At 298K, the highest osmotic pressure is exhibited by a 0.1M solution of
a) urea
b) Glucose
c) KCl
d) CaCl2
Osmotic pressure is a colligative property and is effected by no of ions in the solution.
Osmotic pressure, = iCRT
where, i = vant hoff factor; C = concentration; R = gas constant and T = temperature
​Since urea and glucose do not dissociate their osmotic pressure will remain not be effected by dissociation. KCl will dissociate to give two ions (i=2) and CaCl2 will give 3 ions (i=3). Hence the osmotic pressure of CaCl2 will be the highest.
Osmotic pressure, = iCRT
where, i = vant hoff factor; C = concentration; R = gas constant and T = temperature
​Since urea and glucose do not dissociate their osmotic pressure will remain not be effected by dissociation. KCl will dissociate to give two ions (i=2) and CaCl2 will give 3 ions (i=3). Hence the osmotic pressure of CaCl2 will be the highest.