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Effect of pH on photocatalytic degradation of Methylene Blue in water by facile hydrothermally grown TiO2 Nanoparticles under Natural Sunlight

T0 review · 4 major / 5 minor · reviewed 2026-08-12 · deepseek-v4-flash

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Pith's one-line read A hydrothermally grown TiO2 nanoparticle catalyst removes 99.3% of methylene blue from water in 40 minutes under natural sunlight at pH 10.

desk verdict The pH-10 99.3% claim is not supported by the reported kinetics or by the missing controls; the paper is a solid characterization study in need of major revision. read the letter →

arxiv 2411.08515 v1 pith:ZNPFJGOV submitted 2024-11-13 cond-mat.mtrl-sci

Uttama Kumar Saint , Suresh Chandra Baral , Dilip Sasmal , P. Maneesha , Sayak Datta , Farzana Naushin , Somaditya Sen This is my paper · ORCID
classification cond-mat.mtrl-sci
keywords solarphotocatalysishydrothermalsynthesisTiO2nanoparticlesmethylenebluedegradationpHdependencedyewastewatersurfaceareareusability
verification ladder T0 review T1 audit T2 compute T3 formal

The pith

A machine-rendered reading of the paper's core claim, the machinery that carries it, and where it could break.

The reading

This paper reports that a hydrothermally grown anatase-dominant TiO2 catalyst, prepared from a low concentration of titanium precursor, can degrade nearly all methylene blue in water under direct natural sunlight within 40 minutes. The optimized conditions are 1 mg/mL catalyst, 10 ppm dye, and pH 10, giving 99.3% degradation with a first-order rate constant of 0.0845 $min^{-1}$. The authors trace the performance to the catalyst's high surface area (386 m2/g), small particle size, and the pH-dependent electrostatic adsorption of the cationic dye onto the catalyst surface. They also show the catalyst survives five reuse cycles with only gradual loss of activity. If correct, the result points to a cheap, lamp-free route for treating dye-contaminated textile wastewater.

What carries the argument

The central object is the hydrothermally synthesized TiO2 nanoparticle, specifically the high-surface-area S1 sample (386 m2/g, about 14 nm particles, anatase-dominant with a rutile impurity). The mechanism carrying the argument is photocatalysis: sunlight creates electron-hole pairs; holes oxidize hydroxide or water to hydroxyl radicals, and electrons reduce oxygen to superoxide radicals, which then attack the dye. The pH dependence is carried by the electrostatic interaction between the negatively charged TiO2 surface at high pH and the cationic methylene blue molecule, which raises adsorption and therefore degradation. The paper uses first-order rate constants from UV-vis absorbance decay as the measure of activity.

What would settle it

Run the pH 10, 1 mg/mL catalyst experiment in parallel with a catalyst-free control and a dark control, and measure the dissolved carbon remaining after 40 minutes; if the catalyst-free beaker loses similar color or the carbon removal is far below 99.3%, the claim that the dye is photocatalytically destroyed is not supported.

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Extended reading notes

Core claim

On the paper's own terms, the central discovery is that the concentration of titanium tetra-isopropoxide in the hydrothermal synthesis controls the TiO2 surface area and photocatalytic activity: the 6 mM sample (S1) has a BET surface area of 386 m2/g and degrades 99.3% of methylene blue in 40 minutes at pH 10 under sunlight of about 474 W/m2, while the 60 mM sample (S2), with 102 m2/g, reaches 97.9%. The degradation follows first-order kinetics, with the S1 rate constant rising from 0.0346 $min^{-1}$ at pH 8 to 0.0845 $min^{-1}$ at pH 10 and falling to 0.0619 $min^{-1}$ at pH 11. Dark adsorption also peaks at pH 10 (73.0% for S1), and the authors attribute the optimum to enhanced hydroxide-ion availability for hydroxyl radical generation, favorable surface charge for MB adsorption, and competing reactions at higher pH. The paper further claims the catalyst is reusable for five cycles with only gradual efficiency loss.

Load-bearing premise

The load-bearing premise is that the measured drop in light absorption at the dye's characteristic wavelength equals destruction of the dye; the paper includes no catalyst-free sunlight controls at each pH and no test of complete breakdown into carbon dioxide and water, so part of the reported 99.3% could be adsorption or sunlight bleaching rather than oxidation.

Editorial extensions

If this is right

  • A 10 ppm methylene blue solution can be almost completely decolorized in 40 minutes of natural sunlight with only 1 mg/mL of this TiO2, which is much faster than several lamp-based literature values listed in the paper.
  • The optimum pH of 10 implies that mildly alkaline conditions, not extreme pH, are the practical operating regime for this catalyst.
  • Lowering the precursor concentration in the hydrothermal step is a lever for increasing surface area and rate constant, so synthesis can be tuned without adding dopants or reagents.
  • Five reuse cycles with gradual loss means the catalyst could be collected, washed, and recycled in repeated batches.

Reading between the lines

Editorial extensions of the paper, not claims the author makes directly.

  • Because degradation is measured as absorbance loss, the 99.3% figure likely overstates true mineralization; a total organic carbon measurement would be needed to confirm the dye is oxidized to CO2 and water rather than adsorbed or bleached.
  • The lack of catalyst-free sunlight controls at each pH means part of the pH trend could be photobleaching of MB at high pH; adding such controls would isolate the photocatalytic contribution.
  • The 73% dark adsorption at pH 10 suggests the fast apparent kinetics may be partly an adsorption-assisted removal; a desorption step after irradiation would reveal how much dye remains on the catalyst.
  • The same surface-charge reasoning predicts similar pH-optimized behavior for other cationic dyes, so the approach could transfer to mixed-dye wastewater, though anionic dyes would likely need acidic conditions.
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Editorial analysis

A structured set of objections, weighed in public.

Desk editor's note, referee report, and a circularity audit.

Referee Report

4 major / 5 minor

Summary. The manuscript reports a hydrothermal synthesis of TiO2 nanoparticles at two precursor concentrations (S1 and S2), with extensive materials characterization (XRD, Raman, BET, DRS, FESEM), and tests their photocatalytic degradation of methylene blue (MB) in water under natural sunlight. The central claim is that S1, at a catalyst loading of 1 mg/mL, degrades 99.3% of a 10 ppm MB solution at pH 10 within 40 minutes under ~474 W/m2 sunlight, with a reported first-order rate constant of 0.0845 min-1. The authors also report pH-dependent adsorption and degradation, a mechanistic discussion based on band-edge positions, a reusability test over five cycles, and a comparative table with literature values.

Significance. If the central claim were fully supported, the work would be of practical interest because it demonstrates near-complete dye removal under natural sunlight with a low catalyst loading and a simple hydrothermal synthesis route. The materials characterization is fairly complete, and the comparative table usefully situates the results against prior TiO2-based photocatalysts. However, the significance is currently undercut by missing control experiments, an internally inconsistent kinetic analysis, and a direct contradiction between the abstract and the reusability section. The paper's own stated limitations—lack of photolysis controls, no mineralization assay, and explicit mention of decreasing efficiency upon reuse—are not reflected in the abstract's claims.

major comments (4)
  1. [Section 3.2 / Table 2] The reported first-order rate constants are inconsistent with the stated degradation percentages. For S1 at pH 10, 99.3% degradation in 40 minutes implies k ≈ 0.124 min-1, not the reported 0.0845 min-1; for S1 at pH 8, 87.9% in 40 minutes implies k ≈ 0.053 min-1, not 0.0346 min-1. The same inconsistency appears for S2 in Table 2. Because the rate constants are presented as quantitative kinetic evidence, this discrepancy must be reconciled, either by reporting the correct fitted values or by clarifying how the percentage was computed.
  2. [Section 2.1 and Section 3] The degradation percentage is calculated solely from the decrease in UV-vis absorbance at the MB peak using Degradation (%) = [(A0 - At)/A0] × 100. The paper asserts that direct photolysis is "nearly non-existent," but no catalyst-free photolysis controls are shown for any pH, and no TOC, HPLC, or other mineralization assay is provided. This matters especially at pH 10, where Table 1 reports 73.01% dark adsorption on S1; after such extensive adsorption, the remaining dissolved MB is small, and continued dark uptake, aggregation, or photobleaching of the residual dye could inflate the calculated percentage. The claim that 99.3% corresponds to photocatalytic destruction is therefore not established by the presented data.
  3. [Abstract vs. Re-usability test] The abstract states that repeated use of the nanoparticles "without sacrificing performance five times" confirmed stability, but the Re-usability section explicitly states that the results demonstrate "a gradual decrease in efficiency across consecutive cycles, potentially resulting from the loss of nanomaterials during the filtering and washing stages." These two statements are directly contradictory, and the abstract's claim of no performance loss is not supported by the paper's own data.
  4. [Section 4, mechanism bullet] The third bullet under the pH 10 explanation states that at pH 10 "the photocatalyst surface may have a positive charge at this pH, while the MB dye may carry a negative charge due to its ionization." This contradicts the paper's own explanation in Section 3.2 and Table 1, where higher pH is said to make the TiO2 surface negatively charged, increasing electrostatic attraction to the cationic MB dye. Methylene blue is a cationic dye, and the mechanism bullet, as written, is internally inconsistent with the adsorption data and the rest of the manuscript.
minor comments (5)
  1. [Section 3.1 / Figure 6(f)] The caption for Figure 6(f) states "taking the S1 sample as a model catalyst for 80 minutes," but the figure appears in the catalyst-concentration section; please clarify whether the curves correspond to the 80-minute total irradiation time or to another condition.
  2. [Section 4, paragraph after Eq. for ECB/EVB] The sentence "Then, the reactive." is an incomplete fragment and should be finished or removed.
  3. [Table 3] The abbreviation "NM" is used in the rate-constant column without definition; please define it in the table footnote.
  4. [Section 2.1, materials list] "Methylene Blue dehydrate" appears to be a typo; the intended reagent is likely methylene blue hydrate or the dehydrated form, and the spelling should be corrected.
  5. [Section 2.1 / BET results] The reported BET surface area for S1 (386 m2/g) is exceptionally high for hydrothermally grown TiO2 nanoparticles; please verify the measurement, report the adsorption isotherm and BET consistency criteria (e.g., Rouquerol plot), and discuss whether such a high area is consistent with the FESEM particle size.

Circularity Check

0 steps flagged · score 0.0 of 10

No circularity: the paper reports fitted degradation percentages and rate constants as descriptive outputs, with no prediction or derived quantity that reduces to its own inputs.

full rationale

This is an experimental study with no claimed derivation chain that could be circular. The degradation percentage is defined operationally as Degradation (%) = [(A0 - At)/A0] x 100, and the first-order rate constants in Table 2 are fitted to the measured absorbance time series; they are presented as descriptive kinetic outputs, not as predictions derived from a model, nor as inputs that are later 'predicted' from the same fit. The conduction- and valence-band edges are computed from the standard Mulliken electronegativity relations with chi = 5.81 eV (reference [45]) and the measured band gap, both independent of the dye-degradation results, so this step is not circular. The mechanism section invokes well-established TiO2 photochemistry (references [15], [16], [44]) and standard radical redox potentials; the authors' own prior works appear only in general introductory or background citations and are not load-bearing for the central measured claims. No uniqueness theorem, ansatz-by-self-citation, or renaming-of-known-result pattern is present. The substantive weaknesses of the paper are validity concerns rather than circularity: there are no per-pH catalyst-free photolysis controls and no mineralization assay to prove that absorbance loss equals photocatalytic destruction, and the reported rate constants are numerically inconsistent with the stated degradation percentages (99.3% in 40 min implies k about 0.126 min-1, not 0.0845 min-1; 87.9% implies about 0.053 min-1, not 0.0346 min-1). These are correctness and evidence-quality issues, not cases of a result being equivalent to its inputs by construction. Accordingly, no circular step is identified and the score is 0.

Assumptions & free parameters 0 free parameters · 5 assumptions · 0 invented entities

The central claim rests on the absorbance protocol, assumed first-order kinetics, the electrostatic adsorption model, and a single measured sunlight intensity. No ad hoc fitted parameters or invented entities are introduced into a derivation.

assumptions (5)
  • domain assumption Methylene blue concentration is proportional to UV-vis absorbance at the dye peak, and absorbance loss equals photocatalytic degradation.
    Section 2.1 defines degradation percentage from A0 and At; no mineralization assay, no pH-matched photolysis control.
  • domain assumption First-order kinetics describe MB removal, and the reported k_app values come from linear fits to concentration data.
    Section 3.1 and Figures 6 and 9 fit the absorbance data to first-order decay; this is used for the rate constants.
  • domain assumption Electrostatic surface-charge model: increasing pH makes TiO2 more negative and adsorbs cationic MB.
    Section 3.2 invokes this model to explain adsorption; Section 4 later contradicts it with a positive-surface claim.
  • domain assumption Natural sunlight intensity was approximately constant during the experiments at 65000 lx, about 474 W/m2.
    Section 2.1 reports one intensity measurement; no monitoring of cloud cover, angle, or time-of-day variation.
  • standard math Williamson-Hall UDM isotropic strain model and Tauc/Kubelka-Munk relations give reliable crystallite size, strain, and band gap values.
    Used in the Results section to extract crystallite size, microstrain, and Eg; peripheral to the main photocatalytic claim.

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Pith. "Pith review of Effect of pH on photocatalytic degradation of Methylene Blue in water by facile hydrothermally grown TiO2 Nanoparticles under Natural Sunlight." pith.science (2026). https://pith.science/paper/ZNPFJGOV

@misc{pith2026241108515,
  author       = {Pith},
  title        = {Pith review of: Effect of pH on photocatalytic degradation of Methylene Blue in water by facile hydrothermally grown TiO2 Nanoparticles under Natural Sunlight},
  year         = {2026},
  howpublished = {\url{https://pith.science/paper/ZNPFJGOV}},
  note         = {Machine review of arXiv:2411.08515}
}
read the original abstract

Each year, the production of synthetic dye wastewater reaches a trillion tons, posing a significant challenge to addressing water scarcity on a global level. Hence, the treatment of wastewater to prevent water scarcity is of prime importance, and failing to do so will increase ecotoxicological risks and human health. Textile wastewater contains harmful dye. Photocatalytic degradation of such dye-contaminated wastewater is crucial to purifying the dye-contaminated water. However, this process takes time, uses high-power lamps, and is expensive. Here, we report the effect of the concentration of precursor on the size and surface morphology of TiO2 nanostructures prepared by facile hydrothermal synthesis and its ability to perform as a photocatalyst to degrade the most common industrial textile dye, methylene blue (MB), under natural sunlight. The impact of particle size on the photocatalytic activity and photocarrier migration rate was thoroughly examined. Also, the effect of pH on adsorption and photocatalytic degradation has been evaluated in detail. With several optimized conditions, almost complete dye degradation was achieved within 40 minutes under the direct illumination of natural sunlight. The enhanced photocatalytic performance can be correlated to the synergetic effect of a higher charge transfer mechanism, good catalytic active surface area availability (386 m2/g), and several optimized parameters that affect the reaction efficacy. Additionally, repeated use of NPs without sacrificing performance five times confirmed its stability and Sustainability as a promising candidate for large-scale industrial textile wastewater remedies.

Figures

Figures reproduced from arXiv: 2411.08515 by the authors.

Figure 1
Figure 1. Both samples, S1 and S2, were used for further characterization. [PITH_FULL_IMAGE:figures/full_fig_p004_1.png] view at source ↗
Figure 3
Figure 3. (Upper panel) specific surface area calculation from N2 adsorption-desorption isotherms, while the insets represent the corresponding BET plots (a, c), (Lower panel) Pore size distribution, was confirmed by BJH plots considering the desorption data (b, d) for S1 and S2 respectively. XRD confirmed the phase purity after the surface morphology and specific surface area determination. The samples are of mixed phases of… view at source ↗
Figure 5
Figure 5. Tauc Plot showing Eg values of 3.33 eV and 3.23 eV for S1 and S2, respectively. 3. Photocatalytic degradation of Methylene Blue Generally, photocatalytic activity experiments require a costly apparatus using a high-power (250~300W) UV/Xenon lamp. The lamp is both costly and requires a considerable amount of electricity. Such high power consumption has an equivalent carbon dioxide emission, which affects the environm… view at source ↗
Figures from the paper (6 more)
Figure 6
Figure 6. Figure 6: Photocatalytic properties of the TiO2 NPs (with catalyst concentration = 1 mg/mL) revealed from (a, b) the reduction of absorbance, (c) Relative concentration change (d) Rate of Change of concentration (e) Degradation percentage of with light-irradiation time, while th…
Figure 7
Figure 7. Figure 7: (a, b, c, d) shows the absorbance vs Wavelength curve of the S1 sample at pH 8, 9, 10, and 11 under sunlight [PITH_FULL_IMAGE:figures/full_fig_p015_7.png]
Figure 8
Figure 8. Figure 8: (a, b, c, d) shows the absorbance vs Wavelength curve of the S2 sample at pH 8, 9, 10, and 11 under sunlight [PITH_FULL_IMAGE:figures/full_fig_p016_8.png]
Figure 9
Figure 9. Figure 9: (a, c) relative concentration change, (b, d) calculated rate constants, and (e, f) degradation percentage for both S1 and S2 samples, respectively [PITH_FULL_IMAGE:figures/full_fig_p017_9.png]
Figure 10
Figure 10. Figure 10: Schematic of generalized photocatalytic degradation mechanism for organic dyes using both S1 and S2 catalysts. Additionally, the efficiency of MB dye degradation may be relatively low at highly acidic pH values (1 to 3) [25]. This is because acidic conditions can hind…
Figure 11
Figure 11. Figure 11: (a, b) XRD pattern of the fresh and recovered samples, (c, d) reusability test showing degradation percentage for five times uses of S1 and S2, respectively [PITH_FULL_IMAGE:figures/full_fig_p021_11.png]

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Reference graph

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Pith tools

Reviewed August 12, 2026 · model on record in the stance chip above.