1.0 × 10^-10

Question 22

Which of the following is a weak acid?

A)HNO₃
B)H₃PO₄
C)NH₃
D)HCl
E)OH^-

Question 23

Which of the following is a strong acid?

A)HNO₃
B)H₃PO₄
C)NH₄⁺
D)HCO₃^-
E)H₂O

Question 24

What is the conjugate base of water?

A)H₂O (l)
B)H₃O⁺ (aq)
C)OH^- (aq)
D)H⁺ (aq)
E)O₂^- (aq)

Question 25

Which of the following is a triprotic acid?

A)H₃PO₄
B)CH₃COOH
C)HNO₃
D)NH₃
E)Al(OH)₃

Question 26

Which reaction best illustrates the behavior of the weak base H₂PO₄^- in aqueous solution?

A)H₂PO₄^- (aq)+ H₂O (l)

HPO₄^2- (aq)+ H₃O⁺ (aq)
B)H₂PO₄^- (aq)+ H₂O (l)

H₃PO₄ (aq)+ OH^- (aq)
C)H₂PO₄^- (aq)

2H⁺ (aq)+ PO₄^3- (aq)
D)H₂PO₄^- (aq)

H⁺ (aq)+ HPO₄^2- (aq)
E)H₂PO₄^- (aq)+ H⁺ (aq)

H₃PO₄ (aq)

Question 27

Water and HSO₄^- can either accept protons or donate protons.Such substances are said to be

A)amphoteric.
B)conjugate.
C)diprotic.
D)monoprotic.
E)triprotic.

Question 28

Which compound has a value of K_a that is close to 10^-5?

A)NaCl
B)HNO₃
C)CH₃CH₂CO₂H
D)KOH
E)NH₃

Question 29

The classification of an acid or a base as weak or strong is determined by

A)the solubility of the acid or base.
B)the extent of dissociation of the dissolved acid or base.
C)the concentrations of the acid or base.
D)more than one choice is correct.

Question 30

What is the conjugate acid of water?

A)H₂O (l)
B)H₃O⁺ (aq)
C)OH^- (aq)
D)H⁺ (aq)
E)O₂^- (aq)

Question 31

Which one of the following is the strongest weak acid?

A)HCN (Ka = 4.9 × 10^-10)
B)HClO (Ka = 3.0 × 10^-8)
C)HNO₂ (Ka = 4.5 × 10^-4)
D)HF (Ka = 6.8 × 10^-4)

Question 32

Hydrogen cyanide,HCN,is a weak acid.Which equation best represents its aqueous chemistry?

A)HCN (aq)+ H₂O (l)

CN^- (aq)+ H₃O⁺ (aq)
B)HCN (aq)+ H₂O (l)

H₂CN⁺ (aq)+ OH^- (aq)
C)HCN (aq)

H⁺ (aq)+ CN^- (aq)
D)HCN (aq)

H^- (aq)+ CN⁺ (aq)
E)H₂O (l)

H⁺ (aq)+ OH^- (aq)

Question 33

Which one of the following is the weakest acid?

A)HCN (Ka = 4.9 × 10^-10)
B)HClO (Ka = 3.0 × 10^-8)
C)HNO₂ (Ka = 4.5 × 10^-4)
D)HF (Ka = 6.8 × 10^-4)

Question 34

What is the conjugate acid of HSO₄^-?

A)SO₄^2-
B)H₂SO₄
C)H₃O⁺
D)OH^-
E)H₂SO₃

Question 35

Ammonia reacts with acids because

A)it contains the hydroxide group.
B)it is neutral.
C)it is itself an acid.
D)it is a salt.
E)it contains a lone pair of electrons.

Question 36

At 25°C,the value of K_w is ________.

A)1.00
B)1.00 × 10^-7
C)1.00 × 10^-14
D)1.00 × 10⁷
E)1.00 × 10¹⁴

Question 37

Acetic acid is a weak acid in water because it is

A)dilute.
B)only slightly soluble.
C)unable to hold onto its hydrogen ion.
D)only slightly dissociated into ions.
E)completely dissociated into hydronium ions and acetate ions.

Question 38

Which statement is correct for pure water?

A)Pure water contains equal amounts of hydroxide,[OH^-],and hydronium,[H₃O⁺],ions.
B)Pure water contains larger amounts of hydroxide,[OH^-],ions than hydronium,[H₃O⁺],ions.
C)Pure water contains larger amounts of hydronium,[H₃O⁺],ions than hydroxide,
[OH^-],ions.
D)Pure water is an electrolyte.
E)Pure water contains no ions.

Question 39

Which compound has a very large value of K_a in aqueous solution?

A)NaCl
B)HNO₃
C)H₃PO₄
D)KOH
E)NH₃

Question 40

In an aqueous solution that is basic,[H₃O⁺] is ________ than 1.0 × 10^-7 and ________ than [OH^-].

A)greater; less
B)less; greater
C)greater; greater
D)less; less
E)none of the above

Question 41

Which of the following statements is correct?

A)In a basic solution,[H₃O⁺] < 10^-7; [OH^-] < 10^-7.
B)In a basic solution,[H₃O⁺] > 10^-7; [OH^-] > 10^-7.
C)In a basic solution,[H₃O⁺] > 10^-7; [OH^-] < 10^-7.
D)In a basic solution,[H₃O⁺] < 10^-7; [OH^-] > 10^-7.
E)In a basic solution,[H₃O⁺] > 10^-7; [OH^-] = 10^-7.

Question 42

What is the pH of a solution in which the hydrogen ion concentration is 5.1 × 10^-8 M?

A)6.71
B)1.96 × 10^-7
C)8.90
D)5.10
E)7.29

Question 43

What is the pH of a solution in which [H₃O⁺] = 3.8 × 10^-8 M?

A)7.42
B)6.58
C)3.80
D)1.0 × 10^-8
E)2.6 × 10^-7

Question 44

An increase in solution pH corresponds to

A)an increase in hydronium ion concentration.
B)a decrease in hydronium ion concentration.
C)no change in hydronium ion concentration.
D)a decrease in hydroxide ion concentration.

Question 45

What is the value of [H₃O⁺] in a solution with pH = 10.82?

A)6.6 × 10^-4 M
B)1.5 × 10^-11 M
C)1.03 M
D)10.82 M
E)3.18 M

Question 46

What is the hydrogen ion concentration in a solution with pH = 2.34?

A)4.57 × 10^-3 M
B)2.34 × 10^-3 M
C)2.19 × 10^-12 M
D)1.17 × 10¹ M
E)4.27 × 10^-12 M

Question 47

The pH of a solution with [H₃O⁺] = 5.9 × 10^-3 M,to the correct number of significant figures,is ________.

A)5.9 × 10^-3
B)2.2
C)2.23
D)1.01
E)2.229

Question 48

What is the pH of a solution in which [H₃O⁺] = 1.2 × 10^-3 M?

A)1.20
B)2.92
C)11.08
D)12.80
E)8.33 × 10^-12

Question 49

What is the pH of a solution in which [H₃O⁺] = 4.1 × 10^-2 M?

A)12.61
B)1.39
C)1.10
D)12.90
E)4.10

Question 50

If the concentration of OH^- in an aqueous solution is 1.4 × 10^-7 M,the concentration of H₃O⁺ is ________.

A)7.1 × 10⁺⁶ M
B)1.0 × 10^-7 M
C)1.4 × 10^-7 M
D)7.1 × 10^-8 M
E)1.3 × 10^-8 M

Question 51

In an aqueous solution that is acidic,[H₃O⁺] is ________ than 1.0 × 10^-7 and ________ than [OH^-].

A)greater; less
B)less; greater
C)greater; greater
D)less; less
E)none of the above

Question 52

Which example is not acidic?

A)orange juice
B)soil for azaleas with pH of 4.8
C)a solution of NH₄NO₃ with pH < 7.00
D)lake water that turns blue litmus to red
E)a solution in which [H₃O⁺] = 1.00 × 10^-7

Question 53

Which example is not basic?

A)shampoo
B)vinegar
C)window cleaner
D)limewater
E)Mg(OH)₂,used in remedies for upset stomach

Question 54

The pH of a cup of coffee is measured as 5.45.Express this measurement as [H⁺],using the correct number of significant figures.

A)3.548 × 10^-6 M
B)3.55 × 10^-6 M
C)3.5 × 10^-6 M
D)4 × 10^-6 M
E)2.82 × 10⁵ M

Question 55

If the [H₃O⁺] of a water sample is 1 × 10^-4 M,the pH of the sample is ________,and the sample is ________.

A)-4; acidic
B)4; acidic
C)4; basic
D)10; basic
E)-10; basic

Question 56

If the concentration of OH^- is 1 × 10^-2 M,the concentration of H₃O⁺ is ________ M.

A)1 × 10⁰
B)1 × 10^-2
C)1 × 10^-7
D)1 × 10^-12
E)1 × 10^-14

Question 57

Which of the following statements is correct?

A)In an acidic solution,[H₃O⁺] < 10^-7; [OH^-] < 10^-7.
B)In an acidic solution,[H₃O⁺] > 10^-7; [OH^-] > 10^-7.
C)In an acidic solution,[H₃O⁺] > 10^-7; [OH^-] < 10^-7.
D)In an acidic solution,[H₃O⁺] < 10^-7; [OH^-] > 10^-7.
E)In an acidic solution,[H₃O⁺] > 10^-7; [OH^-] = 10^-7.

Question 58

If the [H⁺] of a water sample is 1 × 10^-4 M,the [OH^-] is

A)1 × 10^-4 M.
B)1 × 10^-14 M.
C)1 × 10⁴ M.
D)1 × 10^-10 M.
E)none of the above

Question 59

If the concentration of H₃O⁺ in an aqueous solution is 7.6 × 10^-9 M,the concentration of OH^- is ________.

A)7.6 × 10^-23 M
B)1.3 × 10⁺⁸ M
C)6.4 × 10^-5 M
D)1.3 × 10^-6 M
E)7.6 × 10^-9 M

Question 60

If the concentration of H₃O⁺ is 3.5 × 10^-3 M,the concentration of OH^- is ________ M.

A)2.9 × 10^-12
B)1.0 × 10^-12
C)1.0 × 10^-7
D)3.5 × 10^-11
E)10.5 × 10^-3

Question 61

Calculate the hydrogen ion concentration in a solution with pH = 6.35.

A)7.65 M
B)6.35 M
C)4.5 × 10^-7 M
D)0.80 M
E)2.2 × 10^-8 M

Question 62

The pH of a 250.mL sample of a buffer solution is 9.85.If 1.0 mL of 6 M HCl is added,the pH of the resulting mixture is closest to ________.

A)0.00
B)1.65
C)7.00
D)9.70
E)10.00

Question 63

A buffer solution

A)is a salt solution.
B)maintains pH at 7.00.
C)is a strong base.
D)neutralizes only acids.
E)closely maintains its original pH.

Question 64

Which of the following pH's corresponds to a strongly basic solution?

A)11.5
B)2.7
C)6.9
D)7.4
E)4.3

Question 65

The normality of a solution prepared by dissolving 50.0 g of Ca(OH)₂ in water to make 250.mL solution is ________ N.

A)1.35
B)2.70
C)3.51
D)5.40
E)7.02

Question 66

To prepare a buffer using sodium phosphate,which of the following would also be needed?

A)hydrochloric acid
B)ammonium hydroxide
C)ammonium phosphate
D)phosphoric acid
E)sodium hydroxide

Question 67

The [OH^-] and the pH of 0.035 M KOH at 25°C are,respectively,

A)0.035 M and +1.46.
B)0.035 M and -1.46.
C)2.9 × 10^-13 M and -12.54.
D)0.035 and +12.54.
E)2.9 × 10^-13 M and +12.54.

Question 68

The normality of a solution prepared by dissolving 25.0 g of Ca(OH)₂ in water to make 250.mL solution is ________ N.

A)2.70
B)1.35
C)0.675
D)3.51
E)1.75

Question 69

Which of these,if dissolved in 1.0 L of pure water,would produce a buffer solution?

A)0.1 mol NaCl + 0.1 mol KCl
B)0.1 mol H₃O⁺ + 0.1 OH^-
C)0.1 mol NaH₂PO₄ + 0.1 mol Na₂HPO₄
D)0.1 mol HCl + 0.1 mol NaOH
E)0.1 mol H₃O⁺ + 0.1 mol Cl^-

Question 70

Which of the following solutions is a buffer?

A)a solution of acetic acid and sodium acetate
B)a solution of acetic acid and sodium sulfate
C)a solution of hydrochloric acid and sodium sulfate
D)a solution of hydrochloric acid and sodium acetate
E)a solution of sulfuric acid and sodium sulfate

Question 71

All of the statements regarding equivalents of acids and bases are true except

A)equivalents are the same as moles.
B)equivalents of acid are based on the number of hydrogen ions produced per formula unit of acid.
C)equivalents are used to determine normality of solutions.
D)the equivalent weight of a base is the weight that produces one mole of hydroxide ions.
E)one equivalent of any acid will neutralize one equivalent of any base.

Question 72

Explain the term "amphoteric." Use the hydrogen carbonate ion,HCO₃^- to illustrate amphoteric behavior.

Question 73

What is the [H₃O⁺] in a solution with pH = 11.61?

A)1.16 × 10⁺¹ M
B)2.39 × 10⁺¹ M
C)4.07 × 10^-3 M
D)1.00 × 10^-14 M
E)2.45 × 10^-12 M

Question 74

What is the normality of a solution prepared by dissolving 37.5 g citric acid,a triprotic acid with molar mass of 192.14 g,in water to make 250.mL solution?

A)2.34 N
B)0.780 N
C)0.147 N
D)0.0865 N
E)0.288 N

Question 75

What is the normality of a solution prepared by dissolving 75.0 g citric acid,a triprotic acid with molar mass of 192.14 g,in water to make 250.mL solution?

A)0.173 N
B)0.0576 N
C)0.293 N
D)4.68 N
E)1.56 N

Question 76

Which of the following pH's corresponds to a weakly acidic solution?

A)5.3
B)1.4
C)7.8
D)9.2
E)11.5

Question 77

What is the normality of a solution containing 100.g HNO₃ in 500.mL of solution?

A)1.26 N
B)1.59 N
C)3.17 N
D)0.500 N
E)0.630 N

Question 78

Which of the following pH's corresponds to a neutral solution?

A)7.0
B)1.8
C)6.2
D)8.5
E)14.0

Question 79

What is the normality of a solution containing 49 g of H₂SO₄ in enough water to make 400 mL of solution?

A)2.5 N
B)5.0 N
C)1.0 N
D)10 N
E)0.20 N

Question 80

All of the following species are involved in the blood buffer system except ________.

A)CO₂
B)H₂CO₃
C)HCO₃^-
D)CO₃^2-
E)none of the above