Belay Zeleke Dilnesa - Eawag-Empa Library

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CHAPTER 3 SYNTHETIC FE-CONTAINING HYDRATES Fig. 28 Spectral range 100 cm -1 – 1500 cm -1 of Raman spectra from sample Fe-Ms-20 °C (comparison with Al-monosulfate spectra [79]). The small peak at 1085 cm -1 was assigned to carbonate which was present due to carbon dioxide contamination. Sulfate vibrations are less intense in the Fe-monosulfate compound compared to Al-monosulfate compound. The vibration mode of sulfate was shifted from the more intense 1 mode: 992 cm -1 for Fe-Ms compared with 982 cm -1 for Al-monosulfate (or 981 cm -1 on Kuzel’s salt) [79, 90]. The 1 position of Fe-monosulfate synthesized at 20 °C corresponds to that of Al-monosulfate treated at 117 °C (i.e. 993 cm - 1 ) [79]. The band position of Fe(OH)6 appeared at 508 cm -1 , which is significantly lower than for Al(OH)6 (532 cm -1 ). The shifts of the bands could indicate a possible substitution of Al by Fe as was previously observed between Al- and Fe- ettringite [79]. The hydrogen bond network (Fig. 29) is highly modified in Fe-monosulfate compared to that in Al-monosulfate. 75
Intensity 4500 4000 3500 3000 2500 2000 1500 1000 500 0 CHAPTER 3 SYNTHETIC FE-CONTAINING HYDRATES 2800 3000 3200 3400 3600 3800 4000 Raman shift (cm -1 ) Fe-Ms 50°C Al-Ms Fig. 29 Spectral range 2800 cm -1 – 4000 cm -1 of Raman spectra from sample Fe-Ms-50 °C (comparison with Al-monosulfate spectra [79]). The weight loss of monosulfate observed by TGA/DTG analysis (Fig. 30) was assigned as follows: Ca4[(Al, Fe)2(OH)12]SO4 6H2O → Ca4[(Al, Fe)2(OH)12]SO4 + 6H2O: interlayer water removal Ca4[(Al, Fe)(OH)12]SO4 → Ca4[(Al, Fe )2O6]SO4 + 6H2O : dehydroxylation The loss of water is controlled by the interlayer structure and occurs in several steps for both Al- and Fe-monosulfate. The 6 molecules of the interlayer water of Al-monosulfate escaped in the temperature range up to 260 °C comparable to other observations [61, 73]. The remaining water molecule bond in main layer escaped above 260 °C. The water loss observed for Fe-monosulfate had less well defined steps due to the water loss of Fe(OH)3 in this temperature range [16]. Water loss up to 260 °C was 4.5 in the case of Fe- monosulfate taking account the presence of other solids. 76
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Fe-containing hydrates and their fa
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The measured composition of the liq
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ZUSAMMENFASSUNG Thermodynamische Mo
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konnten die Fe-haltigen Hydrate im
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I owe to thank all the laboratory t
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Table 19 Compositions of Al/Fe-mono
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LIST OF FIGURES Fig. 1 Calculated v
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Fig. 34 Calculated solubility produ
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Fig. 62 Calculated solubility produ
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Table of Contents TABLE OF CONTENTS
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TABLE OF CONTENTS 3. SYNTHETIC FE
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TABLE OF CONTENTS 3.5.4. Solid solu
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1 INTRODUCTION CHAPTER 1 INTRODUCTI
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CHAPTER 1 INTRODUCTION be formed. T
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cm 3 /100 g cement 85 80 75 70 65 6
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CHAPTER 1 INTRODUCTION 1.4 Characte
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CHAPTER 1 INTRODUCTION Fig. 4 Sampl
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CHAPTER 1 INTRODUCTION Identificat
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CHAPTER 2 MATERIALS AND METHODS han
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3CaOAl2O3 + 6H2O → 3CaOAl2O36H2O
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CHAPTER 2 MATERIALS AND METHODS Tab
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CHAPTER 2 MATERIALS AND METHODS 2.2
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CHAPTER 2 MATERIALS AND METHODS fil
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CHAPTER 2 MATERIALS AND METHODS at
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Page 80 and 81: o layer thickness (A) 8.0 7.8 7.6 C
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CHAPTER 3 SYNTHETIC FE-CONTAINING H
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CHAPTER 4 FE-CONTAINING HYDRATES IN
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(Al+Fe)/Ca (Al+Fe)/Ca 0.8 0.6 0.4 0
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k 3 (k) CHAPTER 4 FE-CONTAINING HYD
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differentiated relative weight Weig
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Early reaction CHAPTER 4 FE-CONTAIN
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weight loss in % differentiated rel
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5. GENERAL CONCLUSION AND OUTLOOK a
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Speciation of iron(III) in hydrated
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5. GENERAL CONCLUSION AND OUTLOOK
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Techniques XRD X-ray diffraction TG
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APPENDIX APPENDIX Appendix A: Addit
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Intensity (arb. Units) P Fe 2O 3 R
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APPENDIX Appendix B7 XRD patterns o
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REFERENCES REFRENCES [1] H.F.W. Tay
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REFRENCES [29] M. Vespa, R. Dähn,
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REFRENCES [54] M. Balonis, B. Lothe
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REFRENCES [81] H.F.W. Taylor, Cryst
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REFRENCES [107] K. Kyritsis, N. Mel
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REFRENCES [134] M. Wilke, F. Farges
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CURRCULUM VITAE Curriculum Vitae Na
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