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Byju's Answer
Standard XII
Chemistry
Concentration Terms
The freezing ...
Question
The freezing point depression of 0.001m Kx[Fe(CN)6] is 7.10?10^-3 K. Determine the valueof x. Kf =1.86K kg /mol for water.
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Solution
F
r
e
e
z
i
n
g
p
o
i
n
t
d
e
p
r
e
s
s
i
o
n
∆
T
f
=
i
×
K
f
×
m
i
=
∆
T
f
K
f
×
m
=
7
.
10
×
10
-
3
1
.
86
×
0
.
001
=
3
.
82
≈
4
T
h
e
t
o
t
a
l
n
u
m
b
e
r
o
f
v
a
l
u
e
o
f
i
=
4
T
h
e
g
i
v
e
n
c
o
m
p
l
e
x
K
x
[
F
e
(
C
N
)
6
]
h
a
s
a
l
r
e
a
d
y
c
o
m
p
l
e
x
i
o
n
[
F
e
(
C
N
)
6
]
a
s
1
.
S
o
t
h
e
r
e
m
a
i
n
i
n
g
a
r
e
K
i
o
n
s
=
4
-
1
=
3
T
h
u
s
t
h
e
v
a
l
u
e
o
f
x
=
3
a
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d
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h
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c
o
m
p
l
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x
i
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K
3
[
F
e
(
C
N
)
6
]
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Similar questions
Q.
The freezing point depression of
0.001
m
K
x
[
F
e
(
C
N
)
6
]
is
7.4
×
10
−
3
K
. The value of
x
is:
(Assuming complete dissociation,
K
f
=
1.85
K
k
g
m
o
l
−
1
for water)
Q.
The freezing point depression of
0.001
m
K
x
[
F
e
(
C
N
)
6
]
is
7.44
×
10
−
3
K
.
Determine the value of x.
Given:
(
K
f
)
w
a
t
e
r
=
1.86
K
k
g
m
o
l
−
1
Assume complete ionisation of
K
x
[
F
e
(
C
N
)
6
]
Q.
The freezing point depression of
10
−
3
molal aqueous solution of a compound
K
x
[
F
e
(
C
N
)
6
]
is
7.44
×
10
−
3
K. Find
x
.
Given :
K
f
of
H
2
O
=
1.86
K mol
−
1
kg
Q.
The depression in freezing point for
0.01
m
aqueous solution of
K
x
[
F
e
(
C
N
)
6
]
is
0.0744
K
. The motal depression constant for solvent is
1.86
K
k
g
m
o
l
−
1
. If the solute undergoes complete dissociation, what is the correct molecular formula for the solute?
Q.
The freezing point (in
o
C
)
of a solution containing 0.1g of
K
3
[
F
e
(
C
N
)
6
]
(Mol. Wt. 329) in 100
g
of water
(
K
f
=
1.86
K
kg mol
−
1
)
is:
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