Calcium nitrate tetrahydrates [Ca(NO3)2·4H2O] (Mol. Wt., 236.15) and aluminum nitrate nonahydrates [Al(NO3)3·9H2O] (Mol. Wt., 375.134) are extra pure 98% and produced from Loba Chemie – India, these chemicals have been used as raw materials for synthesis of CA, C2A and C3A with appropriate molar ratio (1:2, 2:2 & 3:2) respectively.

For the preparation of gel, the stoichiometric requirement of the solution is prepared. The nitrate salts of calcium and aluminum [Ca(NO3)2·4(H2O) & AlNO3)3·9(H2O)] were dissolved in distilled water for preparing CA, C2A as well as C3A with appropriate molar ratio. Calcium nitrate solution was dropwisely added to the aluminum nitrate solution with continuous stirring. The liquid “sol” was heated up to 300°C to remove the nitrates as well as gases. - Water evaporated and solution becomes dense, then fumes of nitrogen oxides were detected. With continuous heating process, a white solid “gel” phase has been formed with disappearing of fumes at the end of the heating process. This method is called aqueous sol–gel method. Scheme of the synthesis is shown in Fig. 1.

Fig. 1.

Flow chart for preparation calcium aluminate phases powder via sol–gel method.

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The sample was prepared and annealed at different temperatures. The calcination process was done by muffle furnace at different temperatures ranged between 500 and 1200°C for 1h. In addition, the phases (CA & C3A) are calcined at 1000 and 1200°C, respectively with soaking time 2 as well as 4h.

Calcium aluminate phases’ pastes has been prepared by mixing calcined phases of CA as well as C3A at 1000 and 1200°C for 1 & 2h, respectively with required water of consistency according to ASTM C-191 [20]. Then, each paste has been casted in a cubic steel mold with dimension 2×2×2cm. The mold was manually vibrated for few minutes to remove any air bubbles and gave a better compaction paste. Immediately after casting, the mold was kept in a humidity chamber at 100% relative humidity and constant temperature (20±2°C) for the first 24h. Hardened cubes were demolded and then cured in 100% humidity for 28 days. After the desired curing time (28 days), the hydration process of the hardened (thee) cubes was stopped though dried in oven at 105°C for 24h.

The formed starting oxide composite and the phases have been studied by XRD (Bruker D8 Advance, Cu target, wavelength 1.5¿, 40kV, 40mA), SEM (FEI Quanta 250 FEG-SEM), TGA & DTA (Shimadzu thermogravimetric analyzer TGA-50H, 20°C/min heating rate), FTIR (JASCO FTIR spectroscope model FT/IR-6100 type A) and DLS (Zetasizer ver. 6.32, and used acetone as a solvent). The hydrated hardened cubes have been examined (compressive strength, porosity as well as bulk density) were determined as described elsewhere [21] and SEM technique.

The sol–gel method is a good technique for synthesis of advanced materials. It is used at relatively low temperature as compared with the traditional methods. Fig. 2 represents XRD pattern of starting material composite prepared via sol–gel technique which was dried and preheated at 300°C. It shows only existence calcium nitrate hydrate [Ca(NO3)3·n(H2O)] in crystalline state, and there is no existence any sign of aluminum nitrate nonahydrate. Aluminum nitrate nonahydrate has been decomposed by heating up to 300°C and amorphous γ-Al2O3 was produced according to the following equation

Fig. 2.

XRD pattern of starting material composite preheated at 300°C.

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At the beginning, H2O as well as HNO3 are released in large quantities with increasing heat temperature up to 150°C. As the reaction continues, a big amount of NO2 and NO gases are evolved up to 255°C and at the end, some of N2O is produced [22] is in agreement with the present result.

Fig. 3 shows XRD patterns (a–c) of prepared calcium aluminate phases (CA, C2A and C3A, respectively) at different temperatures ranged between 500 and 1200°C for 1h. It appears that no peaks are formed at 500 up to 700°C, this means that all constituents become amorphous. Also, amorphous γ-Al2O3 did not transform and calcium nitrate hydrate has been decomposed.

Fig. 3.

XRD pattern of prepared calcium aluminate phases: (a) CA, (b) C2A and (c) C3A calcined at different temperatures.

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Calcium nitrate tetrahydrate loses partially its crystalline water at 120°C and becomes hydrated with less water molecules which losses all the water molecule subsequently at 155, 160 and 210°C, then the anhydrous decomposes starting at 561°C to produce calcium oxide and nitrogen oxide [23,24]. XRD curves in Fig. 3(a–c) exhibits appearance of some peaks at 800°C, where the amorphous γ-Al2O3 transforms to crystalline δ-Al2O3 at 750°C and therefore, crystalline calcium aluminate phases are formed [25]. CA and C3A phases have been formed starting at 900°C as shown in Fig. 3(a & c) and mayenite (Ca12Al14O33) was also produced. While, mayenite was formed and C2A did not produced as shown in Fig. 2(b). So, C2A has been prepared under specific condition at 1250°C and 25000 bars [26].

From Fig. 3(a & c) we noticed also that, with increasing calcination temperature from 900 to 1200°C, the transformation process of CA and C3A phases to CA phase at 1000°C. Fig. 3(a) looks better than at 900°C. However, there is no significant change at 1100 and 1200°C. In contrast, the transformation to C3A as in Fig. 3(c) looks better at 1200°C. Also, with increasing the amount of calcium oxide percent in the constituents as in CA, C2A and C3A phases, we can detect a small peak at 800°C (Fig. 3a–c). Increasing CaO content accelerates the formation of phases at lower temperature.

Fig. 4(a & b) represents the XRD patterns for CA as well as C3A calcined at 1000 and 1200°C, respectively for 1, 2 and 4h. In Fig. 4(a), CA phase pattern showed no significant effect of calcination time on the phase. While, C3A phase has been affected by the calcination time, therefore the transformation at 2h is better than 1h and there is no change at 4h.

Fig. 4.

XRD pattern of (a) CA and (b) C3A calcined at 1000°C and 1200°C, respectively for different periods.

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Fig. 5 represents thermal gravimetric and differential thermal analyses (TG and DTA) curves of the starting materials composite preheated at 300°C. TG and DTA curves exhibit thee endothermic peaks located at 134.8, 422.9 and 585.25°C. The mass loss of the first step is attributable to the loss of interlayer water below 200°C (73–200°C). The weight loss at the second step (300–450°C) is due to the decomposition of aluminum nitrate hydrate forming Al2O3 as well as N2O. The gas produced from the decomposition of the anhydrous aluminum nitrate has been lost at 300–450°C. Finally at the last step, the loss weight is attributed to decomposition of anhydrous calcium nitrate at 500–600°C producing CaO and NO2.

Fig. 5.

TGA and DTA curves of starting materials composite preheated at 300°C.

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Fig. 6(a & b) shows the dynamic light scattering (DLS) curves of size distribution for CA and C3A phases’ constituents, respectively at 300, 900, 1000 and 1100°C. As shown in Fig. 6(a), the CA's particles size at 300°C is about 93nm, increased up to 168nm at 900°C, then the particles size reduced to 49nm at 1000°C and finally increased to 467nm at 1100°C. Increasing of size at 900°C can be explained as a result of the formation of a mixture of monoclinic CA and cubic C12A7 (mayenite) which is bigger in crystal size than CA [27], Increasing the temperature up to 1000°C induces the transformation of mayenite to CA which is smaller crystal size. CA's particle size increases with increasing the calcination temperature up to 1100°C.

Fig. 6.

DLS curves of size distribution of prepared calcium aluminate phases: (a) CA and (b) C3A at different temperatures.

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Fig. 6(b) represents the C3A constituent's particle size behavior with increasing the calcination temperature. The particle size of the components at 900°C is more reduced than the size at 300°C due to the formation of only cubic mayenite phase with smaller size. Increasing calcination temperature up to 1000°C as well as 1100°C, led to an increase in the particle size. This is due to the transformation process of cubic maynite to cubic C3A, which is bigger crystal size [27].

The FTIR spectra of prepared CA and C3A phases at different temperatures are shown in Fig. 7(a & b). It is found that, the spectra at 300°C shows the formation of a characteristic peaks of water at 3400cm−1 as well as at 1700–1600cm−1 due to O–H bending vibration and stretching, this peak become smaller with increasing the calcination temperature up to 1200°C. The presence of O–H group is due to the existence of absorbed water on the active phase surface. At 1400–1300cm−1 there was a peak due to N–O of nitrate (NO3−) which disappeared with increasing temperature starting from 800 up to1200°C as a sign to complete decomposition. The peak at 2425cm−1 due to atmospheric carbon dioxide (CO2) appeared at 300°C then disappeared in the spectra starting from 800 up to1200°C. A broad peak appeared in all spectra at 1083–300cm−1 is assigned to Al–O due to formation and vibration of tetrahedron AlO4 and octahedron AlO6.

Fig. 7.

FTIR spectra for prepared calcium aluminate phases: (a) CA and (b) C3A at different temperatures.

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Fig. 8 shows the SEM image of starting material composite of the calcium aluminate which preheated at 300°C for 1h. We can observe non-isolated aggregates particles. It seems like gelatinous or hydrated matter, so there is no existence of porous and it is difficult to measure the particle size.

Fig. 8.

SEM image for starting material composite preheated at 300°C for 1h.

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The image of Fig. 9(a), shows a small extend of adsorbed water and the grain size was found to increase with increasing calcination period (soaking time) (Fig. 9a–c). The grain size of calcined powder at 1000°C for 1h has been detected in the range of 36–96nm, while it becomes around 190–360nm after 2h. However, the size of calcined powder after 4h could not be measured because the particles were in coagulated state. The SEM results are in agreement with XRD and DLS analyses. In addition, the grain size has been increased with elevation the calcination temperature followed by decreasing the porosity as in Fig. 9(a & d).

Fig. 9.

SEM images for CA phase calcined at 1000°C for 1, 2 and 4h in (a, b and c) images respectively and CA phase calcined at 1100̊C for 1h in (d) image.

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The images of Fig. 10, exhibited an increase in the grain size with increasing the calcination period (soaking time) as in images (a–c). The grain size of calcined powder at 1200°C for 1h has been measured in the range of 219–269nm, but increased up to 348–563nm for 2h. Finally, the grain size was found to be in the range of 380–600nm at period of 4h. The elevation in the calcination temperature led to an increase in the particle size and decrease in the porosity as shown in Figs. 10(a & d).

Fig. 10.

SEM images for C3A phase calcined at 1200°C for 1, 2 and 4h in (a, b and c) images in respectively and C3A phase calcined at 1100̊C for 1h in (d) image.

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Fig. 11(a) shows the SEM image of the hydrated CA phase calcined at 1000°C for 1h cured in 100% humidity up to 28 days. It is clear that, the presence of composite of monoclinic gibbsite AH3 and cubic hydrated tricalcium aluminate C3AH6 crystals. This is due to the conversion of metastable hexagonal hydrated calcium aluminate CAH10 and hydration products of mayenite as well as, a big size porous has been observed which causes a weak texture [7]. Fig. 11(b) illustrates the hydrated C3A phase calcined at 1200°C for 2h cured in 100% humidity up to 28 days, which exhibits the presence of cubic C3AH6 and little amount of monoclinic AH3 (gibbsite) due to the hydration of C3A and conversion of metastable hydration products of small quantity of mayenite. Also, the texture is more compacted and homogenous as result of the presence a smaller size porous than in Fig. 11(a) of CA hydrated.

Fig. 11.

SEM images for calcined CA and C3A at (1000 & 1200°C) as in (a and b) respectively after hydration for 28 days.

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Table 1 represents the calculated values of compressive strength, bulk density as well as porosity percent of hydrated CA and C3A at 28 days. The bulk density and the porosity percent values of CA are higher than C3A hydrated phases. The hydration of CA is temperature dependent, at temperature less than 20°C, CAH10 is produced. C2AH8 as well as AH3 are produced at about 30°C, Finally, C3AH6 and AH3 are generated at temperature greater than 55°C. Also, the conversion of CAH10 and C2AH8 to C3AH6 releases free water, which results in a decrease in strength due to higher porosity [28]. While in the case of C3A only a small quantity of the hydration products from mayenite has been done. Also, C3A has higher CaO/Al2O3 molar ratio which decreased the porosity and consequently increased the mechanical properties as discussed by [1]. The compressive strength value of CA is less than C3A as a result of the conversion process of the hydration products and high difference in the porosity percent formed though the hydration of CA and C3A phases. The physico-mechanical measurements are in good agreement with the SEM results.

The hydration of calcium aluminate phases are summarized as

Tricalcium aluminate phase (C3A) hydrates very quickly known as ‘flash-set’ can occur on its own in water to form the hexagonal plate hydrates C2AH8 and C4AH13 in the first instance which convert with time to the more stable cubic form C3AH6, or if the temperature is sufficiently high (>40°C) directly to C3AH6[29,30]. The chemical equation can be expressed as