An ethanol (C2H5OH) solution contains 51.4 mL of C2H5OH and 110.8 mL of H2O at 20°C. Calculate the molality of the solution. The density of the C2H5OH is 0.789 g/mL at 20°C and the molar mass of C2H5OH is 46.07 g/mol. Assume the density of water at this temperature is 1.00 g/mL.

Consider a solution made by dissolving 339 g of sucrose in 123 ml of water at 45˚C. The vapor pressure of water at 45˚C is 0.095 atm and the density of water at 45˚C is 0.992 g/ml. What is the vapor pressure of the sucrose/water solution, in atm? (Note: The molar mass of sucrose is 180.2 g/mol.)

245. mg of an unknown protein are dissolved in enough solvent to make 5.00 mL of solution. The osmotic pressure of this solution is measured to be 0.180 atm at 25.0 °C. Calculate the molar mass of the protein. Be sure your answer has the correct number of significant digits. g x10 mol

A solution is made by dissolving 41.3 g urea (CH4N20), a nonelectrolyte, in 275 g water. Calculate the vapor pressure of this solution at 25°C and 45°C. vapor pressure of water 25°C 23.8 torr 45°C 71.9 torr vapor pressure at 25°C = torr vapor pressure at 45°C = torr

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?

Ethanol (C₂H₂OH) has a vapor pressure of 93.0 torr and a density of 0.785 g/mL. Pentane (C₂H₁₂) has a vapor pressure of 435.0 torr and a density of 0.626 g/mL. Calculate the vapor pressure (in torr) of a solution containing 495 mL of ethanol and 165 mL of pentane. Assume this solution behaves ideally.

a sodium hydroxide solution that contains 41.5 grams of NaOH per L of solution has density of 1.08 g/mL. Calculate the molality of the NaOH in this solution

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?