A student determined the molar mass of an ionic solid by the method used in this experiment. She found the equilibrium temperature of the ice water mixture to be 0.50C on her thermometer. When she added 3.1g of her solid to the mixture, the temperature fell to 4.3C. She then poured off the solution into a beaker. The mass of the solution was 34.59 g. Kf=1.86C/m 1. What was the freezing point depression Tf ? C 2. What was the molality of the unknown solution? m 3. How much water was in the solution? g 4. What did she find to be the observed molar mass of the ionic solid, assuming she made the calculation properly? g If the true molar mass is 110.97g/mol, what would the van't hoff factor be for this ionic solid? vanthofffactor(i)=observedMolarMassTrueMolarMass