Acids and Bases Flashcards
1
Q
bronsted acid
A
- donates H+
2
Q
lewis acid
A
- accepts e-
- electrophile
3
Q
bronsted base
A
- accepts H+
4
Q
lewis base
A
- donates e-
- nucleophile
5
Q
acid
A
- e- acceptor
- H+ donor
- electrophile
- leaving group
- ox. agent (gets reduced)
- cation
6
Q
base
A
- e- donor
- H+ acceptor
- nucleophile
- part that isn’t LG
- reducing agents (gets oxidized)
- anion
- ligand/chelate
- coordinate bond
7
Q
recognizing acids
A
- generally have more electronegative atoms bonded to H
8
Q
recognizing bases
A
- generally have less electronegative atoms with lone pairs
9
Q
atoms without H
A
- can be acids if electron deficient or with large positive charges
10
Q
atoms without lone pairs
A
- are not usually basic
11
Q
amphoteric compounds
A
- have characteristics of both acids and bases
12
Q
stability of conjugate
A
- tells strength of original
- if very stable, is not very strong so the original is strong
13
Q
increases acidity
A
- more positive charge
- more electronegative atom
- larger atom
14
Q
increases basicity
A
- more negative charge
- less electronegative
- smaller atom
15
Q
acid dissociation constant
A
[A:-][H3O+]
_________ = Ka
[HA}
16
Q
increased Ka
A
- increased numerator
- increased products
- increased acidity
17
Q
decreased Ka
A
- decreased acidity
18
Q
base dissociation constant
A
[BH+][HO-]
_________ = Kb
[B}
19
Q
increased Kb
A
- increased numerator
- increased products
- increased basicity
20
Q
decreased Kb
A
- decreased basicity
21
Q
strong acids
A
- dissociate completely
- Ka > 1
- equilibrium favors products
- produce bases so weak they’re not basic
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
common strong acids
- H2SO4 (diprotic)
- HClO4
- HCl
- HBr
- HI
26
common strong bases
- O2- (diprotic)
- OH-
- OR-
- NH2-
- NR2-
- H-
- R-
27
acidic salt
- contains an ion that is a weak acid
28
basic salt
- contains an ion that is a weak base
29
group 1 and 2 cation
- are not acidic
30
what does p mean
- inverse
31
formula for pH
- pH= -log[H+]
32
formula for pKa
- pKa= -log[Ka]
33
autoionization of H2O formulas
pH + pOH = 14
KaKb = Kw = 1e-14
pKa + pKb = PKw = 14
34
as A increases
- Ka increases
| - pKa decreases
35
as B increases
- Kb increases
| - pKb decreases
36
strong acid or base calculation
- assume complete dissociation
| - pH = - log [H3O+]
37
weak acid or base calculation
- use Ka or Kb to determine how much dissociates
Ka = [A:-](H3O+]
______________
[HA]
38
buffer calculation
- use Henderson Hasselbach
39
buffers
- mixtures of conjugate acid/base pairs
| - minimize changes in pH
40
Henderson-Hasselbach equation
pH = pKa + log [A-]/[HA]
41
a reaction between an acid and a base
- neutralization reaction
42
conjugate acid/base of a strong acid/base
- unreactive
- spectator ion
- pH neutral
43
conjugate acid/base of a weak acid/base
- weakly reactive but still somewhat reactive
44
half equivalence point
- where it goes more horizontal
45
equivalence point
- mol H+ = mol OH-
| - goes vertical again
46
where is the equivalence point in a titration of a strong base with a weak acid?
- greater than 7
47
where is the equivalence point in a titration of a weak base with a strong acid
- less than 7
48
titration curve of a diprotic acid with a strong base
- 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
color indicators in terms of pH and pKa
- pH < pKa color 1
- pH = pKA mix of color 1 and color 2
- pH > pKa color 2
50
way to remember Lewis acid/base
- same lewis from dot structures concerned with electrons
51
algebraic solution from ICE table
pH = -1/2 log (Ka [WA])
OR
pOH = -1/2 log (Kb [WB])
52
neutralization reactants are always
- exothermic
53
half equivalence point
- 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
first equivalence point of a diprotic
- 1/2 (pKa1 + pKa2)
| - also called isoelectric point
