a thermodynamic approach to cement hydration - Eawag-Empa ...

More documents

Recommendations

Info

1.6 References Anderson, G. M. and Crerar, D. A., 1993. Thermodynamics in Geochemistry. The 16 Equilibrium Model. Oxford University Press, New York, Oxford. Ayora, C., Chinchón, S., Aguado, A., and Guirado, F., 1998. Weathering of iron sulfides and concrete alteration: Thermodynamic model and observation in dams from Central Pyrenees, Spain. Cement and Concrete Research 28, 1223-1235. Babushkin, V. I., Matveyev, G. M., and Mchedlov-Petrossyan, O. P., 1985. Thermodynamics of Silicates. Springer-Verlag, Berlin. Bennett, D. G., Read, D., Atkins, M., and Glasser, F. P., 1992. A thermodynamic model for blended cements. II: Cement hydrate phases; thermodynamic values and modelling stuides. Journal of Nuclear Materials 190, 315-325. Berner, U., 1990. A thermodynamic description of the evolution of pore water chemistry and uranium speciation during degradation of cement. Report 90-12, PSI, Villigen, Switzerland 68. Blezard, R. G., 1998. The history of calcareous cements. In: Hewlett, P. C. (Ed.), Lea's Chemistry of Cement and Concrete. Arnold, London. Brown, P. W., 1987. Early hydration of tetracalcium aluminoferrite in gypsum and limegypsum solutions. Journal of the American Ceramic Society 70, 493-496. Buhlert, R. and Kuzel, H.-J., 1971. Ueber den Einbau von Cr 3+ und Fe 3+ in Ettringit. Zement-Kalk-Gips 2, 83-85. Collepardi, M., Monosi, S., and Moriconi, G., 1979. Tetracalcium aluminoferrite hydration in the presence of lime and gypsum. Cement and Concrete Research 9, 431-437. Ecker, M., 1998. Diadochiebeziehungen in Calciumaluminatferraten und deren Hydratationsprodukten; Hallesches Jahrbuch für Geowissenschaften, Reihe B, Martin-Luther-Universität Halle-Wittenberg.
Ecker, M. and Pöllmann, H., 1994. Investigations on lamellar calciumaluminate- ferratehydrates at different atmospheres and temperatures by in situ X-ray powder diffraction. Materials Science Forum 166-169, 565-570. Edmeades, R. M. and Hewlett, P. C., 1998. Cement admixtures. In: Hewlett, P. C. (Ed.), Lea's Chemistry of Cement and Concrete. Arnold, London. Emanuelson, A. and Hansen, S., 1997. Distribution of iron among ferrite hydrates. Cement and Concrete Research 27, 1167-1177. Fortune, J. M. and Coey, J. M. D., 1983. Hydration products of calcium aluminoferrite. Cement and Concrete Research 13, 696-702. Fukuhara, M., Goto, S., Asage, K., Daimon, M., and Kondo, R., 1981. Mechanisms and kinetics of C4AF hydration with gypsum. Cement and Concrete Research 11, 407- 414. Galimova, L. A., Danilov, V. P., Lepeshkov, I. N., Yudovich, B. E., and Shebanov, N. A., 1988. A study of the formation and decomposition of the calcium iron(III) double hydroxide sulphate Ca6Fe2(OH)12(SO4)3 . 26H2O in the 3Ca(OH)2 + Fe2(SO4)3 --> 3CaSO4 + 2Fe(OH)3-H2O system at 20 °C. Russian Journal of Inorganic Chemistry 33, 445-448. Gallias, J. L., 1998. Microstructure of the interfacial transition zone around corroded reinforcement. In: Katz, A. (Ed.),Second International Conference on the Interfacial Transition Zone in Cementitious Composites. RILEM proceedings. London : E & FN Spon, Haifa, Israel. Gartner, E. M., Tang, F. J., and Weiss, S. T., 1985. Saturation factors for calcium hydroxide and calcium sulfates in fresh Portland cement pastes. Journal of the American Ceramic Society 68, 667-673. Hong, S.-Y. and Glasser, F. P., 1999. Alkali binding in cement pastes: Part I. The C-S-H phase. Cement and Concrete Research 29, 1893-1903. 17
Page 1: DISS. ETH NO. 17422 A THERMODYNAMIC
Page 5: “Lisa, in this house we obey the
Page 8 and 9: VI 3.3 Methods ....................
Page 10 and 11: aluminates (Ca3Al2O6) and the alumi
Page 13 and 14: Zusammenfassung Die Eigenschaften v
Page 15 and 16: Die Mischkristallreihe zwischen Al-
Page 17 and 18: 1 Introduction 1.1 Ordinary Portlan
Page 19 and 20: solution is dominated by K, Na, and
Page 21 and 22: notation AFt-phases (Al2O3 - Fe2O3
Page 23 and 24: 1.3 Admixtures Admixtures are liqui
Page 25 and 26: Retarding admixtures Retarding admi
Page 27 and 28: about their stabilities and possibl
Page 29 and 30: or diffusion R t 2 3 K 2 × ( 1 −
Page 31: and undersaturation. After equilibr
Page 35 and 36: Meller, N. and Hall, C., 2004. ESEM
Page 37: zur Strassen, H. and Schmitt, C. H.
Page 40 and 41: 2.2 Introduction Aluminium containi
Page 42 and 43: (0.001 - 1.0 M) for the precipitati
Page 44 and 45: were present in the liquid phases,
Page 46 and 47: presence of a second atomic shell a
Page 48 and 49: Due to the very low solubility and
Page 50 and 51: 34 counts counts A pH measured 1200
Page 52 and 53: Ca4[Al(OH)6]2(OH)2·6H2O is only st
Page 54 and 55: Table 2.3. Calculated ion activitie
Page 56 and 57: 2 0 14 2.047 7 - - - - - - - - 2.04
Page 58 and 59: From the loss of water of the solid
Page 60 and 61: Liquid phase of the precipitation a
Page 62 and 63: Table 2.6. Thermodynamic data of th
Page 64 and 65: solubility of Fe-monocarbonateis ca
Page 66 and 67: c(Ca, Fe, S) in mmol/L c(Ca, Fe, S)
Page 68 and 69: o The heat capacity C can be calcul
Page 70 and 71: (Babushkin et al., 1985). The condi
Page 72 and 73: Ecker, M. and Pollmann, H., 1991. P
Page 74 and 75: Lothenbach, B. and Winnefeld, F., 2
Page 77 and 78: 3 Solid solution between Al-ettring
Page 79 and 80: postulated a possible miscibility g
Page 81 and 82: HNO3 suprapur qualitiy, 65%, with h
Page 83 and 84:
114, 116 and 216, cf. Table 1), das
Page 85 and 86:
The c-parameter of pure Fe-ettringi
Page 87 and 88:
XAl,total = 0.5 and XAl,total = 0.0
Page 89 and 90:
differentiated relative weight in %
Page 91 and 92:
3.4.2 Liquid phase of the solid sol
Page 93 and 94:
Table 3.4. Thermodynamic data given
Page 95 and 96:
Assuming a continuous solid solutio
Page 97 and 98:
The calculated ion concentrations a
Page 99 and 100:
On the basis of the measured ion co
Page 101 and 102:
experiments were simulated, conside
Page 103 and 104:
Emanuelson, A. and Hansen, S., 1997
Page 105 and 106:
Moore, A. and Taylor, H. F. W., 197
Page 107 and 108:
4 Thermodynamic modeling of the inf
Page 109 and 110:
4.3 Materials and methods 4.3.1 Exp
Page 111 and 112:
4.3.2 Thermodynamic calculations Th
Page 113 and 114:
4.4 Results and discussion 4.4.1 Ca
Page 115 and 116:
much less pronounced retardation in
Page 117 and 118:
elative peak intensity 20 15 10 5 0
Page 119 and 120:
elative weight [%] counts 100 90 80
Page 121 and 122:
very low during the first day of hy
Page 123 and 124:
During the first day the pore solut
Page 125 and 126:
4.4.4 Citrate The amount of dissolv
Page 127 and 128:
Table 4.4. Calculated concentration
Page 129 and 130:
grains. The precipitated or adsorbe
Page 131:
Schwarz, W., Sujata, K., Jennings,
Page 134 and 135:
ettringite structure. But not a con
Page 137 and 138:
6 Outlook With regard to the refine
Page 139 and 140:
Appendix 1: Solubility of Fe-ettrin
Page 141 and 142:
Table A1.3. Thermodynamically calcu
Page 143:
Table A1.5. Thermodynamically calcu
Page 146 and 147:
Table A2.2. Values of the a-paramet
Page 148 and 149:
Table A2.6.Calculated concentration
Page 150 and 151:
Table A2.9. Calculation of the theo
Page 153 and 154:
Appendix 3: Influence of citric aci
Page 155 and 156:
Table A3.4. Calculated relative pea
Page 157 and 158:
Table A3.8. Calculated saturation i
Page 159:
g/100g solid 50 40 30 20 10 C 3 S C
Page 162 and 163:
Table A4.2. Normative phase composi
Page 164 and 165:
Table A4.4. Measured concentrations
Page 166 and 167:
elative weight [%] 100 90 80 70 60
Page 169:
CURRICULUM VITAE Göril Möschner B
show all

a thermodynamic approach to cement hydration - Eawag-Empa ...

Create successful ePaper yourself

Delete template?

Save as template?