Deck 9: Acids, Bases, and Salts

Question 1

A water solution is found to have a molar OH ⁻ concentration of 3.2 × 10 ^{− 5}. The solution would be classified as _____ .

A)acidic
B)basic
C)neutral
D)can't be classified

Answer 1

basic

Question 2

A solution for which [OH ⁻ ] = 3.0 × 10 ^{− 10} is classified as _____ .

A)acidic
B)basic
C)neutral
D)More than one response is correct.

Answer 2

acidic

Question 3

Some salts isolated by evaporation retain water that is called

A)water of hydration.
B)hydroxide.
C)hydronium.
D)crystallized water.

Answer 3

water of hydration.

Question 4

Which of the following statements is true for neutral solutions in which water is the solvent?

A)Neutral solutions contain no H₃O⁺ ions.
B)Neutral solutions contain no OH ⁻ ions.
C)Neutral solutions contain H₃O⁺ and OH ⁻ ions in equal concentrations.
D)More than one response is correct.

Question 5

Which of the following is present in pure water?

A)H₃O⁺
B)OH ⁻
C)H₂O
D)all of them

Question 6

Which of the following substances could behave as an Arrhenius base?

A)Na₂CO₃
B)Na₃PO₄
C)K₂S
D)KOH

Question 7

The cation (positive ion)in a salt comes from _____ .

A)an acid
B)a base
C)either an acid or a base
D)water

Question 8

In the following reaction, all substances are soluble, and all dissociate except H₂O. Identify the spectator ions.  HCl + KOH → KCl + H₂O

A)H⁺ and OH ⁻
B)K⁺ and Cl ⁻
C)H⁺ and K⁺
D)Cl ⁻ and OH ⁻

Question 9

What salt would be produced by the reaction of H₂SO₄ with LiHCO₃?

A)Li₂S
B)LiSO₄
C)Li₂SO₄
D)Li₂CO₃

Question 10

What volume of 6.0 M HNO₃ would be needed to make 500 mL of 0.50 M solution?

A)6 mL
B)417 mL
C)42 mL
D)6 liters

Question 11

In the Brønsted theory, both acids and bases are defined in terms of how substances lose or gain

A)OH^-.
B)H₃O⁺.
C)H⁺.
D)Cl ⁻ .

Question 12

What is the function of in the first ionization of citric acid?

A)The ion serves as an Arrhenius acid in this reaction.
B)The ion serves as an Arrhenius base in this reaction.
C)The ion serves as the conjugate base of the acid, H₃C₆H₅O₇.
D)The ion serves as the conjugate acid of the base, H₃C₆H₅O₇.

Question 13

A solution for which [H⁺] = 1.0 × 10 ^{− 3} will have a pH of _____ .

A)5.00
B)3.00
C)− 5.00
D)− 9.00

Question 14

According to the Arrhenius theory, what is produced when an acid dissolves in water?

A)H⁺
B)OH^-
C)H₃O⁺
D)

Question 15

Many cleaning agents contain bases because bases react with _____ .

A)fats or oils
B)glass
C)salts
D)More than one response is correct.

Question 16

The molar concentration of H⁺ ions in a solution is 5.8 × 10 ^{− 9}. The pH is _____ .

A)9.00
B)5.80
C)between 8.00 and 9.00
D)between 9.00 and 10.00

Question 17

Which of the following is a property of acid solutions?

A)sour taste
B)slippery feel
C)change red litmus to blue
D)More than one response is correct.

Question 18

What are the missing products in the following reaction when it is written as a full equation? 2HBr + SrCO₃ → ____ + ____ + H₂O

A)SrBr₂ + CO₂
B)SrBr₂ +
C)Sr₂ + H₂CO₃
D)HBr + CO₂

Question 19

Identify the Brønsted acid(s)in the reaction. HIO₃(aq)+ H₂O (l) H₃O⁺ (aq)+ IO₃^- (aq)

A)HIO₃
B)HIO₃ and H₃O⁺
C)H₂O
D)H₂O and HIO₃

Question 20

Identify all Brønsted base(s)in the reaction. N₃^- (aq)+ H₂O (l) HN₃ (aq)+ OH^- (aq)

A)H₂O
B)
C)OH^-
D) and OH^-

Question 21

How many equivalents are contained in 0.25 moles of H₂SO₄?

A)0.25
B)0.13
C)0.50
D)can vary

Question 22

Which salt shifts the pH when dissolved in water?

A)KCl
B)Al(NO₃)₃
C)NaCl
D)NaNO₃

Question 23

Phosphoric acid, H₃PO₄, undergoes three dissociation reactions. Which of the three acids is the weakest?

A)
B)
C)
D)More than one response is correct.

Question 24

Antacids contain a substance that neutralizes hydrochloric acid. What is a candidate for use as an antacid?

A)Al(NO₃)₃
B)MgCl₂
C)Al₂(SO₄)₃
D)MgCO₃

Question 25

A 25.00 mL sample of H₂SO₄ acid solution requires 17.35 mL of 0.118 N base for titration. What is the normality of the acid solution?

A)0.0819 N
B)0.164 N
C)0.0409 N
D)0.236 N

Question 26

Identify the substance with the lowest pH.

A)orange juice
B)household ammonia
C)baking soda, NaHCO₃
D)milk

Question 27

Which of the following is a weak acid?

A)HNO₃
B)HCl
C)H₂CO₃
D)H₂SO₄

Question 28

Which of the following mixtures would represent a buffer?

A)sodium chloride\hydrochloric acid
B)sodium sulfate\sulfuric acid
C)sodium formate\formic acid
D)none of these

Question 29

A higher pH corresponds to _____ .

A)a higher [H⁺]
B)a lower [H⁺]
C)no change in [OH⁺]
D)a lower [OH ⁻ ]

Question 30

If a solution of acetic acid (a weak acid)is titrated with NaOH solution, what will be the pH at the equivalence point?

A)higher than 7
B)lower than 7
C)equal to 7
D)can't predict

Question 31

A solution has a pH of 11.60. The value of [H⁺] is _____ .

A)2.5 × 10 ^{− 4}
B)4.0 × 10 ^{− 3}
C)4.0 × 10 ^{− 11}
D)2.5 × 10 ^{− 12}

Question 32

In a buffer solution made up of equal concentrations of acetic acid and sodium acetate, NaC₂H₃O₂, which component is used to buffer against added OH ⁻ ?

A)C₂H₃O₂
B)Na⁺
C)OH ⁻
D)HC₂H₃O₂

Question 33

Which of the following salts would produce a basic solution (pH higher than 7)upon being dissolved in pure, distilled water?

A)NaCl
B)Na₂CO₃
C)Mg(NO₃)₂
D)NH₄Cl

Question 34

The procedure commonly used to determine the amount of base in a solution by adding a measured quantity of acid is called _____ .

A)dissociation
B)titration
C)ionization
D)normalization

Question 35

When an acid is analyzed by adding a measured quantity of base, the point at which all the acid has reacted is correctly called

A)the equivalence point.
B)the neutral point.
C)the endpoint.
D)the analysis point.

Question 36

What would be the pH of a solution of NH₄Cl in pure water?

A)higher than 7
B)lower than 7
C)equal to 7
D)can't be predicted

Question 37

Identify two Brønsted base(s)in the reaction. HIO₃ (aq)+ H₂O (I) H₃O⁺ (aq)+ 10₃^- (aq)

A)HIO₃, H₂O
B)HIO_3, H₃O⁺
C)HIO₃,  IO₃^-
D)H₂O, IO₃^-

Question 38

A 25.00 mL sample of hydrochloric acid solution, HCl, is titrated with 0.0512 M NaOH solution. The volume of NaOH solution required is 21.68 mL. What is the molarity of the HCl solution?

A)0.0444
B)0.0590
C)0.0295
D)0.0148

Question 39

A solution has a pH of 8.72. What is the value of [H⁺]?

A)5.2 × 10 ^{− 6}
B)1.9 × 10 ^{− 9}
C)5.2 × 10 ^{− 8}
D)1.9 × 10 ^{− 5}

Question 40

The classification of an acid or base as weak or strong is based upon

A)the solubility of the acid or base.
B)the extent of dissociation of the acid or base.
C)the concentration of acid or base in solution.
D)More than one response is correct.

Question 41

Which of the following sets of reactants could be used to prepare CaI₂?

A)CaO and HI
B)Ca(OH)₂ and HI
C)Ca and HI
D)Any of these could be used.

Question 42

A patient comes to you suffering from a battery acid burn (sulfuric acid). What is the best thing to use to neutralize the acid, while you continue to run cool water over the affected area?

A)a 1 M sodium hydroxide solution (NaOH)
B)a 1 M sodium bicarbonate solution (NaHCO₃)
C)a 1 M acetic acid solution (CH₃COOH)
D)a 1 M carbonic acid solution (H₂CO₃)

Question 43

Seageroic acid has a p K _a of 8.23, whereas slabaughic acid has a p K _a of 18.65.  From these facts, which of the following is true?

A)Slabaughic acid is less water soluble than seageroic acid.
B)Seageroic acid is a stronger acid than slabaughic acid.
C)Slabaughic acid dissociates to a greater extent in water.
D)Seageroic acid is a weaker acid than slabaughic acid.

Question 44

HCl will react with

A)BaO
B)CaCO₃
C)Mg
D)All three are correct.

Question 45

To determine the number of equivalents of Al(NO₃)₃ in a 0.750 M solution, the conversion factor would be which of the following?

A)
B)
C)
D)

Question 46

When a solution of HNO₃ is added to a solution of NaHCO₃, the net ion equation for reaction that occurs is which of the following?

A)
B)
C)
D)

Question 47

The expression for the K _a of the weak acid HF would be which of the following?

A)
B)
C)
D)

Question 48

The term, strong acid, refers to

A)the number of hydrogens attached to the acid molecule.
B)the speed at which it will dissolve metal.
C)if it will cause burns to the skin.
D)the ability for the acid to completely dissociate in solution.

Question 49

When your liver detoxifies ethyl alcohol, the concentration of the hydrogen ion increases. This will result in

A)respiratory acidosis.
B)metabolic acidosis.
C)respiratory alkalosis.
D)metabolic alkalosis.

Question 50

A reaction in which an acid and a base react completely, leaving only a salt and water, is referred to as a(n)

A)hydrolysis reaction.
B)neutralization reaction.
C)oxidation reaction.
D)None of the choices.

Question 51

Sodium phosphate can be used as a driveway degreaser.  When added to water, the following equilibrium is attained.  Sodium phosphate is acting as a(n)______. Na₃PO_{4 (aq)} + 3H₂O _(l) H₃PO_{4 (aq)} + 3OH^- _(aq)

A)Brønsted acid
B)Brønsted base
C)Arrhenius acid
D)Arrhenius base

Question 52

The dissociation reaction for the weak acid, H₂PO₃^- would be which of the following?

A)
B)
C)
D)

Question 53

How many meq are contained in 25.00 mL of a 0.225 M solution of CaCl₂?

A)5.62 × 10^-3 meq
B)2.81 meq
C)1.12 × 10^-2 meq
D)1.12 × 10¹ meq

Question 54

Which of the following would you expect to be a weak electrolyte?

A)acetic acid
B)sodium acetate
C)water
D)More than one answer is correct.

Question 55

The buffer capacity is the amount of ____ that can be absorbed without causing significant changes in pH.

A)acid
B)base
C)neither acid or base
D)either acid or base

Question 56

What is the p K _a of an acid with a K _a of 1.82 × 10 ^{− 5}?

A)4.74
B)− 4.74
C)9.26
D)− 9.26

Question 57

When a strong acid is added to a weak base and mixed, which of the following would not be produced?

A)conjugate acid
B)conjugate base
C)salt
D)water

Question 58

During a field trip to study the problem of acid rain, you test one lake that had observed a major fish kill.  It was found to have a pH of 5.37.  What is the [H⁺]?

A)2.3 × 10^-9
B)3.7 × 10^-5
C)4.3 × 10^-6
D)1.7 × 10⁵

Question 59

Consider the following list of p K _a values for a series of acids.  Which is the strongest acid?

A)5.74
B)3.21
C)10.6
D)Cannot be determined.

Question 60

A 10^-8 M solution of HCl is prepared.  It would be expected to be _____.

A)basic
B)acidic
C)neutral
D)insufficient information

Question 61

It has been proposed that atmospheric CO₂ could be reduced by absorption in to the Earth's oceans.  Which of the following reactions would be involved?

A)CO₂ (g)+ H₂O (l) H₂CO₃ (aq)
B)H₂CO₃ (aq) H⁺ (aq)+ HCO₃^- (aq)
C)HCO₃^- (aq)   H⁺ (aq)+ CO₃^2- (aq)
D)all of the above

Question 62

Sodium nitrate in water will produce a basic solution.

Question 63

pH changes can be determined with a(n)___.

A)pH meter
B)chemical indicator
C)indicating paper
D)all of these

Question 64

KOH is a strong base.

Question 65

The reason pure water has a pH of 7 is that there is the same concentration of hydrogen and hydroxide ions on the self-ionization of water.

Question 66

NaH₂PO₄ alone in a water solution could behave as a buffer.

Question 67

The salt of a strong acid with a strong base could behave as a buffer.

Question 68

Ammonium chloride in water will produce an acidic solution.

Question 69

According to the Brønsted Theory, a conjugate pair is composed of a Brønsted acid and a Brønsted base.

Question 70

When an inorganic acid and an inorganic base, as defined by Arrhenius, react, the products are salt and water.

Question 71

The pH of household ammonia is expected to be above 7 because household ammonia is NH₄OH.

Question 72

The salt of a strong acid and a weak base will give an acidic solution.

Question 73

The major difference between the Arrhenius Theory and the Brønsted Theory is that there is no hydrogen in the Brønsted Theory.

Question 74

NaCl is an example of a good buffer.

Question 75

The pH of a solution of baking soda, NaHCO₃, would be expected to be above 7.

Question 76

Nitric acid, HNO₃, is a weak acid.

Question 77

Most acids are weak acids.

Question 78

The salt of a weak base with a weak base could behave as a buffer.

Question 79

A Brønsted base is a proton donor.

Question 80

Solutions with a pH less than 7.00 are basic.