Fish blood has an osmotic pressure equal to that of...

Fish blood has an osmotic pressure equal to that of seawater. If seawater freezes at $-2.3^{\circ} \mathrm{C}$, what is the osmotic pressure of the blood at $25^{\circ} \mathrm{C} ?$ To solve this problem, what assumptions must be made?

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Key Concepts

Temperature Dependence of Colligative Properties

An essential assumption in this problem is that the osmotic pressure depends linearly on the absolute temperature, as described by the van’t Hoff equation (? = iCRT). This means that when converting a property measured at one temperature to another, it is assumed that the solute concentration remains unchanged and that the relationship holds true over the temperature range being considered.

Ideal Solution Assumption

The problem assumes that the fish blood behaves as an ideal solution, meaning that interactions between solute particles and between solute and solvent are negligible. This assumption allows the use of simple formulas such as the van’t Hoff equation for osmotic pressure and the freezing point depression equation without corrections for non-ideal behavior.

Colligative Properties

This concept refers to properties of solutions that depend on the number of solute particles rather than their nature. In problems like this, the freezing point depression and the osmotic pressure are viewed as colligative properties, meaning they are directly related to solute concentration. It is assumed that both these phenomena behave similarly, allowing comparisons and conversions based on solute counts.

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