Question

Determine the osmotic pressure of a 0.0125 M solution of CrCl3 at 25°C. Assume 100% dissociation of CrCl3. 0.280 atm 0.560 atm 0.840atm 1.22atm 1.40atm

Answer 1

Option 4.) 1.22 atm is correct

of Concentration Temperature Coll, Colla solution = 0.0125M of Colla delution = 25°C = 298 K Cor3+ + 3 e- We know r=iCRT r = Osmotic pressure, c = Concentration of Collz, i = Van't R = has constant T = Temperature i= lt (n-1) n = number of ions formed after dissociation x = 1 (because 100% dissociation) + (4-1) 1 = i = 4 r = 4X 0.0125X0.08218298 atm r = 1.22 atm r = 1.22 atm