Chapter 12: Problem 84

Solutions A and B have osmotic pressures of 2.4 atm and 4.6 atm, respectively, at a certain temperature. What is the osmotic pressure of a solution prepared by mixing equal volumes of \(\mathrm{A}\) and \(\mathrm{B}\) at the same temperature?

Short Answer

Expert verified

The osmotic pressure of the mixed solution will be 3.5 atm.

Step by step solution

Understand the Concept of Osmotic Pressure

Osmotic pressure is the minimum pressure which needs to be applied to a solution to prevent the inward flow of its pure solvent across a semipermeable membrane. Since both Solutions A and B are mixed in equal volumes, the resulting solution will have an osmotic pressure that is the average of the two initial pressures.

Calculate the Average

To calculate the average osmotic pressure, add the osmotic pressures of Solutions A and B. This sum is then divided by 2, the number of solutions mixed. In this exercise, this translates to: (osmotic pressure of Solution A + osmotic pressure of Solution B) / 2 or, using the given numbers, (2.4 atm + 4.6 atm) / 2.

Find the Osmotic Pressure of the Mixture

By plugging in the given pressures into the formula in step 2, we are then left with the following calculation to be made: (7 atm) / 2, which simplifies to 3.5 atm.

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Solutions A and B have osmotic pressures of 2.4 atm and 4.6 atm, respectively, at a certain temperature. What is the osmotic pressure of a solution prepared by mixing equal volumes of \(\mathrm{A}\) and \(\mathrm{B}\) at the same temperature?

Short Answer

Step by step solution

Understand the Concept of Osmotic Pressure

Calculate the Average

Find the Osmotic Pressure of the Mixture

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