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?
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter13: The Chemistry Of Solutes And Solutions
Section: Chapter Questions
Problem 106QRT: Calculate the molality of a solution made by dissolving 115.0 g ethylene glycol, HOCH2CH2OH, in 500....
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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 Kf = 1.856. Given this information, what is the molar mass of the solute species, in g/mol?
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