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

`p=0.65` atm, `C=0.01` M, `R=0.0821" L atm K"^(-1)" mol"^(-1),T=273+27=300" K"`
`pi=" I CRT"`
`0.65=ixx0.01xx300xx0.0821`
`i=(0.65)/(0.01xx300xx0.0821)=2.639`
As the van.t Hoff factor is greater than 1, this indicates that the electrolyte undergoes dissociation in the given solution.