E T Q ¼ ½Qþ Š½X Š2 þ½Q þ Š½X Š2EQX T ½QXŠ¼½Q þ Š½X Š2E T Q 2 X 2¼ ½Q 2X 2 Š½Q þ Š½X Š 2 ð45Þð46Þð47ÞBy using Eqs (42)–(47), the values <strong>of</strong> E T Q þ, ET QX, EQ T 2 X 2, <strong>and</strong> the distribution constantm are evaluated. Corrections for the mean activity coefficient in the organic phase weremade using the Marshall <strong>and</strong> Grunwald expression, <strong>and</strong> the values <strong>of</strong> m, K da , K do , <strong>and</strong> were calculated by a numerical iteration method. Beronius <strong>and</strong> Bra¨ ndstro¨ m [91] evenclarified the identical value <strong>of</strong> K do at ½QXŠ ¼0 within the limits <strong>of</strong> experimental error<strong>and</strong> the conductance measurement. In view <strong>of</strong> past reports [87–92], most K da valueswere located in the range between 1 <strong>and</strong> 10; K do values were located in the range between10 1 <strong>and</strong> 10 5 . The dissociation ability <strong>of</strong> quaternary salt in the aqueous phase is greaterthan that in the organic phase.The quaternary salts QX can be completely dissociated to free ions (Q þ <strong>and</strong> X )inthe aqueous phase (, ½Q þ Š=½QXŠ > 100Þ <strong>and</strong> partially dissociated in the organic phasewhen the concentration <strong>of</strong> the quaternary salt is 0.0125 kmol/m 3 . The quaternary salts QXcan be partially dissociated to free ions in the aqueous <strong>and</strong> the organic phases when theconcentration <strong>of</strong> quaternary salt is 0:1 kmol=m 3 . The incremental rules <strong>of</strong> the dissociationdegree <strong>of</strong> the quaternary salts were obtained as follows: (1) increasing the charge-tovolumeratio <strong>of</strong> the central cation or counteranion (e.g., P þ > N þ or I > Br > Cl ),(2) increasing the electron-releasing groups on the quaternary cation (e.g., Aliquat336 > TBAC), <strong>and</strong> (3) increasing the electron-withdrawing groups on the quaternaryanion (e.g., TBA-TBPO > TBA-BPO > TBAC). Electron-releasing (or electron-withdrawing)groups apparently make the transition state more stable on the quaternarycation (or anion) while the ion-pair type <strong>of</strong> quaternary salts transferring through theinterface between two phases is a transition state. Bockries <strong>and</strong> Reddy [93] reportedthat the association constant decreased when the effective ionic radius <strong>of</strong> the ion pairwas increased.Quaternary salts in an organic phase must be determined experimentally to knowwhether the salts are dissociated or associated, <strong>and</strong>, if so, to what degree. The hydration <strong>of</strong>the anion plays an important role in dissociating the catalyst. Furthermore, the solvation<strong>of</strong> the anions increases the size <strong>of</strong> the ions, decreases their mobility <strong>and</strong> diffusion rate, <strong>and</strong>reduces the reactivity <strong>of</strong> the reactant. How many molecules <strong>of</strong> the coextracted water doeseach quaternary salt carry? Hence, the equation for the distribution <strong>of</strong> a tetralkylammoniumhalide into an organic phase can be written as [94,95]Q þ þ X þjH 2 O Ð Q þ þ X :jH 2 OQ þ þ X þjH 2 O Ð Q þ X :jH 2 Oð48Þð49ÞDepending on whether the species in the organic phase is dissociated as free ions [Eq. (48)]or associated as ion pairs [Eq. (49)], the corresponding equilibrium constants can bewritten asCopyright © 2003 by Taylor & Francis Group, LLC
E T Q þ ;H 2 O ¼ ½Qþ Š½X :jH 2 OŠ 2 ½Q þ Š½X Š½H 2 OŠ j 2 EQX;H T ½QX:jH2 O ¼2 OŠ½Q þ Š½X Š½H 2 OŠ j 2ð50Þð51ÞThe j value can be calculated by dividing ðH 2 OÞ by the amount <strong>of</strong> quaternary salts in theorganic phase. The water content difference in the organic phase ððH 2 OÞÞ equals thedifference between the measured water content in the solvent <strong>and</strong> that in the solution atthe same temperature.The order <strong>of</strong> magnitude <strong>of</strong> H 2 O in the organic phase for quaternary salts is Aliquat336 > TBA-TBPO > TBAI > TBPB > TBAB > TBAC. The sequence <strong>of</strong> ½H 2 OŠ for solventsis 1,2-C 2 H 4 Cl 2 > CH 2 Cl 2 > CHCl 3 > C 6 H 5 Cl. This tendency <strong>of</strong> the sequence <strong>of</strong> thecoextracted water is identical to that <strong>of</strong> the solubility <strong>of</strong> water in the organic phase <strong>of</strong> 1,2-C 2 H 4 Cl 2 ð1:3Þ > CH 2 Cl 2 ð0:81Þ > CHCl 3 ð0:08Þ > C 6 H 5 Cl ð0:05Þ at 20 C. The orders <strong>of</strong>influencing extraction capability <strong>of</strong> H 2 O are Cl > Br 3 C 6 H 2 O > Br > I <strong>and</strong> N þ > P þfor the anion <strong>and</strong> central cation, respectively. The trend for water content in the organicphase varied with increasing temperature. L<strong>and</strong>ini et al. [96] indicated that the solvatingcapability between quaternary salt <strong>and</strong> water could reduce the quaternary salt’s reactivityin the organic phase in a PT-catalyzed reaction. This result was confirmed by previous work[61,76]. Hence, it is significant to study the liquid–liquid PT-catalyzed reaction <strong>and</strong> toevaluate how many molecules <strong>of</strong> the coextracted water are carried by each quaternarysalt. The water content in the organic phase increased with increasing temperature. The ½H 2 OŠ value increased when the charge-to-volume ratio <strong>of</strong> the anion increased <strong>and</strong> when thepolarity <strong>of</strong> the solvent increased, but decreased as the lipophilicity <strong>of</strong> the quaternary saltincreased. These tendencies correspond to those reported by L<strong>and</strong>ini <strong>and</strong> coworkers[97,98]. Kenjo <strong>and</strong> Diamond [95] reported that the average water contents in a nitrobenzene/watersystem at 23 C were 3.3, 1.8, <strong>and</strong> 1 (mol/mol quaternary salt) for Cl ,Br , <strong>and</strong>I , respectively. Starks <strong>and</strong> Owens [99] reported that the hydration numbers <strong>of</strong>C 16 H 33 Bu 3 P þ X were 0.4, 4, <strong>and</strong> 5 for NO 3 ,Cl , <strong>and</strong> CN , respectively. The averagewater content in the organic phase ð½H 2 OŠÞ was about 1–3 mol/mol quaternary salt, exceptfor TBAC. Because the hydration numbers for different anions were different when thequaternary salt was TBA þ [(n-C 4 H 9 Þ 4 N þ Š, the results demonstrate that the water <strong>of</strong> hydrationis primarily associated with the anion, rather than with the quaternary cation.Quaternary ammonium ions are used as PT catalysts because they are least likely tointerfere in chemical reactions. According to the experimental results <strong>of</strong> Bra¨ ndstro¨ m [48],Herriott <strong>and</strong> Picker [100], <strong>and</strong> L<strong>and</strong>ini et al. [97], the organophilic quaternary cationsserved as more effective PT catalysts than quaternary cations with small alkyl chains.Thus, the incremental number <strong>of</strong> C atoms surrounding the central atom (e.g., N) <strong>of</strong> aquaternary salt will increase its lipophilicity, thus raising the extraction constant.However, these researchers did not give the relationship between the extraction constant<strong>and</strong> the structure <strong>of</strong> quaternary salts. According to the literature, four relationships forquaternary cations have been reported.1. Gustavii [101] observed a linear relationship between log E QX <strong>and</strong> n, the number<strong>of</strong> C atoms in an ammonium ion. He extracted picrates into methylene chloride usingprimary amines as well as symmetrical secondary <strong>and</strong> tertiary amines <strong>and</strong> symmetricalquaternary ammonium salts. The relationships for quaternary ammonium salts islog E Q picrate ¼ 2:0 þ 0:54n.Copyright © 2003 by Taylor & Francis Group, LLC