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GEN CHEM 2 > Exam 2 - ch.15-17 > Flashcards

Exam 2 - ch.15-17 Flashcards

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1
Q

chemical equilibrium

A

occurs when the forward and reverse reaction rates are equal

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2
Q

once equilibrium is achieved…

A

the concentration of products and reactants remain constant

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3
Q

do K constants have units?

A

no

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4
Q

K»1

A

rxn favors products/forward

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5
Q

K«1

A

rxn favors reactants/reverse

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6
Q

homogeneous equilibria

A

all reactants and products are in the same phase

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7
Q

heterogeneous equilibria

A

reactants and products are in different phases

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8
Q

are pure solids and liquids included in equilibrium expression?

A

no

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9
Q

reaction quotient, Q

A

identical to calculating K, but for current conditions

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10
Q

Q<K

A

rxn moving toward products

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11
Q

Q>K

A

rxn moving toward reactants

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12
Q

Q=K

A

reaction is at equilibrium

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13
Q

inc in concentration of reactants

A

shift to right

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14
Q

dec in concentrations of products

A

shift to left

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15
Q

inc in concentrations of products

A

shift to left

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16
Q

dec in concentration of products

A

shift to right

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17
Q

dec in volume=inc in pressure

A

shift to fewer moles

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18
Q

inc in volume=dec in pressure

A

shift to more moles

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19
Q

endo temp inc

A

shift right

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20
Q

endo temp dec

A

shift left

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21
Q

exo temp inc

A

shift left

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22
Q

exo temp dec

A

shift right

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23
Q

effect of catalyst on equilibrium shift

A

no shift

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24
Q

arrhenius acid

A

will increase [H+] when dissolved in water

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25
Q

arrhenius base

A

will increase [OH-] when dissolved in water

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26
Q

bronsted-lowry acid

A

a proton donor

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27
Q

bronsted-lowry base

A

a proton acceptor

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28
Q

lewis acid

A

electron pair acceptor

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29
Q

lewis base

A

electron pair donor

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30
Q

amphiprotic substance

A

can act as an acid or base
ex: water

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31
Q

conjugate acid-base pair

A

compound pair which differ by a H+

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32
Q

the stronger the acid…

A

the weaker the conjugate base

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33
Q

the weaker the acid…

A

the stronger the conjugate base

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34
Q

Kw=

A

1.0x10^-14

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35
Q

neutral solution

A

[H3O+]=[OH-]

36
Q

acidic solution

A

[H3O+]>[OH-]

37
Q

basic solution

A

[H3O+]<[OH-]

38
Q

p=

A

-log

39
Q

strong acids

A

HCl, HBr, HNO3, HI, H2SO4, HClO3, HClO4

40
Q

strong bases

A

alkali metal and heavier earth metal +hydroxides

41
Q

%I=

A

[H+]/[HA] x100

42
Q

%I>5%

A

we can not assume that the x value is really small and negligible

43
Q

polyprotic acid

A

has more than one acidic proton

44
Q

Ka1>

A

Ka2

45
Q

hydrolysis

A

breaking apart water to produce H+/OH- ions

46
Q

cations can be…

A

acidic/neutral

47
Q

anions can be…

A

acidic/basic/neutral

48
Q

anions of strong acids are…

A

neutral

49
Q

anions of weak acids form…

A

basic solutions

50
Q

Ka>Kb anion is…

A

acidic

51
Q

Ka<Kb anion is…

A

basic

52
Q

neutral metal cations

A

group 1/ group 2

53
Q

acidic metal cations

A

transition and post-transition metals

54
Q

hydrated cations

A

more acidic than free water molecules

55
Q

hydrated metal cations w/ higher charges

A

=stronger metal/ water complex

56
Q

both an anion and cation that do not react w/ water

A

pH is neutral

57
Q

an anion which reacts w/ water and a cation that doesn’t

A

pH is basic

58
Q

cation which reacts w/ water and anion that doesn’t

A

pH is acidic

59
Q

both anion and cation reacts w/ water

A

compare Ka and Kb values

60
Q

bond polarity: more polar

A

=more acidic

61
Q

bond strength: decrease bond strength

A

=acid strength

62
Q

stability: more stable

A

=more acidic

63
Q

w/in a group look at…

A

bond strength to determine acidity

64
Q

w/in a period look at…

A

polarity to determine acidity

65
Q

oxyacid

A

H,O, and nonmental: XOH

66
Q

as electronegativity increases, acidity…

A

increases

67
Q

oxidation # increase=

A

increase in acidity

68
Q

carboxylic acids

A

organic acids containing the -COOH group

69
Q

buffers

A

soln of weak acid and it’s conjugate or weak base and it’s conjugate

70
Q

buffer —— pH change

A

resist

71
Q

henderson-hasselback equation

A

pH=pKa+ log([A-]/[HA])

72
Q

when [HA]=[A-]…

A

pH=pKa

73
Q

equivalence point

A

when the amount of acid equals the amount of base

74
Q

titration of strong acid w/ strong base

A

pH=7 at equivalence point

75
Q

titration of weak acid w/ a strong base

A

at the equivalence point the pH>7

76
Q

titration of weak base w/ strong acid

A

at equivalence point the pH<7

77
Q

weak acid/ weak base titration pH=pKa at

A

halfway to the equivalence point

78
Q

Ksp=

A

[cation][anion] (w/ respect to coefficients and powers)

79
Q

solubility

A

the quantity of solute which can dissolve (g/L or mol/L)

80
Q

common ion effect

A

when one of the ions are in solution it affects the solubility of the salt by decreasing it

81
Q

when a salt has an anion that is the conj. base of a weak acid it is ——- soluble in an acidic solution

A

more

82
Q

when a salt has an anion that is the conj. base of a strong acid solubility ——-

A

is unchanged

83
Q

amphoteric oxides + hydroxides

A

ions which are soluble in strong acid or strong base

84
Q

Q=Ksp

A

at equilibrium, saturated, no ppt

85
Q

Q>Ksp

A

excess solute, ppt formed

86
Q

Q<Ksp

A

no ppt

87
Q

selective precipitation

A

ions can be separated from soln based on their solubilities in the presence of different ions

GEN CHEM 2 (3 decks)

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