УТВОРЕННЯ ПОДВІЙНОГО ЕЛЕКТРИЧНОГО ШАРУ В КИСЛИХ ТА НЕЙТРАЛЬНИХ ВОДНИХ РОЗЧИНАХ НА 3–5 dM-МЕТАЛАХ
The rate-limiting steps of the electrolysis of water solution, taking into account hydrogen evolution overpotential were considered. A functional relationship between the electrical resistivity of 3–5 dm metals and their quantization energy of atomic electrons, as well as the coordination of metal a...
Збережено в:
| Дата: | 2021 |
|---|---|
| Автори: | , , |
| Формат: | Стаття |
| Мова: | Англійська |
| Опубліковано: |
V.I.Vernadsky Institute of General and Inorganic Chemistry
2021
|
| Онлайн доступ: | https://ucj.org.ua/index.php/journal/article/view/278 |
| Теги: |
Додати тег
Немає тегів, Будьте першим, хто поставить тег для цього запису!
|
| Назва журналу: | Ukrainian Chemistry Journal |
| Завантажити файл: |  |
Репозитарії
Ukrainian Chemistry Journal| _version_ | 1871465683935559680 |
|---|---|
| author | Fedorenko, Oleksandr Fedorenko, Andrey Pershina, Katherine |
| author_facet | Fedorenko, Oleksandr Fedorenko, Andrey Pershina, Katherine |
| author_institution_txt_mv | [
{
"author": "Oleksandr Fedorenko",
"institution": "V. I. Vernadskii Taurida National University, Dzhona Makkeina St., 33, Kyiv 01042, Ukraine"
},
{
"author": "Andrey Fedorenko",
"institution": "1V. I. Vernadskii Taurida National University, Dzhona Makkeina St., 33, Kyiv 01042, Ukraine"
},
{
"author": "Katherine Pershina",
"institution": "Vernadsky Institute of General and Inorganic Chemistry N.A.S of Ukraine, Kiev, Palladin av., 32\/34,03142 Ukraine"
}
] |
| author_sort | Fedorenko, Oleksandr |
| baseUrl_str | https://ucj.org.ua/index.php/journal/oai |
| collection | OJS |
| datestamp_date | 2026-07-22T08:23:45Z |
| description | The rate-limiting steps of the electrolysis of water solution, taking into account hydrogen evolution overpotential were considered. A functional relationship between the electrical resistivity of 3–5 dm metals and their quantization energy of atomic electrons, as well as the coordination of metal atoms and hydrogen compounds, has been revealed. The rule of selecting effective metals for cathodes has been validated. Based on these rules, a reduction-relay mechanism of the hydrogen migration process in the electrical double layer in the electrochemical reduction of TiO2+ ions to Ti3+ and Fe3+ to Fe2+ in sulfuric acid process solutions for the production of pigment titanium dioxide was proposed. The method of the multistage electrochemical reduction of Fe3+ and [TiO2+ * nH2O] in process solutions for the production of titanium dioxide was design based on this study. |
| doi_str_mv | 10.33609/2708-129X.87.02.2021.87-94 |
| first_indexed | 2025-09-24T17:43:37Z |
| format | Article |
| fulltext |
87
UDK 621.357.12+544.636.2 doi: 10.33609/2708-129X.87.02.2021.87-94
THE FORMATION OF AN ELECTRICAL DOUBLE LAYER IN ACID
AND NEUTRAL WATER SOLUTIONS ON THE 3-5 dm METALS
A. A. Fedorenko1, A. M. Fedorenko1, K. D. Pershina2
1V. I. Vernadskii Taurida National University, Dzhona Makkeina St., 33, Kyiv 01042, Ukraine
2Vernadskii Institute of General and Inorganic Chemistry, Academician Palladin Av., 32/34, Kyiv
03142, Ukraine
e-mail: Pershina@ionc.kiev.ua
The rate-limiting steps of the electrolysis of water solution, taking into account hydrogen
evolution overpotential were considered. A functional relationship between the electrical re-
sistivity of 3–5 dm metals and their quantization energy of atomic electrons, as well as the
coordination of metal atoms and hydrogen compounds, has been revealed. The rule of select-
ing effective metals for cathodes has been validated. Based on these rules, a reduction-relay
mechanism of the hydrogen migration process in the electrical double layer in the electro-
chemical reduction of TiO2+ ions to Ti3+ and Fe3+ to Fe2+ in sulfuric acid process solutions
for the production of pigment titanium dioxide was proposed. The method of the multistage
electrochemical reduction of Fe3+ and [TiO2+ * nH2O] in process solutions for the production
of titanium dioxide was design based on this study.
Key words: double electric layer, hydrogen evolution, cathode, electron transfer, reduc-
tion-relay mechanism.
INRTRODUCNION When improving the
sulfate technology for the production of pig-
ment titanium dioxide with the replacement
of the chemical reduction of Fe3+ ions to Fe2+
and Ti4+ to Ti3+ with scrap iron and powdered
aluminum by the electrochemical method, se-
rious problems arose as to the processes oc-
curring at different cathodes in the electrical
double layer (EDL) [1–5]. This especially con-
cerns the electrochemical processes of Fe3+
and [TiO2+*nH2O] ion reduction in sulfu-
ric acid process solutions with pH = 2.5-3.0.
In this particular case, the use of the theoreti-
cal fundamentals of electrochemistry in prac-
tice turned out to be very difficult, especially
when using the theory of EDL structure [3].
This primarily concerns the Volmer discharge
and Heyrovsky electrochemical desorption
stages, which are based on introducing the hy-
droxonium ion (H+-OH2) into near-cathode
electrochemical processes, and based on these
concepts, the contradictory slow discharge (SD)
theory has been developed. In this theory, it is
considered that a significant part of the ener-
gy is spent on the rupture of the bond between
H+ and H2O [4, 6–8]. In the book “Double
Layer Theory” [9], published in 2015, no an-
swers as to the use of the EDL theory in applied
PHISICAL CHEMISTRY THE FORMATION OF AN ELECTRICAL DOUBLE LAYER IN ACID AND NEUTRAL WATER SOLUTIONS ON THE 3-5 dm METALS
88 ISSN 2708-129X. Укр. хім. журн., 2021
electrochemistry have been unfortunately
found. Moreover, neither the recombination
theory of hydrogen evolution overpotential (ηH)
nor the SD theory is universal. For the metals
with high hydrogen adsorption energy, a lower
ηH is observed; therefore, it is recommended to
use the recombination theory, and for the metals
with lower adsorption, where ηH takes on higher
values, the SD theory is recommended, the use
of which sometimes gives rise to very contradic-
tory results. There are also questions as to the
description of the hydrogen recombination step
(Tafel reaction) 2Hads→H2, i.e. hydrogen moliza-
tion at the cathode. The complete analysis with
using the mathematical analysis of the EDL
taking into account the Debye screening length
considering heat energy at 298.15 0 K, and tak-
ing into account the following factors (the role
of the hydroxonium ion in the Helmholtz cath-
ode layer, the dependence between of η H and
the electrical resistivity of nd m metals, the im-
pact of the complexing ability of nd m metals to
hydrogen, impact of the cathode materials and
their chemical composition, detection the mech-
anism of electron transfer from the cathode to
the solution the above questions should make it
possible to reveal the conditions of the intensi-
fication of electrochemical reduction processes
of compounds in acid and neutral solutions.
EXPERIMENT AND DISCUSSION OF THE
RESULTS. The experimental investigations:
measuring and recording instruments: KEL 1M,
Shch300.1, Shch1413 conductometers, a digital
camera (Kodak Easu Share C 142), a Ts1241
thermostat. Reagents and materials: chemical-
ly pure sulfuric acid, bidistilled water, smooth
platinum of 99.99 purity, NBR-0 niobium,
S-0 lead.
Theoretical and experimental investigations
have been carried out to make corrections in the
electrolysis theories and concepts of the EDL
developed earlier. This primarily concerns the
role of the hydroxonium ion and its effect on in-
crease in ηH. Here, attention should be paid to
the dissociation of the complex ion H3O
+:
In the eq. (1) the logarithm of the constant
pKa = -1.7011; it follows that the equilibrium
is shifted to the right, and that it displays the
properties of a medium acid, which decom-
poses spontaneously into ions. Besides, the re-
search carried out by Conway, Borkis and Lin-
ton (1956) to determine the stability of H3O
+,
which was, in terms of time, 0.024 x 10-12 s,
should be taken into consideration [6]. Sub-
sequent research to determine the lifetime of
H3O
+ was carried out by the scientist Meiboom
in 1961 by the NMR method at 298.15 o K,
which was 1.7 x 10-12 s. In the opinion of the
above scientists, such a low stability of the
species H3O
+ does not allow it to move inde-
pendently in water (the mobility of H2O is
3.62 x 10-3 cm2V-1s-1) as a structural unit, and
the very high mobility of H+ is due solely to
proton exchange. In this particular case, in the
presence of polarization of water molecules, the
proton is transferred along a chain of hydrogen
bonds by the Grotthuss relay mechanism. The
presence of the independent species H3O
+ in
water is also ruled out because of the formation
of hydrogen bonds of neighboring molecules to
it [10, 12], i.e. the formation of [H+…(OH2)n],
where n ≥ 2. When a potential is applied in elec-
trolysis, the H+ ions will be the first to reach the
cathode surface because at the equal positive
charges of H+ and H3O
+, the positive charge of
the latter species will be smaller because of its loss
by electrostatic interaction between water and
proton dipoles. Besides, the mass of H+ ≈ 1 µu
UCJ № 2 / Vol. 87A. A. Fedorenko, A. M. Fedorenko, K. D. Pershina
89https://ucj.org.ua
should be taken into account, and the mass of
H3O
+ is 19 times larger. It follows that H3O
+ is
a more inert species. Research has been carried
out to determine the functional dependence of
hydrogen evolution overpotential (ηH) on the
electrical resistivity of ndm metals [13]. Based
on electron energy quantization and the theory
of the chemistry of coordination compounds
[13, 14], a well-defined functional dependence
of ηH for 3dm, 4dm and 5dm transition metals
on the electron occupancy of dm orbitals is re-
vealed. This dependence for 3dm elements is
shown in Figs 1 and 2.
Fig 1. Dependence of electrical resistivity (ρ) on
the electron occupancy of 3dm orbitals.
Fig 2. Dependence of hydrogen evolution over-
potential on the electron occupancy of 3dm4sn
orbitals.
When comparing the plots in Figs 1 and 2,
within filling the orbitals with 1 to 10 elec-
trons, an analogous (symbatic) behavior of the
curves is observed, which corroborates this de-
pendence. For the p electrons of large-period
atoms, an antibatic behavior of the curves is
observed; therefore, it is recommended to use
the electronegativity (EN) of elements relative
to ENH = 2.1. A decrease in ηH is observed only
if ENH < 2.1.
For the d elements, the theory of the che
mistry of coordination compounds should
be taken into account, on the basis of which
it becomes possible to explain the causes of
the decrease in ηH. First of all, the ndm me
tals must be divided into two groups: I, metals
with filled orbitals, where m = 1–8 electrons;
II, metals with ndm sublevels filled with up
to 10 electrons. Group I includes metals with
specific adsorption (chemisorption), which is
characterized by a high hydrogen adsorption
energy (solid solutions) and manifests itself by
a decrease in ηH in electrolysis, and group II
includes metals with low hydrogen adsorption
energy, which results from electrostatic forces.
Therefore, these metals possess a higher ηH va
lue. The manifestation of specific adsorption is
observed in the case of the presence of unoccu-
pied orbitals or unpaired electrons on the orbi
tals of ndm metals. This results in the formation
of shared pairs between the metal and hydrogen
compounds according to the scheme:
(1)
(2)
(3)
(4)
PHISICAL CHEMISTRY THE FORMATION OF AN ELECTRICAL DOUBLE LAYER IN ACID AND NEUTRAL WATER SOLUTIONS ON THE 3-5 dm METALS
90 ISSN 2708-129X. Укр. хім. журн., 2021
The products of reactions (1) and (2) appear
because of the formation of an electric field
intensity by an electron, which reaches tens of
millions of volts per centimeter at a distance of
1.0 nm. This results in the appearance of atom-
ic hydrogen, followed by its deformation po-
larization and the formation of a hydride ion.
The cause of decrease in ηH of group I met-
als is explained by the theory of coordination
compounds . Consider this decrease for the
55.849Fe metal as an example:
As a result of interaction between Fe and H-,
in view of (3) and (4), the electronic configura-
tion of the iron atom, 3d6 (term 5D4), changes
into 3d8 (term 3F4); thus, Fe takes on the config-
uration of nickel, which has minimum ρ values
(Fig 1) and the same ηH value (Fig 2). It is pro-
posed to consider, as an example, a brass alloy
(ω, %: Cu, 60; Zn, 40): electronic configura-
tion of atoms (ECA) (Cu, 3d104s1; Zn, 3d104s2);
ρbrass * 106 * Ω * cm = 6.81; the activity of metals for
coordination to hydrogen is low (group II). Ex-
ample with polymetallic steel (12Kh18N10T):
ECA (Cr, 3d54s1; Ni, 3d84s2); ρsteel * 106 * Ω * cm =
70–75; they interact actively with hydrogen
(I). From the above information it follows that
ρbrass is 10 times lower than ρ of 12Kh18N10T.
However, when determining ηH, the Tafel
constant for brass at 50 oC a = -1.02, the ex-
change current j0 = 6.8 x 10-9 A/cm2, and for
12Kh18N10T, a = 0.87, j0 = 6.5 x 10-8 A/cm2;
therefore, it is better to use steels containing
ndm metals with m < 10 and Pd with double
dip of electrons.
Thus, the chief thing is that the formation
of a H- coordination bond to the metals Fe,
Cr, Ni contained in the cathode surface took
place, which affected greatly the electron
transfer from the cathode to the EDL satu-
rated with unreduced hydrogen compounds.
The following compounds are meant in the
first place: H+, H2
+ (Dc = 2.80 eV), H3
+ (Dc =
3.04 eV), H4
+ (Dc = 1.10 eV), where Dc is the
dissociation energy. The reason of the variety
of the compounds of H0 is its relatively high
electronegativity (EN(H) = 2.10; for compari-
son, EN(F) = 3.98), which provides filling its
inert gas (He) type electron shell. Among
100 elements of the periodic table with estab-
lished EN, EN(H) predominates in 77 of them;
most of them reveal the formation of various
hydride compounds.
When there is a potential at the cathode
in the presence of electrostatic and specific
adsorption, the following processes can oc-
cur simultaneously in the Helmholtz layer:
[e-]c * H+ = H0; (2) H0 + H+ → H2
+; (3) [e-]c * H0 → H-;
(4) H- + H+ → H2; (5) H0 + H0 → H2; (6) H2 + H+ → H3
+;
(7) H3
+ → H2
+ + H0; (8) H4
+ → H3
+ + H0; (9) H- +
H0 → H2
-, where [e-]c is the cathode. The series
of hydrogen transformations has been made
up on the basis of an extensive review of publi-
cations and experimental data. The presence of
species directly at the cathode surface with the
manifestation of pronounced specific adsorp-
tion in electrochemical processes is determin-
ing in ηH decrease and the reduction of Fe3+,
[TiO2+ * nH2O].
The hydrogen species H-, H2
-, H0, H+, H2
+
are involved to a greater extent in these pro-
cesses; this manifests itself especially when
the electron is transferred from the cathode
via the hydride ion along a reduction-relay
chain by means of a molecular hydrogen ion
(Ha
0-Hb
+). In view of quantum mechanics, the
transfer of a single electron in the molecular
ion (Ha
0-Hb
+) occurs owing to electron oscil-
UCJ № 2 / Vol. 87A. A. Fedorenko, A. M. Fedorenko, K. D. Pershina
91https://ucj.org.ua
lation between two nuclei. This state is more
fully described by the resonance integral
Hab = Hba = ∫ϕaHϕb dτ = ∫ϕbHϕadτ, which is
a ground for creating a theory of the reduc-
tion-relay mechanism of H+ reduction and
electron transfer to the acceptor. To confirm
these judgments, the systems H2SO4-H2O (I*)
and H2SO4-TiOSO4-H2O(II*) with the same
pH = 0.87 (Fig 3) have been investigated. Nb
metal [14, 15] and 12Kh18N10T steel were
used as the cathodes, and a 12Kh18N10T mesh
coated with a MnO2(therm) multilayer coating
was used as the anodes (Fig 3).
Fig 3. Dependence of voltage on the solution
temperature in the systems:
(12Kh18N10T)(c)-(MnO2)(a)-H2SO4- H2O (I*)
(12Kh18N10T)(c)-(MnO2)(a)-TiOSO4-H2SO4-H2O
(II*)
As a result of investigating the systems I*
and II* (Fig 3), a functional dependence of
voltage on temperature (25–60 o C) has been
established; a noticeable decrease in voltage in
the systems is clearly visible. In the system II*,
however, this decrease is more noticeable be-
cause of electron transfer by the reduction-re-
lay mechanism via the ions H-, H2
+, etc, to the
acceptor cation [TiO2+ * nH2O]. In the electro
lysis in the system I*, the rate-limiting step
of the H+ reduction process is the molization
H0 + H0 = H2, which is hindered by the pres-
ence in the Helmholtz layer of molecular spe-
cies H2
+, H3
+, etc, which affect the cathode po-
tential. However, this state is favorable for elec-
tron transfer to the acceptor.
The process of electrochemical reduction
of [TiO2+ * nH2O] in the Gouy layer is con-
firmed by a thermal effect, measured directly
on the Nb cathode. During hydrogen reduc-
tion in the systems I*-Nb and II*-Nb, the sen-
sors recorded small heat energy changes of
∆t = 0.188 oC (I*-Nb) and 0.334 oC (II*-Nb),
which is unexpected since during hydrogen
recombination and molization, an energy of
18.1 eV is released. In view of this, a calcu-
lation taking into account the change ∆t, the
heat capacity of the niobium cathode (15 μm
foil), the heat capacity and heat conductivity
of adsorbed hydrogen on the cathode and a
determination of the size of the fixed Helm-
holtz layer have been performed. When pro-
cessing the experimental data on hydrogen
reduction in the system I*-Nb, it turned out
that the experimental heat energy (Qexp) was
9.5 x 1016 eV, and the theoretical heat ener-
gy (Qtheor) with allowance for release at the
cathode must be 5.4 x 1021 eV, i.e. 5.6 x 104
times as high. Thus, the ion reduction pro-
cess occurs outside the cathode, i.e. at some
distance from it. To determine the size of the
Helmholtz layer, quantum-mechanical calcu-
lations have been made to establish the de-
pendence of the Debye screening length of
electrode potential on the concentration of
solutions (Fig 4). The number of hydrogen
species on the cathode surface has been de-
termined taking into account the heat energy
of 0.013 eV at 298.15 oK.
PHISICAL CHEMISTRY THE FORMATION OF AN ELECTRICAL DOUBLE LAYER IN ACID AND NEUTRAL WATER SOLUTIONS ON THE 3-5 dm METALS
92 ISSN 2708-129X. Укр. хім. журн., 2021
Fig 4. Electric potential distribution in the catho
de region for H+ ion concentration values (ω, % =
0.1–10) in sulfuric acid solutions at 298.15 oK.
In view of Fig 4, the electrochemical re-
duction of Fe3+ and [TiO2+ * nH2O] in process
solutions for the production of titanium di-
oxide should be performed in the presence of
5.0–10.0 % sulfuric acid in multistage electro-
lyzers (Fig 5), for at these concentrations, the
thinnest fixed Helmholtz layer with a thickness
of 2–3 hydrogen species is formed. The basic
diagram of a multistage electrolyzer is shown
in Fig 5.
This electrolyzer provides an accelerat-
ed electron transfer from the cathode to the
electron acceptors, with the reduction ener-
gy (Qexp) increasing to 1.6 x 1017 eV (system
B*-Nb). Hence the electrochemical reduction
process is carried out with maximum values
of convective diffusion in the Gouy layer. The
group I ndm metals must be used for the catho
de materials, but still more effective results are
achieved when using their alloys because be-
sides the existence of specific adsorption, the
property of the hydrogen evolution synergism
manifests itself.
Fig 5. Basic diagram of a multistage electro-
lyzer: (1) electrolyzer body, (2) mesh cathode,
(3) anode, (4) membrane, (5) direction of elec-
trolyte movement, (6) electrolyte drain cock,
(7) electrolyzer cover, (8, 9) gas outlet tube of
the anode and cathode, (10) electrolyte level,
(11) cock.
Conclusions
A method for identifying promising met-
als and their alloys for cathodes based on the
electrical resistivity of ndm metals and the
theory of the chemistry of coordination com-
pounds has been proposed. The factors af-
fecting the hydrogen evolution overpotential
in the EDL have been determined based on
quantum-mechanical calculations. A model
of the reduction-relay mechanism of electron
transfer from the cathode to the Helmholtz
EDL , followed by electron migration into the
Gouy slip layer and to the electron acceptors
(Fe3+, [TiO2+ * nH2O], H+, etc), has been pro-
posed. Thermal effects on the cathode have
been studied, which support the mechanism
of electron transfer under hydrogen reduc-
tion and the reduction of ions in the Helm-
holtz layer (H+) and in the Gouy layer (H+,
UCJ № 2 / Vol. 87A. A. Fedorenko, A. M. Fedorenko, K. D. Pershina
93https://ucj.org.ua
[TiO2+ * nH2O]), Fe3+, etc. The method of the
multistage electrochemical reduction of Fe3+
and [TiO2+ * nH2O] in process solutions for
the production of titanium dioxide was de-
signed based on this study.
The work was done under finan
cial support of the Ministry of Edu
cation and Science of Ukraine ac
cording themes: «Development of
basics of solution chemistry, improvement
of chemical-technological processes, study
of structure, physicochemical properties
and methods of analysis of natural sorbents,
biopolymers, glycosides, food, winemaking
and food impurities» (DR № 0106U003194);
«Improvement of chemical-technological
processes; study of physicochemical pro
perties of coordination compounds, natu
ral zeolites, bentonites, plant enzymes,
glycosides, polysaccharides and obtaining
nanocomposite materials based on them
«(DR № 0111U000644).
УТВОРЕННЯ ПОДВІЙНОГО ЕЛЕКТРИЧНОГО
ШАРУ В КИСЛИХ ТА НЕЙТРАЛЬНИХ ВОДНИХ
РОЗЧИНАХ НА 3–5 dM-МЕТАЛАХ
Федоренко А. А.1, Першина К. Д.2,
Федоренко А. М.1
1Таврійський національний університет
ім. В. І. Вернадського, вул. Джона Маккейна,
33, Київ 01042, Україна
2Інститут загальної та неорганічної хімії
ім. В. І. Вернадського, просп. Акад. Палладі-
на 32/34, Київ 03142, Україна
e-mail:Pershina@ionc.kiev.ua
Розглянуто стадії електролізу розчинів у
водних розчинниках, що впливають на об-
меження швидкості електрохімічної реакції
з урахуванням потенціалу перенапруги ви-
ділення водню. Виявлено функціональний
взаємозв’язок між електричним опором ме-
талів 3–5 дм та енергією квантування їхніх
атомних електронів, а також координацією
атомів металів та сполук водню. Встановле-
но правило вибору ефективних металів для
катодів. Виходячи з цього правила, було
запропоновано реле-редукційний меха-
нізм процесу міграції водню в подвійному
електричному шарі при електрохімічному
відновленні іонів TiO2
+ до Ti3+ і Fe3+ до Fe2+
у технологічних розчинах сірчаної кислоти
для отримання пігменту діоксиду титану.
На основі цього дослідження було розроб
лено метод багатоступеневого електро
хімічного відновлення Fe3+ і [TiO2
+ * nH2O]
у технологічних розчинах для отримання
діоксиду титану.
Ключові слова: подвійний електрич-
ний шар, виділення водню, 3–5 dm-метали,
катод, перенесення електрону, редукцій-
но-естафетний механізм.
PHISICAL CHEMISTRY THE FORMATION OF AN ELECTRICAL DOUBLE LAYER IN ACID AND NEUTRAL WATER SOLUTIONS ON THE 3-5 dm METALS
94 ISSN 2708-129X. Укр. хім. журн., 2021
REFERENCES
1. Skomoroha V.M., Zarechnyj V.G., Voro
b’eva I.P., Vakal S.V. Proizvodstvo dvuokisi
titana sul’fatnym sposobom. Sumy : ATZT
«Arsenal press». 2002. 204 p. (In Russian).
2. Antropov L.І. Teoreticheskaya elektrohi
miya. K.: Lybid’. 1993. 544 p. (In Russian)
3. Fedorenko A.M., Fedorenko A.A. . Quan-
tum theory of electronic conductivity of
substances and problems of electroche
mistry. Simferopol’: IP Baranovskiy A.E. RF
Respublika Krym. 2019. 200 p. (In Russian)
4. Fetter K. Electrochemical kinetics. M.:
Khimiya. 1967. 856 p. (In Germany)
5. Pershina, E.D., Karpushin, N.A. & Ka-
zdobin, K.A. Aluminosilicate conductivity
at the presence of water. Surf. Engin. Appl.
Electrochem. 2010. 46: 339–347.
https://doi.org/10.3103/S1068375510040083
6. Bockris J. O’M. and Reddy A. K. N.. Mo
dern Electrochemistry 1:Ionics. Plenum
Press, New York. 1998.
7. Henderson, D., & Boda, D. Insights from
theory and simulation on the electrical
double layer. Physical Chemistry Chemical
Physics. 2009. 11(20): 3822–3830.
DOI: 10.1039/b815946g
8. Skorchelletti V.V. Theoretical electroche
mistry. Leningrad: Khimiya. 1974. (In Rus-
sian)
9. Salem R.R. Double layer theory. Moscow:
Fizmatlit. 2015. (In Russian)
10. Zatsepina G.N. Properties and structure
of water. Moscow: Moscow State University
Press. 1974. (In Russian)
11. Pershina, E.D., Kazdobin, K.A. Conducti
vity of water media as an alternative of
electronic and ionic transfer. J. Water
Chem. Technol. 2008. 30: 358–367.
https://doi.org/10.3103/S1063455X0806
0052
12. Pershina, E.D., Kokhanenko, V.V., Mas
lyuk, L.N. et al. Conductivity of aqueous
suspensions of alumosilicates. Surf. Engin.
Appl.Electrochem. 2011. 47: 441–445.
https://doi.org/10.3103/S1068375511050176
13. Kotton F., Uilkinson Dzh. Sovremennaya
neorganicheskaya himiya chast’. 1. M.: Mir.
1969. 224 p. (In Russian)
14. Henrici-Olive G., Olive S. Coordination
and catalysis. Moscow: Mir. 1980. (In Rus-
sian)
15. Bairachnyi B.I., Fedorenko A.A., Tul-
skii G.G. et al. Resursosberegayushchie
elektrohimicheskie processy v proiz
vodstve pigmentnogo dioksida titana.
Zhurnal prikladnoj himii. 2013. 86(7):
1069–1073. (In Russian)
Стаття надійшла 14.02.2020.
|
| id | oai:ojs2.1444248.nisspano.web.hosting-test.net:article-278 |
| institution | Ukrainian Chemistry Journal |
| keywords_txt_mv | keywords |
| language | English |
| last_indexed | 2026-07-23T01:05:56Z |
| publishDate | 2021 |
| publisher | V.I.Vernadsky Institute of General and Inorganic Chemistry |
| record_format | ojs |
| resource_txt_mv | ucjorgua/f1/54aabc210b13b0fb3af2d469e4c846f1.pdf |
| spelling | oai:ojs2.1444248.nisspano.web.hosting-test.net:article-2782026-07-22T08:23:45Z THE FORMATION OF AN ELECTRICAL DOUBLE LAYER IN ACID AND NEUTRAL WATER SOLUTIONS ON THE 3-5 dm METALS УТВОРЕННЯ ПОДВІЙНОГО ЕЛЕКТРИЧНОГО ШАРУ В КИСЛИХ ТА НЕЙТРАЛЬНИХ ВОДНИХ РОЗЧИНАХ НА 3–5 dM-МЕТАЛАХ Fedorenko, Oleksandr Fedorenko, Andrey Pershina, Katherine double electric layer, hydrogen evolution, cathode, electron transfer, reduction-relay mechanism. The rate-limiting steps of the electrolysis of water solution, taking into account hydrogen evolution overpotential were considered. A functional relationship between the electrical resistivity of 3–5 dm metals and their quantization energy of atomic electrons, as well as the coordination of metal atoms and hydrogen compounds, has been revealed. The rule of selecting effective metals for cathodes has been validated. Based on these rules, a reduction-relay mechanism of the hydrogen migration process in the electrical double layer in the electrochemical reduction of TiO2+ ions to Ti3+ and Fe3+ to Fe2+ in sulfuric acid process solutions for the production of pigment titanium dioxide was proposed. The method of the multistage electrochemical reduction of Fe3+ and [TiO2+ * nH2O] in process solutions for the production of titanium dioxide was design based on this study. V.I.Vernadsky Institute of General and Inorganic Chemistry 2021-03-19 Article Article Physical chemistry Физическая xимия Фізична xімія application/pdf https://ucj.org.ua/index.php/journal/article/view/278 10.33609/2708-129X.87.02.2021.87-94 Ukrainian Chemistry Journal; Vol. 87 No. 2 (2021): Ukrainian Chemistry Journal; 87-94 Украинский химический журнал; ##issue.vol## 87 ##issue.no## 2 (2021): Украинский химический журнал; 87-94 Український хімічний журнал; Том 87 № 2 (2021): Український хімічний журнал; 87-94 2708-129X 2708-1281 en https://ucj.org.ua/index.php/journal/article/view/278/155 Copyright (c) 2021 Oleksandr Fedorenko, Andrey Fedorenko, Katherine Pershina https://creativecommons.org/licenses/by-nc/4.0 |
| spellingShingle | Fedorenko, Oleksandr Fedorenko, Andrey Pershina, Katherine УТВОРЕННЯ ПОДВІЙНОГО ЕЛЕКТРИЧНОГО ШАРУ В КИСЛИХ ТА НЕЙТРАЛЬНИХ ВОДНИХ РОЗЧИНАХ НА 3–5 dM-МЕТАЛАХ |
| title | УТВОРЕННЯ ПОДВІЙНОГО ЕЛЕКТРИЧНОГО ШАРУ В КИСЛИХ ТА НЕЙТРАЛЬНИХ ВОДНИХ РОЗЧИНАХ НА 3–5 dM-МЕТАЛАХ |
| title_alt | THE FORMATION OF AN ELECTRICAL DOUBLE LAYER IN ACID AND NEUTRAL WATER SOLUTIONS ON THE 3-5 dm METALS |
| title_full | УТВОРЕННЯ ПОДВІЙНОГО ЕЛЕКТРИЧНОГО ШАРУ В КИСЛИХ ТА НЕЙТРАЛЬНИХ ВОДНИХ РОЗЧИНАХ НА 3–5 dM-МЕТАЛАХ |
| title_fullStr | УТВОРЕННЯ ПОДВІЙНОГО ЕЛЕКТРИЧНОГО ШАРУ В КИСЛИХ ТА НЕЙТРАЛЬНИХ ВОДНИХ РОЗЧИНАХ НА 3–5 dM-МЕТАЛАХ |
| title_full_unstemmed | УТВОРЕННЯ ПОДВІЙНОГО ЕЛЕКТРИЧНОГО ШАРУ В КИСЛИХ ТА НЕЙТРАЛЬНИХ ВОДНИХ РОЗЧИНАХ НА 3–5 dM-МЕТАЛАХ |
| title_short | УТВОРЕННЯ ПОДВІЙНОГО ЕЛЕКТРИЧНОГО ШАРУ В КИСЛИХ ТА НЕЙТРАЛЬНИХ ВОДНИХ РОЗЧИНАХ НА 3–5 dM-МЕТАЛАХ |
| title_sort | утворення подвійного електричного шару в кислих та нейтральних водних розчинах на 3–5 dm-металах |
| topic_facet | double electric layer hydrogen evolution cathode electron transfer reduction-relay mechanism. |
| url | https://ucj.org.ua/index.php/journal/article/view/278 |
| work_keys_str_mv | AT fedorenkooleksandr theformationofanelectricaldoublelayerinacidandneutralwatersolutionsonthe35dmmetals AT fedorenkoandrey theformationofanelectricaldoublelayerinacidandneutralwatersolutionsonthe35dmmetals AT pershinakatherine theformationofanelectricaldoublelayerinacidandneutralwatersolutionsonthe35dmmetals AT fedorenkooleksandr utvorennâpodvíjnogoelektričnogošaruvkislihtanejtralʹnihvodnihrozčinahna35dmmetalah AT fedorenkoandrey utvorennâpodvíjnogoelektričnogošaruvkislihtanejtralʹnihvodnihrozčinahna35dmmetalah AT pershinakatherine utvorennâpodvíjnogoelektričnogošaruvkislihtanejtralʹnihvodnihrozčinahna35dmmetalah AT fedorenkooleksandr formationofanelectricaldoublelayerinacidandneutralwatersolutionsonthe35dmmetals AT fedorenkoandrey formationofanelectricaldoublelayerinacidandneutralwatersolutionsonthe35dmmetals AT pershinakatherine formationofanelectricaldoublelayerinacidandneutralwatersolutionsonthe35dmmetals |