0.2650 g of a compound of unknown molecular mass were dissolved in 18.00 mL of a non-ionizing solvent with specific gravity of 0.7480. The pure solvent was determined to have a freezing point of 6.80°C. The freezing point of the solution was determined graphically. Trial one yielded a freezing point of 5.31°C for the solution. Trial two indicated the freezing point to be 5.23°C. Kf (solvent) = 12.8 C°/m
a. Calculate the molecular mass of the unknown.
b. If 5.50 grams of solvent freeze out of the original solution, what is the freezing point of the new solution expected to be?
0.2650 g of a compound of unknown molecular mass were dissolved in 18.00 mL of a...
What is the molar mass of a nonpolar molecular compound if 6.34 g dissolved in 53.4 g benzene begins to freeze at 2.81 °C? The freezing point of pure benzene is 5.50 °C and the freezing point depression constant, Kf, is -5.12 °C/m. A. 2.26 x 10-4 g/mol B. 0.226 g/mol C. 12.1 g/mol D. 226 g/mol
The molar mass of unknown molecular compound is determined using freezing point depression. The substance is dissolved in benzene (C6H), an organic solvent. Use the data below to determine the molar mass of the substance. 8.65 g Mass of unknown compound Freezing point of solution Volume of benzene -10.21°C 35.0 mL 5.53°C Freezing point of benzene Density of benzene Kf for benzene 0.8765 g/mL 5.12°C/m Molar mass = g/mol
The freezing point of a solution of 1.104 g of an unknown nonelectrolyte dissolved in 36.81 g of benzene is 1.08°C. Pure benzene freezes at 5.48°C and its Kf value is 5.12°C/m. What is the molecular weight of the compound?
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. b) The molality of the solution is 3.63. How many moles of the unknown compound were dissolved in the solution? C) what is the molar mass of the unknown compound?
3a. Calculate the molar mass (in g/mol) of an unknown 1:1 electrolyte if 0.482 g dissolved in 223.1 mL of water at 74.75 °C has an osmotic pressure of 54.4 mmHg. R = 0.082058 L⋅atm⋅mol−1⋅K−1. 1.00 atm = 760 mmHg. Report your answer to THREE significant figures. 3b. Calculate the required mass of an unknown nonelectrolyte (ℳ = 131.5599 g/mol) dissolved in 140.1 g of solvent that gives a solution that boils at 36.04 °C. The boiling point of the...
p-dichlorobenzene is an organic molecular (covalent) compound with i = 1 and Kf = 7.10 oC/m A student weighed 11.20 mL of p-dichlorobenzene and recorded mass of it as 10.820 g. The freezing point of the pure p-dichlorobenzene liquid was determined as 53.1 oC. 1.118 g of an unknown solid compound was added and completely dissolved in the previous sample of pure p-dichlorobenzene liquid. The freezing point determination procedure was conducted for the solution and the freezing point of this...
The freezing point of a solution that contains 1.00 g of an unknown compound, (A), dissolved in 10.0 g of benzene is found to be 2.17 oC. The freezing point of pure benzene is 5.48 oC. The molal freezing point depression constant of benzene is 5.12 oC/molal. What is the molecular weight of the unknown compound?
When 0.60 grams of a non-electrolyte unknown compound is dissolved in 10 grams of water, the freezing point of the solution is -1.86o C. Given that the freezing point of pure water is 0o C and that the freezing-point depression constant for water is 1.86 o C/mol/kg, calculate the molecular mass (g/mol) of the unknown compound.
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