Freezing Point Depression and Boiling Point Elevation

Freezing Point Depression and Boiling Point Elevation -...

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Freezing Point Depression and Boiling Point Elevation Problems Name __________________________________ Block _________ 1. Determine the boiling point elevation for 2.5 g of HCl in 1000 mL of water ( Kb of water = 0.51°C/m ) 2. Determine the number of moles of ammonium nitrate in a solution that contains ammonium nitrate and 450 mL of water. The freezing point of the solution is – 0.2°C and the Kf of water = -1.86°C/m . 3. What is the freezing point of a solution that contains 17.1 g of sucrose, C 12 H 22 O 11 , and 200 g of water? 4. The freezing point of an aqueous sodium chloride solution is – 20.0 °C. What is the molality of the solution? 5. What is the expected boiling point elevation of water for a solution that contains 150.0 g of magnesium sulfate dissolved in 1.0 kg of water? 6. Given 0.01 m aqueous solutions of each of the following, arrange the solutions in order of
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Unformatted text preview: increasing change in the freezing point of the solution. a. NaI b. CaCl 2 c. K 3 PO 4 d. C 6 H 12 O 6 7. Determine the expected boiling point of a solution made by dissolving 25 g of barium iodide in 0.150 L of water. 8. The boiling point for a solution of sodium phosphate and water is 100.65°C. Determine the molality of this solution. 9. Which solution will have a higher boiling point: A solution containing 105 grams of sucrose (C 12 H 22 O 11 ) in 500 grams of water or a solution containing 35 grams of sodium chloride in 500 grams of water? 10. Determine the van’t Hoff factor for an electrolyte solution that contains 0.04 moles of solute in 0.5 kg of water and its freezing point is –0.45°C....
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This note was uploaded on 12/09/2011 for the course SP 108 taught by Professor Whittenburg during the Summer '11 term at Montgomery College.

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