Question: 2. What would change in your calculation for freezing point depression if you mixed an ionic compound with lauric acid (or any other solvent)? Explain.

2. What would change in your calculation for freezing point depression if you mixed an ionic compound with lauric acid (or any other solvent)? Explain. 3. A solution containing 2.00g of an unknown substance in 50.0g of cyclohexane freezes at 1.05C. The normal freezing point. of cyclohexane is 6.60C and K1=20.4C/m. Both substances are molecular. a. Calculate the molality of the solution using T=Kfmi b. The units of molality are moles /kg. Moles of what over kilograms of what? Label the equation below. Moles of Kilograms of c. How many moles of the unknown substance are in this solution? d. What is the molar mass of the unknown substance

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