International Journal of Nonferrous Metallurgy
Vol.08 No.02(2019), Article ID:91585,16 pages

Effect of Calcination Condition on Thermal Activation of Ibere Clay and Dissolution of Alumina

Udochukwu Mark*, Charles Nwachukwu Anyakwo, Okechukwu Onyebuchi Onyemaobi, Chijioke Samson Nwobodo

Department of Materials and Metallurgical Engineering, Federal University of Technology, Owerri, Nigeria

Copyright © 2019 by author(s) and Scientific Research Publishing Inc.

This work is licensed under the Creative Commons Attribution International License (CC BY 4.0).

Received: January 30, 2019; Accepted: March 31, 2019; Published: April 3, 2019


Bauxite deposits for production of alumina are lacking in Nigeria and there is an aluminium smelter plant in the country which requires alumina for its operation. Development of alternative alumina resource using clays that are abundant in the country is the focus of this paper. The thermal activation of Ibere clay from southeastern Nigeria for optimal leaching of alumina was investigated. The clay assayed 28.52% Al2O3 and 51.6% SiO2, comprising mainly kaolinite mineral and quartz or free silica. The alumina locked up in the clay structure was rendered acid-soluble by thermal activation which transformed the clay from its crystalline nature to an amorphous, anhydrous phase or metakaolinite. The clay samples were heated at calcination temperatures of 500˚C, 600˚C, 700˚C, 800˚C, and 900˚C at holding times of 30, 60, and 90 minutes. Uncalcined clay samples and samples calcined at 1000˚C (holding for 60 minutes) were used in the control experiments. The result of leaching the clay calcines in 1 M hydrochloric acid solution at room temperature, showed that the clay calcines produced at 600˚C (holding for 60 minutes) responded most to leaching. Samples calcined for 60 minutes also responded better than those held for 30 or 90 minutes. Based on activation energy studies, it was observed that calcines produced at 600˚C (for 60 minutes) had both the highest leaching response (50.27% after 1 hour at leaching temperature of 100˚C) and the lowest activation energy of 24.26 kJ/mol. It is concluded therefore that Ibere kaolinite clay should be best calcined for alumina dissolution by heating up to 600˚C and holding for 60 minutes at that temperature. The clay deposit has potential for use as alternative resource for alumina production in Nigeria where bauxite is scarce.


Ibere Clay, Bauxite, Kaolinite, Alumina, Calcination, Thermal Activation, Leaching

1. Introduction

Aluminium is the second most-produced and consumed metal after iron and steel. It is produced by the electrolytic reduction of alumina (Al2O3) in the Hall-Héroult process [1] [2] [3] [4] . Alumina is refined from bauxite, which has remained the most important ore for aluminium [5] [6] . About 90 percent of the world production of bauxite is used for making alumina, most of which is consumed in the manufacture of aluminium. The remainder is used in the production of abrasives, refractories, chemicals used chiefly in water purification and in the manufacture of paper, petroleum catalysts, aluminous cements, materials for the purification of kerosene and other petroleum products, and for other purposes [7] [8] [9] [10] . West Africa is one of the world’s major bauxite provinces and has the largest bauxite resources [11] [12] [13] . The US Geological Survey reported about 55 billion tonnes as the world’s bauxite reserve with West Africa having the highest share of 32% [10] . Again, countries in the sub-region (Nigeria’s neighbours) hold about one-third of the world’s bauxite reserves, and the resource is sold at locally unfavourable internationally competitive prices [10] . Bauxite deposits are found in Guinea, Sierra Leone, Ghana, Mali, Cameroon, and Gabon [11] [13] [14] . In Nigeria, however, no such deposits have been discovered [13] [14] . Only minor occurrences with low concentrations of bauxite minerals are reported from some regions like Ekiti province [15] [16] and the Jos Plateau [17] [18] . Again, only the occurrence of bauxitic clay is reported from the Mambilla Plateau (the western extension of the Adamawa Highland, near the border with Cameroon) [11] [12] [13] [14] . This shows that the raw material for manufacture of alumina (i.e. bauxite) is very scarce in Nigeria.

The high-volume consumption of aluminium in Nigeria and the establishment of an aluminium smelter plant at Ikot-Abasi [19] [20] calls for the development of methods for producing alumina from nonbauxite alumina/aluminium bearing raw materials. The kaolinitic clays are aluminous raw materials and are well distributed on a large scale in Nigeria [21] [22] [23] .

Kaolinite clay has the structural formula in which the silica tetrahedral layer, represented by ( Si 2 O 5 ) 2 is made electrically neutral by an adjacent aluminium octahedral layer, Al 2 ( OH ) 4 2 + [24] [25] . Taking one silicon tetrahedral unit and one aluminium octahedral unit, the structural formula of kaolinite can be written as Al 2 ( OH ) 4 ( Si 2 O 5 ) or Al 2 Si 2 O 5 ( OH ) 4 or in terms of oxides as Al 2 O 3 2 SiO 2 2 H 2 O . In its pure form, kaolinite has the theoretical composition of 46.54% SiO2, 39.50% Al2O3, and 13.96% H2O (equivalent to loss on ignition or LOI). This makes kaolinite the clay mineral with the highest content of alumina [26] [27] . Kaolinite clays are therefore potential sources of alumina where bauxite is scarce or depleted. In view of Nigeria’s situation, the abundant reserve of kaolinitic clays is thought as a suitable substitute for bauxite from which alumina of high purity can be obtained [23] [28] [29] .

However, the alumina content of kaolinite (and other clay minerals) is locked up in the clay structure. Proper thermal treatment or activation is usually necessary to render the alumina soluble under atmospheric leaching conditions [30] . It was reported that an attempt to recover alumina from clay using pressure hydrometallurgy was being developed in Canada. It is hoped that alumina content of aluminosilicates minerals such as clays could be recovered without the thermal activation step [31] . If achieved, this will certainly save energy and ultimately improve the process economics making it compete with the Bayer’s process [30] . However, the plant (operated by Orbite Aluminae) was shut down in 2017 due to bankruptcy [29] .

As illustrated in Figure 1, four temperature ranges are important in the thermal transformation of clays [32] , namely: the drying range or free-water dehydration range (50˚C - 120˚C); the clay stability range (120˚C - 600˚C); the anhydrous clay range (600˚C - 900˚C); and the recrystallization range (above 900˚C).

For example, kaolinite is reported to change from hydroplastic condition to leather hard, then stone hard and finally to anhydrous condition or metakaolinite as it is heated between room temperature and about 600˚C because of drying, dehydration and dehydroxylation [32] [33] [34] :

1) Drying or loss of wetness or physically adsorbed water by evaporation occurs at temperatures below 120˚C. The loss of physically attached water is endothermic and results in measurable weight loss. The weight loss is usually minor, and the changes due to loss of physical water do not alter the crystalline structure of the clay [32] . Within the drying range, liquid water is removed from the clay, and the resulting material is referred to as leather dry or leather hard clay [34] .

2) Dehydration or further loss of any remaining physically held water occurs between 120˚C and about 550˚C. The resulting material after this transformation is referred to as bone-dry or stone hard clay. Throughout the drying and dehydration temperature range (where physical water is removed), the expulsion of water is reversible as shown in Figure 1 [32] [34] .

3) De-hydroxylation is the loss of constitutional or chemically combined water (the OH water). Around 550˚C, the chemically combined water in clays begins to be released. This transformation continues until all chemically combined water is expelled resulting in the formation of metakaolinite, an anhydrous form of kaolinite [32] [33] . As with the loss of physically adsorbed water, the loss of the chemically combined water is an endothermic process that is accompanied by weight loss. The magnitude of the weight loss depends on the amount of chemically combined water in the clay. After de-hydroxylation, metakaolinite appears amorphous on X-ray diffraction, but the short-range ordering of the cations within the sheets that make up the kaolinite structure is retained. Metakaolinite is a homogeneous molecular-level mixture of non-crystalline alumina and silica

Figure 1. Effect of temperature on the physical state of clay minerals ( [32] , p. 174).

and does not spontaneously rehydrate when it is exposed to water and it remains stable up to approximately 980˚C [35] [36] [37] .

The thermal changes of kaolinite heated above 600˚C can be outlined in accordance with the following sequential reactions [30] [38] :

Al 2 O 3 2 SiO 2 2 H 2 O Kaolinite Dehydration above 600 ˚ C Al 2 O 3 2 SiO 2 Metakaolinite + 2 H 2 O Constitutional WaterRemoved (1)

4( Al 2 O 3 2 SiO 2 ) Metakaolinite 950˚C-980˚C 3 Al 2 O 3 2 SiO 2 Primary Mullite + γ -Al 2 O 3 Gamma-Alumina ( fcc ) + 6 SiO 2 Amorphous Silica (2)

γ -Al 2 O 3 Gamma-Alumina ( fcc ) + 3SiO 2 Amorphous Silica 1000 ˚ C - 1400 ˚ C 3 Al 2 O 3 2 SiO 2 SecondaryMullite + SiO 2 Tridymite (3)

3 Al 2 O 3 2 SiO 2 SecondaryMullite + SiO 2 Tridymite 1400 ˚ C - 1580 ˚ C 3 Al 2 O 3 2 SiO 2 Mullite + SiO 2 Cristobalite (4)

Thus, the thermal changes of kaolinite heated above 600˚C progress in four major steps, namely: endothermic dehydration by de-hydroxylation of kaolinite (Al2O3∙2SiO2∙2H2O) to metakaolinite (Al2O3∙2SiO2); sudden exothermic crystallization at about 980˚C resulting to the formation of primary mullite (3Al2O3∙2SiO2), γ-alumina and amorphous silica; further recrystallization to secondary mullite and tridymite; and then transformation of tridymite to cristobalite. Whereas reaction (1) or the first transformation is associated with loss in weight (due to LOI); all four transformations are accompanied by considerable volume and enthalpy changes [30] [32] [38] .

The temperatures at which these transformations (phase changes) begin and end depends on: 1) degree of crystallinity of the kaolinite, 2) its impurity oxides contents, 3) particle sizes, rate of heating, and duration of heating at a given temperature. Therefore, clays from different localities vary considerably not just in mineralogy and chemical composition, but in degree of crystallinity and purity [27] [32] [37] . The current investigation is focused therefore on determining the thermal treatment required to transform Ibere clay found in southeastern Nigeria to an anhydrous amorphous phase or metakaolinite. The response of the clay calcines to alumina leaching in hydrochloric acid solution vis-à-vis the thermal treatments was also investigated.

2. Materials and Methods

Raw clay sample obtained from Ibere clay deposit (Lat. 5˚25'36''N, Long. 7˚33'48''E) in Ikwuano Council of Abia state, Nigeria was sun-dried, crushed and ground. The ground clay sample was placed on a 300 μm ASTM sieve and shaken for 5 minutes. The oversize was further ground and sieved on the same sieve. The procedure was repeated until the entire clay sample passed through the 300 μm sieve (50 standard Tyler mesh).

2.1. Mineralogical and Chemical Analysis

Representative sample of the sieved clay was analysed using Pananalytical XRD (Empyrean model) to determine the constituent minerals. Optimally calcined sample of the clay was also analysed with XRD to determine the effect of thermal transformation on the clay. Similarly, the chemical composition (amounts of Al2O3, SiO2, TiO2, etc.) was determined by means of Buckscientific AAS (model 210 VGP). The loss on ignition (LOI) was determined by placing one gramme of dry clay sample (dried at 105˚C for 12 hours in an oven) into a platinum crucible of known weight ( W d ). This was subsequently fired at 1000˚C for 1 hour in a muffle furnace. At lapse of time, the crucible was brought out of the furnace and reweighed ( W f ) after cooling down to room temperature. The LOI was calculated in percentage as ( W d W f / W d ) × 100 .

2.2. Calcination Procedures

Ground and sieved clay samples passing 300 μm sieve were subjected to thermal treatments in a muffle furnace at a heating rate of 15˚C per minute up to the holding temperature (500˚C, 600˚C, 700˚C, 800˚C or 900˚C) and held for 30, 60 or 90 minutes before furnace-cooling to room temperature. For the control experiment; a sample of the clay was reserved in the uncalcined condition (room temperature) and used as control 1, while another sample was heated up to 1000˚C and held for 60 minutes and used as control 2.

2.3. Leaching of Clay Calcines

Analytical grade HCl acid and pure deionized water were used to prepare the leaching reagent. 1 molar standard solution of hydrochloric acid was prepared using deionized water. This was used as the leaching reagent for the leaching studies to determine the leaching response of the various clay calcines and the controls. The leaching was done under moderate leaching conditions, i.e. hydrochloric acid concentration of 1 M, leaching temperature at ambient (~25˚C), shaking speed of 100 rpm, and solid/liquid ratio or clay weight to acid volume ratio of 0.02 g/ml, using clay particles passing 300 μm (−50 mesh).

The leach contact time or duration ranged from 0 to 120 minutes at intervals of 30 minutes. The flask or reaction bottle was shaken at a constant rate of 100 rpm during the contact time (duration of leaching) to facilitate the reaction. This was achieved by means of a KOMA orbital shaker (model KED11). By the end of leaching, the resulting slurry was filtered to separate undissolved materials (residue) from the filtrate (leachate or pregnant solution). The leachate was analysed for aluminium ion concentration.

This procedure was repeated for all the clay calcines and the control samples, which were prepared at different temperatures and duration of calcination. The optimum condition for calcining the clay was determined using solubility data (concentration and fraction of aluminium ion solubilized).

After examination of the extent of aluminium extraction or solubilization from the clay calcines, the calcine with the best leaching response for each calcination temperature was subjected to activation energy studies to establish the thermodynamic basis for their better leaching kinetics. This was in accordance with the Arrhenius rate law, viz:

k = A e ( E a R T ) or ln k = ( E a R ) 1 T + ln A (5)

where, k is the leaching rate constant, A is the Arrhenius frequency factor, Ea is the activation energy for the leaching reaction, R is the universal gas constant (= 8.314 J∙mol−1∙K−1), and T is the leaching temperature on the absolute scale [39] .

Thus, samples held for 60 minutes at different temperatures of calcination were leached in 1 M HCl at 25˚C, 50˚C, 75˚C and 100˚C for a reaction contact time of 60 minutes. All other variables such as clay particle size, shaking speed, and solid/liquid ratio were kept constant at less than 300 µm (−50 mesh), 100 rpm and 0.02 g/ml, respectively. The natural logarithm of rate constants (lnk) as deduced from the solubility data (based on second-order reaction kinetics which appeared to fit the data) and the reciprocal of absolute temperature (1/T) were used for Arrhenius plots to determine the activation energy (Ea) in the case of each clay calcine [39] [40] .

3. Results and Discussion

3.1. Type and Composition of Clay

Ibere clay is dominated by kaolinite mineral, with free silica or quartz and anatase as accessory minerals (Figure 2). The chemical composition is shown in Table 1. The alumina content of 28.52% is considered good enough for hydrometallurgical treatment of the clay as a source of alumina, and hence aluminium [6] [40] [41] .

The peaks for constituent mineral phases are clearly identified in the X-ray diffraction pattern of the uncalcined clay (Figure 2). However, the XRD pattern for the optimal clay calcine (Figure 3) shows that the sharp kaolinite peaks in Figure 2 are no longer distinct. The disappearance of the kaolinite peaks is indicative of the appearance of an amorphous phase (metakaolinite) due to thermal transformation or complete dehydroxylation of the clay [35] [36] . A study of the phase transformations of kaolinite from different deposits in Russia and Ukraine showed similar observations [37] . It is this amorphous metakaolinite (Al2O3∙2SiO2) that releases its alumina (Al2O3) for dissolution making the clay respond to acid leaching. Thus, proper thermal treatment and transformation of the clay activates it for acid leaching [30] [36] .

Figure 2. XRD pattern (diffractogram) of uncalcined Ibere clay.

Figure 3. XRD pattern of Ibere clay calcined at 600˚C for 1 hour.

Table 1. Chemical composition of Edda clay.

3.2. Dissolution of Alumina in Response to Acid Leaching

The presence of Al3+ ions in the leach solutions shows that a dissolution reaction occurred between the alumina in the clay calcine and the leaching reagent. It is proposed that hydrochloric acid ionized in water to produce protons or hydrogen ions (H+) in the hydrated form known as hydronium (H3O+) in accordance with reaction (6) [42] .

HCl + H 2 O H 3 O + aq + Cl aq or HCl aq H + aq + Cl aq (6)

The dissolution of alumina (Al2O3) from the clay is therefore the result of interaction between hydrogen ions (H+) and aluminium atoms of the alumina in accordance with reaction (7):

Al 2 O 3 2SiO 2 Metakaolinite ( Claycalcine ) + 6 ( H + Cl ) Hydrochloricacid solution ( 2 Al 3 + 6 Cl ) + 3 H 2 O LeachSolution ( Tobeinfiltrate ) + 2SiO 2 Residue (7)

The extent of dissolution was expressed in percentage or as a fraction where the fraction of Al ions (XAl) leached out of the clay into the solution was given as X Al = concentration of Al ions in the solution concentration of Al ions in the original clay sample while the percent Al ions (%Al) leached out of the clay into the solution was expressed as % Al = 100 X Al .

The results showed that thermal treatment (calcination temperature and holding time) has significant effect on the amount of Al ions taken into solution. The effect of calcination temperatures at different durations of heating (30, 60 or 90 minutes) is illustrated in Figures 4-6. As shown, response to leaching is lowest for the uncalcined clay sample (control 1) followed by that calcined at 1000˚C (control 2). The ability of the acid (1 M HCl) to extract alumina from the clay (and enrich the leach solution with aluminium ions) varied as calcination temperature increased from 500˚C to 900˚C. However, at 1000˚C (control 2), the ability of the acid to attack the clay and remove alumina dropped drastically. Under 30, 60 and 90 minutes holding times (Figures 4-6); the peak leaching response occurred in the case of samples calcined at 600˚C. As shown, between 500˚C and 900˚C; the response of Ibere clay to leaching by acid attack increased and dropped, reaching its peak at 600˚C. This behaviour is probably due to the transformation of the clay from its room temperature crystalline form (kaolinitic) to various degrees of amorphous state (metakaolinitic) and back to high temperature crystalline form at 1000˚C and beyond, as the clay steadily lost physically combined water (through drying and dehydration) and chemically combined water (de-hydroxylation) as temperature increased. In other words, the clay was completely de-hydrolyzed and transformed to metakaolinite (amorphous phase) when it was heated to 600˚C. Consequently, the kaolinite clay was completely crystalline or had various degrees of crystallinity below and above 600˚C.

3.3. Effect of Holding Time

Another interesting observation is that samples held for 60 minutes in the furnace responded better on leaching than those held for 30 or 90 minutes at all calcination temperatures investigated (Figure 7). This means that the ability of the acid to attack alumina in the clay and remove aluminium was low at 30 minutes holding time, reached peak value at 60 minutes holding time, and declined again when holding time was extended to 90 minutes at all temperatures studied (500˚C, 600˚C, 700˚C, 800˚C, and 900˚C). This observation could be because at 30 minutes, the transformation of the clay to amorphous (non-crystalline) state

Figure 4. Effect of calcination temperature at 30 minutes holding time on the solubilization of Al from Ibere clay leached at room temperature.

Figure 5. Effect of calcination temperature at 60 minutes holding time on the solubilization of Al from Ibere clay leached at room temperature.

Figure 6. Effect of calcination temperature at 90 minutes holding time on the solubilization of Al from Ibere clay leached at room temperature.

Figure 7. Effect of calcination duration (holding time) at different temperatures on solubilization of Al from Ibere clay under 120 minutes leaching time.

was just beginning, at 60 minutes, the transformation to amorphous metakaolinitewas completed, but holding up to 90 minutes resulted to the reappearance of some crystallinity. Prolonged heating can therefore make the silica and alumina contents of clay to react, resulting in reduction of solubility. Furthermore, prolonged heating may also bring about the sintering of particles or phases leading to reduction in leaching response [37] [38] . It can be concluded therefore that 60 minutes or 1 hour is the optimum calcination holding time for thermally activating Ibere clay to respond maximally to leaching in acid.

These observations are in conformity with XRD patterns shown in Figure 2 and Figure 3 for the raw and optimally calcined clays. Thermal treatment therefore broke down the clay structure by removing the OH water (chemically combined) holding the network of silica tetrahedra and alumina octahedra, thus rendering the alumina acid-soluble. At sufficiently high temperatures or for prolonged heating durations, the silica and alumina recrystallized to form a crystalline and insoluble phase such as mullite.

3.4. Effect of Leaching Temperature and Thermal Activation

As observed previously (Figure 7), clay calcines produced by holding for 60 minutes in the furnace (at all calcination temperatures studied) responded to leaching better than those held for 30 or 90 minutes. The effect of leaching temperature on the leaching response of calcines produced under 60 minutes duration of calcination was studied further (Figure 8). As shown, at all calcination temperatures investigated, leaching response increased as leaching temperature increased. In the case of the optimal calcine (600˚C held for 60 minutes), the amounts of aluminium solubilized after leach contact time of 1 hour in 1 M HCl were 12.42%, 23.85%, 37.58%, and 50.27% for leaching temperatures of 25˚C, 50˚C, 75˚C, and 100˚C, respectively. It can be concluded that leaching temperature has a significant effect on the rate of alumina dissolution from the clay. This

Figure 8. Effect of leaching temperature on the leaching response of selected Ibere clay calcines within leach contact time of 60 minutes.

is because high temperatures enhance diffusion or mobility and hence collision frequency of reacting species in addition to providing extra thermal energy for overcoming the energy barrier or activation energy for the process. Similar observations were made by other researchers [43] [44] [45] [46] .

The effect of thermal activation on leaching of clay calcines at different leaching temperatures is also shown in Figure 8. For example, the amount of Al extracted within 1 hour of leaching in 1 M HCl at 100˚C increased from 7.36% to 50.27% over the activation temperature range 25˚C (for uncalcined clay) to 600˚C (optimal calcine). Then there was a decline in Al extraction to 24.32% (for calcine produced at 1000˚C). Similar trends were also observed at leaching temperatures of 25˚C, 50˚C and 75˚C. This can be explained based on solid phase changes or transformations in the clay brought about by thermal treatment [36] [43] [44] .

3.5. Effect of Thermal Treatment on Activation Energy

The activation energy of leaching was found to depend on the thermal treatment given to the clay, specifically the temperature and duration of calcination (Figure 9). Low activation energies were obtained in the case of the clay calcines that responded well to leaching i.e. those with high level of Al extraction. This implies that the optimal temperature and duration of calcination corresponded with the lowest activation energy (Figures 8-10). Figure 9 shows plots of lnk versus 1/T for samples calcined under 60 minutes holding time and leached at different temperatures, i.e. 25˚C (298 K), 50˚C (323 K), 75˚C (348 K) and 100˚C (373 K). The leaching activation energies generated in Figure 9 are plotted against calcination temperature as shown in Figure 10. The lowest activation energy for leaching (24.26 kJ/mol) corresponded with the overall best calcine for the clay. Given that activation energy is the energy barrier that must be surmounted for a reaction to occur; the lowering of this energy means that leaching

Figure 9. Arrhenius plots for the leaching of Ibere clay calcined at various temperatures and leached in 1 M HCl at 198, 323, 348 and 373 Kelvin.

Figure 10. Effect of calcination temperature on activation energy of leaching for Ibere clay leached in 1 M HCl for 60 minutes contact time.

reaction is made thermodynamically or energetically easier, thus enhancing reaction rates or kinetics. This explains why clay calcine produced at 600˚C (holding for 60 minutes) yielded the highest solubility of alumina from the clay as shown by the %Al in leach solution. It was also observed that the uncalcined sample of the clay required the highest activation energy of leaching (34.84 kJ/mol); explaining why it was very difficult to leach alumina from such sample, as seen in its very low solubility data. Thus, the alumina in uncalcined or unactivated clay is locked up in the clay chemistry, responding very sluggishly to acid attack. Similarly, clay sample calcined at 1000˚C for 60 minutes recorded the next highest activation energy (31.05 kJ/mol) after the uncalcined clay. Leaching of alumina was also difficult in this case because at 1000˚C, crystalline phases had formed. Thus, the alumina is again locked up in the mullite network, making it difficult for acid attack. Similar findings were reported in literature [36] [44] . As shown in Figure 10, values of activation energy varied between the extremes of the high values reported for the uncalcined clay (at ~25˚C) and those for samples calcined at 1000˚C; reaching the lowest value of 24.26 kJ/mol at 600˚C.

4. Conclusions

The effect of thermal treatment on the transformation of Ibere kaolinite clay and subsequent leaching of alumina was investigated under atmospheric pressure1. Different thermal treatments produced different degrees of leaching response from the clay based on the nature and extent of phase transformation. X-ray diffraction studies confirmed that the optimal leaching response corresponded with the thermal treatment that transformed the clay to an amorphous phase or metakaolinite. The clay was transformed from its low-temperature crystalline form to an amorphous form at 600˚C and then back to high-temperature crystalline phases. Prolonged heating (above 90 minutes) under isothermal conditions also caused the appearance of crystalline phases and loss of solubility. Best results were achieved under 60 minutes heating duration at 600˚C. Thermal treatment also affected the activation energy of leaching such that high solubility (high leaching response) corresponded with low activation energy. Thermally activated Ibere clay can be used as alternative resource for alumina in Nigeria where bauxite is scarce or non-existent.

The present work has established the optimal calcination conditions for Ibere clay. Further work is recommended to investigate the effects of the leaching variables such as clay particle size, acid concentration, leaching temperature, solid/liquid ratio of clay weight to acid volume, and shaking rate. This will establish the optimal leaching conditions for solubilizing the alumina in the clay. Methods of recovering alumina from the leach solution should also be investigated.


This work was financially supported by a research fellowship of the Federal University of Technology, Owerri (REG/EST/SPMU/SP.2318). The authors would like to thank the unknown reviewers for their helpful comments and suggestions.

Conflicts of Interest

The authors declare no conflicts of interest regarding the publication of this paper.

1The authors acknowledge that pressure hydrometallurgy as proposed by Habashi [29] may be used to leach alumina from clay without the need for thermal activation.

Cite this paper

Mark, U., Anyakwo, C.N., Onyemaobi, O.O. and Nwobodo, C.S. (2019) Effect of Calcination Condition on Thermal Activation of Ibere Clay and Dissolution of Alumina. International Journal of Nonferrous Metallurgy, 8, 9-24.


  1. 1. Hudson, K., Misra, C. and Wefers, K. (1997) Aluminium Oxide. In: Habashi. F., Ed., Handbook of Extractive Metallurgy, Volume II, Part 3: Light Metals, John Wiley & Sons, New York, 1062-1068.

  2. 2. Hudson, K., Misra, C. and Wefers, K. (1997) Bauxite, the Principal Alumina Raw Material. In: Habashi. F., Ed., Handbook of Extractive Metallurgy, Volume II, Part 3: Light Metals, John Wiley & Sons, New York, 1068-1072.

  3. 3. Hudson, K., Misra, C. and Wefers, K. (1997) Other Processes for Alumina Production. In: Habashi. F., Ed., Handbook of Extractive Metallurgy, Volume II, Part 3: Light Metals, John Wiley & Sons, New York, 1091-1094.

  4. 4. Hudson, L.K., Misra, C., Perrotta, A.J., Wefers, K. and Williams, F.S. (2011) Aluminum Oxide. In: Elvers, B., Ed., Ullman’s Encyclopedia of Industrial Chemistry, 7th Edition, Wiley-VCH, Weiheim, 1-40.

  5. 5. Habashi, F. (1995) Bayer’s Process for Alumina Production: A Historical Perspective. Bulletin of Historical Chemistry No.17-18, 15-19.

  6. 6. Habashi, F. (2005) A Short History of Hydrometallurgy. Hydrometallurgy, 79, 15-22.

  7. 7. United States Geological Survey (USGS) (2013) Bauxite and Alumina. Compiled by Lee Bray, E., White, L.M. and Miller, L.D., 2013 Minerals Yearbook (Advance Release), 13 p.

  8. 8. United States Geological Survey (USGS) (2015) Aluminium: Mineral Commodity Summaries. Compiled by Lee Bray, E., 16-17.

  9. 9. United States Geological Survey (USGS) (2015) Bauxite and Alumina: Mineral Commodity Summaries. Compiled by Lee Bray, E., 26-27.

  10. 10. United States Geological Survey (USGS) (2015) Bauxite and Alumina: Mineral Industry Surveys, First Quarter of 2015. Compiled by Lee Bray, E. and Barnes, L.M., 1-5.

  11. 11. Schwarz, T. (1997) Distribution and Genesis of Bauxite on the Mambilla Plateau, SE Nigeria. Applied Geochemistry, 12, 119-131.

  12. 12. Petters, S.W. (1993) Metallic and Nonmetallic (Industrial) Minerals. In: Adalemo, I.A. and Baba, J.M., Eds., Nigeria: Giant in the Tropics, Volume 1: A Compendium, Gabuno Pub. Ltd., Lagos, 61.

  13. 13. Obaje, N.G. (2009) Geology and Mineral Resources of Nigeria: Lecture Notes in Earth Sciences 120. Springer, London, 52, 118-119, 183-201.

  14. 14. Wright, J.B., Hastings, D.A., Jones, W.B. and Williams, H.R. (1985) Geology and Mineral Resources of West Africa. George Allen & Unwin, London, 35, 48-49, 87, 119, 145, 157.

  15. 15. Malomo, S. (2011) Framework and Opportunities for Sustainable Private Sector Participation in Solid Minerals Development in Ekiti State. Ekiti State Economic Development Summit.

  16. 16. Talabi, A.O., Ademilua, O.L., Ajayi, O.Z. and Ogunniyi, S.O. (2013) Preliminary Geophysical Evaluation of Orin Bauxite Deposit, Southwestern Nigeria. Journal of Emerging Trends in Engineering and Applied Sciences, 4, 432-437.

  17. 17. Sada, M.M. (2013) Mid-Term Report for the Minerals and Metals Sector. Ministerial Platform Presented by Minister, Ministry of Mines and Steel Development (MMSD).

  18. 18. Adeniji, G. (2009) An Overview of Nigeria’s Solid Minerals Sector. ACCENTURE Knowledge Event, 1-10.

  19. 19. Pabalkar, V.V. (1999) Nigerian Aluminium Industry: Scope and Prospects. Proceedings of the 16th Annual Conference of the Nigerian Metallurgical Society, Abuja, 3-5 November 1999, 1-7.

  20. 20. Okorie, B.A. (2000) The Metallurgical Industry and National Development. 2nd Annual NAMMES Conference Tagged, Owerri, 16-17 March 2000, 1-8.

  21. 21. Aliyu, A. (1996) Potentials of the Solid Minerals Industry in Nigeria. RMRDC, Abuja, 1-40, 63-83, 164-172.

  22. 22. Fejokwu, L.C. (1996) Nigeria: A Viable Black Power, Vol. 2: Resources, Potentials and Challenges. Polcom Press, Lagos, 375-385.

  23. 23. Mark, U. and Onyemaobi, O.O. (2009) Assessment of the Industrial Potentials of Some Nigerian Kaolinitic Clay Deposits. International Research Journal in Engineering, Science & Technology, 6, 77-84.

  24. 24. Barsoum, M.W. (2003) Fundamentals of Ceramics. 2nd Edition, IOP Publishing Ltd., Bristle, 70-74.

  25. 25. Shackelford, J.F. (2015) Introduction to Materials Science for Engineers. 8th Edition, Pearson Higher Education, Upper Saddle River, 71-72.

  26. 26. Attah, L.E. and Oden M.I. (2010) Physico-Chemical Properties and Industrial Potential of Some Clay Deposits in Calabar Area, South Eastern Nigeria. Global Journal of Environmental Sciences, 9, 39-49.

  27. 27. Velde, B. (1995) Composition and Mineralogy of Clay Minerals. In: Velde. B., Ed., Origin and Mineralogy of Clays: Clays and the Environment, Springer, Berlin, 8-42.

  28. 28. International Committee for Study of Bauxite, Alumina and Aluminium (ICSOBA) (2018) Rusal and Russia Aluminium Industry. Upcoming Events. ICSOBA Newsletter, Vol. 17, 11-18.

  29. 29. Habashi, F. (2017) Alumina from Silicates. Technical Paper, ICSOBA Newsletter, Vol. 17, 12-14.

  30. 30. Chakraborty, A.K. (2014) Phase Transformations of Kaolinite Clay. Springer, New Delh, 3-12, 43-47, 185-206, 327-329.

  31. 31. Habashi, F. (2014) A New Era in Pressure Hydrometallurgy. Metall, 68, 27-34.

  32. 32. Velde, B. (1992) Introduction to Clay Minerals: Chemistry, Origins, Uses and Environmental Significance. Chapman & Hall, London, 1-17, 55-82, 96.

  33. 33. Fahrenholtz, W.G. (2008) Clays. In: Shackelford, J.F. and Doremus, R.H., Eds., Ceramic and Glass Materials: Structure, Properties and Processing, Springer, New York, 111-133.

  34. 34. Kaolinite (2015) In Wikipedia.

  35. 35. Ilic, B.R., Mitrovic, A.A. and Milicic, L.R. (2010) Thermal Treatment of Kaolin Clay to Obtain Metakaolin. Hemijskaindustrija, 64, 351-356.

  36. 36. Pinna, E.G., Suarez, D.G., Rosales, G.D. and Rodriguez, M.H. (2017) Hydrometallurgical Extraction of Al and Si from Kaolinitic Clays. International Engineering Journal, 70, 451-457.

  37. 37. Lamberov, A.A., Sitnikova, E.Y. and Abdulga, A.S. (2012) Kinetic Features of Phase Transformation of Kaolinite into Metakaolinite for Kaolin Clays from Different Deposits. Russian Journal of Applied Chemistry, 85, 892-897.

  38. 38. Duval, D.J., Risbud, S.H. and Shackelford, J.F. (2008) Mullite. In: Shackelford. J.F. and Doremus, R.H., Eds., Ceramic and Glass Materials: Structure, Properties and Processing, Springer, New York, 27-39.

  39. 39. Ghosh, A. and Ghosh, S. (2014) A Textbook of Metallurgical Kinetics. PHI Learning Private Ltd., Delhi, 1-10, 82-100, 151-185, 301-319.

  40. 40. Gupta, C.K. (2003) Chemical Metallurgy: Principles and Practice. Wiley-VCH Verlag GmbH & Co., Weinheim, 31-52, 459-499.

  41. 41. Rao, S.R.R. (2006) Hydrometallurgical Processes. Waste Management Series, 7, 71-108.

  42. 42. Brown, T.L., LeMay, H.E., Bursten, B.E., Murphy, C.J. and Woodward, P.M. (2012) Chemistry: The Central Science. 12th Edition, Pearson Educationm New Yorkm 512-655,

  43. 43. Al-Zahrani, A.A. and Abdul-Majid, M.H. (2009) Extraction of Alumina from Local Clays by Hydrochloric Acid Process. Engineering Science Journal of King Abdulaziz University, 20, 29-41.

  44. 44. Al-Ajeel, A.W.A. and Al-Sindy, S.I. (2006) Alumina Recovery from Iraqi Kaolinitic Clay by Hydrochloric Acid Route. Iraqi Bulletin of Geology and Mining, 2, 67-76.

  45. 45. Ajemba, R.O. and Onukwuli, O.D. (2012) Determination of the Optimum Dissolution Conditions of Ukpor Clay in Hydrochloric Acid Using Response Surface Methodology. International Journal of Engineering Research and Applications, 2, 732-742.

  46. 46. Udeigwe, U., Onukwuli, O.D., Ajemba, R. and Ude, C.N. (2015) Kinetic Studies of Hydrochloric Acid Leaching of Alumina from Agbaja Clay. International Journal of Research in Advanced Engineering and Technology, 1, 64-72.