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ARTICLE
Cite as
Nano-Micro Lett.
(2025) 17:51
Received: 30 June 2024
Accepted: 23 September 2024
© The Author(s) 2024
https://doi.org/10.1007/s40820-024-01542-x
Scalable Ir‑Doped
NiFe
2
O
4
/TiO
2
Heterojunction
Anode for Decentralized Saline Wastewater
Treatment and H
2
Production
Sukhwa Hong
1
, Jiseon Kim
1
, Jaebeom Park
1
, Sunmi Im
1
, Michael R. Hoffmann
2
,
Kangwoo Cho
1,2,3
*
HIGHLIGHTS
Ir-doped
NiFe
2
O
4
(NFI) spinel with
TiO
2
heterojunction overlayer brought about outstanding chlorine evolution reaction in circum-
neutral pH.
Electroanalyses including operando X-ray absorption spectroscopy uncovered the active role of
TiO
2
for
Cl
chemisorption.
NFI/TiO
2
anode boosted both
NH
4
+
-to-N
2
conversion and
H
2
generation in wastewater, and the practical applicability was confirmed
with scaled-up anodes and real wastewater.
ABSTRACT
Wastewater electrolysis cells (WECs) for
decentralized wastewater treatment/reuse coupled with
H
2
production can reduce the carbon footprint associated with
transportation of water, waste, and energy carrier. This study
reports Ir-doped
NiFe
2
O
4
(NFI,
~ 5 at% Ir) spinel layer with
TiO
2
overlayer (NFI/TiO
2
), as a scalable heterojunction
anode for direct electrolysis of wastewater with circum-
neutral pH in a single-compartment cell. In dilute (0.1 M)
NaCl solutions, the NFI/TiO
2
marks superior activity and
selectivity for chlorine evolution reaction, outperforming
the benchmark
IrO
2
. Robust operation in near-neutral pH
was confirmed. Electroanalyses including
operando
X-ray
absorption spectroscopy unveiled crucial roles of
TiO
2
which serves both as the primary site for
Cl
chemisorption and a protective layer for NFI as an ohmic contact. Galvanostatic electrolysis
of
NH
4
+
-laden synthetic wastewater demonstrated that NFI/TiO
2
not only achieves quasi-stoichiometric
NH
4
+
-to-N
2
conversion, but also
enhances
H
2
generation efficiency with minimal competing reactions such as reduction of dissolved oxygen and reactive chlorine. The
scaled-up WEC with NFI/TiO
2
was demonstrated for electrolysis of toilet wastewater.
KEYWORDS
Wastewater electrolysis cell; Ir-doped
NiFe
2
O
4
; Reactive chlorine species; Decentralized
H
2
production; On-site
wastewater treatment
*
Kangwoo Cho, kwcho1982@postech.ac.kr
1
Division of Environmental Science and Engineering, Pohang University of Science and Technology (POSTECH), Pohang 790−784, Korea
2
Linde Laboratory, California Institute of Technology, Pasadena, CA 91125, USA
3
Institute for Convergence Research and Education in Advanced Technology (I-CREATE), Yonsei University International Campus, Incheon 21983,
Republic of Korea
Nano-Micro Lett. (2025) 17:51
51
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©
The authors
Abbreviations
EOP
Electrochemical oxidation process
ClER
Chlorine evolution reaction
RCS
Reactive chlorine species
WECs
Wastewater electrolysis cells
HER
Hydrogen evolution reaction
BDD
Boron-doped diamond
OER
Oxygen evolution reaction
NF
NiFe
2
O
4
NFI
Ir-doped
NiFe
2
O
4
FE-SEM
Field emission scanning electron microscope
EDS
Energy-dispersive X-ray spectrometer
XRF
X-ray fluorescence
XRD
X-ray diffraction
XPS
X-ray photoelectron spectroscopy
PAL
Pohang accelerate laboratory
XANES
X-ray absorption near-edge structure
OCV
Open circuit voltage
CI
Current interruption
CV
Cyclic voltammetry
LSV
Linear sweep voltammetry
CDL
Double-layer capacitance
ECSA
Electrochemically active surface area
EIS
Electrochemical impedance spectroscopy
R
s
Solution resistance
R
f
Films resistance
R
ct
Charge transfer resistance
PZC
Potential of zero charge
M-S
Mott–Schottky
DPD
N,N-diethyl-p-phenylenediamine
HHV
Higher heating value
TN
Total nitrogen
COD
Chemical oxygen demand
IC
Ion chromatography
GC-TCD
Gas chromatography with thermal conductiv
-
ity detector
EEM
Excitation-emission matrix
DOM
Dissolved organic matter
RHE
Reversible hydrogen electrode
CE
Current efficiency
EE
Energy efficiency
TOC
Total organic carbon
1 Introduction
The current societal pursuit toward carbon neutrality
would necessitate self-contained systems, ultimately to be
independent on the existing water and energy grid. For
example, on-site wastewater treatment and reuse are ben-
eficial for a sustainable water cycle in adaptation to the
climate change [
1
]. In addition, a reduction in water and
waste transportation would decrease the carbon footprint
[
2
] for sanitation and hygiene to meet the Sustainability
Development Goals established by the United Nations. To
this end, electrochemical oxidation processes (EOPs) have
emerged as a promising way of decentralized treatment of
toilet wastewater and effluent reuse [
3
]. While achieving
adequate effluent level set by the International Organiza-
tion for Standardization (
e.g
., ISO 30500 [
4
]), the EOPs
could be advantageous with respect to ease of automation
and connection with renewable energy sources (
e.g
., using
photovoltaic panels) [
5
]. A long-term operation of a com-
bined anaerobic digester and EOP has been demonstrated
for a self-contained public toilet with a nonpotable water
reuse (flushing) [
6
].
The chlorine evolution reaction (ClER) on electrocatalysts
oxidizes chloride ion to reactive chlorine species (RCS), the
core mediator to degrade aqueous organic pollutants and
ammonium
(NH
4
+
) [
7
9
]. In particular, the efficient deam-
monification by the electrolytic RCS has been a subject of
significant attention [
10
12
], which has been rarely achieved
by conventional septic systems or other non-sewered sanita-
tion systems based on biological (de)nitrification, stripping,
ion exchange, and wet chemical treatments [
10
,
13
]. Almost
stoichiometric conversion of
NH
4
+
to
N
2
by the
in situ
gener
-
ated RCS without a generation of N-containing greenhouse
gases (
e.g
., N
2
O,
NH
3
) should be environmentally sustain
-
able, while alleviating concerns related to
NH
4
+
such as
eutrophication and odors.
On the other hand, a distributed electrolysis of nontra-
ditional water sources including wastewater (effluent) can
be involved within the
H
2
economy [
14
]. A local produc-
tion of deionized water by reverse osmosis is known to
contribute marginally to the overall
H
2
production cost by
electrolysis. However, it can compete with drinking water
production in the areas with surplus renewable energy
(
e.g
., desert). In this regard, contributions from Hoffmann
and coworkers [
15
] advocate wastewater electrolysis cells
(WECs) for localized conversion of renewable energy into
H
2
, reducing the costs and
CO
2
emission for (waste) water
treatment and transportation. A usage of separator (
e.g
.,
proton exchange membrane) in a direct wastewater elec-
trolysis could bring about proliferating ohmic losses and
Nano-Micro Lett. (2025) 17:51
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51
contamination of the separator in wastewater matrix. In
the single-compartment WEC, therefore, oxygen reduction
reaction competes with the hydrogen evolution reaction
(HER), substantially decreasing the current and energy
efficiency [
15
]. Relatively low-grade
H
2
(<
60%) in mix-
ture with
N
2
(from deammonification) and
CO
2
(from min-
eralization) can be utilized by combustion, in a decent
analogy with the existing chloralkali processes that gen-
erates
H
2
as a byproduct. This approach might be more
available and appropriate practice.
Nonetheless, the bottlenecks of WEC include require-
ments of precious element-based electrocatalysts and unsat-
isfactory selectivity of ClER. The current anode materials in
EOPs exclusively rely on dimensional stable anode (DSA;
IrTaO
x
and
RuTiO
x
) [
16
,
17
] and boron-doped diamond
(BDD) [
18
], unaffordable for a decentralized system. In
spite of the recent developments on electrocatalysts based
on earth-abundant elements (
e.g
., Ni, Fe, Co, Cu, Zn, Mo
among others) [
19
23
], their instability in near-neutral pH
required an alkalified wastewater, while inferior ClER selec
-
tivity with dominant oxygen evolution reaction (OER) ruled
out a concurrent pollutants degradation during the electroly
-
sis [
24
]. To this end, evidences have been presented that
TiO
2
outer layers in heterojunction with conductive Ir-based
DSA could enhance both the ClER selectivity and durability
[
7
9
], although the underlying mechanism remains ambigu-
ous. In addition, we recently reported
NiFe
2
O
4
(NF) elec-
trocatalysts with a tiny amount (5 mol%) of Ir doping (NFI)
could enable extraordinary OER activity and stability [
25
].
A scaling relation between OER and ClER on (mixed) metal
oxide electrocatalysts motivated us to further deploy the NFI
for ClER in circumneutral pH in combination with the
TiO
2
heterojunction layer.
Within the aforementioned context, this study reports that
NFI/TiO
2
heterojunction anode (prepared by a straightfor
-
ward solution casting) allows ClER activity superior to the
benchmark
IrO
2
and almost absolute ClER selectivity in
0.1 M NaCl solutions. Electrolysis of
NH
4
+
-laden synthetic
wastewater demonstrated that the admirable ClER metrics
simultaneously enhanced the kinetics of pollutants degrada-
tion and
H
2
generation. Electroanalyses coupled with
oper
-
ando
X-ray absorption spectroscopy revealed active ClER
primarily on
TiO
2
, while the underlying NFI served as an
ohmic contact. The practical applicability was validated by
a scaled-up WEC with toilet wastewater.
2 Experimental Section
2.1 Preparation of NFI/TiO
2
Anode
Ti foils (Alfa Aesar, 3
× 1 cm
2
, 0.25 mm thick, 99.5%
purity) underwent pretreatments to remove impurities,
including SiC sandblasting, degreasing by ultrasonication
in a mixed solvent (with equal volumes of ethanol, acetone,
and deionized (DI) water (18.2 MΩ, Millipore)) for 0.5 h,
and immersion in 10 wt% boiling oxalic acid for 0.5 h. The
precursors for mixed Ni–Fe oxides were prepared using
nitrate salts (Ni(NO
3
)
2
·6H
2
O and Fe(NO
3
)
3
·9H
2
O, both
from Alfa Aesar in 99% purity) dissolved in DI water with
0.1 M urea, in variable molar ratios of Ni to Fe ([total
metal]
= 250 mM). In particular, the precursor with Ni-
to-Fe ratio of 1:2 was used for NF. For
IrO
2
preparation,
250 mM
H
2
IrCl
6
was dissolved in a mixed solution with
equi-volumes of ethanol, isopropanol, and 0.3 M HCl. A
calculated amount of the Ir-precursor was added to the NF
precursor ([Ir]
= 12 mM) for the NFI. Ti-glycolate precur
-
sor for
TiO
2
layer was prepared by a peroxo-method [
7
,
26
].
In short, 0.25 M Ti(C
4
H
9
O)
4
was dissolved in 0.4 M gly
-
colic acid solution by addition of concentrated
H
2
O
2
, and
the final pH was adjusted to be circumneutral by addition
of concentrated
NH
4
OH. All anodes interrogated in this
study were fabricated by drop-casting (1 μL
cm
−2
), drying
for 15 min (80 °C), and annealing for 15 min (425 °C for
NF, NFI, and
TiO
2
; 525 °C for
IrO
2
). This sequence was
repeated up to total 6 coats which underwent final anneal-
ing for 1.5 h (Fig.
1
a). A commercial BDD electrode as a
control was provided by Wesco Electrode.
2.2 Anode Characterization
The surface morphology was observed by high-resolution
field emission scanning electron microscope (FE-SEM,
JSM 7800F PRIME). The elemental compositions were
estimated by energy-dispersive X-ray spectrometer (EDS,
LN2 Free SDD type) with FE-SEM, X-ray fluorescence
(ED-XRF, SII Nano technology Inc., SEA1200VX), and
glow discharge spectrometry (GDS, LECO GDS850A
with Radio Frequency Lamp). The crystalline struc
-
ture was analyzed by X-ray diffraction (XRD, Phillips
X’Pert Panalytical diffractometer) at 30 mA, 40 kV, and
Nano-Micro Lett. (2025) 17:51
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©
The authors
monochromated Cu Kα1 radiation. Raman spectra were
collected by Alpha 300R (WITec) with a
× 50 objec-
tive and wavelength of 488 nm using an
Ar
+
excitation
source. The composition and oxidation states on surface
(up to
~ 10 nm) were investigated by K-ALPHA X-ray
photoelectron spectroscopy (XPS, Thermo Fisher Scien-
tific, UK) using a monochromated Al Kα (12 kV, 72 W,
1486.6 eV, 400 μm spot size). The bulk electronic struc-
ture was interrogated by X-ray absorption spectroscopy at
the 10C beamline in Pohang Accelerate Laboratory (PAL),
to give X-ray absorption near-edge structure (XANES)
spectra.
operando
XANES analysis proceeded with the
working electrode attached to the cell window by Kapton
tape, under open circuit voltage (OCV), pre-ClER, and
ClER condition at a minute interval.
2.3 Electroanalysis
A single-compartment cell (working volume: 35 mL)
was used with three-electrode configuration including an
anode under investigation (effective geometric area: 2
× 1
cm
2
), a Pt coil cathode (BASi), and a reference electrode.
Ag/AgCl (BASi) and Hg/HgO (BASi) reference elec-
trodes were used for electrolyte with neutral and alkaline
pH, respectively. The spacing between the working and
counter electrode was maintained at 0.5 cm. The meas-
ured potentials were converted to RHE scale by
E
RHE
=
E
Ag/
AgCl
+ 0.197
+ 0.059
× pH
= E
Hg/HgO
+ 0.140
+ 0.059
× pH.
The working electrode potential (
E
we
) was compensated with
ohmic (
iR
) drop, based on a current interruption (CI) method
at 85% level. The electrochemical activity and stability were
Fig. 1
Preparation and characterization of NFI/TiO
2
anode.
a
Schematic illustration of the synthesis procedure.
b‑c
Horizontal SEM images of
NFI and NFI/TiO
2
.
d
XRD profiles of NFI and NFI/TiO
2
with references.
e–g
Ex situ
XANES for Ni K-edge, Fe K-edge, and Ti K-edge of NFI/
TiO
2
in comparison with NFI or Ti/TiO
2
Nano-Micro Lett. (2025) 17:51
Page 5 of 18
51
evaluated based on cyclic voltammetry (CV), linear sweep vol-
tammetry (LSV), and chronopotentiometry using a potentio-
stat (VSP, BioLogic). Double-layer capacitance
(C
DL
), which
represents the electrochemically active surface area (ECSA),
was measured by CV in a non-Faradaic potential window at
variable scan rates (1 to 100 mV
s
−1
) in 0.1 M NaCl (
j
a
j
c
at
0.861
V
RHE
) and 1 M KOH (
j
a
j
c
at 1.17
V
RHE
). The electro-
chemical impedance spectroscopy (EIS) estimated solution
resistance (
R
s
), films resistance (
R
f
), and charge transfer resist-
ance (
R
ct
), with fitting by EC
− Lab software (VSP, BioLogic).
The baseline potential for EIS was 1.3 V Ag/AgCl in 0.1 M
NaCl, while the sinus amplitude of 10 mV and frequency scan
range of 100 kHz to 100 mHz were used. The potential of zero
charge (PZC) was determined based on the potential where the
capacitance was minimized [
27
]. The changes in capacitance
at different potentials were tracked using EIS operated through
a potentiostat (VSP, BioLogic). These impedance measure-
ments, which varied with the applied potential, were taken in
0.05 M NaCl solutions, using a frequency of 150 mHz and a
sinus amplitude of 5 mV. By applying 6th-order polynomial
fitting to the spectra, the point where F was at its minimum was
established as the PZC [
27
]. The Mott–Schottky (M-S) plots
were obtained by EIS (sinus amplitude: 10 mV, frequency
range: 10 kHz to 10 Hz, and potential range: 0 to 1 V versus
reference electrode). The M-S slope from the following equa-
tion was used to comparatively evaluate the electrical conduc-
tivity [
28
,
29
]:
where
C
SC
is the space charge capacitance (F),
ε
is the
dielectric constant,
ε
0
is the permittivity of the vac-
uum (8.854 ×
10
−12
F
m
−1
),
e
is the elementary charge
(1.602 ×
10
−19
C),
N
d
is donor density
(m
−3
),
A
is active sur
-
face area
(m
2
),
E
we
is the applied potential to the working
electrode (V),
E
FB
is the flat band potential (V),
k
is Boltz-
mann’s constant (8.62 ×
10
−5
eV K
−1
), and
T
is the absolute
temperature (K). Prior to all electroanalyses, the cell was
rested in open circuit for 15 min.
2.4
RCS Generation by Galvanostatic Bulk Electrolysis
The ClER in aqueous electrolyte generates free chlorine spe-
cies including HOCl and
OCl
by pH-dependent hydrolysis
of
Cl
2
[
10
]. The performance of ClER (RCS generation) was
evaluated by galvanostatic electrolysis of 0.1 M NaCl solutions
(1)
1
C
2
sc
=

2
휀휀
0
eA
2
N
d



E
we
E
FB

kT
e

at variable current density (
j
, 10 to 50 mA
cm
−2
). The evolu-
tion of [RCS] was periodically quantified with DPD reagents
for initial 7 min, where
ClO
3
or
ClO
4
generations were neg-
ligible. This study used the following metrics for fair compari-
son of anodes [
7
,
8
]. The
CE
ClER
, EE
ClER
, and
SR
ClER
of ClER
were estimated by the equations below [
7
,
8
]:
where
V
represents the volume of the electrolyte (0.035 L),
F
is Faraday constant (96,485.3 C
mol
−1
), d[RCS]/dt is RCS
generation rate (M
s
−1
),
j
is current density (A
m
−2
),
t
is
electrolysis time (s), and
E
c
is cell voltage (V).
2.5
RCS‑Mediated Wastewater Treatment Coupled
with H
2
Generation
Using the aforementioned cell, bulk galvanostatic
(30 mA
cm
−2
) electrolysis experiments for RCS-medi-
ated conversion of
NH
4
+
to
N
2
with simultaneous
HER proceeded in synthetic wastewater samples. The
[Cl
]
0
was fixed at 0.1 M, while
[NH
4
+
]
0
was varied
([NH
4
+
]
0
:[Cl
]
0
= 2:1, 1.5:1, 1:1, 1:1.5, 1:2, 1:3, and 1:4
in molar basis) by mixing
NH
4
Cl, NaCl, and
(NH
4
)
2
SO
4
.
The CE of pollutants oxidation as well as CE and EE for
HER were estimated by following equations [
15
]:
where
n
is the number of electron transfer for oxidation of
aqueous pollutants (3 for
NH
4
+
-to-N
2
conversion),
dC/dt
is
decreased pollutants concentration per unit electrolysis time
of
t
(M
s
−1
),
Q
is the observed
H
2
production rate (mol
s
−1
),
and HHV is higher heating value of
H
2
(78 Wh
mol
−1
).
(2)
CEClER
(%)=
2
VFd
[
RCS
]
jAdt
(3)
EE
ClER

mmolWh
1

=
Vd
[
RCS
]
E
c
jAdt
×
3.6
×
10
6
(4)
SR
ClER
(
mmolcm
2
h
1
)=
Vd[RCS]
Adt
×
360
(5)
CE
(
pollutantsoxidation
)=
nVFdC
jAdt
(6)
CE
HER
=
2
FQ
j
A
(7)
EE
HER
=
HHVQ
E
c
jA
Nano-Micro Lett. (2025) 17:51
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The authors
To demonstrate practical applicability, a pilot-scale
WEC was manufactured in working volume of 10 L (with
internal circulation). Scaled-up NFI/TiO
2
anodes and com-
mercial stainless steel 304 cathode were prepared in size
of 35.8 × 26.6
cm
2
. Three anodes and cathodes were alter
-
nately sandwiched (with inter-electrodes distance of 1 cm)
and connected to a power supply (ODA Tech, EX30-60)
in monopolar configuration. The geometric surface area
of the electrode module exposed to electrolyte was 0.191
m
2
. Toilet wastewater was mimicked by mixing livestock
excretion (collected from Gyungju wastewater treatment
plant, Korea), seawater (collected in Pohang, Korea), and
tap water by volume ratio of 5:20:75. The composition
of the toilet wastewater was summarized with 102 mgN
L
−1
of
NH
4
+
, 104 mgN
L
−1
of total nitrogen (TN), 580
mgO
2
L
−1
of chemical oxygen demand (COD), 120 NTU
of turbidity, 121 mM of
Cl
, 7.9 of pH, and 14.7 mS
cm
−1
of conductivity. The wastewater sample was subjected to
electrolysis at constant current of 52.5 A (corresponding
to 27.5 mA
cm
−2
) for 3 h.
Quantification of anions (
e.g.
,
Cl
, ClO
3
, NO
2
,
and
NO
3
) was carried out by ion chromatography (IC,
DX-120). The concentration of free chlorine and total
chlorine were measured using DPD (N,N-diethyl-p-phe-
nylenediamine) and DPD/KI reagents, respectively, based
on absorbance at 530 nm in UV–Vis spectrometer (DR
3900, HACH). Combined chlorine (e.g., chloramines) was
estimated from the difference between free chlorine and
total chlorine [
30
]. TN was quantified using alkaline per
-
sulfate digestion [
31
] based on absorbance of nitrate at
420 nm.
NH
3
-N was analyzed by salicylate method with
commercial kits
(NH
3
-N TNT kit, HACH) and absorbance
at 610 nm [
32
]. [COD] was measured by dichromate diges-
tion with colorimetric detection at 348 nm [
33
]. Gaseous
H
2
, N
2
, and
O
2
in reactor headspace were streamed with
carrier Ar gas to pass through a gas flow meter (Ritter
MilliGascounter), and the composition was measured by
gas chromatography with thermal conductivity detector
(GC-TCD, 6890-N, Agilent Technologies). Turbidity of
toilet wastewater was measured using turbidity colorimeter
(HUMAS, TURBY 1000). The excitation-emission matrix
(EEM) with fluorescence spectrometer (FluoroMax-4) was
collected to qualitatively investigate the variations in dis-
solved organic matter (DOM).
3 Results and Discussion
3.1 Characterization of NFI/TiO
2
Heterojunction
Anode
The NFI/TiO
2
anodes were fabricated through a straightfor
-
ward drop-casting method (Fig.
1
a). The horizontal images
of FE-SEM discovered NFI nanoparticles sized in the range
of 50–100 nm (Fig.
1
b) which aggregated during the thermal
treatment to bring about tableland and ridge morphology on
the Ti substrate, as shown by EDS mapping (Fig. S1). The
M-edge signals of Ir and K-edge signals of Ni, Fe, Ti, and O
revealed even elemental distributions on the NFI aggregates.
The EDS-based molar fraction of Ir was 5.27% for NFI, in
decent agreement with 5.15% from ED-XRF analysis (Fig.
S2). These values close to the precursor composition (5%)
suggested homogeneous Ir doping on NFI. XRD patterns of
NF and NFI powders (physically abraded from the Ti sub-
strate) confirmed that the
NiFe
2
O
4
spinel crystalline lattice
(JCPDS No. 10–0325, 2θ
= 36°, 43°, and 63° corresponding
to (311), (400), and (440)) [
25
] of NF was retained for NFI
despite the Ir dopants (Fig. S3a). Raman spectra for NF and
NFI (Fig. S3b) both exhibited congruence with the
NiFe
2
O
4
spinel structure of space group Fd-3 m, as affirmed with
active bands including
A
1g
(symmetric stretch),
E
g
(sym-
metric bend), and
T
2g
(asymmetric stretch) for tetrahedral
and octahedral sites [
34
]. This evidence substantiated the
uniform doping of Ir into NF nanoparticles without insig-
nificant structural perturbation and segregation into
IrO
2
.
The SEM/EDS analysis on NFI/TiO
2
noticed a stacked
film of
TiO
2
nanoparticles sized by 10–20 nm (Fig.
1
c), to
allow more even deposition of
TiO
2
outer layer reducing
surface tortuosity (Fig. S4). The nanoporous property of
the
TiO
2
layer would allow diffusive penetration of reac-
tants such as
H
2
O,
OH
, and
Cl
[
26
]. The XRD patterns of
NFI and NFI/TiO
2
electrodes (Fig.
1
d) were dominated by
signals from the Ti metal substrate (JCPDS No. 44–1294,
= 35°, 38°, 40°, 52°, 62°, 70°, 76°, and 77°) that largely
overlapped with those of spinel
NiFe
2
O
4
peaks. NFI/TiO
2
showed additional diffraction peaks from anatase
TiO
2
(JCPDS No. 21–1272, 2θ
= 25° and 48° corresponding to
(101) and (200), respectively). These evidences character
-
ized the NFI/TiO
2
as Ir-doped
NiFe
2
O
4
in heterojunction
with nanoporous
TiO
2
layer. A GDS analysis (Fig. S5)
Nano-Micro Lett. (2025) 17:51
Page 7 of 18
51
estimated the thickness of
TiO
2
and NFI to be
~ 250 nm
and ~ 2.75 μm, respectively.
XPS for NF and NFI (Fig. S6) clarified partial charge
transfer from Ni and Fe to the Ir dopants. The fractions of
Ni
3+
and
Fe
3+
from deconvoluted Ni 2
p
3/2
(854.5 eV for
Ni
2+
and 856 eV for
Ni
3+
with two satellite peaks at 861
and 865 eV) [
35
] and Fe 2
p
3/2
[
36
] (710 eV for
Fe
2+
and
711.5 eV for
Fe
3+
) photoelectron spectra were elevated in
NFI, whereas the binding energy of Ir 4
f
peak was between
those of
Ir
4+
(61.8 eV) and
Ir
0
(60.9 eV) [
37
]. The decon-
volution of O 1
s
spectra noted escalated fraction of oxygen
vacancy upon the Ir doping. These observations were in
agreement with the prior report on NFI coated on Ni foam
[
25
]. On the other hand, the Ti 2
p
photoelectron spectra for
NF/TiO
2
and NFI/TiO
2
both indicated a partial oxidation
of Ti (Fig. S7), in comparison with the
TiO
2
layers directly
coated on the Ti substrate (Ti/TiO
2
). However, the concur
-
rent shifts in electronic structure of the underlying layers
were intangible due to the limited analytical depth of XPS.
To this end, XANES unambiguously informed on the elec-
tronic interaction across the heterojunction, based on the
edge position of individual metal components at the half-
maximum intensity to represent the oxidation state. The Ti
K-edge position of NFI/TiO
2
was positively shifted com-
pared to Ti/TiO
2
(Fig.
1
f), whereas both Ni and Fe K-edge
region absorbance spectra for NFI/TiO
2
suggested decreased
valency compared to NFI (Fig.
1
e, f). The
ex situ
XANES
thus provides compelling evidence of charge transfer from
the outer
TiO
2
to the underlying NFI across the interface.
3.2
Electrocatalytic Behaviors of NFI/TiO
2
Heterojunction Anode
Given the scaling relation between OER and ClER interme-
diates for (mixed) metal oxide electrocatalysts [
38
], screen-
ing electrocatalysts in terms of OER activity could be a
precedent step to employ the OER intermediates as ClER
center [
26
]. Due to a composition-dependent instability of
Ni
x
Fe
1-x
O
y
electrocatalysts in acidic-to-neutral pH, moreo-
ver, it was inevitable to evaluate them in alkaline electrolyte
where OER would overwhelm ClER. LSV curves in 1 M
KOH confirmed extraordinary OER activity of
NiFe
2
O
4
spi-
nel oxide substantially outperforming the other
Ni
x
Fe
1-x
O
y
compositions (x
= 0, 0.2, 0.5, 0.67, 0.8, and 1) identically
synthesized by dip coating (Fig. S8) [
26
,
39
]. Mixing Ir
within the
NiFe
2
O
4
precursor at variable atomic ratio (0, 1%,
3%, 5%, 7%, and 10%) enhanced OER activity up to 5% Ir
on the modified electrocatalysts, judging from overpotential
(
η
) at 10 mA
cm
−2
(Fig. S9). Further elevation in Ir contents
marginally influenced the current wave, in compatible with
the previous report [
25
].
Armed with the supreme OER activity of NFI (5% Ir-
doped
NiFe
2
O
4
), the electrochemical performances of NFI
and NFI/TiO
2
were assessed in 0.1 M NaCl electrolyte with
circumneutral pH, and compared with NF and
IrO
2
with or
without the
TiO
2
overlayer. It should be noted that ClER
and OER would occur in parallel in this experimental con-
dition. The XRD for the control group samples confirmed
crystallinity of spinel
NiFe
2
O
4
, rutile
IrO
2
(JCPDS No.
15–870), and anatase
TiO
2
. (Fig. S10). The voltammograms
(Fig.
2
a) estimated required potentials at 10 mA
cm
−2
to
be 2.00, 2.07, 1.81, 1.83, 1.88, and 1.90 V versus revers-
ible hydrogen electrode (RHE) for NF, NF/TiO
2
, NFI, NFI/
TiO
2
, IrO
2
, and
IrO
2
/TiO
2
, respectively. The NFI exhibited
the most facile charge transfer kinetics, even outperforming
the benchmarked
IrO
2
. Although the
TiO
2
overlayer moder
-
ately lowered the anodic wave, NFI/TiO
2
still marked supe
-
rior activity compared to the
IrO
2
. The
C
DL
was measured
by plotting charging current density (
j
a
j
c
) as linear func-
tions of scan rate (Figs.
2
b and S11). The
C
DL
value, as a
surrogate of ECSA, showed analogous trend with the LSV.
Nyquist plot from EIS disentangled
R
f
and
R
ct
[
40
], as shown
in Fig. S12. The
IrO
2
exhibited singular semicircle owing
to the conductor-like property, whereas the
R
f
was noted for
NF and NFI by additional semicircles in lower frequency
ranges. The
R
ct
based on diameter of the higher frequency
semicircles agreed with the activity trends, while the
TiO
2
overlayers substantially increased the
R
f
for the heterojunc-
tion anodes. Therefore, the moderate current reduction by
the
TiO
2
layer was ascribed to resistance to charge migration
(due to an inferior electrical conductivity of
TiO
2
) and/or
pore diffusion through the nanoporous film that was incom-
pletely compensated by the CI method.
The overall activity trends were maintained in voltam-
mograms obtained in 1 M KOH (Fig. S13), because of the
scaling relation between adsorption energy for intermediates
of OER (*OOH) and ClER (*OCl) on metal oxide electro-
catalysts [
7
,
8
]. The OER
η
of NFI (330 mV) at 10 mA
cm
−2
was lower than NF and
IrO
2
. We previously presented evi-
dences that Ir doping on
NiFe
2
O
4
could shift the active motif
from Fe–O–Fe to Ni–O–Fe to concurrently escalate ECSA
Nano-Micro Lett. (2025) 17:51
51
Page 8 of 18
https://doi.org/10.1007/s40820-024-01542-x
©
The authors
and intrinsic OER activity of NF [
25
]. If the porous
TiO
2
layers were electrochemically inert, on the other hand, the
reduction of ECSA by the
TiO
2
deposition would be inde-
pendent on the electrolyte while the mass transport resist-
ance through the
TiO
2
film could be alleviated in 1 M KOH.
However, the
TiO
2
layer reduced the
C
DL
value (Fig. S14)
of NFI more significantly in 1 M KOH compared to those
in 0.1 M NaCl. It implicitly elucidated an active electro-
catalytic roles of
TiO
2
for ClER. Mott–Schottky slopes both
in 1 M KOH and 0.1 M NaCl (Fig. S15) further revealed
substantially elevated donor density and electrical conduc-
tivity for NFI, compared to NF. The observed p-type prop-
erty of
NiFe
2
O
4
[
41
] rationalized the electron withdrawing
from the
TiO
2
(well-known n-type semiconductor) through
Fig. 2
Electrochemical performances.
a
LSV curves (scan rate: 10 mV
s
−1
) with 85%
iR
correction.
b
Capacitive
j
a
j
c
versus scan rate from CV
(potential range: 0–0.5 V vs. Ag/AgCl, scan rate: 10, 20, 50, and 100 mV
s
−1
) for NFI, NFI/TiO
2
, NF, NF/TiO,
IrO
2
, and
IrO
2
/TiO
2
electrocata-
lysts in 100 mM NaCl.
c
Chrono-potentiometric profile for long-term stability test of NFI, NFI/TiO
2
, NF, NF/TiO
2
in 0.5 M
NaClO
4
.
d‑i
CE
ClER
and
EE
ClER
during galvanostatic electrolysis of 0.1 M NaCl solutions for NF, NFI
IrO
2
, NF/TiO
2
, NFI/TiO
2
, and
IrO
2
/TiO
2