When 6.31 g of a certain nonvolatile solute is dissolved in 505 g of water, the freezing point of the resultant aqueous solution is 0.55˚C lower than that of pure water. The cryoscopic constant for water is Kf = 1.856. Given this information, what is the molar mass of the solute species, in g/mol?

When 6.31 g of a certain nonvolatile solute is dissolved in 505 g of water, the freezing point of the resultant aqueous solution is 0.55˚C lower than that of pure water. The cryoscopic constant for water is Kf = 1.856. Given this information, what is the molar mass of the solute species, in g/mol?

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter8: Solutions

Section: Chapter Questions

Problem 8.10EP: A solution is made by dissolving 0.455 g of PbBr2 in 100 g of H2O at 50C. Based on the data in Table...

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When 6.31 g of a certain nonvolatile solute is dissolved in 505 g of water, the freezing point of the resultant aqueous solution is 0.55˚C lower than that of pure water. The cryoscopic constant for water is K_f = 1.856. Given this information, what is the molar mass of the solute species, in g/mol?

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