The osmotic pressure of a solution formed by dissolving 25.0 mg of aspirin (C₉H₈O₄)in 0.250 L of water at 25°C is __________ atm. A)13.6 B)1.14 × 10^-3 C)0.0136 D)2.45 E)1.38

Question

Quizplus · Accepted Answer

We can use the equation for calculating the osmotic pressure of a solution π = MRT, where M is the molar concentration of the solute, R is the gas constant, and T is the temperature in Kelvin.

First, we need to calculate the molar concentration of aspirin: 
Molar mass of aspirin = 180.16 g/mol 
Moles of aspirin = 25.0 mg / 180.16 g/mol = 0.000139 moles 
Molarity of aspirin = 0.000139 moles / 0.250 L = 0.000556 M

Next, we can plug in the values into the equation: 
π = (0.000556 M)(0.0821 L·atm/mol·K)(298 K) = 0.0136 atm

Therefore, the osmotic pressure of the solution is 0.0136 atm. The answer is (C).

The Osmotic Pressure of a Solution Formed by Dissolving 25