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

Satoshi Ikeda^{}, Saya Morioka^{}, Yoshihiro Kudo^{}

Graduate School of Science and Engineering, Chiba University, Chiba, Japan.

**DOI: **10.4236/ajac.2020.111003
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Graduate School of Science and Engineering, Chiba University, Chiba, Japan.

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 (*o*DCBz) were performed at 298 K by changing volume ratios (*V _{org}/V*) between water and

Keywords

Standard Distribution Constants, Volume Ratios, Distribution Equilibrium Potentials, Ionic Strength Dependence, Extraction Constant, Ion-Pair Formation Constant, *o*-Dichlorobenzene

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Ikeda, S. , Morioka, S. and Kudo, Y. (2020) Distribution of Ag(I), Li(I)-Cs(I) Picrates, and Na(I) Tetraphenylborate with Differences in Phase Volume between Water and Diluents. *American Journal of Analytical Chemistry*, **11**, 25-46. doi: 10.4236/ajac.2020.111003.

1. Introduction

In electrochemistry at liquid/liquid interfaces, such as water/nitrobenzene (w/NB) and w/1,2-dichloroethane (w/DCE) ones, formal potentials (
${\text{dep}}_{j}^{0}{}^{\prime}$ ) 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 (
${\text{Ph}}_{\text{4}}{\text{As}}^{+}{\text{BPh}}_{4}^{-}$ ) and so on [1] [2] [3] in many cases. In these studies, there are many data for the potentials
${\text{dep}}_{j}^{0}{}^{\prime}$ 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
${\text{dep}}_{j}^{0}{}^{\prime}$ values have been converted with the relation,
${\text{dep}}_{j}^{0}{}^{\prime}=-\left(1/{z}_{j}f\right)\mathrm{ln}{K}_{\text{D},j}^{\text{S}}$ [7] [8], at dep = 0 V into standard distribution constants (
${K}_{\text{D},j}^{\text{S}}$ ) 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
${\text{dep}}_{\text{M}}^{0}{}^{\prime}=-\left(0.0\text{5916}\right)\mathrm{log}{K}_{\text{D},\text{M}}^{\text{S}}$ {or
${\text{dep}}_{\text{+}}^{0}{}^{\prime}=-\left(0.0\text{5916}\right)\mathrm{log}{K}_{\text{D},\text{+}}^{\text{S}}$ } with j = M^{+} holds at dep = 0 V and T = 298.1_{5} K. Generally such
${K}_{\text{D},j}^{\text{S}}$ values have been determined by solvent extraction experiments with j = M^{+}, M^{2+}, 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,
${K}_{\text{D},j}^{\text{S}}$, at dep = 0 V and T ≈ 298 K for j = Ag^{+}, Li^{+}-Cs^{+}, and
${\text{BPh}}_{4}^{-}$ into some diluents. The
${K}_{\text{D},\text{Ag}}^{\text{S}}$ values were obtained from NB, DCE, oDCBz, and dichloromethane (DCM) systems with the reported
${K}_{\text{D},\text{Pic}}^{\text{S}}$ value [5] [8] [11] of picrate ion (Pic^{−}), the
${K}_{\text{D},j}^{\text{S}}$ values at j = Li^{+}-Cs^{+} from oDCBz one with that [5] of Pic^{−}, and the
${K}_{\text{D},\text{BPh4}}^{\text{S}}$ values from NB and DCE ones with the
${K}_{\text{D},\text{Na}}^{\text{S}}$ 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
${\text{BPh}}_{4}^{-}$ or Cs^{+}, differences among its
${K}_{\text{D},{\text{BPh}}_{\text{4}}}$ or K_{D,Cs} values were considered in their experimental conditions and thereby classified into two groups, such as K_{D,j} and
${K}_{\text{D},j}^{\text{S}}$.

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 NaBPh_{4} {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: 7.34_{3}% for M(I) = Li; 6.23_{2} for Na; 1.23_{0} for K; 2.76_{7} 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 AgNO_{3} (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 NaBPh_{4} 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 NaBPh_{4} 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 NaBPh_{4} distribution systems were back-extracted by using 0.1 mol/L HNO_{3}, 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.

^{a}Values at I & I_{org} → 0. ^{b}Values calculated from Equation (3a). See the footnotes e & h for the
$\mathrm{log}{K}_{\text{D},\text{Pic}}^{\text{S}}$ &
$\mathrm{log}{K}_{\text{D},\text{Na}}^{\text{S}\%}$ values. ^{c}Average values. ^{d}Ref. [14]. ^{e}Values calculated from
$\mathrm{log}{K}_{\text{D},\text{Pic}}^{\text{S}}=0.0\text{5}$ at I & I_{NB} → 0; −1.01_{1} at I & I_{DCE} → 0; −2.73_{7} at [Li_{2}SO_{4}]_{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. ^{f}Values calculated from the original data of ref. [14]. ^{g}Values determined at 295 - 298 K, where
$\mathrm{log}{K}_{\text{D},\text{Ag}}^{\text{S}}$ corresponds
$\mathrm{log}{K}_{\text{D},\text{Ag}}^{\text{S}\%}$. See the text & Equation (T8) in Table 3 for the
$\mathrm{log}{K}_{\text{D},\text{Ag}}^{\text{S}\%}$ estimation. ^{h}Calculated from
$\mathrm{log}{K}_{\text{D},\text{Na}}^{\text{S}\%}=-\text{5}.\text{18}$ for w/NB; −6.09 for w/DCE. See ref. [8]. ^{i}The 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.

^{a}Values at I & I_{o}_{DCBz} → 0. ^{b}Values calculated from
$\mathrm{log}{K}_{\text{D},\text{Pic}}^{\text{S}\%}=-\text{2}.{\text{73}}_{\text{7}}$ at [Li_{2}SO_{4}]_{t} = 0.0035 mol/L, [PNP^{+}DCC^{−}]_{t,org} = 0.01, & 295 K using Equation (3a). See ref. [5]. ^{c}Values determined at 295 - 298 K. ^{d}Values expressed as the errors which equal those of logK_{D}_{,±}. See the text. ^{e}Average values. ^{f}Ref. [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 NaBPh_{4} 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,
${\text{M}}^{+}+{\text{A}}^{-}\rightleftharpoons \text{MA}$, in water, we can easily propose a quadratic equation
${K}_{\text{MA}}{}^{V}\left[{\text{M}}^{+}\right]{}^{\text{2}}+{}^{V}\left[{\text{M}}^{+}\right]-{\left[\text{M}\right]}_{\text{t},\text{w}}=0$ {see Equation (1) for the symbols ^{V}[M^{+}] & [M]_{t,w}} and then obtain from it

${}^{V}\left[{\text{M}}^{+}\right]={}^{V}\left[{\text{A}}^{-}\right]=\left\{{\left(\text{1}+\text{4}{K}_{\text{MA}}{\left[\text{M}\right]}_{\text{t},\text{w}}\right)}^{1/2}-\text{1}\right\}/\text{2}{K}_{\text{MA}}$. From the latter equation,

we calculated self-consistent ^{V}[A^{−}] and K_{MA} values by a successive approximation with
$\mathrm{log}{K}_{\text{MA}}=\mathrm{log}{K}_{\text{MA}}^{0}+\text{2}\mathrm{log}{y}_{\pm}$ [8]. Here, the symbols, K_{MA},
${K}_{\text{MA}}^{0}$, 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:

${\left[\text{M}\right]}_{\text{t}}V={\left[\text{M}\right]}_{\text{t},\text{w}}V+{\left[\text{M}\right]}_{\text{t},\text{org}}{V}_{\text{org}},$ (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

$\begin{array}{c}{r}_{\text{org}/\text{w}}{\left[\text{M}\right]}_{\text{t},\text{org}}/{}^{V}\left[{\text{M}}^{+}\right]=\left({\left[\text{M}\right]}_{\text{t}}-{\left[\text{M}\right]}_{\text{t},\text{w}}\right)/{}^{V}\left[{\text{M}}^{+}\right]\\ ={r}_{\text{org}/\text{w}}\left({\left[{\text{M}}^{+}\right]}_{\text{org}}+{\left[\text{MA}\right]}_{\text{org}}\right)/{}^{V}\left[{\text{M}}^{+}\right],\end{array}$ (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,
${{K}^{\prime}}_{\text{ex}}$, 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

$\begin{array}{c}\text{dep}=\varphi -{\varphi}_{\text{org}}=0.0\text{5916}\left(\mathrm{log}{K}_{\text{D},\text{M}}-\mathrm{log}{K}_{\text{D},\text{M}}^{\text{S}}\right)\\ =-0.0\text{5916}\left(\mathrm{log}{K}_{\text{D},\text{A}}-\mathrm{log}{K}_{\text{D},\text{A}}^{\text{S}}\right).\end{array}$ (3)

Here, the symbols
$\varphi $ (or
${\varphi}_{\text{org}}$ ), 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
${K}_{\text{D},\text{M}}^{\text{S}}$ and
${K}_{\text{D},\text{A}}^{\text{S}}$. 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).

$\text{dep}={\text{dep}}_{\pm}=0.0\text{5916}\left(\mathrm{log}{K}_{\text{D},}{}_{\pm}-\mathrm{log}{K}_{\text{D},\text{M}}^{\text{S}}\right)=-0.0\text{5916}\left(\mathrm{log}{K}_{\text{D},}{}_{\pm}-\mathrm{log}{K}_{\text{D},\text{A}}^{\text{S}}\right)$ (3a)

So from rearranging Equation (2) with
${K}_{\text{D},\pm}^{2}$ which is defined as
${K}_{\text{D},\text{M}}^{\text{S}}{K}_{\text{D},\text{A}}^{\text{S}}$ {=K_{D,M}K_{D,A}: the condition (C3) in Appendix A}, the following equation was obtained.

$\begin{array}{c}{r}_{\text{org}/\text{w}}{\left[\text{M}\right]}_{\text{t},\text{org}}/{}^{V}\left[{\text{M}}^{+}\right]={r}_{\text{org}/\text{w}}{D}_{\text{M}}^{\text{expl}.}={K}_{\text{D},\text{M}}+{{K}^{\prime}}_{\text{ex}}{r}_{\text{org}/\text{w}}{}^{V}\left[{\text{A}}^{-}\right]\\ ={K}_{\text{D},}{}_{\pm}+{{K}^{\prime}}_{\text{ex}}{r}_{\text{org}/\text{w}}{}^{V}\left[{\text{A}}^{-}\right]\end{array}$ (4)

under the conditions of K_{D,M} = K_{D,A} (see above) and
${K}_{\text{D},\text{M}}^{\text{S}}\ne {K}_{\text{D},\text{A}}^{\text{S}}$. Here
${r}_{\text{org}/\text{w}}{D}_{\text{M}}^{\text{expl}.}$ equals an experimental (expl.) value, ^{V}[M]_{t,org}/^{V}[M^{+}], corresponding to the distribution ratio of M(I) [8]. Hence, the plot of
${r}_{\text{org}/\text{w}}{D}_{\text{M}}^{\text{expl}.}$ versus
${r}_{\text{org}/\text{w}}{}^{V}\left[{\text{A}}^{-}\right]$ based on Equation (4) can give
${{K}^{\prime}}_{\text{ex}}$ 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} (
$={r}_{\text{org}/\text{w}}{}^{V}\left[{\text{A}}^{-}\right]$ or ^{V}[A^{−}]) → 0 and P^{*} (≈K_{ex}).

The symbol
${{K}^{\prime}}_{\text{ex}}$ is converted with r_{org}_{/w} into
${K}_{\text{ex}}\left(={r}_{\text{org}/\text{w}}{{K}^{\prime}}_{\text{ex}}\right)$ which is thermodynamically expressed as
${\left({K}_{\text{D},}{}_{\pm}\right)}^{\text{2}}{K}_{\text{MA},\text{org}}={K}_{\text{D},\text{M}}{K}_{\text{D},\text{A}}{K}_{\text{MA},\text{org}}={K}_{\text{D},\text{M}}^{\text{S}}{K}_{\text{D},\text{A}}^{\text{S}}{K}_{\text{MA},\text{org}}$ (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
${\left({K}_{\text{D},\pm}\right)}^{\text{2}}={K}_{\text{D},\text{M}}{K}_{\text{D},\text{A}}={K}_{\text{D},\text{M}}^{\text{S}}{K}_{\text{D},\text{A}}^{\text{S}}$, the K_{D,M} and K_{D,A} values must satisfy the same experimental conditions, such as I and I_{org}, and also
${K}_{\text{D},\text{A}}^{\text{S}}$ and
${K}_{\text{D},\text{M}}^{\text{S}}$ 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
${r}_{\text{DCE}/\text{w}}{D}_{\text{Ag}}^{\text{expl}.}=\left({1.4}_{0}\pm {0.5}_{1}\right)\times {10}^{-4}+\left(0.0366\pm 0.0007\right)\times {r}_{\text{DCE}/\text{w}}{}^{V}\left[{\text{Pic}}^{-}\right]$ at correlation coefficient (R_{ }) = 0.997. From these intercept and slope, the logK_{D}_{,±} value was evaluated to be −3.8_{5} ± 0.1_{6}, while the logK_{ex} one was to be −1.0_{2} ± 0.3_{9}. In the latter K_{ex} evaluation, the K_{ex} values were obtained from
${K}_{\text{ex}}={r}_{\text{DCE}/\text{w}}{{K}^{\prime}}_{\text{ex}}$ for given r_{DCE}_{/w} values and then their values were averaged. Additionally, the
$\mathrm{log}{K}_{\text{D},\text{Ag}}^{\text{S}}$ and log K_{AgPic,DCE} values were calculated to be −6.6_{9} (
$=\text{2}\mathrm{log}{K}_{\text{D},}{}_{\pm}-\mathrm{log}{K}_{\text{D},\text{Pic}}^{\text{S}}$ ) with the calculation error of ±0.2_{2} 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 (= −1.4_{1}) was close to that (= −1.49 [14]) reported before and also the minimum logK_{D,AgPic} value (= −1.7_{4}) was somewhat larger than the

Figure 1. Plot of
${r}_{\text{DCE}/\text{w}}{D}_{\text{Ag}}^{\text{expl}.}$ vs.
${r}_{\text{DCE}/\text{w}}{}^{V}\left[{\text{Pic}}^{-}\right]$ for the AgPic distribution into DCE at vari ous r_{DCE}_{/w} values (see Table 1). The broken line is a regression one based on Equation (4) (see the text).

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 NaBPh_{4} distribution into several diluents and Table 2 does results for the LiPic-CsPic distribution into oDCBz.

In the relation of $\text{2}\mathrm{log}{K}_{\text{D},}{}_{\pm}=\mathrm{log}\left({K}_{\text{D},\text{M}}^{\text{S}}{K}_{\text{D},\text{A}}^{\text{S}}\right)$, the pair of the ${K}_{\text{D},\text{M}}^{\text{S}}$ and ${K}_{\text{D},\text{A}}^{\text{S}}$ values must satisfy the same experimental conditions. In other words, the use of $\mathrm{log}{K}_{\text{D},\text{Ag}}^{\text{S}}=\text{2}\mathrm{log}{K}_{\text{D},}{}_{\pm}-\mathrm{log}{K}_{\text{D},\text{Pic}}^{\text{S}}$ basically reflects the experimental conditions of ${K}_{\text{D},\text{Pic}}^{\text{S}}$ in the ${K}_{\text{D},\text{Ag}}^{\text{S}}$ estimation. The same is also true of $\mathrm{log}{K}_{\text{D},\text{Ag}}=\text{2}\mathrm{log}{K}_{\text{D},}{}_{\pm}-\mathrm{log}{K}_{\text{D},\text{Pic}}$.

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.

${D}_{\text{M}}^{\text{expl}.}={K}_{\text{D},}{}_{\pm}/{r}_{\text{org}/\text{w}}+{{K}^{\prime}}_{\text{ex}}{}^{V}\left[{\text{A}}^{-}\right].$ (5)

As examples, these common logarithmic K_{D,}_{±} and K_{ex} values for the AgPic distribution into DCE were −3.2_{3} ± 0.3_{8} and −1.0_{2} ± 0.3_{8}, respectively. From these values, the
$\mathrm{log}{K}_{\text{D},\text{Ag}}^{\text{S}}$ and logK_{AgPic,DCE} values were also estimated to be −5.4_{5} ± 0.5_{3} 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
${r}_{\text{org}/\text{w}}{D}_{\text{M}}^{\text{expl}.}$ versus ^{V}[A^{−}] based on Equation (4) was not able to give the straight line, indicating that the
${{K}^{\prime}}_{\text{ex}}{r}_{\text{org}/\text{w}}$ (=K_{ex}) term in the plot is not the constant. This fact shows that the parameter
${r}_{\text{org}/\text{w}}{}^{V}\left[{\text{A}}^{-}\right]$ is more important than the
${{K}^{\prime}}_{\text{ex}}{r}_{\text{org}/\text{w}}$ 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
${K}_{\text{AgPic}}^{0}$ 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
${K}_{\text{D},\text{Ag}}^{\text{S}}$ values were in the order NB > oDCBz ≥ DCE > DCM (see Table 1), although the value for the oDCBz system was calculated from
${K}_{\text{D},\text{Pic}}^{\text{S}}$ [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
${K}_{\text{D},\text{M}}^{\text{S}}$ ) in Table 2, except for the oDCBz system of Table 1, we can suppose that the differences in
${K}_{\text{D},\text{M}}^{\text{S}}$ between T = 295 ± 3 [5] and 298 K are negligible. However, the
${K}_{\text{D},\text{Pic}}^{\text{S}}$ determination at 298 K will be necessary for the determination of the more-exact
${K}_{\text{D},\text{M}}^{\text{S}}$ values.

3.5. $log{K}_{D,M}^{S\%}$ Estimation

We derived the following equation from the definition of
${K}_{\text{D},\text{M}}^{\text{S}\%}={y}_{+,\text{org}}{K}_{\text{D},\text{M}}^{\text{S}}/{y}_{+}$ 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.

$\mathrm{log}{K}_{\text{D},\text{M}}^{\text{S}}=\mathrm{log}\left({y}_{+}{K}_{\text{D},\text{M}}^{\text{S}\%}/{y}_{+,\text{org}}\right)=\mathrm{log}{K}_{\text{D},\text{M}}^{\text{S}\%}-A{z}_{j}^{2}f\left(I\right)+{A}_{\text{org}}{z}_{j}^{2}{\left({I}_{\text{org}}\right)}^{1/2}$ (6)

Here, the symbol,
${K}_{\text{D},\text{M}}^{\text{S}\%}$, 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,
${K}_{\text{D},\text{M}}^{\text{S}}\left(={K}_{\text{D},\text{M}}^{\text{S}u/x}\right)$ equals [M^{+}]_{org}/[M^{+}] as the concentration expression for a given I = x or I_{org} = u,
${K}_{\text{D},\text{M}}^{\text{S}u/0}$ does [M^{+}]_{org}/a_{M} for a given I_{org} = u, and
${K}_{\text{D},\text{M}}^{\text{S}0/x}$ 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
$\mathrm{log}{K}_{\text{D},\text{Pic}}^{\%}$ reported cyclic-volammetrically for the w/oDCBz system [5] satisfies the condition of dep = 0 V, the
$\mathrm{log}{K}_{\text{D},\text{M}}^{\text{S}\%}$ values were calculated from its
$\mathrm{log}{K}_{\text{D},\text{Pic}}^{\%}$ value (= −2.73_{7}, see Appendix B for the calculation) with
$2\mathrm{log}{K}_{\text{D},\pm}^{\%}=\mathrm{log}{K}_{\text{D},\text{M}}^{\%}{K}_{\text{D},\text{A}}^{\%}$ at dep = 0 V. From the data in Table 2, the logarithmic values of the average
${K}_{\text{D},\text{M}}^{\text{S}\%}$, which was calculated from the intercepts,
${K}_{\text{D},\pm}^{\%}$ (for example see Figure 2), can be estimated easily. These
$\mathrm{log}{K}_{\text{D},\text{M}}^{\text{S}\%}$ values were −8.3_{4} ± 0.4_{1} for M = Li, −5.4_{5} ± 0.9_{6} for Na, −3.1_{3} ± 0.7_{2} for K, −6.7_{8} for Rb, and −5.9_{5} for Cs. Here, the errors corresponding to log K_{D,±} were approximately employed as the errors of
$\mathrm{log}{K}_{\text{D},\text{M}}^{\text{S}\%}$, because of a lack [5] of the
$\mathrm{log}{K}_{\text{D},\text{Pic}}^{\text{S}\%}$ ’s error (see Table 1 & Table 2). The
${K}_{\text{D},\text{M}}^{\text{S}\%}$ 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)
$\gg $ 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.

^{a}The parameters x, u, & v show unknown values & zero, u_{1}, & x_{1} do the known ones. ^{b
${K}_{\text{D},j}={K}_{\text{D},j}^{u/x}={\left[j\right]}_{\text{org}}/\left[j\right]$ }. ^{c}Basic equation. ^{d
${K}_{\text{D},j}^{0/x}={a}_{j}{}_{,\text{org}}/\left[j\right]$ }.
${K}_{\text{D},j}^{u/0}={\left[j\right]}_{\text{org}}/{a}_{j}$. ^{f
${K}_{\text{D},j}^{\%}={a}_{j}{}_{,\text{org}}/{a}_{j}$ }. ^{g}Defined as
${K}_{\text{D},j}^{\text{S}\%}={a}_{j}{}_{,\text{org}}/{a}_{j}$ at dep = 0 V.

Figure 2. Plot of
${r}_{o}{}_{\text{DCBz}/\text{w}}{D}_{\text{Li}}^{\text{expl}\text{.}}$ vs.
${r}_{o}{}_{\text{DCBz}/\text{w}}{}^{V}\left[{\text{Pic}}^{-}\right]$ for the LiPic distribution into oDCBz at various r_{DCE}_{/w} values. The lines are straight ones based on the regression analysis with Equation (4). These plots are those under the conditions of I = 0.026 mol/L (circle), 0.058 (square), 0.070 (diamond), and 0.082 (full & open triangles). Essentially, all the intercepts must indicate the same value.

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
$\mathrm{log}{K}_{\text{D},\text{M}}^{\text{S}\%}$ for the MPic distribution into DCE at 298 K were −8.07 for M = Li, −6.0_{9} for Na, and −5.9_{5} for K (−5.37 for Rb & −4.6_{0} 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
$\mathrm{log}{K}_{\text{D},\text{Ag}}^{\text{S}\%}$ value for the oDCBz system was estimated to be −6.30 (see Table 1) from the relation
$\mathrm{log}{K}_{\text{D},\text{Ag}}^{\text{S}\%}=2\mathrm{log}{K}_{\text{D},\pm}-\mathrm{log}{K}_{\text{D},\text{Pic}}^{\text{S}\%}$.

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_{o}_{DCBz} 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
$log{K}_{D,M}^{S}$

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} = (0.0_{6} ± 0.3_{0}) − (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,M}K_{D,A}K_{MA,org}). Introducing Equation (3) in this cycle, we immediately obtain

$\begin{array}{c}\mathrm{log}{K}_{\text{ex}}=-\text{dep}/0.0\text{5916}+\mathrm{log}\left({K}_{\text{D},\text{M}}{K}_{\text{D},\text{A}}^{\text{S}}{K}_{\text{MA},\text{org}}\right)\\ =-\text{16}.\text{9}0\text{dep}+\mathrm{log}\left({K}_{\text{D},\text{M}}{K}_{\text{D},\text{A}}^{\text{S}}{K}_{\text{MA},\text{org}}\right)\end{array}$ (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
${K}_{\text{D},\text{M}}^{\text{S}\%}$ and K_{MPic,org} were −3._{8} ± 1._{8} and 7.8_{9} ± 0.8_{9}, respectively, and
$\mathrm{log}{K}_{\text{D},\text{Pic}}^{\text{S}\%}$ was −2.73_{7} (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
$\mathrm{log}{K}_{\text{D},\text{Pic}}^{\text{S}\%}$ ). The estimated
$\mathrm{log}\left({K}_{\text{D},\text{M}}^{\text{S}\%}{K}_{\text{DD},\text{A},\text{M}}^{\text{S}\%}{K}_{\text{MA},\text{org}}\right)$ value was in accord

Figure 3. Plot of logK_{ex} vs. dep (at 295 K) for the MPic distribution with M = Li-Cs into oDCBz. The broken line is a regression one (see the text) corresponding to Equation (7), except for the point (full circle) of the AgPic system.

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
$\mathrm{log}{K}_{\text{D},\text{M}}^{\text{S}\%}$ plot. This plot can come from the relation

$\begin{array}{c}\mathrm{log}{K}_{\text{ex}}=\mathrm{log}\left({y}_{+}{K}_{\text{D},\text{M}}^{\text{S}\%}/{y}_{+,\text{org}}\right)+\mathrm{log}\left({y}_{-}{K}_{\text{D},\text{A}}^{\text{S}\%}/{y}_{-,\text{org}}\right)+\mathrm{log}{K}_{\text{MA},\text{org}}\\ =\mathrm{log}{K}_{\text{D},\text{M}}^{\text{S}\%}+\mathrm{log}\left({K}_{\text{D},\text{A}}^{\text{S}\%}{K}_{\text{MA},\text{org}}\right)+\text{2}\mathrm{log}\left({y}_{\pm}/{y}_{\pm ,\text{org}}\right).\end{array}$ (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
$\mathrm{log}{K}_{\text{ex}}=\left(0.62\pm 0.07\right)\mathrm{log}{K}_{\text{D},\text{M}}^{\text{S}\%}+\left({1.9}_{1}\pm {0.4}_{8}\right)$ at R = 0.903. Unfortunately, the slope and intercept were smaller than unity and the log (the product between
$\mathrm{log}{K}_{\text{D},\text{Pic}}^{\text{S}\%}$ and the average of K_{MA,org}) value of 5.2 (≈7.8_{9} − 2.73_{7}) with the error of about ±0.9, respectively. While, the result obtained from the slope fixed at unity was
$\mathrm{log}{K}_{\text{ex}}=\mathrm{log}{K}_{\text{D},\text{M}}^{\text{S}\%}+\left({4.4}_{8}\pm {0.2}_{0}\right)$ 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
${K}_{\text{D},\text{M}}^{\text{S}\%}$ 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
${K}_{\text{ex}}^{0}$ as K_{ex} based on the activity expression, we can obtain

${K}_{\text{ex}}^{0}={a}_{\text{MA},\text{org}}/{a}_{\text{M}}{a}_{\text{A}}={K}_{\text{ex}}/{y}_{+}{y}_{-},$ (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:

$\mathrm{log}{K}_{\text{ex}}\approx \mathrm{log}{K}_{\text{ex}}^{0}-\text{2}Af\left(I\right)$ (8a)

with $\mathrm{log}{y}_{+}{y}_{-}=-\text{2}Af\left(I\right)$ (8b)

and $f\left(I\right)\approx {I}^{1/2}/\left(1+{I}^{1/2}\right)-0.3I$. (8c)

Hence, a non-linear regression analysis of the plots of logK_{ex} versus I^{1/2} can yield experimental
$\mathrm{log}{K}_{\text{ex}}^{0}$ and A values.

Figure 4 shows an example of such plots. The regression line was logK_{ex} = (−1.5_{4} ± 0.7_{2}) – 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} = (0.2_{4} ± 0.7_{4}) – 2 ´ (7._{3} ± 1._{9})f(I_{ }) at R = 0.885 and = (1.2_{4} ± 0.6_{7}) – 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
$\mathrm{log}{K}_{\text{ex}}^{0}$ values for the MPic distribution were in the order M = Li < Na ≤ K {>Rb (
$\mathrm{log}{K}_{\text{ex},\text{av}}^{0}=-\text{1}.{\text{6}}_{\text{5}}$ ) < Cs (−1.1_{4})}, where
${K}_{\text{ex},\text{av}}^{0}$ denotes the average of
${K}_{\text{ex}}^{0}$.

3.8. On the I_{org} Dependence of logK_{MA,org}

As similar to the I dependence of logK_{ex}, we considered
${K}_{\text{MA},\text{org}}^{0}$ based on an

Figure 4. Plot of logK_{ex} vs. (I)^{1/2} for the LiPic distribution into oDCBz. The broken line was a regression one based on Equation (8a).

activity ex pression as follows.

${K}_{\text{MA},\text{org}}^{0}={\left[\text{MA}\right]}_{\text{org}}/{a}_{\text{M},\text{org}}{a}_{\text{A},\text{org}}={K}_{\text{MA},\text{org}}/{y}_{+,\text{org}}{y}_{-,\text{org}}$ (9)

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

$\mathrm{log}{K}_{\text{MA},\text{org}}=\mathrm{log}{K}_{\text{MA},\text{org}}^{0}-\text{2}{A}_{\text{org}}{\left({I}_{\text{org}}\right)}^{1/2}$ (9a)

with $-\text{2}{A}_{\text{org}}{\left({I}_{\text{org}}\right)}^{1/2}=\mathrm{log}{y}_{+,\text{org}}{y}_{-,\text{org}}$. (9b)

A plot of logK_{MA,org} versus
${I}_{\text{org}}^{1/2}$ can give a straight line with the slope of –2A_{org} and the intercept of
$\mathrm{log}{K}_{\text{MA},\text{org}}^{0}$.

Figure 5 shows an example of the NaPic distribution system with org = oDCBz. The broken line was the experimental regression one,
$\mathrm{log}{K}_{\text{NaPic},\text{org}}=\left({8.1}_{6}\pm {0.1}_{3}\right)-2\times \left(422\pm 43\right){\left({I}_{\text{org}}\right)}^{1/2}$ at R = 0.980. Similar results were obtained from the other two systems:
$\mathrm{log}{K}_{\text{LiPic},\text{org}}=\left({8.9}_{8}\pm {0.2}_{8}\right)-2\times \left(1819\pm 350\right){\left({I}_{\text{org}}\right)}^{1/2}$ at R = 0.949 and
$\mathrm{log}{K}_{\text{KPic},\text{org}}=\left({6.8}_{8}\pm {0.4}_{0}\right)-2\times \left(260\pm 134\right){\left({I}_{\text{org}}\right)}^{1/2}$ 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
$\mathrm{log}{K}_{\text{MPic},o\text{DCBz}}^{0}$ values at I_{o}_{DCBz} → 0 were in the order M = Li > Na > K (≤ Rb ≈ Cs, see Table 2). This order recalls that (Li > Na ≤ K) of
${K}_{\text{MPic}}^{0}$ [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^{+}.

Figure 5. Plot of log K_{NaPic,org} vs.
${I}_{\text{org}}^{1/2}$ for the distribution into org = oDCBz. The broken line was a regression one based on Equation (9a).

3.9. On the Differences between
${K}_{D,BP{h}_{4}}$ or K_{D,Cs} Values in the NB, DCE, and oDCBz Systems

The
$\mathrm{log}{K}_{\text{D},{\text{BPh}}_{\text{4}}}^{\text{S}\%}$ 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 [MgSO_{4}]_{t} = 1 mol/L and
${\left[{\text{CV}}^{+}{\text{BPh}}_{4}^{-}\right]}_{\text{t},\text{DCE}}=0.05$ (CV^{+}: crystal violet cation) and 6.13 [18] at I → 0 for the DCE ones. Their experimental
$\mathrm{log}{K}_{\text{D},{\text{BPh}}_{\text{4}}}^{\text{S}\%}$ 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
$\mathrm{log}{K}_{\text{D},{\text{BPh}}_{\text{4}}}$ values, as described in the Section 3.5.

Although numbers of the data sets of
$\mathrm{log}{K}_{\text{D},{\text{BPh}}_{\text{4}}}$ and I or I_{org} were few, Equation (6) employed for A^{−} has possibility for showing the I or I_{org} dependence of the
$\mathrm{log}{K}_{\text{D},{\text{BPh}}_{\text{4}}}$ values. So, using Equations (3) and (6), we can immediately derive the following basic equation:

$\begin{array}{c}\mathrm{log}{K}_{\text{D},j}=\mathrm{log}{K}_{\text{D},j}^{\text{S}\%}+\left(f/\text{2}.\text{3}0\text{3}\right){z}_{j}\text{dep}-A{z}_{j}^{2}f\left(I\right)+{A}_{\text{org}}{z}_{j}^{2}{\left({I}_{\text{org}}\right)}^{1/2}\\ \approx \mathrm{log}{K}_{\text{D},j}^{\text{S}}+\left(f/\text{2}.\text{3}0\text{3}\right){z}_{j}\text{dep}\end{array}$ (10)

with j = M^{+}, A^{−} and
${K}_{\text{D},j}^{\text{S}\%}={y}_{j}{}_{,\text{org}}{K}_{\text{D},j}^{\text{S}}/{y}_{j}\left(={y}_{j}{}_{,\text{org}}{K}_{\text{D},j}^{\text{S}u/x}/{y}_{j}\right)$. 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
$\text{4}.\text{2}=\mathrm{log}{K}_{\text{D},j}^{\text{S}\%}+\left(f/2.303\right){z}_{j}\times 0-A{z}_{j}^{2}f\left(0\right)+{A}_{\text{NB}}{z}_{j}^{2}\times {0}^{1/2}=\mathrm{log}{K}_{\text{D},j}^{\text{S}\%}+0-0+0$ with A = 0.5114, b = 0.3, and A_{NB} = 1.725 at
$j={\text{BPh}}_{4}^{-}$, we immediately obtained
$\mathrm{log}{K}_{\text{D},j}^{\text{S}\%}=\text{4}.\text{2}$ at z_{j} = −1. From
$6.3=4.2-\left(f/2.303\right)v-Af\left(x\right)+{A}_{\text{NB}}{u}^{1/2}$, the –16.90v – Af(x) + A_{NB}u^{1/2} term at 298 K was obtained to be 2.1 at z_{j} = −1. Also, using
$5.6+Af\left(0\right)=4.2-\left(f/2.303\right)v+{A}_{\text{NB}}{u}^{1/2}$, the –(f/2.303)v + A_{NB}u^{1/2} term equals 1.4 with
$\text{5}.\text{6}=\mathrm{log}{K}_{\text{D},{\text{BPh}}_{\text{4}}}^{u/0}=4.2-16.90v+1.725{u}^{1/2}$. These cases suggest that the former of 6.3 is
$\mathrm{log}{K}_{\text{D},{\text{BPh}}_{\text{4}}}^{u/x}$ {Equation (10) or (T1) in Table 3} and the latter of 5.6 is
$\mathrm{log}{K}_{\text{D},{\text{BPh}}_{\text{4}}}^{u/0}$ {Equation (T4)}. Strictly speaking, it is difficult to compare 6.3 with 5.6.

Similarly, the relation
$-1.4=\mathrm{log}{K}_{\text{D},j}^{\text{S}\%}+0-0+{A}_{\text{DCE}}\times {0}^{1/2}$ gave −1.4 as
$\mathrm{log}{K}_{\text{D},j}^{\text{S}\%}$ with A_{DCE} = 10.63 at
$j={\text{BPh}}_{4}^{-}$. For
$5.396\left(=\mathrm{log}{K}_{\text{D},{\text{BPh}}_{\text{4}}}^{0.0\text{5}//\text{1}}\right)=-\text{1}.\text{4}-\left(f/2.303\right)v-Af\left(0.87\right)+{A}_{\text{DCE}}\times 0.00{\text{86}}^{1/2}$, dep (= v) became −0.3_{5} V with 5.396 + 0.5114f(0.87) − 10.63 × 0.0086^{1/2} = 4.52_{7} = −1.4 – 16.90v at b = 0.3 and 298 K: see Appendix C for the estimation of I = 0.86_{7} 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
$6.13=-1.4-\left(f/2.303\right)v-0+{A}_{\text{DCE}}{u}^{1/2}$, the –(f/2.303)v + A_{DCE}u^{1/2} term at 298 K became 7.5 with
$6.13+Af\left(0\right)=-1.4-16.90v+10.63{u}^{1/2}$. As similar to the w/NB results, the former of 5.396 + Af(0.87) − A_{DCE} × 0.0086^{1/2} (= 4.53) is
$\mathrm{log}{K}_{\text{D},{\text{BPh}}_{\text{4}}}^{\%}$ {Equation (T7)} and the latter of 6.13 is
$\mathrm{log}{K}_{\text{D},{\text{BPh}}_{\text{4}}}^{u/0}$ ^{ }{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 MgSO_{4})/ oDCBz(0.05 CVBPh_{4}) 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
$\mathrm{log}{K}_{\text{D},\text{Cs}}^{\text{S}\%}=-{5.9}_{5}$ (see Section 3.5) based on the average value in Table 2, the following relation holds:
$-\text{2}.0\text{3}\left(=\mathrm{log}{K}_{\text{D},\text{Cs}}^{0.0\text{5}//\text{1}}\right)\approx -\text{5}.{\text{9}}_{\text{5}}+\left(f/2.303\right)v-Af\left(0.87\right)+{A}_{o}{}_{\text{DCBz}}{u}^{1/2}$. Hence, the relation 16.90v + 11.3u^{1/2} ≈ 4.0 was obtained with
$-2.03+Af\left(0.\text{87}\right)=-1.91\approx \mathrm{log}{K}_{\text{D},\text{Cs}}^{u/0}=-{5.9}_{5}+16.90v+11.3{u}^{1/2}$. Here, we were not able to estimate the dep and I_{o}_{DCBz} values, because the K_{MA,oDCBz} value for
$\text{MA}={\text{CV}}^{+}{\text{BPh}}_{4}^{-}$ (the supporting electrolyte) in the oDCBz phase had not been found [6].

As another example, the
$\mathrm{log}{K}_{\text{D},\text{Cs}}^{\text{S}\%}$ value has been reported to be −6.3_{5} [21] for the CsPic distribution into DCE at 298 K. Similarly, the relation
$\mathrm{log}{K}_{\text{D},\text{Cs}}+Af\left(x\right)-{A}_{\text{DCE}}{u}^{1/2}=-{6.3}_{5}=\mathrm{log}{K}_{\text{D},\text{Cs}}^{\%}=-{4.6}_{0}+16.90v$ 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
$\mathrm{log}{K}_{\text{D},\text{C}}^{u/0}$ {Equation (T4)} and the latter of −6.3_{5} is
$\mathrm{log}{K}_{\text{D},\text{Cs}}^{\%}$ {Equation (T7)}.

Thus, these results support the above understanding about the conditional
${K}_{\text{D},{\text{BPh}}_{\text{4}}}$ or K_{D,Cs} and self-consistently suggest that their values are functions [16] [22] containing dep, I, and I_{org}, that is,
${K}_{\text{D},{\text{BPh}}_{\text{4}}}={K}_{\text{D},{\text{BPh}}_{\text{4}}}^{\text{S}\%}\left({y}_{-}/{y}_{-,\text{org}}\right)\mathrm{exp}\left(-f\text{dep}\right)$ or
${K}_{\text{D},\text{Cs}}={K}_{\text{D},\text{Cs}}^{\text{S}\%}\left({y}_{+}/{y}_{+,\text{org}}\right)\text{exp}\left(f\text{dep}\right)$. Also, the condition of dep = 0 V gives
${K}_{\text{D},{\text{BPh}}_{\text{4}}}^{\text{S}}={K}_{\text{D},{\text{BPh}}_{\text{4}}}^{\text{S}\%}\left({y}_{-}/{y}_{-,\text{org}}\right)$. 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
${K}_{\text{D},\text{A}}^{\text{S}}$ (or
${K}_{\text{D},\text{M}}^{\text{S}}$ ), 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
${\text{BPh}}_{4}^{-}$ is the standard material in the
${\text{dep}}_{j}^{{0}^{\prime}}$ 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
${K}_{\text{D},\text{M}}^{\text{S}}$ or
${K}_{\text{D},\text{A}}^{\text{S}}$ 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
${K}_{\text{D},\text{M}}^{\text{S}\%}$,
${K}_{\text{D},\text{M}}^{\text{S}u/0}$, or
${K}_{\text{D},\text{M}}^{\text{S}0/x}$ 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
${K}_{\text{D},\text{A}}^{\text{S}\%}$ determination was smaller than that of the dep term at least. This result indicates that the
$\mathrm{log}\left({K}_{\text{D},\text{A}}^{\text{expl}.\text{1}}/{K}_{\text{D},\text{A}}^{\text{expl}.2}\right)$ 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.

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)
${K}_{\text{D},\pm}^{2}={K}_{\text{D},+}{K}_{\text{D},}{}_{-}$.

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

${\text{dep}}_{+}^{0}{}^{\prime}+\left(2.303/f\right)\mathrm{log}{K}_{\text{D},+}={\text{dep}}_{-}^{0}{}^{\prime}-\left(2.303/f\right)\mathrm{log}{K}_{\text{D},}{}_{-}$ (A1)

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

$\left(2.303/f\right)\mathrm{log}{K}_{\text{D},\pm}=\left({\text{dep}}_{-}^{0}{}^{\prime}-{\text{dep}}_{+}^{0}{}^{\prime}\right)/2$ (A2)

(B) Derivation of another equation based on (C2). Similarly, using $\left(2.303/f\right)\mathrm{log}{K}_{\text{D},-}^{\text{S}}={\text{dep}}_{-}^{0}{}^{\prime}$, we rearranged Equation (3) as

$\left(2.303/f\right)\mathrm{log}{K}_{\text{D},}{}_{-}=\left(2.303/f\right)\mathrm{log}{K}_{\text{D},+}={\text{dep}}_{-}^{0}{}^{\prime}-{\text{dep}}_{-}.$ (A3)

Introducing Equation (A3) in ${\text{dep}}_{+}={\text{dep}}_{+}^{0}{}^{\prime}+\left(2.303/f\right)\mathrm{log}{K}_{\text{D},+}$ {another expression of Equation (3)}, we can immediately obtain ${\text{dep}}_{+}={\text{dep}}_{+}^{0}{}^{\prime}+{\text{dep}}_{-}^{0}{}^{\prime}-{\text{dep}}_{-}$ under the condition of (C2). Rearranging this equation based on (C1) can yield

${\text{dep}}_{+}={\text{dep}}_{-}=\left({\text{dep}}_{+}^{0}{}^{\prime}+{\text{dep}}_{-}^{0}{}^{\prime}\right)/2.$ (A4)

Here, we define
$\left({\text{dep}}_{+}^{0}{}^{\prime}+{\text{dep}}_{-}^{0}{}^{\prime}\right)/2$ 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

${\text{dep}}_{\pm}={\text{dep}}_{-}^{0}{}^{\prime}-\left(2.303/f\right)\mathrm{log}{K}_{\text{D},\pm}.$ (A5)

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

${\text{dep}}_{\pm}={\text{dep}}_{+}^{0}{}^{\prime}+\left(2.303/f\right)\mathrm{log}{K}_{\text{D},\pm}.$ (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
${\text{dep}}_{-}^{0}{}^{\prime}=\left(2.303/f\right)\mathrm{log}{K}_{\text{D},-}^{\text{S}}$ and
${\text{dep}}_{+}^{0}{}^{\prime}=-\left(2.303/f\right)\mathrm{log}{K}_{\text{D},+}^{\text{S}}$.

Appendix B

The I_{o}_{DCBz} value for the oDCBz solution in 0.01 mol/L CA and the I value for the 0.0035 mol/L Li_{2}SO_{4} 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
${\text{C}}_{\text{org}}^{+}+{\text{A}}_{\text{org}}^{-}\rightleftharpoons {\text{CA}}_{\text{org}}$ in the oDCBz (= org) solution of 0.01 mol/L CA^{ }at 295 K has been reported to be 2 × 10^{3} L/mol from conductivity data [5]. From the quadratic equation for [C^{+}]_{org} (= [A^{−}]_{org}), therefore, we obtained

${\left[{\text{C}}^{+}\right]}_{\text{org}}/\text{mol}\cdot {\text{L}}^{-\text{1}}=\left\{{\left(\text{1}+0.04{K}_{\text{CA},\text{org}}\right)}^{1/2}-\text{1}\right\}/2{K}_{\text{CA},\text{org}}=0.0020$ (A7)

with K_{CA} = 2 × 10^{3}. This [C^{+}]_{org} value basically equals the I_{o}_{DCBz} one.

Similarly, the association constant (
${K}_{{\text{LiSO}}_{\text{4}}}$ ) for
${\text{Li}}^{+}+{\text{SO}}_{4}^{2-}\rightleftharpoons {\text{LiSO}}_{4}^{-}$ 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,

$\left[{\text{Li}}^{+}\right]/\text{mol}\cdot {\text{L}}^{-\text{1}}\approx \left\{{\left(\text{1}+0.0140{K}_{{\text{LiSO}}_{\text{4}}}\right)}^{1/2}-\text{1}\right\}/2{K}_{{\text{LiSO}}_{\text{4}}}={0.0033}_{5}\approx \left[{\text{SO}}_{4}^{2-}\right]$ (A8)

with
${K}_{{\text{LiSO}}_{\text{4}}}\approx 13\text{\hspace{0.17em}}\text{L}/\text{mol}$ and I ≈ 0.010_{2} mol/L under the condition of [LiSO_{4}]_{t} = 0.0035 mol/L [24] in the w phase at 298 K.

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

$\mathrm{log}{K}_{\text{D},\text{Pic}}^{\%}\approx \mathrm{log}{K}_{\text{D},\text{Pic}}^{u/x}+Af\left(x\right)-{A}_{\text{org}}{\left(u\right)}^{1/2}\approx \mathrm{log}{K}_{\text{D},\text{Pic}}^{\%}-16.90v$ (A9)

holds in this case at 298 K. Using x ≈ 0.010_{2} mol/L and u = 0.0020 with b = 0.3 for the oDCBz systems, we immediately obtained
$\mathrm{log}{K}_{\text{D},\text{Pic}}^{\%}\approx \mathrm{log}{K}_{\text{D},\text{Pic}}^{0.002/0.01}-0.{\text{46}}_{0}=-\text{2}.\text{277}-0.{\text{46}}_{0}=-\text{2}.{\text{73}}_{\text{7}}$. This value was assumed to be that at I and I_{o}_{DCBz} → 0 (see the text) and then employed for the
$\mathrm{log}{K}_{\text{D},\text{M}}^{\%}$ evaluation with
$\mathrm{log}{K}_{\text{D},\text{M}}^{\%}=2\mathrm{log}{K}_{\text{D},\pm}-\mathrm{log}{K}_{\text{D},\text{Pic}}^{\%}=2\mathrm{log}{K}_{\text{D},\pm}+\text{2}.{\text{73}}_{\text{7}}$ in this study. Also, the dep values at 298 K in Table 2 were calculated from the rearranged equation of Equation (3a):

$\text{dep}=0.05916\left(\mathrm{log}{K}_{\text{D},}{}_{\pm}-\mathrm{log}{K}_{\text{D},\text{M}}^{\text{S}\%}\right).$ (A10)

Appendix C

As similar to Appendix B, the I and I_{DCE} values for the w(1 mol/L MgSO_{4})/DCE(0.05 CVBPh_{4}) system were evaluated. The thermodynamic association constant (
${K}_{\text{MA}}^{0}$ ) for
${\text{Mg}}^{\text{2}+}+{\text{SO}}_{4}^{2-}\rightleftharpoons {\text{MgSO}}_{\text{4}}$ (=MgA) in water at 298 K has been reported to be 135 L/mol [24]. With the successive approximation method, its [Mg^{2+}] (=[
${\text{SO}}_{4}^{2-}$ ]) in the total concentration, [MgSO_{4}]_{t} = 1 mol/L [20], can be evaluated to be 0.21_{7} mol/L, which was calculated from the equation

$\left[{\text{Mg}}^{\text{2}+}\right]=\left\{{\left(\text{1}+4{K}_{\text{MgA}}\right)}^{1/2}-\text{1}\right\}/2{K}_{\text{MgA}}.$ (A11)

Consequently, the I (=4[Mg^{2+}]) value of the aqueous
${\text{BPh}}_{4}^{-}$ solution with 1 mol/L MgSO_{4} became 0.86_{7} mol/L at which K_{MgA} was estimated to be 16.7 L/mol. In this computation, the K_{MgA} value was evaluated from
$\mathrm{log}{K}_{\text{MgA}}=\mathrm{log}{K}_{\text{MgA}}^{0}-\text{2}\times 0.\text{5114}\times {\left(+\text{2}\right)}^{\text{2}}\times f\left(I\right)$. Accordingly, logy_{−} = −0.114 at I = 0.86_{7} was approximately obtained from
$-0.5114\times {\left(-1\right)}^{2}\times \left\{{I}^{1/2}/\left(1+{I}^{1/2}\right)-0.3I\right\}$ for the
${\text{BPh}}_{4}^{-}$ solution. Here, the symbol K_{MgA} denotes the concentration equilibrium constant. The estimated log y_{−} value suggests the ion-pair formation of
${\text{BPh}}_{4}^{-}$ in water.

Similarly, the association constant (K_{CVA,DCE}) for
${\text{CV}}_{\text{DCE}}^{+}+{\text{A}}_{\text{DCE}}^{-}\rightleftharpoons {\text{CVA}}_{\text{DCE}}$ in the DCE solution of 0.05 mol/L crystal violet cation CV^{+} with
${\text{A}}^{-}={\text{BPh}}_{4}^{-}$ at 298 K has been reported to be 560 L/mol [20]. Therefore,

$\begin{array}{l}{\left[{\text{CV}}^{+}\right]}_{\text{DCE}}/\text{mol}\cdot {\text{L}}^{-\text{1}}={\left[{\text{A}}^{-}\right]}_{\text{DCE}}\\ =\left\{{\left(\text{1}+0.20{K}_{\text{CVA},\text{DCE}}\right)}^{1/2}-\text{1}\right\}/2{K}_{\text{CVA},\text{DCE}}=0.00{\text{86}}_{0}\end{array}$ (A12)

which equals the I_{DCE} value.

Conflicts of Interest

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

[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. (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° 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°C and 45°C. Bulletin of the Chemical Society of Japan, 46, 106-109. https://doi.org/10.1246/bcsj.46.106 |

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