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Byju's Answer
Standard XII
Chemistry
Basic Buffer Action
Calculate the...
Question
Calculate the pH of
0.1
M
solution of
N
H
4
O
C
N
.
K
b
for
N
H
3
is
1.75
×
10
−
5
and
K
a
for
H
O
C
N
is
3.3
×
10
−
4
.
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Solution
Ammonium acetate is a salt of weak acid and weak base.
So
p
H
=
7
+
1
2
(
p
K
a
−
p
K
b
)
p
H
=
7
+
1
2
(
−
log
K
a
+
log
K
b
)
p
H
=
7
+
1
2
(
log
1.75
×
10
−
5
3.3
×
10
−
4
)
p
H
=
7
−
0.635
=
6.365
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0
Similar questions
Q.
[
H
+
]
in a solution containing
0.1
M
H
C
O
O
H
and
0.1
M
H
O
C
N
is
X
×
10
−
3
M
. Nearest integer to X is
K
a
for
H
C
O
O
H
and
H
O
C
N
are
1.8
×
10
−
4
and
3.3
×
10
−
4
respectively
Q.
Calculate
[
H
+
]
in a solution containing
0.1
M
H
C
O
O
H
and
0.1
M
H
O
C
N
.
K
a
for
H
C
O
O
H
and
H
O
C
N
are
1.8
×
10
−
4
and
3.3
×
10
−
4
respectively.
Q.
A mixture of weak acid is 01M in
H
C
O
O
H
(
K
a
=
1.8
×
10
−
4
)
and 0.1M in
H
O
C
N
(
K
a
=
3.3
×
10
−
4
)
. Hence,
[
H
3
O
+
]
is:
Q.
Calculate the
p
H
of
0.01
M solution of
N
H
4
C
N
. The dissociation constants
K
a
for
H
C
N
=
6.2
×
10
−
10
and
K
b
for
N
H
3
=
1.6
×
10
−
5
.
Q.
Calculate the percentage of hydrolysis in
0.003
M
aqueous solution of
N
a
O
C
N
.
K
a
for
H
O
C
N
=
3.33
×
10
−
4
.
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