What is the freezing point and boiling point of an aqueous solution with 0.050 m of ? The cryoscopic constant () of water is 1.853 oC kg mol-1, while the ebullioscopic constant () of water is 0.512 oC kg mol-1. The van't Hoff factor of is 2.7.
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A solution was prepared by dissolving 0.800 g of sulfur, , in 100.0 g of acetic acid. . What is the freezing point of the solution? The freezing point of pure acetic acid is 16.6 oC. The cryoscopic constant of acetic acid is 3.90 oC kg/mol.
A 1.60-g sample of a mixture of naphthalene () and anthracene () is dissolved in 20.0 g of benzene (). The freezing point of the solution is 2.81 oC. What is the composition, as mass percent, of the sample mixture? The freezing point of pure benzene is 5.51 oC and its cryoscopic constant (Kf) is 5.12 oC kg mol-1.
1) Assuming ideal behavior, what is the ionic concentration of a 0.135 M solution of trisodium phosphate?
2) What is the boiling point of a solution (in oC) that was prepared by dissolving 13.38 g of MgCl2 in 250.0 g water. MgCl2 is an ionic solid with a measured van't Hoff factor of 2.7. KbH2O= 0.52 oC.kg/mol