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

Given: `pi = 0*65 atm, c = 0.01 M`
`R = 0*0821 1 atm K^(-1) Mol^(-1)`,
`T = 273+27 = 300 K`
Now, `pi = i xx CRT`
`0*65 = ixx 0*01 xx 300 xx 0*0821`
`i = (0*65)/(0*01 xx 300 xx 0*0821)`
`= 2.639`.
van.t Hoff factor `i = 2*639`. It indicates that the electrolyte undergoes dissociation in given solution.