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Answer :
At equilibrium, Side B will have a lower column of fluid due to the net effect of both water and Na[tex]^+[/tex] movement.
In this experiment, we're dealing with a selectively permeable membrane that separates two sides of a U-tube: Side A containing pure water and Side B containing an aqueous solution with Na[tex]^+[/tex] and Br[tex]^-[/tex] ions.
Membrane Permeability: The membrane allows water and Na[tex]^+[/tex] ions to pass through but not Br[tex]^-[/tex] ions.
Concentration Gradient: Side B has a higher concentration of solute due to the presence of Na[tex]^+[/tex] and Br[tex]^-[/tex] ions compared to Side A, which is pure water.
Movement of Water: Initially, water will tend to move from Side A (pure water) to Side B (higher solute concentration) to try to equalize the concentration on both sides due to osmosis.
Equilibrium: However, because the membrane is permeable to water and Na[tex]^+[/tex], Na[tex]^+[/tex] ions will also move from Side B to Side A. The movement of Na[tex]^+[/tex] to Side A reduces the concentration of solute on Side B.
Final Equilibrium: When equilibrium is reached, the net movement of water stops as the osmotic pressure balance is achieved.
Fluid Level Outcome: Since the water moves initially towards Side B and Na[tex]^+[/tex] moves towards Side A to balance out concentration differences, the fluid column height will increase on Side A as water and Na[tex]^+[/tex] accumulate there.
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Side B will have a lower column of fluid; when equilibrium is reached and there is no net movement of water across the selectively permeable membrane.
Initially, water molecules will move from Side A (pure water) to Side B (aqueous solution of Na+ and Br-) through the membrane by osmosis, diluting the solution on Side B.
However, since the membrane is permeable to Na+ ions, they will also move from Side B to Side A, down their concentration gradient.
At equilibrium:
The concentration of water is equal on both sides.
The concentration of Na+ is equal on both sides.
But Br- ions, being impermeable to the membrane, remain only on Side B.
The presence of Br- ions on Side B contributes to the total osmotic pressure, but they cannot cross the membrane to equalize their concentration.
Since Side B still has the impermeable Br- ions, its osmotic pressure remains higher than Side A.
To balance this, the column of fluid on Side B will be lower than Side A due to the difference in osmotic pressure.
This phenomenon is known as Donnan equilibrium or Gibbs-Donnan effect.
