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Byju's Answer
Standard XII
Chemistry
Electrolytes
Calculate the...
Question
Calculate the percentage ionization of 0.01M acetic acid in 0.1M
H
C
l
.
K
a
of acetic acid is
1.8
×
10
−
5
.
A
0.18
%
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B
0.018
%
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C
1.8
%
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D
18
%
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Solution
The correct option is
C
0.018
%
H
C
l
⇌
H
+
+
C
l
−
initial
0.1
0
0
0
0.1
0.1
after it's complete dissociation
H
2
O
is also added in case of weak acid
C
H
3
C
O
O
H
+
H
2
O
(
l
)
⇌
C
H
3
C
O
O
−
+
H
+
initial
0.01
0
0
0.1
(from
H
C
l
dissociation)
0.01
−
x
0
x
x
+
0.1
(after dissociation)
K
a
=
[
C
H
3
C
O
O
−
]
[
H
+
]
[
C
H
3
C
O
O
H
]
given,
K
a
of acetic acid
=
1.8
×
10
−
5
1.8
×
10
−
5
=
x
(
0.1
+
x
)
0.01
1.8
×
10
−
7
=
x
(
0.1
)
+
x
2
↘
negligible
x
=
1.8
×
10
−
7
0.1
x
=
1.8
×
10
−
6
M
So, % ionisation of acid
=
x
0.01
×
100
=
1.8
×
10
−
2
%
=
0.018
%
Percentage ionisation is
0.018
%
Suggest Corrections
0
Similar questions
Q.
The
[
H
+
]
of a resulting solution that is
0.01
M
acetic acid
(
K
a
=
1.8
×
10
−
5
)
and
0.01
M
in benzoic acid
(
K
a
=
6.3
×
10
−
5
)
:
Q.
5.0
m
L
of
0.1
M
N
a
O
H
solution is added to
50
m
L
of the
0.1
M
acetic acid solution. Calculate the
p
H
of the resulting acetic acid solution.
(
K
a
=
1.8
×
10
−
5
)
Q.
The degree of ionization of
0.4
M
acetic acid will be:
(
K
a
=
1.8
×
10
−
5
)
Q.
Find the percentage ionization of
0.2
M acetic acid solution, whose disassociation constant is
1.8
×
10
−
5
Q.
Calculate
H
+
ion concentration from acetic acid
(
C
H
3
C
O
O
H
)
if 0.2 mole of
H
C
l
is added to 1 L of the solution
For acetic acid
K
a
=
1.8
×
10
−
5
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