Journal of Earth Sciences & Environmental Studies

ISSN: 2472-6397

Impact Factor: 1.135

VOLUME: 1 ISSUE: 3

Page No: 109-119

Removing of Hardness Salts from Groundwater by Thermogenic Synthesis Zeolite


Affiliation

Abd El Hay Ali Farrag1, Th. Abdel Moghny2,Atef Mohamed Gad1,3, Saleem Sayed Saleem3, Mahmoud Fathy2,MuhamedAtef Ahmed3

1Assiut university faculty of science geology department, Box. No. 71516, Assiut, Egypt

2Applications Department, Egyptian Petroleum Research Institute (EPRI), 1 Ahmed El-Zomer, Nasr City, Box. No. 11727, Cairo, Egypt

3Assiut and new valley company for water and waste water fax No: 088229347

Citation

Atef Mohamed Gad, Removing of Hardness Salts from Groundwater by Thermogenic Synthesis Zeolite(2016)SDRP Journal of Earth Sciences & Environmental Studies 1(3)

Abstract

Abstract Calcium and magnesium hardness salts in groundwater are very common and caused major problems for drinking and household purposes. This study aims to synthesize zeolite-4A from kaolinite for removing the total hardness ions from Assiut Governorate groundwater wells. Therefore, the kaolin was calcinated hydrothermally through the metakaolinization and zeolitization processes to produce crystalline zeolite-4A. The chemical composition andmorphology ofcrystalline zeolite-4A were characterized using X-ray diffraction (XRD) and scanning electron microscopy (SEM). Then the column experiments were conducted to study the performance of crystalline salt-4A as ion exchange and investigate their operation parameters and regeneration conditions. Thomas and Yoon-Nelson models were applied to predict the adsorption capacity and time required for 50% breakthrough curves. The effects of initial concentrations of 550 mg/l for total Ca+2 and Mg+2 hardness, feed flow rate of 10-30 ml/min, and height range of 1.0– 4.0 cm on the breakthrough behavior of the adsorption system were studied. The obtained results indicated that the synthesized zeolite-A4 can remove total hardness (Ca+2 + Mg+2) ions from groundwater to the permissible limit according to the standards drinking water law.

Introduction

Groundwater as an essential source of fresh water used for drinking, household, agriculture, industry after rivers and rain in most parts of the world.But many components involved in groundwater affectinghistaste and quality.Total hardness and calcium hardness salts are common components affecting negatively on the taste and quality of the drinking water, especially in the locations nearrivers or channels, whichdoesn’t recharge from the aquifer of limestone or clays (Ben Abda, Schäf et al. 2015). For this reason, soils are one of the most important natural filter for the water by far in agricultural and forest soils(Brevik et al., 2015; Keesstra et al., 2012; Keesstra, 2007). For instance, soil erosion (Rodrigo Comino et al., 2016a, 2016b) or soil pollutants (Novara et al., 2016, 2013) must be controlled.

Water hardness are due to calcium and magnesium cations, and can be reduced by several methods such as electrode ionization process, electro membrane processes, capacitive deionization, fluidized pellet reactor, and reverse osmosis membrane(Chen, Zhang et al. 2012). Reverse osmosis treatment is a usefulmethod to avoidthese hardness salts, but it’s not satisfactory due to several reasons: i) it’s slow and produce more waste water; ii)  a few amount of potable water is produced in a long time; iii) consumes great electricity energy support; and, iv) requires highly convenient technicians for the operation process and loses large amount of raw water as a waste within the production process. In addition,  less one gallon of potable water is produced within more than six hours, as well as, seven to eight gallons of waste water are generated in that time(Mahmoud Fathy 2016).

Finally, it’s required a high pressure associated with high electrical energy costs to operate the unit.  For those reasons, the authors (citation) suggest to use ions exchange process based on synthetic zeolite as filtration media for adsorption of hardness salts, because it is low cost sorbents and that process can be consider one of the promising techniques. The mechanism of synthetic zeolites as ion exchange depends on use their granular negative charge to exchange ions present in their structure with ions present in the water, thereby, it can produced a very large amount of treated water through a short time, and it’s very easy regeneration by passing10% NaCl solution  through it(Calvo, Canoira et al. 2009, Cai, Turner et al. 2015).

This study aimed to applyzeolite synthesized from Egyptian kaolin as ion exchanger to remove excess total and calcium hardness ions in groundwater wells of Assiut Governorate, according to WHO (2004) and the standards Egyptian drinking water Law No. (458/2007). In this respect, columns experiments of synthesized zeolite-4A were conducted to study their performance as ion exchange and investigate their operation parameters and regeneration conditions.

 

 

Novara, A., Gristina, L., Guaitoli, F., Santoro, A., Cerdà, A., 2013. Managing soil nitrate with cover crops and buffer strips in Sicilian vineyards. Solid Earth 4, 255–262. doi:10.5194/se-4-255-2013

 

Novara, A., Keesstra, S., Cerdà, A., Pereira, P., Gristina, L., 2016. Understanding the role of soil erosion on co2-c loss using 13c isotopic signatures in abandoned Mediterranean agricultural land. Sci. Total Environ. 550, 330–336. doi:10.1016/j.scitotenv.2016.01.095

Materials & Methods

2.1. Materials

Groundwater samples were taken from about 850 plots producing drinking water, covering all Assiut Governorate duirng2010-2015 and to identify the most contaminated wells with about 40 % of total hardness and Calcium hardness ions. Thefiltration media mainly consistedof zeolite-4A with grain size <0.8 mm that synthesized from natural kaolin that available in south-east Abu zenima in Sinai region-Egypt.

Finally, sandstone has diameter ranged from (0.5 mm to 1.2 mm) was used as filter in the packed column.

Methods and procedures

2.2.1 Preparation of Zeolite 4A

Zeolite-4A was synthesized based on Abu zenima kaolin through a) metakaolinization(calcinations or thermal treatment), and (b) zeolitizationstep (alkaline treatment).

  1. a) Calcination or thermal treatment

Natural occurring kaolin was crushed and sieved to the grain size < 80 micron, then expose to high temperature(greater than 800 °C at approximately 4 hour) to convert kaolin to metakaolin (calcinatedkaolin)(Bhatia, Abdullah et al. 2009). The heating process drives off water from the main constituent of kaolin clay mineral (Al2Si2O5(OH)4), and collapses the material structure by producing an amorphous aluminosilicate (Al2Si2O7), metakaolin. The process is known as dehydroxylation,hence, both the surface and chemical combined water are removed, rendering kaolin non-plastic and presented by the following equation,

Al2Si2O5(OH)4+2H2O   --------------->Al2Si2O7   +   2H2O.

(Natural kaolin)                                                (Meta kaolin)

  1. b) Zeolitization (alkaline treatment)

This process was achieved by mixed of metakaolin powder with 3M sodium hydroxide solution at ratio of 1: 5 (solid: liquid) with 4 hours stirring at temperature of 100 Co. After that the mixture was filtered, washed with distilled water to remove the excess alkali, decanted and filtered several times till pH 10, then dried at 90°C overnight and crushed to particle size <80 micron. Finally the product was characterized by XRD and ESM examinations (Devrim and Albostan , Guo, Zeng et al. 2013).

 

  1. c) Column Study

Three PVC filter columns having 5 cm inner diameter and 12 cm height were setups and packed with mixing ratio of 1: 1 of< 0.8mm synthetic zeolite and 0.5-1.2 mm sand. Three filtration media of 30, 60, and 120-gm weight (that represented bed heights of 1.0 cm, 2.0 cm, and 4.0 cm, respectively), were packed in P.V.C columns  at three adjusted filtration rate of 10, 20, and 30 ml / min, respectively. The concentration of total and calcium hardness, of water samples, was analyzed before and after the treatment by selected sequentially every 100 mL of filtered water for analysis according to standard test methods. After filtration, the ion concentrations in the aqueous phase were measured using spectrophotometer model HACH DR6000(Grande and Rodrigues 2004).

 

Results

3.1. XRD analysis

The XRD pattern of hexagonal kaolin mineral sheets before calcination or any treatment shows that the hydroxysodalite having several common peaks located at 13.96, 19.98o, 24.42o, and 35.00oas shown in Figure 1(El Tahlawi, Farrag et al. 2008, Mustafa and Zaiter 2011).  The XRD spectra analysis of hexagonal kaolin was very difficult because kaolin contained several mineral phases and many impurities. This led to appear of overlapping peaks due to complex structure of hexagonal kaolin. Therefore, additional treatments will be used to remove some ambiguity(Abd El Hay Ali Farrag 2016). At low diffraction angles, there was a fairly large continuous background because of Lorentz polarization and the presence of amorphous phases. Two broad peaks (the first one between 19° and 33° and the second one between 34° and 43°) were also observed. Furthermore, the low intensity and the more or less pronounced symmetry of the peaks at the smallest angles were likely as a result of the greater disorder of the structure of this kaolin(Mustafa and Zaiter 2011).

Figure 2presents the XRD pattern of complete poorly crystalline metakaolin formed by calcination of   kaolin (at 800 for 4 hours), Indicating on the formation of a new phase of dehydroxylated, hence the internal structure was destroyed with containing negative charges and shows only one characteristic diffraction peaks located at peaks located at 19.75°, that is attributed to kaolinite remains in the calcined kaolin.The contents of orthoclase and muscovite are also reduced according to diffraction peak strength, but the content of quartz is still high, so quartz seems inert during calcination. Nepheline (NaAlSiO4) and little amount of anhydrous sodium aluminosilicateNa2(Al2Si3O10) are found in the treated kaolin, in addition to disappearing of peaksrelated to all raw minerals .

Finally, the XRD pattern in Figure 3 illustrated the agglomerated cubic crystals of final synthesized zeolite 4A after treated with  NaOH solution at 100 Co for 4 hours, and exhibit characteristic peaks at 2q values of 7.2o, 10.3o, 12.6o, 16.2o,21.8o,24o, 26.2o, 27.2o,30o, 30.9o, 31.1o, 32.6o, 33.4o and 34.3o its typically matches XRD pattern of zeolite4A that synthesized  at 3 M NaOH concentrations by (Abd El Hay Ali Farrag 2016) and found that the synthetic zeolites4A have more crystalline SiO2 in the form of quartz tetrahedral crystal lattices structures.

3.2. Escaning Electron Microscope SEM analysis

It is known that the framework structure of zeolite is described as a combination of two interconnected channel systems. SEM micrographs of kaolinite prior to treatment, after calcination and the final synthesized zeolite-4A, are shown in Figures (4a, 4b, 4c).

Figure4a represents SEM images of kaolin powders at different particle sizes. As can be observed, the kaolin particles at both particle sizes show crystallinity flake-like structure. This is because that powder has a random structure that induces different shapes and sizes and could change due to the process preparation. Nevertheless, the particle agglomeration is observed especially for type A kaolin (Fig. 4(a) Hosseini et al., 2014Figure 4bshowsthe SEM of kaolin after calcination (metakaolinite) at 800 Coduring4 hours. Itwasclear that the calcination process increasing all of the whiteness, hardness, improves the electrical properties, and alters the size and shape of the kaolin particles. Calcination process that occurs at 800°C for the dehydroxylation kaolin indicating on the formation of complete poorly crystalline metakaolin as a new phase of dehydroxylated, hence the internal structure was destroyed with containingnegative charges as illustrated in XRD of kaolin after calcination (Figure 2)(Inglezakis and Grigoropoulou 2004).Such process can be describe by the following chemical equations,

Al2O3.2SiO2.2H2O    ------------→ Al2O3.2SiO2 + 2H2O (g).

 

During this reaction, as SEM showed, the higher-order reflections lost their intensity and vanished in the SEM background. This result led to the opinion, that the metakaolinite can be amorphous, now a conception of the short-range order crystalline structure of metakaolinite predominates.

As shown from the images in Figure 4c, a marked change took place in the morphology of the starting materials. The cubic crystalline morphology in Figure 4c, typically of the zeolitic products obtained consisting of sinusoidal channels (along ) with a circular cross section interconnected with straight channels (along) of elliptic cross section (5. 3 Å × 5.6 Å). The scanning electron micrographs (SEM) of the synthesized zeolite reveals on the presence of slightly different crystals sizes with the same cubic morphology at an average diameter of approximately 4 μm.In addition, this technique reveals on the absence of any amount of amorphous material in the synthesized zeolite, which indicates the presence of zeolite A4 in a high degree of crystallinity. It is known that the framework structure of zeolite is described as a combination of two interconnected channel systems. Also, this methodology advantage by the low cost-effective alternative to produce zeolite A4(Kazemimoghadam and Mohammadi 2007)

3.3. Contact time research

The influence of contact time on adsorption of calcium and  total hardness at flow rate of 20ml/min from raw water containing 550mg·L−1 calcium hardness and  420mg·L−1 total hardness have been studied, the results are shown in Figure5.   It’s found that the initial adsorption was slightly rapid within the first 100 min due to the adsorption of Ca+2 and total hardness onto the exterior surface.  Then the ions enter into interior zeolite-4A (Kazemimoghadam and Mohammadi 2007). After that, the adsorption rate decreased substantially with time till equilibrium position. The adsorption process was attained to equilibrium at 160 and 200 min, as well as, the removal efficiency reached to 35% and 100% for calcium and total hardness, respectively.

3.3.1. Effect of flow rate

Flow rate variations another factors influenceson the breakthrough. Therefore, the adsorption of 550 mg/l total hardness salts concentrate ionsonzeolite media was investigated at varying flow rate of 10, 20 and 30 ml/min and at bed height of 4 cm (120g) as shown in Figure 6. From figure it was observed a significant shrinkage in breakthrough curves as the flow rate increased from 10 to 30 mL/min, this because, an increase in  flow rate led to reduce the external film mass resistance over the zeolite4A surface leading to decrease the residence time. Thereby, the decreasing of saturation time leads to dominate the removal efficiency. Conversely, at lower flow rate, the period of mass transfer inside the zeolite-4A pores, would increase and allow more binding accession sites in all cases (calcium and total hardness).

3.3.2. Effect of bed height

The adsorption of total hardness (Ca+2, Mg+2) ions in the packed column is largely dependent on the bed height, which is directly proportional to the quantity of synthetic zeolite A4.  For this respect, three bed height of 1, 2 and 4 cm were selected for packed column filtration that corresponding of  30 g, 60 g and 120 g synthetic zeolite A4, respectively. The adsorption breakthrough curves obtained by varying the bed heights at a flow rate of 10 mL/min and at550 mg/L inlet total hardness (Ca+2, Mg+2) concentrations is presented in Figure 7.It’s found that the faster breakthrough curves were observed at bed height of 1 cm, while the slowest breakthrough curve was observed at a bed height of 2 and 4 mm. That is means the bed capacity was increased when the bed height increased from 1 to 4 cm, i.e., higher beds contain more adsorbent; therefore, more binding sites will be available for the total hardness ions (Ca+2, Mg+2) to attach(Mahmoud Fathy 2016), which will eventually lead to the attainment of a higher bed capacity. Additionally, an increased bed height resulted in more contact time being available for the total hardness ions (Ca+2, Mg+2)to interact with the adsorbent(Mahmoud Fathy 1 and 1 2015). This phenomenon has allowed the total hardness ions (Ca+2, Mg+2) to diffuse deeper into the adsorbent. Subsequently, the percentage of total hardness ions removal increased when the bed height was increased (Gupta et al., 2004).

3.3.3. Regeneration cycles of zeolite media filtration

Figure8 illustrates the adsorption/desorption of total hardness for three regeneration cycles. Several regenerated times (more than 3 cycles) were conducted for solution employed 10% NaCl and 550 mg/l total hardness (Ca+2, Mg+2) concentrations to determine the adsorption/desorption capacity of the mineral. In the first run before using NaCl as regeneration, the adsorption capability of zeolite is approximately not exceed than 70% and reach to 100% after using NaCl.  The adsorption/desorption capability of zeolite reach to about 100% within the first three regeneration, and the removal efficiency of total hardness reduced to approximately 50%.  Finally, the regeneration efficiency reduced as the number of regeneration cycles increased. The decrease in adsorption/desorption with increasing cycles was steeper. One can conclude that at first cycle the adsorbent solutions exhibited the highest desorption performance. It wasobserved that the adsorption capacity of mineral increased during the first two cycles when using NaCl as desorbing agent because it's enhanced the metal uptake capability of zeolite by replacing mobile ions originally present in the mineral. This finding agrees with previous research work (Abd El Hay Ali Farrag 2016).

Z-(Ca+2, Mg+2) + Na+Cl-<----------------------->   Z-Na+ + (Ca+2, Mg+2) Cl

3.3.4. Breakthrough curves modeling

In  order  to describe  the fixed  bed  column  behavior  and  scale up  for  the industrial  applications,  two  models, Thomas,  and Yoon-Nelson were conductedto fit the experimental  column  data (Abanades, Arias et al. 2015). Thomas model is widely used in performance modeling of columns. The arithmetic expression for the model of adsorption column is given in Equation 1 (Gupta, Gaur et al. 2004):

Ct/C0 = 1/1+exp[(KThqwx/Q)-KThC0t]                        Equation Eq.1

were kTh (mL/min.mg) is the Thomas model constant, qe (mg/g) is the predicted adsorption capacity, x is mass of adsorbent (g), Q is influent flow rate (mL/min), C0 is initial solution concentration (mg/l), and Ct is effluent solution concentration (mg/L). The second linear equation of Thomas model is expressed below

  Ct/C0 – 1= (KThqwx/Q)-KThC0t                                              Equation Eq.2(Marcussen 1982)

From the regression coefficient (?2) and other parameters, it can be concluded that the experimental data fitted well with Thomas model. The models parameters are listed in Tables 1 and2show that as the flow rate increased, the value of ?th decreased whereas the value of ?0 showed a reverse trend, that is, increased with increasing of the flow rate. Similarly, ?0 values decreased and ?th values increased with increasing the flow rate. Similar trend has also been observed for sorption of total hardness (Ca+2 + Mg+2)by zeolite-A4. The well-fitting of the experimental data with the Thomas model indicate that the external and internal diffusion will not be the limiting step (Bertoni, Medeot et al. 2015).     

Yoon-Nelson model does not requiredata about the characteristics of the system including the type of adsorbent as well as the physical properties of the adsorption bed. The Yoon-Nelson equation is expressed as

ct/c0-ct=exp(KYNt- tKYN)              Equation Eq.3(M. El-Sayed 2016)

where (KYN) is the rate constant (min-1) and (τ) is the time required for 50 % breakthrough (min). The values of the rate constant KYN increased with the flow rate and the initial concentration(Padilha, Padilha et al. 2015).

The Yoon-Nelson is a linear model for a single component system as expressed by(Abd El Hay Ali Farrag 2016),

Eq.4  ct/c0-ct=KYNt- tKYN                                          Equation Eq.4

A model based on the assumption that the rate of decrease in the probability of adsorption of adsorbate molecule and the adsorbate breakthrough on the adsorbent is proportional to the probability of the adsorbate adsorption (Fathy, Moghny et al. 2014).

The values of ?YN and ? along with other statistical parameter are listed in Tables 1 and2. It is seen from the s that the values of τ obtained by themodel are notclose to the experimental results. Thus, this model is not suitable for our case. This due to that the values of ?YN decrease with decreasing the flow rate, whereas, the corresponding values of ? increased with increasing flow rate. A similar trend was followed for sorption of total hardness (Ca+2 + Mg+2) for zeolite- A4 column sorption(Razavi, McCoy et al. 1978).

 

Conclusion

The ground water sample that collected from Assiut Governoratewellswere analyzed to determine the various physicochemical parameters such as TDS (Total Dissolved Salts), EC  (Electrical Conductivity), Total Hardness (Ca2+, Mg2+) and total Alkalinity, the results revels that physicochemical parameters are more than thedesirable limit of WHO drinking water quality guideline. In this research,severalsynthetic zeolite A4 dose are selected and their efficiency as hardness removal from ground water were checked. The zeolite A4 synthesized was characterized using SEM, XRD. The packed bed investigation on the zeolite A4 revealed the importance of bed height, flow rate and inlet solute concentration on zeolite A4. The column performance was better at higher inlet concentration, while the lowest flow rate and bed depth favored the column chemisorption.It’s found that the efficiency of synthetic zeolite A4 on removal of totalhardness removal ranged from 35% to 100% for Ca2+andMg2+, respectively.The column data were well described using Thomas and Yoon–Nelson models. The Yoon–Nelson model was successfully used to predict the breakthrough curves at different flow rates and inlet MG concentrations.

Acknowledgement

First of all mysupervisors Prof. Dr. Abdel Hay Ali Farrag(Geology Department,Assiut University) and Prof. Dr. Thanaa Abdel Moghny.Weappreciate the supporting offered by the research assistant Mahmoud Fathy Mubarak (ApplicationsDepartment, Egyptian Petroleum Research Institute).

Special thanks tothe Head of Assiut and new valley company for water and waste water Eng. Mohamed Salah El Deen Abdel Ghaffar for his supporting to our Team Research.

Finally, thanks to Ch.Esslam M. Hassanin,Ch. Zainab Fathy Mahmoud, Ch. Aliaa Mokhtar, Ch. Mariana Essmatand other my colleagues of theentire Laboratories Sector staff ofAssiut and new valley company for water and waste water for using the facilities of the Laboratories Tools.

Images and Tables

q (mg g−1)

R 2

k Th

Flow (mL min−1)

1550.395

-0.90151

0.002764309

10

2620.772

-0.89109

-0.001416225

20

-2425.1

0.941445

0.001533116

30

τ

R 2

KYN

Flow (mL min−1)

-585.62

0.8466

-7E-05

10

-152.57

0.9513

-0.0012

20

-57.829

0.9355

-0.0022

30

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