A glucose solution contains 55.8 g of glucose (C6H12O6) in 455 g of water. Determine the freezing point of the solution. The freezing point depression constant (Kf) for water is 1.86°C/m. What is the freezing point of the solution?

Calculate the molar mass of an unknown molecular (nonelectrolyte) compound in an aqueous solution containing 35.9 g of the compound in 150.0 g of water with a freezing point of -1.3 °C.

Is the question formulated correctly for calculating the freezing point and boiling point of each solution, assuming complete dissociation of the solute? For the following: a. 10.5 g FeCl3 in 1.50 * 10^2 g water b. 3.5% KCl by mass (in water) c. 0.150 m MgF2.

A 0.95 m aqueous solution of an ionic compound with the formula MX has a freezing point of -3.0 °C. Calculate the van’t Hoff factor (i) for MX at this concentration.

What is the freezing point of an aqueous solution that boils at 106.5 °C?

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?

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?