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Standard XII
Chemistry
Ostwald Dilution Law
Question
0.02
M
solution of
N
H
4
O
H
is
3
% dissociated. Calculate the dissociation constant of
N
H
4
O
H
.
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Solution
Verified by Toppr
N
H
4
O
H
⇌
N
H
4
+
O
H
−
K
=
[
N
H
+
4
]
[
O
H
−
]
[
N
H
4
O
H
]
K
=
[
N
H
+
4
]
[
O
H
−
]
[
N
H
4
O
H
]
=
C
α
×
C
α
C
(
1
−
α
)
≃
C
α
2
=
0.02
×
(
0.03
)
2
=
1.8
×
10
−
5
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Similar Questions
Q1
0.02
M
solution of
N
H
4
O
H
is
3
% dissociated. Calculate the dissociation constant of
N
H
4
O
H
.
View Solution
Q2
Calculate the pH of
0.01
M
N
H
4
O
H
solution having 2% dissociation.
View Solution
Q3
Dissociation constants of
C
H
3
C
O
O
H
and
N
H
4
O
H
in aqueous solution are
10
−
5
. If pH of a
C
H
3
C
O
O
H
solution is
3
. What will be the pH of
N
H
4
O
H
?
View Solution
Q4
Calculate pH of
0.002
N
N
H
4
O
H
having 2 % dissociation.
View Solution
Q5
Degree of dissociation of
N
H
4
O
H
in water is
1.8
×
10
−
5
, then hydrolysis constant of
N
H
4
O
H
is:
View Solution