Use the References to access important values if needed for

Use the References to access important values if needed for this question. The normal freezing point of water (H2O) is 0.000 °C and its Kp, value is 1.86 °C/m. In a laboratory experiment, students synthesized a new compound and found that when 10.30 grams of the compound were dissolved in 248.0 grams of water, the solution began to freeze at -1.345 \'C. The compound was also found to be nonvolatile and a nonelectrolyte. What is the molecular weight they determined for this compound? g/mol Submit Answer

Solution

The depressin in freezing point = 1.348 C

mass of solute = 10.80g

mass of water solvent = 248.0g

Kf of water = 1.86 K Kg/mol

Thus molality of solution = [10.80/molar mass]mol/0.248Kg

We know from colligativ eproperties

depression in freezing point = Kf x molality

1.348K = 1.86K.Kg/mol x [10.80/molar mass] mol /0.248Kg

Thus

molar mass of solute = 60.089 g/mol