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Class 12
>>Chemistry
>>Solutions
>>Abnormal Molar Masses
>>Calculate the depression in the freezing
Question
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Calculate the depression in the freezing point of water when 10 g of CH
3
CH
2
CHClCOOH is added to 250 g of water.
[Ka=1.4×10
−3
,K
f
=1.86 K kg mol
−1
]
Hard
Updated on : 2022-09-05
Solution
verified
Verified by Toppr
The molar mass of 2-chloro butanoic acid is 122.5 g/mol.
Number of moles =
122.5
10
=0.0816 mol
Molality of solution =
250
0.0816×1000
=0.3265 m
Let α be the degree of dissociation and c be the initial concentration. The concentration after dissociation is as shown.
c(1−α)
CHClCOOH
⇌
cα
CHClCOO
−
+
H
The equilibrium constant expression is
K=
cα×cα
=cα
α=
c
K
=
0.3265
1.4×10
=0.065
Calculation of vant Hoff factor:
(1−α)
α
i=
1
1−α+α+α
=1+α=1+0.065=1.065
The depression in the freezing point ΔT
=iK
m=1.065×1.86×0.3265=0.647
o
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Answer:
search-icon-header
Search for questions & chapters
search-icon-image
Class 12
>>Chemistry
>>Solutions
>>Abnormal Molar Masses
>>Calculate the depression in the freezing
Question
Bookmark
Calculate the depression in the freezing point of water when 10 g of CH
3
CH
2
CHClCOOH is added to 250 g of water.
[Ka=1.4×10
−3
,K
f
=1.86 K kg mol
−1
]
Hard
Updated on : 2022-09-05
Solution
verified
Verified by Toppr
The molar mass of 2-chloro butanoic acid is 122.5 g/mol.
Number of moles =
122.5
10
=0.0816 mol
Molality of solution =
250
0.0816×1000
=0.3265 m
Let α be the degree of dissociation and c be the initial concentration. The concentration after dissociation is as shown.
c(1−α)
CH
3
CH
2
CHClCOOH
⇌
cα
CH
3
CH
2
CHClCOO
−
+
cα
H
+
The equilibrium constant expression is
K=
c(1−α)
cα×cα
=cα
2
α=
c
K
=
0.3265
1.4×10
−3
=0.065
Calculation of vant Hoff factor:
(1−α)
CH
3
CH
2
CHClCOOH
⇌
α
CH
3
CH
2
CHClCOO
−
+
α
H
+
i=
1
1−α+α+α
=1+α=1+0.065=1.065
The depression in the freezing point ΔT
f
=iK
f
m=1.065×1.86×0.3265=0.647
o
Hii.......
Hope these 3 attachments will help u...
MARK IT AS BRAINLIEST....❤️