14. Solutions

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?

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?

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.

What is the freezing point in °C of a solution prepared by dissolving 6.80 g of MgCl2 in 110 g of water? The value of Kf for water is 1.86 (°C·kg)/mol, and the van't Hoff factor for MgCl2 is i = 2.7.

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 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.