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CHEM1212 > TEST 3: 13, 14.1-14.6, 17.8-17.9 > Flashcards

TEST 3: 13, 14.1-14.6, 17.8-17.9 Flashcards

1
Q

If Kc is much less than one it favors

A

reactants

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2
Q

If Kc favors reactants

A

equilibrium shift to the left

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3
Q

Q>K

A

products>reactants, reactant favored, shift left

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4
Q

Q<K

A

reactants>products, product favored, shift right

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5
Q

When a reaction is product favored the shift will cause

A

concentration of products to increase and reactants to decrease

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6
Q

Homogeneous equilibrium

A

in the same phase, excludes concentration of pure solids and liquids

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7
Q

Heterogeneous equilibrium

A

not in the same phase, excludes concentration of pure solids and liquids

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8
Q

In a reactant favored reaction, the rate of the forward

A

is slower than rate of reverse

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9
Q

A reaction will proceed forward

A

when Q<K, reactants converted to products

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10
Q

A reaction will proceed in the reverse

A

when Q>K, products converted to reactants

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11
Q

K»1

A

product favored

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12
Q

K«1

A

reactants favored

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13
Q

If Q<K gibbs free energy

A

is negative regardless of gibbs under standard conditions

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14
Q

What causes a change in Gibbs free energy to shift with equilbrium?

A

A concentration-gradient reflected in the fact that the change in entropy under non-standard conditions is not the change in entropy under standard conditions–remember the natural tendency to disperse evenly throughout a system

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15
Q

Change in instantaneous gibbs free energy that is positive

A

Q>K

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16
Q

Negative change in instantaneous gibbs free energy

A

reaction is not at equilibrium

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17
Q

When standard conditions are restored from equilibrium, the value of Q progressively decreases. This must mean that we have

A

standard change in gibbs free energy that is negative

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18
Q

Reversible reactions do not

A

go to completion

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19
Q

At equilibrium

A

no net change in concentration, rate forward = rate reverse, these reactions do not stop

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20
Q

A reaction will essentially go to completion if

A

K > 10^10

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21
Q

A reaction will essentially not occur if

A

K < 10^-10

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22
Q

What are not included in equilibrium constant expressions

A

solids and liquid

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23
Q

Kc does not depend on

A

initial concentrations

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24
Q

Kc changes when

A

temperature changes, directly related

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25
Q

Things to check when doing equilibrium constant calculations

A

Is it balanced? Are there solids or liquids? Are equilibrium concentrations given and not initial concentrations?

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26
Q

When volume is decreased

A

pressure increases and reaction shifts to less gas

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27
Q

La Chatelier

A

system changes rates

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28
Q

Shift right will cause

A

increase reactants, decrease products, rate forward increase

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29
Q

Shift left will cause

A

decrease reactants, increase products, rate reverse increase

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30
Q

Decrease pressure

A

shift right

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31
Q

Consider heat

A

reactant in endothermic, product in exo

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32
Q

Add heat in exo

A

shift left, heat added to products and temp increased

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33
Q

Add heat in endo

A

shift right, heat added to reactants

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34
Q

Equation free energy and Kq

A

delta G°= -RTlnK

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35
Q

R in delta G° equation

A

0.008314 kJ / mol

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36
Q

ΔG° < 0

A

K>1, products

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37
Q

ΔG° > 0

A

K< 1, reactants

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38
Q

Equation relating Q and free energy

A

ΔG = ΔG° + RTlnQ
ΔG = -RTlnK + RTlnQ

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39
Q

ΔG < 0

A

K > Q, products

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40
Q

ΔG > 0

A

K < Q, reactants

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41
Q

PH =

A

-log[H+]

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42
Q

Increasing Ka

A

increasing acidity

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43
Q

When the concentration of hydroxide ions is. less than hydronium ions

A

acidic

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44
Q

How to find the concentration of hydronium ions from hydroxide ions?

A

(1.0x10^-14) / given concentration

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45
Q

Hydronium ion

A

H3O+ ion, a hydrated proton

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46
Q

Conjugate base

A

everything that remains of the acid molecule after a proton is lost

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47
Q

Conjugate acid

A

formed when the proton is transferred to the base

48
Q

Ka equation

A

[H3O+] [A-] / [HA]

49
Q

Acid dissolved in water equation:

A

HA (aq) + H2O (l) -> H3O+ (aq) + A- (aq)

50
Q

Ka definition

A

association dissociation constnat

51
Q

Strong acid

A

equilibrium lies far to the right, almost all HA ionized

52
Q

What do strong acids yield

A

a weak conjugate base (low proton affinity)

53
Q

Weak acid

A

equilibrium lies far to the right, dissociates only to a very small extent

54
Q

Weak acid is a conjugate base that is

A

much strong base than water

55
Q

Oxyacids

A

weak acid, phosphoric acid, nitrious acid, hypochlorous acid

56
Q

Organic acids

A

carbon atom backbone, contain carboxyl group, usually weak

57
Q

Organic acid examples

A

acetic acid, benzoic acid

58
Q

Autoionization of water equation

A

2H2O (l) -> H3O+ (aq) + OH- (aq)

59
Q

Kw equation

A

[H3O+] [OH-] = [H+] [OH-]

60
Q

in pH [H+] =

A

1.0 x 10^-7 <

61
Q

Arrhenius Acid

A

contain hydrogen and increase H+ ion concentration in solutions

62
Q

Arrhenius Base

A

contain hydroxide and increase OH- concentration in solutions

63
Q

Bronsted-Lowry acid

A

donates proton H+ to some accepting species

64
Q

Bronsted-Lowry base

A

chemical species accepts proton H+ from donating species

65
Q

Bronsted-Lowry equation

A

reactions are reversible, acids on one side can be a base on the other side

66
Q

All acids or bases can be classified

A

as lewis acids or bases

67
Q

Conjugate acid and base

A

acids and bases ionize and separate from their protons or hydroxides and leave behind these

68
Q

Water acts as an

A

amphoteric, can be acid or base, frequent conjugate of both acids and bases

69
Q

Water ionization constant Kw

A

= 1.o x 10^-14 at 25 degrees

70
Q

If H3O+ concentration is higher than OH-

A

solution is an acid

71
Q

pH for H3O+

A

-log[H3O+]

72
Q

pH for OH-

A

-log[OH-]

73
Q

[H3O+] related to pH

A

10^-pH

74
Q

A Ka and Kb much greater than one

A

strong acid or base

75
Q

A high PKa and PKb show

A

a low percentage ionization

76
Q

A low PKa and PKb show

A

a high percentage ionization

77
Q

PKa and PKb =

A

-log

78
Q

Strong Acids phrase

A

So I BRough No CLean CLOthes

79
Q

Strong Bases Remember

A

metal cations in group 1 (without Fr), and heavy group 2 metals (without Ra)

80
Q

If acid concentration is more an 100 x Ka

A

“X” in HA-X can be ignored

81
Q

Standard Free energy

A

tells whether product or reactant favored

82
Q

Change in free energy

A

to reach equilibrium how will the reaction have to shift

83
Q

ΔG° compares

A

G to 0 and K to 1

84
Q

ΔG compares

A

Q to K

85
Q

Degree of ionization a

A

a = [Molarity of the Conjugate Base of HA] / [Initial Molarity of HA]
a = [Molarity of Conjugate Base of HB] / [Initial Molarity of B]

86
Q

Percent ionization =

A

a x 100

87
Q

For weak acids, percent ionization increases with

A

increasing dilution

88
Q

Strong acids and bases degree of ionization =

A

100%

89
Q

Stronger the acid

A

weaker conjugate base

90
Q

Large Kb
Small Ka

A

strong base
weak conjugate acid

91
Q

Small Kb
Large Ka

A

weak base
strong conjugate acid

92
Q

Small Kb
Large Ka

A

weak base
strong conjugate aci

93
Q

Use Ka or Kb for acid and base to find X

A

Ka

94
Q

Which are ignored for strong bases

A

Na+ and K+

95
Q

Which are ignored for strong acids

A

Cl- and NO3-

96
Q

When are strong acids and water ionized

A

Strong acids completely ionize first and then water

97
Q

When H3O+ concentration > OH- concentration

A

Acidic

98
Q

A large pKa

A

weak acid, pH is still acidic

99
Q

When finding overall Kc, the Kc of each reaction

A

MULTIPLIED not added

100
Q

Adding inert gas at constant pressure

A

shift to side with more moles of gas

101
Q

Adding inert gas at constant volume

A

no effect

102
Q

Percent dissociation

A

amount dissociated / initial concentration x100%

103
Q

All acid base reactions favor

A

direction where strong acid or base react to form weaker acid or base

104
Q

Strong acid with strong base

A

Large equilibrium constant, water and neutral salt as product, neutral effect on solution

105
Q

Strong acid with weak base

A

Large equilibrium constant, water and acidic salt as products, acidic effect on solution

106
Q

Weak acid with strong base

A

Large equilibrium constant, water and basic salt as products, basic effect on solution

107
Q

Weak acid with weak base

A

Small equilibrium constant, water and salt as products whose pH depends on strength of conj acid and base present, effect on solution depends on pH

108
Q

pH and temperature

A

inversely proportional

109
Q

Kw and temperature

A

directly proportional

110
Q

Strong acids completely dissociate so

A

given M you know that -log will be pH

111
Q

If a base or acid is % dissociated (in ICE chart)

A

the % x M is the Change in ICE table

112
Q

The conjugate of a strong acid

A

is a very weak base

113
Q

K value increase or decrease with increase in temperature

A

decrease (does not change with P or V)

114
Q

Amphoteric example

A

HPO4 2-

115
Q

As temperature and Q increase, how does G change

A

increases

CHEM1212 (5 decks)

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