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.

          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.

Added by Steven H.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Madhur L

02/14/2023

Step 1

In this case, the solute is bovine insulin and the solvent is water. To calculate the concentration of solute, we need to know the molar mass of the insulin. The molar mass of insulin is $5700 \mathrm{g}$ mol $^{-1}$. To calculate the concentration of solvent, Show more…

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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.