Calculate boiling point depression and freezing point depression of .25 m K2SO4.

Students are investigating a solvent for use in freezing point depression experiments. They measured the freezing point of the solvent as −12.6 ⁰C. The solution they made by dissolving 0.484 g of ethanol (46.07 g/mol) in 8.254 g of the solvent has a freezing point of -18.3 ⁰C.  Determine the freezing point depression constant, Kf, for the solvent.

Calculate the freezing point of a solution that contains 5 grams of sucrose in 1000.00 grams of water, if the Kf of water is 1.86 K kg mol-1.

Calculate the molality of phosphoric acid (H3PO4) in a 35.3% (by mass) aqueous solution.

A compound contains 42.9%C,2.4%H,16.6%N, and 38.1%O by mass. The addition of 3.16 g of this compound to 75 mL of cyclohexane (density is 0.779 g/mL) gives a solution with a freezing point of 0°C. The normal freezing point of cyclohexane is 6.5°C and its freezing point depression constant is 20.2°C/m. What is the empirical mass? A. 84 g/mol B. 88 g/mol C. 36 g/mol D. 55 g/mol E. 98 g/mol F. 44 g/mol

A 11.7MHCIO4 (aq) solution has a density of 1.671g/ml. Use this information to calculate m the molality, mole fraction, and mass percentage of perchloric acid in this solution.

A solution is prepared by dissolving 30.4 g urea, (NH2)2CO, in 120.0 g water. Calculate the boiling point of the solution. Urea is a nonelectrolyte.

A certain substance X melts at a temperature of -4.2 °C. But if a 600. g sample of X is prepared with 25. g of urea ((NH-),Co) dissolved in it, the sample is found to have a melting point of - 5.5 °C instead. Calculate the molal freezing point depression constant K, of X. Round your answer to 2 significant digits. -1

Calculate the freezing point of a glass of water of volume 200 cm3in which 10 g of glucose has been dissolved.

The elemental analysis of an organic solid extracted from gum arabic (a gummy substance used in adhesives, inks, and pharmaceuticals) showed that it contained 40.0 percent by mass C, 6.7 percent by mass H, and 53.3 percent by mass O. A solution of 0.515 g of the solid in 31.7 g of the solvent diphenyl gave a freezing-point depression of 1.08 °C. Calculate the molar mass and molecular formula of the solid. (K °C for diphenyl is 8.00- - m Part 1 of 2 Round your answer to 3 significant digits. molar mass: .) Part 2 of 2 mol molecular formula: