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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

(115 cards)

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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
Things to check when doing equilibrium constant calculations
Is it balanced? Are there solids or liquids? Are equilibrium concentrations given and not initial concentrations?
26
When volume is decreased
pressure increases and reaction shifts to less gas
27
La Chatelier
system changes rates
28
Shift right will cause
increase reactants, decrease products, rate forward increase
29
Shift left will cause
decrease reactants, increase products, rate reverse increase
30
Decrease pressure
shift right
31
Consider heat
reactant in endothermic, product in exo
32
Add heat in exo
shift left, heat added to products and temp increased
33
Add heat in endo
shift right, heat added to reactants
34
Equation free energy and Kq
delta G°= -RTlnK
35
R in delta G° equation
0.008314 kJ / mol
36
ΔG° < 0
K>1, products
37
ΔG° > 0
K< 1, reactants
38
Equation relating Q and free energy
ΔG = ΔG° + RTlnQ ΔG = -RTlnK + RTlnQ
39
ΔG < 0
K > Q, products
40
ΔG > 0
K < Q, reactants
41
PH =
-log[H+]
42
Increasing Ka
increasing acidity
43
When the concentration of hydroxide ions is. less than hydronium ions
acidic
44
How to find the concentration of hydronium ions from hydroxide ions?
(1.0x10^-14) / given concentration
45
Hydronium ion
H3O+ ion, a hydrated proton
46
Conjugate base
everything that remains of the acid molecule after a proton is lost
47
Conjugate acid
formed when the proton is transferred to the base
48
Ka equation
[H3O+] [A-] / [HA]
49
Acid dissolved in water equation:
HA (aq) + H2O (l) -> H3O+ (aq) + A- (aq)
50
Ka definition
association dissociation constnat
51
Strong acid
equilibrium lies far to the right, almost all HA ionized
52
What do strong acids yield
a weak conjugate base (low proton affinity)
53
Weak acid
equilibrium lies far to the right, dissociates only to a very small extent
54
Weak acid is a conjugate base that is
much strong base than water
55
Oxyacids
weak acid, phosphoric acid, nitrious acid, hypochlorous acid
56
Organic acids
carbon atom backbone, contain carboxyl group, usually weak
57
Organic acid examples
acetic acid, benzoic acid
58
Autoionization of water equation
2H2O (l) -> H3O+ (aq) + OH- (aq)
59
Kw equation
[H3O+] [OH-] = [H+] [OH-]
60
in pH [H+] =
1.0 x 10^-7 <
61
Arrhenius Acid
contain hydrogen and increase H+ ion concentration in solutions
62
Arrhenius Base
contain hydroxide and increase OH- concentration in solutions
63
Bronsted-Lowry acid
donates proton H+ to some accepting species
64
Bronsted-Lowry base
chemical species accepts proton H+ from donating species
65
Bronsted-Lowry equation
reactions are reversible, acids on one side can be a base on the other side
66
All acids or bases can be classified
as lewis acids or bases
67
Conjugate acid and base
acids and bases ionize and separate from their protons or hydroxides and leave behind these
68
Water acts as an
amphoteric, can be acid or base, frequent conjugate of both acids and bases
69
Water ionization constant Kw
= 1.o x 10^-14 at 25 degrees
70
If H3O+ concentration is higher than OH-
solution is an acid
71
pH for H3O+
-log[H3O+]
72
pH for OH-
-log[OH-]
73
[H3O+] related to pH
10^-pH
74
A Ka and Kb much greater than one
strong acid or base
75
A high PKa and PKb show
a low percentage ionization
76
A low PKa and PKb show
a high percentage ionization
77
PKa and PKb =
-log
78
Strong Acids phrase
So I BRough No CLean CLOthes
79
Strong Bases Remember
metal cations in group 1 (without Fr), and heavy group 2 metals (without Ra)
80
If acid concentration is more an 100 x Ka
"X" in HA-X can be ignored
81
Standard Free energy
tells whether product or reactant favored
82
Change in free energy
to reach equilibrium how will the reaction have to shift
83
ΔG° compares
G to 0 and K to 1
84
ΔG compares
Q to K
85
Degree of ionization 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
Percent ionization =
a x 100
87
For weak acids, percent ionization increases with
increasing dilution
88
Strong acids and bases degree of ionization =
100%
89
Stronger the acid
weaker conjugate base
90
Large Kb Small Ka
strong base weak conjugate acid
91
Small Kb Large Ka
weak base strong conjugate acid
92
Small Kb Large Ka
weak base strong conjugate aci
93
Use Ka or Kb for acid and base to find X
Ka
94
Which are ignored for strong bases
Na+ and K+
95
Which are ignored for strong acids
Cl- and NO3-
96
When are strong acids and water ionized
Strong acids completely ionize first and then water
97
When H3O+ concentration > OH- concentration
Acidic
98
A large pKa
weak acid, pH is still acidic
99
When finding overall Kc, the Kc of each reaction
MULTIPLIED not added
100
Adding inert gas at constant pressure
shift to side with more moles of gas
101
Adding inert gas at constant volume
no effect
102
Percent dissociation
amount dissociated / initial concentration x100%
103
All acid base reactions favor
direction where strong acid or base react to form weaker acid or base
104
Strong acid with strong base
Large equilibrium constant, water and neutral salt as product, neutral effect on solution
105
Strong acid with weak base
Large equilibrium constant, water and acidic salt as products, acidic effect on solution
106
Weak acid with strong base
Large equilibrium constant, water and basic salt as products, basic effect on solution
107
Weak acid with weak base
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
pH and temperature
inversely proportional
109
Kw and temperature
directly proportional
110
Strong acids completely dissociate so
given M you know that -log will be pH
111
If a base or acid is % dissociated (in ICE chart)
the % x M is the Change in ICE table
112
The conjugate of a strong acid
is a very weak base
113
K value increase or decrease with increase in temperature
decrease (does not change with P or V)
114
Amphoteric example
HPO4 2-
115
As temperature and Q increase, how does G change
increases

CHEM1212 (5 decks)

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