A solution is made by dissolving 0.741 mol of nonelectrolyte solute in 857 g of benzene. Calculate the freezing point, T¡, and boiling point, T,, of the solution. Constants can be found in the table of colligative constants.

The freezing point of 59.49 g of a pure solvent is measured to be 44.96 ºC. When 2.18 g of an unknown solute (assume the van 't Hoff factor = 1.0000) is added to the solvent the freezing point is measured to be 42.65 ºC. If the freezing point depression constant of the pure solvent is 7.66 ºC·kg solvent/mol solute calculate the molar mass of the solute. ?=g/mol

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Enumerate at least two colligative properties and explain its principle

The freezing point of a solution that contains 1.1 g of an unknown compound, (A), dissolved in 12 g of benzene is found to be 2.97 °C. The freezing point of pure benzene is 5.48 °C. The freezing point depression constant of benzene is 5.12 °C/molal. What is the molecular weight of the unknown compound?

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A solution is made by dissolving 0.517 mol of nonelectrolyte solute in 839 g of benzene. Calculate the freezing point, T;, and boiling point, T,, of the solution. Constants can be found in the table of colligative constants. Tf = °C T, = °C

At a certain temperature the vapor pressure of pure heptane C7H16 is measured to be 178. torr. Suppose a solution is prepared by mixing 110. g of heptane and 90.9g of benzene C6H6.

The freezing point of pure benzene is 5.50^o C. A solution is made by dissolving 0.300 g of naphthalene, C10H8, in 15.00 g of benzene. Calculate the freezing point of this solution. Calculate the molarity of naphthalene in the resulting solution.

A solution is made by dissolving 0.535 mol of nonelectrolyte solute in 819 g of benzene. Calculate the freezing point, Tr, and boiling point, Th. of the solution. Constants can be found in the table of colligative constants. T₁ = 81.83 Incorrect T = 2.16 Incorrect 'C 'C