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CHEM1212 > TEST 4- 14.7-14.12, 15 > Flashcards

TEST 4- 14.7-14.12, 15 Flashcards

1
Q

Autoionization of water yields

A

the same number of hydronium and hydroxide ions

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2
Q

Monoprotic

A

can only accept or donate one proton

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3
Q

Polyprotic

A

has more than one proton it can donate or accept

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4
Q

Monoprotic example

A

HCl, NaOH, NaCl, H2O

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5
Q

Polyprotic example

A

acid H2SO4, base Ca(OH)2

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6
Q

Characteristics of strong acid

A

large Ka and small PKa

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7
Q

Characteristics of strong base

A

large kb and small PKb

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8
Q

When a strong acid or strong base produces concentrations of H3O+ and OH- that are greater than

A

10^-6 contributions from autoionization can be ignored

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9
Q

In autoionization of water, K

A

Kw is used

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10
Q

An increase difference in pKas

A

further equilibrium lies toward higher pKa (or weaker acid)

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11
Q

Ka is much larger in which step

A

first step

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12
Q

For pH of strong acids and bases when must autoionizaiton of water be a factor

A

when [H3O+] is less than 10^-6

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13
Q

Higher electronegativity Acid

A

stronger acid, increases across period

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14
Q

Larger atom Acid

A

stronger acid, increase down group

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15
Q

Higher electronegativity Base

A

weaker base, increase from right to left

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16
Q

Larger atom Base

A

weaker base, increase up group

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17
Q

The strength of an acid, HA depends on

A

strength or stability of its conjugate base A-

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18
Q

More stable conjugate base

A

stronger conjugate base

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19
Q

More positive charge

A

stronger acid

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20
Q

F- is the most stable conjugated base

A

HF is the strongest acid

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21
Q

Weaker base (stable or not)

A

more stable

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22
Q

CARDIO

A

Charge, atom (electronegativity and size), resonance (stabilization), dipole induction (nearby electronegativy substituent), orbitals (hybridization)

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23
Q

Charge

A

more positive is more acidic, more negative more basic

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24
Q

Atom

A

atom next to acidic hydrogen, if same row look at electronegativity, if same group look at size

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25
Resonance
of conjugate base, more resonance, more stable, stronger
26
Dipole induction
more electronegative substitute and closer to hydrogen is more acidic
27
Orbitals
higher s character is more acidic
28
If two atoms have the same structure
closer to acidic hydrogen is more acidic
29
S versus P orbitals
s orbitals are closer to the nucleus and are more electronegative, higher % s orbitals is more acidic
30
4 electron domains
SP3
31
Conjugate acid of weak base
acidic
32
Conjugate base of weak acid
basic
33
Conjugate base from strong acid
neutral
34
Conjugate acid from strong base
neutral
35
Cation of strong base
neutral
36
Weak acid and weak base
if ka > kb it is acidic, if kb > ka it is basic
37
Amphoteric ion acidity
compare ka with its own kb, the larger one dominates
38
Bigger ion
weaker bond, stronger acid
39
Strong acid with strong base
Large equilibrium constant, water and neutral salt as product, neutral effect on solution
40
Strong acid with weak base
Large equilibrium constant, water and acidic salt as products, acidic effect on solution
41
Weak acid with strong base
Large equilibrium constant, water and basic salt as products, basic effect on solution
42
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
43
Example of strong acids that will not effect pH
Cl, Br, I, NO3, ClO4
44
Examples of strong bases that will not effect pH
Li, Na, K, Mg, Ca, Sr, Ba
45
Acidic pH < 7
NH4+, HSO4-, HSO3-, H3PO4-
46
Basic pH > 7
CH3CO2-, HCO2-, HCO3-, F-, CN-, HS-, NO2-, OCl-, CO3 2-, S 2-, SO3 2-, PO4 3-
47
Neutral pH = 7
Li+, Na+, K+, Mg2+, Ca2+, Sr2+, Ba2+, Cl-, Br-, I-, NO3-, ClO4-
48
Which are ignored for strong bases
Na+ and K+
49
Which are ignored for strong acids
Cl- and NO3-
50
If acidic hydrogen is on the same atom in two compounds
cannot consider electronegativity or size
51
If acidic hydrogen is on a different atom in two compounds
cannot consider hybridization, resonance, or inductive
52
What is needed to make a buffer
a weak acid and its conjugate base or a weak base and its conjugate acid
53
Most effective buffers
pH values within range of + - 1 of the pKa of weak acid
54
If the ratio of weak acid to conjugate base remains close to original buffer solution
even after acid or base is added, the pH will not be altered drastically
55
When can you ignore -x
If Ka * 100 < [HA]0
56
Buffer equation pH=
pH = pKa + log (conjugate base) / (weak acid)
57
Common Ion Effect
When a reagent added to a solution already in equilibrium (ion already present), the reaction will shift opposite of addition
58
Shift in common ion effect
opposite of addition
59
To get rid of log in an equation
10^
60
To get rid of ln in an equation
e
61
Adding a strong acid to a buffer
will react with the basic component of the buffer and produce the acidic component of the buffer
62
Adding a strong base to a buffer
will react with the acidic component of the buffer system and produce the basic component of the buffer
63
When given additive volume in a problem
convert to mol to use with log
64
Titration curve
plot of pH versus volume of titrant added to solution
65
At equivalence point
number of moles of base is equal to number of moles of acid
66
Half equivalence point
pH = Pka
67
End point
no further change in pH
68
Titration of strong acid with strong base
neutral salts, pH at equivalence will always be 7, [H3O+] and [OH-] always is 1*10^-7 M
69
The compound in excess if strong acid or base
will hydrolize in water in a second step (NaOH -> Na+ + OH-) then find pOH and pH
70
To neutralize a reaction
moles of H+ = moles of OH-
71
Titration of weak acid with strong base
basic salt produced, pH greater than 7, at half equivalence [weak acid] = [conjugate base], Ka = [H3O+] and pKa = pH
72
Titration of weak base with strong acid
acidic salt produced, pH less than 7, pKb = pOH
73
What in ICE table affects pH
when the lower number is subtracted in "C" to = 0, that value does not affect
74
pH indicators
allow for a color change to take place when the pH of the solution that the indicator dissolves in reaches some point
75
Maximum buffer capacity
when [HA] and [A-] are large
76
Buffer range
pKa + - 1
77
Weaker acid
stronger conjugate base
78
Best buffer shows
least change in pH
79
Finding volume in titration
volume = mol / M
80
The most what means the greater buffer capacity
greatest HA and A-
81
If you add strong acid to a solution of weak acid
diminishes the amount of weak acid ionization
82
The more stable to conjugate base of an acid
the more acidic the acid is
83
What determines acidity
stability of conjugate base
84
Meaning of pKa
pKa = pH at which [HA] = [A-]
85
Acids with multiple ionizable protons will have
multiple Ka's for each proton and therefore multiple pkas
86
pH > pKa
proton off
87
pH < pKa
proton on, more acidic
88
strong acid and strong base graph
pH = 7
89
If strong acid is added to a buffer
will react with weak base, slightly decrease pH
90
If you add a strong acid to a solution of weak acid
diminishes weak acid ionization
91
If you add strong base to a solution of weak base
diminishes weak base ionization
92
More stable
more acidic
93
In a buffer what is the limiting reactant
strong base
94
Buffer resists change in pH when
acid added, base added, buffer is diluted
95
Have no effect on pH
neutral salts (NaCl)
96
Examples of strong electrolytes
salts, strong acids, strong bases
97
In a reaction with strong electrolytes
one direction reaction with electrolyte on reactant side

CHEM1212 (5 decks)

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