Assuming ideal solution behavior, what is the freezing temperature of a solution of 115.0 g of sucrose (FW = 342.3 g/mol), in 350.0 g of water? Kf for water is 1.86 C/molal.

Urea (molar mass: 60.056 g/mol) is a non-volatile solute with a solubility of 17.0 g per 100 mL of methanol at 20 ºC. The vapor pressure of pure methanol (molar mass: 32.042 g/mol; density: 0.792 g/mL) at 20 ºC is 95.7 torr. What is the vapor pressure of a saturated solution of urea in methanol at 20 ºC? Select one: a.5.00 torr b.9.83 torr c.85.9 torr d.55.6 torr

1.613 g sample of an unknown nonionizing molecular compound is added to 250.0 g of benzene(C6H6, MW = 78.11 g/mol). The normal freezing point of the solution is 0.17 C lower than the normalfreezing point of pure benzene. Based on this information, find the molecular weight of the unknowncompound. benzene =  Kf = 5.12 kg x Degrees C/mol.

Determine the freezing point depression of a solution that contains 30.7 g glycerin (C 3H 8O 3, molar mass = 92.09 g/mol) in 376 mL of water. Some possibly useful constants for water are K f = 1.86°C/ m and K b = 0.512°C/ m.        2.18°C        0.654°C        3.33°C        1.65°C        0.887°C

A solution of 0.890 g of an organic compound in 100.0 g of benzene has a freezing point of 5.107°C. What are the molality of the solution and the molar mass of the solute? The normal freezing point of benzene is 5.500°C and the Kf for benzene is 5.12°C/m. molality molar mass = g/mol

When 14.4 g14.4 g of an organic compound known to be 55.81% C55.81% C, 7.0% H7.0% H, and 37.17% O37.17% O by mass is dissolved in 825.8 g825.8 g of benzene, the freezing point is 4.80 ∘C4.80⁢ ∘C. The normal freezing point of benzene is 5.49 ∘C5.49⁢ ∘C. What is the molecular formula for the organic compound? Assume that the organic compound is a molecular solid and does not ionize in water. ?fKf values for various solvents are given in the colligative constants table. molecular formula: CHO

When 86 g of a nonelectrolyte compound are dissolved in exactly 76 g of water, the solution has a freezing point of -22 °C. What is the molar mass of this molecule? Kf of water is 1.86°C/m.

What would be the theoretical freezing point of a solution made by dissolving 5.052 g of CuCl 2 in 150.0 g of water? The freezing point constant of water is 1.86 °C/molal. The molar mass of CuCl 2 is 134.345 g/mol.     1.399 °C     -1.061 °C     -0.8277 °C     0.7148 °C     -1.399 °C