1) What is the molality of the solution with a boiling point elevation of 2.56 degrees Celsius? The Kb value is 3.8 and the Kf value is 2.37. 2) What is the molality of the solution with 3.55 g of solute dissolved in 75.0 mL of water? The molar mass of the solute is 75.4 g/mol while that of water is 18 g/mol. Water has density of 1.0 g/mL

A pure solvent has a freezing point of −3.62°C. A solute is added to the solvent and the solution freezes at −7.81°C. If the solute is RbF what is the molality of the solution. kf,solvent = 3.68°C•kg/mol

What mass of H2O is needed to dissolve 4.69 g KMnO4 to produce a solution having a molality of 0.299 m? Assume that the density of the solution is 1.00 g/mL. The molar mass of KMnO4 is 158.03 g/mol and the molar mass of H2O is 18.02 g/mol.

A solution has a density of 0.889 g/mL and has 5.9 g of toluene (C7H8) and 231 g of benzene. Identify the solute and the solvent. Calculate the molarity of the solution. Calculate the molality of the solution.

When potassium phosphate is added to water the boiling point increases 50°C. What is the molality of the solution of the solution if the Kbp for water is 0.512°C/m?

A solution made by dissolving 150.0 g of an unknown compound in 425.0 mL of benzene to make a solution which has a freezing point 18.6 °C lower than that of pure benzene. Kf for benzene is 5.12 °C/m and the density of benzene is 0.877 g/mL.     What was the molality of the solution?   How many moles of the unknown compound were dissolved in the solution?   What is the molar mass of the unknown compound?