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?

A solution containing 20.0 g of an unknown liquid and 110.0 g of water has a freezing point of -1.32 °C. Given Kf = 1.86 °C/m for water, the molar mass of the unknown liquid is ________ g/mol.

A solvent has a freezing point of 10.1°C and a freezing point depression constant of 6.16°C/m. If a solution, made by dissolving 1.218 g of an unknown solute into 25.0 g of the solvent, has a freezing point of 8.8°C, what is the molar mass of the solute?

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?

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?

Determine the freezing point of a solution that contains 78.8 g of naphthalene (C10H8, molar mass = 128.16 g/mol) dissolved in 722 mL of benzene (density = 0.877 g/mL). Pure benzene has a melting point of 5.50°C and a freezing point depression constant of 4.90°C/m. What is the new freezing point of the solution?

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?