An aqueous solution sntaining 1.248 g of barium chloride `("molar mass"= 208.34 g mol^(-1))` in 100 g of water boils at `100-0832^(@)C`. Calculate degree of dissoviation of barium of barum choride `(K_(b)"for water"=0.52 K kg mol^(-1))`

An aqueous solution containing 12.48g of barium chloride in 1.0 kg of water boils at 373.0832 K. Calculate the degree of dissociation of barium chloride. [Given K_(b) for H_(2)O =0.52 Km^(-1) , Molar mass of BaCl_(2) =208.34 "g mol"^(-1) ]

An aqueous solution containing 12.48 g of barium chloride in 1.0 kg of water boils at 373.08321K. Calculate the d.egree of dissociation of barium I chloride. (Given K_(b) , of H_(2)O = 0.52 K m^(-1) , molar mass of Ba CI_(2) = 208.34 g mol^(-1) ]

A solution containing 0.11kg of barium nitrate in 0.1kg of water boils at 100.46^(@)C . Calculate the degree of ionization of the salt. K_(b) (water) = 0.52 K kg mol^(-1) .

A solution containing 0.11kg of barium nitrate in 0.1kg of water boils at 100.46^(@)C . Calculate the degree of ionization of the salt. K_(b) (water) = 0.52 K kg mol^(-1) .

A solution containing 0.11kg of barium nitrate in 0.1kg of water boils at 100.46^(@)C . Calculate the degree of ionization of the salt. K_(b) (water) = 0.52 K kg mol^(-1) .

3.100 g of BaCl_(2) in 250g of water boils at 100.83^(@)C . Calculate the value of van't Hoff factor and molality of BaCl_(2) in this solution. ( K_(f) for water = 0.52 Km^(-1) , molar mass of BaCl_(2) = 208.3" g mol"^(-1) ).

A solution containing 1.23g of calcium nitrate in 10g of water, boils at 100.975^(@)C at 760 mm of Hg. Calculate the vant Hoff factor for the salt at this concentration. ( K_(b) for water = 0·52" K kg mol"^(-1) , mol. wt. of calcium nitrate = 164" g mol"^(-1) ).