Vitamin K is involved in normal blood clotting. When 1.76 g of vitamin K is dissolved in 25.0 g of camphor, the freezing point of the solution is lowered by 5.89 °C. Look up the freezing point and Kf constant for camphor in the Colligative Constants table. Calculate the molar mass of vitamin K. molar mass: g/mol

When 2.60 g of a nonelectrolyte solute is dissolved in water to make 275 mL of solution at 29 °C, the solution exerts an osmotic pressure of 915 torr. What is the molar concentration of the solution? concentration: How many moles of solute are in the solution? mol moles of solute: What is the molar mass of the solute? molar mass: g/mol

A solution is made by dissolving 0.533 mol of nonelectrolyte solute in 797 g of benzene. Calculate the freezing point, Tj, and boiling point, Tb, of the solution. Constants can be found in the table of colligative constants. °C Ть %3 °C

Use Raoult's Law to determine the vapor pressure of a solution at 55°C that contains 34.2 grams of sodium chloride in 375 grams of water. The par pressure of pure water at 55°C is 118.1 torr. Assume 100% dissociation of the solute. 871 to 115 torr

Vitamin K is involved in normal blood clotting. When 0.641 g of vitamin K is dissolved in 25.0 g of camphor, the freezing point of the solution is lowered by 2.15 °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

Calculate the freezing point of a solution of 1.82 g of NaCl in 152.2 g of water.  Kf for water is 1.86°C/m and the freezing point of pure water is 0.0 °C.  Assume that NaCl completely dissociates into its ions and its molar mass is 58.44 g/mol.

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

Suppose a group of students tell you that they added solid sodium chloride NaCls to 35 mL of deionized water and they did not record how many grams of NaCl they added but they got a freezing point depression of 1.25°C. Calculate how many grams of NaCl the students added. The pure freezing point of water is 0.00°C and the freezing point depression constant (K) of water is 1.858 °C/m. Remember that NaCl is a solid salt and an ionic compound therefore it contributes a negligible amount to the overall additive volume and keep track of its van't Hoff factor. The density of water at 20°C is 0.9982 g/mL.