The osmotic pressure of 1.75 x102 M solutions of CaCl2 and urea at 25°C are 1.05 and 0.427 atm, respectively. Calculate the van't Hoff factor for the CaCl2 solution.
The osmotic pressure of 1.75 x102 M solutions of CaCl2 and urea at 25°C are 1.05 and 0.427 atm, respectively. Calculate the van't Hoff factor for the CaCl2 solution.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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![O 5. The osmotic pressure of 1.75 x102 M solutions of CaCl2 and urea at 25°C are 1.05
and 0.427 atm, respectively. Calculate the van't Hoff factor for the CaCl2 solution.
6. What mass of insulin must be dissolved in 38.0 mL of water to produce a solution with an
osmotic pressure of 15.5 mmHg at 25°C? The molar mass of insulin is 5808 g/mol.
7. A solution of 4.75 g of carbohydrate in 100.0 g of water has a density of 1.017 g/mL and an
osmotic pressure of 3.24 atm at 20.0°C. Calculate the molar mass of the carbohydrate.
moon!](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe8e7ecd1-00b2-4f87-97f4-1e990180b5ce%2Ff3afcb84-4e11-47a3-ab9f-51fadedb11df%2F1iul0r4_processed.jpeg&w=3840&q=75)
Transcribed Image Text:O 5. The osmotic pressure of 1.75 x102 M solutions of CaCl2 and urea at 25°C are 1.05
and 0.427 atm, respectively. Calculate the van't Hoff factor for the CaCl2 solution.
6. What mass of insulin must be dissolved in 38.0 mL of water to produce a solution with an
osmotic pressure of 15.5 mmHg at 25°C? The molar mass of insulin is 5808 g/mol.
7. A solution of 4.75 g of carbohydrate in 100.0 g of water has a density of 1.017 g/mL and an
osmotic pressure of 3.24 atm at 20.0°C. Calculate the molar mass of the carbohydrate.
moon!
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