Multiple Choice
What is the osmotic pressure of a solution formed by dissolving 44.3 mg of aspirin (C9H8O4) in 0.358 L of water at 25 °C, assuming complete dissociation and ideal behavior?
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14. Solutions
Osmotic Pressure
Multiple Choice
Which of the following factors is responsible for the osmotic pressure of a solution?
A
Temperature of the solution
B
Pressure of the gas above the solution
C
Concentration of solute particles
D
Volume of the solvent
Verified step by step guidance1
Understand that osmotic pressure is a colligative property, which means it depends on the number of solute particles in a solution, not their identity.
Recall the formula for osmotic pressure: \( \Pi = iMRT \), where \( \Pi \) is the osmotic pressure, \( i \) is the van't Hoff factor (number of particles the solute dissociates into), \( M \) is the molarity of the solution, \( R \) is the ideal gas constant, and \( T \) is the temperature in Kelvin.
Identify that the concentration of solute particles (\( M \)) directly affects the osmotic pressure, as it is a part of the formula.
Note that while temperature (\( T \)) is a factor in the formula, the problem specifically asks for the factor responsible for osmotic pressure, which is primarily the concentration of solute particles.
Conclude that the correct answer is the concentration of solute particles, as it is the primary factor determining the osmotic pressure of a solution.
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