having a little trouble with question not sure where to startor how to start a s

Question

having a little trouble with question not sure where to startor how to start a solution is prepared by mixing 3.72g of an unknownnon-electroylte with 325.0g of chloroform. the freezing point ofthe mixture is -64.10 degree celius, while the freezing point ofpure chloroform is -63.50 degrees celius. using a value of 4.68degrees celius/m as the kf of chloroform, calculate the molar massof the unknown. having a little trouble with question not sure where to startor how to start a solution is prepared by mixing 3.72g of an unknownnon-electroylte with 325.0g of chloroform. the freezing point ofthe mixture is -64.10 degree celius, while the freezing point ofpure chloroform is -63.50 degrees celius. using a value of 4.68degrees celius/m as the kf of chloroform, calculate the molar massof the unknown.

Explanation / Answer

molality = moles/ kg solvent = (grams solute / molar mass)/kgsolvent T = Kf*molality = -63.50 C - (-64.10 C) = 0.6 C molaity = 0.6 C / Kf = (0.6 / 4.68 C/m)) = 0.128205128 m =0.128205128 mol solute / kg chloroform 325.0 g chloroform * (1 kg/ 1000g) * 0.128205128 mol solute / kgchloroform = 0.0416666666 mol solute MW = 3.72 g / 0.0416666666 mol = 89.2800001 g/mol = 89.3g/mol

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