Acids and Bases Flashcards
(27 cards)
1
Q
pH =
A
pH = -log[H3O+]
2
Q
[H3O+] =
A
[H3O+] = 10^-pH
3
Q
pOH =
A
pOH= -log[OH-]
4
Q
[OH-] =
A
[OH-] = 10^-pOH
5
Q
Kw =
A
Kw= [H3O+][OH-]
6
Q
Kw = [H3O+][OH-] =
A
1.00 x 10^-14 at 25’C
or pKw = 14.0
7
Q
[H3O+] = [OH-] means…
A
The reaction is neutral
8
Q
[H3O+]>[OH-] means…
A
The reaction is acidic
9
Q
[H3O+]
A
The reaction is basic
10
Q
Strong acids…
A
HCl; HBr; HI; HNO3; H2SO4; HClO4
11
Q
Strong bases…
A
MOH or M(OH)2
M= Group 1 or 2 metal
12
Q
HA + H2O =
A
HA + H20 = H3O+ + A-
Reaction lies well to the left
13
Q
Ka =
A
Ka = [H3O+][A-]/[HA]
14
Q
pKa =
A
pKa = -logKa
15
Q
Weak acid concentration =
A
[H3O+] ≈ (Ka x c) ^1/2
16
Q
B + H2O =
A
B + H2O = HB+ + OH-
the reaction lies well to the left
17
Q
Kb =
A
Kb = [OH-][HB+]/[B]
18
Q
pKb =
A
-logKb
19
Q
Weak base concentration =
A
[OH-] ≈ (Kb x c)^1/2
20
Q
Kw =
A
Kw = Ka x Kb
21
Q
Ka =
A
Ka = Kw/Kb
22
Q
Kb =
A
Kb = Kw/Ka
23
Q
pKw =
A
pKw = pKa + pKb
24
Q
pKa =
A
pKa = pKw - pKb
25
pKb =
pKb = pKw - pKa
26
At 25'C, pKa + pKb =
14.00
27
Henderson-Hasselbalch equation =
pH = pKa + log ([B]/[A])
