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Byju's Answer
Standard XII
Chemistry
Equilibrium Constant from Nernst Equation
Calculate the...
Question
Calculate the pH of following solutions:
Pt,
H
2
|
H
C
l
,
E
=
0.25
V
Open in App
Solution
1
2
H
2
→
H
+
+
e
−
E =
E
0
−
0.0591
n
l
o
g
H
+
0.25 = 0 +
0.0591
1
p
H
pH = 4.230
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Similar questions
Q.
Calculate the
p
H
of the following half-cells solutions:
(a)
P
t
H
2
(
1
a
t
m
)
|
H
+
(
H
C
l
)
;
E
=
0.25
v
o
l
t
(b)
P
t
H
2
(
1
a
t
m
)
|
H
+
(
H
2
S
O
4
)
;
E
=
0.3
v
o
l
t
Q.
For the cell
P
t
|
H
2
(
1
a
t
m
)
|
H
C
l
(
0.01
M
)
|
|
H
C
l
(
p
H
=
X
)
|
H
2
(
0.01
a
t
m
)
|
P
t
. Calculate x, when there is no flow of electricity.
Q.
The emf of the following cell at
25
o
C
.
P
t
,
H
2
P
1
=
2
a
t
m
,
|
H
C
l
|
P
t
,
H
2
P
2
=
10
a
t
m
[
E
o
c
e
l
l
=
0.0
v
;
2.303
R
T
F
=
0.0591
]
Q.
pH of a dilute solution HCL of is 6.95.
Calculate molarity of HCL solution.
Q.
The pH of the solution
0.1
M
H
2
S
O
4
(
50
m
L
)
+
0.4
M
H
C
l
50
(
m
L
)
is:
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