Assume a living cell with $$0.9%(\omega / \omega)$$ of glucose solution (aqueous). This cell is immersed in another solution having equal mole fraction of glucose and water. (Consider the data upto first decimal place only) The cell will

A living cell contains $$0.9\%$$ (w/w) glucose solution and is immersed in a solution with equal mole fractions of glucose and water.

Equal mole fractions of glucose and water means $$x_{glucose} = x_{water} = 0.5$$, so the moles of glucose and water are equal. Assuming 1 mol of each, the mass of glucose is $$180\text{ g}$$ and the mass of water is $$18\text{ g}$$, giving a total mass of $$198\text{ g}$$ and a percentage by mass of $$\%(w/w) = \frac{180}{198}\times 100 \approx 90.9\%$$ for the external solution.

The cell has $$0.9\%$$ glucose, while the external solution has approximately $$90.9\%$$ glucose, making the external solution extremely hypertonic compared to the cell.

Because the external solution has a much higher solute concentration and a correspondingly lower water activity, water will flow out of the cell by osmosis, causing the cell to shrink dramatically. However, the calculated concentration (~90.9\%) does not match any of the specific percentages given in options A, B, or C.

The correct answer is Option D) None of these.