Question

The experimentally measured freezing point of a 1.25 m aqueous solution of FeCl3 is -7.91°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. What is the value of the Van't Hoff factor in this equation? What is the predicted freezing point if there were no ion clustering in this solution? 

          The experimentally measured freezing point of a 1.25 m aqueous solution of FeCl3 is -7.91°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. What is the value of the Van't Hoff factor in this equation? What is the predicted freezing point if there were no ion clustering in this solution?
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Chemistry: Structure and Properties
Chemistry: Structure and Properties
Nivaldo Tro 2nd Edition
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The experimentally measured freezing point of a 1.25 m aqueous solution of FeCl3 is -7.91°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. What is the value of the Van't Hoff factor in this equation? What is the predicted freezing point if there were no ion clustering in this solution?
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Transcript

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00:01 To calculate the vaugh factor, we'll be using the freezing point depression equation.
00:06 With the decrease in freezing point will be equal to the vaugh factor multiplied by the molality of the solute, multiplied by kf for water.
00:16 Rearranging this, we get i, the vaugh factor, equal to the decrease in the freezing point, divided by the molality and kf.
00:27 The decrease in freezing point is 7 .91 degrees celsius.
00:30 The molality of iron three chloride is 1 .25.
00:35 And the kf value for water is 1 .86 degrees celsius per molal...
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