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Byju's Answer
Standard XII
Chemistry
Molarity
Calculate the...
Question
Calculate the pH of the solution obtained by mixing
10
m
L
of
0.1
M
H
C
l
and
40
m
L
of
0.2
M
H
2
S
O
4
.
Open in App
Solution
[
H
+
]
=
N
1
×
V
1
+
N
2
×
V
2
V
[
H
+
]
=
10
×
0.1
+
40
×
0.4
50
=
0.34
p
H
=
−
l
o
g
(
[
H
+
]
)
=
0.4685
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0
Similar questions
Q.
A solution of weak acid
H
A
was titrated with base
N
a
O
H
. The equivalence point was reached when
36.12
m
L
of
0.1
M
N
a
O
H
has been added. Now
18.06
m
L
of
0.1
M
H
C
l
were added to titrated solution, the
p
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was found to be
4.92
. What will be the
p
H
of the solution obtained by mixing
10
m
L
of
0.2
M
N
a
O
H
and
10
m
L
of
0.2
M
H
A
?
Q.
Calculate the pH of solution obtained by mixing 10 mL of 0.1 M HCl and 40 mL of 0.2 M
H
2
S
O
4
.
Take log 3.4 = 0.53
Q.
Calculate the
p
H
of the resultant mixtures:
a) 10 mL of 0.2M
C
a
(
O
H
)
2
+ 25 mL of 0.1M
H
C
l
b) 10 mL of 0.01M
H
2
S
O
4
+ 10 mL of 0.01M
C
a
(
O
H
)
2
c) 10 mL of 0.1M
H
2
S
O
4
+ 10 mL of 0.1M
K
O
H
Q.
Calculate the
p
H
of the resulting solution formed by mixing the following solutions.
20
m
L
of
0.2
M
B
a
(
O
H
)
2
+
30
m
L
of
0.1
M
H
C
l
Q.
0.1
M
H
C
l
and
0.1
M
H
2
S
O
4
each of volume
2
m
L
are mixed and the volume is made up to
6
m
L
by adding
2
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L
of
0.01
N
N
a
C
l
solution. The pH of the resulting mixture is:
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