A membrane permeable to water but not to glucose (C₆H₁₂O₆)separates two aqueous solutions.Solution A is 0.156 M glucose and solution B contains pure water.There will be a net flow of water molecules across the membrane from solution B to solution A until equilibrium is established across the membrane.What pressure would have to be applied to solution A to prevent osmosis flow across the membrane at 25 °C? A)1.00 atm B)3.82 atm C)0.320 atm D)1.91 atm E)0.382 atm

Question

Quizplus · Accepted Answer

The pressure required to prevent the net flow of water molecules from solution B to solution A is known as the osmotic pressure (Π). The Van't Hoff equation gives the relationship between the concentration of the solute and the osmotic pressure:
Π = MRT, where M is the molarity of the solute, R is the gas constant, and T is the temperature in Kelvin.
In this case, we can calculate the osmotic pressure of solution A as follows:
M = 0.156 M glucose
R = 0.0821 L·atm/(mol·K)
T = 25 + 273 = 298 K
Π = (0.156 M)(0.0821 L·atm/(mol·K))(298 K) = 3.82 atm
Therefore, the pressure that would have to be applied to solution A to prevent osmosis flow across the membrane is 3.82 atm, which is option (B).

A Membrane Permeable to Water but Not to Glucose (C6H12O6)separates

A Membrane Permeable to Water but Not to Glucose (C₆H₁₂O₆)separates