An aqueous solution containing `0.25` moles of a non-volatile but strong electrolyte solute '`"X"`' ' in `500g` water freezes at `-2.79^(@)C` .The number of ions furnished in water per formula unit of '`"X"`' is ` (K_(f)=1.86)`

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"]

A solution containing 6.8 g of non-ionic solute in 100g of water was found to freeze at -0.93^(@)C . If K_(f) for water is 1.86, the mol. Mass of solute is

A solution containing 18 g of a non - electrolytic solute in 200g of H_(2)O freezes at 272.07 K . Find the molecular mass of the solute . ( K_(f) = 1.86 Km^(-1) ).

6g of non-volatile, non-electrolyte x dissolved in 100g of water freezes -0.93^(@)C . The molar mass of x in "g mol"^(-1) is : (K_(f) "of" H_(2)O=1.86 "K kg mol"^(-1))

For a silute solution conatining 2.5 g of a non-volatile non-electrolyte solute in 100g of water, the elevation in boiling point at 1 atm pressure is 2^(@)C . Assuming concentration of solute is much lower than the concentration (take K_(b) = 0.76 K kg mol^(-1))

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) )