At $$20$$°C, the vapor pressure of $$0.1$$ molal aqueous solutions of urea is $$0.03$$ mm less than that of water, and the vapor pressure of $$0.1$$ molal solutions of KCl is $$0.0594$$ mm less than that of water. The apparent percentage dissociation of KCl in water at the given temperature is (Neglect$$ the moles of solute particles in comparison to the moles of water in both $$solutions).

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$$T=20$$∘C $$0.1m$$ solution of urea Δ$$P=0.03mmKCl$$→$$0.1m$$ Δ$$P=0.0594$$Δ$$PP=x$$β→$$0.1$$ mole  in $$1kg0.03P=0.10.1+55.5P=0.03$$×$$55.650.1=16.695$$Δ$$PP=iX$$ρ$$0.059416.695=i$$  [$$0.00179$$]$$i=1.987$$

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