A solution of $$\mathrm{KCl}(\mathrm{M}=74.5 \mathrm{~g} \mathrm{~mol}^{-1})$$ containing $$1.9 \mathrm{~g}$$ per $$100 \mathrm{~mL}$$ of $$\mathrm{KCl}$$ is isotonic with a solution of urea $$(\mathrm{M}=60.0 \mathrm{~g} \mathrm{~mol}^{-1}$$) containing $$3 \mathrm{~g}$$ per $$100 \mathrm{~mL}$$ of urea. The degree of dissociation of $$\mathrm{KCl}$$ is: [Assume both the solutions are kept at same temperature]

Which among the following compounds has the highest freezing point of its 1 molal aqueous solution?

In the following question a statement of Assertion (A) followed by a statement of Reason (R) is given. Choose the correct option out of the choices given below.

Assertion (A): van't Hoff factor for a solution of benzoic acid in benzene is less than one.

Reason(R): Benzoic acid undergoes dissociation in benzene and its calculated molecular mass using colligative properties is lower than its actual molecular mass.

$$\mathrm{K}_{\mathrm{H}}$$ 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 $$=1 \mathrm{~g} / \mathrm{ml}$$)