Calculate the freezing point and boiling point in each solution, assuming complete dissociation of the solute. Calculate the freezing point of a solution containing 15.1 gg FeCl3FeCl3 in 180 gg water. Calculate the boiling point of the solution above.

Molality is defined as g solute/L of solvent mol solute/kg of solution mol solute/L of solution mol solute/kg of solvent

Use Henry's law to express the vapor pressure of a soluble gas in terms of the number of moles of gas dissolved in a solution. (Use the following as necessary: K to represent the Henry's law constant, n2 to represent the number of moles dissolved, and nT to represent the total number of moles.) What is the equation for P2?

23. An ethylene glycol solution contains 28.3 g of ethylene glycol, C2H602 in 97.2 mL of water. Calculate the freezing point of the solution. The density of water 1.00 g/mL.

When a 22.275 g sample of Compound B,  is dissolved in 480.2 g of benzene, the freezing point of the following solution is 3.73 ˚C. The freezing point of  benzene is 5.48 ˚C, and the Kf for benzene is 5.12 ˚C/m. Determine the molar mass of Compound B.

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 student dissolves 20. g of benzoic acid (C,H,O,) in 125. mL of a solvent with a density of 1.07 g/mL. The student notices that the volume of the solvent does not change when the benzoic acid dissolves in it. Calculate the molarity and molality of the student's solution. Be sure each of your answer entries has the correct number of significant digits. molarity Ox10 molality %D

Calculate the freezing point of a 0.383 m solution of a nonelectrolyte. The freezing point of the pure solvent is 5.45 °C and Kf is equal to 6.70 °C/m