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Find the osmotic pressure of an aqueous solution of BaCl2 at 288 K containing 0.39 g per 60 ml. The salt is 60% dissociated. (Ba = 137; Cl = 35.5)

3.58g of NaCl was dissolved in 120g of water at 77 degree celsius. The osmotic pressure is 26.31atm. Calculate the degree of dissociation of NaCl

An aqueous solution is 1.00% NaCl by mass and has a density of 1.071 g/cm^3 at 25 degree celsius. The osmotic pressure of this solution is 7.83 atm at 25 degree celsius. What fraction of thr moles of NaCl in this solution exist as ion pairs?

2 mols of Ba(ClO4)2 were placed in 1L of water at 45 degree celsius. 15% of the salt was dissociated at equilibrium. Calculate the osmotic pressure of the solution

What is the osmotic pressure of a 0.3M solution of MgSO4 if this salt is 80% dissociated at 20 degree celsius?

Please solve both exercices

That is , if we placed the same number of mols of a non electrolyte and weak electrolyte into 1L of water , which solution will have the higher osmotic pressure ?