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In Binary ideal solution forms by liquid A and B, at constant temperature, mole-fraction of liquid A in vapour state is 0.4 and its partial vapour pressure is 400 mm, then what will be the partial vapour pressure of B ?

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Explanation

$ Y_A = 0.4 and P_A = 400 mm $ $ P_B = 1000 - 400 = 600 mm $ $ P_A = P_{Total} \times Y_A $ $ \therefore 400 = P \times 0.4 $ $ \therefore P_{Total} = 1000 mm $

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1.0 molal aqueous solution of a substance boils at $ 100.55 ^\circ C ; then, at what approximate temperature, it freezes ? (Kb = 0.51 ^\circ C – kg - mole^{-1} and Kb = 1.86 ^\circ C – kg - mole^{-1}) $

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Explanation

$ { \triangle Tf \over \triangle Tb } = { kf \over Kb } $ $ \therefore \triangle T_f = { Kf \over Kb } \times \triangle T_b $ $ = { 1.86 \over 0.51 } \times 0.55 = 2 K $ $ \therefore T_f = 273 - 2 = 271 K $

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Ionic substances are completely dissociates, then aqueous solution of which of the following substances having least freezing point ?

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Explanation

The freezing point depression of a solution is directly proportional to the number of particles present in the solution. Al2(SO4)3 dissociates into five ions (2Al^3+ and 3SO4^2-), which is the highest number of particles compared to the other options, leading to the greatest freezing point depression.

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0.2 M aqueous solution of $ NH_4Cl$ is isotonic with which of the following aqueous solution ?

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At constant temperature, osmotic pressure of an aqueous solution of 1.5 M $ NH_4NO_3 and xN Al_2(SO_4)_3 $ are equal, then mention the value of X. (Assume that ionic solid substances completely dissociates in the solution)

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Explanation

$ n_1 M_1 = n_2 M_2$ $ For NH_4 NO_3 values for n_1 and M_1 are 2 and 1.5 resp$ $ For Al_2 (SO)_4 n_2 = 5 $ $ \therefore M_2 = {2 \over 5 } \times 1.5 = 0.6 $ $ normality of Al_2(SO_4) _3 = 6 \times molarity $ $ = 6 \times 0.6 $ $ = 3.6 N $

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Boiling point of the aqueous solution prepared by dissolving 1.5 mole substances in 1000 gm water at 1 atmosphere pressure is $ 100.5 ^\circ C; then which of the following alternative is correct for the solution ? (Kb = 0.152 ^\circ C – kg - mole^{-1}) $

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Which of the following aqueous solution is isotonic with $ 0.2 m Na_4[CoF_6] $ solution ? (Assume that ionic solid substances completely dissociates in the solution)

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Which type of solution, moist air is ?

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Explanation

Moist air is a mixture of gaseous components, primarily nitrogen, oxygen, water vapor, and other trace gases. Since air is a gas under normal conditions, and the water vapor present in moist air is also in the gaseous state, moist air is classified as a gaseous solution.

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Aqueous solutions are separated by semipermeable membrane. For which pair of the given solution having maximum osmotic pressure ? (Assume that ionic solid substances completely dissociates in the solution)

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Explanation

Answer = D Highest osmotic pressure is for that pair having highest difference between $ n_1 M_1 and n_2 M_2 $

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At constant temperature, the vapour pressure of an aqueous solution of $ Na_2SO_4 and 0.3 m Na_3PO_4 are approximately equal; then, what would be the molality of an aqueous solution of Na_2SO_4 $ ? (Assume that ionic solid substances completely dissociates in the solution)

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