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Byju's Answer
Standard XII
Chemistry
Hyperconjugation
Calculate the...
Question
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
Open in App
Solution
(a)
H
2
→
2
H
+
+
2
e
E
H
2
/
H
+
=
E
∘
H
2
/
H
+
−
0.0591
2
log
[
H
+
]
2
P
H
2
=
0.0
−
0.0591
log
[
H
+
]
1
0.25
=
0.0591
p
H
p
H
=
0.25
0.0591
=
4.23
(b)
E
H
2
/
H
+
=
E
∘
H
2
/
H
+
−
0.0591
2
log
[
H
+
]
2
P
H
2
=
0.0
−
0.591
log
[
H
+
]
1
0.3
=
0.0591
p
H
p
H
=
0.3
0.0591
=
5.076
.
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0
Similar questions
Q.
The cell
P
t
(
H
2
)
(
1
a
t
m
)
|
H
+
(
p
H
=
?
)
,
I
−
(
a
=
1
)
/
A
g
l
(
s
)
,
A
g
h
a
s
e
m
f
,
E
298
K
=
0
. The electrode potential for the reaction
A
g
l
+
e
−
→
A
g
+
I
⊖
i
s
−
0.151
volt. Calculate the
p
H
value :-
Q.
Calculate the emf of the following cell:
P
t
(
H
2
1
a
t
m
)
|
C
H
3
C
H
2
C
O
H
(
0.15
M
)
|
|
0.01
M
N
H
4
O
H
|
H
2
(
1
a
t
m
)
P
t
K
a
for
C
H
3
C
H
2
C
O
O
H
=
1.4
×
10
−
5
K
b
for
N
H
4
O
H
1.8
×
10
−
5
.
Q.
Calculate the pH of following solutions:
Pt,
H
2
|
H
C
l
,
E
=
0.25
V
Q.
For the half cell reaction at 298 K,
H
+
(
a
q
)
+
e
−
→
1
2
H
2
(
g
)
(1 atm
)
Q.
What is pH of the half-cell
P
t
|
H
2
(
g
)
|
H
+
if
E
∘
H
+
|
H
2
=
−
0.0295
V
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