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प्रश्न
Suggest the most important type of intermolecular attractive interaction in the following pair.
NaClO4 and water
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उत्तर
Ion-dipole interactions, as water molecules are polar by nature, whereas NaClO4 becomes ionised in solution and provides Na+ and \[\ce{ClO^-_4}\] ions.
संबंधित प्रश्न
Heptane and octane form an ideal solution. At 373 K, the vapour pressures of the two liquid components are 105.2 kPa and 46.8 kPa respectively. What will be the vapour pressure of a mixture of 26.0 g of heptane and 35 g of octane?
Define an ideal solution and write one of its characteristics.
The KH for the solution of oxygen dissolved in water is 4 × 104 atm at a given temperature. If the partial pressure of oxygen in air is 0.4 atm, the mole fraction of oxygen in solution is ______.
Assertion: An ideal solution obeys Raoults Law.
Reason: In an ideal solution, solvent – solvent as well as solute – solute interactions are similar to solute-solvent interactions.
For ideal solution the enthalpy of mixing of the pure components to form the solution is ____________.
Which of the following condition is not satisfied by an ideal solution?
Which relationship is not correct?
Which of the following is an example of a solid solution?
Intermolecular forces between two benzene molecules are nearly of same strength as those between two toluene molecules. For a mixture of benzene and toluene, which of the following are not true?
(i) ∆mix H = zero
(ii) ∆mix V = zero
(iii) These will form minimum boiling azeotrope.
(iv) These will not form ideal solution.
Assertion: Molarity of a solution in liquid state changes with temperature.
Reason: The volume of a solution changes with change in temperature.
Assertion: When a solution is separated from the pure solvent by a semipermeable membrane, the solvent molecules pass through it from pure solvent side to the solution side.
Reason: Diffusion of solvent occurs from a region of high concentration solution to a region of low concentration solution.
Explain the terms ideal and non-ideal solutions in the light of forces of interactions operating between molecules in liquid solutions.
Dissociation constant and molar conductance of an acetic acid solution are 1.78 × 10–5 mol L–1 and 48.15 S cm–2 mol–1 respectively. The conductivity of the solution is (considering molar conductance at infinite dilution is 390.5 S cm–2 mol–1)
The pH of a solution of hydrochloric acid is 1.5. Calculate the concentration of the acid.
Lowering of vapour pressure of an aqueous solution of a non-volatile, non-electrolyte 1 molal aqueous solution at 100°C is ______.
If liquids A and B form an ideal solution, the ______.
5 moles of liquid X and 10 moles of liquid Y make a solution having a vapour pressure of 70 torr. The vapour pressures of pure X and Y are 63 torr and 78 torr respectively. Which of the following is true regarding the described solution?
