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Gen Chem 2 > Exam 3 > Flashcards

Exam 3 Flashcards

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1
Q

what are formed when an acid neutralizes a base

A

a salt

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2
Q

salt solutions can be

A

neutral and not neutral

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3
Q

what does the neutralness of a salt solution depend on

A

tendency of ions to react with water

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4
Q

neutral solutions are formed by salts of

A

metal cations of a strong base with a conjugate base anions of monoprotic strong acids

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5
Q

acidic solutions are formed by salts that came from a strong ______ and weak ________. and what is important about these

A

acid
base
the conjugate acid of the weak base is not ignorably weak

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6
Q

basic solutions are formed by salts that came from the reaction of a weak ______ and a strong _______. and what is important about these

A

acid
base
the conjugate base of the weak acid is not ignorably weak

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7
Q

when calculating the pH of salt solutions
ignore ions that _____ _____ ______ the pH
treat ions that do affect the pH like weak _______ or ______
for salts formed by the reaction of weak acids and weak bases the _______ ion will win

A

do not affect
acids or bases
stronger

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8
Q

compare ____ and _____ of the ions, the larger number will have a _______ influence

A

Ka and Kb
stronger

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9
Q

small highly charges ________ _______ _____ give acidic solutions because they _______ the OH bond in the coordinated water molecules making it easier to ________ water molecules

A

hydrated metal ions
polarize
ionize

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10
Q

what are some small highly charges hydrated metal ions because they _______ the OH bond in the coordinated water molecules making it easier to ________ water molecules

A

Al3+, Cr3+, Fe3+

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11
Q

basic oxides form

A

hydroxides

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12
Q

acidic oxides form

A

oxoacids

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13
Q

what can behave either like an acidic oxide or like a basic oxide conditions

A

amphoteric oxode

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14
Q

metals that form amphoteric oxides also form

A

amphoteric hydroxides

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15
Q

Lewis bases are

A

electron pair donors

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16
Q

Lewis acids are

A

electron pair acceptors

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17
Q

H+ can be regarded and an acid that accepts an

A

electron pair

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18
Q

all Bl bases are also
any proton ______ must have a lone pair to _______ the proton
but no _______ are needed for the definition

A

lewis bases
acceptor
accept
protons

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19
Q

Lewis acids encompass a ________ group of compounds than the BL acid concept

A

larger

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20
Q

what oxides can accept lone pairs from water

A

non metal

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21
Q

_______ transfer forms an oxoacid

A

proton

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22
Q

what is the Boltzmann equation

A

s=kln(W)

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23
Q

entropy change equation

A

delta S0= sum S0(products)- sum S0(reactants)

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24
Q

what law states that in any process, the total energy of a system and its surroundings is constant. Delta Euniv=delta E system + delta E surroundings = 0

A

first law

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25
Q

what law states that in ant SPONTANEOUS process, the total entropy of a system and its surroundings will increase. deltaSuniv= delta s system + delta s surroundings

A

second law

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26
Q

what law states that the entropy of a perfectly ordered crystalline substance at 0K is zero

A

third law

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27
Q

pKa equation

A

-log(Ka)

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28
Q

pKb equation

A

-log(Kb)

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29
Q

what does pKa + pKb =

A

pKw=14

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30
Q

Henderson haselbalch equation

A

pH=pKa+log[base]/[acid]

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31
Q

solubility equation

A

Ksp=pie(ions)eqX

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32
Q

ion products equation

A

IP= pie(ions)tX

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33
Q

what is it called when salts of counter ions in weak acid solutions drive the reaction to the left

A

counterion effect

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34
Q

pH changes _________ when [acid]/[base] changes

A

slightly

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35
Q

a solution that contains significant amounts of a _______ acid and its conjugate base _______ in pH. this type of solution is called a what

A

weak
resists
buffer

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36
Q

a buffer works most efficiently as pH values around the ______ value of the weak acid

A

pKa

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37
Q

what is the amount of acid or base that can be added without significantly changing the pH called

A

buffer capacity

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38
Q

the ___________ __________ depends on the absolute concentration of the conjugate acid/base pair

A

buffer capacity

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39
Q

when ______ is added to a buffer the _____ acid reacts with us and it gets converted into a conjugate base

A

OH-
weak

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40
Q

when ______ is added to a buffer the ______ base reacts with it and gets converted to a _______ acid

A

H3O+
conjugate
weak

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41
Q

what equation makes it very easy to calculate the pH at which an acid is dissociated to a certain percentage

A

henderson Haselbalch

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42
Q

what is the process of neutralizing an acid of an unknown concentration with a base of a known concentration called

A

acid-base titration

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43
Q

what can be used to determine the unknown concentration by measuring the oH as a function of volume of added base

A

acid base titration

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44
Q

at the _________ ________ of an acid base titration, equimolar amounts of acid and base have reacted

A

equivalence point

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45
Q

what are the 4 steps to a modified ice table

A

initial moles
completion moles
completion concentration
equilibrium concentration

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46
Q

buffers form with what ratio

A

10:1 or 1:10
10>[conjugate base]/[weak acid] > 0.1

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47
Q

the pH after the equivalence point is deterred only by the excess of _______ or _______ above what is needed to neutralize the weak _____ or _______

A

acid
base
base
acid

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48
Q

titrations of polyprotic acids have multiple ________ ______ and multiple ________ ______

A

equivalence points
buffer regions

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49
Q

original definition of acid/base referred to color change of what

A

litmus

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50
Q

compounds that define acid/base are called

A

acid base indicators

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51
Q

indicators are

A

weak acids

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52
Q

indicators change color in different ______ ranges

A

pH

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53
Q

acid base indicators allow pH determination to ~

A

+ or - 1 units

54
Q

what is often used for pH measurements and is a mixture of several indicators

A

universal indicator

55
Q

what pH does a universal indicator work best between

A

3 and 10

56
Q

precise pH measurements can be obtained with what

A

pH meter

57
Q

what is a natural indicator

A

red cabbage

58
Q

solubility can be affected by what

A

what else is in the solution

59
Q

the solubility product only changes with

A

TEMPERATURE

60
Q

what shifts the equilibrium in solubility products

A

common ion effect

61
Q

pH has no effect on the solubility of salts that contain _______ that are conjugate bases of _______ ______

A

anions
strong acids

62
Q

salts of basic anions that are conjugate bases of weak acids are _______ soluble in ______

A

more
acids

63
Q

basic _____ and ______ are more soluble in acids

A

oxides and hydroxides

64
Q

what can increase the solubility of a salt significantly

A

complex formation

65
Q

formation of soluble ______ ______ increases solubility ______ _____

A

complex ions
A LOT

66
Q

what is it called when a compound behaves as both an acid and a base

A

amphoteric

67
Q

if IP > Ksp:

A

precipitaton occurs

68
Q

IP = Ksp :

A

saturated soltion, equilibrium exists

69
Q

IP<Ksp:

A

unsaturated solution, no precipitation

70
Q

If we add equal volumes all _______ are cut in ______

A

concentrations
half

71
Q

what is based on the different solubility of metal salts with a number of anions is a very old, traditional process

A

qualitative analysis

72
Q

what are grouped based on the solubility of their salts and whether they will form precipitates in the presence of certain anion

A

cations

73
Q

if Kp is positive the reaction will move _______ towards equilibrium (spontaneously)

A

right

74
Q

if Kp is negative than the reaction will move _____ towards equilibrium (spontaneously)

A

left

75
Q

comparing what and what allows us to predict spontaneous reactions

A

K and Q

76
Q

what is the study the interconversion of heat and other forms of energy

A

thermodynamics

77
Q

what is a process that occurs on its own without influence

A

spontaneous process

78
Q

we know that a spontaneous process can be very _______

A

slow

79
Q

spontaneous endothermic reactions

A

spontaneous dissolution of NH4NO3 in water
ice melts spontaneously at 273K

80
Q

what is the measure of molecular randomness, plays important role in determining the spontaneity if a reaction

A

entropy

81
Q

a system moves towards ________ randomness

A

more

82
Q

______ makes a difference in entropy and in gasses ______ is also important

A

temperate
pressure

83
Q

_______ is a qualitative measure of how spread out or disperse a systems energy is

A

entropy

84
Q

any increase in _______ _______ will contribute to higher entropy, as there are more ______ _____ that molecules can occupy

A

motional energy
different states

85
Q

what are different motional energy

A

translational energy
rotational energy
vibrational energy

86
Q

who discovers that entropy of a state is related to the number of ways in which a state can be achieved

A

Ludwig boltzmann

87
Q

random distribution equations

A

delta s = nRln(Vfinal/Vintitial)
delta s = nRln(Pintital/Pfinal)

88
Q

for monatomic species the ________ atom has ______ entropy

A

heavier
higher

89
Q

what increase entropy

A

melting, vaporization. and sublimation

90
Q

solution formation of non _________ increases entropy

A

electrolytes

91
Q

solution formation of ________ compounds can lead to increase or decrease in entropy

A

ionic

92
Q

first law of thermodynamics equation

A

Euniv = E system + E surroundings = 0

93
Q

second law of thermodynamics equation

A

Suniv = Ssystem + Surroundings

94
Q

> 0
= 0
< 0

A

spontaneous
equilibrium
non=spontanous

95
Q

Delta S surr equation

A

delta S surr = - delta H sys/T

96
Q

Delta S universe equation

A

delta S Univ = delta s sys + delta s surr = delta s sys - delta H sys/ T

97
Q

disorder is favored because there is a _______ ________ of achieving a disordered state

A

higher probability

98
Q

the entropy of a perfectly ordered ________ substance at ____ K is ______

A

crystalline
0
zero

99
Q

how much energy is available to increase the entropy of the universe to use for “useful work”

A

Free or available

100
Q

delta G < 0
delta G = 0
delta G > 0

A

spontaneous
equilibrium
reverse reaction is spontaneous

101
Q

when H is neg and S is pos

A

G is neg and spontaneous

102
Q

when H is pos and S is neg

A

G is pos and not spontaneous

103
Q

when H is neg and S is neg

A

neg when TS<H>H
spont at low T
nonspont at high temp</H>

104
Q

when H is pos and S is pos

A

pos when TS<H>H
spont at high T
nonspont at low temp</H>

105
Q

derivative of free energy equation

A

-TdeltaSuniv = delta G

106
Q

equation used for delta G0 rxn

A

delta G0rxn = sum delta G0f(products)-sum delta G0f(reactants)

107
Q

real life reaction equation

A

delta G = delta G0 + RTln(Q)

108
Q

at equilibrium equation
this equation provides the fundamental connection between _________ and ________

A

delta G0= -RTln(K)
thermodynamics and equilibrium

109
Q

the drive for a reaction is always _______: The process moves______ the curve towards the ________

A

downhill
down
minimum

110
Q

oxidation is the _____ of electron

A

loss

111
Q

reduction is the _____ of electrons

A

gain

112
Q

oxidation and reduction always occur

A

simultaneously

113
Q

electrons move between ________ species

A

chemical

114
Q

electron flow on a __________ _______ is called electricity

A

larger scale

115
Q

what are energetic electrons called

A

galvanic or voltaic

116
Q

uphill, __________ reactions can be driven if energetic electrons are provided and these cells are called _________

A

non-spontaneous
electrolytic

117
Q

the _____ is the electrode at which ______ occurs

A

anode
oxidation

118
Q

the ______ is the electrode at which ______ occurs

A

cathode
reduction

119
Q

what is where oxidation occurs, where electrons are produces, anions migrate toward is and has a negative sign

A

anode

120
Q

what is where reduction occurs, where electrons are consumed, cations migrate towards it, has a positive sign

A

cathode

121
Q

ions move across a ____ _____ to equilibrate charges

A

salt bridge

122
Q

cells can be characterized by an _________ _______ that drives the electrons

A

electromotive force (emf)

123
Q

galvanic cells have ______ emf

A

postitive

124
Q

emf depends on _________ and ________

A

concentration and temperature

125
Q

the ______ ______ ______ is set to E0H+H2=0V, and all cell potentials are reported as measured against the SHE

A

standard hydrogen electrode

126
Q

the SHE can be either an _______ or ______

A

anode or cathode

127
Q

the measured ____ ______ gives the overall driving force for a reaction

A

cell voltage

128
Q

standard potentials measured against a SHE can have a _________ or _______ sign depending on how the electric leads are connected

A

positive or negative

129
Q

equation to calculate overall cell potentials

A

E0Ccell = Ered0(cathode)-Ered0(anode)

130
Q

combining half cell reactions by addition equation

A

E0cell= E0red(cathode)+E0ox(anode)

131
Q

in the table if the value is above SHE: ______ side is reduced by SH

A

left

132
Q

in the table if the value is below SHE: ______ side is reduced by SH

A

right

Gen Chem 2 (3 decks)

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