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Question
1 mol each of 1the following compounds is dissolved in 1L of solution. Which will have the largest ᐃTb value ?
Options
A.HF
B.HCl
C.HBr
D.Hl.
Solution
The value of ᐃTb depends upon two factors ′i′ and ′m′. It is given that 1 mol of solution. Hence molerity is same for all the compounds. Now the van′t Hoff factor depends on number of particle i.e. on degree of ionisation which further depends on the bond dissociation energy which is in the order
HI < HBr < HCl < HF
i.e. bond dissociation energy of HI is least. Lower the bond dissociation energy, higher is the degree of ionisation and hence hogher the number of particle thus i will be maximum for HI and hence ᐃTb value wil be larger for HI.
HI < HBr < HCl < HF
i.e. bond dissociation energy of HI is least. Lower the bond dissociation energy, higher is the degree of ionisation and hence hogher the number of particle thus i will be maximum for HI and hence ᐃTb value wil be larger for HI.
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