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General chemistry II > Unit 3 (ch 15,17) > Flashcards

Unit 3 (ch 15,17) Flashcards

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1
Q

K»>1

A

favor product

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2
Q

K«<1

A

favor reactant

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3
Q

Does K have units?

A

no

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4
Q

K positive or negative?

A

positive

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5
Q

Kc=

A

[products]/[reactants]

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6
Q

Kp=

A

Pproducts/Preactants

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7
Q

Kc=Kp when

A

same number moles of gases

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8
Q

Kp=

A

Kc(RT)^delta n

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9
Q

K for the forward reaction = (blank) for the reverse

A

1/K

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10
Q

K overall =

A

K1xK2

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11
Q

If K is always at equilibrium, Q can be

A

any concentration

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12
Q

In non-equilibrium conditions find

A

Q

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13
Q

Q tells us

A

where we are relative to equilibrium and in which direction the reaction will proceed

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14
Q

Q

A

reaction to right/products/forward

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15
Q

If you go from a normal reaction to half the reaction, what process do you use?

A

K^1/2

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16
Q

Q=K

A

equilibrium

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17
Q

Q>K

A

reaction to left/reactants/reverse

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18
Q

Heterogeneous equilibrium

A

solid and liquid excluded

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19
Q

LeChatelier’s principle

A

stressed/preturbed reactions work to regain equilibrium

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20
Q

what is LC useful for?

A

drive reaction to form more products

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21
Q

Effect of pressure change

A

increase pressure favors side with fewer moles, decreasing favors side with more moles

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22
Q

increasing temp

A

help endo move forward and hinder exo

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23
Q

What do catalysts change?

A

time to reach equilibrium, not K

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24
Q

How can we determine how much K changes with T?

A

ln(K2/K1)= delta H/R(1/T2-1/T1)

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25
Q

if you have a strong acid or base, the concentration of the acid or base will be

A

same as concentration of ions it dissociates into

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26
Q

is water included in Ka expressions?

A

no

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27
Q

What is equilibrium?

A

rate forward= rate reverse

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28
Q

What happens to concentrations and reaction rates when equilibrium is reached?

A

concentrations of reactants and products remain constant over time and the rate of a reaction in the forward matches reverse

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29
Q

How do we arrive at the relationship for the equilibrium constant, K?

A

Rate law forward/rate law reverse

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30
Q

What information does K»>1 or K«<1 give us about the ratio of products and reactants?

A

K»1, concentrations of products larger than reactant

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31
Q

What are the effects of volume changes?

A

-increase volume shifts equilibrium toward side of reaction with moles of gas

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32
Q

How can we relate K to enthalpy, entropy, and free energy?

A

value of K decreases as temp increase for exo

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33
Q

What are acids according to the Bronsted-Lowry definition?

A

acids donate protons (H+)

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34
Q

What are bases according to the Bronsted-Lowry definition?

A

bases accept protons (H+)

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35
Q

What is the difference between a strong and weak acid?

A

strong acid fully dissociates

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36
Q

What is the difference between a strong and weak base?

A

strong base fully dissociates

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37
Q

How do we calculate Ka for an acid?

A

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

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38
Q

Kb=

A

[HB+][OH-]/[B]

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39
Q

strong base kb

A

> > 1

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40
Q

fewer moles in products, (blank) pressure

A

increase-favors products

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41
Q

Q

A

reaction proceeds forward

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42
Q

Q=K

A

reaction at equilibrium

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43
Q

Q>K

A

reaction proceeds reverse

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44
Q

remove reactant =

A

slower

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45
Q

increase partial pressure of reactant/product shifts equilibrium so

A

more substance consumed

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46
Q

decrease in partial pressure shifts toward

A

products

47
Q

decrease volume shifts equilibrium toward

A

side of reaction with fewer moles of gas

48
Q

is water included in ka expressions?

A

no

49
Q

pH=

A

-log[H+]

50
Q

pOH=

A

-log[OH-}

51
Q

pH+pOH=

A

14.00

52
Q

polyprotic acids

A

have more than 1 ionizable proton

53
Q

protons and polyprotic acids

A

it gets harder to pull of protons from these (1st easiest) and sometimes second or third can be hard enough to remove that we can ignore it

54
Q

acids and bases are weak or strong because of

A

structure

55
Q

if conjugate is stable, then acid or base will be more likely to (blank)

A

give up or accept proton/H+ (resonance and anions with more resonance structures= more stable)

56
Q

if we dissolve salt what happens

A

change pH

57
Q

what happens if the salt produces the conjugate base/acid of a weak acid/base

A

it can react with water to produce OH- or H3O+ and change pH

58
Q

what can be used to relate pKa of a proton to pH of the solution

A

pKa+log(base/acid)

59
Q

pKa=

A

-log(Ka) and the point where [base]=[acid]

60
Q

when [base]=[acid] what does it mean?

A

half the acid is deprotonated

61
Q

pKa+pKb=

A

14.00

62
Q

what is the Henderson-Hasselbalch equation used for

A

figure out how much of an acid and base we need to give a particular pH or how much pH will change when we add a strong acid or base to our buffered solution

63
Q

how do buffers work?

A

weak acid/base reacting with the strong base/acid you’re adding to neutralize them and limit the pH change

64
Q

indicators show

A

pH change happening in system

65
Q

when do indicators work best?

A

within +/- 1 pH unit of pKa

66
Q

Why do indicators change color?

A

near pKa, losing or gaining a proton which changes their structure and electronic properties, which effects what wavelengths of light they absorb

67
Q

indicators used in titration how?

A

look for when we’ve added enough acid or base to neutralize the other and determine concentration of unknown

68
Q

determine concentration of unknown in titration problem

A

MaVa=MbVb

69
Q

Ksp

A

solubility product constant- measure of how much of a solid will dissolve- usually just products

70
Q

Kw is specific to

A

water

71
Q

Kw always=

A

1.00x10^-14

72
Q

pH and autoionization of H2O

A

H2O(l) base+H2O(l) acid–> H3O+ (aq) conjugate acid+ OH- (aq) conjugate base

73
Q

pH=

A

potential of hydrogen ion

74
Q

pH=

A

-log[H+]

75
Q

[ ] =

A

10^-pH

76
Q

sig figs with pH

A

first # not considered significant

77
Q

if we have a weak and strong acid at some [ ], which is more acidic/has lower pH?

A

strong acid

78
Q

pOH=

A

-log[OH-]

79
Q

pH + pOH

A

14, pKw, -log[1x10^-14]

80
Q

strong acid

A

complete dissociation, no ice, no K, no reverse

81
Q

strong base

A

complete dissociation, no K, no ice, no reverse

82
Q

weak acid

A

partly dissociates

HA—<> H+ + A-, Ka= [H+][A-]/[HA]

83
Q

the larger Ka is, the stronger

A

weak acid is- wants to donate H+

84
Q

weak bases

A

partially accept an H+ from water
B+H2O(l)–>< HB+ + OH-
Kb= [OH-]{HB+]/[B]

85
Q

The larger Kb is, the stronger

A

the weak base, the more it wants to accept a H+ from water

86
Q

[H+][OH-]=

A

Kw

87
Q

Ka=

A

kw/kb

88
Q

ka x kb=

A

kw (1,00x10^-14)

89
Q

larger Ka is, smaller (blank)

A

kb for conjugate base

90
Q

weakest weak bases include

A

Cl-, Br-, I-, NO2-, VSO4-, ClO4-

91
Q

pKa=

A

-log[ka]

92
Q

pkb=

A

-log[kb]

93
Q

small pka means

A

larger Ka, strong acid

94
Q

small pkb means

A

larger kb, strong base

95
Q

polyprotic

A

acids with more than 1 H+ to donate, bases which will accept more than 1 H+

96
Q

oxoacids

A

atom (usually nonmetal) bonded to 1 or more O with some H+ as well

97
Q

in a series of oxoacids, what happens?

A

acid strength goes up with more O

98
Q

examples of organic amines

A

nitrogen, ammonium

99
Q

organic amines

A

ammonia type areas of organic (c) molecules

N surrounded by 3 other atoms/ R groups with a lone pair (will accept H+)

100
Q

anions tend to be

A

bases

101
Q

Buffers

A

resist change in pH, mixture of a weak acid and its conjugate base

102
Q

weak acids

A

eat OH-

103
Q

weak bases

A

eat H+

104
Q

Henderson-Hassel Balch equation pKa

A

-log[H+]+-log([A-]/[HA])

105
Q

Henderson-Hassel Balch equation pH

A

pKa + log [A-]/[HA]

106
Q

common ion has to do with

A

LeP and stress on system

107
Q

ksp helps determine

A

how soluble a compound is

108
Q

ksp=

A

[M^n+]^M [Z^y-]^Z

109
Q

pH indicators work by

A

being ionized (gain or lose H+)

110
Q

How can we use pH and pKa to find the acid base ratio?

A

pH=pKa + log (base/acid)

111
Q

acid base titration

A

pH refers to a solution while pKa refers to a specific molecule/H+ on a molecule

112
Q

[base]=[acid]

A

pH = pKa

113
Q

equivalence point for strong acid/strong base

A

7.00

114
Q

equivalence point for strong acid/weak base

A

pH < 7.00

General chemistry II (4 decks)

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