2. 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.

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2. 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.
3. What mass of ethylene glycol must be added to 1255 g water to raise the boiling point to
103.9°C?
4. A solution is prepared by dissolving 384 g of sucrose (C12H22O11) in 647 g of water. What is
the vapor pressure of this solution at 30°C? (The vapor pressure of water is 31.8 mmHg at
30°C.)
Transcribed Image Text:2. 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. 3. What mass of ethylene glycol must be added to 1255 g water to raise the boiling point to 103.9°C? 4. A solution is prepared by dissolving 384 g of sucrose (C12H22O11) in 647 g of water. What is the vapor pressure of this solution at 30°C? (The vapor pressure of water is 31.8 mmHg at 30°C.)
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