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Chem 102 > Exam 2 > Flashcards

Exam 2 Flashcards

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1
Q

Aqueous solution: solvent = ?

A

water = solvent

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2
Q

Dissociation

A

species break apart;
A –> B + C

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3
Q

Ionization

A

dissociation into 2 ionic species;
A –> B- + C+

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4
Q

M =

A

mol/L

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5
Q

Cm^3 =

A

mL

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6
Q

Equilibrium constant for dissociation in water @ 25°C (Kw) =

A

1.0 x 10^(-14)

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7
Q

[H+] > 1 x 10^(-7) M =

A

acidic!
(implies [OH-] < 1 x 10^(-7) M)

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8
Q

[H+] < 1 x 10^(-7) M =

A

basic!
(implies [OH-] > 1 x 10^(-7) M)

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9
Q

[H+] = 1 x 10^(-7) M =

A

neutral!
(implies [OH-] = 1 x 10^(-7) M)

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10
Q

pH

A

calculated w/ equilibrium concentration of H+ and OH-

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11
Q

↑ acidity = ____ pH

A

↓ pH

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12
Q

↑ basic = _____pOH

A

↓pOH

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13
Q

↑ pH = _____ pOH

A

↓ pOH (inverse)

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14
Q

pOH + pH =

A

14 (at 298 K)

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15
Q

pH < 7 =

A

acidic

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16
Q

pH = 7

A

neutral

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17
Q

pH > 7

A

basic

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18
Q

strong acids (list):

A

HCl, HBr, HI, HNO3, HClO4, H2SO4

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19
Q

strong bases (list):

A

Group 1: LiOH, NaOH, KOH
Group 2: Ca(OH)2, Sr(OH)2, Ba(OH)2

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20
Q

Strong acids (SA):

A
  • completely ionize in water
  • Release 1 mol H+ / 1 mole of strong acid in water
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21
Q

Group 1A (alkali metals) strong bases:

A

Release 1 mol OH- / 1 mol strong base in water

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22
Q

Group 2A (alkaline earth metals) strong bases:

A

Release 2 mol OH- / 1 mol strong base in water

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23
Q

Weak acid:

A

partially dissociate in water
- Holds onto proton
- Smaller dissociation constants

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24
Q

Ka =

A

(products) / (reactants)

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25
Q

Cations behave like ___ ____ except strong bases (Li+, Na+, Ca2+, Sr2+, Ba2+)

A

weak acids

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26
Q

Weaker acid =

A

↓ Ka = ↑ pKa

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27
Q

Stronger acid =

A

↑ Ka = ↓ pKa

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28
Q

the acid dissociation constant of a weak acid will be…

A

much smaller than 1

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29
Q

Calculating H+ concentration due to a weak acid will invariably involve _____ ______

A

equilibrium tables!

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30
Q

cation

A

positively charged ion

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31
Q

anion

A

negatively charged ion

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32
Q

M =

A

mol/L (molarity)

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33
Q

x =

A

extent of hydroxide ionization

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34
Q

WGJ equation: x =

A

x = [OH-] = sqrt (KbMb) = (KbMb)^(1/2)

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35
Q

Weaker acid =

A

↓ Ka = ↑ pKa

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36
Q

Stronger acid =

A

↑ Ka = ↓ pKa

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37
Q

Weaker base =

A

↓ Kb = ↑ pKb

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38
Q

Stronger base =

A

↑ Kb = ↓ pKb

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39
Q

how basic are hydroxides?

A

the strongest bases!

40
Q

Bronsted Lowry model

A
  • acid = proton donor
  • base = proton acceptor
41
Q

Acid/base reaction = (another name)

A

proton transfer reaction

42
Q

Bronsted Lowry: Conjugate acid

A

formed when a proton (hydrogen ion) is added to a base
- H+ donor! (reactant)

43
Q

Bronsted Lowry: Conjugate base

A

formed when a proton (hydrogen ion) is removed from an acid
- loses an H+ (b/w reactants–>products)

44
Q

In the forward direction,

A

CA = H+ donor (reactant)
CB = lost an H+ (product)

45
Q

In the reverse direction,

A

CA = H+ donor (product)
CB = lost an H+ (reactant)

46
Q

Monoprotic acid

A

containing 1 ionizable proton (H+)

47
Q

Diprotic acid

A

containing 2 ionizable protons (H+)

48
Q

Polyprotic acid

A

containing multiple ionizable protons (H+)

49
Q

Sulfuric acid

A

strong acid w/ 2 H+ to give

50
Q

Second H+ is…

A

harder to remove than first
- Ka2 < Ka1

51
Q

Conjugate Acid

A

proton donor (loses an H+ b/w reactants –> products)

52
Q

Conjugate Base

A

compound w/ 1 less H+ (product)
- usually (-)

53
Q

if conjugate acid is strong, conjugate base is usually…

A

weak

54
Q

if conjugate bas is strong, conjugate acid is usually…

A

weak

55
Q

many anions (-) behave as __ in water…

A

weak base

56
Q

many cations (+) behave as ___ in water…

A

weak acids

57
Q

titration

A

driven acid/base reaction
- @ least 1 is strong: SA/SB, SA/WB, SB/WA

58
Q

buffer system

A

A/B/water solution (Acid + Base + Water)
- contains comparable amounts of conjugates (ex: 1:10 or 10:1 or 3:5 –> close)
- moL A/ moL B / in water where moL A ≈ moL B

59
Q

Ka (cation) > Kb (anion) =

A

acidic

60
Q

Ka (cation) < Kb (anion) =

A

basic

61
Q

pKa (cation) > pKb (anion) =

A

acidic

62
Q

pKa (cation) > pKb (anion) =

A

basic

63
Q

A buffer is resistant to pH change from addition of a …

A

SMALL amount of strong acid or of strong base

64
Q

the buffer buffets the over-production of either __ or ___ . Thus, a buffer is resistant to __ or ___ change.

A

H+ or OH-ion
- to pH or pOH change

65
Q

if the strong species is the limiting reactant….

A

you will have a buffer at the end of the reaction

66
Q

if you use mols, you must use ___ for volume

A

Liters

67
Q

if you use mL for volume, you must use

A

mm. mol

68
Q

For conjugates, pKb + pKa =

A

14

69
Q

steps to identify if a solution is a buffer after a reaction?

A
  1. cross out spectator ions
  2. if both are weak; do you have HB/B-? = buffer!
    - if not (SA/WB, SB/WA, or SA/SB):
  3. if SA/SB: no buffer (unless Mol SA = Mol SB)
  4. if SA/WB or WB/SA: write net ionic (mol ~= mol?)
70
Q

Can you demonstrate how HClO2 behaves as a weak acid in water?

A

HClO2 (aq) –>/<– H+ (aq) + ClO2 ̄ (aq)

71
Q

When can the protons, H+, released by the water reaction be ignored compared to the protons
released by a weak acid in water?

A

protons released by water dissociation can be ignored compared to those
released by a WA in water when…
sqrt(KwMw) =7.5 &laquo_space;sqrt(KaM)

72
Q

define buffer

A

an aqueous system containing comparable amounts of a weak acid, HB, and its conjugate weak base B ̄ —perhaps after a reaction!!!

73
Q

limiting reactant is…

A

the reactant that results in the least amount of product if all other reactants were in excess

74
Q

when a strong acid (SA) is added to an (aq) solution w/ a weak base (WB) a ___ will occur

A

titration

75
Q

if the weak species = limiting reactant, there will be ____ after the reaction.

A

NO BUFFER

76
Q

you can replace strong acids w/ ____ in the reaction b/w SA/SB

A

H+ (aq)
- H+ + OH- –> H2O

77
Q

you can replace strong bases w/ ____ in the reaction b/w SA/SB

A

OH- (aq)
- H+ + OH- –> H2O

78
Q

you can replace strong acids w/ ____ in the reaction b/w SA/WB

A

H3O+
- H3O+ + B- –> HB + OH-

79
Q

you can replace weak bases w/ ____ in the reaction b/w SA/WB

A

B-
- H3O+ + B- –> HB + OH-

80
Q

you can replace strong bases w/ ____ in the reaction b/w SB/WA

A

OH-
- OH- + HB –> B- + H2O

81
Q

you can replace weak acids w/ ___ in the reaction b/w SB/WA

A

HB
- OH- + HB –> B- + H2O

82
Q

INDICATORS are subtances added…

A

in a few drops to a solution
- the solution is titrated and the indicator changes color as a function of the solution pH
-they are weak acids (Hin) that change color according as HIn or In- is the predominant species in the solution to be examined

83
Q

The indicator solution changes color when

A

[In-] ~ [HIn]; the precise condition [In-] = [HIn] is called the endpoint of the titration (when color changes)

84
Q

at the endpoint of the titration, ______ relationship exists

A

[H+] = Ka –> pKa = pH

85
Q

titrating a SA/WB, the equivalence point will occur at ___

A

pH < 7

86
Q

titrating a SA/SB, the equivalence point will occur at ____

A

pH = 7

87
Q

titrating a WA/SB, the equivalence point will occur at ___

A

pH > 7

88
Q

at equivalence point, the mmMoL product =

A

mmMoL reactant

89
Q

in a buffer regime:

A

as long as added OH- < 25 mmMoL, you will have a buffer regime (region)

90
Q

titration curve: stronger acid =

A

more narrow curve (more vertical)

91
Q

A/B/N: anion (-)

A

basic
- neutral if part of SA/SB

92
Q

A/B/N: cation (+)

A

acidic
- neutral if part SA/SB

93
Q

A/B/N: neutral if…

A

part of SA/SB (memorized list!)

94
Q

Bronsted Lowry: pKb + pKa =

A

14

95
Q

if given Ka1 and Ka2, use ___ for x = sqrt(M*K)

A

ONLY the larger Ka

96
Q

equivalence point

A

point in titration at which the amount of titrant added is just enough to completely neutralize the analyte solution
- strong species = 100%

Chem 102 (6 decks)

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