The osmotic pressure of a dilute solution of an ionic compound XY in water is four times that of a solution 0.01 M in water. Assuming complete dissociation of the given ionic compounds in water, the

Question

The osmotic pressure of a dilute solution of an ionic compound XY in water is four times that of a solution 0.01 M  in water. Assuming complete dissociation of the given ionic compounds in water, the concentration of XY (in mol L⁻¹) in solution is

Canvas Classes · Accepted Answer

Strategy:
 Relate the osmotic pressures () using the effective concentrations (). Assume complete dissociation to determine the van't Hoff factor ().

Step 1: Determine effective concentration for } \ce{BaCl2} 	ext{
Formula is , so  ions ().

Step 2: Determine effective concentration for XY
We are told .

Step 3: Solve for } C{XY} 	ext{
For a 1:1 electrolyte , .

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