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Question

When 9.45 g of ClCH2COOH is added to 500 mL of water , its freezing point drops by 0.50C . The dissociation constant of ClCH2COOH is x ×103 . The value of x is ( Rounded off to the nearest integer )[Kf(H2O)=1.86 Kg mol1]

A
35.0
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B
35
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C
35.00
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Solution

Moles of ClCH2COOH=9.4594.5=0.1 moles

ClCH2COOHClCH2COO+H+

At eqb. C(1α) Cα Cα

vant't Hoff factor (i)=1+α

C=molesvolume in L=0.10.5=0.2 M

Assuming molarity = molality

ΔTf=i×Kf×m=(1+α)×1.86×0.2
0.5=(1+α)×1.86×0.2


(1+α)=0.50.2×1.861+α=1.34

α=0.34

Ka of(ClCH2COOH)=CαCαC(1α)

Ka=Cα21α=0.2×(0.34)210.34

Ka=35×103x=35


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