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Byju's Answer
Standard XII
Chemistry
Salt of Weak Acid and Strong Base
Kb for a mono...
Question
K
b
for a monoacidic base whose
0.1
M
solution has a
p
H
of
10.50
is:
A
K
b
=
10
−
3
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B
K
b
=
10
−
6
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C
K
b
=
10
−
9
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D
None of these
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Solution
The correct option is
A
K
b
=
10
−
6
p
H
=
−
l
o
g
[
H
+
]
=
10.5
p
O
H
=
14
−
p
H
=
3.5
Also,
for a mono-acidic base
[
O
H
−
]
=
c
×
α
K
b
=
c
×
α
2
=
[
O
H
−
]
2
C
So by putting value of
C
=
0.1
M
, we get
K
b
=
10
−
6
Suggest Corrections
0
Similar questions
Q.
K
b
for a monoacidic base whose
0.2
M
solution has a
p
H
of
9.50
is:
Q.
Calculate
K
b
for a base whose
0.1
M
solution has pH of
10.5
.
Q.
1
M
weak monoacidic base
(
B
O
H
)
solution is dliuted by
100
times. The
p
H
change of the solution is:
(
K
b
=
10
−
5
)
Q.
pH of M/100 monoacidic base MOH having Kb = 4*10^(-4) is
A) 2.6990 B) 2.3010 C) 11.6990 D) 11.3010
Q.
Consider a weak monoacidic base
B
O
H
having a concentration C with dissociation
α
<
<
1.
The pH of this weak base in terms of base dissociation constant
K
b
and concentration
C
is :
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