I need help with 5 and 6. The initial temperature for all 3 solutions was 0.9 degrees C. Calculations1. Using the solute formulas provided, convert grams of solute to moles of solute. For the hydratedsalts be sure to include the waters of hydration in the molar mass.2. It is reasonable to assume that the total mass of solvent includes the mass of both the waterand the ice. If you used exactly 50.0 g of each, then you would have used 100.0 g or 0.100 kg ofsolvent. Use the actual masses of water and ice recorded in your lab notebook to calculate themass of solvent.3. Calculate the molality of the solution using the moles of solute (from Step 1) and the mass ofsolvent (from Step 2):moles of solutemass of solvent, kgmolality, m =4. Determine the value for the van't Hoff factor (i) for each of your solutes. For molecular solutesthe value is i = 1. For ionic solutes, you can determine the value of i by examining the molecularformula. The value will be a small whole number; partial ionization is not expected, and watersof hydration are not included.5. Calculate the theoretical freezing point depression for each of the solutions in °C. The k, forwater is 1.86°C/m.6. Calculate the theoretical freezing point of each solution, and compare it with theexperimentally observed freezing point for your solutes.7. Comment in your lab notebook about the relationship between the observed freezing pointsand the number of particles in solution (i) for each solute.14Colligative Pr o perties of Solutions- Freezing Point Depression | Labor atory 2 Mass ofMass ofMass ofObservedMolalityTheoreticalSolutesolute (g)ice (g)water (g)f.p. (°C)(m)f.p. (°C)2.91 4894 49.92-1°CC 049 20.0c 0t3 13NaClCaCl, · 2H,O 7.37 5643 51.700.0c17.12 485 51.170.5% 043 1C12H2,O1117.12A8551.17Fe(NO3)3 · 9H,OINANANA NANANA NA

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5. Calculate the theoretical freezing point depression for each of the solutions in °C. The k, for water is 1.86°C/m. 6. Calculate the theoretical freezing point of each solution, and compare it with the experimentally observed freezing point for your solutes.

5. Calculate the theoretical freezing point depression for each of the solutions in °C. The k, for water is 1.86°C/m. 6. Calculate the theoretical freezing point of each solution, and compare it with the experimentally observed freezing point for your solutes.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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