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Article

Effect of Low Nesquehonite Addition on the Hydration Product and Pore Structure of Reactive Magnesia Paste

by
Run Shi
,
Yuehan Hao
,
Deping Chen
* and
Wenxin Liu
Beijing Key Laboratory of Urban Underground Space Engineering, School of Civil and Resource Engineering, University of Science and Technology Beijing, Beijing 100083, China
*
Author to whom correspondence should be addressed.
Materials 2023, 16(6), 2445; https://doi.org/10.3390/ma16062445
Submission received: 3 February 2023 / Revised: 27 February 2023 / Accepted: 6 March 2023 / Published: 18 March 2023
(This article belongs to the Special Issue Advances in Sustainable Construction and Building Materials)
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Abstract

:
Reactive magnesia cement is considered an eco-efficient binder due to its low synthesis temperature and CO2 absorption properties. However, the hydration of pure MgO–H2O mixtures cannot produce strong Mg(OH)2 pastes. In this study, nesquehonite (Nes, MgCO3·3H2O) was added to the MgO–H2O system to improve its strength properties, and its hydration products and pore structure were analyzed. The experimental results showed that the hydration product changed from small plate-like Mg(OH)2 crystals to interlaced sheet-like crystals after the addition of a small amount of Nes. The porosity increased from 36.3% to 64.6%, and the total pore surface area increased from 4.6 to 118.5 m2/g. At the same time, most of the pores decreased in size from the micron scale to the nanometer scale, which indicated that Nes had a positive effect on improving the pore structure and enhancing the compressive strength. Combined with an X-ray diffractometer (XRD), a Fourier transform infrared spectrometer (FTIR), and a simultaneous thermal analyzer (TG/DSC), the hydration product of the sample after Nes addition could be described as xMgCO3·Mg(OH)2·yH2O. When Nes was added at 7.87 and 14.35 wt%, the x-values in the chemical formula of the hydration products were 0.025 and 0.048, respectively. These small x-values resulted in lattice and property parameters of the hydration products that were similar to those of Mg(OH)2.

1. Introduction

The cement industry is a serious source of fuel consumption and greenhouse gas (GHG) emissions; it is responsible for 5% of GHG emissions and is among the top industrial sources of carbon dioxide (CO2) emissions [1]. Various efforts have been made worldwide to reduce the cement industry’s large CO2 emissions, with the goal of improving the overall cost-effectiveness of energy use [2,3,4]. Compared with Portland cement clinker, reactive magnesia cement (RMC) is considered an eco-efficient binder due to its low synthesis temperature and CO2 absorption [5,6,7,8,9]. RMC is an emerging material whose ability to mineralize CO2 makes it useful for reducing the life-cycle global warming intensity (GWI) of concrete. Reactive MgO can be obtained through the calcination of MgCO3 and precipitation of Mg(OH)2 from seawater or brine [6,10,11]. Depending on the calcination temperature, four different grades of MgO can be produced: lightly fired (700–1000 °C), hard-fired (1000–1500 °C), dead-fired (1500–2000 °C), and molten (>2800 °C) [12,13,14]. Due to the loss of CO2 gas or water during calcination, lightly fired MgO has a porous structure and large surface area, making it highly reactive compared with other forms of MgO [15,16,17]. The MgO hydration product Mg(OH)2 has a very high heat absorption capacity and releases non-toxic water vapor during the dehydration process. The dehydrated product is a refractory material with a melting temperature of about 2800 °C [18,19], and Mg(OH)2-based materials offer great potential for fire protection applications in underground structures [20,21].
However, the hydration of a pure MgO–H2O mixture will not lead to a strong Mg(OH)2 paste. Studies have shown that the hydration of MgO can be significantly improved under additive and CO2 curing conditions [22,23,24,25,26,27]. The main products of MgO hydration consist of dypingite (Dyp, Mg5(CO3)4(OH)2·5H2O), nesquehonite (Nes, MgCO3·3H2O), and Mg(OH)2. The use of hydrated magnesium carbonate (HMC) additives, such as hydromagnesite [Hmgs, Mg5(CO3)4(OH)2·4H2O] [24,28], Nes [25], and Dyp [16], allows for the production of high-strength pastes without CO2 curing conditions. Kuenzel et al. [28] found that the compressive strength of MgO–H2O pastes with Hmgs additives at MgO: Hmgs mass ratios of 9:1, 8:2, and 7:3, and a water-to-binder ratio of 0.62 all reached values above 23 MPa after 28 days of curing in deionized water. The hydration product was mainly Mg(OH)2 with low crystallinity. HMCs can promote the hydration of MgO and improve the strength of the pastes. However, the composition of the hydration products and the pore structure characteristics of these pastes have not been well studied, and only the strength data have been reported for Nes additives [25]. In addition, as a CO2 sequestration product, Nes can be prepared from magnesium-oxide-rich minerals and rocks, mining and metallurgical solid wastes, and seawater at room temperature and atmospheric pressure [29,30,31,32].
In this study, the hydration mechanism, hydration product characteristics, and pore structure characteristics during the hardening and curing process were investigated using a field emission scanning electron microscope (FESEM), mercury intrusion porosimetry (MIP), an X-ray diffractometer (XRD), a simultaneous thermal analyzer (TG-DSC), and Fourier transform infrared spectroscopy (FTIR) analysis using a reactive MgO hybrid cementitious material with added Nes as the object of study. This provided an important basis for an in-depth study of the hydration mechanism of MgO in the presence of HMCs.

2. Materials and Methods

2.1. Materials

The reactive MgO used in this study was obtained from Shanghai Macklin Biochemical Co., Ltd., Shanghai, China, and consisted of an AR-grade chemical reagent of lightly burned MgO with particle diameter distributions of d90, d50, and d10, which were measured as 7.4, 3.3, and 1.3 μm, respectively.
Nesquehonite (Nes) was synthesized using the carbonation of a reactive MgO suspension at room temperature. The experimental setup is shown in Figure 1a. First, 200 g of MgO was dispersed in 10 kg of deionized water to form a suspension. The flow rate of the CO2 gas was set to 0.8 L/min, the suspension was stirred at 500 rpm with a mixer until the pH value decreased to 7.8, and then it was allowed to stand for 15 min. After the reaction, the slurry was filtered, and the solid was placed in a blower drying oven and dried at 60 °C for 2 days. Figure 1b is the diffraction pattern of MgO and synthetic Nes. According to XRD and thermal gravimetric analyses, the dry solid contained 81.25% Nes by mass and 18.75% MgO residue by mass. The dry solid was pulverized into a powder, which particle diameter distributions of d90, d50, and d10, which were measured as 59.4, 11.5, and 2.9 μm, respectively.
The deionized water used was purchased from Shanghai Aladdin Biochemical Technology Co., Ltd., Shanghai, China.

2.2. Paste Preparation and Curing

The studied reactive MgO and synthesized Nes powder were mixed at MgO:Nes molar ratios of 1:0, 64:1, 32:1, and 16:1, and the actual mass fractions of the Nes additive in the MgO–Nes mixtures were 0%, 4.14%, 7.87%, and 14.35%, respectively (Table 1). Deionized water was added to form pastes without any other chemical agents, and the water-to-solid ratio used in all samples was 1.1, which was the minimum water content required to form a homogenous paste in all cases. The fresh pastes were cast into 20 mm × 20 mm × 20 mm cubic molds, vibrated for 5 min to remove air bubbles, and then covered with a plastic film to retain moisture and isolate from atmospheric CO2. The samples were then hydrated in a cement-curing chamber at 20 ± 1 °C for 24 h. The film was then removed, and the samples were immersed in deionized water at 20 ± 1 °C for 3, 7, and 28 days (referred to as “water curing”). For comparison, some samples were maintained at 20 ± 1 °C and relative humidity above 90% until the corresponding age (denoted as “air curing”). The flow of the experiments is shown in Figure 2.

2.3. Testing Methods

2.3.1. Compressive Strength Test

The cured pastes were removed at a certain period from the water bath and chamber and tested in uniaxial compression at a loading rate of 50 N/s to obtain compressive strength.

2.3.2. Pore Size Distribution and Total Pore Volume Test

Sample pieces 5–10 mm in size were submitted to a pore structure test by mercury intrusion porosimetry (MIP) using an Autopore V 9600 porosimeter (Micromeritics Instruments Co., Norcross, GA, USA). The samples were dried at 60 °C for 2 days before testing.

2.3.3. Morphology of the Hydration Product and Pore Structure Observations

Field emission scanning electron microscope (FESEM) observations were conducted for the characterization of the cured pastes using a Zeiss Supra55 scanning electronic microscope (Carl Zeiss Microscopy LLC, White Plains, NY, USA). A thin gold layer was deposited on the samples to create a conductive surface for analysis.

2.3.4. Hydration Product Analyses

The dried samples were crushed and manually ground with an alumina mortar and pestle. Their phase compositions were examined by XRD using a SmartLab diffractometer (Rigaku Co., Tokyo, Japan), with Cu Kα radiation in the range of 5–80° with a step size of 0.02°. Additional phases in the reaction products were detected by Fourier transform infrared spectroscopy (FT-IR) with a Nicolet is50 FT-IR spectrometer in the spectral range of 400–4000 cm−1.

2.3.5. Weight Loss and Heat Absorption Capacity Test

The powder samples were submitted for thermal analysis in a TG/DSC 3+ thermogravimetry analyzer (Mettler-Toledo Inc., Columbus, OH, USA), which allowed for simultaneous TG and DSC analysis. Sample powders of approximately 33 mg were heated from room temperature to 1000 °C at a heating rate of 10 °C/min in N2. The weight loss and heat absorption of dehydration were calculated from the TG/DSC data.

3. Results

3.1. Compressive Strength

Figure 3 shows the variations in compressive strength of the hydrated samples with Nes ratio, curing conditions, and time. When the curing condition was water curing, for sample #1 with pure MgO, the compressive strength decreased with increased curing age and fell below 1 MPa, and then leveled off when the curing age was greater than 7 days. The compressive strength values of samples #2 and #3 increased with increased curing age and stabilized after 7 days. The compressive strength trend of sample #4 was similar to that of #1, but the overall strength was higher than that of sample #1, and the compressive strength remained between 3.7 and 7.9 MPa. Unlike water curing, the development of compressive strength of the air-cured samples showed an increasing trend, and the strength of samples added with Nes was higher than that of #1 samples with pure MgO. Among them, sample #2 reached a maximum strength of 9.0 MPa after 28 days of air curing. Therefore, we found that the introduction of Nes into the MgO-H2O system, whether cured in air or in water, tended to increase the compressive strength of the MgO paste for a given addition amount.

3.2. Pore Structure Characteristics

The cumulative pore volume distribution curves of the water-cured samples are shown in Figure 4. For the 28-day-aged sample (#1-28d) consisting of pure MgO, the total pore volume was 351.3 mm3/g, of which 97.11% of the pore diameters were distributed between 150 and 500 nm. Meanwhile, without pores smaller than 150 nm, the pore volume of the pores above 500 nm accounted for only 2.89% of the total volume (Figure 4a), with an average pore diameter of 303.5 nm and total pore area of 4.6 m2/g. Compared with the pure MgO samples, the samples with less Nes additive had a larger total pore volume and finer pore diameters, mostly consisting of nanopores, and the total pore area increased. At the same curing time of 28 days, the curves of samples #2 and #3 were similar (Figure 4b,d), and the total pore volume, total pore area, and average pore diameter were similar. Among them, 97.30% of the pore diameters of sample #3 were below 30 nm, with an average pore size of 15.2 nm and a total pore area of 112.7 m2/g. Meanwhile, sample #4, with the 14.35% Nes addition (Figure 4e), had a much higher cumulative pore volume of 1059.6 mm3/g. The average pore diameter was 35.8 nm. As the amount of Nes added increased, the dry bulk density decreased.
The pore structure parameters of the samples are listed in Table 2. Table 2 shows that the dry bulk density of the samples of the same age decreased with an increase in the Nes addition and that the porosity increased. The bulk density and porosity of the pure MgO (#1-28d) samples were 1032 kg/m3 and 36.25%, respectively, and those of the #4-28d samples with 14.35% addition of Nes changed significantly to 609 kg/m3 and 64.55%, respectively. We observed that the addition of a small amount of Nes decreased the pore diameter and increased the total pore area of the samples. It should be noted that the same changes were found for sample #3 with a shorter 3-day curing time.

3.3. Morphology of the Hydration Products and Pores

Figure 5a shows the microstructural characteristics of the fractured samples with hydration products consisting of pure MgO under a FESEM after 28 days of maintenance in water. The fine plate-like hydration products of different particle sizes were stacked together, where most of the particles were less than 500 nm in size, and the pores between the particles were irregular in shape. Figure 5b shows the microstructural characteristics of the #3-3d sample with the 7.87% Nes addition, and three structures were observed; namely, (1) the interlaced growth of thin sheet-like hydration products with a large number of about 0.5–1 μm pores inside; (2) irregular round-shaped particles of unhydrated MgO with a particle size smaller than 200 nm; (3) cross-shaped lamellar aggregates hidden below the MgO particles, with a large number of nanoscale pores inside (box in Figure 5b). Based on the analysis of the MIP results, the third structure of the #3-3d sample was its main characteristic structure. With a longer curing time of 28 days (sample #3-28d), the third similar texture became the key feature of sample #3. Figure 5c shows the microscopic features of sample #3-28d, which exhibited a third structure similar to sample #3-3d, with interlaced growth of thin lamellar hydration products and the development of nanoscale pores inside. Figure 5d shows the #4-28d sample with the 14.35% Nes addition, which had similar characteristics as the #3-28d sample, with the difference that its lamellar hydration products were thicker and the pores were not uniformly distributed. Figure 5e shows the microstructure characteristics of the unhydrated MgO raw material, irregular round particles with different particle sizes, which is the same as the second structure in Figure 5b below.

3.4. XRD Analysis and Phase Characteristics

The XRD patterns of the water-cured samples are shown in Figure 6a. For the pure MgO paste (samples #1-3d and #1-28d), the diffraction peaks of brucite Mg(OH)2 were narrow and strong, while the diffraction peaks of periclase MgO were very weak, even at a curing time of 3 days. This indicated the high hydration reactivity of MgO as a raw material. As shown in Figure 5a, the hydration product had good crystallinity under the FESEM, which was typical of brucite plate crystals. For the crystals that contained the Nes addition, the brucite peaks became lower and wider, especially in the (001), (101), and (102) lattice planes. In all samples with the Nes addition, the diffraction peaks of the unhydrated MgO were evident in the 3-day-aged samples.
Figure 6b shows the comparison of the brucite peaks on the (001), (101), and (102) crystalline planes of the four samples at a curing time of 28 days. We found that as the percentage of the Nes addition increased, the intensity of the peaks decreased, the peaks became wider, and their corresponding 2θ decreased, or d-spacing increased accordingly. For the #4-28d sample with the 14.35 wt% Nes addition, the peak at (001) was no longer identified, and a diffraction peak close to the artinite ( 2 — 01) appeared. The chemical formula of artinite was MgCO3·Mg(OH)2·3H2O, and the ( 2 — 01) peak was the second-strongest peak in the JCPDS standard model with 2θ of 16.587°. After subtracting the background diffraction, the intensity of the brucite diffraction peak at (001) and its FWHM (width at half peak) values were plotted, as shown in Figure 6c. As shown in the figure, FWHM increased and gradually stabilized with an increase in Nes addition, and the peak intensity decreased and stabilized with an increase in Nes addition for the 3- and 28-day curing aged samples.

3.5. FT-IR Analysis and Group Properties

The FTIR spectra of the four samples and the synthesized Nes are shown in Figure 7. The 3691 cm−1 band in Figure 7a referred to the antisymmetric O–H stretching vibration of the oxide lattice in Mg(OH)2 [33]. This band also appeared in the samples containing Nes, but its peak shifted toward a larger wave number as the Nes addition increased, as shown in Figure 7b. At the same curing time of 28 days, the peak wave number was 3691 cm−1 for sample #1 with pure MgO and increased to 3694 and 3695 cm−1 for samples #3 and #4 with Nes additions, respectively. For sample #3 with the same Nes content, the corresponding peaks remained constant at 3694 cm−1 for curing times of 3 and 28 days. The band at 1411 cm−1 was only present in samples #3 and #4 with Nes (Figure 7a). This band was located in the 1400–1420 cm−1 region and represented a strong absorption band of the HCO3– unit [34]. This was slightly different from the absorption band of the HCO3– unit in the Nes raw material at 1394 cm−1 [35,36]. The two bands at 847 and 1101 cm−1 in the Nes spectrum, representing the absorption band of the CO32– unit, did not appear in samples #3 and #4, as they may have been too weak to detect. Sample #4 shows a weak and small peak at 1092 cm−1, which may be Artinite [28]. The information for each absorption peak corresponding to Figure 7 is presented in Table 3.

3.6. TG/DSC Analysis and Thermal Effects

The TG/DSC curves of the four water-cured samples are shown in Figure 8a. All samples showed significant weight loss due to Mg(OH)2 dehydration. The TG and DSC curves of all samples showed similar morphology, and the decreasing rate of the TG curve indicated a slow-fast-slow trend with increasing temperature. At the same time, the TG curves showed a single-step decreasing trend with a step temperature range of 357–406 °C, and all DSC curves showed a single heat absorption peak at 384–390 °C. Table 4 shows the dehydration temperature range, mass loss, inflection point of the TG curve Tip, and a peak temperature of the DSC curve Tp_DSC for Mg(OH)2. These two temperature values were 390 °C and 384 °C for the Mg(OH)2 dehydration process of the #1-28d sample with pure MgO, and the values were 395 °C and 390 °C for the #3-28d sample with the 7.87% Nes addition and 396 °C and 389 °C for the #4-28d sample with the 14.35% Nes addition. This implied that the samples with Nes required higher temperatures than the pure MgO paste to reach a certain dehydration state.
Notably, the TG curves of all samples containing Nes showed slight weight loss in the temperature range of 50–200 °C. Among these, a maximum weight loss of 2.1% was observed in sample #4-28d, while for the pure MgO paste (sample #1), almost no weight change was found in this range. Figure 8b shows the local DTG curves obtained after the differentiation of the TG curves with respect to temperature. We found that the weight loss (DTG peak area) at a temperature of 50–200 °C increased with the amount of Nes addition and the curing time of the samples with a corresponding increase in the peak temperature. The weight loss at this temperature range was due to the effect of dehydration, which meant that the samples containing the Nes additive contained a small amount of water with molecular crystallization.

4. Discussion

When the chemically pure, lightly burned MgO with fine particles was mixed with water, the surfaces of the MgO particles started to dissolve. When the concentration of Mg2+ and OH– ions in the solution reached supersaturation, the Mg(OH)2 crystals precipitated out. With the progression of the hydration process, the mixture coagulated, hardened, and eventually formed a block with a certain strength. Under the wet-air condition, the compressive strength increased with age. However, when the demolded samples were immersed in deionized water, the original dissolution–crystallization process was changed, and Mg(OH)2 developed into fine plate-like crystals, which were stacked together (Figure 5a). This structure was detrimental to the strength development of the samples.
The presence of HCO3– ions in the mixed solution after the addition of Nes changed the hydration process of MgO and affected the precipitation of the hydration products. This made the total pore volume of the samples larger, and the pore size smaller, with most of the pores consisting of nanopores, and the total pore surface area increased significantly (Table 2). The hydration products showed lamellar–lamellar interlacing growth (Figure 5b–d). The mechanism associated with this phenomenon remains to be explored. The paste still had good strength and high porosity due to the refinement of the pore size and the interlaced growth of the hydration products. XRD analysis showed that the crystal structure of the hydration products in the samples containing Nes was similar to that of brucite Mg(OH)2. With the 14.35 wt% Nes addition, the diffraction peak of brucite in the (001) plane was too weak and could not be observed, and a peak similar to that of the artinite ( 2 — 01) plane appeared. However, in the FTIR spectrum of sample #4-28d, no symmetric stretching peak at 1092 cm−1 [28,38] for the CO32– unit of this indeterminate phase was observed, and no other strong diffraction peaks of the indeterminate were found in the XRD spectrum.
The FTIR spectra of samples #3 and #4 with Nes additions showed a clear absorption peak at the 1411 cm−1 position, while sample #1 with pure MgO had no peak. The 1411 cm−1 peak corresponded to a strong absorption of HCO3–, indicating that the hydration product contains HCO3– structural units. From the TG and DTG curves, the sample with the Nes addition contained crystalline water that could be removed at low temperatures. The study of the MgO hydration product after Hmgs addition by Kuenzel et al. [28] found that although the XRD spectrum showed low crystallinity Mg(OH)2, the combined morphology, FTIR, and Raman spectroscopy results suggested that the hydration product composition should be between Mg(OH)2, Hmgs, and H2O in one of the phases. Based on the chemical expression of HMC, the hydration product of the Nes addition was written as xMgCO3·Mg(OH)2·yH2O, or against the structural formula of Nes crystals Mg(HCO3)(OH)·2H2O [37,38], this hydration product could be expressed as x[Mg(HCO3)(OH)]·Mg(OH)2·zH2O. Therefore, the hydration process of MgO with the Nes addition, as well as the total reaction, could be expressed using Equation (1) or Equation (2):
MgO + x[MgCO3·3H2O] → xMgCO3·Mg(OH)2·yH2O + (3x-y-1) H2O
MgO + x[Mg(HCO3)(OH)·2H2O] → xMg(HCO3)(OH)·Mg(OH)2·zH2O + (2x-z-1) H2O
Neglecting the dissolution loss or formation of other phases during hydration, the x-values of the final hydration products of samples #3 (7.87% Nes) and #4 (14.35% Nes) were calculated as 0.025 and 0.048, respectively. Due to the very small x-values, the hydration products showed structures and properties similar to Mg(OH)2. With an increase in Nes addition, the peaks of Mg(OH)2 in the XRD spectra of the cured paste hydration products showed a tendency to become lower and wider, indicating that the crystals were small and may have been new phases. In this case, the poor X-ray crystallinity was due to either being very thin in the direction perpendicular to the basal plane, or possibly due to some other kind of internal disorder. In the FTIR spectrum, the band at 3691 cm−1 changed regularly in the direction of the larger wavenumber.

5. Conclusions

(1)
The addition of a small amount of Nes also helped to improve the strength of reactive MgO paste under water-curing conditions. The hydration product changed from small plate-like Mg(OH)2 crystals to interlaced sheet-like crystals in samples containing Nes.
(2)
The porosity increased from 36.25% to 64.55%, and the total pore surface area increased from 4.6 m2/g to 118.5 m2/g. The total pore volume increased, the pore diameter decreased, and most of the pores were nanopores in the samples with a small amount of Nes addition.
(3)
Compared with the pure MgO sample, the hydration product diffraction peak of the sample with the Nes addition became lower and wider. The crystal structure of the hydration products was similar to that of Mg(OH)2, with a larger d-spacing at the (001), (101), and (102) planes.
(4)
FTIR and TG results showed that the hydration products contained HCO3– structural units and a small amount of crystallized water, which could be expressed as xMgCO3·Mg(OH)2·yH2O or x[Mg(HCO3)(OH)]·Mg(OH)2·zH2O. The samples with 7.87% and 14.35% Nes additions had x-values in the final hydration products of 0.025 and 0.048, respectively.

Author Contributions

Conceptualization, D.C.; Methods, R.S. and Y.H.; Software, R.S. and W.L.; Validation, R.S., D.C., and Y.H.; Formal analysis, D.C.; Investigation, R.S.; Data collation, Y.H.; Writing-original draft preparation, R.S. and D.C.; Writing-review and editing, R.S. and W.L. All authors have read and agreed to the published version of the manuscript.

Funding

This work was supported by a grant from the National Key Technologies Research and Development Program of China (No. 2022YFB2602605).

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

Not applicable.

Conflicts of Interest

The authors declare no conflict of interest.

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Materials 16 02445 g001 550
Figure 1. Diagram of Nes preparation apparatus: (a) schematic (1—CO2 gas cylinder; 2—hose; 3—CO2 flow controller; 4—mixing motor; 5—slurry drum; 6—slurry; 7—mixing blades; 8—mixer stand); (b) the diffraction pattern of MgO and Nes.
Figure 1. Diagram of Nes preparation apparatus: (a) schematic (1—CO2 gas cylinder; 2—hose; 3—CO2 flow controller; 4—mixing motor; 5—slurry drum; 6—slurry; 7—mixing blades; 8—mixer stand); (b) the diffraction pattern of MgO and Nes.
Materials 16 02445 g001
Materials 16 02445 g002 550
Figure 2. Experimental flow (weighing raw materials, mixing and casting of the slurry, and curing and testing of the samples).
Figure 2. Experimental flow (weighing raw materials, mixing and casting of the slurry, and curing and testing of the samples).
Materials 16 02445 g002
Materials 16 02445 g003 550
Figure 3. Compressive strength vs. curing time of the hydrated samples.
Figure 3. Compressive strength vs. curing time of the hydrated samples.
Materials 16 02445 g003
Materials 16 02445 g004 550
Figure 4. Cumulative pore size distribution curve of the hardened pastes. (a) #1-28d, (b) #2-28d, (c) #3-3d, (d) #3-28d, and (e) #4-28d.
Figure 4. Cumulative pore size distribution curve of the hardened pastes. (a) #1-28d, (b) #2-28d, (c) #3-3d, (d) #3-28d, and (e) #4-28d.
Materials 16 02445 g004
Materials 16 02445 g005 550
Figure 5. FESEM image of the hardened paste fracture. (a) #1-28d (×5000), (b) #3-3d (×40,000), (c) #3-28d (×40,000), (d) #4-28d (×50,000), and (e) MgO (×10,000).
Figure 5. FESEM image of the hardened paste fracture. (a) #1-28d (×5000), (b) #3-3d (×40,000), (c) #3-28d (×40,000), (d) #4-28d (×50,000), and (e) MgO (×10,000).
Materials 16 02445 g005
Materials 16 02445 g006 550
Figure 6. X-ray diffraction pattern of the hardened pastes and diversity of the Mg(OH)2 main peaks. (a) The XRD patterns of the water-cured samples; (b) the comparison of the brucite peaks on the (001), (101), and (102) crystalline planes; (c) the intensity of the brucite diffraction peak at (001) and its FWHM (width at half peak) values.
Figure 6. X-ray diffraction pattern of the hardened pastes and diversity of the Mg(OH)2 main peaks. (a) The XRD patterns of the water-cured samples; (b) the comparison of the brucite peaks on the (001), (101), and (102) crystalline planes; (c) the intensity of the brucite diffraction peak at (001) and its FWHM (width at half peak) values.
Materials 16 02445 g006
Materials 16 02445 g007 550
Figure 7. FTIR spectra of the hardened pastes and Nes raw material. (a) The four samples and the synthesized Nes; (b) local graph at 3691 cm−1.
Figure 7. FTIR spectra of the hardened pastes and Nes raw material. (a) The four samples and the synthesized Nes; (b) local graph at 3691 cm−1.
Materials 16 02445 g007
Materials 16 02445 g008 550
Figure 8. TG/DSC and partial DTG curves for the hardened pastes. (a) The TG/DSC curves of the four water-cured samples (The left arrow is the percentage weight loss and the right arrow is Heat Flow); (b) the local DTG curves.
Figure 8. TG/DSC and partial DTG curves for the hardened pastes. (a) The TG/DSC curves of the four water-cured samples (The left arrow is the percentage weight loss and the right arrow is Heat Flow); (b) the local DTG curves.
Materials 16 02445 g008
Table
Table 1. Correspondence of MgO–Nes molar ratios and their mass fractions.
Table 1. Correspondence of MgO–Nes molar ratios and their mass fractions.
Sample No.Designed MgO:Nes Molar RatioWater-to-Solid RatioPercentage of Nes Addition (wt%)
MgONes
#1101.10
#26411.14.14
#33211.17.87
#41611.114.35
Table
Table 2. Pore structure parameter of the hardened pastes.
Table 2. Pore structure parameter of the hardened pastes.
Sample No.#1-28d#2-28d#3-3d#3-28d#4-28d
MgO:Nes molar ratio1:064:132:132:116:1
Nes addition (wt%)04.147.877.8714.35
Total pore volume (mm3/g)351.3473.0506.1428.51059.6
Total pore area (m2/g)4.6121.3111.1112.7118.5
Average pore diameter (nm)303.515.618.215.235.8
Dry bulk density (kg/m3)103210541070893609
Porosity (%)36.2549.8354.1238.2764.55
Table
Table 3. Summary of the bands detected and their origins for the FTIR spectra in Figure 7.
Table 3. Summary of the bands detected and their origins for the FTIR spectra in Figure 7.
Band Position (cm−1)OriginMovementReference
603Mg-OMg-O bending vibration[36,37]
847CO32− from Nesν2 symmetric bending vibration[35,36]
1101CO32− from Nesν1 symmetric stretching vibration[35,36]
1394, 1514CO32−/HCO3− from Nesν3 antisymmetric stretching vibration[35,36]
1411HCO3− from unknown phase [34]
1641H2OH-O-H bending vibration[28]
3551Nes water of crystallization [36]
3691~3695Mg(OH)2Anti-symmetrical O-H stretching vibration of lattice hydroxide[28,33]
Table
Table 4. Thermal dehydration data for the hardened pastes from TG/DSC analyses.
Table 4. Thermal dehydration data for the hardened pastes from TG/DSC analyses.
Sample No.#1-28d#3-3d#3-28d#4-28d
Temperature range of dehydration (°C)310–602296–613293–604298–631
Inflection point of dehydration by TG (Tip) (°C)390394395396
Peak temperature of dehydration by DSC (Tp_DSC) (°C)384388390389
Mass loss of dehydration (%)27.125.927.828.3
Calculated Mg(OH)2 content in hydrated product (wt%)87.683.990.191.7
Heat absorption of dehydration (J/g)10741116975905
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MDPI and ACS Style

Shi, R.; Hao, Y.; Chen, D.; Liu, W. Effect of Low Nesquehonite Addition on the Hydration Product and Pore Structure of Reactive Magnesia Paste. Materials 2023, 16, 2445. https://doi.org/10.3390/ma16062445

AMA Style

Shi R, Hao Y, Chen D, Liu W. Effect of Low Nesquehonite Addition on the Hydration Product and Pore Structure of Reactive Magnesia Paste. Materials. 2023; 16(6):2445. https://doi.org/10.3390/ma16062445

Chicago/Turabian Style

Shi, Run, Yuehan Hao, Deping Chen, and Wenxin Liu. 2023. "Effect of Low Nesquehonite Addition on the Hydration Product and Pore Structure of Reactive Magnesia Paste" Materials 16, no. 6: 2445. https://doi.org/10.3390/ma16062445

APA Style

Shi, R., Hao, Y., Chen, D., & Liu, W. (2023). Effect of Low Nesquehonite Addition on the Hydration Product and Pore Structure of Reactive Magnesia Paste. Materials, 16(6), 2445. https://doi.org/10.3390/ma16062445

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