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Boiling point of an aqueous solution of 0.5 m ionic solid substance is 100.5OC; then state the value of i ? $ (Kb = 0.512 ^\circ C -kg – mole^{-1}) $
Aqueous solution of substance boils at $ 100.5 ^\circ C at 1 bar pressure; then at what temperature it freezes ? (Kb = 0.512 ^\circ C -kg - mole^{-1}, Kf = 1.86 ^\circ C - kg – mole^{-1} ) $
1.4 m aqueous solution of a weak electrolyte AB2 ionizes 20%, then, state boiling point and freezing point of the solution respectively.
For a weak electrolyte solution, the boiling point elevation and freezing point depression depend on the degree of ionization. If the 1.4 m solution of AB2 ionizes 20%, then the effective molality is 1.4 x (1 + 0.2 x 2) = 2.24 m. Using the given values of Kb and Kf, the calculated boiling point and freezing point match option 2.
Solute substance in a 1.4 m aqueous solution associates by 25%, then, find the boiling point and freezing point of solution; where, solute exists as trimer in the solution; thus,n = 3. $ (Kb = 0.512 ^\circ C • kg • mole ^{-1} , Kf = 1.86 ^\circ C • kg • mole^{-1}) $
Molecular mass of a weak acid HA is 60gm/mo1 Ifs experimental molecular mass in its 0.7 M aqueous solution obtained from colligative properties is 50gm/mo1. Then calculate ionistion consteint of weak acid HA.
According to Boyle-van’t - Hoff law at a constant temperature, osmotic pressure of a solution is directly proportional to its molarity. It means $ \pi \alpha C where C = molarity of solution \therefore \pi = Kc Then calculate the value of k in SI unit at 24 ^\circ c temperature. (R = 8. 314 J/mole k) $
According to the Boyle-van't Hoff law, the osmotic pressure (π) is directly proportional to the molarity (C) of the solution at a constant temperature. The constant of proportionality is represented by k, known as the van't Hoff factor. The value of k can be calculated using the gas constant (R) and the absolute temperature (T). k = RT, where R = 8.314 J/mol·K and T = 24°C + 273.15 = 297.15 K. Substituting the values, k = (8.314 J/mol·K) × (297.15 K) = 2494.2 J/mol.
Boiling point of an aqueous solution of urea at one bar pressure is 373.41 k. Then at a constant temperature, calculate the percentage decrease in vapoure pressure of a solution compared to $ (k_b = 0.512 k.kg. mol ^{-1}) $
Calculate $ P^H of a solution prepared by mixing equal volume of an aqueous solution of HCI having P^H = 2 and P^H = 5 at 298 k temp $ .
Which of the following is the correct formula for Rqoult’s law when non-volatile solute is mixed with liquid solvent. where n=mole traction of solute N= mok fraction of solvent, P= vapour pressure of solution Po = vapour pressure of pure solvent and ïP=Decrease in vapour pressure
Which of the following is correct option when kcl is dissolved in $ H_20 $ .?
When KCl (an ionic solid) dissolves in water, the lattice enthalpy is overcome, which is an endothermic process (ΔH is positive). The ions become disordered in solution, increasing entropy (ΔS is positive). The overall process is spontaneous, so ΔG is negative.
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