Exam 3 Flashcards
(132 cards)
1
Q
what are formed when an acid neutralizes a base
A
a salt
2
Q
salt solutions can be
A
neutral and not neutral
3
Q
what does the neutralness of a salt solution depend on
A
tendency of ions to react with water
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
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
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
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
8
Q
compare ____ and _____ of the ions, the larger number will have a _______ influence
A
Ka and Kb
stronger
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
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+
11
Q
basic oxides form
A
hydroxides
12
Q
acidic oxides form
A
oxoacids
13
Q
what can behave either like an acidic oxide or like a basic oxide conditions
A
amphoteric oxode
14
Q
metals that form amphoteric oxides also form
A
amphoteric hydroxides
15
Q
Lewis bases are
A
electron pair donors
16
Q
Lewis acids are
A
electron pair acceptors
17
Q
H+ can be regarded and an acid that accepts an
A
electron pair
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
19
Q
Lewis acids encompass a ________ group of compounds than the BL acid concept
A
larger
20
Q
what oxides can accept lone pairs from water
A
non metal
21
Q
_______ transfer forms an oxoacid
A
proton
22
Q
what is the Boltzmann equation
A
s=kln(W)
23
Q
entropy change equation
A
delta S0= sum S0(products)- sum S0(reactants)
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
25
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
second law
26
what law states that the entropy of a perfectly ordered crystalline substance at 0K is zero
third law
27
pKa equation
-log(Ka)
28
pKb equation
-log(Kb)
29
what does pKa + pKb =
pKw=14
30
Henderson haselbalch equation
pH=pKa+log[base]/[acid]
31
solubility equation
Ksp=pie(ions)eqX
32
ion products equation
IP= pie(ions)tX
33
what is it called when salts of counter ions in weak acid solutions drive the reaction to the left
counterion effect
34
pH changes _________ when [acid]/[base] changes
slightly
35
a solution that contains significant amounts of a _______ acid and its conjugate base _______ in pH. this type of solution is called a what
weak
resists
buffer
36
a buffer works most efficiently as pH values around the ______ value of the weak acid
pKa
37
what is the amount of acid or base that can be added without significantly changing the pH called
buffer capacity
38
the ___________ __________ depends on the absolute concentration of the conjugate acid/base pair
buffer capacity
39
when ______ is added to a buffer the _____ acid reacts with us and it gets converted into a conjugate base
OH-
weak
40
when ______ is added to a buffer the ______ base reacts with it and gets converted to a _______ acid
H3O+
conjugate
weak
41
what equation makes it very easy to calculate the pH at which an acid is dissociated to a certain percentage
henderson Haselbalch
42
what is the process of neutralizing an acid of an unknown concentration with a base of a known concentration called
acid-base titration
43
what can be used to determine the unknown concentration by measuring the oH as a function of volume of added base
acid base titration
44
at the _________ ________ of an acid base titration, equimolar amounts of acid and base have reacted
equivalence point
45
what are the 4 steps to a modified ice table
initial moles
completion moles
completion concentration
equilibrium concentration
46
buffers form with what ratio
10:1 or 1:10
10>_[conjugate base]/[weak acid] >_ 0.1
47
the pH after the equivalence point is deterred only by the excess of _______ or _______ above what is needed to neutralize the weak _____ or _______
acid
base
base
acid
48
titrations of polyprotic acids have multiple ________ ______ and multiple ________ ______
equivalence points
buffer regions
49
original definition of acid/base referred to color change of what
litmus
50
compounds that define acid/base are called
acid base indicators
51
indicators are
weak acids
52
indicators change color in different ______ ranges
pH
53
acid base indicators allow pH determination to ~
+ or - 1 units
54
what is often used for pH measurements and is a mixture of several indicators
universal indicator
55
what pH does a universal indicator work best between
3 and 10
56
precise pH measurements can be obtained with what
pH meter
57
what is a natural indicator
red cabbage
58
solubility can be affected by what
what else is in the solution
59
the solubility product only changes with
TEMPERATURE
60
what shifts the equilibrium in solubility products
common ion effect
61
pH has no effect on the solubility of salts that contain _______ that are conjugate bases of _______ ______
anions
strong acids
62
salts of basic anions that are conjugate bases of weak acids are _______ soluble in ______
more
acids
63
basic _____ and ______ are more soluble in acids
oxides and hydroxides
64
what can increase the solubility of a salt significantly
complex formation
65
formation of soluble ______ ______ increases solubility ______ _____
complex ions
A LOT
66
what is it called when a compound behaves as both an acid and a base
amphoteric
67
if IP > Ksp:
precipitaton occurs
68
IP = Ksp :
saturated soltion, equilibrium exists
69
IP
unsaturated solution, no precipitation
70
If we add equal volumes all _______ are cut in ______
concentrations
half
71
what is based on the different solubility of metal salts with a number of anions is a very old, traditional process
qualitative analysis
72
what are grouped based on the solubility of their salts and whether they will form precipitates in the presence of certain anion
cations
73
if Kp is positive the reaction will move _______ towards equilibrium (spontaneously)
right
74
if Kp is negative than the reaction will move _____ towards equilibrium (spontaneously)
left
75
comparing what and what allows us to predict spontaneous reactions
K and Q
76
what is the study the interconversion of heat and other forms of energy
thermodynamics
77
what is a process that occurs on its own without influence
spontaneous process
78
we know that a spontaneous process can be very _______
slow
79
spontaneous endothermic reactions
spontaneous dissolution of NH4NO3 in water
ice melts spontaneously at 273K
80
what is the measure of molecular randomness, plays important role in determining the spontaneity if a reaction
entropy
81
a system moves towards ________ randomness
more
82
______ makes a difference in entropy and in gasses ______ is also important
temperate
pressure
83
_______ is a qualitative measure of how spread out or disperse a systems energy is
entropy
84
any increase in _______ _______ will contribute to higher entropy, as there are more ______ _____ that molecules can occupy
motional energy
different states
85
what are different motional energy
translational energy
rotational energy
vibrational energy
86
who discovers that entropy of a state is related to the number of ways in which a state can be achieved
Ludwig boltzmann
87
random distribution equations
delta s = nRln(Vfinal/Vintitial)
delta s = nRln(Pintital/Pfinal)
88
for monatomic species the ________ atom has ______ entropy
heavier
higher
89
what increase entropy
melting, vaporization. and sublimation
90
solution formation of non _________ increases entropy
electrolytes
91
solution formation of ________ compounds can lead to increase or decrease in entropy
ionic
92
first law of thermodynamics equation
Euniv = E system + E surroundings = 0
93
second law of thermodynamics equation
Suniv = Ssystem + Surroundings
94
> 0
= 0
< 0
spontaneous
equilibrium
non=spontanous
95
Delta S surr equation
delta S surr = - delta H sys/T
96
Delta S universe equation
delta S Univ = delta s sys + delta s surr = delta s sys - delta H sys/ T
97
disorder is favored because there is a _______ ________ of achieving a disordered state
higher probability
98
the entropy of a perfectly ordered ________ substance at ____ K is ______
crystalline
0
zero
99
how much energy is available to increase the entropy of the universe to use for "useful work"
Free or available
100
delta G < 0
delta G = 0
delta G > 0
spontaneous
equilibrium
reverse reaction is spontaneous
101
when H is neg and S is pos
G is neg and spontaneous
102
when H is pos and S is neg
G is pos and not spontaneous
103
when H is neg and S is neg
neg when TSH
spont at low T
nonspont at high temp
104
when H is pos and S is pos
pos when TSH
spont at high T
nonspont at low temp
105
derivative of free energy equation
-TdeltaSuniv = delta G
106
equation used for delta G0 rxn
delta G0rxn = sum delta G0f(products)-sum delta G0f(reactants)
107
real life reaction equation
delta G = delta G0 + RTln(Q)
108
at equilibrium equation
this equation provides the fundamental connection between _________ and ________
delta G0= -RTln(K)
thermodynamics and equilibrium
109
the drive for a reaction is always _______: The process moves______ the curve towards the ________
downhill
down
minimum
110
oxidation is the _____ of electron
loss
111
reduction is the _____ of electrons
gain
112
oxidation and reduction always occur
simultaneously
113
electrons move between ________ species
chemical
114
electron flow on a __________ _______ is called electricity
larger scale
115
what are energetic electrons called
galvanic or voltaic
116
uphill, __________ reactions can be driven if energetic electrons are provided and these cells are called _________
non-spontaneous
electrolytic
117
the _____ is the electrode at which ______ occurs
anode
oxidation
118
the ______ is the electrode at which ______ occurs
cathode
reduction
119
what is where oxidation occurs, where electrons are produces, anions migrate toward is and has a negative sign
anode
120
what is where reduction occurs, where electrons are consumed, cations migrate towards it, has a positive sign
cathode
121
ions move across a ____ _____ to equilibrate charges
salt bridge
122
cells can be characterized by an _________ _______ that drives the electrons
electromotive force (emf)
123
galvanic cells have ______ emf
postitive
124
emf depends on _________ and ________
concentration and temperature
125
the ______ ______ ______ is set to E0H+H2=0V, and all cell potentials are reported as measured against the SHE
standard hydrogen electrode
126
the SHE can be either an _______ or ______
anode or cathode
127
the measured ____ ______ gives the overall driving force for a reaction
cell voltage
128
standard potentials measured against a SHE can have a _________ or _______ sign depending on how the electric leads are connected
positive or negative
129
equation to calculate overall cell potentials
E0Ccell = Ered0(cathode)-Ered0(anode)
130
combining half cell reactions by addition equation
E0cell= E0red(cathode)+E0ox(anode)
131
in the table if the value is above SHE: ______ side is reduced by SH
left
132
in the table if the value is below SHE: ______ side is reduced by SH
right
