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Byju's Answer
Standard X
Chemistry
pH
Calculate the...
Question
Calculate the ration of pH of a solution containing 1 mole of
C
H
2
C
O
O
N
a
+ 1 mole of HCI per litre and of other solution containing 1 mole of
C
H
2
C
O
O
N
a
+ 1 mole of acetic acid per litre.
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Solution
C
H
3
C
O
O
N
a
+
H
C
l
⟶
C
H
3
C
O
O
H
+
N
a
C
l
m
o
l
e
s
b
e
f
o
r
e
r
x
n
1
m
o
l
e
s
a
f
t
e
r
r
x
n
0
1
0
0
1
0
1
[
C
H
3
C
O
O
H
]
=
1
1
=
1
m
o
l
e
[
H
+
]
=
c
α
=
c
√
K
a
c
=
√
K
a
c
=
√
K
a
c
=
1
p
H
1
=
1
2
l
o
g
K
a
f
o
r
C
H
3
C
O
O
N
a
+
C
H
3
C
O
O
H
1
m
o
l
e
+
1
m
o
l
e
p
H
2
=
−
log
K
a
+
log
1
1
=
−
log
K
a
H
e
n
c
e
t
h
e
r
a
t
i
o
w
i
l
l
b
e
p
H
1
+
p
H
2
=
1
:
2
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Similar questions
Q.
Calculate the ratio of
p
H
of a solution containing
1
m
o
l
e
of
C
H
3
C
O
O
N
a
+
1
m
o
l
e
of
H
C
l
per litre and of other solution containing
1
m
o
l
e
C
H
3
C
O
O
N
a
+
1
m
o
l
e
of acetic acid per litre
Q.
The ratio of
p
H
of a solution containing
1
mole of
C
H
3
C
O
O
N
a
+
1
mole of
H
C
l
per litre and of other solution containing
1
mole of
C
H
3
C
O
O
N
a
+
1
mole of acetic acid per litre is:
Q.
Calculate the ratio of pH of a solution containing 1 mol of
C
H
3
C
O
O
N
a
+ 1 mol of
H
C
l
per litre to another solution containing 1 mol of
C
H
3
C
O
O
N
a
+ 1 mol of acetic acid per litre.
Q.
What is the pH of the solution when 0.2 mole of hydrochloric acid is added to one litre of a solution containing 1 M acetic acid and acetate ion? Assume that the total volume is one litre.
K
a
for
CH
3
COOH
=
1.8
×
10
−
5
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