A `0.5%` aqueous solution of `KCl` was found to freeze at `-0.24^(@)C`. Calculate the Van,t Hoff factor and degree of dissociation of the solute at this concentration. (`K_(f)` for water =`1.86 K kg mol`^(-1)`)

A 0.5 percent aqueous solution of KCl was found to freeze at 272.76K. Calculate the Van.t Hoff factor and degree of dissociation of the solute at this concentration (K_(f)" for water = 1.86 k.kg.mol"^(-1)) . Normal molar mass of KCl = 74.5.

A 0.5 percent aqueous solution of KCl was found to freeze at 272.76K. Calculate the Van.t Hoff factor and degree of dissociation of the solute at this concentration (K_(f)" for water = 1.86 k.kg.mol"^(-1)) . Normal molar mass of KCl = 74.5.

A 0.5 percent aqueous solution of KCl was found to freeze at 272.76K. Calculate the Van't Hoff factor and degree of dissociation of the solute at this concentration (K_(f)" for water = 1.86 k.kg.mol"^(-1)) . Normal molar mass of KCl = 74.5.

0.2m aqueous solution of KCl freezes at -0.68^(@)C calculate van't Hoff factor. K _(f) for water is 1.86 K kg mol ^(-1).

0.2m aqueous solution of KCI freezes at -0.680^@C . Calcuate van't Hoff factor and osmotic pressure of solution at 0^@C . (K_f=1.86 K kg mol^(-1) .