When 2.41 g of vitamin K is dissolved in 25.0 g of camphor, the freezing point of the solution is lowered by 8.07 °C. Look up the freezing point and K, constant for camphor in the Colligative Constants table. Calculate the molar mass of vitamin K. molar mass: g/mol

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We mixed some ethylene glycol with 346 g water to reduce the equilibrium vapor pressure of water from 23.76 Hg to 22.5 Hg at 25°C. The molar masses of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol, respectively. Assume ideal behavior for the solution. What is the boiling point of this solution? (Hint: find the molality first, and for water, kb = .510 m/°C; boiling point of water: 100.0°C.)

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

When 15.0 g of an organic compound known to be 54.53% C, 9.2% H, and 36.32% O by mass is dissolved in 721.4 g of water, the freezing point is -0.293 °C. The normal freezing point of water is 0 °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. Kf values for various solvents are given in the colligative constants table. molecular formula: CHO

Q2: High pressure (2-5 atm) is applied to increase the solubility of CO2 in soda. When a can of soda is open, the pressure drops to 1 atm. If you leave the can open for a long time, the soda will taste flat. How can you explain this in terms of solubility and pressure?