An 1% solution of `KCI(I),NaCI(II), BaCI_(2)(III)` and urea (IV), have their osmotic pressure at the same temperature in the ascending order (molar masses of `NaCI, KCI, BaCI_(2)` and urea are respectively `58.5, 74.5, 208.4, 60 g mol^(-1)` Assume 100% ionization of the electrolytes at this temperature

A 1% (wt/ wt) solution of KCl (I) , NaCl(II) , BaCl_(2) (III) and urea (IV) have their osmotic pressures at the same temperature in the ascending order (molar masses of NaCl , KCl , BaCl_(2) and urea are 58.5 , 74.5 , 208.4 and 60 g mol^(-1) ) assuming 100 % ionisation of the electrolytes at this temperature :

Statement-I: 0.1M solution of NaCI has greater osmotic pressure than 0.1M solution of glucose at same temperature. Because Statement-II: In solution, NaCI dissociates to produce more number of particles.

Statement-I: 0.1M solution of NaCI has greater osmotic pressure than 0.1M solution of glucose at same temperature. Because Statement-II: In solution, NaCI dissociates to produce more number of particles.

At a constant temperature, which of the following aqueous solutions will have the maximum vapour pressure? (Mol wt NaCl = 58.5, H_(2)SO_(4) = 98.0 g mol^(-1) )

At a constant temperature, which of the following aqueous solutions will have the maximum vapour pressure? (Mol wt NaCl = 58.5, H_(2)SO_(4) = 98.0 g mol^(-1) )

If 0.1 M solution of NaCl is isotonic with 1.1 w % urea solution, the degree of ionisation of NaCl is (molar masses of urea and NaCl are 60 and 58.5 g mol ^(-1) respectively )

For a 5% solution of urea (Molar mass - 60 g/mol), calculate the osmotic pressure at 300 K. [R = 0.0821 L atm K^(-1) mol^(-1)]