Assuming ideal solution behavior, what is osmotic pressure...

Assuming ideal solution behavior, what is osmotic pressure of a solution of bovine insulin (molar mass, $5700 \mathrm{g}$ mol $^{-1}$ ) at $18^{\circ} \mathrm{C}$ if $100.0 \mathrm{mL}$ of the solution contains $0.103 \mathrm{g}$ of the insulin? (a) Outline the steps necessary to answer the question. (b) Answer the question.

Assuming ideal solution behavior, what is osmotic pressure of a solution of bovine insulin (molar mass, $5700 \mathrm{g}$ mol $^{-1}$ ) at $18^{\circ} \mathrm{C}$ if $100.0 \mathrm{mL}$ of the solution contains $0.103 \mathrm{g}$ of the insulin?
(a) Outline the steps necessary to answer the question.
(b) Answer the question.

Key Concepts

Osmotic Pressure

Osmotic pressure is a colligative property of solutions that represents the pressure required to stop the net flow of solvent through a semipermeable membrane from a pure solvent into the solution. This property depends solely on the number of solute particles present in the solution rather than on their specific nature.

Osmotic Pressure Equation

The osmotic pressure can be calculated using the equation ? = iMRT, where ? is the osmotic pressure, i is the van’t Hoff factor (which equals 1 for non-dissociating species), M is the molar concentration of the solute, R is the universal gas constant, and T is the absolute temperature in Kelvin.

Molar Concentration Calculation

Molar concentration (M) is determined by dividing the number of moles of solute by the volume of the solution in liters. This requires converting the given mass of the solute to moles using its molar mass, and then using the resulting moles in the calculation of molarity.

Temperature Conversion

When applying thermodynamic equations like the osmotic pressure equation, it is essential to convert the temperature from Celsius to Kelvin by adding 273.15, ensuring that the temperature is in the proper units required by the universal gas constant.

Ideal Solution Behavior

Assuming ideal solution behavior implies that the interactions among particles in the solution are such that the solute does not affect the behavior of the solvent significantly. This simplifies calculations as it allows the direct application of colligative property equations without corrections for non-ideal behavior.

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