JEE Main 2026 — Chemistry Physical Chemistry

For Statement I:

Molarity of the solution in Chamber 1 ($M_1$M1​) = $\dfrac{18 / 180}{100 / 1000} = 1$100/100018/180​=1 M

Molarity of the solution in Chamber 2 ($M_2$M2​) = $\dfrac{30 / 180}{250 / 1000} = \dfrac{1/6}{1/4} = 0.667$250/100030/180​=1/41/6​=0.667 M

Since $M_1 > M_2$M1​>M2​, the solution in Chamber 1 has a higher solute concentration. During osmosis, the solvent (water) moves from the region of lower solute concentration to the region of higher solute concentration across a semi-permeable membrane. Thus, water will move from Chamber 2 to Chamber 1. Statement I is false.

For Statement II:

The osmotic pressure is given by $\pi = iCRT$π=iCRT

For $K_2SO_4$K2​SO4​, assuming complete dissociation ($K_2SO_4 \rightarrow 2K^+ + SO_4^{2-}$K2​SO4​→2K++SO42−​), the van't Hoff factor $i = 3$i=3.

Concentration $C = \dfrac{50 \times 10^{-3}}{174 \times 2}$C=174×250×10−3​ mol/L

$$\pi = 3 \times \left( \dfrac{50 \times 10^{-3}}{174 \times 2} \right) \times 0.083 \times 300$$π=3×(174×250×10−3​)×0.083×300

$\pi = \dfrac{3 \times 0.05 \times 24.9}{348} = \dfrac{3.735}{348} \approx 0.0107$π=3483×0.05×24.9​=3483.735​≈0.0107 bar

Statement II is true.

Therefore, Statement I is false but Statement II is true.

Answer: Statement I is false but Statement II is true