Distribution of Ag(I), Li(I)-Cs(I) Picrates, and Na(I) Tetraphenylborate with Differences in Phase Volume between Water and Diluents

Ionic strength conditions in distribution experiments with single ions are very important for evaluating their distribution properties. Distribution experiments of picrates (MPic) with M = Ag(I) and Li(I)-Cs(I) into o-dichlorobenzene ( oDCBz) were performed at 298 K by changing volume ratios ( V_org/V) between water and oDCBz phases, where “org” shows an organic phase. Simultaneously, an analytic equation with the V_org/V variation was derived in order to analyze such distribution systems. Additionally, the AgPic distribution into nitrobenzene (NB), dichloromethane, and 1,2-dichloroethene (DCE) and the NaB(C ₆H ₅) ₄ (=NaBPh ₄) one into NB and DCE were studied at 298 K under the conditions of various V_org/V values. So, extraction constants ( K _ex) for MPic into the org phases, their ion-pair formation constants ( K _MA,org) for MA = MPic in the org ones, and standard distribution constants ( ) for the M(I) transfers between the water and org bulk phases with M = Ag and Li-Cs were determined at the distribution equilibrium potential (dep) of zero V between the bulk phases and also the K _ex (NaA), K _NaA,org, and values were done at A ^-=BPh ^- ₄ . Here, the symbols K _ex, K _MA,org, and or were defined as [MA] _org/[M ⁺][A ^-], [MA] _org/[M+] _org [A ^-] _org, and [M ⁺] _org/[M+] or [A ^-] _org/[A ^-] at dep = 0, respectively. Especially, the ionic strength dependences of K _ex and K _MPic,org were examined at M = Li(I)-K(I) and org = oDCBz. From above, the conditional distribution constants, K _D,BPh4 and K _D,Cs, were classified by checking the experimental conditions of the I, I _org, and dep values.

• Standard Distribution Constants
• Volume Ratios
• Distribution Equilibrium Potentials
• Ionic Strength Dependence
• Extraction Constant
• Ion-Pair Formation Constant
• <i>o</i>-Dichlorobenzene

1. Introduction

In electrochemistry at liquid/liquid interfaces, such as water/nitrobenzene (w/NB) and w/1,2-dichloroethane (w/DCE) ones, formal potentials ( dep j 0 ′ ) for the transfer of single ions j across the interfaces have been determined [1] [2]. These potentials have been obtained at 298 K from standardized potentials of cations or anions based on the extra-thermodynamic assumption for the distribution of tetraphenylarsonium tetraphenylborate ( Ph 4 As + BPh 4 − ) and so on [1] [2] [3] in many cases. In these studies, there are many data for the potentials dep j 0 ′ in the w/NB and w/DCE systems [1] [2] [3] [4], while there are some data [5] [6] for w/o-dichlorobenzene (oDCBz) one. Especially, the data [6] for the metal ions (M^z+ at z = 1) seems to be very few. Also, the dep j 0 ′ values have been converted with the relation, dep j 0 ′ = − ( 1 / z j f ) ln K D , j S [7] [8], at dep = 0 V into standard distribution constants ( K D , j S ) of j in a mol/L unit. Here, the symbols, z_j, f, and dep, denote a formal charge of j with its sign, F/RT (these symbols are usual meanings), and a distribution equilibrium potential between w and organic (org) bulk phases, respectively. That is, the relation of dep M 0 ′ = − ( 0.0 5916 ) log K D , M S {or dep + 0 ′ = − ( 0.0 5916 ) log K D , + S } with j = M⁺ holds at dep = 0 V and T = 298.1₅ K. Generally such K D , j S values have been determined by solvent extraction experiments with j = M⁺, M²⁺, univalent cation, and its anion (A⁻) [3] [7] [8] [9] [10]. However, there are few studies [7] [10] for understanding distribution and extraction phenomena based on the dep values. So, it is expected that the above studies facilitate both an electrochemical understanding of the distribution and extraction phenomena and an extraction-chemical one of the ion transfers across the liquid/liquid interfaces.

In this study, we determined the standard distribution constants, K D , j S , at dep = 0 V and T ≈ 298 K for j = Ag⁺, Li⁺-Cs⁺, and BPh 4 − into some diluents. The K D , Ag S values were obtained from NB, DCE, oDCBz, and dichloromethane (DCM) systems with the reported K D , Pic S value [5] [8] [11] of picrate ion (Pic⁻), the K D , j S values at j = Li⁺-Cs⁺ from oDCBz one with that [5] of Pic⁻, and the K D , BPh4 S values from NB and DCE ones with the K D , Na S value [8] of Na⁺. In the experiments corresponding to the above systems, volume ratios (=V_org/V = r_org/w) of the both phases were changed and accordingly an equation for analyzing such systems was derived; V_org and V refer to an experimental volume (L unit) of the org phase and that of the w one, respectively. Also, the K_ex, K_MA,org, and K_D,MA values were obtained at 298 K from the same combinations of M⁺A⁻ and the diluents. Here, the symbols K_ex, K_MA,org, and K_D,MA were defined as [MA]_org/[M⁺][A⁻], [MA]_org/[M⁺]_org[A⁻]_org, and [MA]_org/[MA], respectively. Moreover, extraction, ion-pair formation, and distribution properties for the above systems were discussed based on their equilibrium constants. Additionally, using the Davies equation or the Debye-Hückel limiting law [12], dependences of K_ex and K_MPic,org (M = Li-K) on the ionic strength of both w and oDCBz (=org) phases were examined. About the distribution with BPh 4 − or Cs⁺, differences among its K D , BPh 4 or K_D,Cs values were considered in their experimental conditions and thereby classified into two groups, such as K_D,j and K D , j S .

2. Experimental

2.1. Chemicals

The procedures for the preparation of MPic, except for NaPic, were the same as those [13] [14] reported before. Commercial NaPic (monohydrate, extra pure reagent: ≥95.0%, Kanto Chemical) and NaBPh₄ {guaranteed pure reagent (GR): ≥95.0%, Kanto} were dissolved into pure water and then recrystallized by concentrating their aqueous solutions with a rotary evaporator. The thus-obtained crystals were filtered and then dried for > 20 h in vacuum. Amounts of the water of crystallization in these picrates were determined with a Karl-Fischer titration: 7.34₃% for M(I) = Li; 6.23₂ for Na; 1.23₀ for K; 2.76₇ for Rb; 0.414 for Cs. Water was not detected for the AgPic crystal [14].

Commercial NB (GR: > 99.5%, Kanto), DCE (GR: > 99.5%, Kanto), oDCBz (GR: > 99.0%, Kanto), and DCM (GR: > 99.5%, Kanto), used as the diluents, were washed three times with pure water and kept at states saturated with water until use [15]. Commercial nitric acid (GR: 60% - 61%, Wako Pure Chemical Industries) and hydrochloric acid (for amino acid analysis, GR: 35.0% - 37.0%, Kanto) were employed for the preparation of the calibration curves with AgNO₃ (GR: ≥ 99.8%, Kanto) and LiCl-CsCl (GR, Kanto, Wako, & Nacalai Tesque). Used pure water was purified by the same procedure as that [15] reported previously.

2.2. Experiments for the MPic and NaBPh 4 Distribution

Aqueous solutions of MPic or NaBPh₄ were mixed with some diluents in the various r_org/w (see Table 1 & Table 2 for their ratios) in stoppered glass tubes of about 30 mL and then they were shaken for 3 minutes (in the experiments with the AgPic and NaBPh₄ distribution) or one minute (in those with the LiP-ic-CsPic one) by hand. After this operation, these tubes were mechanically agitated at 25˚C ± 0.3˚C for 2 h and centrifuged for 5 minutes in order to separate the two phases. The separated diluent phases were taken into the glass tubes and treated as follows. The diluent phases of AgPic, NaPic, and NaBPh₄ distribution systems were back-extracted by using 0.1 mol/L HNO₃, pure water, and 0.02 mol/L HCl, respectively. For the NaPic system, the w phases back-extracted were separated, transferred to 5 mL tubes produced by polypropylene, and then their separated phases were diluted with the HCl solution. Total amounts of Ag(I) and Na(I) in these aqueous solutions were analyzed at 328.1 nm for Ag and 589.0 for Na with a Hitachi atomic absorption spectrometer (type Z-6100). In addition to

Table 1

Fundamental data for AgPic and NaBPh 4 distribution into several diluents at 298 K with various r org /w conditions

MA	Diluent (org)	logKD,±a	depb/V	log( K D , Ag S or K D , BPh 4 S % )
AgPic	NB at rorg/w = 1	−2.12 ± 0.03	0.13	−4.30a,e
	DCE at rorg/w = 1d	−3.74	0.16	−6.47a,e
	DCE at rorg/w = 0.12 - 8.3	−3.85 ± 0.16	0.17	−6.69 ± 0.22a,e
	oDCBz at rorg/w = 1.2 - 20	−4.52 ± 0.07	0.11f	−6.30e,g
	DCM at rorg/w = 1.0 - 27	−3.95 ± 0.15	0.19	−7.23 ± 0.15e
NaBPh4	NB at rorg/w = 0.50 - 7.5	−0.50 ± 0.21	0.36	4.2 ± 0.2a,h,i
	DCE at rorg/w = 1.0 - 8.0	−3.74 ± 0.28	0.14	−1.4 ± 0.3a,h,i
I/mol·L−1	logKex	logKD,MA	Iorgc/mol·L−1	logKMA,org
0.022	−0.46 ± 0.03	−0.79 ± 0.05	1.6 × 10−4	3.79 ± 0.05
0.020e	−1.49	−1.83f	3.6 × 10−6e	5.992
0.023	−1.02 ± 0.39	−1.35 ± 0.39	3.2 × 10−6	6.3 ± 0.4
0.043	−2.52 ± 0.37	−2.81 ± 0.37	1.3 × 10−6	6.5 ± 0.4
0.044	−1.58 ± 0.28	−1.86 ± 0.28	4.9 × 10−6	6.3 ± 0.4
0.00025	3.90 ± 0.27	2.76 ± 0.27	8.0 × 10−5	4.9 ± 0.4
0.019	−0.71 ± 0.37	−1.76 ± 0.37	3.4 × 10−6	6.8 ± 0.8

^aValues at I & I_org → 0. ^bValues calculated from Equation (3a). See the footnotes e & h for the log K D , Pic S & log K D , Na S % values. ^cAverage values. ^dRef. [14]. ^eValues calculated from log K D , Pic S = 0.0 5 at I & I_NB → 0; −1.01₁ at I & I_DCE → 0; −2.73₇ at [Li₂SO₄]_t = 0.0035 mol/L, [PNP⁺DCC⁻]_t,oDCBz = 0.01, & 295 K; −0.68 for the w/DCM system. See refs. [5], [8], & [11] & Appendix B. ^fValues calculated from the original data of ref. [14]. ^gValues determined at 295 - 298 K, where log K D , Ag S corresponds log K D , Ag S % . See the text & Equation (T8) in Table 3 for the log K D , Ag S % estimation. ^hCalculated from log K D , Na S % = − 5 . 18 for w/NB; −6.09 for w/DCE. See ref. [8]. ⁱThe maximum values among errors used for calculation were described.

Table 2

Fundamental data for MPic (M = Li-Cs) distribution into org = oDCBz at 298 K with various I and r org /w conditions

M	I/mol·L−1 (rorg/w range)	logKD,±a	depb,c/V	log K D , M S % c,d	logKex	logKD,MPic	Iorge/mol·L−1	logKMPic,org
Li	0.026 (1.0 - 4.0)	−5.53 ± 0.61	0.17	−8.32 ± 0.61	−3.15 ± 0.24	−4.4	7.6 × 10−8	7.9 ± 0.9
	0.058 (1.0 - 3.0)	−5.44 ± 0.28	0.16	−8.14 ± 0.28	−3.59 ± 0.17	−4.5	2.1 × 10−7	7.3 ± 0.4
	0.070 (1.0)	−6.0 ± 2.3	0.2	−9.2 ± 2.3	−4.19 ± 0.55	−5.1	7.6 × 10−8	7.7 ± 2.4
	0.082 (2.0 - 4.1)	−5.3f	0.15	−7.86 ± 0.39	−3.87 ± 0.09	−4.7	4.1 × 10−7	6.7 ± 0.6
	0.082 (1.0 - 2.9)	−6.2 ± 1.2	0.2	−9.7 ± 1.2	−4.02 ± 0.14	−4.9	4.7 × 10−8	8.5 ± 1.7
Na	0.038 (1.0 - 7.5)	−4.91 ± 0.57	0.13	−7.09 ± 0.57	−2.14 ± 0.32	−2.6	4.6 × 10−7	7.7 ± 0.9
	0.049 (6.0 - 12)	−3.71 ± 0.01	0.057	−4.68	−1.85 ± 0.12	−2.3	9.6 × 10−6	5.6 ± 0.1
	0.070 (1.0 - 12)	−5.10 ± 0.41	0.14	−7.45 ± 0.41	−2.64 ± 0.39	−3.1	5.6 × 10−7	7.5 ± 0.7
	0.090 (4.0 - 15)	−4.8f	0.12	−6.90 ± 0.46	−2.52 ± 0.20	−2.9	1.4 × 10−6	7.1 ± 0.7
	0.11 (1.2 - 6.0)	−5.06 ± 0.83	0.14	−7.38 ± 0.83	−3.01 ± 0.28	−3.4	9.2 × 10−7	7.1 ± 1.2
	0.13 (1.0 - 12)	−5.44 ± 0.74	0.16	−8.14 ± 0.74	−3.08 ± 0.34	−3.5	4.6 × 10−7	7.8 ± 1.1
K	0.0017 (1.5 - 3.0)	−2.6 ± 1.0	−0.01	−2.5 ± 1.0	0.56 ± 0.12	−0.5	3.8 × 10−6	5.8 ± 1.4
	0.0040 (1.5 - 6.0)	−3.49 ± 0.22	0.043	−4.25 ± 0.22	−0.55 ± 0.23	−1.3	1.3 × 10−6	6.4 ± 0.4
	0.0078 (1.0 - 3.0)	−3.76 ± 0.31	0.060	−4.78 ± 0.31	−1.37 ± 0.18	−2.1	1.4 × 10−6	6.1 ± 0.5
	0.020 (1.2 - 4.0)	−3.9f	0.071	−5.10 ± 0.39	−1.67 ± 0.20	−2.3	2.5 × 10−6	6.2 ± 0.6
Rb	0.0047 (1.7 - 6.0)	−4.62 ± 0.80	0.11	−6.50 ± 0.80	−1.62 ± 0.19	−3.4	1.1 × 10−7	7.6 ± 1.1
	0.0071 (2.0 - 7.5)	−5.3 ± 1.2	0.2	−7.9 ± 1.2	−1.84 ± 0.20	−3.6	3.2 × 10−8	8.8 ± 1.7
Cs	0.0032 (1.1 - 12)	−4.22 ± 0.16	0.14	−6.63 ± 0.19	−1.01 ± 0.30	−3.0	2.0 × 10−7	7.4 ± 0.4
	0.0032 (1.0 - 12)	−4.69 ± 0.19	0.060	−5.69 ± 0.16	−1.52 ± 0.40	−3.5	6.7 × 10−8	7.9 ± 0.5

^aValues at I & I_oDCBz → 0. ^bValues calculated from log K D , Pic S % = − 2 . 73 7 at [Li₂SO₄]_t = 0.0035 mol/L, [PNP⁺DCC⁻]_t,org = 0.01, & 295 K using Equation (3a). See ref. [5]. ^cValues determined at 295 - 298 K. ^dValues expressed as the errors which equal those of logK_D,±. See the text. ^eAverage values. ^fRef. [17].

589.0 for Na, amounts of the other M(I) were analyzed at 670.8 nm for M(I) = Li, 766.5 for K, 780.0 for Rb, and 852.1 for Cs by a flame spectrophotometry.

Total concentrations of MPic in the w phases before the distribution experiments into oDCBz were as follows: 0.025 & 0.052 mol/L for the AgPic distribution, 0.026 - 0.034, 0.083, 0.094 - 0.12, & 0.13 - 0.14 for LiPic, 0.042, 0.056, 0.084, 0.11, 0.13, & 0.17 for NaPic, 0.0017, 0.0040, 0.0081, & 0.022 for KPic, 0.0061 & 0.010 for RbPic, and 0.0043 for CsPic. In the AgPic distribution into other org phases, the total concentrations were 1.0 × 10⁻⁴-0.041 mol/L for org = NB, 0.012 - 0.030 for DCE, and 0.025, 0.040, & 0.049 for DCM. In the NaBPh₄ distribution into NB and DCE, the concentrations were 4.9 × 10⁻⁵-0.0061 mol/L and 0.0040 - 0.035, respectively.

2.3. Data Analyses

Based on the ion-pair formation, M + + A − ⇌ MA , in water, we can easily propose a quadratic equation K MA [ M + ] V 2 + [ M + ] V − [ M ] t , w = 0 {see Equation (1) for the symbols ^V[M⁺] & [M]_t,w} and then obtain from it

[ M + ] V = [ A − ] V = { ( 1 + 4 K MA [ M ] t , w ) 1 / 2 − 1 } / 2 K MA . From the latter equation,

we calculated self-consistent ^V[A⁻] and K_MA values by a successive approximation with log K MA = log K MA 0 + 2 log y ± [8]. Here, the symbols, K_MA, K MA 0 , and y_±, denote an ion-pair formation constant for MA in water at concentration expression, that at ^V[A⁻] (= ionic strength) → 0 mol/L, and a mean activity coefficient for M⁺ and A⁻ in water, respectively.

3. Results and Discussion

3.1. Derivation of Analytic Equation under the Conditions of Different Phase Volumes

Under the condition that V_org is different from V in the MA distribution into the org phase, we considered the following equation as a total mass balance at mol unit:

[ M ] t V = [ M ] t , w V + [ M ] t , org V org , (1)

where [M]_t, [M]_t,w, and [M]_t,org denote a total concentration of the 1:1 electrolyte MA in the w phase before the extraction experiment, that of species with M(I) in the w one, and that of those in the org phase after the experiment (namely, at equilibrium), respectively. In these concentrations, the [M⁺]_t,org value can be experimentally determined with some analytical methods, such as AAS, flame spectrophotometry, and potentiometry with ISE. Equation (1) was divided by ^V[M⁺]V and then rearranged into

r org / w [ M ] t , org / [ M + ] V = ( [ M ] t − [ M ] t , w ) / [ M + ] V = r org / w ( [ M + ] org + [ MA ] org ) / [ M + ] V , (2)

using the mass balance relation of [M]_t,org = [M⁺]_org + [MA]_org in the org phase. Here, the symbols, ^V[M⁺] and r_org/w[M⁺]_org, show the concentration of M⁺ in the w phase of the volume V and that of M⁺ in the org phase of V, respectively. In other words, the [M⁺]_org value is converted with r_org/w into ^V[M⁺]_org, the concentration of M⁺ in the org phase of V: namely ^V[M⁺]_org equals r_org/w[M⁺]_org {= (V_org/V )[M⁺]_org}. Therefore, we can define r_org/w[M⁺]_org/^V[M⁺] (= ^V[M⁺]_org/^V[M⁺]) as a conditional distribution constant [7], K_D,M, of M⁺ and additionally do [MA]_org/^V[M⁺]^V[A⁻] as the apparent extraction constant, K ′ ex , of MA, respectively. Obviously. from the charge balance relations of [M⁺]_org = [A⁻]_org and ^V[M⁺] = ^V[A⁻] in the MA distribution system, we can see immediately that K_D,M = (r_org/w[M⁺]_org/^V[M⁺] =) r_org/w[A⁻]_org/^V[A⁻] = K_D,A.

According to our previous paper [7], the K_D,M and K_D,A values at 298 K have been expressed as

dep = ϕ − ϕ org = 0.0 5916 ( log K D , M − log K D , M S ) = − 0.0 5916 ( log K D , A − log K D , A S ) . (3)

Here, the symbols ϕ (or ϕ org ), K_D,M, and K_D,A denote an inner potential of the w (or org) phase, the conditional distribution constant of M⁺, and that of A⁻, respectively, in this equation; see the introduction for the symbols K D , M S and K D , A S . This dep practically means a total energy which is necessary for the M⁺ or A⁻ transfer across the interface between the two bulk phases at equilibrium. Equation (3) is the modified form of the Nernst equation [16]; this expression has a little problem in its definition (see ref. [17]). As similar to Equation (3), the following equation can hold (see Appendix A for its derivation).

dep = dep ± = 0.0 5916 ( log K D , ± − log K D , M S ) = − 0.0 5916 ( log K D , ± − log K D , A S ) (3a)

So from rearranging Equation (2) with K D , ± 2 which is defined as K D , M S K D , A S {=K_D,MK_D,A: the condition (C3) in Appendix A}, the following equation was obtained.

r org / w [ M ] t , org / V [ M + ] = r org / w D M expl . = K D , M + K ′ ex r org / w [ A − ] V = K D , ± + K ′ ex r org / w [ A − ] V (4)

under the conditions of K_D,M = K_D,A (see above) and K D , M S ≠ K D , A S . Here r org / w D M expl . equals an experimental (expl.) value, ^V[M]_t,org/^V[M⁺], corresponding to the distribution ratio of M(I) [8]. Hence, the plot of r org / w D M expl . versus r org / w [ A − ] V based on Equation (4) can give K ′ ex as the slope and K_D,± as the intercept. Interestingly, we can obtain the plot with changing r_org/w under the constant condition of ^V[A⁻], namely, the constant ionic strength (I) in the w phases. Here, we can see that the intercept is the K_D,± value under the condition of I (=^V[A⁻] = ^V[A⁻]_org/K_D,±) → 0 [8] at least, because of r_org/w > 0. When K_D,± > 0, this fact, I = ^V[A⁻]_org/K_D,± → 0, also means ^V[A⁻]_org (= I_org) → 0 [8]. Therefore, the intercept, K_D,±, satisfies both the conditions of I and I_org → 0. Equation (4) is essentially similar to the Czapkiewicz equation [18] with P^1/2 (≈K_D,±) at C_II ( = r org / w [ A − ] V or ^V[A⁻]) → 0 and P^* (≈K_ex).

The symbol K ′ ex is converted with r_org/w into K ex ( = r org / w K ′ ex ) which is thermodynamically expressed as ( K D , ± ) 2 K MA , org = K D , M K D , A K MA , org = K D , M S K D , A S K MA , org (see the introduction for K_MA,org). Accordingly, we can obtain the K_MA,org value from the intercept and the modified slope based on Equation (4). In the relation of ( K D , ± ) 2 = K D , M K D , A = K D , M S K D , A S , the K_D,M and K_D,A values must satisfy the same experimental conditions, such as I and I_org, and also K D , A S and K D , M S ones do the same condition.

3.2. Reproducibility of the Experimental Values in Equation (4)

Figure 1 shows an example of the AgPic extraction into DCE. The straight line was r DCE / w D Ag expl . = ( 1.4 0 ± 0.5 1 ) × 10 − 4 + ( 0.0366 ± 0.0007 ) × r DCE / w [ Pic − ] V at correlation coefficient (R ) = 0.997. From these intercept and slope, the logK_D,± value was evaluated to be −3.8₅ ± 0.1₆, while the logK_ex one was to be −1.0₂ ± 0.3₉. In the latter K_ex evaluation, the K_ex values were obtained from K ex = r DCE / w K ′ ex for given r_DCE/w values and then their values were averaged. Additionally, the log K D , Ag S and log K_AgPic,DCE values were calculated to be −6.6₉ ( = 2 log K D , ± − log K D , Pic S ) with the calculation error of ±0.2₂ and 6.3 (= logK_ex − logK_D,±) with that of ±0.4 at I_DCE = 3.2 × 10⁻⁶ mol/L, respectively. Here, I_DCE (or I_org) refers to the ionic strength in the DCE (or org) phase. These values were in agreement with those [14] at r_DCE/w = 1 reported before within their experimental errors, except for the logK_ex and logK_D,AgPic values. About these two constants, the minimum logK_ex value (= −1.4₁) was close to that (= −1.49 [14]) reported before and also the minimum logK_D,AgPic value (= −1.7₄) was somewhat larger than the

calculated one (= −1.83): see Table 1. The deviation of the latter value (=logK_ex − logK_AgPic, see the section 3.4 for K_AgPic) can depend on the error of logK_ex. Table 1 lists the results for the AgPic and NaBPh₄ distribution into several diluents and Table 2 does results for the LiPic-CsPic distribution into oDCBz.

In the relation of 2 log K D , ± = log ( K D , M S K D , A S ) , the pair of the K D , M S and K D , A S values must satisfy the same experimental conditions. In other words, the use of log K D , Ag S = 2 log K D , ± − log K D , Pic S basically reflects the experimental conditions of K D , Pic S in the K D , Ag S estimation. The same is also true of log K D , Ag = 2 log K D , ± − log K D , Pic .

3.3. Comparable Validity of Equation (4)

For K_D,± and K_ex determination, another simple analytic equation was derived from Equation (4) as follows.

D M expl . = K D , ± / r org / w + K ′ ex [ A − ] V . (5)

As examples, these common logarithmic K_D,± and K_ex values for the AgPic distribution into DCE were −3.2₃ ± 0.3₈ and −1.0₂ ± 0.3₈, respectively. From these values, the log K D , Ag S and logK_AgPic,DCE values were also estimated to be −5.4₅ ± 0.5₃ and 5.4 ± 0.7 at I_DCE = 3.2 × 10⁻⁶ mol/L, respectively. However, except for the logK_ex and logK_AgPic,DCE values, their values were in less agreement with those [14] (see Table 1) reported before, compared with the values determined in terms of Equation (4).

The form of Equation (5) was simpler than that of Equation (4). Although the difference in reproducibility between the two equations was few, we did not adopt here Equation (5) for the K_D,± and K_ex determination. Also, the plot of r org / w D M expl . versus ^V[A⁻] based on Equation (4) was not able to give the straight line, indicating that the K ′ ex r org / w (=K_ex) term in the plot is not the constant. This fact shows that the parameter r org / w [ A − ] V is more important than the K ′ ex r org / w one in Equation (4). Simultaneously, both the plots lose the advantage of the constant I (=^V[A⁻]) condition in the experiments. On the basis of the above results, we employed here Equation (4) for the determination of the K_D,± and K_ex values.

3.4. On Features of the AgPic Distribution Systems

Table 1 showed the order of org = NB > DCE ≥ DCM > oDCBz for the K_D,± values at I and I_org → 0 mol/L, that for K_ex in the I range of 0.020 to 0.044, and that for K_D,AgPic. Here, the K_D,AgPic value was calculated from the thermodynamic relation of K_D,AgPic = K_ex/K_AgPic with K_AgPic = [AgPic]/[Ag⁺][Pic⁻], which was evaluated from the K AgPic 0 value (=2.8 L/mol [19]) reported at I → 0 and 298 K. On the other hand, the K_AgPic,org values showed the reverse order: org = NB < DCE ≤ DCM ≤ oDCBz in the I_org range of 1.3 × 10⁻⁶ to 1.6 × 10⁻⁴ mol/L (Table 1). These orders seem to reflect polarities of the diluents, except for K_D,AfPic. Also, the K D , Ag S values were in the order NB > oDCBz ≥ DCE > DCM (see Table 1), although the value for the oDCBz system was calculated from K D , Pic S [5] reported at T = 295 ± 3 K and K_D,± obtained here at 298 K. Moreover, it was assumed that the logK_D,Pic values for the oDCBz and DCM systems satisfy the conditions of I and I_org → 0 and dep = 0; for the former system, that of I and I_org → 0 or an activity expression was cleared as described in Appendix B.

Considering the experimental errors of K_D,± (or K D , M S ) in Table 2, except for the oDCBz system of Table 1, we can suppose that the differences in K D , M S between T = 295 ± 3 [5] and 298 K are negligible. However, the K D , Pic S determination at 298 K will be necessary for the determination of the more-exact K D , M S values.

3.5. l o g K D , M S % Estimation

We derived the following equation from the definition of K D , M S % = y + , org K D , M S / y + for the present distribution systems at dep = 0 V, the individual activity coefficients y_+,org (=y_M,org), and y₊ (=y_M) and rearranged it.

log K D , M S = log ( y + K D , M S % / y + , org ) = log K D , M S % − A z j 2 f ( I ) + A org z j 2 ( I org ) 1 / 2 (6)

Here, the symbol, K D , M S % , denotes a thermodynamic equilibrium constant (=a_M,org/a_M in activity unit) of K_D,M at I_org and I → 0 mol/L and the superscripts, S and %, mean the experimental conditions of dep = 0 V and the ionic strength for the both phases, respectively. As the description of the superscript % (or u_t//x_t), its numerator shows the condition of I_org → 0 (or the left hand side of // does the total concentration, u_t, of an electrolyte in the org phase), while its denominator does that of I → 0 (or its right hand side does the total one x_t in the w phase). According to Equation (6) at dep = 0 V, K D , M S ( = K D , M S u / x ) equals [M⁺]_org/[M⁺] as the concentration expression for a given I = x or I_org = u, K D , M S u / 0 does [M⁺]_org/a_M for a given I_org = u, and K D , M S 0 / x does a_M,org/[M⁺] for a given I = x; the latter two equations are both the semi-activity expressions (see the footnotes b, d-f in Table 3).

Assuming that log K D , Pic % reported cyclic-volammetrically for the w/oDCBz system [5] satisfies the condition of dep = 0 V, the log K D , M S % values were calculated from its log K D , Pic % value (= −2.73₇, see Appendix B for the calculation) with 2 log K D , ± % = log K D , M % K D , A % at dep = 0 V. From the data in Table 2, the logarithmic values of the average K D , M S % , which was calculated from the intercepts, K D , ± % (for example see Figure 2), can be estimated easily. These log K D , M S % values were −8.3₄ ± 0.4₁ for M = Li, −5.4₅ ± 0.9₆ for Na, −3.1₃ ± 0.7₂ for K, −6.7₈ for Rb, and −5.9₅ for Cs. Here, the errors corresponding to log K_D,± were approximately employed as the errors of log K D , M S % , because of a lack [5] of the log K D , Pic S % ’s error (see Table 1 & Table 2). The K D , M S % values were in the order M = Li < Na < K > Rb < Cs. This order is the same as that of the distribution with the neutral MPic. The log K_D,MPic order was M = Li (log K_D,MPic,av = −4.6 ± 0.2) < Na (−2.8 ± 0.4) < K (−1.0 ± 0.6) ≫ Rb (−3.5) < Cs (−3.2) (see Table 2). Here the symbol K_D,MPic,av refers to the average value of K_D,MPic. These orders for

Table 3

Various equations of experimental logK D,j based on some conditions

Equation no	Unknown or known conditionsa			Symbol for KD,j	Equations
	I/mol·L−1	Iorg/mol·L−1	dep/V
T1 or 10	x	u	v	KD,jb or K D , j u / x b	log K D , j = log K D , j S % + ( f / 2 . 3 0 3 ) z j v − A z j 2 f ( x ) + A org z j 2 ( u ) 1 / 2 c
T2 or 6	x	u	0	K D , j S or K D , j S u / x	log K D , j = log K D , j S % − A z j 2 f ( x ) + A org z j 2 ( u ) 1 / 2
T3	x	0 or u1	v	K D , j 0 / x d	log K D , j = log K D , j S % + ( f / 2 . 3 0 3 ) z j v − A z j 2 f ( x ) or log K D , j 0 / x = log K D , j − A org z j 2 ( 0   or   u 1 ) 1 / 2
T4	0 or x1	u	v	K D , j u / 0 e	log K D , j = log K D , j S % + ( f / 2 . 3 0 3 ) z j v + A org z j 2 ( u ) 1 / 2 or log K D , j u / 0 = log K D , j + A z j 2 f ( 0   or   x 1 )
T5	x	0 or u1	0	K D , j S 0 / x	log K D , j = log K D , j S % − A z j 2 f ( x ) or log K D , j S 0 / x = log K D , j − A org z j 2 ( 0   or   u 1 ) 1 / 2
T6	0 or x1	u	0	K D , j S u / 0	log K D , j = log K D , j S % + A org z j 2 ( u ) 1 / 2 or log K D , j S u / 0 = log K D , j + A z j 2 f ( 0   or   x 1 )
T7	0 or x1	0 or u1	v	K D , j % f	log K D , j = log K D , j S % + ( f / 2 . 3 0 3 ) z j v or log K D , j % = log K D , j + A z j 2 f ( 0   or   x 1 ) − A org z j 2 ( 0   or   u 1 ) 1 / 2
T8	0 or x1	0 or u1	0	K D , j S %	log K D , j = log K D , j S % g or log K D , j S % = log K D , j + A z j 2 f ( 0   or   x 1 ) − A org z j 2 ( 0   or   u 1 ) 1 / 2

^aThe parameters x, u, & v show unknown values & zero, u₁, & x₁ do the known ones. ^{b K D , j = K D , j u / x = [ j ] org / [ j ]} . ^cBasic equation. ^{d K D , j 0 / x = a j , org / [ j ]} . K D , j u / 0 = [ j ] org / a j . ^{f K D , j % = a j , org / a j} . ^gDefined as K D , j S % = a j , org / a j at dep = 0 V.

M = Li-K are in agreement with those for the MPic distribution into NB [3,8] and DCE; that is, the order increases in going from M = Li to K (monotonically to Cs). The data of log K D , M S % for the MPic distribution into DCE at 298 K were −8.07 for M = Li, −6.0₉ for Na, and −5.9₅ for K (−5.37 for Rb & −4.6₀ for Cs), reported by one (Y. K.) of the authors in Chemistry Journal, 2013, vol. 3, pp. 37-43 (now this journal has not been open access). Further experiments will be needed for the RbPic and CsPic distribution into oDCBz. Similarly, the log K D , Ag S % value for the oDCBz system was estimated to be −6.30 (see Table 1) from the relation log K D , Ag S % = 2 log K D , ± − log K D , Pic S % .

From Table 2, the maximum logy₊ and logy_+,org values at org = oDCBz were calculated to be −0.02 {= −0.5114f(0.0017)} and 0.00 {= −(11.3)(3.2 × 10⁻⁸)^1/2}, respectively. On the other hand, their minimum values were done to be −0.11 from I = 0.13 mol/L and −0.03 from I_org = 9.6 × 10⁻⁶, respectively. These results indicate that, as a measure, the predicted changes of log K_D,M due to I and I_oDCBz are less than about 0.1 {= |log[y₊(min.)/y_+,org(max.)]|}. In other words, this suggests the larger dep dependence of logK_D,M (or logK_D,A), compared with its I and I_org dependences. The suggestion is supported by the following results. The many dep values, except for KPic distribution at I = 0.0017 mol/L, were present in the range of 0.057 to 0.2 V in Table 2. The |dep/0.05916| terms {see Equations (7) & (10)} at 298 K corresponding to log y were calculated to be 0.96 to 3.₃. At least, the deviation of about 0.1 in log(y₊/y_+,oDCBz) seems to be effective for deviations in the NB and DCE distribution systems.

3.6. Correlation between logK ex and Dep or l o g K D , M S

Figure 3 shows a plot of logK_ex versus dep (see Table 2 & Appendix B) for the MPic distribution with M = Li-Cs and Ag into oDCBz. A regression line was logK_ex = (0.0₆ ± 0.3₀) − (19.₇ ± 2.₃) dep at R = 0.899 without the AgPic system (see the full circle in Figure 3 & Table 1). Thus we can see that the logK_ex values decrease with an increase in the dep values. Also, this fact suggests that the dep values are barriers to the distribution or extraction of M⁺ with Pic⁻ (or Pic⁻ with M⁺) into oDCBz. On the other hand, according to the K_ex definition by the thermodynamic cycle, logK_ex is expressed as log (K_D,MK_D,AK_MA,org). Introducing Equation (3) in this cycle, we immediately obtain

log K ex = − dep / 0.0 5916 + log ( K D , M K D , A S K MA , org ) = − 16 . 9 0 dep + log ( K D , M K D , A S K MA , org ) (7)

at T = 298 K. Comparing this equation with the experimental regression line, one can suppose that the experimental slope of −20 V⁻¹ is close to the theoretical one of −17 at 298 (& 295) K. In addition to this fact, the logarithmic values of average K D , M S % and K_MPic,org were −3.₈ ± 1.₈ and 7.8₉ ± 0.8₉, respectively, and log K D , Pic S % was −2.73₇ (see Appendix B) for org = oDCBz at 295 K. A sum of the three values became +1.₃ ± 2.₀ (the approximate value calculated without the error of log K D , Pic S % ). The estimated log ( K D , M S % K DD , A , M S % K MA , org ) value was in accord

with the intercept (= 0.1) of the plot within both the errors, ±2 for the estimated value and ±0.3 for the intercept. These results indicate that the regression line is essentially based on Equation (7). Also, from the above, it can be seen that the dep term is included in log K_ex at least.

The same is also true of the plot of logK_ex versus log K D , M S % plot. This plot can come from the relation

log K ex = log ( y + K D , M S % / y + , org ) + log ( y − K D , A S % / y − , org ) + log K MA , org = log K D , M S % + log ( K D , A S % K MA , org ) + 2 log ( y ± / y ± , org ) . (7a)

Additionally, the symbols, y₋ and y_−,org, refer to the activity coefficients of A⁻ in the w and org phases, respectively; y_± and y_±,org show their mean activity ones. The corresponding regression line with the MPic system was log K ex = ( 0.62 ± 0.07 ) log K D , M S % + ( 1.9 1 ± 0.4 8 ) at R = 0.903. Unfortunately, the slope and intercept were smaller than unity and the log (the product between log K D , Pic S % and the average of K_MA,org) value of 5.2 (≈7.8₉ − 2.73₇) with the error of about ±0.9, respectively. While, the result obtained from the slope fixed at unity was log K ex = log K D , M S % + ( 4.4 8 ± 0.2 0 ) at R = 0.716. Considering 4.5 ≈ 5.2 + 2log(y_±/y_±,org), this improvement of the intercept suggests log(y_±/y_±,org) < 0. Similarly, from this result, it can be seen that the K D , M S % term is included in log K_ex.

3.7. On the I Dependence of logK ex

In this section, using the data in Table 2, we tried to examine a dependence of logK_ex on the I values at 298 K. In general, it is empirically known that the Davies equation [12] is effective for analyzing the I dependences of equilibrium constants in the I ranges of less than 1 mol/L. Defining K ex 0 as K_ex based on the activity expression, we can obtain

K ex 0 = a MA , org / a M a A = K ex / y + y − , (8)

where a_j denotes the activities of j = M⁺ and A⁻ in the w phase and a_MA,org does that of MA in the org phase, being equal to a molar concentration [MA]_org. Taking logarithms of both the sides of Equation (8) and then rearranging it, the following equation was obtained:

log K ex ≈ log K ex 0 − 2 A f ( I ) (8a)

with log y + y − = − 2 A f ( I ) (8b)

and f ( I ) ≈ I 1 / 2 / ( 1 + I 1 / 2 ) − 0.3 I . (8c)

Hence, a non-linear regression analysis of the plots of logK_ex versus I^1/2 can yield experimental log K ex 0 and A values.

Figure 4 shows an example of such plots. The regression line was logK_ex = (−1.5₄ ± 0.7₂) – 2 × (6.₂ ± 2.₀)f(I) at R = 0.875 for the LiPic distribution into oDCBz. Also, the lines for the NaPic and KPic distribution systems were logK_ex = (0.2₄ ± 0.7₄) – 2 ´ (7.₃ ± 1.₉)f(I ) at R = 0.885 and = (1.2₄ ± 0.6₇) – 2 ´ (13.₆ ± 4.₂)f(I ) at 0.916, respectively. These A values were 12- to 27-times larger than that {= 0.5114 (L/mol)^1/2} calculated for pure water at 298 K. The log K ex 0 values for the MPic distribution were in the order M = Li < Na ≤ K {>Rb ( log K ex , av 0 = − 1 . 6 5 ) < Cs (−1.1₄)}, where K ex , av 0 denotes the average of K ex 0 .

3.8. On the I org Dependence of logK MA,org

As similar to the I dependence of logK_ex, we considered K MA , org 0 based on an

activity ex pression as follows.

K MA , org 0 = [ MA ] org / a M , org a A , org = K MA , org / y + , org y − , org (9)

Taking logarithms of the both sides of this equation and then rearranging it, the following equation was obtained:

log K MA , org = log K MA , org 0 − 2 A org ( I org ) 1 / 2 (9a)

with − 2 A org ( I org ) 1 / 2 = log y + , org y − , org . (9b)

A plot of logK_MA,org versus I org 1 / 2 can give a straight line with the slope of –2A_org and the intercept of log K MA , org 0 .

Figure 5 shows an example of the NaPic distribution system with org = oDCBz. The broken line was the experimental regression one, log K NaPic , org = ( 8.1 6 ± 0.1 3 ) − 2 × ( 422 ± 43 ) ( I org ) 1 / 2 at R = 0.980. Similar results were obtained from the other two systems: log K LiPic , org = ( 8.9 8 ± 0.2 8 ) − 2 × ( 1819 ± 350 ) ( I org ) 1 / 2 at R = 0.949 and log K KPic , org = ( 6.8 8 ± 0.4 0 ) − 2 × ( 260 ± 134 ) ( I org ) 1 / 2 at 0.809. These A_org values were 23- to 161-times larger than that {=11.3 (L/mol)^1/2} calculated for pure oDCBz (= org) at 298 K. These results are similar to those of A_DCE for the AgPic extraction system with benzo-18-crown-6 ether into DCE [14]. The log K MPic , o DCBz 0 values at I_oDCBz → 0 were in the order M = Li > Na > K (≤ Rb ≈ Cs, see Table 2). This order recalls that (Li > Na ≤ K) of K MPic 0 [19] in water potentiometrically-determined at 298 K to us. The difference in order between Na (=M) and K may reflect that between the water and oDCBz phases in the hydration to M⁺.

3.9. On the Differences between K D , B P h 4 or K D,Cs Values in the NB, DCE, and oDCBz Systems

The log K D , BPh 4 S % values determined with the present experiments (see Table 1) were much smaller than the values reported from the distribution [3] [8] [18] and electrochemical experiments [20]. Their values have been reported to be 6.3 [3] at I = x and 5.6 [8] at I → 0 for the NB systems; 5.396 [20] at [MgSO₄]_t = 1 mol/L and [ CV + BPh 4 − ] t , DCE = 0.05 (CV⁺: crystal violet cation) and 6.13 [18] at I → 0 for the DCE ones. Their experimental log K D , BPh 4 S % values were obtained here to be 4.2 for NB and −1.4 for DCE (Table 1). These differences may be understood by the dep dependence of the log K D , BPh 4 values, as described in the Section 3.5.

Although numbers of the data sets of log K D , BPh 4 and I or I_org were few, Equation (6) employed for A⁻ has possibility for showing the I or I_org dependence of the log K D , BPh 4 values. So, using Equations (3) and (6), we can immediately derive the following basic equation:

log K D , j = log K D , j S % + ( f / 2 . 3 0 3 ) z j dep − A z j 2 f ( I ) + A org z j 2 ( I org ) 1 / 2 ≈ log K D , j S + ( f / 2 . 3 0 3 ) z j dep (10)

with j = M⁺, A⁻ and K D , j S % = y j , org K D , j S / y j ( = y j , org K D , j S u / x / y j ) . This expression can be an overall one about K_D,j = [j]_org/[j]. Table 3 summarizes variation of Equation (10) based on the conditions of I, I_org, and dep. These equations can be classified into two groups in whether the equation contains the dep term or not. So this difference can give the larger difference in logK_D,j between the two groups, such as Equations (10), (T3), (T4), and (T7) and Equations (6), (T5), (T6), and (T8). In particular, we can expect that differences in value among Equations (6), (T5), (T6), and (T8) are the smaller than those among Equations (10), (T3), (T4), and (T7), since log(y_j/y_j,org) ≈ ±0.1 and |dep/0.05916| = 1 to 3, as estimated above (the section 3.5).

Based on Equation (10) or (T1), we can handle the above data for the w/NB systems as follows. Using the relation 4 . 2 = log K D , j S % + ( f / 2.303 ) z j × 0 − A z j 2 f ( 0 ) + A NB z j 2 × 0 1 / 2 = log K D , j S % + 0 − 0 + 0 with A = 0.5114, b = 0.3, and A_NB = 1.725 at j = BPh 4 − , we immediately obtained log K D , j S % = 4 . 2 at z_j = −1. From 6.3 = 4.2 − ( f / 2.303 ) v − A f ( x ) + A NB u 1 / 2 , the –16.90v – Af(x) + A_NBu^1/2 term at 298 K was obtained to be 2.1 at z_j = −1. Also, using 5.6 + A f ( 0 ) = 4.2 − ( f / 2.303 ) v + A NB u 1 / 2 , the –(f/2.303)v + A_NBu^1/2 term equals 1.4 with 5 . 6 = log K D , BPh 4 u / 0 = 4.2 − 16.90 v + 1.725 u 1 / 2 . These cases suggest that the former of 6.3 is log K D , BPh 4 u / x {Equation (10) or (T1) in Table 3} and the latter of 5.6 is log K D , BPh 4 u / 0 {Equation (T4)}. Strictly speaking, it is difficult to compare 6.3 with 5.6.

Similarly, the relation − 1.4 = log K D , j S % + 0 − 0 + A DCE × 0 1 / 2 gave −1.4 as log K D , j S % with A_DCE = 10.63 at j = BPh 4 − . For 5.396 ( = log K D , BPh 4 0.0 5 / / 1 ) = − 1 . 4 − ( f / 2.303 ) v − A f ( 0.87 ) + A DCE × 0.00 86 1 / 2 , dep (= v) became −0.3₅ V with 5.396 + 0.5114f(0.87) − 10.63 × 0.0086^1/2 = 4.52₇ = −1.4 – 16.90v at b = 0.3 and 298 K: see Appendix C for the estimation of I = 0.86₇ and I_DCE = 0.0086. The absolute value of this dep was in good agreement with the E_I=0 value (=0.358 V) reported by the polarographic measurements at the w/DCE interface [20]. Moreover, from 6.13 = − 1.4 − ( f / 2.303 ) v − 0 + A DCE u 1 / 2 , the –(f/2.303)v + A_DCEu^1/2 term at 298 K became 7.5 with 6.13 + A f ( 0 ) = − 1.4 − 16.90 v + 10.63 u 1 / 2 . As similar to the w/NB results, the former of 5.396 + Af(0.87) − A_DCE × 0.0086^1/2 (= 4.53) is log K D , BPh 4 % {Equation (T7)} and the latter of 6.13 is log K D , BPh 4 u / 0 {Equation (T4)}. Therefore, we cannot directly compare 5.396 (or 4.53) with 6.13.

A half-wave potential for the Cs⁺ transfer across the w (1 mol/L MgSO₄)/ oDCBz(0.05 CVBPh₄) interface has been reported to be 0.12 V at 298 K [6]. It is well known that this value is generally close to the standard electrode potential (namely, its free energy) in electrochemical measurements. Reducing its value to logK_D,Cs, it corresponds to −2.03. So, using log K D , Cs S % = − 5.9 5 (see Section 3.5) based on the average value in Table 2, the following relation holds: − 2 .0 3 ( = log K D , Cs 0.0 5 / / 1 ) ≈ − 5 . 9 5 + ( f / 2.303 ) v − A f ( 0.87 ) + A o DCBz u 1 / 2 . Hence, the relation 16.90v + 11.3u^1/2 ≈ 4.0 was obtained with − 2.03 + A f ( 0. 87 ) = − 1.91 ≈ log K D , Cs u / 0 = − 5.9 5 + 16.90 v + 11.3 u 1 / 2 . Here, we were not able to estimate the dep and I_oDCBz values, because the K_MA,oDCBz value for MA = CV + BPh 4 − (the supporting electrolyte) in the oDCBz phase had not been found [6].

As another example, the log K D , Cs S % value has been reported to be −6.3₅ [21] for the CsPic distribution into DCE at 298 K. Similarly, the relation log K D , Cs + A f ( x ) − A DCE u 1 / 2 = − 6.3 5 = log K D , Cs % = − 4.6 0 + 16.90 v holds. So, we can estimate its dep (=v) value to be −0.1 V at 298 K. In these cases, the former of −2.03 + Af(0.87) is approximately log K D , C u / 0 {Equation (T4)} and the latter of −6.3₅ is log K D , Cs % {Equation (T7)}.

Thus, these results support the above understanding about the conditional K D , BPh 4 or K_D,Cs and self-consistently suggest that their values are functions [16] [22] containing dep, I, and I_org, that is, K D , BPh 4 = K D , BPh 4 S % ( y − / y − , org ) exp ( − f dep ) or K D , Cs = K D , Cs S % ( y + / y + , org ) exp ( f dep ) . Also, the condition of dep = 0 V gives K D , BPh 4 S = K D , BPh 4 S % ( y − / y − , org ) . From such an equation, we can see that the apparent I or I_org values, such as [supporting electrolyte]_t, [MA]_t, and [MA]_t,org, are not effective for estimating K D , A S (or K D , M S ), but their practical I or I_org values become more effective. This indicates that comparing such conditional K_D.A and K_D,M values is very difficult. Especially, it is very important for evaluating the K_D,BPh4 value, because BPh 4 − is the standard material in the dep j 0 ′ determination, as described in the introduction.

4. Conclusions

The logK_ex and logK_MA,org values were well expressed by Equation (8a) with I and Equation (9a) with I_org, respectively. Now, it is unclear why the experimental A and A_org values are much larger than their theoretical ones. Also, the MA distribution experiments based on the V_org/V variation provided us a procedure for the K D , M S or K D , A S determination under the constant condition of I, namely ^V[A⁻] = ^V[M⁺] = a constant value. So, in the single MA distribution, we could get the experimental procedure without the addition of any ionic strength conditioners (ISC) into the w phase. Besides, by introducing K D , M S % , K D , M S u / 0 , or K D , M S 0 / x in the K_D,M expression, a possibility for interpreting differences among various experimental values of K_D,M or K_D,A was shown with Equation (10). The effect of the activity coefficients terms for both the phases on the K D , A S % determination was smaller than that of the dep term at least. This result indicates that the log ( K D , A expl . 1 / K D , A expl .2 ) term is approximately proportional to the −(dep^expl.1 − dep^expl.2) one by using Equation (T7) for the same A⁻ and diluent. In comparing various experimental K_D,A or K_D,M values, readers need a suitable attention to the experimental concentrations of the salts, the supporting electrolytes, and ISC added in both phases. So, it is difficult to critically evaluate various K_D,M or K_D,A values without such a precise description of experimental conditions.

From the above, we propose a clear description of the I and I_org conditions in the distribution experiments at least. If possible, ion-pair formation or ion association data for the supporting electrolytes or ISC in the phases should be also added.

Conflicts of Interest

The authors declare no conflicts of interest regarding the publication of this paper.

Appendix A

We derived Equation (3a) as follows. First, the following reasonable conditions in the present distribution system were assumed for the derivation: (C1) dep₊ = dep₋, (C2) K_D,+ = K_D,−, and (C3) K D , ± 2 = K D , + K D , − .

(A) Derivation of a basic equation starting from (C1). Next, we obtained from Equation (3) the relation

dep + 0 ′ + ( 2.303 / f ) log K D , + = dep − 0 ′ − ( 2.303 / f ) log K D , − (A1)

with f = F/RT. Applying (C3) to this relation and rearranging it, the following equation was derived.

( 2.303 / f ) log K D , ± = ( dep − 0 ′ − dep + 0 ′ ) / 2 (A2)

(B) Derivation of another equation based on (C2). Similarly, using ( 2.303 / f ) log K D , − S = dep − 0 ′ , we rearranged Equation (3) as

( 2.303 / f ) log K D , − = ( 2.303 / f ) log K D , + = dep − 0 ′ − dep − . (A3)

Introducing Equation (A3) in dep + = dep + 0 ′ + ( 2.303 / f ) log K D , + {another expression of Equation (3)}, we can immediately obtain dep + = dep + 0 ′ + dep − 0 ′ − dep − under the condition of (C2). Rearranging this equation based on (C1) can yield

dep + = dep − = ( dep + 0 ′ + dep − 0 ′ ) / 2 . (A4)

Here, we define ( dep + 0 ′ + dep − 0 ′ ) / 2 as dep_± and accordingly this means dep₊ = dep₋ = dep_±.

Lastly, adding Equation (A2) in Equation (A4) in each side and then rearranging it give the equation

dep ± = dep − 0 ′ − ( 2.303 / f ) log K D , ± . (A5)

Also, subtracting Equation (A4) from Equation (A2) in each side and then rearranging it give

dep ± = dep + 0 ′ + ( 2.303 / f ) log K D , ± . (A6)

These equations, (A5) and (A6), are applicable to the MA distribution system with the univalent anion A⁻ and that with the cation M⁺, respectively. Therefore, the combination of Equations (A5) and (A6) becomes Equation (3a) with the relations of dep − 0 ′ = ( 2.303 / f ) log K D , − S and dep + 0 ′ = − ( 2.303 / f ) log K D , + S .

Appendix B

The I_oDCBz value for the oDCBz solution in 0.01 mol/L CA and the I value for the 0.0035 mol/L Li₂SO₄ solution were estimated in the following way. Here, the symbol CA means PNP⁺DCC⁻ [5], μ-nitrido-bis(triphenylphosphorus) 3,3-como-bis(undecahydro-1,2-dicarba-3-cobalta-closododecarbo)ate. The association constant (K_CA,org) for C org + + A org − ⇌ CA org in the oDCBz (= org) solution of 0.01 mol/L CA at 295 K has been reported to be 2 × 10³ L/mol from conductivity data [5]. From the quadratic equation for [C⁺]_org (= [A⁻]_org), therefore, we obtained

[ C + ] org / mol ⋅ L − 1 = { ( 1 + 0.04 K CA , org ) 1 / 2 − 1 } / 2 K CA , org = 0.0020 (A7)

with K_CA = 2 × 10³. This [C⁺]_org value basically equals the I_oDCBz one.

Similarly, the association constant ( K LiSO 4 ) for Li + + SO 4 2 − ⇌ LiSO 4 − in the aqueous solution of I = 0.244 mol/kg at 298 K has been reported to be 10^0.77 kg/mol [23]. Therefore,

[ Li + ] / mol ⋅ L − 1 ≈ { ( 1 + 0.0140 K LiSO 4 ) 1 / 2 − 1 } / 2 K LiSO 4 = 0.0033 5 ≈ [ SO 4 2 − ] (A8)

with K LiSO 4 ≈ 13   L / mol and I ≈ 0.010₂ mol/L under the condition of [LiSO₄]_t = 0.0035 mol/L [24] in the w phase at 298 K.

On the basis of the above calculation, the log K D , Pic u / x value (= −2.277 [5]) was changed into the log K D , Pic % one as follows. According to Equation (T7) in Table 3, the relation

log K D , Pic % ≈ log K D , Pic u / x + A f ( x ) − A org ( u ) 1 / 2 ≈ log K D , Pic % − 16.90 v (A9)

holds in this case at 298 K. Using x ≈ 0.010₂ mol/L and u = 0.0020 with b = 0.3 for the oDCBz systems, we immediately obtained log K D , Pic % ≈ log K D , Pic 0.002 / 0.01 − 0. 46 0 = − 2 . 277 − 0. 46 0 = − 2 . 73 7 . This value was assumed to be that at I and I_oDCBz → 0 (see the text) and then employed for the log K D , M % evaluation with log K D , M % = 2 log K D , ± − log K D , Pic % = 2 log K D , ± + 2 . 73 7 in this study. Also, the dep values at 298 K in Table 2 were calculated from the rearranged equation of Equation (3a):

dep = 0.05916 ( log K D , ± − log K D , M S % ) . (A10)

Appendix C

As similar to Appendix B, the I and I_DCE values for the w(1 mol/L MgSO₄)/DCE(0.05 CVBPh₄) system were evaluated. The thermodynamic association constant ( K MA 0 ) for Mg 2 + + SO 4 2 − ⇌ MgSO 4 (=MgA) in water at 298 K has been reported to be 135 L/mol [24]. With the successive approximation method, its [Mg²⁺] (=[ SO 4 2 − ]) in the total concentration, [MgSO₄]_t = 1 mol/L [20], can be evaluated to be 0.21₇ mol/L, which was calculated from the equation

[ Mg 2 + ] = { ( 1 + 4 K MgA ) 1 / 2 − 1 } / 2 K MgA . (A11)

Consequently, the I (=4[Mg²⁺]) value of the aqueous BPh 4 − solution with 1 mol/L MgSO₄ became 0.86₇ mol/L at which K_MgA was estimated to be 16.7 L/mol. In this computation, the K_MgA value was evaluated from log K MgA = log K MgA 0 − 2 × 0. 5114 × ( + 2 ) 2 × f ( I ) . Accordingly, logy₋ = −0.114 at I = 0.86₇ was approximately obtained from − 0.5114 × ( − 1 ) 2 × { I 1 / 2 / ( 1 + I 1 / 2 ) − 0.3 I } for the BPh 4 − solution. Here, the symbol K_MgA denotes the concentration equilibrium constant. The estimated log y₋ value suggests the ion-pair formation of BPh 4 − in water.

Similarly, the association constant (K_CVA,DCE) for CV DCE + + A DCE − ⇌ CVA DCE in the DCE solution of 0.05 mol/L crystal violet cation CV⁺ with A − = BPh 4 − at 298 K has been reported to be 560 L/mol [20]. Therefore,

[ CV + ] DCE / mol ⋅ L − 1 = [ A − ] DCE = { ( 1 + 0.20 K CVA , DCE ) 1 / 2 − 1 } / 2 K CVA , DCE = 0.00 86 0 (A12)

which equals the I_DCE value.

References

1. Sanchez Vallejo, L.J., Ovejero, J.M., Fernández, R.A. and Dassie, E.A. (2012) Single Ion Transfer at Liquid/Liquid Interface. International Journal of Electrochemistry, 2012, Article ID: 462197. https://doi.org/10.1155/2012/462197

2. Markin, V.S. and Volkov, A.G. (1989) The Gibbs Free Energy of Ion Transfer between Two Immiscible Liquids. Electrochimica Acta, 34, 93-107. https://doi.org/10.1016/0013-4686(89)87072-0

3. Rais, J. (1971) Individual Extraction Constants of Univalent Ions in the System Water-Nitrobenzene. Collection of Czechoslovak Chemical Communications, 36, 3253-3262. https://doi.org/10.1135/cccc19713253

4. Levitskaia, T.G., Maya, L., Van Berkel, G.J. and Moyer, B.A. (2007) Anion Partitioning and Ion Pairing Behavior of Anions in the Extraction of Cesium Salts by 4,5-Bis(tert-octylbenzo)dibenzo-24-crown-8 in 1,2-Ddichloroethane. Inorganic Chemistry, 46, 261-272. https://doi.org/10.1021/ic061605k

5. Hundhammer, B. and Müller, C. (1991) Ion Transfer across the Water-o-dichloro-benzene Interface. Journal of Electroanalytical Chemistry, 319, 125-135. https://doi.org/10.1016/0022-0728(91)87072-C

6. Kihara, S., Suzuki, M., Maeda, K., Ogura, K., Umetani, S. and Matsui, M. (1986) Fundamental Factors in the Polarographic Measurement of Ion Transfer at the Aqueous/Organic Solution Interface. Analytical Chemistry, 58, 2954-2961. https://doi.org/10.1021/ac00127a013

7. Kudo, Y. and Katsuta, S. (2015) On an Expression of Extraction Constants without Interfacial Equilibrium-Potential Differences for the Extraction of Univalent and Divalent Metal Picrates by Crown Ether into 1,2-Dichloroethane and Nitrobenzene. American Journal of Analytical Chemistry, 6, 350-363. https://doi.org/10.4236/ajac.2015.64034

8. Kudo, Y., Harashima, K., Hiyoshi, K., Takagi, J., Katsuta, S. and Takeda, Y. (2011) Extraction of Some Univalent Salts into 1,2-Dichloroethane and Nitrobenzene: Analysis of Overall Extraction Equilibrium Based on Elucidating Ion-Pair Formation and Evaluation of Standard Potentials for Ion Transfer at the Interface between Their Diluents and Water. Analytical Sciences, 27, 913-919. https://doi.org/10.2116/analsci.27.913

9. Makrlík, E., Vaňura, P. and Selucky, P. (2008) Solvent Extraction of Ba2+, Pb2+, and Cd2+ into Nitrobenzene by Using Strontium Dicarbollylcobaltate in the Presence of Tetraethyl p-tert-butylcalix[4]arene Tetraacetate. Acta Chimica Slovenica, 55, 430-433. https://doi.org/10.1007/s10967-007-7110-6

10. Takeda, Y., Ezaki, T., Kudo, Y. and Matsuda, H. (1995) Distribution Study on Electroneutral and Protonated Amino Acids between Water and Nitrobenzene. Determination of the Standard Ion-Transfer Potentials of Protonated Amino Acids. Bulletin of the Chemical Society of Japan, 68, 787-790. https://doi.org/10.1246/bcsj.68.787

11. Danil de Namor, A.F., Traboulssi, Y., Salazar, F.F., Dianderas de Acosta, V., Fernández de Vizcardo, Y. and Portugal, J.M. (1989) Transfer and Partition Free Energies of 1:1 Electrolytes in the Water-Dichloromethane Solvent System at 298.15 K. Journal of the Chemical Society, Faraday Transactions I, 85, 2705-2712. https://doi.org/10.1039/f19898502705

12. De Levie, R. (1999) Aqueous Acid-Base Equilibria and Titrations. In: Davies, S.G., Compton, R.G., Evans, J. and Gladden, L.F., Eds., Oxford Chemistry Primers, Oxford University Press, Oxford, 59-63.

13. Kudo, Y., Wakasa, M., Ito, T., Usami, J., Katsuta, S. and Takeda, Y. (2005) Determination of Ion-Pair Formation Constants of Univalent Metal-Crown Ether Complex Ions with Anions in Water Using Ion-Selective Electrodes: Application of Modified Determination Methods to Several Salts. Analytical and Bioanalytical Chemistry, 381, 456-463. https://doi.org/10.1007/s00216-004-2885-6

14. Kudo, Y., Ikeda, S., Morioka, S. and Katsuta, S. (2017) Silver(I) Extraction with Benzo-18-crown-6 Ether from Water into 1,2-Dichloroethane: Analyses on Ionic Strength of the Phases and Their Equilibrium Potentials. Inorganics, 5, 42. https://doi.org/10.3390/inorganics5030042

15. Kudo, Y., Ishikawa, Y. and Ichikawa, H. (2018) CdI2 Extraction with 18-Crown-6 Ether into Various Diluents: Classification of Extracted Cd(II) Complex Ions Based on the HSAB Principle. American Journal of Analytical Chemistry, 9, 560-579. https://doi.org/10.4236/ajac.2018.911041

16. Kakiuchi, T. (1996) Equilibrium Electric Potential between Two Immiscible Electrolyte Solutions. In: Volkov, A.G. and Dreamer, D.W., Eds., Liquid-Liquid Interfaces: Theory and Methods, CRC Press, New York, Ch. 1.

17. Kudo Y. ,et al. (2019)On the Definition of Distribution Equilibrium Potentials in the Distribution Systems with Simple Salts Journal of Analytical & Pharmaceutical Research 8, 172-174.

18. Czapkiewcz, J. and Czapkiewcz-Tutaj, B. (1980) Relative Scale of Free Energy of Transfer of Anions from Water to 1,2-Dichloroethane. Journal of the Chemical Society, Faraday Transactions I, 76, 1663-1668. https://doi.org/10.1039/f19807601663

19. Kudo, Y. (2013) Potentiometric Determination of Ion-Pair Formation Constants of Crown Ether-Complex Ions with Some Pairing Anions. In: Khalid, M.M.A., Ed., Water Using Commercial Ion-Selective Electrodes in Electrochemistry, InTechOpen Access Publisher, Rijeka, 108-109. https://doi.org/10.5772/48206

20. Yoshida, Y., Matsui, M., Shirai, O., Maeda, K. and Kihara, S. (1998) Evaluation of Distribution Ratio in Ion Pair Extraction Using Fundamental Thermodynamic Quantities. Analytica Chimica Acta, 373, 213-225. https://doi.org/10.1016/S0003-2670(98)00367-5

21. Kikuchi, Y., Sakamoto, Y. and Sawada, K. (1998) Partition of Alkali-Metal Ion and Complex Formation with Poly(oxyethylene) Derivatives in 1,2-Dichloroethane. Journal of the Chemical Society, Faraday Transactions, 94, 105-109. https://doi.org/10.1039/a704622g

22. Hung, L.Q. (1980) Electrochemical Properties of the Interface between Two Immiscible Electrolyte Solutions. Part I. Equilibrium Situation and Galvani Potential Difference. Journal of Electroanalytical Chemistry, 115, 159-174. https://doi.org/10.1016/S0022-0728(80)80323-8

23. Reardon, E.J. (1975) Dissociation Constants of Some Univalent Sulfate Ion Pairs at 25&deg; from Stoichiometric Activity Coefficients. The Journal of Physical Chemistry, 79, 422-425. https://doi.org/10.1021/j100572a005

24. Katayama, S. (1973) Conductometric Determination of Ion-Association Constants for Magnesium and Nickel Sulfates at Various Temperatures between 0&deg;C and 45&deg;C. Bulletin of the Chemical Society of Japan, 46, 106-109. https://doi.org/10.1246/bcsj.46.106