The osmotic pressure of a ldilute solution of an ionic 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 mol `L^(-1)`) in solution is :
The osmotic pressure of a dilute solution of a 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 "mol" L^(-1) ) in solution is:
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____.
The osmotic pressure of a decimolar solution of BaCl_(2) in water is
The osmotic pressure of 0.1 M sodium chloride solution at 27^@C is
The osmotic pressure of 1 M solution of sucrose is 22.4 atm. What will be the osmotic potential of 0.1 M sucrose solution?
A base dissolved in water yields a solution with a hydroxide ion concentration of 0.05 mol litre^(-1) . The solution is
0.1 M solution of a solute has a water potential of
