Question
A solution is prepared by dissolving 0.490 g of an unknown compound in 50.00 mL of water. The freezing point of the solution is –0.201°C. Assuming the compound is a non-electrolyte, what is the molecular mass of the compound? Use 1.00 g/mL as the density of water.
Answers
delta T = 0-(-.201) = ?
delta T = Kf*m
You know delta T and Kf, solve for m = molality.
m = mols/kg solvent. You know kg solvent and m, solve for mols.
mols = grams/molar mass. You know grams and mols, solve for molar mass.
delta T = Kf*m
You know delta T and Kf, solve for m = molality.
m = mols/kg solvent. You know kg solvent and m, solve for mols.
mols = grams/molar mass. You know grams and mols, solve for molar mass.
90.74
Related Questions
A solution is prepared with an unknown compound with an empirical formula of C3H7NO.
The solution...
an aqueous solution was prepared by dissolving 1438.0g of a nonelectrolyte in 469.0g of water at 25*...
solution A was prepared by dissolving 0.63g of HNO3 in 100cm3 solution. Solution B is a sodium calci...
Determine the molecular mass of a solution if prepared by dissolving 6.00 g of an unknown nonelectro...