13. A 0.230 m solution of an unknown electrolyte depresses the freezing point of water by...
Freezing point depression can be used to experimentally determine the van't Hoff factor of a solute in solution. Given the data in the table, please answer the questions below and determine the "real" van't Hoff factor of the solute. Experimental Results Mass of solvent (water) Freezing point of water Freezing point depression constant (Kf) of water Mass of solution Freezing point of solution 8.515 g 0.00°C 1.86°C/m 9.3589 -5.45°C a. What mass of solute was used? b. What is the...
1. What is the freezing point depression for the unknown solution for each trial? 2. How do you determine the van't Hoff factor for each trial, and what is the average van't Hoff factor? Trial 1: 18mL of 0.200 m unknown, ionic compound solution initial temp: 17.90 degrees C. observed freezing point of solution: -1.55 degrees C. Observed freezing point of water: -0.84 degrees C. Trial 2: 20 mL of 0.200 m unknown, ionic compound solution initial temp: 17.66 degrees...
The freezing point depression constant of water is -1.86 C/m. If 7.50 g NaCl is dissolved in 45.0 g H, O, the freezing point is changed by -9.71 *C. Calculate the van't Hoff factor for Naci. Select one: O a. 1,00 . OOOO c. 1.83
colligative properties: freezing point depression. Gen chem 2 HINKI Acetic acid is known as a weak acid (electrolyte) when it is dissolved in water. A solution was prepared by dissolving acetic acid in cyclohexane to yield a concentration of 1.0 molukg. The freezing point depression of the solution was determined to be 13.2 °C. What is the van't Hoff factor for acetic acid dissolved in cyclohexane? Is acetic acid an electrolyte when it is dissolved in cyclohexane? Explain. Kre20 °C/m...
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.
Pre-Laboratory Questions 1. The freezing point of 20.024 grams of distilled water was determined by recording a thermogram (see plot below). 1.006 grams of an unknown, nonelectrolyte compound was added to the water, and a second thermogram was recorded to determine the freezing point of the solution. Freezing Point Curves for Water and Unknown Nonelectrolyte Temperature, c -Water -0.270 °C Time, s a. Determine the freezing point depression, Tg, for the unknown solution. b. Determine the molality, m, of the...
21. What mass of Na2SO4 must be dissolved in 100.0 grams of water to lower the freezing point by 2.50 °C? The freezing point depression constant, Kfp, of water is -1.86 °C/m. Assume the van't Hoff factor for Na2SO4 is 2.95.
Calculate the molality of an aqueous solution of KBr whose freezing point is -4.95 degrees celsius. The Kf of water is 1.86 degrees C/m. Calculate the ideal Van't Hoff factor for KBr? Show work
You have a aqueous solution of NaCl that has a freezing point of -9.35°C. Assuming a van't Hoff factor of 1.9 for NaCl, what is the mass percent of chloride ion in the solution? (Kf for water is 1.86°C kg/mol).
The experimentally measured freezing point of a 1.50 m aqueous solution of CaCl2 is -6.70°C. The freezing point depression constant for water is Kf = 1.86°C/m. Assume the freezing point of pure water is 0.00°C. The experimentally measured freezing point of a 1.50 m aqueous solution of CaCl2 is -6.70°C. The freezing point depression constant for water is Kf = 1.86°C/m. Assume the freezing point of pure water is 0.00°C. What is the predicted freezing point if there were no...