Answered: When 148.g of urea CH4N2O are dissolved…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter10: Solutions

Section: Chapter Questions

Problem 48QAP: The Rast method uses camphor (C10H16O) as a solvent for determining the molar mass of a compound....

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When 148.g of urea CH4N2O are dissolved in 1100.g of a certain mystery liquid X, the freezing point of the solution is 2.00°C less than the freezing point of pure X.Calculate the mass of iron(III) nitrateFeNO33 that must be dissolved in the same mass of X to produce the same depression in freezing point. The van't Hoff factor =i3.20 for iron(III) nitrate in X.Be sure your answer has a unit symbol, if necessary, and round your answer to 3 significant digits. The please do not round untill the end please

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Step 1

When a non-volatile solute is added to a pure solvent, the freezing point of the resulting solution is less than that of the pure solvent.

This depression in freezing point is given as:

$∆ T_{f} = i K_{f} m - - - - - (1) ∆ T_{f} = D e p r e s s i o n i n f r e e z i n g p o i n t i = V a n' t H o f f f a c t o r m = m o l a l i t y o f t h e s o l u t i o n K_{f} = F r e e z i n g p o i n t d e p r e s s i o n c o n s \tan t o f t h e s o l v e n t$

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