1. KCl  K+ = Cl- by moles therefore K+ = KCl so ………………….
13.75) i = osmotic pressure measured/osmotic pressure calculated.
Osmotic pressure = MRT = mol x L ATM x 298 K =0.24 ATM
L mol K
i = ATM/ 0.24 ATM = 2.8
The closer i measured is to the i calculated the more ideal the solution is. Ion paring and other attractive forces reduce the number of particles in solution.
13.88) ppm (parts per million) = mass solute/ mass solution) x 106
KCl  K+ = Cl- by moles therefore K+ = KCl so ………………….
260 ppm KCl = g KCl x g K+ = g K = 136 ppm
1 x 106g soln g KCl x 106 g soln

2. i = ∆Tf (measured) / ∆Tf (calculated)
13.95
i = ∆Tf (measured) / ∆Tf (calculated)
Hg(NO3)2 m = g Hg(NO3)2 x 1 mol Hg(NO3)2 = m
1,00Kg H g Hg(NO3)2 .
∆Tf = -1.86(0.0308) = oC (note♪ - assume non electrolyte)
i = oC = 2.83 oC