Symmetric closure

In electrochemistry, ITIES is an acronym for the "Interface between Two Immiscible Electrolyte Solutions". Usually, one electrolyte is an aqueous electrolyte composed of hydrophilic ions such as NaCl dissolved in water and the other electrolyte is a lipophilic salt such as tetrabutylammonium tetraphenylborate dissolved in an organic solvent immiscible with water such as nitrobenzene, or 1,2-dichloroethane.

An ITIES is an electrochemical interface that is either polarisable or polarised. An ITIES is said polarisable if one can change the Galvani potential difference, or in other words the difference of inner potentials between the two adjacent phases, without noticeably changing the chemical composition of the respective phases (i.e. without noticeable electrochemical reactions taking place at the interface). An ITIES system is said polarised if the distribution of the different charges and redox species between the two phases determines the Galvani potential difference.

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Charge transfer reactions at ITIES

Three major classes of charge transfer reactions can be studied at ITIES:

• Ion transfer reactions.
• Assisted ion transfer reactions.
• Heterogeneous electron transfer reactions.

The Nernst equation for an ion transfer reaction reads

$\Delta _{\text{o}}^{\text{w}}\phi =\phi ^{\text{w}}-\phi ^{\text{o}}=\Delta _{\text{o}}^{\text{w}}\phi _{i}^{\ominus }+{\frac {RT}{z_{i}F}}\ln \left({\frac {a_{i}^{\text{o}}}{a_{i}^{\text{w}}}}\right)$,

where $\Delta _{\text{o}}^{\text{w}}\phi _{i}^{\ominus }$ is the standard transfer potential defined as the Gibbs energy of transfer expressed in a voltage scale.

$\Delta _{\text{o}}^{\text{w}}\phi _{i}^{\ominus }={\frac {\Delta G_{tr,i}^{\ominus ,{\text{w}}\rightarrow {\text{o}}}}{z_{i}F}}$

The Nernst equation for a single heterogeneous electron transfer reaction reads

$\Delta _{\text{o}}^{\text{w}}\phi =\Delta _{\text{o}}^{\text{w}}\phi _{\text{ET}}^{\ominus }+{\frac {RT}{F}}ln\left({\frac {a_{{\text{R}}_{1}}^{\text{w}}a_{{\text{O}}_{2}}^{\text{o}}}{a_{{\text{O}}_{1}}^{\text{w}}a_{{\text{R}}_{2}}^{\text{o}}}}\right)$,

where $\Delta _{o}^{\text{w}}\phi _{\text{ET}}^{\ominus }$ is the standard redox potential for the interfacial transfer of electrons defined as the difference the standard redox potentials of the two redox couples but referred to the aqueous Standard Hydrogen Electrode (SHE).

$\Delta _{\text{o}}^{\text{w}}\phi _{\text{ET}}^{\ominus }=\left[E_{{\text{O}}_{2}/{\text{R}}_{2}}^{\ominus }\right]_{\text{SHE}}^{\text{o}}-\left[E_{{\text{O}}_{1}/{\text{R}}_{1}}^{\ominus }\right]_{\text{SHE}}^{\text{w}}$

Four-Electrode cell

To study charge transfer reactions at ITIES, a 4-electrode cell is used.

Two reference electrodes are used to control the polarisation of the interface, and two counter electrodes made of noble metals are used to pass the current. The aqueous supporting electrolyte must be hydrophilic, such as LiCl, and the organic electrolyte must be lipophilic, such as tetraheptylammonium tetra-pentafluorophenyl borate.

Ion partition coefficient/Ion distribution coefficient

Contrary to a neutral solute, the partition coefficient of an ion depends of the Galvani potential difference between the two phases:

$P_{i}={\frac {a_{i}^{\text{o}}}{a_{i}^{\text{w}}}}=\exp \left[{\frac {z_{i}F}{RT}}(\Delta _{\text{o}}^{\text{w}}\phi -\Delta _{\text{o}}^{\text{w}}\phi _{i}^{\ominus })\right]=P_{i}^{\ominus }\exp \left[{\frac {z_{i}F}{RT}}\Delta _{\text{o}}^{\text{w}}\phi \right]$

Distribution potential

When a salt is distributed between two phases, the Galvani potential difference is called the distribution potential and is obtained from the respective Nernst equations for the cation C+ and the anion A– to read

$\Delta _{\text{o}}^{\text{w}}\phi ={\frac {\Delta _{\text{o}}^{\text{w}}\phi _{\text{C+}}^{\ominus }+\Delta _{\text{o}}^{\text{w}}\phi _{\text{A-}}^{\ominus }}{2}}+{\frac {RT}{2F}}\ln {\left({\frac {\gamma _{\text{C+}}^{\text{o}}\gamma _{\text{A-}}^{\text{w}}}{\gamma _{\text{C+}}^{\text{w}}\gamma _{\text{A-}}^{\text{o}}}}\right)}$

where γ represents the activity coefficient.

See also

• Ionic partition diagram
• Distribution law

References

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