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?

Explanation

`pi= 0.65 atm, C= 0.01M, R= 0.0821 L atm K^(-)mol^(-1)`
`T= 273+27= 300K`
`pi= iCRT`
`0.65 = ixx 0.01 xx 300 xx 0.0821`
`i= (0.65)/(0.01 xx 300 xx 0.0821)= 2.639`
As the van.t Hoff factor is greater than 1, this indicates that the electrolyte undergoes dissociation in the given solution.