Influence and its mechanism of temperature variation in a muffle furnace during calcination on the adsorption performance of rod-like MgO to Congo red

doi:10.1007/s11706-018-0427-y

Front. Mater. Sci.

2018, Vol. 12

Issue (3) : 304-321 https://doi.org/10.1007/s11706-018-0427-y

RESEARCH ARTICLE

Influence and its mechanism of temperature variation in a muffle furnace during calcination on the adsorption performance of rod-like MgO to Congo red

Yajun ZHENG^1,², Liyun CAO¹(

), Gaoxuan XING², Zongquan BAI², Hongyan SHEN³, Jianfeng HUANG¹, Zhiping ZHANG²(

)

¹. School of Material Science and Engineering, Shaanxi University of Science and Technology, Xi’an 710021, China
². School of Chemistry and Chemical Engineering, Xi’an Shiyou University, Xi’an 710065, China
³. School of Earth Sciences and Engineering, Xi’an Shiyou University, Xi’an 710065, China

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Abstract

Calcination temperature plays a crucial role in determining the surface properties of generated MgO, but the influence of temperature variation in a muffle furnace during calcination on its performance is rarely reported. Herein we observed that the temperature in a muffle furnace during calcination demonstrated a gradually increasing trend as the location changed from the furnace doorway to the most inner position. The variation in temperature had a great impact on the adsorption performance of generated rod-like MgO without and/or with involvement of Na₂SiO₃ to Congo red in aqueous solution. To get a better understanding on the detailed reasons, various techniques including actual temperature measurement via multimeter, N₂ physical adsorption, CO₂ chemical adsorption and FT-IR spectrometry have been employed to probe the correlation between the adsorption performance of generated MgO from various locations and the inner actual temperature of used muffle furnace as well as their physicochemical properties. In addition, two mechanisms were proposed to elucidate the adsorption process of Congo red over the surface of generated MgO without and/or with presence of Na₂SiO₃, respectively.

Keywords magnesium oxide calcination muffle furnace placed location adsorption performance

Corresponding Author(s): Liyun CAO,Zhiping ZHANG

Online First Date: 23 August 2018 Issue Date: 10 September 2018

Cite this article:

Yajun ZHENG,Liyun CAO,Gaoxuan XING, et al. Influence and its mechanism of temperature variation in a muffle furnace during calcination on the adsorption performance of rod-like MgO to Congo red[J]. Front. Mater. Sci., 2018, 12(3): 304-321.

URL:

https://academic.hep.com.cn/foms/EN/10.1007/s11706-018-0427-y
https://academic.hep.com.cn/foms/EN/Y2018/V12/I3/304

Fig.1 (a) Schematic illustration of the placed location of samples in used muffle furnace (20 cm width and 30 cm length) for calcination. (b) SEM image of the obtained rod-like particles from the reaction between Mg(NO₃)₂ and Na₂CO₃ in the presence of 0.1 g Na₂SiO₃. (c) XRD pattern of the generated product. (d)(e) Photographs of the Congo red solutions (initial concentration: 2500 mg·L⁻¹ for MgO without Na₂SiO₃, and 3000 mg·L⁻¹ for MgO with Na₂SiO₃ in preparation; volume: 10 mL) treated with 10 mg of MgO particles obtained from calcination at 500°C, in which the placed location of the MgO samples in used muffle furnace is indicated as shown in (a).

Fig.2 Contour maps of the adsorption capacities of obtained MgO particles from the reaction between Mg(NO₃)₂ and Na₂CO₃ (a) in the absence and (b) in the presence of 0.1 g of Na₂SiO₃ followed by placing at different locations in used muffle furnace for calcination at 500°C. Note: The adsorption capacity was evaluated by the residual concentration of Congo red solution (initial concentration: 3000 mg·L⁻¹; volume: 10 mL) treated with 10 mg of MgO particles obtained from calcination at 500°C.

Fig.3 (a) Photographic image of the front view of used muffle furnace for measuring the inner actual temperature. (b) Detailed view for the distribution of the measurement probes inside the furnace. (c) Back view of used muffle furnace for measurement. (d) Contour map of the measured inner actual temperatures in used muffle furnace when the controller temperature was set as 100°C (each data point was an average of three replicates, and the deviation between them was less than 0.5°C).

Tab.1 Texture properties of obtained MgO particles from various locations in calcination

Fig.4 CO₂-TPD profiles of MgO particles from the reaction between Mg(NO₃)₂ and Na₂CO₃ (a) in the absence and (b) in the presence of 0.1 g of Na₂SiO₃ followed by placing at different locations (#1, #2 and #3 as indicated in Fig. 1(a)) in used muffle furnace for calcination at 500°C.

Fig.5 FT-IR spectra of the collected MgO particles after the following treatments: (a)(b) from the reaction between Mg(NO₃)₂ and Na₂CO₃ in the absence and in the presence of 0.1 g of Na₂SiO₃ followed by placing at different locations (#1, #2 and #3 as indicated in Fig. 1(a)) in used muffle furnace for calcination at 500°C, (c)(d) from the hydration systems by mixing 0.01 g obtained MgO particles with aqueous solution (10 mL) under gentle stirring for 90 min followed by centrifugation, washing and drying, and (e)(f) from the adsorption systems by mixing 0.01 g obtained MgO particles with Congo red aqueous solution (3000 mg·L⁻¹, 10 mL) under gentle stirring for 90 min followed by centrifugation, washing and drying. Note: The used MgO in (c)(e) and (d)(f) were from the systems without and with the involvement of Na₂SiO₃, respectively.

Fig.6 SEM images of generated products (a)(c) before and (b)(d) after hydration of 0.01 g of the MgO without and with Na₂SiO₃ in 10 mL of aqueous solution for 90 min. Suggested adsorption mechanism of Congo red over the surface of MgO (e) without and (f) with Na₂SiO₃ during preparation.

Fig. S1 Photographic image of the distribution of the samples for calcination in used muffle furnace (20 cm width × 30 cm length).

Fig. S2 UV-vis spectra of initial Congo red solutions (2500 mg·L⁻¹ for MgO without Na₂SiO₃ and 3000 mg·L⁻¹ for MgO with Na₂SiO₃, 10 mL) treated with 10 mg of MgO particles obtained from the reaction between Mg(NO₃)₂ and Na₂CO₃ (a) in the absence and (b) in the presence of 0.1 g of Na₂SiO₃ followed by calcination at 500°C, in which #1–#12 mean the placed locations of samples in used muffle furnace as indicated in Fig. 1(a).

Fig. S3 Photographs of initial Congo red solutions (2500 mg·L⁻¹ for 400°C, 3000 mg·L⁻¹ for 500°C, 2000 mg·L⁻¹ for 600°C, and 700 mg·L⁻¹ for 700°C, 10 mL) treated with 10 mg of MgO particles obtained from the reaction between Mg(NO₃)₂ and Na₂CO₃ in the absence [(a)(c)(e)(g)] and in the presence [(b)(d)(f)(h)] of 0.1 g of Na₂SiO₃ followed by calcination at (a)(b) 400°C, (c)(d) 500°C, (e)(f) 600°C, and (g)(h) 700°C [Note: The marked numbers 1–12 mean the placed locations of samples in used muffle furnace as indicated in Fig. 1(a)].

Fig. S4 Contour maps of the adsorption capacities of obtained MgO particles from the reaction between Mg(NO₃)₂ and Na₂CO₃ in the absence [(a)(c)(e)] and in the presence [(b)(d)(f)] of 0.1 g of Na₂SiO₃ followed by placing at different locations in used muffle furnace for calcination at (a)(b) 400°C, (c)(d) 600°C and (e)(f) 700°C [Note: The adsorption capacity was evaluated by the residual concentrations of Congo red solutions (initial concentration: 2500 mg·L⁻¹ for 400°C, 2000 mg·L⁻¹ for 600°C and 700 mg·L⁻¹ for 700°C, 10 mL) treated with 10 mg of MgO particles obtained from calcination at different temperatures].

Fig. S5 Contour maps of the adsorption capacities of obtained MgO particles from the reaction between Mg(NO₃)₂ and Na₂CO₃ followed by placing at different locations in used muffle furnace for calcination at 500°C with different heating rates: (a) 10.7°C/min; (b) 5.3°C/min; (c) 2.7°C/min [Note: The adsorption capacity was evaluated by the residual concentrations of Congo red solutions (initial concentration: 3000 mg·L⁻¹, 10 mL) treated with 10 mg of obtained MgO particles].

Fig. S6 Photographs of initial Congo red solutions (10 mL) treated with 10 mg of MgO particles obtained from the following reaction systems: (a) from the reactions between Mg(NO₃)₂ and K₂CO₃, MgCl₂ and Na₂CO₃ and Mg(NO₃)₂ and (NH₄)₂CO₃ followed by placing in the positions of 1, 2 and 3 as indicated in Fig. 1(a) for calcination (initial concentration of Congo red solution: 2500 mg·L⁻¹); (b) from the reactions between Mg(NO₃)₂ and Na₂CO₃ in the presence of 0.0004 mol Fe(NO₃)₃·9H₂O, Al(NO₃)₃·9H₂O and Na₂C₂O₄ followed by placing in the positions of 1, 2 and 3 as indicated in Fig. 1(a) for calcination (initial concentration of Congo red solution: 2500 mg·L⁻¹); (c) from the reactions between Mg(NO₃)₂ and Na₂CO₃ in the presence of 0.0004 mol Na₅P₃O₁₀, Na₃PO₄·12H₂O and NaF followed by placing in the positions of 1, 2 and 3 as indicated in Fig. 1(a) for calcination (initial concentration of Congo red solution: 3000 mg·L⁻¹ for the systems with Na₅P₃O₁₀ and Na₃PO₄·12H₂O and 2700 mg·L⁻¹ for the system with NaF).

Fig. S7 Photographs of the obtained MgO with different morphologies: (a) trapezoidal MgO; (b) spherical MgO; (c) spherical-like MgO; (d) nest-like MgO. Photographs of initial Congo red solutions (300 mg·L⁻¹ for trapezoidal MgO, 700 mg·L⁻¹ for spherical MgO, 2300 mg·L⁻¹ for spherical-like and nest-like MgO, 10 mL) treated with 10 mg of MgO particles with different morphologies from the system (e) in the absence and (f) in the presence of 0.1 g of Na₂SiO₃ followed by calcination at 500°C [Note: The marked numbers 1–3 mean the placed locations of samples in used muffle furnace as indicated in Fig. 1(a)].

Fig. S8 Contour maps of measured inner actual temperatures in used muffle furnace when the controller temperatures were, respectively, set as (a) 50°C, (b) 75°C and (c) 125°C (each data point was an average of three replicates, and the deviation between them was less than 0.5°C).

Table S1 Comparison of the residual concentration of Congo red solution after adsorption by generated MgO from various reaction systems

Table S2 Comparison of the residual concentration of Congo red solution after adsorption by generated MgO with different morphologies in the absence and/or the presence of Na₂SiO₃

1	Abdullah H, Kuo D H, Kuo Y R, et al.. Facile synthesis and recyclability of thin nylon film-supported n-type ZnO/p-type Ag2O nano composite for visible light photocatalytic degradation of organic dye. The Journal of Physical Chemistry C, 2016, 120(13): 7144–7154 https://doi.org/10.1021/acs.jpcc.5b12153
2	Zhang G, Li X, Li Y, et al.. Removal of anionic dyes from aqueous solution by leaching solutions of white mud. Desalination, 2011, 274(1–3): 255–261 https://doi.org/10.1016/j.desal.2011.02.016
3	Patel Y, Mehta C, Gupte A. Assessment of biological decolorization and degradation of sulfonated di-azo dye Acid Maroon V by isolated bacterial consortium EDPA. International Biodeterioration & Biodegradation, 2012, 75: 187–193 https://doi.org/10.1016/j.ibiod.2012.10.004
4	Vahid B, Khataee A. Photoassisted electrochemical recirculation system with boron-doped diamond anode and carbon nanotubes containing cathode for degradation of a model azo dye. Electrochimica Acta, 2013, 88: 614–620 https://doi.org/10.1016/j.electacta.2012.10.069
5	Yoo E S, Libra J, Adrian L. Mechanism of decolorization of azo dyes in anaerobic mixed culture. Journal of Environmental Engineering, 2001, 127(9): 844–849 https://doi.org/10.1061/(ASCE)0733-9372(2001)127:9(844)
6	Akhtar S, Khan A A, Husain Q. Potential of immobilized bitter gourd (Momordica charantia) peroxidases in the decolorization and removal of textile dyes from polluted wastewater and dyeing effluent. Chemosphere, 2005, 60(3): 291–301 https://doi.org/10.1016/j.chemosphere.2004.12.017 pmid: 15924947
7	Wawrzkiewicz M. Removal of C.I. Basic Blue 3 dye by sorption onto cation exchange resin, functionalized and non-functionalized polymeric sorbents from aqueous solutions and wastewaters. Chemical Engineering Journal, 2013, 217: 414–425 https://doi.org/10.1016/j.cej.2012.11.119
8	Bai Z, Zheng Y, Zhang Z. One-pot synthesis of highly efficient MgO for the removal of Congo red in aqueous solution. Journal of Materials Chemistry A, 2017, 5(14): 6630–6637 https://doi.org/10.1039/C6TA11087H
9	Zhong P S, Widjojo N, Chung T S, et al.. Positively charged nanofiltration (NF) membranes via UV grafting on sulfonated polyphenylenesulfone (sPPSU) for effective removal of textile dyes from wastewater. Journal of Membrane Science, 2012, 417–418: 52–60 https://doi.org/10.1016/j.memsci.2012.06.013
10	Shi B, Li G, Wang D, et al.. Removal of direct dyes by coagulation: the performance of preformed polymeric aluminum species. Journal of Hazardous Materials, 2007, 143(1–2): 567–574 https://doi.org/10.1016/j.jhazmat.2006.09.076 pmid: 17070993
11	Bhatia D, Sharma N R, Singh J, et al.. Biological methods for textile dye removal from wastewater: A review. Critical Reviews in Environmental Science and Technology, 2017, 47(19): 1836–1876 https://doi.org/10.1080/10643389.2017.1393263
12	Raval N P, Shah P U, Shah N K. Adsorptive amputation of hazardous azo dye Congo red from wastewater: a critical review. Environmental Science and Pollution Research International, 2016, 23(15): 14810–14853 https://doi.org/10.1007/s11356-016-6970-0 pmid: 27255316
13	Ahmad A, Mohd-Setapar S H, Chuong C S, et al.. Recent advances in new generation dye removal technologies: novel search for approaches to reprocess wastewater. RSC Advances, 2015, 5(39): 30801–30818 https://doi.org/10.1039/C4RA16959J
14	Lawal I A, Chetty D, Akpotu S O, et al.. Sorption of Congo red and reactive blue on biomass and activated carbon derived from biomass modified by ionic liquid. Environmental Nanotechnology Monitoring & Management, 2017, 8: 83–91 doi:10.1016/j.enmm.2017.05.003
15	Seyahmazegi E N, Mohammad-Rezaei R, Razmi H. Multiwall carbon nanotubes decorated on calcined eggshell waste as a novel nano-sorbent: Application for anionic dye Congo red removal. Chemical Engineering Research & Design, 2016, 109: 824–834 https://doi.org/10.1016/j.cherd.2016.04.001
16	Debnath S, Maity A, Pillay K. Impact of process parameters on removal of Congo red by graphene oxide from aqueous solution. Journal of Environmental Chemical Engineering, 2014, 2(1): 260–272 https://doi.org/10.1016/j.jece.2013.12.018
17	Yang J M. A facile approach to fabricate an immobilized-phosphate zirconium-based metal-organic framework composite (UiO-66-P) and its activity in the adsorption and separation of organic dyes. Journal of Colloid and Interface Science, 2017, 505: 178–185 https://doi.org/10.1016/j.jcis.2017.05.040 pmid: 28578280
18	Lei C, Pi M, Jiang C, et al.. Synthesis of hierarchical porous zinc oxide (ZnO) microspheres with highly efficient adsorption of Congo red. Journal of Colloid and Interface Science, 2017, 490: 242–251 https://doi.org/10.1016/j.jcis.2016.11.049 pmid: 27912123
19	Zheng Y, Zhu B, Chen H, et al.. Hierarchical flower-like nickel(II) oxide microspheres with high adsorption capacity of Congo red in water. Journal of Colloid and Interface Science, 2017, 504: 688–696 https://doi.org/10.1016/j.jcis.2017.06.014 pmid: 28622562
20	Feng J, Gao M, Zhang Z, et al.. Fabrication of mesoporous magnesium oxide nanosheets using magnesium powder and their excellent adsorption of Ni(II). Journal of Colloid and Interface Science, 2018, 510: 69–76 https://doi.org/10.1016/j.jcis.2017.09.047 pmid: 28938178
21	Pilarska A A, Klapiszewski Ł, Jesionowski T. Recent development in the synthesis, modification and application of Mg(OH)2 and MgO: A review. Powder Technology, 2017, 319: 373–407 https://doi.org/10.1016/j.powtec.2017.07.009
22	Ahmed S, Guo Y, Huang R, et al.. Hexamethylene tetramine-assisted hydrothermal synthesis of porous magnesium oxide for high-efficiency removal of phosphate in aqueous solution. Journal of Environmental Chemical Engineering, 2017, 5(5): 4649–4655 https://doi.org/10.1016/j.jece.2017.09.006
23	Zhu K, Hu J, Kübel C, et al.. Efficient preparation and catalytic activity of MgO(111) nanosheets. Angewandte Chemie, 2006, 45(43): 7277–7281 https://doi.org/10.1002/anie.200602393 pmid: 17024713
24	Sutradhar N, Sinhamahapatra A, Pahari S K, et al.. Controlled synthesis of different morphologies of MgO and their use as solid base catalysts. The Journal of Physical Chemistry C, 2011, 115(25): 12308–12316 https://doi.org/10.1021/jp2022314
25	Wang F, Ta N, Shen W. MgO nanosheets, nanodisks, and nanofibers for the Meerwein–Ponndorf–Verley reaction. Applied Catalysis A: General, 2014, 475: 76–81 https://doi.org/10.1016/j.apcata.2014.01.026
26	Liu X, Niu C, Zhen X, et al.. Novel approach for the synthesis of Mg(OH)2 nanosheets and lamellar MgO nanostructures and their ultra-high adsorption capacity for Congo red. Journal of Materials Research, 2015, 30(10): 1639–1647 https://doi.org/10.1557/jmr.2015.113
27	Zhang Z, Zheng Y, Chen J, et al.. Facile synthesis of monodisperse magnesium oxide microspheres via seed-induced precipitation and their applications in high-performance liquid chromatography. Advanced Functional Materials, 2007, 17(14): 2447–2454 https://doi.org/10.1002/adfm.200600906
28	Zhu Y M, Han Y X, Liu G L. Cubic-shaped nano-MgO powder and its infrared absorption properties. Advanced Materials Research, 2010, 92: 35–40 doi:10.4028/www.scientific.net/AMR.92.35
29	Xiang L, Liu F, Li J, et al.. Hydrothermal formation and characterization of magnesium oxysulfate whiskers. Materials Chemistry and Physics, 2004, 87(2–3): 424–429 https://doi.org/10.1016/j.matchemphys.2004.06.021
30	Yan Y, Zhou L, Zhang J, et al.. Synthesis and growth discussion of one-dimensional MgO nanostructures: nanowires, nanobelts, and nanotubes in VLS mechanism. The The Journal of Physical Chemistry C, 2008, 112(28): 10412–10417 https://doi.org/10.1021/jp712149g
31	Yan C, Sun C, Shi Y, et al.. Surface fabrication of oxides via solution chemistry. Journal of Crystal Growth, 2008, 310(7–9): 1708–1712 https://doi.org/10.1016/j.jcrysgro.2007.11.092
32	Sharma M, Jeevanandam P. Synthesis of magnesium oxide particles with stacks of plates morphology. Journal of Alloys and Compounds, 2011, 509(30): 7881–7885 https://doi.org/10.1016/j.jallcom.2011.04.151
33	Boddu V M, Viswanath D S, Maloney S W. Synthesis and characterization of coralline magnesium oxide nanoparticles. Journal of the American Ceramic Society, 2008, 91(5): 1718–1720 https://doi.org/10.1111/j.1551-2916.2008.02344.x
34	Kim K H, Lee M S, Choi J S, et al.. Microstructural and textural characterization in MgO thin film using HRTEM. Thin Solid Films, 2009, 517(14): 3995–3998 https://doi.org/10.1016/j.tsf.2009.01.167
35	Purwajanti S, Zhou L, Ahmad Nor Y, et al.. Synthesis of magnesium oxide hierarchical microspheres: A dual-functional material for water remediation. ACS Applied Materials & Interfaces, 2015, 7(38): 21278–21286 https://doi.org/10.1021/acsami.5b05553 pmid: 26348829
36	Zhang X, Zheng Y, Yang H, et al.. Controlled synthesis of mesocrystal magnesium oxide parallelogram and its catalytic performance. CrystEngComm, 2015, 17(13): 2642–2650 https://doi.org/10.1039/C5CE00136F
37	Wu X, Cao H, Yin G, et al.. MgCO3·3H2O and MgO complex nanostructures: controllable biomimetic fabrication and physical chemical properties. Physical Chemistry Chemical Physics, 2011, 13(11): 5047–5052 https://doi.org/10.1039/C0CP01271H pmid: 21170433
38	Eubank W R. Calcination studies of magnesium oxides. Journal of the American Ceramic Society, 1951, 34(8): 225–229 https://doi.org/10.1111/j.1151-2916.1951.tb11644.x
39	Gai P L, Montero J M, Lee A F, et al.. In situ aberration corrected-transmission electron microscopy of magnesium oxide nanocatalysts for biodiesels. Catalysis Letters, 2009, 132(1–2): 182–188 https://doi.org/10.1007/s10562-009-0085-x
40	Mastuli M S, Roshidah R, Mahat A M, et al.. Sol–gel synthesis of highly stable nano sized MgO from magnesium oxalate dihydrate. Advanced Materials Research, 2012, 545: 137–142 https://doi.org/10.4028/www.scientific.net/AMR.545.137
41	Moorthy V K. Influence of calcination treatments on the development of morphology in magnesia powders. Transactions of the Indian Ceramic Society, 2014, 35(5): 89–98 https://doi.org/10.1080/0371750X.1976.10840870
42	Ikegami T, Kobayashi M, Moriyoshii Y, et al.. Characterization of sintered MgO compacts with fluorine. Journal of the American Ceramic Society, 1980, 63(11–12): 640–643 doi:10.1111/j.1151-2916.1980.tb09852.x
43	Thomas D K, Baker T W. An X-ray study of the factors causing variation in the heats of solution of magnesium oxide. Proceedings of the Physical Society, 1959, 74(6): 673–679 https://doi.org/10.1088/0370-1328/74/6/301
44	Anderson P J, Livey D T. Physical methods for investigating the properties of oxide powders in relation to sintering. Powder Metallurgy, 1961, 4(7): 189–203 https://doi.org/10.1179/pom.1961.4.7.010
45	Zhang X, Zheng Y, Feng X, et al.. Calcination temperature-dependent surface structure and physicochemical properties of magnesium oxide. RSC Advances, 2015, 5(105): 86102–86112 https://doi.org/10.1039/C5RA17031A
46	Pei L Z, Yin W Y, Wang J F, et al.. Low temperature synthesis of magnesium oxide and spinel powders by a sol–gel process. Materials Research, 2010, 13(3): 339–343 https://doi.org/10.1590/S1516-14392010000300010
47	Valcheva-Traykova M L, Davidova N P, Weiss A H. Thermal decomposition of Mg, Al-hydrotalcite material. Journal of Materials Science, 1993, 28(8): 2157–2162 https://doi.org/10.1007/BF00367577
48	Sharma L, Kakkar R. Hierarchical porous magnesium oxide (Hr-MgO) microspheres for adsorption of an organophosphate pesticide: Kinetics, isotherm, thermodynamics, and DFT studies. ACS Applied Materials & Interfaces, 2017, 9(44): 38629–38642 https://doi.org/10.1021/acsami.7b14370 pmid: 29027786
49	Zhang Z, Zhang S, Chen J, et al.. Characterization of the surface properties of Mg/Al oxides by the solvation parameter model. Journal of Chromatography A, 2006, 1115(1–2): 58–63 https://doi.org/10.1016/j.chroma.2006.02.069 pmid: 16530209
50	Ciesielczyk F, Bartczak P, Klapiszewski Ł, et al.. Treatment of model and galvanic waste solutions of copper(II) ions using a lignin/inorganic oxide hybrid as an effective sorbent. Journal of Hazardous Materials, 2017, 328: 150–159 https://doi.org/10.1016/j.jhazmat.2017.01.009 pmid: 28110149
51	Ciesielczyk F, Bartczak P, Zdarta J, et al.. Active MgO–SiO2 hybrid material for organic dye removal: A mechanism and interaction study of the adsorption of C.I. Acid Blue 29 and C.I. Basic Blue 9. Journal of Environmental Management, 2017, 204(Pt 1): 123–135 https://doi.org/10.1016/j.jenvman.2017.08.041 pmid: 28865307
52	Jesionowski T, Przybylska A, Kurc B, et al.. The preparation of pigment composites by adsorption of C.I. Mordant Red 11 and 9-aminoacridine on both unmodified and aminosilane-grafted silica supports. Dyes and Pigments, 2011, 88(1): 116–124 https://doi.org/10.1016/j.dyepig.2010.05.011

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