1.
pH and hydrolysis of salt
Prasenjit Bhunia

2.
2H2O H3O+
+ OH
-
H2O H+
+ OH
-
OR
H+ =
𝐾𝑤
OH−
=
10−14
OH−
OH− =
𝐾𝑤
H+
=
10−14
H+
H+ = OH− = 10−7 M
𝐾𝑤 = H+
OH−
= 10−14
(at 25°C)
𝑝𝐻
= −log⁡
[H+
]
𝐾𝑤 = H+ OH− = 10−12 (at 50°C)
𝑝𝐻 = 7
H+ = 10−7 M OH− = 10−7 M
𝑝𝑂𝐻 = 7
H+
OH−
= 10−14
𝑝𝐻 + 𝑝𝑂𝐻
= 14
𝑝𝐻 =?
H+
= OH−
= 10−6
M
𝑝𝐻 = 6
Søren Sørensen, Biochemist
Denmark, 1909

3.
Hydrolysis of Salt

4.
Salt formed from Nature pH equations
SA+SB Neutral No such equations
SA+WB Acidic
𝑝𝐻 = 7 − 𝑝𝐾𝑏 −
1
2
log 𝐶
WA+SB Basic
𝑝𝐻 = 7 +
1
2
𝑝𝐾𝑎 +
1
2
log 𝐶
WA+WB Depends
𝑝𝐻 = 7 +
1
2
𝑝𝐾𝑏 −
1
2
𝑝𝐾𝑏