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Chemistry 2 > Chapter 16 Acids & Bases > Flashcards

Chapter 16 Acids & Bases Flashcards

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1
Q

Define Acid

A

Sour taste; has the ability to dissolve many metals, neutralize bases, turns blue litmus paper red and has a pH under 7

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2
Q

Define Base

A

Bitter taste and slippery feel; has the ability to neutralize acids, turns red litmus paper blue and has a pH above 7

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3
Q

Define Arrhenius Acid

A

Acids are substances that produces H+ ions (proton) in an aqueous solution

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4
Q

Define Arrhenius Base

A

Bases are substances that produces OH- ions in an aqueous solution

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5
Q

Define Neutralization

A

Acids and bases that combine to form water

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6
Q

Define Bronsted-Lowry Acid

A

Proton (H+ ion) donor

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7
Q

Define Bronsted-Lowry Base

A

Proton (H+ ion) acceptor

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8
Q

In the Bronsted-Lowry Acid-Base theory how are Acids and Bases defined?

A

In this theory acids and bases are defined by the way they react with each other

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9
Q

Define Amphoteric

A

Substances that can act as acids or bases

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10
Q

What element can be an example of an Amphoteric substance?

A

H2O

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11
Q 
Identify which of the substances are Acids and which are Bases
I) KOH (aq) 
II) HNO3 (aq) 
III) CH3COOH (aq) 
IV) HBR (aq) 
V) NH4+ (aq) 
VI) Sr(OH)2 (aq) 
VII) H2SO4 (aq)
A 
I) Base 
II) Acid
III) Acid 
IV) Acid
V) Acid
VI) Base 
VII) Acid
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12
Q

Define Conjugate Acid Base Pair

A

2 substances related to each other by the transfer of a proton

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13
Q

A Conjugate Acid Base Pair only differs by ____ _______

A

1 proton

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14
Q

A base accepts a proton and becomes a ___________ ______

A

Conjugate Acid

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15
Q

An acid donates a proton and becomes a ____________ ______

A

Conjugate Base

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16
Q

The original base becomes a _________ _______ in the reverse reaction and the original acid becomes a _________ _________ in the reverse reaction

A

Conjugated acid; conjugated base

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17
Q 
Write out the Conjugate Acids for each base 
I) NH3+ 
II) OH-
III) H2O 
IV) CO3 2-
A

I) NH4+
II) H2O+
III) H3O+
IV) HCO3 -

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18
Q 
Write out the Conjugate Bases for each acid
I) HCl 
II) HBr 
III) HNO3 
IV) CH3COOH
A

I) Cl-
II) Br-
III) NO3-
IV) CH3COO-

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19
Q

Write the Conjugate Acids for each base
I) ClO4-
II) HSO4-
III) H2PO4

A

I) HClO4
II) H2SO4
III) H3PO4

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20
Q

Write the Conjugate Bases for each acid
I) H2SO3
II) HCHO2
III) HF

A

I) HSO3-
II) HCOO-
III) F-

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21
Q

What does the Lewis definition of acids and bases focus on?

A

The transfer of electron pairs

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22
Q

Define Lewis Acid

A

Electron pair acceptor

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23
Q

Define Lewis Base

A

Electron pair donor

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24
Q

What are the types of Lewis acids and bases?

A

I) Incomplete octet
II) Molecules that contain double bonds
III) Small and highly charged cations that have empty orbitals allowing them to act as Lewis acids

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25
Q 
Identify the following as a Lewis Acid or Base 
I) Fe3+ 
II) BH3 
III) NH3 
IV) F- 
V) BeCl2 
VI) OH- 
VII) B(OH)3 
VIII) CN-
A 
I) Lewis Acid 
II) Lewis Acid 
III) Lewis Base 
IV) Lewis Base 
V) Lewis Acid 
VI) Lewis Base 
VII) Lewis Acid
VIII) Lewis Base
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26
Q

Define Strong Acid

A

An acid that completely ionizes in a solution

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27
Q

In regards to Strong Acids which way does the equilibrium lie?

A

The equilibrium lies far to the right with a single arrow

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28
Q

What are some examples of Strong Acids?

A
  • Hydrochloric Acid (HCl)
  • Hydrobromic Acid (HBr)
  • Hyrdoiodic Acid (HI)
  • Nitric Acid (HNO3)
  • Perchloric Acid (HClO4)
  • Sulfuric Acid (H2SO4)
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29
Q

For Strong Acids what is the [H3O+] value?

A

The [H3O+] value is the same as the acid initial

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30
Q

Define Weak Acid

A

An acid that only partially ionizes in a solution

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31
Q

In regards to Weak Acids which way does the equilibrium lie?

A

The equilibrium is double arrowed and lies both ways

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32
Q

What are some examples of Weak Acids?

A
  • Chlorous Acid (HClO2)
  • Nitrous Acid (HNO2)
  • Hydroflouric Acid (HF)
  • Formic Acid (HCHO2)
  • Benzoic Acid (HC7H5O2)
  • Acetic Acid (HC2H3O2)
  • Hypochlorous Acid (HClO)
  • Hydrocyanic Acid (HCN)
  • Phenol (HC6H5O)
  • Sulfurous Acid (H2SO3)
  • Carbonic Acid (H2CO3)
  • Phosphoric Acid (H3PO4)
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33
Q

For Weak Acids what is the [H3O+] value?

A

The [H3O+] value is smaller than the initial concentration of the acid

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34
Q

Strong Acids have ______ attractions and __________ ionization, Weak Acids have _______ attractions and ___________ ionization

A

Weak; complete, strong; partial

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35
Q

Define Acid Ionization (Dissociation) Constant (Ka)

A

The equilibrium constant for the ionization reaction of the weak acid

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36
Q

Larger Ka = ?

Smaller Ka = ?

A

Larger Ka = stronger weak acid

Smaller Ka = weaker weak acid

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37
Q

Define Autoionization

A

When a molecular can act as an acid and a base with itself

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38
Q

Define Ion Product Constant for Water (Kw)

A

The equilibrium constant for the Autoionization of water

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39
Q

Kw = ?

A

Kw = [H3O+][OH-] = 1.0x10^-14

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40
Q

The concentration of H3O+ times the concentration of OH- is always _____________ at ______ degrees celsius

A

1.0x10^-14, 25 degrees celsius

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41
Q

In acidic solutions is [H3O+] less than or greater than [OH-]

A

[H3O+] > [OH-]

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42
Q

In basic solutions is [H3O+] less than or greater than [OH-]

A

[H3O+] < [OH-]

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43
Q

If the concentration of [H3O+] increase what happens to the concentration of [OH-]

A

Concentration of [OH-] decreases

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44
Q

What are the equations used to find pH?

A
  • Kw = [H3O+][OH-]
  • pH = -log [H3O+]
  • pOH = -log [OH-]
  • pH + pOH = 14.00
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45
Q

What is the equation for finding pKa?

A

pKa = -logKa

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46
Q

The larger the Ka the ________ the pKa and the __________ the weak acid

A

Smaller, stronger

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47
Q

The smaller the Ka the __________ the pKa and the __________ the weak acid

A

Larger, weaker

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48
Q

How do you find [H3O+] and pH for a Strong Acid?

A

The concentration of [H3O+] for a strong acid = the concentration of the strong acid

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49
Q

How do you find [H3O+] and pH for a Weak Acid?

A

The concentration of [H3O+] for a weak acid does not equal the concentration of the strong acid, you must use an ICE Table to find [H3O+]

50
Q

T/F Strong Acids completely ionize in solutions however we must not ignore the contribution of the Autoionization of water

A

False; strong acids do completely ionize in solutions and we can also ignore the contribution of Autoionization of water

51
Q

T/F Weak acids are not equal to the concentrations of the weak acid since it does not ionize completely

A

True

52
Q

Define Percent Ionization

A

The ratio of the ionized acid concentration to the initial acid concentration, multiplied by 100%

53
Q

For 2 weak acids of the same initial concentration which one results in the higher Percent Ionization value?

A

The stronger weak acid results in higher Percent Ionization

54
Q

If the initial acid concentration increases what happens to the [H3O+] equilibrium and Percent Ionization?

A

[H3O+] equilibrium increases and Percent Ionization decreases

55
Q

If you have a Strong and a Weak Acid, which would you use to solve for pH?

A

The Strong Acid

56
Q

If you have 2 Weak Acids, which would you use to solve for pH?

A

You would use the stronger Weak Acid (the weak acid with the higher Ka)

57
Q

Define Strong Base

A

A base that completely dissociates in a solution

58
Q

T/F There are 2 groups of Strong Bases

A

True

59
Q

What is the difference between group 1 and group 2 Strong Bases?

A

Group 1: highly soluble

Group 2: slightly soluble

60
Q

What are the common Strong Bases in both group 1 and group 2?

A 
Group 1
- Lithium Hydroxide (LiOH) 
- Sodium Hydroxide (NaOH)
- Potassium Hydroxide (KOH) 
Group 2 
- Strontium Hydroxide (Sr(OH)2) 
- Calcium Hydroxide (Ca(OH)2) 
- Barium Hydroxide (Ba(OH)2)
61
Q

Define Weak Base

A

A base that produces OH- by accepting protons from water (ionizing water to form OH-)

62
Q

What is the main difference between Strong and Weak Bases?

A

Weak bases must accept protons from water to produce OH- whereas strong bases already contain OH and dissociate into water

63
Q

For Weak Bases is the [OH-] smaller, larger, or the same as the initial concentration of the base?

A

Smaller

64
Q

What are the common Weak Bases?

A
  • Methylamine (CH3NH2)
  • Ethylamine (C2H5NH2)
  • Pyridine (C5H5N)
  • Aniline (C6H5NH2)
  • Carbonate Ion (CO3 2-)
  • Bicarbonate Ion (HCO3-)
  • Ammonia (NH3)
65
Q

What is the Ionization Reaction of Methylamine (CH3NH2)

A

CH3NH2 (aq) + H2O (l) –> CH3NH3 (aq) + OH- (aq)

66
Q

What is the Ionization Reaction of Ethylamine (C2H5NH2)

A

C2H5NH2 (aq) + H2O (l) –> C2H5NH3 (aq) + OH- (aq)

67
Q

What is the Ionization Reaction of Pyridine (C5H5N)

A

C5H5N (aq) + H2O (l) –> C5H5NH (aq) + OH- (aq)

68
Q

What is the Ionization Reaction of Aniline (C6H5NH2)

A

C6H5NH2 (aq) + H2O (l) –> C6H5NH3 (aq) + OH- (aq)

69
Q

What is the Ionization Reaction of Carbonate Ion (CO3 2-)

A

CO3 2- (aq) + H2O (l) –> HCO3 (aq) + OH- (aq)

70
Q

What is the Ionization Reaction of Bicarbonate Ion (HCO3-)

A

HCO3- (aq) + H2O (l) –> H2CO3 (aq) + OH- (aq)

71
Q

What is the Ionization Reaction of Ammonia (NH3)

A

NH3 (aq) + H2O (l) –> NH4 (aq) + OH- (aq)

72
Q

What do all of the Weak Base pairs have in common?

A

All of the bases have a nitrogen atom and a lone pair

73
Q

Lone pairs act as a what?

A

Acts as a proton acceptor

74
Q

Define Base Ionization Constant (Kb)

A

The equilibrium constant for the ionization of a weak base

75
Q

The larger the Kb, the ___________ the pKb, and the ___________ the weak base

A

Smaller, stronger

76
Q

The smaller the Kb, the __________ the pKb, and the ___________ the weak base

A

Larger, weaker

77
Q

Define Salt

A

A chemical compound consisting of an assembly of cations and anions

78
Q

A cation can potentially serve as a __________ and an anion can potentially serve as a __________

A

Acid, base

79
Q

Think of any anion as the __________ ________ of an acid

A

Conjugate Base

80
Q

An anion thats conjugate base is weak acid =

A

Weak base

81
Q

An anion thats conjugate base is strong acid =

A

pH neutral

82
Q 
Classify each anion as a strong or weak acid and then identify the conjugate base 
I) Cl- 
II) F- 
III) NO3- 
IV) C2H3O2-
A

I) HCl, strong acid, pH neutral
II) HF, weak acid, weak base
III) HNO3, strong acid, pH neutral
IV) HC2H3O2, weak acid, weak base

83
Q

Classify each anion as a strong or weak acid and then identify the conjugate base
I) NO3-
II) C2H3O2-
III) I-

A

I) HNO3, strong acid, pH neutral
II) HC2H3O2, weak acid, weak base
III) HI, strong acid, pH neutral

84
Q 
Which of the following anions CANNOT act as a base?
I) F- 
II) NO2- 
III) C2H3O2- 
IV) CN- 
V) I-
A 
I) HF, weak acid 
II) HNO2, weak acid
III) HC2H3O2, weak acid 
IV) HCN, weak acid 
V) HI, strong acid (can't act as a base)
85
Q

What is the equation for finding pKb?

A

pKb = -logKb

86
Q

Which statement is false about acids and bases?
I) Arrhenius acid is a substance that produces H+ ions in aqueous solutions
II) Arrhenius base is a substance that produces OH- ions in aqueous solutions
III) Bronsted bases are considered as OH- acceptors
IV) H2O can act as an acid
V) H2O can act as a base

A

III is false; Bronsted bases are considered proton (H+ ion) acceptors

87
Q

What is the conjugate acid of C17H19NO3?

A

C17H20N03+

88
Q 
Which of the following is a conjugate acid-base pair? 
I) HI, NaOH
II) H3O+, OH+ 
III) H3PO4, PO4 3- 
IV) H2SO4, HSO4- 
V) NH3, NH4-
A

IV ; H2SO4, HSO4-

89
Q 
How many of these compounds are considered as Lewis Acids? 
I) Al3+ 
II) H2O 
III) NH4+ 
IV) CN- 
V) FeCl3 
VI) NH3
A

4 ; Al3+, H2O, NH4+ and FeCl3

90
Q

What is the most accurate and complete description of a Lewis Acid and Lewis Base respectively?
I) A proton donor and proton acceptor
II) A proton acceptor and proton donor
III) Electron donor and electron acceptor
IV) Electron acceptor and electron donor

A

IV ; Electron acceptor and electron donor

91
Q 
How many of the following are weak acids?
I) CH3COOH
II) HF
III) HCl
IV) HI 
V) H2SO4 
VI) HCOOH
A

3 ; CH3COOH, HF and HCOOH

92
Q 
How many of the following is/are weak bases?
I) CH3NH2 
II) NH3 
III) LiOH 
IV) C5H5N 
V) NaCl
A

3 ; CH3NH2, NH3 and C5H5N

93
Q

Which statement is incorrect about bases?
I) Strong bases completely dissociate in water and donate OH-
II) Weak bases produce OH- by accepting protons from water, ionizing water to form OH-
III) Most weak bases contain a lone pair and a nitrogen atom
IV) For weak bases, OH- is equal to the initial concentration of the base

A

IV

94
Q

What are the different ways of categorizing Cations?

A
  • Cations of strong bases
  • Cations of conjugated acids
  • Cations of highly charged metals
95
Q

Define Cations of Strong Bases

A

Cations that are the counterions of strong bases; results in pH neutral

96
Q

Define Cations of Conjugated Acids

A

Cations that are the conjugate acid of a weak base; results in weak acid

97
Q

Define Cations of Highly Charged Cations

A

Cations that are small and highly charged metals; results in weak acid

98
Q

What is an example of Highly Charged Cations?

A

Al3+ and Fe3+

99
Q

Classify each of the following as a weak acid or pH neutral
I) Ca2+
II) C5H5NH+
III) Cr3+

A

I) pH neutral
II) Weak acid
III) Weak acid

100
Q

What is the equation comparing the strength of Conjugate Acid-Base Pairs?

A

Ka x Kb = Kw

101
Q

The ____________ the acid, the ____________ the conjugate base (vise versa)

A

Stronger ; weaker

102
Q

Conjugate acid of a weak base results in a ________ Cation, paired with conjugate base of a strong acid results in a _________ Anion. Together resulting in __________

A

Acidic ; neutral ; acidic

103
Q

Small highly charged metal ion results in a ________ Cation, paired with conjugate base of a strong acid results in a _________ Anion. Together resulting in __________

A

Acidic ; neutral ; acidic

104
Q

Counterion of strong base results in a __________ Cation, paired with conjugate base of a strong acid results in a _________ Anion. Together resulting in __________

A

Neutral ; neutral ; neutral

105
Q

Conjugate acid of a weak base results in a _________ Cation, paired with conjugate base of a weak acid results in a _________ Anion. Together resulting in __________

A

Acidic ; basic ; would be acidic or basic depending on the relative strength

106
Q

Small highly charged metal ion results in a __________ Cation, paired with conjugate base of a weak acid results in a _________ Anion. Together resulting in __________

A

Acidic ; basic ; would be acidic or basic depending on the relative strength

107
Q

Counterion of strong base results in a __________ Cation, paired with conjugate base of a weak acid results in a _________ Anion. Together resulting in _________

A

Neutral ; basic ; basic

108
Q

Define Monoprotic Acid

A

Acid containing one ionizable proton

109
Q

What are some examples of Monoprotic Acids?

A

HF, HCl and HCOOH

110
Q

Define Diprotic Acids

A

Acids containing two ionizable protons

111
Q

What are some examples of Diprotic Acids?

A

H2SO4, H2SO3 and H2CO3

112
Q

Define Triprotic Acids

A

Acids containing three ionizable protons

113
Q

What are some examples of Triprotic Acids?

A

H3PO4

114
Q

Define Polyprotic Acids

A

Acids containing two or more ionizable protons

115
Q

In regards to Polyprotic Acids, will the successive Ka value following the first be smaller, larger or the same?

A

Smaller than the first Ka value

116
Q

Define Binary Acids

A

Acids that contain a Hydrogen and only one other element (nonmetal)

117
Q

What is the acid strength of Binary Acids?

A

Increases LEFT to RIGHT and TOP to BOTTOM

118
Q

Define Oxyacids

A

Acids that contain a Hydrogen atom bonded to an oxygen atom that is bonded to another element

119
Q

What is the acid strength of Oxyacids?

A

The GREATER the number of OXYGEN atoms bonded to the same Y the STRONGER the Oxyacid

120
Q

How do you determine the strength of Oxyacids with the same number of Oxygen atoms?

A

The MORE ELECTRONEGATIVE (to the right or to the top) the element Y, the STRONGER the Oxyacid

Chemistry 2 (10 decks)

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