Multiple Choice
The osmotic pressure of blood is 5950.8 mmHg at 41ºC. What mass of glucose, C6H12O6, is needed to prepare 5.51 L of solution. The osmotic pressure of the glucose solution is equal to the osmotic pressure of blood.
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9. Solutions
Osmotic Pressure
Multiple Choice
The osmotic pressure of a solution containing 7.0 g of insulin per liter is 23 torr at 25ºC. What is the molar mass of insulin? (1 atm = 760 torr)
A
474.5 g/mol
B
6x103 g/mol
C
5.2x103 g/mol
D
5.7x103 g/mol
0 Comments
Verified step by step guidance1
First, understand that osmotic pressure (π) can be calculated using the formula: π = iMRT, where i is the van't Hoff factor (which is 1 for non-electrolytes like insulin), M is the molarity of the solution, R is the ideal gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin.
Convert the given osmotic pressure from torr to atm: 23 torr * (1 atm / 760 torr).
Convert the temperature from Celsius to Kelvin: T(K) = 25 + 273.15.
Calculate the molarity (M) of the solution using the rearranged formula: M = π / (iRT). Substitute the values for π (in atm), R, and T (in Kelvin) into the equation.
Finally, determine the molar mass of insulin by using the formula: Molar mass = mass of solute (g) / moles of solute. Use the calculated molarity to find the moles of solute in 1 liter of solution, and then use the given mass of insulin (7.0 g) to find the molar mass.
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