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Acids & Bases > Acids & Bases > Flashcards

Acids & Bases Flashcards

Acid-base chemistry, identification of strong, weak, and negligible acids and bases.

1
Q

HI –>

A

strong acid

Conjugate base = I- (negligible)

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2
Q

HBr –>

A

strong acid

Conjugate base = Br- (negligible)

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3
Q

HCl –>

A

strong acid

Conjugate base = Cl- (negligible)

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4
Q

H2SO4 –>

A

strong acid

Conjugate base = HSO4- (negligible)

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5
Q

HNO3 –>

A

strong acid

Conjugate base: NO3- (negligible)

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6
Q

HClO4 –>

A

strong acid

Conjugate base = ClO4- (negligible)

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7
Q

HClO3 –>

A

strong acid

Conjugate base = ClO3- (negligible)

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8
Q

HSO4- <=>

A

weak acid

Conjugate base = SO4^2-

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9
Q

H3PO4 <=>

A

weak acid

Conjugate base = H2PO4-

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10
Q

HF <=>

A

weak acid

Conjugate base = F-

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11
Q

CH3COOH <=>

A

weak acid

Conjugate base = CH3COO-

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12
Q

H2CO3 <=>

A

weak acid

Conjugate base = HCO3-

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13
Q

H2S <=>

A

weak acid

Conjugate base = HS-

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14
Q

H2PO4- <=>

A

weak acid

Conjugate base = HPO4^2-

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15
Q

NH4+ <=>

A

weak acid

Conjugate base = NH3

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16
Q

HCO3- <=>

A

weak acid

Conjugate base = CO3^2-

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17
Q

HPO4^2- <=>

A

weak acid

Conjugate base = PO4^3-

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18
Q

OH- –>

A

strong base

Conjugate acid = O^2-

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19
Q

H2 –>

A

strong base

Conjugate acid = H-

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20
Q

CH4 –>

A

strong base

Conjugate acid = CH3-

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21
Q

The Inductive Effect

A

In general, the more electronegative the atoms, the stronger the oxyacid ( hydrogen attached to oxygen)

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22
Q

oxyacid

A

an acid where acidic proton (H+) is attached to an oxygen

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23
Q

weaker O-H bond =

A

stronger acid

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24
Q

stronger O-H bond =

A

weaker acid

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25
Q

more oxygens =

A

stronger oxyacid

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26
Q

the stronger the acid =

A

the weaker the conjugate base

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27
Q

the stronger the base =

A

the weaker the conjugate acid

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28
Q

strong acids

A

dissociate completely in the forward direction

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29
Q

strong bases

A

dissociate completely in the backwards direction

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30
Q

weak acids and bases

A

dissociate partially in the forward direction, these undergo acid/base equilibria

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31
Q

negligible acids and bases

A

too weak to be called weak, they are just spectator ions

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32
Q

the conjugate of a strong acid is a…

A

… negligible base

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33
Q

the conjugate of a strong base is a…

A

… negligible acid

34
Q

The Taylor Swift Hypothesis

A

once a strong acid dissociates, it will never ever ever get back together

35
Q

weaker acid =

A

stronger conjugate base

36
Q

stronger acid =

A

weaker conjugate base

37
Q

weaker base =

A

stronger conjugate acid

38
Q

stronger base =

A

weaker conjugate acid

39
Q

the conjugate of a weak thing is…

A

a weak thing

40
Q

Arrhenius acid

A

any compound that dissociates in water to form H3O+

41
Q

Arrhenius base

A

any compound that dissociates in water to form OH-

42
Q

Brønsted-Lowry acid

A

a compound that donates H+

43
Q

Brønsted-Lowry base

A

a compound that accepts H+

44
Q

Lewis acid

A

a compound that accepts electrons (becomes more negative)

45
Q

Lewis base

A

a compound that donates electrons (becomes less negative)

46
Q

transition metals and any cation that isn’t group I or group II metal calcium and below are…

A

… acids

47
Q

transition (and post-transition) metal cations are…

A

… acidic in water

48
Q

Lewis acids can have a…

A

… positive or neutral charge & need/want/can accept more electron density

49
Q

What factors make for a stronger Lewis Acid?

A
  • higher charge
  • smaller size
  • water can get closer
  • stronger interaction
50
Q

Lewis Bases can have a…

A

… negative or neutral charge & need to have a lone pair of electrons to donate

51
Q

Acidic solution concentrations

A

[H+] > [OH-]

52
Q

Neutral solution concentrations

A

[H+] = [OH-]

53
Q

Basic solution concentrations

A

[H+] < [OH-]

54
Q

What is the equilibrium constant expression for auto-ionization of water?

A

Kw[H+][OH-]

55
Q

equation to calculate pH

A

pH = -log [H+]

56
Q

equation to calculate pOH

A

pOH = -log [OH-]

57
Q

at 25 degrees Celcius

A

pH + pOH = 14

58
Q

low pH =

A

High [H+]

59
Q

high pH =

A

Low [H+]

60
Q

Kw = [H+][OH-] @25 C

A

1.0 x 10^-14

61
Q

pKw = -log(Kw)

A

14

62
Q

“p” =

A

-log

63
Q

electrolytes

A

charged particles carry current

64
Q

For a strong acid in aqueous solution:

A

[HA] initial = [H+] final

65
Q

For a weak acid in aqueous solution

A

[HA] initial > [H+] final

66
Q

When in doubt?

A

ICE IT OUT

67
Q

Ka equation for a weak acid, HA

A

Ka = [H+][A-]/[HA]

68
Q

Ka of weaker acids

A

really really small number (ex. 6.8 x 10^-4)

69
Q

Ka of strong acids

A

really really big number (ex. 3.2 x 10^9)

70
Q

4-step process for GREAT results

A
  1. write out the reaction
  2. fill out your ICE table
  3. write equilibrium expression
  4. SOLVE
71
Q

LiOH

A

strong base

72
Q

NaOH

A

strong base

73
Q

KOH

A

strong base

74
Q

RbOH

A

strong base

75
Q

CsOH

A

strong base

76
Q

Ca(OH)2

A

strong base

77
Q

Sr(OH)2

A

strong base

78
Q

Ba(OH)2

A

strong base

79
Q

O2-

A

strong base

80
Q

H-

A

strong base

81
Q

NH2-

A

strong base

Acids & Bases (1 decks)

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