I’d like to ask a question and clear my misunderstanding.
Which of the following 0.01 M solutions have the highest osmotic pressure?
-$\ce{NaCl}$
-$\ce{C12H22O11}$
-$\ce{BaCl2}$
-$\ce{CO(NH2)2}$
-$\ce{[Cr(NH3)4Cl2]Cl}$
I know that the equation for osmotic pressure is
$$\Pi = cRTi$$
I have eliminated sucrose, sodium chloride, and urea from my answer, because sucrose and urea are non-electrolyte. And sodium chloride has smaller van ’t Hoff factor than barium chloride. I ended up in barium chloride and the complex compound. I’m not really sure with the complex compound since from what I learnt, a complex compound is easier to dissolved in water (my teacher in solubility chapter taught me that $\ce{AgI + NH3 -> [Ag(NH3)2]I}$ have a high solubility because it is a complex compound). However I’m not sure if it has a high van ’t Hoff factor as well.