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The osmotic pressure of 0.01 molar solut...

The osmotic pressure of 0.01 molar solution of an electrolyte is found to be 0.65 atm at `27^(@)C`. Calculate the van.t Hoff factor. What conclusion can you draw about the molecular state of the solute in the solution?

Text Solution

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For electrolytes, `pi=i(n)/(V)RT`
where .i. is the vant Hoff factor
According to the given data, `pi = 0.65` atm
`R= 0.0821 " atm mol"^(-1)K^(-1)`
`T=27+273 =300K, n=0.01 "mol", V=1L`
Substituting the values, in the relation,
`pi= i(n)/(V)RT`, we get
`pi= 0.65 = (i xx 0.01)/(1) xx 0.0821L" atm mol"^(-1)K^(-1) xx 300 K`
`=0.246`i atm
`i=(0.65)/(0.246)=2.64`
Since `i gt 1`, the electrolyte undergoes dissociation.
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