Explanation
Greater the no. of instalments, greater is the extraction.
Solubility increases with temp. upto 34oC and then decreases. So the process is endothermic upto 34oC and exothermic thereafter.
Plot of Ptotal versus xA or xB is linear for ideal solution.
For non-ideal solution showing positive dev., ΔV = +ve, ΔH = +ve.
As solution shows positive deviations, A—B interactions are smaller.
There is H-bonding in ethyl alcohol which is cut off on adding n-heptane. Hence it shows positive deviations.
Colligative properties depend upon the number of solute particles.
Higher the concentration, lower is the vapour pressure. Thus S1 has lower conc. than S2. More solvent will flow from S1 to S2.
All relations are correct except (d) .
Depression in F. pt. will be maximum for BaCl2 due to dissociation and hence the F.pt. will be lowest.
Urea does not undergo dissociation or association. Hence van’t Hoff factor (i) =1.
PV = inRT.
By def. of Raoult’s law.
Boiling point of azeotropic mixtures is less when it shows positive deviations.
2KI + HgI2 → K2HgI4 . As a result of this reaction, no. of ions decrease. So the lowering in F pt. is less or the actual F. pt is more.
Molarity is independent of temp. because it involves wts. Only.
For ideal solution, ΔVmixing = 0 and ΔHmixing = 0.
Addition of solute lowers the freezing point.
0.01 m NaCl ≡ 0.02m Na+ and Cl− ions which is maximum. Hence depression in F. pt is max or actual F. pt is minimum.
There is no net movement of the solvent through the semi permeable membrane between two solutions of equal conc.
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