Next Article in Journal
Experience-Based Physico-Chemical Models for Long-Term Reinforcement Corrosion
Previous Article in Journal
Effect of Fluid Flow on the Corrosion Performance of as-Cast and Heat-Treated Nickel Aluminum Bronze Alloy (UNS C95800) in Saline Solution
 
 
Search for Articles:
Title / Keyword
Author / Affiliation / Email
Journal
Article Type
 
 
Advanced Search
 
Section
Special Issue
Volume
Issue
Number
Page
 
Journals
CMD
Volume 2
Issue 1
10.3390/cmd2010005
cmd-logo
Submit to this Journal Review for this Journal Propose a Special Issue
► Article Menu

Article Menu

share Share announcement Help format_quote Cite question_answer Discuss in SciProfiles thumb_up
...
Endorse textsms
...
Comment
first_page
settings
Order Article Reprints
Font Type:
Arial Georgia Verdana
Font Size:
Aa Aa Aa
Line Spacing:
Column Width:
Background:
Article

The Stability and Chloride Entrapping Capacity of ZnAl-NO2 LDH in High-Alkaline/Cementitious Environment

by
Zahid M. Mir
1,*,
Celestino Gomes
2,
Alexandre C. Bastos
2,
Rui Sampaio
2,
Frederico Maia
3,
Cláudia Rocha
3,
João Tedim
2,
Daniel Höche
1,
Mario G. S. Ferreira
2 and
Mikhail L. Zheludkevich
1,4
1
Institute of Materials Research, Helmholtz-Zentrum Geesthacht Centre for Materials and Coastal Research, Max-Planck Str. 1, 21502 Geesthacht, Germany
2
DEMaC—Department of Materials and Ceramic Engineering, and CICECO—Aveiro Institute of Materials, Universidade de Aveiro, 3810-193 Aveiro, Portugal
3
Smallmatek—Rua dos Canhas, 3810-075 Aveiro, Portugal
4
Faculty of Engineering, University of Kiel, Kaiserstrasse 2, 24143 Kiel, Germany
*
Author to whom correspondence should be addressed.
Corros. Mater. Degrad. 2021, 2(1), 78-99; https://doi.org/10.3390/cmd2010005
Submission received: 23 December 2020 / Revised: 9 February 2021 / Accepted: 18 February 2021 / Published: 21 February 2021
Browse Figures
Versions Notes

Abstract

:
In this work, the ZnAl-NO2 LDH (layered double hydroxide) is investigated as a possible additive for mitigating the chloride-induced corrosion of steel in reinforced concrete. The investigation focused on the stability and chloride binding capacity of this LDH in the pH range typical of cementitious materials. Until pH = 12.5 the material was stable and effective in capturing chloride ions from the surrounding aqueous environment. For higher pH, precisely that of hydrated cement, the LDH was partially dissolved and OH− preferentially entrapped instead of Cl−. These results suggested that ZnAl-NO2 has excellent chloride entrapping capability at neutral pH, but this is reduced with increasing pH. However, when the LDH was incorporated into mortars, the chloride ingress was delayed, signifying that the dissolution of LDH leads to a secondary mechanism responsible for chloride capture.

1. Introduction

The corrosion of steel in reinforced concrete affects infrastructures worldwide [1,2,3]. The cost of early repair and the reconstruction of these structures can lead to severe economic losses [4]. Concrete is a porous material [5], and aggressive species like chloride ions can pass through the concrete cover, until reaching the steel reinforcement, where they disrupt the steel native passive layer and initiate corrosion [6,7]. Innovative techniques are required to slow down the chloride ingress in concrete, delay the corrosion process and extend the service life of reinforced concrete infrastructures. Layered double hydroxides (LDHs) are a new class of concrete additives which can entrap aggressive anions from the environment and release selected anions (e.g., corrosion inhibitor) from their galleries. Potential applications include sequestration of chloride and carbonate ions in aggressive environments, which in turn can potentially prolong the service life of structures susceptible to corrosion. LDHs have gained attention in the recent years, due to their ion exchange properties, not only in concrete technology [8] but also in various branches of science and engineering [9], as a de-icing additive for asphalt roads [10], catalysis, [11], pharmaceutical applications [12], photochemistry [13], electrochemistry [14,15], biochemistry [16] and more.
Layered double hydroxides (LDHs), also known as “hydrotalcite-like” materials [9,17], can be synthesized by co-precipitation [18] of metal salts in alkaline medium, resulting in an ionic arrangement of positively charged brucite-like layers, together with anions between the layers, to balance the charge. LDHs can be represented by the following generalized formula: [M(II)1–x M(III)x (OH)2 ]x+ (An−)x/n mH2O, with M(II) as divalent, M(III) as trivalent metallic cations and An− as the interlayer anion [17,19]. LDHs have the potential of intercalating external anions by exchanging them with the anions originally present in their galleries, as represented in Figure 1. This process is called the ion exchange process and is usually dominated by the order of ions in the selectivity series for LDH.
Based on theoretical calculations, Costa et al. [20] concluded that Zn-Al-based LDHs have higher affinity to OH− than Cl−. They reported the anion selectivity order as CO32− > OH– > F– > Cl– > Br– > NO3−. The ions towards the left of the series are preferable towards ion sequestration by LDH, as compared to the ions on the right of the selectivity series. Hibino [21] pointed out that such selectivity series for a particular LDH can change under certain conditions. Apart from the ion preference in the selectivity series, other factors, such as anion size, anion concentration and temperature, can influence the ion exchange process [8]. In cementitious materials, like cement paste, mortars or concrete, the ionic-exchange mechanism can be exploited to entrap chloride ions, thereby retarding their ingress, and simultaneously release anions with corrosion-inhibition properties, e.g., NO2− [8,22]. If effective, this leads to a “self-protection” capability of concrete against corrosion of steel in concrete.
Earlier works on the use of LDH in cementitious environments include the controlled release of organic admixtures [23] and the acceleration of the hardening process with CaAl-Cl LDH [24]. Zhonge et al. analyzed the chloride-binding capacity of MgAl LDH intercalated with CO32− and NO3− and found higher capacity for the NO3− LDH type [25]. The effect of MgAl LDH on the microstructure and carbonation resistance of sulfoaluminate cement concrete was studied by Duan et al. [26]. In a separate study by the present authors [27], in situ XRD analysis revealed that MgAl LDH can possibly lead to the formation of higher amounts of AFm and thereby increase the chloride-binding capacity of concrete. Chen et al. [28] investigated the use of CaAl-NO3 LDH for the removal of chloride ions from concrete pore solutions and from cement paste. The sequestration of Cl− ions was explained by an ionic exchange mechanism following a Langmuir isotherm in cement matrix. Similar Langmuir-type binding isotherms were also reported by Yoon et al. for the capture of chloride ions by on calcined MgAl-based LDH in cement paste [29]. A review of LDH as smart additives of reinforced concrete for anticorrosion applications was provided by Yang et al. [30]. Most of the LDHs tested so far in concrete belong to one of the following systems: MgAl or CaAl. Only a few papers exist with ZnAl LDH studied for the chloride capture and nitrite release in saturated Ca(OH)2, i.e., simulated concrete pore solution [31]. Additionally, a comprehensive review on the various types and applications of LDH in cementitious materials has recently been published by the authors [8].
As mentioned previously, the use of Zn-Al LDH in cementitious systems has not been extensively studied so far. Therefore, in this work, the authors studied the behavior and stability of ZnAl-NO2 in depth. Additionally, this paper reflects on the results obtained in European Union’s LORCENIS project [32], which focused on the ZnAl-NO2 as a potential chloride-entrapping/corrosion-inhibiting additive for concrete. Due to these reasons, ZnAl-NO2 system has been used in this paper.
In the present work, the authors focused on characterizing the working mechanism of ZnAl-NO2 in high-alkaline environments typical to that of concrete and cement pastes. The broader goal of this study was to quantitatively and qualitatively assess the ion exchange process related to chloride ion capture by ZnAl-NO2 in alkaline environments. The assessment is reported for aqueous salt solutions, as well as for pore solutions. A step-wise approach was followed in this study. At first, the LDH was exposed only to an environment containing OH− anions, in order to verify its anion-capture capability, as well as its stability in alkaline environments. This was followed by exposing LDH to a multi-anionic environment, containing both Cl− and OH− ions. Moreover, the sequestration of each anion was evaluated, and the results are discussed in detail. Chloride-binding isotherms as a function of pH of the environment are also presented. Then the compatibility of the LDH with cement was analyzed by observing the effect of the LDH addition to cement paste in terms of the curing time. Furthermore, the chloride transport was monitored in mortars with LDH, by employing cast-in Cl− sensitive sensors. Finally, the corrosion properties of steel embedded in mortars containing LDH are presented, in order to highlight the role of NO2− release from LDH (due to ion exchange or partial dissolution of LDH).

2. Materials and Methods

2.1. Material Synthesis

The Zn-Al-NO2 LDH studied in this work was produced by Smallmatek, Lda, Aveiro, Portugal. It was prepared in a stainless-steel reactor, by co-precipitation of hydroxides from salts of divalent and trivalent cations, in a solution with an excess of sodium nitrite, and the pH adjusted to 10.0 ± 0.5 with sodium hydroxide. More details can be found in Reference [33]. The resulting slurry was washed with deionized water, filtered and dried with an industrial spray dryer, to guarantee uniform and fine powder.

2.2. Materials Characterization

The LDH particle size was measured with a Coulter LS230 Particle Size Analyzer (Coulter Corporation, Miami, FL, USA). XRD diffractograms were obtained with a diffractometer PANalytical X’Pert MPD PRO (Almelo, The Netherlands) with Bragg–Brentano geometry, Ni-filtered CuKα radiation, PIXcel1D detector, and step 0.026. The exposition was 2 s per step, in the angular range between 3° and 65°.

2.3. Stability of ZnAl-NO2 in the High pH Range

The chemical stability of the LDH was analyzed at neutral pH and in the pH range from 11 to 13.5, which encompasses the pH of aged and fresh concrete. One gram of LDH was immersed in 50 mL of aqueous solutions with different pH values, prepared with distilled water and KOH. After 30 days in a closed container, the remaining powders were washed, weighted by a lab scale and analyzed by XRD. The solution pH was measured by the potentiometric method with an Inlab Expert Pro pH combined electrode and a SevenMulti meter, both from Mettler Toledo (Columbus, OH, USA). The amount of NO2− in solution was measured with a UV-3100 UV–Vis–NIR spectrophotometer from Shimadzu (Kyoto, Japan), with the detection peak of interest occurring at 354 nm. Prior to the experimentation, the spectrophotometer was repeatedly calibrated by relating the intensity against various concentrations of NO2− in the calibration solutions.

2.4. Chloride Binding Capacity

The chloride-binding capacity of ZnAl-NO2 was studied with NaCl solutions ranging from 0.01 to 0.5 M at neutral pH, and then with pH from 11 to 13, following the test matrix shown in Figure 2. The tests were extended to leached pore solution extracts, in order to replicate a multi-ion competition scenario. Leached pore solution 1 (PS1) was made by mixing 3.5 g of ordinary Portland cement and 1.5 g of fly ash in 1 L of water, stirring for 24 h and allowed to rest for 3 days. The resulting pH was around 12.0. Leached pore solution 2 (PS2) was prepared by adding 50 g of cement to 1 L of water, stirring for 24 h and allowing to rest for 3 days prior to testing. The resulting pH was around 12.5. For each solution, 50 mL was added to a beaker, and the chloride concentration measured with a DX235-Cl ion-selective electrode (Mettler Toledo) connected with a mercury/mercurous sulfate reference electrode to a SevenMulti meter (Mettler Toledo). After a few minutes of stable reading, 1 g of LDH was added to solution, under stirring, while the Cl− concentration was monitored and pH measurements were carried out just before and after 5 min of LDH addition. The ion-selective electrode was calibrated against standard chloride solutions (0.001 M to 0.5 M), every time, prior to conducting measurements. The experimental setup is pictorially depicted in Figure 3. In some cases, the solid was recovered after 5 min of exposure and characterized by XRD. To verify the effect of time on the binding capacity, the Cl− and pH measurements were repeated after 15 days of the LDH addition.

2.5. Compatibility of LDH with Cement Paste

Cement pastes with 0.5 water-to-cement (w/c) ratio were prepared without (reference) and with 2 wt% LDH. Specimens with 30 × 30 × 10 mm3 were cast and cured in a humidity chamber.

2.6. Chloride Sensors Embedded in Mortars

The effect of LDH on the chloride ingress in mortars was assessed with embedded chloride sensors. The sensors consisted of 1 mm diameter silver wire, coated with silver chloride on the polished surface and encased in epoxy. The silver chloride coat was produced galvanostatically, with a constant current density of 2 mA/cm2, for 30 min, in 0.1 M HCl. Three of these Cl− sensitive sensors were placed at 0.5, 1 and 1.5 mm from the surface of the mortar samples (Figure 4a). Prior to embedment in mortars, the sensors were calibrated by recording potential readings for various concentrations of Cl− in KOH = 0.1 M (pH~13). The response of the sensors to chloride ions in high-pH media is presented in Figure 4b. The chloride concentration in the mortars was then obtained by using the obtained calibration curve. These calibrations were repeated periodically, with sensors permanently immersed in KOH = 0.1 M (pH~13), to certify that the response did not change with the continuous exposure to the alkaline environment of mortar.
The mortars samples were cast in 5 × 5 × 5 cm3 samples, with a composition of 14.5 wt% CEM II/B-L 32.5 N cement, 13% water and 72.5% of 0–2 mm size siliceous sand. The water/cement ratio was equal to 0.9 and was chosen for fast permeation and, consequently, to accelerate the chloride ingress. LDH was added in an amount corresponding to 2 wt% of cement (0.3 wt% of total mass of mortar). The mortar samples were cured for 28 days, in a humidity chamber, and then the samples were immersed in 3.5% NaCl aqueous solution. The potential of the sensors was measured against a saturated calomel electrode (SCE) placed in the external solution, using a CompactStat potentiostat connected to a peripheral differential amplifier (Ivium Technologies, Eindhoven, The Netherlands), for simultaneous measurement of several channels.

2.7. Corrosion Testing

Mortar samples with the composition presented in Section 2.6 and 7 × 4 × 4 cm3 size were produced, with a non-corrugated steel bar of 8 mm diameter placed in the middle. The steel bars were cleaned with 50% vol. HCl solution and abraded down to 1200 grade SiC paper, just before the embedment in the mortars. After 24 h, the samples were demolded and were left curing for 8 days, immersed in water. The samples were finally transferred to 3.5% NaCl solution, and the open-circuit potential and polarization resistance were measured periodically with a Autolab PGSTAT 204 potentiostat with a platinum counter electrode and a SCE electrode as reference. The polarization resistance was measured from −10 to +10 mV, with respect to the open-circuit potential, with a scan rate of 0.1 mV s−1.

3. Results and Discussion

3.1. Characterization of the ZnAl-NO2

The particle size distribution of the LDH powder is presented in Figure 5a. It ranged between 40 nm and 150 μm, with a mean particle size of 22 μm. Almost 10% of the particles exhibited a particle size of less than 5 μm. The XRD pattern prior to exposure is depicted in Figure 5b and shows the reflections 003, 006, 110 and 113 at 11.6°, 23°, 60.2° and 61.5°. These reflections coincide with reflections reported in the literature for ZnAl-NO2 [31] and also with other LDHs with NO2− in the interlayer space [22,34].

3.2. Stability in High-Alkaline Environment

The effect of pH in the range between 11 and 13.5 has been studied. The LDH and solution were analyzed 30 days after 1 g of powder was added to the 50 mL solution. After 30 days, the powders were extracted from the solutions and weighed. LDH powder was present in all samples. However, the amount of powder left at a high pH was less, indicating that a partial dissolution of LDH could have taken place. In a parallel experiment, it was verified that about 95% of solid remained undissolved at pH 12, decreasing to 60% at pH 13 and only 20% at pH 14. The pH of the solution just before and 30 days after the addition of LDH is presented in Figure 6a). The pH of the solutions inside the closed containers decreased noticeably. This was attributed to the capture of OH− in solution by the LDH powder. A drop of three units in the pH scale was observed, showing a remarkable efficiency of this LDH to capture OH−. For a higher pH, the amount of captured OH− decreased (almost no pH drop), because most of the LDH was dissolved. The region of partial dissolution is marked in the figure.

3.2.1. Release of NO2− Ions

Considering that the capture of OH− occurs by an ionic exchange mechanism, as expected for a LDH [9,15,17,22,23,30,31,33,34], the intercalated NO2− ions must leave the LDH interlayer and pass to solution, to allow the entrance of the incoming OH− ions. Indeed, after 30 days of immersion, NO2- was detected in all the solutions. It was observed that the concentration of NO2- increased with an increase of pH, as shown in Figure 6b.

3.2.2. XRD Analysis of LDH Exposed to Alkaline Solutions

After the 30-day immersion period, the remaining powders were filtered, washed and dried in a vacuum oven, at 40 °C, for 24 h. Figure 7 shows the XRD patterns of the LDH before (base) and after immersion in the different solutions. The reflections 006 and 003 are related to basal planes while the peaks 110 and 113 correspond to non-basal planes. The magnification of the plot around the peak 003 (2θ between 10°and 12°) shows a shift towards a higher angle as the pH increases, signifying a contraction of the interlayer.
Bragg’s law [35] was used to calculate the interlayer spacings d003 and d110 from the 2θ peak locations, using λα = 1.540598 Å. The spacing d003 gives the thickness of a single brucite-like layer and one interlayer, while d110 is the distance between two-metallic cations in the brucite-like layer. A shift of d003 on the 2θ axis corresponds to a change in the interlayer distance, as observed in Figure 7b. In Figure 8, the calculated d003 and d110 values are plotted for each pH. A clear d003 shift to the right on the 2θ axis occurs as the pH increases, which is indicative of a smaller interlayer distance, signifying anion exchange with a smaller radius ion. The OH− ion has a smaller size than the NO2− ion; the anionic exchange reduces the interlayer spacing, leading to higher 2-theta reflections. This has also been previously reported by Tedim et al. [15]. However, the 003 peaks in mild pH could also show an overlap of LDH-NO2− and LDH-OH−, due to the possible parallel placement of NO2− in the interlayer. The NO2− ion placed inclined to the cationic layers will tend to show more layer contraction upon ion exchange with OH− (Figure 7b). The parameter for cationic spacing (d110) in the brucite-like layer stays constant as the pH increases, signifying that only anionic exchange has occurred as external concentration of OH− increased, and the cationic layer has stayed intact and unchanged.
These XRD peaks are also indicative of the structural stability in the high alkaline range. The partial dissolution of LDH starts around pH 12.5. The powders until this pH show characteristic peaks of the LDH, despite the shift in the intercalated anion, but from pH 12.5 onwardsup, new peaks are detected and attributed to ZnO, Zn(OH)2, Al2O3, etc. Finally, the XRD pattern of the small amount of solid that did not dissolve at pH 13.48 shows no peaks of the LDH (the LDH structure is lost) and is dominated by the peaks of oxides and hydroxides of Zn and Al, which were already visible in pH 12.45 and 12.82.

3.3. Chloride Entrapment and the Effect of pH

For the application of ZnAl-NO2 as chloride-entrapping additive in cementitious environments, it is highly relevant to verify the Cl− binding capacity of this LDH in the presence of a high concentration of OH− ions. Therefore, the binding capacity of the LDH as a function of chloride concentration and pH was investigated. Representative results are presented in Figure 9, for starting NaCl solutions of 10, 100 and 500 mM with different pH values. The concentrations are plotted normalized, i.e., they appear divided by the starting concentration, for a better comparison of the changes in the different cases. These plots show the drop in chloride concentration after LDH was added to solution. The pH before and after the addition of LDH is also shown.
Figure 9a,b refer to the tests conducted with a starting chloride concentration of 10 mM at different pH. The highest chloride capture occurred at the lowest pH (6.94), where the concentration dropped to ~30 percent of the initial value. The process is very fast, taking less than 1 min to attain equilibrium. The Cl− capture at this pH (6.94) took place with a slight increase in the pH. This pH increase could be due to the release of OH− bound to the surface of the LDH or to a small dissolution of the LDH itself. In fact, the addition of 1 g of LDH to distilled water increased the pH and the conductivity of the solution, confirming that ions have passed from the LDH to solution. At pH 10.59, almost the same amount of chloride ions was captured, and it was accompanied by a decrease of pH from 10.59 to 7.5. This signifies that both Cl− and OH− were captured by the LDH. As the pH rises, so rises the amount of OH− that is captured, while the entrapment of chloride significantly decreases. Above pH 12, the amount of Cl− captured becomes very small.
A similar description applies for the other NaCl concentrations. The higher capture occurs in near-neutral solution, decreasing with the increase in pH, until it becomes almost negligible at a very high pH. However, it is noticeable that, for the same pH, the amount of OH− captured is smaller as the concentration of Cl− increases. The tendencies are better perceived in Figure 10. The ZnAl-NO2 has higher selectivity to OH− than Cl−, and for a higher pH, it is captured preferentially with almost no Cl− captured. However, the capture of OH− is not so effective for a higher concentration of chloride. These results show that, in spite of the higher importance of selectivity, the concentration also counts. It is also evident that LDH leads to a decrease of pH of the surrounding solution, which can bring serious risks to the stability of the passive film on the rebar surface.

3.3.1. Effect of Time on the Chloride Entrapment

The entrapment tests described in the last section were conducted for just 300 s and did not continue, because the ionic exchange was quite fast after the addition of LDH, happening in less than 1 min, with the subsequent readings being stable. In any case, the samples were sealed for 15 days and then analyzed again, to look for any changes in Cl− concentration and pH. As confirmed in Figure 11, with two representative examples, no significant changes were detected in both parameters measured after 300 s and 15 days. This confirms that the process is very fast, without further evolution.
The XRD analysis of two powders after 15-day exposure to alkaline solution, with and without NaCl, is presented in Figure 12. A clear shift of the 003 peak is seen for both the powders, as compared to the base material. The peaks of the powders exposed to just OH− or to OH− and Cl− are quite close to each other and are not clearly distinguishable.

3.3.2. Chloride Binding Capacity

The chloride-binding capacity can be defined as the amount of chloride ion that is bound by a given mass of LDH. It can be expressed as the amount of Cl− ion bound to LDH per unit mass of LDH at the onset of equilibrium. As such, the chloride-binding capacity represents a heterogeneous equilibrium between the Cl− bound to LDH and the free Cl− available in the solution. However, this equilibrium is sensitive to the pH of the environment and is explained later. The chloride-binding capacity can be determined by using the following formula [22,28]:
B c =   V s o l   ( C 0 − C e )   M C l m L D H
where Bc is the binding capacity (in mg/g), Vsol is the volume of solution (L), mLDH is the mass of LDH added to the solution (g), C0 and Ce are the initial and equilibrium chloride concentrations (mM) and MCl is the molar mass of chloride. The binding (or loading) capacity of ZnAl-NO2 for Cl− was calculated from the results of the chloride entrapment studies, using Equation (1), and is presented in Figure 13. The binding capacity increased with the Cl− concentration, up to a value where it then remained constant. The highest chloride loading was ~45 mg/g (1.28 mmol/g) and occurred at near neutral pH for the initial chloride concentration of 250 mM. The binding capacity is strongly dependent of the pH. At pH 12, it was half of the value in near-neutral pH, and above pH = 12.5, no substantial chloride was captured. The data for these equilibrium isotherms were obtained at room temperature (23 ± 1 °C). It is known that the loading capacity of Zn-Al-based LDH increases with temperature [36].

3.4. Compatibility with Cement

The experiments described so far were done in aqueous solution, with most of them at a high pH, to reflect the conditions inside cementitious materials. Naturally, the best approach is to test the LDH directly incorporated in these materials. It was decided to perform tests with mortars with 2% LDH with respect to cement. Before that, the compatibility of the ZnAl-NO2 with cement was investigated (Figure 14). It was observed that addition of LDH had a retarding effect on the cement curing. The sample with LDH displayed a slow curing, as compared to the reference samples. Cement paste (w/c = 0.5) with 2 wt% LDH took a very long time to harden, that is, around 17 days, compared to one day of the reference sample (without LDH). It is well-known that zinc ions can retard the hydration process. Trezza [37] used IR, XPS and calorimetry to investigate the effect of Zn2+ on the hydration processes and observed the delay of the cement hydration and attributed this to the formation of a new phase, Ca(Zn(OH3)2).2H2O. Citing Asavapisit et al. [38], Trezza concluded that the formation of Ca-Zn complexes decreased the concentration of Ca2+ ions required to form the CSH phase. The higher the concentration of Zn2+, the greater the quantity of the Ca-Zn phase and the longer the hydration time. Stephan et al. [39] also concluded that formation of the Ca-Zn phase significantly retards the hydration process by reducing the concentration of OH− and Ca2+ ions.
To confirm that it was the Zn2+ from LDH dissolution that interfered with the curing, cement pastes were cast with Zn(NO3)2. Similar to specimens with LDH, the samples showed a clay-like behavior and took a long time to harden. To rule out the effect of NO3− on the hydration process, samples were cast with NaNO3 with the same amount of NO3− as the samples with Zn(NO3)2 as shown in Figure 14. NO3− ions are traditionally used as setting accelerators in concrete, usually in the form of Ca(NO3)2 [40,41].
It is also important to note that the LDH particle size is a very important factor that should be taken into consideration. In a separate study from the authors [42], it was observed that a curing time similar to the reference samples was obtained when LDH particles of mean size ~125 μm were used, instead of the ~25 μm used in the present study. Therefore, the authors acknowledge that particle size plays a crucial role as bigger LDH agglomerates can have a reduced exposed surface area, leading to a lower dissolution at high pH. The effect of the particle size of LDH on the properties on concrete, especially chloride ingress, has been documented in the studies by Qu et al. [43]. The results reported in this work are confined to only one particular particle size, i.e., ~25 μm. For different particle sizes, reproducibility can be affected. Further studies are being planned to better characterize the effect of LDH and its particle sizes in cement paste hydration, and such studies will be reported in the future.

3.5. Embedded Sensors and Chloride Ingress in Mortar

To directly assess the effect of LDH on the transport of Cl− inside cementitious materials, chloride sensors were cast in mortar samples, as described in Section 2.6. The mortars were immersed in 3.5% NaCl, and the potential of the sensors was measured, over time, against a reference electrode placed in the solution. From the chloride concentrations in the different positions of the mortar and at the different times, it was possible to plot the chloride profile inside the reference mortar and inside the mortar with ZnAl-NO2, presented in Figure 15a,b respectively. In these plots, 0 cm corresponds to the surface of the mortar in contact with the solution, while the other values are the position of the sensors inside the mortar.
The chloride penetration was detected first by the sensors closer to the surface. Interestingly, with time, the peak chloride concentration was found not at the surface but 1 cm inside the mortar. This is a common observation [44,45,46] that has been attributed to a skin effect, i.e., to a different composition of the surface layers, compared to the bulk, due to contact with the casting mold [44,45]. Other authors attributed this effect to the gradient of moisture in the first few layers of the sample [44], as well as to surface reactions of the surface with the exposure environment [46]. The fact that the sensors were able to capture the concentration peak is an indication of their good functioning. The most important observation in Figure 15 is the slower ingress of chloride in the mortar with LDH.

3.6. Corrosion of Steel Bar in Mortar with and without ZnAl-NO2

In a final set of tests, steel rebars were placed in mortars without and with LDH (2 wt%, with respect to cement, or 0.3 wt% with respect to the total mass of mortar). The samples were exposed to 3.5% NaCl, and the corrosion potential (Ecorr) and polarization resistance (Rp) were monitored over time. The results are presented in Figure 16. The less negative Ecorr and the higher Rp of the steel in mortars with LDH point to lower corrosion, compared to the reference samples. The presence of LDH in the mortar seems to play a positive role, which can be even more pronounced if a higher amount of LDH was present.
The experiments with the LDH in mortars showed positive effects (lower ingress of chloride in mortar and higher corrosion resistance of steel), despite the low amount of LDH added (0.3 wt%) and the high porosity of the mortar. It is possible that the dissolution of LDH releases aluminum ions, which will promote the formation of more AFm phases (family of hydrated calcium aluminates) during cement hydration. This has been previously demonstrated by the authors, in a separate study, where the formation of AFm was recently confirmed by using in situ XRD on hydrating cement pastes with 2% Mg-based LDH. The reader is directed to Mir et al. [27], for detailed information on this effect. The dissolution of LDH leads to the formation of extra quantities of AFm which can chemically bind chloride ions. The extra amount of AFm phases can thus lead to additional chemical binding of chloride ions by forming Friedel’s salt and Kuzel’s salt and is also reported in the studies by Chen et al. [47]. Additionally, the filler effect of remaining undissolved LDH particles can play a positive role in chloride ingress by making the microstructure more tortuous, without decreasing the total porosity [43]. The higher corrosion resistance of steel in the mortar that contains LDH can be simply due to the release of NO2− to the pore solution, as a result of the LDH dissolution and ion exchange with OH− on the remaining powder. This contrast between the results with LDH in solution and in mortar needs more investigation, and additional studies are planned for the future.
These results with mortars are still preliminary because the experiments were performed with a limited number of replicate specimens (three of each type), in porous mortar (to accelerate the ion transport process), and the amount of LDH was only 0.3 wt% to the total mass of the mortar. Work is being performed with a higher number of samples, with better quality mortar, higher amounts of LDH and longer testing times in the mortar, in order to better understand the behavior of the LDH inside mortars, and will be reported in the future.

4. Conclusions

Based on the discussion presented in this work, the following conclusions can be drawn.
  • The Zn-Al LDH presents very good chloride-capture capability in near-neutral pH. Our investigations reported a peak binding capacity of about ~45 mg of Cl per gram of LDH. However, as the pH increases, the chloride-capture capability of Zn-Al LDH is reduced.
  • The LDH is stable in alkaline medium, until pH ~12.5. Partial dissolution occurs at a higher pH, with the release of the constituent anions (Zn2+, Al3+, NO2−) to the environment.
  • The ZnAl-NO2 delays the hardening of cement paste and mortars. This has been attributed to the zinc ions released by the partial LDH dissolution which interfere with the cement hydration reaction.
  • The partial dissolution and preferential capture of OH− at the pH values typical of cementitious material suggest the inadequacy of ZnAl-NO2 for the chloride capture inside concrete, where a pH higher than 13 is possible.
  • Mortars with the LDH presented a slower penetration of Cl− ions and led to higher corrosion resistance of the embedded steel rebar, even with a small amount (0.3% of total mass of mortar). Earlier studies pointed out that LDH dissolution can possibly lead to higher amounts of AFm being generated. However, additional experiments are needed to clarify this effect for ZnAl LDH. As a future scope to this work, more work will be performed to investigate the dissolution and working mechanism of LDH in concrete and will be reported in future.

Author Contributions

Conceptualization, Z.M.M., C.G. and A.C.B.; formal analysis, Z.M.M., C.G., A.C.B., R.S., F.M. and C.R.; investigation, Z.M.M., C.G. and A.C.B.; resources, F.M. and C.R.; supervision, A.C.B., F.M., C.R., J.T., D.H., M.G.S.F. and M.L.Z.; writing—original draft, Z.M.M. and A.C.B.; writing—review and editing, A.C.B. and M.L.Z. All authors have read and agreed to the published version of the manuscript.

Funding

This research was funded by the HORIZON 2020 collaborative project “LORCENIS” (Long Lasting Reinforced Concrete for Energy Infrastructure under Severe Operating Conditions, Grant agreement n° 685445), the European Union’s COST Action (SARCOS, Self-healing As preventive Repair of Concrete Structures), under grant agreement No. CA15202, and in the scope of the project CICECO—Aveiro Institute of Materials, POCI-01-0145-FEDER-007679 (FCT Reference UID/CTM/50011/2013). AB acknowledges FCT—Fundação para a Ciência e a Tecnologia, I.P., in the scope of the framework contract foreseen in the numbers 4, 5 and 6 of the article 23, of the Decree-Law 57/2016, of 29 August, changed by Law 57/2017, as of 19 July.

Data Availability Statement

The authors declare that the data presented in this work are available within the article. Extra data could be requested from the corresponding author.

Conflicts of Interest

The authors declare no conflict of interest. The funders had no role in the design of the study; in the collection, analyses or interpretation of data; in the writing of the manuscript; or in the decision to publish the results.

References

  1. Page, C.L. Mechanism of Corrosion Protection in Reinforced-Concrete Marine Structures. Nature 1975, 258, 514–515. [Google Scholar] [CrossRef]
  2. Tuutti, K. Corrosion of Steel in Concrete. Technical Report; Swedish Cement and Concrete Research Institute: Stockholm, Sweden, 1982. [Google Scholar]
  3. Bertolini, L.; Elsener, B.; Pedeferri, P.; Redaelli, E.; Polder, R. Corrosion of Steel in Concrete: Prevention, Diagnosis, Repair; Wiley: Hoboken, NJ, USA, 2013. [Google Scholar]
  4. Angst, U. Challenges and Opportunities in Corrosion of Steel in Concrete. Mater. Struct. 2018, 51, 1–20. [Google Scholar] [CrossRef] [Green Version]
  5. Lian, C.; Zhuge, Y.; Beecham, S. The Relationship between Porosity and Strength for Porous Concrete. Constr. Build. Mater. 2011, 25, 4294–4298. [Google Scholar] [CrossRef]
  6. Alonso, C.; Andrade, C.; Castellote, M.; Castro, P. Chloride Threshold Values to Depassivate Reinforcing Bars Embedded in a Standardized Opc Mortar. Cem. Concr. Res. 2007, 30, 1047–1055. [Google Scholar] [CrossRef]
  7. Ghods, P.; Isgor, O.B.; McRae, G.A.; Li, J.; Gu, G.P. Microscopic Investigation of Mill Scale and Its Proposed Effect on the Variability of Chloride-Induced Depassivation of Carbon Steel Rebar. Corros. Sci. 2011, 53, 946–954. [Google Scholar] [CrossRef]
  8. Mir, M.Z.; Bastos, A.; Höche, D.; Zheludkevich, M.L. Recent Advances on the Application of Layered Double Hydroxides in Concrete—A Review. Materials 2020, 13, 1426. [Google Scholar] [CrossRef] [Green Version]
  9. Li, F.; Duan, X. Applications of Layered Double Hydroxides. In Layered Double Hydroxides; Duan, X., David, E.G., Eds.; Springer: Berlin/Heidelberg, Germany, 2006. [Google Scholar]
  10. Peng, C.; Yu, J.Y.; Zhao, Z.J.; Dai, J.; Fu, J.Y.; Zhao, M.L.; Wang, W. Synthesis and Properties of a Clean and Sustainable Deicing Additive for Asphalt Mixture. PLoS ONE 2015, 10, e0115721. [Google Scholar] [CrossRef] [PubMed]
  11. Kirm, I.; Francesc, M.; Xavier, R.; Cesteros, Y.; Salagre, P.; Sueiras, J. Epoxidation of Styrene with Hydrogen Peroxide Using Hydrotalcites as Heterogeneous Catalysts. Appl. Catalysis A General 2004, 272, 175–185. [Google Scholar] [CrossRef]
  12. Park, D.H.; Choi, G.; Choy, J.H. Bio-Layered Double Hydroxides Nanohybrids for Theranostics Applications. In Photofunctional Layered Materials; Dongpeng, Y., Min, W., Eds.; Springer International Publishing: Cham, Switzerland, 2015. [Google Scholar]
  13. Ogawa, M.; Kazuyuki, K. Photofunctions of Intercalation Compounds. Chem. Rev. 1995, 15, 399–438. [Google Scholar] [CrossRef]
  14. Liao, C.-S.; Wei-Bin, Y. Structure and Conductive Properties of Poly (Ethylene Oxide)/Layered Double Hydroxide Nanocomposite Polymer Electrolytes. Electrochim. Acta 2004, 49, 4993–4998. [Google Scholar] [CrossRef]
  15. Tedim, J.; Kuznetsova, A.; Salak, A.N.; Montemor, F.; Snihirova, D.; Pilz, M.; Zheludkevich, M.L.; Ferreira, M.G.S. Zn-Al Layered Double Hydroxides as Chloride Nanotraps in Active Protective Coatings. Corros. Sci. 2012, 55, 1–4. [Google Scholar] [CrossRef]
  16. Choy, J.H.; Kwak, S.Y.; Park, J.S.; Jeong, Y.J.; Portier, J. Intercalative Nanohybrids of Nucleoside Monophosphates and DNA in Layered Metal Hydroxide. J. Am. Chem. Soc. 1999, 121, 1399–1400. [Google Scholar] [CrossRef]
  17. Martin, K.J.; Thomas, J.P. Layered Double Hydroxides as Supported Anionic Reagents. Halide-Ion Reactivity in Zinc Chromium Hexahydroxide Halide Hydrates [Zn2Cr(OH)6x. NH2O](X = Cl, I). J. Am. Chem. Soc. 1986, 108, 541–542. [Google Scholar] [CrossRef] [PubMed]
  18. Crepaldi, E.L.; Paulo, C.P.; João, B.V. Comparative Study of the Coprecipitation Methods for the Preparation of Layered Double Hydroxides. J. Braz. Chem. Soc. 2000, 11, 64–70. [Google Scholar] [CrossRef] [Green Version]
  19. He, J.; Min, W.; Bo, L.; Yu, K.; David, G.E.; Duan, X. Preparation of Layered Double Hydroxides. In Layered Double Hydroxides; Duan, X., David, G.E., Eds.; Springer: Berlin/Heidelberg, Germany, 2006. [Google Scholar]
  20. Costa, D.G.; Rocha, A.B.; Souza, W.F.; Chiaro, S.S.X.; Leitão, A.A. Comparative Structural, Thermodynamic and Electronic Analyses of Znalan−Hydrotalcite-Like Compounds (an−Cl−, F−, Br−, OH−, CO32− or NO3−): An Ab Initio Study. Appl. Clay Sci. 2012, 56, 16–22. [Google Scholar] [CrossRef]
  21. Hibino, T. Anion Selectivity of Layered Double Hydroxides: Effects of Crystallinity and Charge Density. Eur. J. Inorg. Chem. 2018, 6, 722–730. [Google Scholar] [CrossRef] [Green Version]
  22. Zuo, J.D.; Wu, B.; Luo, C.Y.; Dong, B.Q.; Xing, F. Preparation of Mgal Layered Double Hydroxides Intercalated with Nitrite Ions and Corrosion Protection of Steel Bars in Simulated Carbonated Concrete Pore Solution. Corros. Sci. 2019, 152, 120–129. [Google Scholar] [CrossRef]
  23. Raki, L.; Beaudoin, J.J.; Mitchell, L. Layered Double Hydroxide-Like Materials: Nanocomposites for Use in Concrete. Cem. Concr. Res. 2004, 34, 1717–1724. [Google Scholar] [CrossRef] [Green Version]
  24. Xu, S.; Chen, Z.; Zhang, B.; Yu, J.; Zhang, F.; Evans, D.G. Facile Preparation of Pure CaAl-Layered Double Hydroxides and Their Application as a Hardening Accelerator in Concrete. Chem. Eng. J. 2009, 155, 881–885. [Google Scholar] [CrossRef]
  25. Shui, Z.; Juntao, M.; Wei, C.; Xiaoxing, C. Chloride Binding Capacity of Cement Paste Containing Layered Double Hydroxide (Ldh). J. Test. Eval. 2012, 40, 796–800. [Google Scholar]
  26. Duan, P.; Chen, W.; Ma, J.; Shui, Z. Influence of Layered Double Hydroxides on Microstructure and Carbonation Resistance of Sulphoaluminate Cement Concrete. Constr. Build. Mater. 2013, 48, 601–609. [Google Scholar]
  27. Mir, Z.M.; Alexandre, B.; Celestino, G.; Urs, M.; Alonso, M.C.; Villar, K.; Miguel, P.; Rabade, F.M.; Cláudia, M.; Rocha, P.M.; et al. Numerical and Experimental Analysis of Self-Protection in Reinforced Concrete Due to Application of Mg–Al–No2 Layered Double Hydroxides. Adv. Eng. Mater. 2020, 22, 2000398. [Google Scholar] [CrossRef]
  28. Chen, Y.X.; Shui, Z.H.; Chen, W.; Chen, G.W. Chloride Binding of Synthetic Ca-Al-No3 Ldhs in Hardened Cement Paste. Constr. Build. Mater. 2015, 93, 1051–1058. [Google Scholar] [CrossRef]
  29. Yoon, S.; Moon, J.; Bae, S.; Duan, X.N.; Giannelis, E.P.; Monteiro, P.M. Chloride Adsorption by Calcined Layered Double Hydroxides in Hardened Portland Cement Paste. Mater. Chem. Phys. 2014, 145, 376–386. [Google Scholar] [CrossRef]
  30. Yang, Z.; Fischer, H.; Polder, R. Modified Hydrotalcites as a New Emerging Class of Smart Additive of Reinforced Concrete for Anticorrosion Applications: A Literature Review. Mater. Corros. Werkst. Korros. 2013, 64, 1066–1074. [Google Scholar] [CrossRef]
  31. Tian, Y.W.; Dong, C.F.; Wang, G.; Cheng, X.Q.; Li, X.G. Zn-Al-No2 Layered Double Hydroxide as a Controlled-Release Corrosion Inhibitor for Steel Reinforcements. Mater. Lett. 2019, 236, 517–520. [Google Scholar] [CrossRef]
  32. SINTEF. Norway European Union’s Project, Lorcenis–Long Lasting Reinforced Concrete for Energy Infrastructure under Severe Operating Conditions, European Union Horizon 2020 Programme; SINTEF: Trondheim, Norway, 2016–2020. [Google Scholar]
  33. Poznyak, S.K.; Tedim, J.; Rodrigues, L.M.; Salak, A.N.; Zheludkevich, M.L.; Dick, L.F.P.; Ferreira, M.G.S. Novel Inorganic Host Layered Double Hydroxides Intercalated with Guest Organic Inhibitors for Anticorrosion Applications. Acs Appl. Mater. Interfaces 2009, 1, 2353–2362. [Google Scholar] [CrossRef]
  34. Cao, Y.H.; Dong, S.G.; Zheng, D.J.; Wang, J.J.; Zhang, X.J.; Du, R.G.; Song, G.L.; Lin, C.J. Multifunctional Inhibition Based on Layered Double Hydroxides to Comprehensively Control Corrosion of Carbon Steel in Concrete. Corros. Sci. 2017, 126, 166–179. [Google Scholar] [CrossRef]
  35. Ewald, P.P. William Henry Bragg and the New Crystallography. Nature 1962, 195, 320–325. [Google Scholar] [CrossRef]
  36. Lv, L.; Sun, P.; Gu, Z.; Du, H.; Pang, X.; Tao, X.; Xu, R.; Xu, L. Removal of Chloride Ion from Aqueous Solution by Znal-No(3) Layered Double Hydroxides as Anion-Exchanger. J. Hazard. Mater. 2009, 161, 1444–1449. [Google Scholar] [CrossRef]
  37. Trezza, M.A. Hydration Study of Ordinary Portland Cement in the Presence of Zinc Ions. Mater. Res. 2007, 10, 331–334. [Google Scholar] [CrossRef]
  38. Asavapisit, S.; Fowler, G.; Cheeseman, C.R. Solution Chemistry During Cement Hydration in the Presence of Metal Hydroxide Wastes. Cem. Concr. Res. 1997, 17, 1249–1260. [Google Scholar] [CrossRef]
  39. Stephan, D.H.; Maleki, D.K.; Eber, B.; Härdtl, R. Influence of Cr, Ni, and Zn on the Properties of Pure Clinker Phases: Part, I. C3s. Cem. Concr. Res. 1999, 29, 545–552. [Google Scholar] [CrossRef]
  40. Franke, W.; Magdalena, B.-S.; Tandre, O.; Gaurav, S. The Fate of Nitrate Ions in Concrete under the Focus of Corrosion Inhibition. In Proceedings of the 2nd International Conference on Durability of Concrete Structures, ICDCS 2010, Sapporo, Japan, 24–26 November 2010. [Google Scholar]
  41. Justnes, H.; Nygaard, E.C. Technical Calcium Nitrate as Set Accelerator for Cement at Low Temperatures. Cem. Concr. Res. 1995, 25, 1766–1774. [Google Scholar]
  42. Gomes, G.; Mir, Z.; Sampaio, R.; Bastos, A.; Tedim, J.; Maia, F.; Rocha, C.; Ferreira, M. Use of Znal-Layered Double Hydroxide (Ldh) to Extend the Service Life of Reinforced Concrete. Materials 2020, 13, 1769. [Google Scholar]
  43. Qu, Z.Y.; Yu, Q.L.; Brouwers, H.J.H. Relationship between the Particle Size and Dosage of Ldhs and Concrete Resistance against Chloride Ingress. Cem. Concr. Res. 2018, 105, 81–90. [Google Scholar] [CrossRef]
  44. Andrade, C.; Diez, L.M.; Alonso, C. Mathematical Modeling of a Concrete Surface ’’Skin Effect’’ on Diffusion in Chloride Contaminated Media. Adv. Cem. Based Mater. 1997, 6, 39–44. [Google Scholar] [CrossRef]
  45. Castro, P.; de Rincon, O.T.; Pazini, E.J. Interpretation of Chloride Profiles from Concrete Exposed to Tropical Marine Environments. Cem. Concr. Res. 2001, 31, 529–537. [Google Scholar] [CrossRef]
  46. De Weerdt, K.; Orsáková, D.; Müller, A.C.A.; Larsen, C.K.; Pedersen, B.; Geiker, M.R. Towards the Understanding of Chloride Profiles in Marine Exposed Concrete, Impact of Leaching and Moisture Content. Constr. Build. Mater. 2016, 120, 418–431. [Google Scholar] [CrossRef]
  47. Chen, P.; Ma, B.; Tan, H.; Liu, X.; Zhang, T.; Qi, H.; Peng, Y.; Yang, Q.; Wang, J. Effects of Amorphous Aluminum Hydroxide on Chloride Immobilization in Cement-Based Materials. Constr. Build. Mater. 2020, 231, 117171. [Google Scholar]
Cmd 02 00005 g001 550
Figure 1. Schematic structure of layered double hydroxide (LDH) in original and exposed state and mechanism of ionic exchange.
Figure 1. Schematic structure of layered double hydroxide (LDH) in original and exposed state and mechanism of ionic exchange.
Cmd 02 00005 g001
Cmd 02 00005 g002 550
Figure 2. Test matrix for chloride-binding tests.
Figure 2. Test matrix for chloride-binding tests.
Cmd 02 00005 g002
Cmd 02 00005 g003 550
Figure 3. Experimental sequence for measuring Cl− in the binding tests.
Figure 3. Experimental sequence for measuring Cl− in the binding tests.
Cmd 02 00005 g003
Cmd 02 00005 g004 550
Figure 4. Studies conducted in mortars. (a) Scheme of mortar with sensors and (b) calibration curves for chloride sensors.
Figure 4. Studies conducted in mortars. (a) Scheme of mortar with sensors and (b) calibration curves for chloride sensors.
Cmd 02 00005 g004
Cmd 02 00005 g005a 550Cmd 02 00005 g005b 550
Figure 5. Characteristics of LDH particles. (a) Particle size distribution and (b) XRD pattern of ZnAl-NO2 prior to exposure.
Figure 5. Characteristics of LDH particles. (a) Particle size distribution and (b) XRD pattern of ZnAl-NO2 prior to exposure.
Cmd 02 00005 g005aCmd 02 00005 g005b
Cmd 02 00005 g006 550
Figure 6. Stability and ion exchange property on LDH. (a) OH− capture by LDH and in terms of pH drop and percent capture. (b) Corresponding NO2− release by LDH.
Figure 6. Stability and ion exchange property on LDH. (a) OH− capture by LDH and in terms of pH drop and percent capture. (b) Corresponding NO2− release by LDH.
Cmd 02 00005 g006
Cmd 02 00005 g007 550
Figure 7. XRD analysis of ZnAl-NO2 after 30 days of immersion in alkaline solutions—(a) Full XRD spectra (b) XRD spectra displaying d003 peaks.
Figure 7. XRD analysis of ZnAl-NO2 after 30 days of immersion in alkaline solutions—(a) Full XRD spectra (b) XRD spectra displaying d003 peaks.
Cmd 02 00005 g007
Cmd 02 00005 g008 550
Figure 8. Shift of d003 and d110 as a function of pH.
Figure 8. Shift of d003 and d110 as a function of pH.
Cmd 02 00005 g008
Cmd 02 00005 g009 550
Figure 9. Results of the chloride-entrapment tests with the effect of pH. Plots on the left depict the change of chloride concentration (divided by the initial NaCl concentration) after LDH was added to solution. The graphs on the right show the solution pH before and after the addition of LDH. (a,b) Chloride ion and pH measurement in solutions at an initial chloride concentration of 10 mM, respectively. (c,d) Chloride ion and pH measurement in solutions at an initial chloride concentration of 100 mM, respectively. (e,f) Chloride ion and pH measurement in solutions, at an initial chloride concentration of 500 mM, respectively.
Figure 9. Results of the chloride-entrapment tests with the effect of pH. Plots on the left depict the change of chloride concentration (divided by the initial NaCl concentration) after LDH was added to solution. The graphs on the right show the solution pH before and after the addition of LDH. (a,b) Chloride ion and pH measurement in solutions at an initial chloride concentration of 10 mM, respectively. (c,d) Chloride ion and pH measurement in solutions at an initial chloride concentration of 100 mM, respectively. (e,f) Chloride ion and pH measurement in solutions, at an initial chloride concentration of 500 mM, respectively.
Cmd 02 00005 g009
Cmd 02 00005 g010 550
Figure 10. Comparison of the moles of Cl− and OH− captured, compared to the existing moles before the addition of LDH.
Figure 10. Comparison of the moles of Cl− and OH− captured, compared to the existing moles before the addition of LDH.
Cmd 02 00005 g010
Cmd 02 00005 g011 550
Figure 11. Long-term evaluation of chloride entrapment. (a) Cl− concentration and (b) pH of a 12 mM NaCl solution with initial pH = 12.08 measured before (t = 0 s) and after (300 s and 15 days) the addition of LDH. (c,d) Similar measurements of a solution initially with 100 mM NaCl and pH 12.95.
Figure 11. Long-term evaluation of chloride entrapment. (a) Cl− concentration and (b) pH of a 12 mM NaCl solution with initial pH = 12.08 measured before (t = 0 s) and after (300 s and 15 days) the addition of LDH. (c,d) Similar measurements of a solution initially with 100 mM NaCl and pH 12.95.
Cmd 02 00005 g011
Cmd 02 00005 g012 550
Figure 12. XRD plot detail of the 003 reflection of the LDH before tests (base) and the powder after 15 days of immersion in a solution with pH = 11.91, with and without 250 mM NaCl.
Figure 12. XRD plot detail of the 003 reflection of the LDH before tests (base) and the powder after 15 days of immersion in a solution with pH = 11.91, with and without 250 mM NaCl.
Cmd 02 00005 g012
Cmd 02 00005 g013 550
Figure 13. Chloride binding capacity of ZnAl-NO2 in the alkaline pH range.
Figure 13. Chloride binding capacity of ZnAl-NO2 in the alkaline pH range.
Cmd 02 00005 g013
Cmd 02 00005 g014 550
Figure 14. Compatibility of ZnAl-NO2 with cement. Reference and cement + NaNO3 samples harden in one day. Cement + ZnAlNO2 or Zn(NO3)2 took about 20 days to harden. (w/c = 0.5).
Figure 14. Compatibility of ZnAl-NO2 with cement. Reference and cement + NaNO3 samples harden in one day. Cement + ZnAlNO2 or Zn(NO3)2 took about 20 days to harden. (w/c = 0.5).
Cmd 02 00005 g014
Cmd 02 00005 g015 550
Figure 15. Studies conducted in mortars. (a) Chloride profile inside reference mortar and (b) chloride profile inside mortar with ZnAl-NO2.
Figure 15. Studies conducted in mortars. (a) Chloride profile inside reference mortar and (b) chloride profile inside mortar with ZnAl-NO2.
Cmd 02 00005 g015
Cmd 02 00005 g016 550
Figure 16. Corrosion potential and polarization resistance of steel rebar in mortars without and with 2 wt% (to cement fraction) ZnAl-NO2 immersed in 3.5% NaCl.
Figure 16. Corrosion potential and polarization resistance of steel rebar in mortars without and with 2 wt% (to cement fraction) ZnAl-NO2 immersed in 3.5% NaCl.
Cmd 02 00005 g016
Publisher’s Note: MDPI stays neutral with regard to jurisdictional claims in published maps and institutional affiliations.

Share and Cite

MDPI and ACS Style

Mir, Z.M.; Gomes, C.; Bastos, A.C.; Sampaio, R.; Maia, F.; Rocha, C.; Tedim, J.; Höche, D.; Ferreira, M.G.S.; Zheludkevich, M.L. The Stability and Chloride Entrapping Capacity of ZnAl-NO2 LDH in High-Alkaline/Cementitious Environment. Corros. Mater. Degrad. 2021, 2, 78-99. https://doi.org/10.3390/cmd2010005

AMA Style

Mir ZM, Gomes C, Bastos AC, Sampaio R, Maia F, Rocha C, Tedim J, Höche D, Ferreira MGS, Zheludkevich ML. The Stability and Chloride Entrapping Capacity of ZnAl-NO2 LDH in High-Alkaline/Cementitious Environment. Corrosion and Materials Degradation. 2021; 2(1):78-99. https://doi.org/10.3390/cmd2010005

Chicago/Turabian Style

Mir, Zahid M., Celestino Gomes, Alexandre C. Bastos, Rui Sampaio, Frederico Maia, Cláudia Rocha, João Tedim, Daniel Höche, Mario G. S. Ferreira, and Mikhail L. Zheludkevich. 2021. "The Stability and Chloride Entrapping Capacity of ZnAl-NO2 LDH in High-Alkaline/Cementitious Environment" Corrosion and Materials Degradation 2, no. 1: 78-99. https://doi.org/10.3390/cmd2010005

Article Metrics

Back to TopTop