A solution of `XY` (`100%` ionised) has osmotic pressure equal to four times the osmotic pressure of `0.01 M BaCl_(2)` (`100%` ionised). Find the molarity of `XY`

Compared to the osmotic pressure of 0.1 M urea, the osmotic pressure of 0.01 M KCl will be ( assume 100 % dissociation)

The osmotic pressure of a decimolar solution of BaCl_(2) in water is

The osmotic pressures of equimolar solutions of urea , BaCl_(2) and AlCl_(3) will be in the order :

100 cc of 1.5% solution of urea is found to have an osmotic pressure of 6.0 atm and 100 cc of 3.42% solution of cane sugar is found to have an osmotic pressure of 2.4 atm. If two solutions are mixed, the osmotic pressure of the resulting solution will be

The osmotic pressure of equimolar solutions of urea, BaCl_(2) and AlCl_(3) will be in the order

The osmotic pressure of a dilute solution of an compound XY in water is four times that of a solution of 0.01 M BaCl_(2) in water. Assuming complete dissociation of the given ionic compounds in water, the concentration of XY in solution is x xx 10^(–2) mol/L. The numerical value of x is____.