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 :

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 the observed and theoretical molecular mass of KCl is found to be 38.75 and 74.5, then the degree of dissociation of KCl is

The osmotic pressure of a solution at 273 K is 2.5 atm. The osmotic pressure of the same solution at 273^(@)C is :

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) ).

A decinormal solution of solution chloride exerts an osmotic pressure of 4.82 atmospheres at 27^(@)C . Calculate the degree of dissociation of sodium chloride.

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

A solution of 7.45 g KCl in 1000 mL shows osmotic pressure of 4.68 atm at 300K. Calculate the percentage dissociation of KCl :