`A 0.01` molal solution of ammonia freezes at `-0.02^(@)C`. Calculate the van't Hoff factor, `i` and the percentage dissociation of ammonia in water. `(K_(f(H_(2O))))=1.86` deg `"molal"^(-1)`.

0.15 molal solution of NaCI has freezing point -0.52 ^(@)C Calculate van't Hoff factor . (K_(f) = 1.86 K kg mol^(-1) )

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% 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% 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) )

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).

0.01 molal aqueous solution of K_(3)[Fe(CN)_(6)] freezes at -0.062^(@)C . Calculate percentage dissociation (k_(f)=1.86)

0.01 molal aqueous solution of K_(3)[Fe(CN)_(6)] freezes at -0.062^(@)C . Calculate percentage dissociation (k_(f)=1.86)