Deck 15: Acids, Bases, and Salts

Question 1

Arrhenius defined a base as a substance whose aqueous solution contains an excess of

A)sodium ion.
B)hydroxide ion.
C)chloride ion.
D)hydrogen ion.

Answer 1

hydroxide ion.

Question 2

In the following reaction, the compound CH₃NH₂ behaves as:

A)an acid.
B)a base.
C)a salt.
D)a conjugate acid.

Answer 2

a base.

Question 3

Which is a strong electrolyte?

A)water
B)acetic acid
C)ammonia
D)sodium chloride

Answer 3

acetic acid

Question 4

Which is a strong electrolyte?

A)sulfuric acid
B)sulfurous acid
C)ammonia
D)acetic acid

Question 5

The hydroxide ion is responsible for the properties of

A)acids
B)bases
C)salts

Question 6

Bronsted and Lowry defined a base as a(n)

A)electron donor.
B)electron acceptor.
C)proton donor.
D)proton acceptor.

Question 7

An amphoteric substance is one that

A)may react as an acid or a conjugate acid
B)may react as a salt
C)may react as a base or a conjugate base
D)may react as an acid or a base

Question 8

Acids react with carbonates to produce the gas

A)hydrogen.
B)carbon dioxide.
C)nitrogen.
D)oxygen.

Question 9

Bronsted and Lowry defined an acid as a(n)

A)electron donor.
B)electron acceptor.
C)proton donor.
D)proton acceptor.

Question 10

In the following reaction, water behaves as:

A)an acid.
B)a base.
C)a salt.
D)a conjugate base.

Question 11

In an acidic solution the

A)concentration of hydronium ion is greater than that of hydroxide ion
B)concentration of hydroxide ion greater than that of hydronium ion
C)concentration of hydronium ion and hydroxide ion are equal

Question 12

A hydrogen ion consists of a(n)

A)electron.
B)proton.
C)neutron.
D)proton and electron.

Question 13

The hydronium ion is responsible for the properties of

A)acids
B)bases
C)salts

Question 14

The concentration of an aqueous solution of iron(II)chloride is 0.0550 M.What is the molarity of each ion in this solution?

A)0.0550 M for both the iron(II)and chloride ions.
B)0.0550 M for the iron(II)ion and 0.110 M for the chloride ion.
C)0.110 M for the iron(II)ion and 0.0550 M for the chloride ion.
D)not enough information is given to determine each molarity.

Question 15

Acids react with active metals to produce the gas

A)nitrogen monoxide.
B)carbon dioxide.
C)helium.
D)hydrogen.

Question 16

Arrhenius defined an acid as a substance whose aqueous solution contains an excess of

A)sodium ion.
B)hydroxide ion.
C)chloride ion.
D)hydrogen ion.

Question 17

Which is the hydroxide ion?

A)H ⁺¹
B)H₃O ⁺¹
C)OH ^-1
D)OH₂ ^-1

Question 18

Which is a strong electrolyte?

A)methanol,CH₃OH
B)water
C)hydrosulfuric acid
D)hydrochloric acid

Question 19

In a basic solution the

A)concentration of hydronium ion is greater than that of hydroxide ion
B)concentration of hydroxide ion is greater than that of hydronium ion
C)concentration of hydronium ion and hydroxide ion are equal

Question 20

Which is a strong electrolyte?

A)sugar
B)hypochlorous acid
C)sodium hydroxide
D)hydrosulfuric acid

Question 21

Which pH is most acidic?

A)3
B)7
C)9
D)14

Question 22

Which is the pH of a solution in which the concentration of hydroxide ion is greater than the concentration of hydrogen ion?

A)7
B)2
C)6
D)13

Question 23

In a 0.125 M aqueous solution of potassium phosphate,what is the molarity of each ion?

A)0.125 M for the potassium ion and 0.250 M for the phosphate ion.
B)0.125 M for the potassium ion and 0.375 M for the phosphate ion.
C)0.375 M for the potassium ion and 0.125 M for the phosphate ion.
D)0.250 M for the potassium ion and 0.125 M for the phosphate ion.

Question 24

Which will ionize when placed in water?

A)KOH
B)HCl
C)KCl
D)LiCl

Question 25

A solution of a strong acid has a pH of 3.The concentration of hydronium ions in this solution is

A)0.001 M
B)3 M
C)0.3 M.
D)0.003 M

Question 26

Which acid and base will combine to form sodium sulfite?

A)NaOH and H₂SO₃
B)NaOH and H₂SO₄
C)Na(OH)₂ and H₂SO₃
D)Na(OH)₂ and H₂SO₄

Question 27

Which will dissociate when placed in water?

A)CH₃OH
B)HCl
C)NaCl
D)HClO₄

Question 28

Which is the pH of a solution in which the concentration of hydrogen ion is equal to the concentration of hydroxide ion?

A)7
B)9
C)12
D)4

Question 29

Combining potassium hydroxide and sulfuric acid will produce water and

A)potassium sulfide.
B)potassium sulfate.
C)potassium sulfite.
D)potassium hypersulfate.

Question 30

Which is a strong base?

A)CuOH
B)HCl
C)KOH
D)CH₃OH

Question 31

Which is a strong acid?

A)HNO₃
B)HNO₂
C)HClO
D)HClO₂

Question 32

Which pH is most alkaline?

A)1
B)5
C)7
D)12

Question 33

Which pH is neutral?

A)2
B)4
C)5
D)7

Question 34

Which acid and base will combine to form calcium sulfate?

A)CaOH and H₂SO₃
B)CaOH and H₂SO₄
C)Ca(OH)₂ and H₂SO₃
D)Ca(OH)₂ and H₂SO₄

Question 35

Which is a strong base?

A)NH₄OH
B)Ca(OH)₂
C)HNO₂
D)HNO₃

Question 36

How many times more concentrated is the hydrogen ion concentration in a solution with a pH of 3 than that with a pH of 5?

A)2 times
B)10 times
C)100 times
D)1000 times

Question 37

Which type of compound is not an electrolyte?

A)Alcohol
B)Acid
C)Base
D)Salt

Question 38

Which is the pH of a solution in which the concentration of hydrogen ion is greater than the concentration of hydroxide ion?

A)12
B)9
C)7
D)3

Question 39

Combining sodium hydroxide and hydrochloric acid will produce water and

A)sodium chloride.
B)sodium chlorite.
C)sodium chlorate.
D)sodium hypochlorite.

Question 40

Which is a strong acid?

A)HClO₃
B)HClO₂
C)H₂SO₃
D)H₂SO₄

Question 41

What is the concentration of calcium ion in a 2.0 M solution of calcium chloride?

A)1.0 M
B)2.0 M
C)3.0 M
D)4.0 M

Question 42

What is the boiling point of a 2.0 m aqueous solution of sodium chloride? (The boiling point elevation constant for water is 0.512 ^°C/m. )

A)101.02 ^°C
B)1.02 ^°C
C)2.05 ^°C
D)102.05 ^°C

Question 43

Which is a conjugate acid base pair in the following equation? H₃PO₄ + H₂O H₃O ⁺¹ + H₂PO₄ ^-1

A)H₃PO₄ and H₂O
B)H₃O ⁺¹ and H₂PO₄ ^-1
C)H₂O and H₃O ⁺¹
D)H₃PO₄ and H₃O ⁺¹

Question 44

What is the conjugate acid of OH ^-1?

A)O^-2
B)H ⁺¹
C)O₂H
D)HOH

Question 45

What is the concentration of chloride ion in a 2.0 M solution of calcium chloride?

A)1.0 M
B)2.0 M
C)3.0 M
D)4.0 M

Question 46

Which are the two Bronsted-Lowry bases in the following equation? NH₃ + H₂O NH₂ ^-1 + H₃O ⁺¹

A)H₂O and NH₂ ^-1
B)NH₃ and H₂O
C)H₃O ⁺¹ and NH₃
D)NH₂ ^-1 and H₃O ⁺¹

Question 47

What is the conjugate acid of NH₃?

A)N^-3
B)NH₄ ⁺¹
C)NH₂ ^-1
D)NH ^-2

Question 48

Which is a conjugate acid base pair in the following equation? H₂SO₄ + H₂O HSO₄ ^-1 + H₃O ⁺¹

A)H₂SO₄ and HSO₄ ^-1
B)H₂SO₄ and H₂O
C)HSO₄ ^-1 and H₃O ⁺¹
D)H₃O ⁺¹ and H₂SO₄

Question 49

What is the net ionic equation when hydrobromic acid reacts with potassium hydroxide?

A)H ⁺¹ + OH ^-1 $\rarr$ H₂O
B)H ⁺¹ + Br^--1 $\rarr$ HBr
C)K ⁺¹ + OH ^-1 $\rarr$ KOH
D)K ⁺¹ + H^-1 $\rarr$ KH

Question 50

What are the spectator ions when hydrochloric acid reacts with sodium hydroxide?

A)Na ⁺¹ and H ⁺¹
B)Cl ^-1 and OH ^-1
C)H ⁺¹ and OH ^-1
D)Na ⁺¹ and Cl ^-1

Question 51

The pH of a solution can be calculated from the expression

A)pH = - log [OH ^-1]
B)pH = log [OH ^-1]
C)pH = - log [H ⁺¹]
D)pH = log [H ⁺¹]

Question 52

Which is a conjugate acid base pair in the following equation? HS ^-1 + H₂O S ^-2 + H₃O ⁺¹

A)HS ^-1 and H₃O ⁺¹
B)HS ^-1 and S ^-2
C)H₃O ⁺¹ and S ^-2
D)HS ^-1 and H₂O

Question 53

Which are the two Bronsted-Lowry acids in the following equation? NH₃ + H₂O NH₄ ⁺¹ + OH ^-1

A)NH₃ and H₂O
B)NH₃ and NH₄ ⁺¹
C)NH₃ and OH ^-1
D)NH₄ ⁺¹ and H₂O

Question 54

What is the conjugate base of NH₃?

A)NH₂ ^-1
B)NH ^-2
C)NH₄ ⁺¹
D)H ⁺¹

Question 55

Which are the two Bronsted-Lowry acids in the following equation? H₂S + H₂O HS ^-1 + H₃O ⁺¹

A)HS ^-1 and H₂O
B)H₂S and HS ^-1
C)H₂S and H₃O ⁺¹
D)H₃O ⁺¹ and H₂O

Question 56

Which is a conjugate acid base pair in the following equation? HF + H₂O H₃O ⁺¹ + F ^-1

A)HF and H₃O ⁺¹
B)HF and H₂O
C)H₃O ⁺¹ and F ^-1
D)HF and F ^-1

Question 57

A solution of a strong base has a pH of 11.The concentration of hydronium ions in this solution is

A)11 M
B)
C)
D)

Question 58

What is the conjugate base of HS ^-1?

A)H₂S
B)S ^-2
C)H ⁺¹
D)OH ^-1

Question 59

Which are the two Bronsted-Lowry bases in the following equation? HNO₂ + H₂O H₃O ⁺¹ + NO₂ ^-1

A)H₃O ⁺¹ and HNO₂
B)H₂O and NO₂ ^-1
C)HNO₂ and H₂O
D)H₃O ⁺¹ and NO₂ ^-1

Question 60

Which type of mixture displays Brownian motion and the Tyndall effect?

A)Solution
B)Colloidal dispersion
C)Suspension

Question 61

What is the pH of a 0.01 M solution of hydrochloric acid?

A)0.01
B)1
C)2
D)-2

Question 62

What is the freezing point of a 1.0 m aqueous solution of CaCl₂? (The freezing point depression constant for water is 1.86 ^°C/m. )

A)-1.86 ^°C
B)1.86 ^°C
C)-3.72 ^°C
D)-5.58 ^°C

Question 63

What is the concentration of an HBr solution if 12.0 mL of the solution is neutralized by 15.0 mL of a 0.25 M KOH solution?

A)0.75 M
B)0.31 M
C)0.40 M
D)0.20 M

Question 64

What is the concentration of an HCl solution if 25.0 mL of the solution is neutralizedcompletely by 40.0 mL of a 0.30 M KOH solution?

A)0.19 M
B)300 M
C)46.9 M
D)0.48 M

Question 65

An aqueous solution is 18.7% by mass Na₃PO₄.What is the boiling point of this solution? The K_b for water is 0.512°C/m.Consider if the solute is an electrolyte or a nonelectrolyte.

A)102.89°C
B)100.72°C
C)101.44°C
D)100.00 °C

Question 66

What is the pH of a solution whose H ⁺¹ concentration is 4.0 10 ^-9?

A)4.0
B)8.4
C)3.6
D)9.0

Question 67

What is the pH of a 1.0 M solution of nitric acid?

A)0
B)1
C)-1
D)4

Question 68

What is the pH of a 0.034 M hydrochloric acid solution?

A)-2
B)3.4
C)-1.5
D)1.5

Question 69

What is the concentration of a H₂SO₄ solution if 10.0 mL of the solution is neutralized by 7.8 mL of a 0.20 M NaOH solution?

A)0.0026 M
B)0.078 M
C)0.156 M
D)0.31 M

Question 70

What is the concentration of a HNO₃ solution if 10.0 mL of the solution is neutralized by 3.6 mL of a 0.20 M NaOH solution?

A)0.072 M
B)53.6 M
C)0.56 M
D)5.6 M

Question 71

What is the boiling point of a 0.50 m aqueous solution of Al(NO₃)₃? (The boiling point elevation constant for water is 0.512 ^°C/m. )

A)100.51 ^°C
B)101.02 ^°C
C)102.05 ^°C
D)106.60 ^°C

Question 72

What is the concentration of a H₂SO₄ solution if 15.0 mL of the solution is neutralized by 3.60 mL of a 0.65 M Ca(OH)₂ solution?

A)0.078 M
B)0.16 M
C)0.31 M
D)2.7 M

Question 73

An aqueous solution is 12.5% in Na₂CO₃ and has a density of 1.19 g/mL.What is the molarity of this solution?

A)0.117 M
B)
C)14.9 M
D)

Question 74

What is the concentration of a HCl solution if 20.0 mL of the solution is neutralized by 15.0 mL of a 0.10 M Ca(OH)₂ solution?

A)0.075 M
B)0.038 M
C)0.15 M
D)0.13 M

Question 75

What is the pH of a solution whose H₃O ⁺¹ concentration is 1 10 ^-9?

A)1
B)9
C)-9
D)-1

Question 76

What mass of ethanol,C₂H₅OH,should be added to 200.0 g of water in order to increase its boiling point to 102.5°C? The K_b for water is 0.512°C/m.Consider if the solute is an electrolyte or a nonelectrolyte.

A)4.9 g
B)0.98 g
C)45 g
D)90.g

Question 77

What mass of sodium chloride should be added to 500.0 g of water in order to decrease its freezing point to -1.0 °C? The K_f for water is 1.86°C/m.Consider if the solute is an electrolyte or a nonelectrolyte.

A)0.269 g
B)134 g
C)15.7 g
D)7.85 g

Question 78

A solution is prepared by adding 35.5 mL of ethylene glycol,C₂H₆O₂,to 250.0 g of water.What is the freezing point of this solution? The K_f for water is 1.86°C/m and the density of ethylene glycol is 1.1135 g/mL.Consider if the solute is an electrolyte or a nonelectrolyte.

A)−0.29°C
B)−4.74°C
C)−0.01°C
D)0.00°C

Question 79

What is the pH of a 0.020 M nitric acid solution?

A)0.020
B)-2.0
C)1.7
D)4.0

Question 80

What is the freezing point of a 3.0 m aqueous solution of NaCl? (The freezing point depression constant for water is 1.86 ^°C/m. )

A)5.6 ^°C
B)-5.6 ^°C
C)11 ^°C
D)-11 ^°C