Deck 9: Acids, bases, and Salts

Question 1

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

A)H⁺
B)OH^-
C)H₃O⁺
D)

Answer 1

H⁺

Question 2

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.

Answer 2

The ion serves as the conjugate base of the acid,H₃C₆H₅O₇.

Question 3

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

Answer 3

HIO₃ and H₃O⁺

Question 4

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 5

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

A)Na₂CO₃
B)Na₃PO₄
C)K₂S
D)KOH

Question 6

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

Question 7

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 8

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 9

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 10

Which of the following is present in pure water?

A)H₃O⁺
B)OH ^-
C)H₂O
D)all of them

Question 11

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

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

Question 12

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

A)Li₂S
B)LiSO₄
C)Li₂SO₄
D)Li₂CO₃

Question 13

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 14

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 15

The molar concentration of OH in a water solution is 1.0 * 10^-9.The pH of the solution is _____ .

A)9.00
B)5.00
C)> 9.00
D)< 5.00

Question 16

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 17

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 18

A solution for which [H⁺] = 1.0 *10^-3 will have a pH of _____ .

A)"5.00"
B)"3.00"
C)"-05.00"
D)"-9.00"

Question 19

Some salts isolated by evaporation retain water that is called

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

Question 20

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

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

Question 21

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 22

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 23

Which salt shifts the pH when dissolved in water?

A)KCl
B)Al(NO₃)₃
C)NaCl
D)NaNO₃

Question 24

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 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

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 27

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 28

Identify the substance with the lowest pH.

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

Question 29

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 30

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 *10sup>-⁵

Question 31

A higher pH corresponds to _____ .

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

Question 32

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 33

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 34

Which of the following is a weak acid?

A)HNO₃
B)HCl
C)H₂CO₃
D)H₂SO₄

Question 35

How many equivalents are contained in 0.25 moles of H₂SO₄?

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

Question 36

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 37

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.

Question 38

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 39

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 40

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 41

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

A)
B)
C)
D)

Question 42

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 43

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 44

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 45

HCl will react with

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

Question 46

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 47

What is the pK_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 48

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 49

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

A)
B)
C)
D)

Question 50

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 51

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 52

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 53

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 54

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 55

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 56

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 57

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 58

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 59

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 60

Consider the following list of pK_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 61

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

Question 62

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 63

KOH is a strong base.

Question 64

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

Question 65

Seageroic acid has a pK_a of 8.23,whereas slabaughic acid has a pK_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 66

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

Question 67

Sodium nitrate in water will produce a basic solution.

Question 68

Solutions with a pH less than 7.00 are basic.

Question 69

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

Question 70

Nitric acid,HNO₃,is a weak acid.

Question 71

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

Question 72

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

Question 73

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 74

Ammonium chloride in water will produce an acidic solution.

Question 75

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

Question 76

A Brønsted base is a proton donor.

Question 77

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

Question 78

NaCl is an example of a good buffer.

Question 79

Most acids are weak acids.

Question 80

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

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