(II): Titration of Weak acid Vs Strong base:
Titration of a weak acid
by strong base is a bit more complex than both acid and base are strong this is
because we have consideration the equilibrium involving the weak acid and its
conjugate base.
Titration Table and curve:
|
S.N |
Acid
(0.1M) |
Base (0.1M ) |
pH |
Nature |
Case |
|
1 |
|
0 ml |
2.85 |
WA |
pH=1/2(Pka –logC) |
|
2 |
Volume |
5 ml |
4.22 |
ABS |
pH=(Pka +log [S]/[A] |
|
3 |
Taken |
10 ml |
4.7 |
ABS |
pH=Pka Best Buffer |
|
4 |
20.0 ml |
15 ml |
5.17 |
ABS |
pH=(Pka +log [S]/[A] |
|
5 |
Ka for |
19 ml |
5.98 |
ABS |
pH=(Pka +log [S]/[A] |
|
**6 |
CH3COOH |
20 ml |
8.7 |
SH |
pH=7+1/2(Pka+logC) |
|
7 |
2* 10^-10 |
21 ml |
11.39 |
SB |
NbVb - NaVa=NrVr |
|
8 |
|
25 ml |
12.04 |
SB |
[OH-]= Nr |
|
9 |
|
30 ml |
12.3 |
SB |
Strong base |
|
10 |
|
|
|
|
Remains present |
In titration of any weak acid with strong base, The pH at equivalent point will be greater than “7”
