10 Question (15 points) See page 576 The experimentally measured freezing point of a 1.35 m aqueous solution of AlCl3 is -8.04°C. The freezing point depression constant for water is Kf = 1.86°C/m. Assume the freezing point of pure water is 0.00°C. 1st attempt Part 1 (7.5 points) See Periodic Table See Hint What is the value of the van't Hoff factor for this solution? 3.2 Part 2 (7.5 points) What is the predicted freezing point if there were no ion clustering in the solution? -2.51 °C
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049°C, the molarity (\( m \)) is 1.35, and the Kf value is 1.86, we can rearrange the equation to solve for the van't Hoff factor (\( i \)): \[ i = \frac{\Delta T}{m \cdot K_f} = \frac{-8.049}{1.35 \cdot 1.86} \] Show more…
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