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Gen Chemistry 1 > Gen Chem Final Exam > Flashcards

Gen Chem Final Exam Flashcards

1
Q

3How can the value of Kc be calculated?

A

Using the equilibrium concentrations of reactants and products.

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2
Q

What does a small Kc value distinguish?

A

More reactants than products.
- little reaction takes place

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3
Q

What does a large Kc value distinguish?

A

More products than reactants
- reaction is essentially complete

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4
Q

What does it mean when the Kc = 1?

A

Reactants = Products
- moderate reaction

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5
Q

What does the size of the equilibrium constant not affect?

A

How fast the equilibrium is reached.

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6
Q

Reaction Quotient (Qc)

A

Qc = [products]/[reactants]
- same as Kc

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7
Q

What happens if Qc=Kc?

A

-Reactant and product concentrations are equilibrium concentrations

-Reaction mixture is at equilibrium

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8
Q

What happens if Qc≠Kc?

A

-Reactant concentrations are NOT equilibrium concentrations

-Reaction mixture is NOT at equilibrium

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9
Q

Le Chatelier’s Principle

A

When a stress (a change) is placed on a reaction at equilibrium.

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10
Q

How does the system respond to stress (changes)?

A

Momentarily changing the rate of the forward/reverse reaction in the direction.

= Relieves that stress until the equilibrium is re-established

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11
Q

What happens to the rate of reaction when more reactant is added?

A

Rate of forward reaction increases to form more products until the system re-establishes equilibrium.

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12
Q

What happens to the equilibrium when more reactants are added?

A

The equilibrium shifts toward the products (forward direction)

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13
Q

What happens to the rate of reaction when reactant is removed?

A

Rate of the reverse reaction increases to form more reactant until the system re-establishes the equilibrium.

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14
Q

What happens to the equilibrium when reactants are removed?

A

The equilibrium shifts toward the reactants (reverse direction)

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15
Q

What happens to the rate of reaction when more product is added?

A

Rate of the reverse reaction increases to consume the product until the system re-establishes the equilibrium

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16
Q

What happens to the equilibrium when more products are added?

A

The equilibrium shifts toward the reactants (reverse direction)

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17
Q

What happens to the rate of reaction when product is removed?

A

The rate of the forward reaction increases to form more products until the system re-establishes equilibrium.

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18
Q

What happens to the equilibrium when products are removed?

A

The equilibrium shifts toward the products (forward direction).

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19
Q

What does changing the volume of a gas mixture at equilibrium cause?

A

Change in the concentration of gases in the mixture

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20
Q

What happens to the pressure of a mixture when the volume is decreased?

A

The pressure increases

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21
Q

What happens to the concentration of a mixture when the volume is decreased?

A

The concentration increases

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22
Q

What happens to the equilibrium when the volume is decreased?

A

The equilibrium shifts in the direction of the smaller number of moles to compensate.

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23
Q

What happens to the pressure of a mixture when the volume is increased?

A

The pressure decreases

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24
Q

What happens to the concentration of a mixture when the volume is increased?

A

The concentration decreases

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25
Q

What happens to the equilibrium when the volume is increased?

A

The equilibrium shifts in the direction of the larger number of moles to compensate.

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26
Q

What effect does volume/pressure change have on a reaction with the same amount of reactants and products?

A

NO EFFECT

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27
Q

What happens to the rate of reaction when temperature is increased in ENDOTHERMIC reactions?

A

The rate of the forward reaction increases to consume the added heat energy until the system re-establishes equilibrium.

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28
Q

What happens to the equilibrium when temperature is increased in ENDOTHERMIC reactions?

A

The equilibrium shifts toward the products (forward direction)

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29
Q

What happens to the rate of reaction when temperature is decreased in ENDOTHERMIC reactions?

A

The rate of the reverse reaction increases to generate more heat energy until the system re-establishes the equilibrium.

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30
Q

What happens to the equilibrium when temperature is decreased in ENDOTHERMIC reactions?

A

The equilibrium shifts toward the reactants (reverse direction).

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31
Q

What happens to the rate of reaction when temperature is increased in EXOTHERMIC reactions?

A

The rate of the reverse reaction increases to consume the added heat energy until the system re-establishes the equilibrium.

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32
Q

What happens to the equilibrium when temperature is increased in EXOTHERMIC reactions?

A

The equilibrium shifts toward the reactants (reverse direction).

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33
Q

What happens to the rate of reaction when temperature is decreased in EXOTHERMIC reactions?

A

The rate of the forward reaction increases to generate more heat until the system re-establishes the equilibrium.

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34
Q

What happens to the equilibrium when temperature is decreased in EXOTHERMIC reactions?

A

The equilibrium shifts toward the products (forward direction)

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35
Q

How does the addition of a catalyst affect the rate of reaction?

A

Speeds up a reaction by lowering the activation energy, which increases the rate of the forward and reverse reactions equally.

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36
Q

Are the ratios of reactants and products changed when a catalyst is added?

A

No; only the time to reach equilibrium is shorter

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37
Q

Does the addition of a catalyst shift the equilibrium?

A

No

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38
Q

What are the 5 properties of acids?

A
  1. Have a sour taste
  2. Have a stinging feel
  3. Turn litmus paper red
  4. Neutralize bases
  5. Corrode some metals
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39
Q

What are the 4 properties of bases?

A
  1. Have bitter (chalky) taste
  2. Have a soapy (slippery) feel
  3. Turn litmus paper blue
  4. Neutralize acids
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40
Q

What is the rule of naming a hydrogen ion and nonmetal?

A
  • Use the prefix “hydro”
  • End with “ic acid”

Example:
Hydrochloric Acid

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41
Q

What is the rule of naming a hydrogen ion and polyatomic group?

A

If it ends in “ate”

add “ic acid” to the end

add “ous acid” to the end

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42
Q

What is the exception to naming acids?

A

HCN: Hydrocyanic Acid
- Only follows rule 1

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43
Q

How do you name bases?

A

Add “hydroxide” to the end of the first element

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44
Q

What is the exception to naming bases?

A

NH3: Ammonia

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45
Q

Monoprotic Acids

A

Have only one reactive H+ that can be donated.

46
Q

Diprotic Acids

A

Have two reactive H+ that can be donated

47
Q

Triprotic Acids

A

Have three reactive H+ that can be donated

48
Q

Do all hydrogen ions react?

A

NO

49
Q

How can bases be categorized?

A
  • Monobasic
    -Dibasic
    -Tribasic
    (based on the number of OH- ions)
50
Q

Are categorizing bases or acids more common?

A

Acids

51
Q

What are acids and bases both considered?

A

Electrolytes

52
Q

Why are acids and bases considered electrolytes?

A

They produce ions when dissolved in water.

53
Q

Arrhenius Definition of Acids

A

Acids produce hydrogen ions when dissolved in water.

54
Q

Arrhenius Definition of Bases

A

Bases produce hydroxide ions when dissolved in water

55
Q

What is distinct about ammonia and forming hydroxide ions?

A

Ammonia tests as a base but does not have OH- in the formula.

56
Q

What is a problem with the Arrhenius definition of bases and acids?

A

The definition is too narrow

57
Q

Bronsted-Lowry Definition of Acids

A

Acids donate hydrogen ions/protons when dissolved in water
- lose H+

58
Q

What does the Bronsted-Lowry Definition of Acids expand on?

A

The Arrhenius definition of bases and acids

59
Q

What hydronium ion should we know?

A

H3O+

60
Q

Hydronium Ions

A

H+ bonded to a water molecule

61
Q

Bronsted-Lowry definition of bases

A

Bases accept hydrogen ions/protons when dissolved in water
- Gain H+

62
Q

What is the Bronsted-Lowry Theory summarized?

A
  • An acid is a substance that loses H+
  • A base is a substance that gains H+
63
Q

Amphoteric Substances

A

Have the capability to act as both acids and bases in the solution

64
Q

What are the 3 most common examples of amphoteric substances?

A
  1. HCO3-
  2. H2O
  3. HPO4 2-
64
Q

When do amphoteric substances act as an acid?

A

When they react with a stronger base.

64
Q

When do amphoteric substances act as a base?

A

When they react with a stronger acid.

64
Q

Strong Acids

A

Completely dissociates into ions in aqueous solutions.

65
Q

What are strong acids also known as?

A

Strong electrolytes

66
Q

What arrow is used in a chemical reaction with strong acids?

A

Forward facing arrow

67
Q

What are the 6 common strong acids?

A
  1. HCl
  2. HBr
  3. HI
  4. HNO3
  5. HClO4
  6. H2SO4
68
Q

Weak Acids

A

Dissociates only slightly in water to form few ions in aqueous solutions

69
Q

What are weak acids also known as?

A

Weak electrolytes

70
Q

What arrow is used in a chemical reaction with weak acids?

A

Double arrow

71
Q

What do we refer to an acid as when it is not apart of the strong acid list?

A

A weak acid

72
Q

Strong Bases

A

Completely dissociate into ions in aqueous solutions

73
Q

What are strong bases also known as?

A

Strong electrolytes

74
Q

What are the 8 most common strong bases?

A
  1. LiOH
  2. NaOH
  3. KOH
  4. RbOH
  5. CsOH
  6. Ba(OH)2
  7. Sr(OH)2
  8. Ca(OH)2
75
Q

Weak Base

A

Ionizes only slightly in water to form a few ions in an aqueous solution

76
Q

What are stronger acids correlated with?

A

Weaker conjugate bases

77
Q

What are stronger bases correlated with?

A

Weaker conjugate acids

78
Q

What do aqueous reactions favor?

A

The direction from stronger chemical species to weaker chemical species.

79
Q

What is meant when the product side of a reaction is favored?

A

Favors forward direction of equation

More products than reactants

80
Q

What is meant when the reactant side of a reaction is favored?

A

Favors reverse direction of equation

More reactants than products

81
Q

Reversible Reactions

A

Dissociations of weak acids and bases

82
Q

Ka and Kb Formula

A

[products] / [reactants]

83
Q

What is not included in the Ka and Kb formulas?

A

Pure solids (s) and liquids (l)

84
Q

What is correlated with a Ka/Kb value less than 1?

A

Favors reverse reaction
- more reactants

85
Q

What is correlated with a Ka/Kb value greater than 1?

A

Favors forward reaction
- more products

86
Q

What is correlated with a Ka/Kb value equal to 1?

A

Equilibrium
- same number of products and reactants

87
Q

The larger the Ka value…

A

the stronger the acid

88
Q

The larger the Kb value…

A

the stronger the base

89
Q

pKa formula

A

-log(Ka)

90
Q

The smaller the pKa value…

A

the stronger the acid

91
Q

What can two water molecules react to produce?

A

H3O+ and OH-

92
Q

When there is a reaction with two water molecules, water acts as…

A

Both an acid and a base (amphoteric)

93
Q

Kw

A

Water Dissociation Constant

94
Q

What is the solution called when H3O+ and OH- concentrations are equal?

A

Neutral Solution

95
Q

What is the solution called when the H3O+ concentration is larger than OH-?

A

Acidic Solution

96
Q

What is the solution called when the OH- concentration is larger than the H3O+?

A

Basic Solution

97
Q

What is used to describe the acidity/basicity of solutions?

A

The pH scale

98
Q

What can be used. to determine the pH of a solution?

A
  1. pH meter (probe in solution)
  2. pH paper (paper with dye)
  3. Indicators that turn different colors corresponding to different pH values
99
Q

What is the formula for pH?

A

pH = -log [H3O+]

100
Q

Does pH have any units?

A

No

101
Q

What does the change of 1 pH unit correspond to?

A

A tenfold change in H3O+ .

102
Q

As pH decreases…

A

H3O+ increases
(negative log scale)

103
Q

What values does the pH scale range from?

A

0-14

104
Q

When is the pH of a solution acidic?

A

Values less than 7

105
Q

When is the pH of a solution neutral?

A

Value = 7

106
Q

When is the pH of a solution basic?

A

Values greater than 7

107
Q

How do you find the given H3O+ value when you have the pH value?

A

Anti-log = 10^(-pH)

Gen Chemistry 1 (10 decks)

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