Effect of citric acid and the hemihydrate amount on the properties of a calcium sulphoaluminate cement

G. Velazco *, J.M. Almanza, D.A. Cortés, J.C. Escobedo, J.I. Escalante-Garcia

Cinvestav Saltillo (Coah, México)

*gerardo.velazco@cinvestav.edu.mx

1. INTRODUCTIONTOP

The need to reduce energy consumption and emissions of carbon dioxide into the atmosphere during the manufacture of Portland cement has been a determining factor in the development of alternative cementitious materials with properties that can replace Portland cement. The calcium sulphoaluminate based cements (CSA) have drawn attention recently because during its production, the atmospheric CO₂ emissions are lower compared with those of portland cement PC (1, 2, 3). It has been estimated that the total of CO₂ emissions associated with 1T of PC are 0.815 T; from this, 0.425 T are originated from the decomposition of the raw materials and 0.39 T from the combustion of fossil fuels, including those required to generate the electricity for the plant operation (4). The calcium sulphoaluminate cements consist mainly in the phase Ye’elemite, also called Klein’s salt or tetracalcium trialuminate sulphate (C₄A₃Ŝ) (5). Other advantages of these cements over PC are: lower power consumption, higher early strength development, excellent durability in saline environments and good protection to steel reinforcement (6). The calcium sulphoaluminate (C₄A₃Ŝ) can be synthesized by calcining stoichiometric proportions of calcium carbonate (CaCO₃), aluminium hydroxide (Al(OH)₃) and gypsum (CaSO₄·2H₂O) in a furnace at temperatures ranging from 1250 to 1300 °C for 3 hours (7). F. Puertas et al. (8) studied the thermal behaviour of the calcium sulphoaluminate at a 1300–1500 °C and maintaining the final temperature for 21 hours; they found that as a consequence of the thermal treatment, the C₄A₃Ŝ starts to decompose at 1300 °C by eliminating SO₂ and obtaining CA and CaO, which produced C₁₂A₇ by solid state reaction. Other materials used in calcium sulphoaluminate production are: limestone, bauxite, aluminium-rich clay and gypsum. As a source of alumina, “red mud”, a largely unwanted by-product of the Bayer process for alumina purification, has also been used (9). Besides gypsum, fluorgypsum and anhydrite are also used as a source of calcium sulphate (10).

The early hydration of the CSA cements is mainly governed by the amount and reactivity of the added calcium sulphate (11, 12); the main reaction products are ettringite (C₆AŜ₃H₃₂) and monosulphate (C₄AŜH₁₂) (13). Ettringite is formed by one of two mechanisms; during the setting stage of the pastes by a through-solution mechanism and later after the paste has hardened forming crystals with preferred orientation on the surface of an unhydrated aluminium phase takes place (14).

The degree of hydration of the cement is greatly influenced by the presence of organic admixtures. The formation of insoluble hydration products retards the subsequent hydration of the cement compounds by forming a barrier to water transport. The solubility of the anhydrous cement phases and the precipitation of hydration products are important factors in the setting of cement pastes. It has been found that organic retarders act by forming insoluble complexes when in contact with the strongly alkaline environment of a cement paste (15). Carboxylic acids (citric, tartaric, gluconic, malic, etc.) and their salts are commonly used as retarding admixtures as these delay the setting time of concrete without adversely affecting subsequent strength development, whilst permitting a substantial reduction in the water/cement ratio (16). Tinnea and Young (17) and Singh et al. (18) showed that citric acid has a retarding effect in the system C₃A-gypsum-portlandite-water. Möschner et al. (19) investigated the influence of citric acid on the hydration of Portland cement and pointed that the citric acid retards the cement hydration not by complex formation, but slowing down the dissolution of the clinker grains. Due to the rapid setting of CSA cements, the use of retarder admixtures is necessary in order to increase their workability. This paper presents an investigation on the effects of a citric acid admixture and the amount of hemihydrate on the strength development, microstructures and the hydration during the early curing stages of CSA cements.

2. EXPERIMENTALTOP

Calcium sulphoaluminate (C₄A₃Ŝ) was synthesized at 1350 °C for 4h from a stoichiometric mixture of commercial materials CaCO₃ (OMYA S.A), CaSO₄·½H₂O (Yesera Monterrey S.A.) and Al(OH)₃ (Possehl S.A.). The resulting product was dry ball milled in order to obtain a Blaine specific surface area within 350–400 m²/kg according to ASTM C-204 (20). The proportion of each compound was determined according to the following reaction:

Cement samples of different compositions were prepared by adding 15, 20 and 25wt% of CaSO₄·½H₂O to the C₄A₃Ŝ. Some of the cements were admixed with 0.5% citric acid as a retarder. Table 1 shows the composition of the samples prepared.

Pastes prepared with distilled water using water/cement ratios (w/c) of 0.4 and 0.5. These were cast in Nylamid cubic moulds of 2.54 cm per side. Curing was carried out by immersing the cubes in water at a constant temperature of 20 °C and the evaluation of the mechanical properties was carried out after 1, 3, 7, 14 and 28 days of curing. The development of the compressive strength was evaluated using an automated hydraulic press (Controls 50-C70024) with capacity of 250 kN and a loading rate of 350 N/s. Four cubes were tested, reporting the average for each time of curing. After the completion of the test, pieces were taken from each of the samples and immersed in methanol for 24 h to remove water and stop the hydration reactions. The hydration products and their evolution were identified by X-ray diffraction (XRD) and microstructures of the hydrated samples were observed by scanning electron microscopy (SEM). Samples for XRD characterization were taken out from the cubes crushed in the compressive tests and dried in a vacuum oven for 24 h at 35 °C; these were further ground to pass the sieve of 150 microns using a porcelain mortar. A Phillips PW 3040e diffractometer was used with CuKα radiation (1.542 Å) and a scanning range of 7–60° 2θ. The SEM and EDS analysis were performed using a Philips XL 30 SEM apparatus on fracture surfaces coated with graphite. Samples were analysed using the technique of backscattered electrons. Samples with additions of 15, 20 and 25wt% of hemihydrate were hydrated using a 0.4 w/c and studied by isothermal conduction calorimetry to follow the progress of the hydration reactions of cement pastes. The release rate of heat generated during the hydration was recorded as a function of time from the moment in which the water came in contact with the cement, obtaining curves under isothermal conditions. This technique can be used to study the rate of reactions at different temperatures, as well as for deciphering the role of chemical admixtures on the hydration and setting times (21). Generally, the plot of rate of heat evolution vs. time shows the occurrence of two maxima with the so-called induction period between them. The length of the latter is influenced by the additives that accelerate or retard the hydration, and consequently, the setting and hardening process (22). The calorimeter used was made based on the Forrester’s design (23). Isothermal baths host the insulating cells containing the samples. A sample holder in the form of a copper ring is set inside the cell, the sample seats within the ring and on top of a thin copper plate that is in contact with the heat sensors (Peltier devices). The calorimeter has a data acquisition system to monitor and collect the signals over time.

3. RESULTS AND DISCUSSIONTOP

Figure 1 shows the graphs of compressive strength development of samples with 15wt% hemihydrate, 0 and 0.5wt% of citric acid and with w/c of 0.4 and 0.5. It was noted that the strength was greatly influenced by the addition of the retarder. For samples with the retarder, the strength was very low at 1 day (9 and 6 MPa using w/c = 0.4 and 0.5, respectively), compared with 34 and 30 MPa from the samples without citric acid. After 3 days, the strength increased greatly for samples with citric acid, reaching 70 and 42 MPa for w/c of 0.4 and 0.5, respectively after at 28. The latter meant increases of 40 and 16 MPa relative to 28 day values from the samples without retarder. The strength enhancement is attributed to a modification of the microstructures in the presence of the citric acid, which resulted in denser matrices of reaction products, as reviewed in subsequent sections; this seems to have also reduced the delayed ettringite formation, responsible for strength loss. Winnefeld and Barlag (24) indicated that in systems with low calcium sulphate additions, the ettringite formation is terminated shortly after setting; thus, expansive ettringite reactions cannot occur. On the contrary, the expansive behaviour of systems with ettringite/gypsum molar ratios of about 1:2 and beyond is related to the ongoing formation of ettringite in systems after setting.

Figure 2 shows the graphs of strength vs. time of samples with 20 and 25wt% of hemihydrate and w/c of 0.4 and 0.5, containing 0 and 0.5wt% of citric acid. The behaviour of these samples was similar to that described for samples with 15wt% hemihydrate, since there were relatively lower 1 day strength for samples with retarder and a further increase after 3 days. The 28 days strength reached by those samples with 0.5wt% citric acid and 20wt% hemihydrate were 60 and 46 MPa for w/c of 0.4 and 0.5, respectively; while for 25wt% hemihydrate were 58 and 42 MPa, for w/c of 0.4 and 0.5, respectively. The strength reduction for samples without retarder was caused by the delayed ettringite formation, which is a process of expansive nature that occurs after submerging the samples in water at 1 day of curing.

Figure 3 shows the curves of heat evolution rate vs time corresponding to samples with a) 15%, b) 20% and c) 25wt% of hemihydrate hydrated at 20 °C using a w/c of 0.4. The heat release period was manifested by the appearance of 3 exothermic peaks from the instant at which the water came in contact with cement until it reaches a steady state during which the heat released is not detected by the technique. For the discussion, peaks were named as 1, 2 and 3 in order of appearance. As observed in figure 3 a), in the absence of citric acid, peak 1 was intense (8.5 W/kg) and appeared after 1h and was attributed mainly to the hydration of the hemihydrate, in agreement with (25); however, it is possible that ettringite formed simultaneously. It is noteworthy that peak 1 appeared more intense as the amount of hemihydrate increased in the cements. Peak 2 was more intense (~11 W/kg) and appeared at ~4 hours and is related mainly to ettringite formation. In the presence of citric acid, the maxima of peak 1 was shifted to ~3 h and to ~32 h for peak 2; at the same time, these peaks broadened and showed a decrease in the rate of heat release, reaching 5.5 W/kg and 3 W/kg for peak 1 and 2, respectively. The broadening indicates that the addition of the citric acid strongly retarded the hydration of the cement. These observations are confirmed by the curves of the total heat released, which after 50 h showed that the presence of 0.5 wt% citric acid decreased the total heat released from ~350 kJ/kg to ~300 kJ/kg.

Figure 3 b) shows some differences relative to 3a). In the sample without citric acid, Peak 2, related to ettringite formation, reached ~10 W/kg and appeared slightly earlier than that of the sample with 15wt% of gypsum, at ~3.5 h; also, a wide and weak exothermic manifestation, peak 3, was noted from about 15 to 25 hours, suggesting the continuation of the reactions before reaching a steady state. In the presence of citric acid, peaks 1 and 2 appeared notably less intense, broadened and shifted to longer times; peak 1 shifted from ~1.2 to 3.5 h and reduced from 11 to 4 W/kg; while peak 2 was delayed by ~5.5 h and reduced from 4 to ~2 W/kg. With the admixture of citric acid, peak 3 was well defined and wide, reaching up to ~1.5 W/kg after 35; this peak is attributed to a continued ettringite formation. For the cement with 20% hemihydrate, the total heat release after 50 h decreased from ~325 kJ/kg to ~275 kJ/kg in the presence of 0.5wt% of citric acid, which was consistent with the previous observation. The graphs of Figure 3 c) for cements with 25% hemihydrate showed similar features as those described for 20% hemihydrate. In the absence of citric acid, peak 2 related to ettringite formation (~11.5 W/kg) appeared at 2.7 h, while with citric acid it shifted to 5 h reaching ~5 W/kg; peak 3, also related to ettringite formation appeared at 28 h (~2 W/kg). The total heat release after 50 h decreased from ~360 kJ/kg to ~325 kJ/kg in the presence of 0.5wt% of citric acid.

Figure 4 shows the XRD patterns corresponding to samples with 15, 20 and 25wt% of hemihydrate containing 0.5wt% of citric acid and hydrated using a w/c of 0.4 at 1 (a) and 28 (b) days of curing. The results revealed that the main hydration product was the ettringite phase with its main peak located at 9.09 2θ degrees. The monosulphate phase was identified by a low intensity peak at 9.89 2θ degrees. After 28 days the intensity of the ettringite peaks increased, indicating that its formation continued after the cement had hardened. Besides ettringite and monosulphate, a high portion of non-reacted calcium sulphoaluminate was found, as well as traces of gypsum. The observations for those samples with 0wt% of citric acid were fairly similar.

Figure 5 shows the microstructure of the sample containing 15wt% of hemihydrate and 0.5wt% of citric acid using a w/c of 0.4 at 1 and 28 days of curing. In the micrographs without retarder, Figures a) and b), two hydration products were observed. Microanalysis by EDS indicated that the needle-like morphology corresponds to the main hydration product phase, ettringite (Aft). The second phase exhibits morphology of hexagonal plates and correspond to phase monosulphate (AFm) (26, 27), which formed when there are not enough sulphates to form ettringite.

Figure 6 shows the microstructure of the sample containing 20wt% of hemihydrate and 0.5wt% of citric acid using a w/c of 0.4 at 1 and 28 days of curing. The micrographs of the samples without retarder, (a) and (b), clearly show the needle-like morphology of ettringite as the only hydration product, homogeneously distributed throughout the microstructure and with a length of approximately 10 μm. At 28 days (Figure 6 (c, d)) ettringite morphology shows thicker needles and there is a denser microstructure. The sample with citric acid exhibited a morphology of coarser and shorter needles than those from samples with no citric acid. This modification in morphology (Figure 6 (c, d)) favoured a better distribution of ettringita, reduced the expansion and led to enhancements of the compressive strength of the samples.

Figure 7 shows the microstructure of the sample containing 25wt% of hemihydrate and 0.5wt% of citric acid using a w/c of 0.4 at 1 and 28 days of curing. In the micrographs of samples without retarder, Figure 7 (a, b), some gypsum crystals were observed even at 28 days of curing, which indicates that hydration reactions were not completed and ettringite may be formed at later stages. In the samples with of citric acid, the morphology of ettringite corresponded to small needles of less than 5 μm in length, which appeared to have improved the densification of the microstructure.

4. CONCLUSIONSTOP

The compressive strength of the calcium sulphoaluminate cements was improved by the addition of citric acid. The maximum compressive strength (70 MPa) was observed in the samples with 15wt% of hemihydrate and 0.5wt% of citric acid with w/c = 0.4, which is 40 MPa greater than that of the sample without retarder. The maximum strength reached for the samples containing 20wt% hemihydrate and 0.5wt% citric acid with w/c = 0.4 was 60 MPa and samples with 25wt% hemihydrate and 0.5wt% citric acid reached 58 MPa with w/c = 0.4. The curves of heat evolution rate indicate that the addition of citric acid strongly retarded the hydration of the cement and the total heat released. Analyses by XRD, SEM and EDS showed ettringite as the main hydration product although traces of monosuphate phase were also found. The addition of citric acid increased the setting time, modified the morphology of the ettringite needles, changed the microstructural configuration and prevented the decreasing in compressive strength of the samples caused by delayed ettringite formation.

REFERENCESTOP