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Byju's Answer
Standard XII
Chemistry
Salt of Strong Acid and Weak Base
Calculate the...
Question
Calculate the
K
h
and pH of 0.05N
N
H
4
C
l
solution where
K
b
=
1.8
×
10
−
5
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Solution
For salt of weak base, strong acid like
N
H
3
C
l
,
K
h
=
K
w
K
b
=
10
−
14
1.8
×
10
−
5
=
5.56
×
10
−
10
p
H
=
7
−
1
2
[
p
K
b
+
log
C
]
=
7
−
1
2
{
[
−
log
(
1.8
×
10
−
5
)
]
+
log
0.05
}
=
p
H
=
5.28
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Similar questions
Q.
Calculate the pH of the buffer solution containing
0.15
m
o
l
e
of
N
H
4
O
H
and
0.25
m
o
l
e
of
N
H
4
C
l
.
K
b
for
N
H
4
O
H
is
1.8
×
10
−
5
Q.
Calculate the mass of
N
H
4
C
l
dissolved in
500
m
l
to have
p
H
=
4.5
. (
K
b
of
N
H
4
O
H
=
1.8
×
10
−
5
)
Q.
Calculate the
p
H
of
0.1
M
N
H
4
C
l
solution in water :
K
b
(
N
H
4
O
H
)
=
1.8
×
10
−
5
,
l
o
g
1.8
=
0.25
Q.
Calculate amount of
N
H
4
C
l
required to be dissolved in
500
m
L
water to have
p
H
=
5.
[
K
b
N
H
4
O
H
=
1.8
×
10
−
5
]
.
(Molar mass of
N
H
4
C
l
=
53.5
g
m
o
l
−
1
)
Q.
The
p
H
of a solution of
N
H
4
C
l
is 4.86. calculate the molar concentration of the solution if
K
b
=
1.0
×
10
−
5
and
K
w
=
1.0
×
10
−
14
.
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