When 6.29 g of a certain nonvolatile solute is dissolved in 500 g of water, the freezing point of the resultant aqueous solution is 0.646oC lower than that of pure water. The cryoscopic constant for water is Kf = 1.856 K-kg/mol. Given this information, what is the molar mass of the solute species?
When 6.29 g of a certain nonvolatile solute is dissolved in 500 g of water, the freezing point of the resultant aqueous solution is 0.646oC lower than that of pure water. The cryoscopic constant for water is Kf = 1.856 K-kg/mol. Given this information, what is the molar mass of the solute species?
Chapter11: Properties Of Solutions
Section: Chapter Questions
Problem 5RQ: Define the terms in Raoults law. Figure 10-9 illustrates the net transfer of water molecules from...
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When 6.29 g of a certain nonvolatile solute is dissolved in 500 g of water, the freezing point of the resultant aqueous solution is 0.646oC lower than that of pure water. The cryoscopic constant for water is Kf = 1.856 K-kg/mol. Given this information, what is the molar mass of the solute species?
a. 36.1 g/mol
b. 72.2 g/mol
c. 36.1 kg/mol
d. 18.1 g/mol
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