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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
Q

Resonance

A

of conjugate base, more resonance, more stable, stronger

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26
Q

Dipole induction

A

more electronegative substitute and closer to hydrogen is more acidic

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27
Q

Orbitals

A

higher s character is more acidic

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28
Q

If two atoms have the same structure

A

closer to acidic hydrogen is more acidic

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29
Q

S versus P orbitals

A

s orbitals are closer to the nucleus and are more electronegative, higher % s orbitals is more acidic

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30
Q

4 electron domains

A

SP3

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31
Q

Conjugate acid of weak base

A

acidic

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32
Q

Conjugate base of weak acid

A

basic

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33
Q

Conjugate base from strong acid

A

neutral

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34
Q

Conjugate acid from strong base

A

neutral

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35
Q

Cation of strong base

A

neutral

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36
Q

Weak acid and weak base

A

if ka > kb it is acidic, if kb > ka it is basic

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37
Q

Amphoteric ion acidity

A

compare ka with its own kb, the larger one dominates

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38
Q

Bigger ion

A

weaker bond, stronger acid

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39
Q

Strong acid with strong base

A

Large equilibrium constant, water and neutral salt as product, neutral effect on solution

40
Q

Strong acid with weak base

A

Large equilibrium constant, water and acidic salt as products, acidic effect on solution

41
Q

Weak acid with strong base

A

Large equilibrium constant, water and basic salt as products, basic effect on solution

42
Q

Weak acid with weak base

A

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
Q

Example of strong acids that will not effect pH

A

Cl, Br, I, NO3, ClO4

44
Q

Examples of strong bases that will not effect pH

A

Li, Na, K, Mg, Ca, Sr, Ba

45
Q

Acidic pH < 7

A

NH4+, HSO4-, HSO3-, H3PO4-

46
Q

Basic pH > 7

A

CH3CO2-, HCO2-, HCO3-, F-, CN-, HS-, NO2-, OCl-, CO3 2-, S 2-, SO3 2-, PO4 3-

47
Q

Neutral pH = 7

A

Li+, Na+, K+, Mg2+, Ca2+, Sr2+, Ba2+, Cl-, Br-, I-, NO3-, ClO4-

48
Q

Which are ignored for strong bases

A

Na+ and K+

49
Q

Which are ignored for strong acids

A

Cl- and NO3-

50
Q

If acidic hydrogen is on the same atom in two compounds

A

cannot consider electronegativity or size

51
Q

If acidic hydrogen is on a different atom in two compounds

A

cannot consider hybridization, resonance, or inductive

52
Q

What is needed to make a buffer

A

a weak acid and its conjugate base or a weak base and its conjugate acid

53
Q

Most effective buffers

A

pH values within range of + - 1 of the pKa of weak acid

54
Q

If the ratio of weak acid to conjugate base remains close to original buffer solution

A

even after acid or base is added, the pH will not be altered drastically

55
Q

When can you ignore -x

A

If Ka * 100 < [HA]0

56
Q

Buffer equation pH=

A

pH = pKa + log (conjugate base) / (weak acid)

57
Q

Common Ion Effect

A

When a reagent added to a solution already in equilibrium (ion already present), the reaction will shift opposite of addition

58
Q

Shift in common ion effect

A

opposite of addition

59
Q

To get rid of log in an equation

A

10^

60
Q

To get rid of ln in an equation

A

e

61
Q

Adding a strong acid to a buffer

A

will react with the basic component of the buffer and produce the acidic component of the buffer

62
Q

Adding a strong base to a buffer

A

will react with the acidic component of the buffer system and produce the basic component of the buffer

63
Q

When given additive volume in a problem

A

convert to mol to use with log

64
Q

Titration curve

A

plot of pH versus volume of titrant added to solution

65
Q

At equivalence point

A

number of moles of base is equal to number of moles of acid

66
Q

Half equivalence point

A

pH = Pka

67
Q

End point

A

no further change in pH

68
Q

Titration of strong acid with strong base

A

neutral salts, pH at equivalence will always be 7, [H3O+] and [OH-] always is 1*10^-7 M

69
Q

The compound in excess if strong acid or base

A

will hydrolize in water in a second step (NaOH -> Na+ + OH-) then find pOH and pH

70
Q

To neutralize a reaction

A

moles of H+ = moles of OH-

71
Q

Titration of weak acid with strong base

A

basic salt produced, pH greater than 7, at half equivalence [weak acid] = [conjugate base], Ka = [H3O+] and pKa = pH

72
Q

Titration of weak base with strong acid

A

acidic salt produced, pH less than 7, pKb = pOH

73
Q

What in ICE table affects pH

A

when the lower number is subtracted in “C” to = 0, that value does not affect

74
Q

pH indicators

A

allow for a color change to take place when the pH of the solution that the indicator dissolves in reaches some point

75
Q

Maximum buffer capacity

A

when [HA] and [A-] are large

76
Q

Buffer range

A

pKa + - 1

77
Q

Weaker acid

A

stronger conjugate base

78
Q

Best buffer shows

A

least change in pH

79
Q

Finding volume in titration

A

volume = mol / M

80
Q

The most what means the greater buffer capacity

A

greatest HA and A-

81
Q

If you add strong acid to a solution of weak acid

A

diminishes the amount of weak acid ionization

82
Q

The more stable to conjugate base of an acid

A

the more acidic the acid is

83
Q

What determines acidity

A

stability of conjugate base

84
Q

Meaning of pKa

A

pKa = pH at which [HA] = [A-]

85
Q

Acids with multiple ionizable protons will have

A

multiple Ka’s for each proton and therefore multiple pkas

86
Q

pH > pKa

A

proton off

87
Q

pH < pKa

A

proton on, more acidic

88
Q

strong acid and strong base graph

A

pH = 7

89
Q

If strong acid is added to a buffer

A

will react with weak base, slightly decrease pH

90
Q

If you add a strong acid to a solution of weak acid

A

diminishes weak acid ionization

91
Q

If you add strong base to a solution of weak base

A

diminishes weak base ionization

92
Q

More stable

A

more acidic

93
Q

In a buffer what is the limiting reactant

A

strong base

94
Q

Buffer resists change in pH when

A

acid added, base added, buffer is diluted

95
Q

Have no effect on pH

A

neutral salts (NaCl)

96
Q

Examples of strong electrolytes

A

salts, strong acids, strong bases

97
Q

In a reaction with strong electrolytes

A

one direction reaction with electrolyte on reactant side

CHEM1212 (5 decks)

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