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[" (1) "27g],[" A solution containing "0...

[" (1) "27g],[" A solution containing "0.85g" of "ZnCl_(2)" in "125.0g" of water freezes at "-0.23^(@)C" .The apparent degree of "],[" dissociation of the salt is : "],[(k_(f)" for water "=1.86Kkgmol^(-1)," atomic mass ";Zn=65.3" and "Cl=35.5" ) "]

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A solution containing 0.85 g of ZnCl_(2) in 125.0g of water freezes at -0.23^(@)C . The apparent degree of dissociation of the salt is: (k_(f) for water = 1.86 K kg mol^(-1) , atomic mass, Zn = 65.3 and Cl = 35.5)

A solution containing 0.85 g of ZnCI_(2) in 125.0g of water freezes at -0.23^(@)C . The apparent degree of dissociation of the salt is: (k_(f) for water = 1.86 K kg mol^(-1) , atomic mass, Zn = 65.3 and CI = 35.5)

A solution containing 0.85 g of ZnCI_(2) in 125.0g of water freezes at -0.23^(@)C . The apparent degree of dissociation of the salt is: (k_(f) for water = 1.86 K kg mol^(-1) , atomic mass, Zn = 65.3 and CI = 35.5)

A solution containing 0.5 g of KCI dissolved in 100 g of water and freezes at -0.24^(@)C . Calculate the degree of dissociation of the salt. ( K_(f) for water = 1.86^(@)C . [Atomic weight K = 39, Cl = 35.5]

A solution containing 1g of sodium chloride in 100g of water freezes at - 0.604^@C . Calculate the degree of dissociation of sodium chloride. (Na = 23, Cl = 35.5, Kf for water = 1.87 k "mol"^(-1) )

0.01 m aqueous solution of K_(3)[Fe(CN)_(6)] freezes at -0.062^(@)C . What is the apparent percentage of dissociation ? ( K_(f) for water = 1.86" K kg mol"^(-1) )

A solution containing 6.35g of a non electrolyte dissolved in 500 g of wate freezes at -0.465^(@)"C". Determine the molecular weight of the solute. ["K"_("f")"for water 1.86"^@)"C"//"m"]