| Summary: | 碩士 === 明新科技大學 === 化學工程與材料科技研究所 === 100 === During the process of manufacturing calcium chloride by using hydrochloric acid to dissolve the limestone, some tiny sized matters remain insoluble.The analysis shows that the insoluble matters contain a lot of titanium dioxide (TiO2). The TiO2 can function as photocatalyst to oxidize organic matter. Therefore it is very useful for wastewater treatment to remove dye. The goal of the extraction of TiO2 from this sludge can be considered as an attractive topic in wastewater treatment. It benefits not only the environmental problems but also the economic issues. However due to the actual low quantity of TiO2 extracted from sludge, we changed and replaced the sludge with a commercially available titanium sulfate for the preparation of porous titanium dioxide in the later studies..
This research composes into three parts. The first part is the TiO2 extraction from sludge. The second part is the preparation of porous photocatalyst TiO2. The third part is the treatment of dye (FBL) in wastewater by porous photocatalyst TiO2. X-ray diffraction ( XRD); Scanning Electron Microscopy (SEM) and Surface Area Analyzers (BET)were used to analyze porous photocatalyst TiO2: its crystalline phases; the surface structure as well as particle size. The efficiency of treatment by produced TiO2 were analyzed by ADMI and TOC which showed the true chroma and total organic carbon content of FBL. The comparison of treatment efficiency between the produced porous TiO2 and the commercially available nano-TiO2 was also investigated.
By XRD, the characteristic peaks appeared showed that the porous photocatalyst TiO2 is an anatase crystalline phase. By SEM, the particle size of the porous photocatalys TiO2 was about 2.5μm .By BET, the surface area of the porous photocatalys TiO2 was about 229.6504 (m2/g) . The photocatalytic experiment results showed that when the COD was 100ppm of dye wastewater by using photocatalysis of porous TiO2, TOC removal could reach 80% and ADMI removal reached 90%. The experimental results can fit both the Langmuir adsorption isotherm and Langmuir-Hinshelwood (L.-H.) kinetic model.
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