An aqueous solution containing an ionic salt having molality equal to `0.19` freezes at `-0.704^(@)C`. The Van't Hoff factor of the ionic salt is (`K_(f)` for water=`1.86 K m^(-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).

Calculate the freezing point depression expected for 0.0711 m aqueous solution of Na_(2)SO_(4) . If this solution actually freezes at -0.320 ^(@)C , what would be the value of Van't Hoff factor ? ( K_(f) for water is 1.86 ^(@)C mol^(-1) ) .

Calculate the freezing point depression expected for 0.0711 m aqueous solution of Na_(2)SO_(4) . If this solution actually freezes at -0.320 ^(@)C , what would be the value of Van't Hoff factor ? ( K_(f) for water is 1.86 ^(@)C 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) )

1.2 mL acetic acid having density 1.06 g cm^(-3) is dissolved in 1 litre of water. The depression in freezing point observed for this concentration of acid was 0.041 ""^(@)C . The van't Hoff factor of the acid is ( K_(f) of water = 1.86 K kg mol^(-1) )