7.152g of an unknown solute was dissolved in 0.049883 kg of pure water. This solution has a boiling point of 103.4oC. The Van't Hoff factor of the unknown solute is 3. What is the Molality of the unknown? What is the Molecular weight of the unknown?

A sample of an unknown compound with a mass of 0.546 g was dissolved in 15.0 g of benzene. The freezing point depression was measured as 0.240 oC. a) Calculate the molality of the solute. molality =

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.

A solution is made by mixing 72.1 grams of propyl chloride, C3H7Cl, and 38.4 grams of propyl bromide, C3H7Br.  What is the vapor pressure of propyl chloride in teh solution at 25 degrees C?  Assume that the solution is an ideal solution.  The vapor pressure of pure propyl chloride is 347 torr at 25 deg C and of pure propyl bromide is 133 torr at 25 deg C.   - Thanks - need help!  I've worked this out for my quiz several times and cannot come up with the correct answer.  Heather (middle name).

Calculate the molality of a solution containing 130.6 g of glycine  (NH2CH2COOH)  dissolved in  1.502 kg of H2O.      m

Calculate the molality of a sulfuric acid solution containing 0.10 mole of sulfuric acid in 198 g of water. The molar mass of sulfuric acid is 98.09 g. Molality = Moles solute/ Kg of Solvent O 0.51 O 1.51 O 1.0 123.0

A solution is made using 16.7 percent by mass CH2Cl2 in CHCl3. At 30 °C, the vapor. pressure of pure CH2Cl2 is 490 mm Hg, and the vapor pressure of pure CHCl3 is 260 mm Hg. The normal boiling point of CHCl3 is 61.7 °C. What is the molality of CH2Cl2 in the solution?

A solution is made by dissolving 0.563 mol of nonelectrolyte solute in 821 g of benzene. Calculate the freezing point, Tf, and boiling point, Tp, of the solution. Constants can be found in the table of colligative constants. T = 1.97896467722 °C 78.3650548112 °C Incorrect

The boiling point of 6.05 g of a pure solvent is measured to be 48.000 ºC. When 20.00 g of an unknown solute (assume the van 't Hoff factor = 1.0000 for the solute and Kb =  4.85 °C/m for the solvent) is added to the solvent the boiling point is measured to be 55.500  ºC .  What is the molality ( in m) of the solution?(give your answer to two decimal places)