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Princeton Chemistry > Acids and Bases > Flashcards

Acids and Bases Flashcards

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1
Q

bronsted acid

A
  • donates H+
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2
Q

lewis acid

A
  • accepts e-

- electrophile

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3
Q

bronsted base

A
  • accepts H+
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4
Q

lewis base

A
  • donates e-

- nucleophile

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5
Q

acid

A
  • e- acceptor
  • H+ donor
  • electrophile
  • leaving group
  • ox. agent (gets reduced)
  • cation
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6
Q

base

A
  • e- donor
  • H+ acceptor
  • nucleophile
  • part that isn’t LG
  • reducing agents (gets oxidized)
  • anion
  • ligand/chelate
  • coordinate bond
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7
Q

recognizing acids

A
  • generally have more electronegative atoms bonded to H
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8
Q

recognizing bases

A
  • generally have less electronegative atoms with lone pairs
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9
Q

atoms without H

A
  • can be acids if electron deficient or with large positive charges
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10
Q

atoms without lone pairs

A
  • are not usually basic
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11
Q

amphoteric compounds

A
  • have characteristics of both acids and bases
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12
Q

stability of conjugate

A
  • tells strength of original

- if very stable, is not very strong so the original is strong

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13
Q

increases acidity

A
  • more positive charge
  • more electronegative atom
  • larger atom
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14
Q

increases basicity

A
  • more negative charge
  • less electronegative
  • smaller atom
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15
Q

acid dissociation constant

A

[A:-][H3O+]
_________ = Ka
[HA}

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16
Q

increased Ka

A
  • increased numerator
  • increased products
  • increased acidity
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17
Q

decreased Ka

A
  • decreased acidity
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18
Q

base dissociation constant

A

[BH+][HO-]
_________ = Kb
[B}

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19
Q

increased Kb

A
  • increased numerator
  • increased products
  • increased basicity
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20
Q

decreased Kb

A
  • decreased basicity
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21
Q

strong acids

A
  • dissociate completely
  • Ka > 1
  • equilibrium favors products
  • produce bases so weak they’re not basic
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22
Q

weak acids

A
  • partially dissociate
  • Ka < 1
  • equilibrium factors reactants
  • produce strong conjugate bases (not necessarily strong bases)
23
Q

strong bases

A
  • dissociate completely

- Kb > 1

24
Q

weak bases

A
  • partially dissociate

- Kb < 1

25
Q

common strong acids

A
  • H2SO4 (diprotic)
  • HClO4
  • HCl
  • HBr
  • HI
26
Q

common strong bases

A
  • O2- (diprotic)
  • OH-
  • OR-
  • NH2-
  • NR2-
  • H-
  • R-
27
Q

acidic salt

A
  • contains an ion that is a weak acid
28
Q

basic salt

A
  • contains an ion that is a weak base
29
Q

group 1 and 2 cation

A
  • are not acidic
30
Q

what does p mean

A
  • inverse
31
Q

formula for pH

A
  • pH= -log[H+]
32
Q

formula for pKa

A
  • pKa= -log[Ka]
33
Q

autoionization of H2O formulas

A

pH + pOH = 14
KaKb = Kw = 1e-14
pKa + pKb = PKw = 14

34
Q

as A increases

A
  • Ka increases

- pKa decreases

35
Q

as B increases

A
  • Kb increases

- pKb decreases

36
Q

strong acid or base calculation

A
  • assume complete dissociation

- pH = - log [H3O+]

37
Q

weak acid or base calculation

A
  • use Ka or Kb to determine how much dissociates

Ka = [A:-](H3O+]
______________
[HA]

38
Q

buffer calculation

A
  • use Henderson Hasselbach
39
Q

buffers

A
  • mixtures of conjugate acid/base pairs

- minimize changes in pH

40
Q

Henderson-Hasselbach equation

A

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

41
Q

a reaction between an acid and a base

A
  • neutralization reaction
42
Q

conjugate acid/base of a strong acid/base

A
  • unreactive
  • spectator ion
  • pH neutral
43
Q

conjugate acid/base of a weak acid/base

A
  • weakly reactive but still somewhat reactive
44
Q

half equivalence point

A
  • where it goes more horizontal
45
Q

equivalence point

A
  • mol H+ = mol OH-

- goes vertical again

46
Q

where is the equivalence point in a titration of a strong base with a weak acid?

A
  • greater than 7
47
Q

where is the equivalence point in a titration of a weak base with a strong acid

A
  • less than 7
48
Q

titration curve of a diprotic acid with a strong base

A
  • 2 half equivalence and 2 equivalence points

- first equivalence point will be less than 7. The second equivalence point will be greater than 7

49
Q

color indicators in terms of pH and pKa

A
  • pH < pKa color 1
  • pH = pKA mix of color 1 and color 2
  • pH > pKa color 2
50
Q

way to remember Lewis acid/base

A
  • same lewis from dot structures concerned with electrons
51
Q

algebraic solution from ICE table

A

pH = -1/2 log (Ka [WA])

OR

pOH = -1/2 log (Kb [WB])

52
Q

neutralization reactants are always

A
  • exothermic
53
Q

half equivalence point

A
  • point at which 50% of the acid is dissociated.
  • pKa of the weak acid or base
  • if you have the base then 14-pKa=pKb
54
Q

first equivalence point of a diprotic

A
  • 1/2 (pKa1 + pKa2)

- also called isoelectric point

Princeton Chemistry (6 decks)

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