What is the freezing point depression of a 0.050 m FeCl3 solution at 25.0°C, assuming complete dissociation and using a Kf value of 1.86°C kg/mol for water?

What is the freezing point of a 0.050 m FeCl3 solution, assuming complete dissociation and using a freezing point depression constant (Kf) of 1.86°C/m for water?

Calculate the freezing point of a solution containing 144 g of naphthalene (C10H8) dissolved in 256 g of benzene (C6H6). The freezing point depression constant (Kf) for benzene is 5.12 °C/m. Assume the molar mass of naphthalene is 128.17 g/mol.

What is the freezing point of a 0.100 m aqueous solution, given that the freezing point depression constant (Kf) for water is 1.86 °C/m?

The freezing point of ethanol is -114.6°C. The molal freezing point depression constant for ethanol is 2.00°C/m. What is the freezing point of a solution prepared by dissolving 50.0 g of glycerin (C3H8O3, a nonelectrolyte) in 200.0 g of ethanol?

The freezing point of pure benzene (C₆H₆) is 5.49 °C. The freezing point of a solution made using toluene (C₇H₈) in benzene is determined to be -13.0 °C. What is the molality of the toluene in the solution? (Kf benzene = 5.12 °C/m)

Water has a molal freezing point constant of 1.86°C kg/mol. Calculate the freezing point of a solution containing 34.335 grams of calcium chloride (CaCl2) dissolved in 163.896 grams of water, assuming complete dissociation.

What is the freezing point (in degrees Celsius) of 3.28 kg of water if it contains 170.5 g of CaBr2? The freezing point depression constant for water is 1.86 °C/m and the molar mass of CaBr2 is 199.89 g/mol.