CBSE Class 12-science Answered
19.5g of fluoroacetic acid is dissolved in 500g of water the observed depression in freezing point is i degree celsius . calculate the vant hoff factor and dissociation constant of the acid given kf=1.86kkg/mol
Asked by Akshaya Parthasarathy | 10 Jul, 2011, 12:00: AM
Expert Answer
Number of moles of fluoroacetic acid (CH2FCOOH) = 19.5/78 =0.25
Therefore, molality = (0.25 x1000)/500
= 0.50 mole/kg
?Tf = Kf x m
= 1.86 x 0.50 = 0.93 K
Van't Hoff factor (i) = 1.0/0.93 =1.0753
Since fluoroacetic acid undergo dissociation as
CH2FCOOH ---> CH2FCOO- + H+
So, ? = (i -1) / (n-1) where ? is the degree of dissociation
Here n = 2
?= 1.0753 - 1 =0.0753
Now
Ka = [ CH2FCOO- ] [ H+] / CH2FCOOH
where,
[ CH2FCOO- ] = 0.50 x 0.0753 =0.03765
[ H+] = 0.50 x 0.0753 =0.03765
[CH2FCOOH] = 0.50 (1 - 0.0753) = 0.462
Thus, Ka = 0.03765 x 0.03765/0.462
= 3.07 x 10-3
Answered by | 11 Jul, 2011, 09:52: AM
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