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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}) $
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)
Which type of solution, moist air is ?
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.
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)
Answer = D Highest osmotic pressure is for that pair having highest difference between $ n_1 M_1 and n_2 M_2 $
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)
At constant temperature, solubility of which of the following substances decreases with increase in temperature ?
The solubility of COâ‚‚ in water decreases with an increase in temperature. This is because the dissolution of COâ‚‚ in water is an exothermic process, and according to Le Chatelier's principle, an increase in temperature shifts the equilibrium towards the endothermic direction, decreasing the solubility.
At constant temperature, in a closed vessel, an ideal solution is formed by liquid – A and liquid – B; and mole-fraction of A and B are 0.6 and 0.4 respectively. If vapour pressure of pure liquids are 125.0 and 62.5 mm respectively, then their mole-fraction in vapour state are respectively – (In vessel, no other component is in gaseous form)
For an ideal solution, the mole fraction of a component in the vapor phase is directly proportional to its vapor pressure. Since the vapor pressures of A and B are 125.0 and 62.5 mm, respectively, their mole fractions in the vapor phase will be in the ratio of 2:1, which corresponds to 0.75 and 0.25.
At constant temperature, two liquids having osmotic pressure $ \nu_1 and \nu_2 $ are seperated by semipermeable membrane, then, what will be the osmotic pressure of the system ?
$ p_A = p^0 _A \times X_A $ $ = 125 \times 0.6 $ = 75 mm $ p_B = p ^ 0_B \times X_B = 62.5 \times 0.4 = 25mm $ $ p_{total} = p_A + p_B = 75 + 25 = 100 mm $ $ p_A = p_{Total} \times Y_A $ $ \therefore 75 = 100 \times Y_A $ $ \therefore Y_A = 0.75 $ $ Similarly \therefore Y_B = 0.25 $
Which of the following pair of solutions forms ideal solution ?
Ideal solutions are formed by mixing two liquids that are chemically similar and have similar intermolecular forces. Benzene and toluene are both non-polar, aromatic hydrocarbons, and their molecules have similar sizes and shapes, allowing them to mix easily, forming an ideal solution.
Which of the following pair forms true solutions ?
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