Solubility of a solute mixture (iodine + anthracene) in binary and ternary solvent mixtures of xylenes with or without toluene. Comparison with the ideal-like solution model

Jin, Xiao-Wu; Wang, Zhi‐Chang

doi:10.1006/jcht.1999.0598

Cited by 2 publications

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“…Equation has been verified , by the joint solubility measurements of a solute mixture [iodine (A1) + anthracene (A2)] in {iodine (A1) + anthracene (A2) + toluene (B) + benzene (C)}, {iodine (A1) + anthracene (A2) + toluene (B) + m -xylene (C)}, {iodine (A1) + anthracene (A2) + toluene (B) + o -xylene (C)}, {iodine (A1) + anthracene (A2) + toluene (B) + p -xylene (C)}, {iodine (A1) + anthracene (A2) + m -xylene (B) + o -xylene (C)}, {iodine (A1) + anthracene (A2) + m -xylene (B) + p -xylene (C)}, {iodine (A1) + anthracene (A2) + o -xylene (B) + p -xylene (C)}, and {iodine (A1) + anthracene (A2) + toluene (B) + m -xylene (C) + p -xylene (D)} at 298.15 K, where the concentration of iodine was determined directly by titrimetric measurements but that of anthracene was calculated by deducting the iodine concentration from the total absorption spectrophotometric measurements for the mixture of iodine and anthracene so that the experimental precision for anthracene was limited by the uncertainty of the two methods. The deviations defined by Δ s β = s β − ∑ i true{ x i / ∑ k x k true} s normalβ q ◦ , i for all these systems are |Δ s A1 | ≤ 0.001 and |Δ s A2 | ≤ 0.0001, which are within the experimental uncertainties of the titrimetric and spectrophotometric measurements.…”

Section: Second Extended Zsr Rule Of Wang and The Modelmentioning

confidence: 85%

“…Equation 7c has been verified 10,34 , where the concentration of iodine was determined directly by titrimetric measurements but that of anthracene was calculated by deducting the iodine concentration from the total absorption spectrophotometric measurements for the mixture of iodine and anthracene so that the experimental precision for anthracene was limited by the uncertainty of the two methods. The deviations defined by…”

Section: Second Extended Zsr Rule Of Wang and The Modelmentioning

confidence: 99%

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Relationship Among the Raoult Law, Zdanovskii−Stokes−Robinson Rule, and Two Extended Zdanovskii−Stokes−Robinson Rules of Wang

Wang

2008

J. Chem. Eng. Data

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are presented in a unified way. Similar to the Raoult law, which was first noted empirically in pyridine solutions, the ZSR rule for isopiestic mixed electrolyte and nonelectrolyte aqueous solutions can be extended to every kind of liquid and solid solutions such as organic mixtures, aqueous and nonaqueous electrolyte and nonelectrolyte solutions, liquid and solid alloys, molten salt mixtures, slags, and nonstoichiometric solid solutions, resulting in two extended ZSR rules of Wang. Although the solutions obeying the Raoult law (or the related classically ideal solution model) are very few as compared with the classically nonideal solutions, one classically ideal solution {B+C+...+Z} may mix with many pure components A to form the classically nonideal solutions {A+B+C+...+Z} following the first extended ZSR rule (or the related partial ideal solution model) or mix with much more nonideal solutions {A1+A2+...+Aq} to form the classically nonideal solutions {A1+A2+...+Aq+B+ C+...+Z} obeying the second extended ZSR rule (or the related ideal-like solution model). This would indicate that the ZSR rule and its extended forms are as important as the Raoult law for multicomponent systems.

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