We’re being asked to find the molality of a solution when nicotine is dissolved in water. When calculating the freezing point of a solution, we’re going to use the equation for Freezing Point Depression.
∆Tf = change in freezing point = Tf pure solvent –Tf solution
Kf = freezing point depression constant
i = van' t Hoff factor of the solute = no. of ions
m = molality
Determine the required values for the Freezing Point Depression equation:
Nicotine, extracted from tobacco leaves, is a liquid completely miscible with water at temperatures below 60°C. What is the molality of nicotine (a covalent substance) in an aqueous solution that starts to freeze at -0.450°C? (Note that the Kf for water is 1.86 °C m -1)
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Based on our data, we think this problem is relevant for Professor Delgado's class at FIU.