What is the freezing point of a solution consisting of 88.5 g of sucrose (C12H22O11) in 282 g of water? Assume the freezing point depression constant (Kf) for water is 1.86 °C/m.

What is the freezing point of a solution prepared from 50.0 g of ethylene glycol (C2H6O2) and 85.0 g of water, given that the freezing point depression constant (Kf) of water is 1.86°C/m?

What is the freezing point of a solution that contains 50.0 g of FeBr₃ in 200.0 g of water, given that the freezing point depression constant (Kf) for water is 1.86 °C/m?

What is the freezing point of a solution that contains 50.0 g of NaNO₃ in 200.0 g of water, given that the molal freezing point depression constant (Kf) for water is 1.86 °C/m?

What is the freezing point, in °C, of a solution made with 1.15 mol of CHCl₃ in 530.0 g of CCl₄ (Kf = 29.8 °C/m, normal freezing point, Tf = -22.9 °C)?

What mass in grams of CH₃OH (MM = 32.04 g/mol) would need to be added to 270.1 g of water in order to lower the freezing point of water by 12.0 °C? (Kf for water is 1.86 °C/m)

What mass, in grams, of NaCl needs to be added to 2.5 kg of water in order to create a solution with a freezing point of -5.4 °C? The freezing point depression constant of water is 1.86 °C/m.

A solution was prepared by dissolving 2.500 g of a non-dissociating solute in 125 g of pure water. The resulting solution has a freezing point of -0.190°C. The Kf of water is 1.86°C/m. What is the molar mass of the unknown solute?

Calculate the freezing point of an aqueous solution with 95.21 g of barium chloride (BaCl2) dissolved in 1750 mL of water. Assume complete dissociation and use the freezing point depression constant (Kf) for water as 1.86 °C/m.