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1. Using the solute formulas provided, convert grams of solute to moles of solute. For the hydrated salts 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 water and the ice. If you used exactly 50.0 g of each, then you would have used 100.0 g or 0.100 kg of solvent. Use the actual masses of water and ice recorded in your lab notebook to calculate the mass of solvent. 3. Calculate the molality of the solution using the moles of solute (from Step 1) and the mass of solvent (from Step 2): moles of solute mass of solvent, kg molality, m =

1. Using the solute formulas provided, convert grams of solute to moles of solute. For the hydrated salts 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 water and the ice. If you used exactly 50.0 g of each, then you would have used 100.0 g or 0.100 kg of solvent. Use the actual masses of water and ice recorded in your lab notebook to calculate the mass of solvent. 3. Calculate the molality of the solution using the moles of solute (from Step 1) and the mass of solvent (from Step 2): moles of solute mass of solvent, kg molality, m =

Macroscale and Microscale Organic Experiments
Macroscale and Microscale Organic Experiments
7th Edition
ISBN:9781305577190
Author:Kenneth L. Williamson, Katherine M. Masters
Publisher:Kenneth L. Williamson, Katherine M. Masters
Chapter6: Steam Distillation, Vacuum Distillation, And Sublimation
Section: Chapter Questions
Problem 6Q: A mixture of toluene (bp110.8C) and water is steam distilled. Visual inspection of the distillate...
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The initial temperature for all 3 solutions was 0.9 degrees C. 

Observed Molality i Theoretical Mass of Mass of Mass of Solute solute (g) ice (g) water (g) f.p. (°C) (m) f.p. (°C) 4894 49.92-1°C 2.91 CaClz - 2H,0 0.00 NaCl 7.37564351.70 17.12 A8.5 51.17 NA INA C12H2„O11 0.5°C Fe(NO,)3 · 9H,O|NA NA NA NA NA
Transcribed Image Text:Observed Molality i Theoretical Mass of Mass of Mass of Solute solute (g) ice (g) water (g) f.p. (°C) (m) f.p. (°C) 4894 49.92-1°C 2.91 CaClz - 2H,0 0.00 NaCl 7.37564351.70 17.12 A8.5 51.17 NA INA C12H2„O11 0.5°C Fe(NO,)3 · 9H,O|NA NA NA NA NA
Calculations 1. Using the solute formulas provided, convert grams of solute to moles of solute. For the hydrated salts 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 water and the ice. If you used exactly 50.0 g of each, then you would have used 100.0 g or 0.100 kg of solvent. Use the actual masses of water and ice recorded in your lab notebook to calculate the mass of solvent. 3. Calculate the molality of the solution using the moles of solute (from Step 1) and the mass of solvent (from Step 2): moles of solute mass of solvent, kg molality, m = 4. Determine the value for the van't Hoff factor (i) for each of your solutes. For molecular solutes the value is i = 1. For ionic solutes, you can determine the value of i by examining the molecular formula. The value will be a small whole number; partial ionization is not expected, and waters of hydration are not included. 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. 7. Comment in your lab notebook about the relationship between the observed freezing points and the number of particles in solution (i) for each solute. 14 Colligative Pr o perties of Solutions- Freezing Point Depression | Labor atory 2
Transcribed Image Text:Calculations 1. Using the solute formulas provided, convert grams of solute to moles of solute. For the hydrated salts 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 water and the ice. If you used exactly 50.0 g of each, then you would have used 100.0 g or 0.100 kg of solvent. Use the actual masses of water and ice recorded in your lab notebook to calculate the mass of solvent. 3. Calculate the molality of the solution using the moles of solute (from Step 1) and the mass of solvent (from Step 2): moles of solute mass of solvent, kg molality, m = 4. Determine the value for the van't Hoff factor (i) for each of your solutes. For molecular solutes the value is i = 1. For ionic solutes, you can determine the value of i by examining the molecular formula. The value will be a small whole number; partial ionization is not expected, and waters of hydration are not included. 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. 7. Comment in your lab notebook about the relationship between the observed freezing points and the number of particles in solution (i) for each solute. 14 Colligative Pr o perties of Solutions- Freezing Point Depression | Labor atory 2
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