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Byju's Answer
Standard XII
Chemistry
Salt of Weak Acid and Weak Base
One litre of ...
Question
One litre of a buffer solution has
0.13833
mole of acetic acid and
0.1951
mole of sodium acetate.
Calculate
p
H
(nearest integer) of solution.
Neglect volume change.
K
a
=
1.8
×
10
−
5
.
(log1.8 = 0.255)
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Solution
First, calculate the pKa value.
p
K
a
=
−
l
o
g
K
a
=
−
l
o
g
1.8
×
10
−
5
=
4.75
Now calculate the pH of the solution:
p
H
=
p
K
a
+
l
o
g
s
o
d
i
u
m
a
c
e
t
a
t
e
a
c
e
t
i
c
a
c
i
d
=
4.75
+
l
o
g
(
0.1951
0.13833
)
=
4.75
+
0.1440
=
4.8940
≈
5
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0
Similar questions
Q.
How many moles of acetic acid and sodium acetate each should be dissolved to prepare one litre of
0.063
molar buffer solution of pH
4.5
?
(
K
a
for
C
H
3
C
O
O
H
=
1.8
×
10
−
5
)
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
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3
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=
1.8
×
10
−
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Q.
Suppose it is required to make a buffer solution of pH = 4, using acetic acid and sodium acetate.
How many grams of sodium acetate is to be added to one litre of
N
10
acetic acid?
K
a
=
1.8
×
10
−
5
Q.
What is the pH of the solution when 0.2 mol of
H
C
l
is added to one litre of a solution containing 1M acetic acid and acetate ions. Assume that the total volume is one litre.
K
a
(
C
H
3
C
O
O
H
)
=
1.8
×
10
−
5
l
o
g
(
1.8
)
=
0.255
,
l
o
g
(
0.66
)
=
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Q.
Consider an acidic buffer solution of acetic acid and sodium acetate at
25
o
C
. What should be the ratio of concentration of sodium acetate and acetic acid so that
p
H
=
5
is obtained ?
Given :
K
a
value of acetic acid is
1.8
×
10
−
5
log
10
1.8
=
0.25
and
10
(
0.25
)
=
1.8
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