What is the osmotic pressure of a solution of 55.8 g of sucrose (C₁₂H₂₂O₁₁)in 200 mL of water at room temperature? A) 19.9 atm B) 1.67 atm C) 6.27 atm D) 11.5 atm E) 14.4 atm

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The correct answer is A because the osmotic pressure of a solution is directly proportional to the concentration of the solution. The concentration of the solution is calculated by dividing the mass of the solute by the volume of the solution. In this case, the mass of the solute is 55.8 g and the volume of the solution is 200 mL. Therefore, the concentration of the solution is 55.8 g / 200 mL = 0.279 M. The osmotic pressure of a solution is also directly proportional to the temperature of the solution. In this case, the temperature of the solution is room temperature, which is approximately 25 degrees Celsius. Therefore, the osmotic pressure of the solution is 0.279 M * 0.0821 L * atm / (mol * K) * 298 K = 19.9 atm.

What Is the Osmotic Pressure of a Solution of 55