Chp.15 and 16 Flashcards
1
Q
A Brønsted acid is a proton
A
donor
2
Q
A Brønsted base is a proton
A
acceptor
3
Q
H+] = [OH-]
A
neutral
4
Q
[H+] > [OH-]
A
acidic
5
Q
[H+] < [OH-]
A
basic
6
Q
common weak acids
A
acetic acid-HC2H3O2 or CH3COOH
carbonic acid-H2CO3
hydroflouric acid-HF
phosphoric acid-H3PO4
7
Q
CH2COOH
A
weak acid (acetic acid)
8
Q
CCI3COOH
A
weak acid
9
Q
HF
A
weak acid, hydrofluoric acid
10
Q
HNO2
A
weak acid (nitrous acid)
11
Q
C2H2O4
A
weak acid (Oxalic acid)
12
Q
HCOOH
A
weak acid (formic acid)
13
Q
H2SO3
A
weak acid (sulfurous acid)
14
Q
LiOH
A
strong base
15
Q
NaOh
A
strong base
16
Q
KOH
A
strong base
17
Q
RbOH
A
strong base
18
Q
CaOH
A
strong base
19
Q
Sr(OH)2
A
strong base
20
Q
Ba(OH)2
A
strong base
21
Q
NH4OH
A
weak base
22
Q
N(CH3)3
A
weak base
23
Q
C5H5N
A
weak base
24
Q
H2O
A
weak base
25
HCLO4
strong acid
26
HCl
strong acid
27
HBr
strong acid
28
Hl
strong acid
29
HNO3
strong acid
30
H2SO4
strong acid
31
Buffer solution
consists of a weak acid and its conjugate base; Resist changes in pH
32
A buffer solution can be found in
blood
33
Buffer example
CH3COOH (weak acid) + H2) <> CH3COO- (conjugate base
34
Other examples
CH3CHOOH/C
HNO2/NO2-
NH4+/NH3
35
Examples of non-buffer
HCL/CL- 2-
HNO3/NO3-
H2SO4/SO4
36
What makes a buffer solutio
a weak acid and its conjugate base
37
What does not make a buffer solution
a strong acid and its conjugate base
38
Ka =
[H+][A-]/[HA]
39
[H+] =
Ka x [HA]/[A-]
40
-log[H+]=
ph (-log Ka * [Ha]/[H]
41
pH=
pka + log ([A-]/[HA])
-log([H+])
42
lower the pKa
stronger acid
43
Higher Ka
strong acid
44
Henderson-Hasselbalch equation
pH = pKa + log [A-]/[HA] (pH = pKa)
