# The osmotic pressure of a dilute solution of an ionic compound XY in water is four times that of a solution of 0.01 M BaCl2 in water. Assuming complete dissociation of the given ionic compounds in water, the concentration of XY (in mol L-1) in solution is (a) 16 × 10−4 (b) 4 × 10−4 (c) 6 × 10−2 (d) 4 × 10−2

## Question ID - 52580 :- The osmotic pressure of a dilute solution of an ionic compound XY in water is four times that of a solution of 0.01 M BaCl2 in water. Assuming complete dissociation of the given ionic compounds in water, the concentration of XY (in mol L-1) in solution is (a) 16 × 10−4 (b) 4 × 10−4 (c) 6 × 10−2 (d) 4 × 10−2

3537  2[XY] = 4 ×(0.01)× 3

[XY] = 0.06

= 6 10−2 Next Question :
 Consider the van der Waals constants, a and b, for the following gases.  Gas                               Ar        Ne     Kr      Xe  a/(atm dm6 mol−2)        1.3       0.2     5.1   4.1  b/(10−2 dm3 mol−1)      3.2       1.7     1.0   5.0  Which gas is expected to have the highest critical temperature? (a) Ne (b) Kr (c) Xe (d) Ar 