A `5%` solution of anhydrous `CaCI_(2)` at `0^(@)C`developed 15 atm osmotic pressure. What is the degree of dissociation of `CaCI_(2)`.

A 5% solution of anhydrous MgCl_2 at 0^@ developed 16 atm osmotic pressure. What is the degree of dissociation of MgCl_2?

A 5% solution of CaCl_(2) at 0^(@)C developed 15 atmospheric pressure. Calculate the degree of dissociation. (mol. wt. (M) of CaCl_(2) = 111 a.m.u., R = 0.0821 L atm. K^(-1) "mol"^(-1) )

Decinormal solution of NaCl developed an osmotic pressure of 4.6 atm at 300K. Calculate the degree of dissociations.

A 0.15 M aqueous solution of KCl exerts an osmotic pressure of 6.8 atm at 310 K. Calculate the degree of dissociation of KCl. (R = 0.0821 Lit. atm K^(-1)"mol"^(-1) ).

If the observed and normal osmotic pressure of 1% NaCl solution are 5.7 and 3.0 atm, the degree of dissociation of NaCl is :

If osmotic pressure of a solution is 2 atm at 0^(@)C , then at 546K , the osmotic pressure is

At what temperature (s) a 5% solution (w//V) of glucose will develop an osmotic pressure of 7 atm ?

If the observed and normal osmotic pressures of a KCl solution are 5.85 and 3.20 atm, the degree of dissociation of KCl is :

The osmotic pressure of 5% solution of urea at 300 K is

At a certain temperature, the degree of dissociation of PCI_(5) was found to be 0.25 under a total pressure of 15 atm. The value of K_(P) for the dissociation of PCl_(5) is