$$\mathrm{K}_{\mathrm{H}}$$ for $$\mathrm{O}_2$$ at $$293 \mathrm{~K}$$ is $$34.86 \mathrm{~kbar}$$. What should be the partial pressure of $$\mathrm{O}_2$$ gas so that it has a solubility of $$0.08 \mathrm{~g} / \mathrm{L}$$ in water at $$293 \mathrm{~K}$$ ? (Density of solution $$=1 \mathrm{~g} / \mathrm{ml}$$)

What is the amount of ice that separates out on cooling a solution containing $$60 \mathrm{~g}$$ of Ethylene glycol in $$250 \mathrm{~g}$$ of water to $$-9.3^{\circ} \mathrm{C}$$ ? $$\mathrm{K}_{\mathrm{f}}$$ of $$\mathrm{H}_2 \mathrm{O}=1.86 \mathrm{~K} / \mathrm{m} ;$$ MM of ethylene glycol= $$62 \mathrm{~amu}$$

$$\text { If a compound } \mathrm{X}_3 \mathrm{Y} \text { is } 60 \% \text { ionised in aqueous medium, what is its van't Hoff factor value? }$$

Above figure represents Vapour pressure versus Temperature graphs of 2 pure volatile liquids and a solution formed by the 2 liquids.

(i) Which curve represents the solution?

(ii) Which curve represents the liquid with the strongest intermolecular forces of attraction?