# Averrhoa carambola: A Renewable Source of Oxalic Acid for the Facile and Green Synthesis of Divalent Metal (Fe, Co, Ni, Zn, and Cu) Oxalates and Oxide Nanoparticles

Authors: Nguimezong Nguefack Marius Borel; Josepha Foba-Tendo; Divine Mbom Yufanyi; Ekane Peter Etape; Jude Namanga Eko; Lambi John Ngolui
Journal: Journal of Applied Chemistry
 (2014)

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## Abstract

A green, simple, and environmentally benign synthetic approach has been utilised to obtain some bivalent metal oxalates fromAverrhoa carambola juice extract, without any purification or special treatment of the juice. The main acid components (oxalic acid and ascorbic acid) of the juice were identified by HPLC technique. The effect of temperature on the purity of the product has been investigated. The as-synthesized metal oxalates were thermally decomposed at low temperatures to their respective metal oxide nanoparticles. The metal oxalates and their respective thermal decomposition products were characterized by Fourier Transform Infrared spectroscopy, X-ray diffraction analysis, and thermogravimetry.


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## Body

## 1. Introduction

Metal carboxylates have been widely investigated and have been used as precursors in the production of metal oxide nanomaterials [1–6]. Generally, these metal carboxylates are thermally decomposed at relatively low temperatures into the corresponding metal oxide nanomaterials. The precursors are usually obtained when the metal salt reacts with the free acid or any of its labile carboxylates. The reactants are generally synthetic, but many of these carboxylates are readily available in our environment (mostly in plants) and need only to be harnessed. They include, amongst others, citric acid, tartaric acid, and oxalic acid. The latter is known to be one of the major acids in many plants (e.g., Rhubarb andAverrhoa carambola).Averrhoa carambola, known as carambola or star fruit, is an attractive, exotic, tropical, and shrub-like ornamental tree of the Oxalidaceae family [7–10]. The ripe fruits can be eaten fresh or used to produce juice, jelly, or wine [11]. The fruit is also widely used in traditional medicine for the treatment of a wide range of ailments [10, 12]. It is also a potential source of pectin [12]. Carambola fruit juice has been shown [7, 13] to contain active constituents such as vitamins, amino acids, ascorbic acid, oxalic acid, tartaric acid, citric acid, carbohydrates, fats, and proteins. Assessment of the physicochemical properties of carambola fruit juice from ripe and unripe fruits showed that the pH of the fruits increased with advance in maturity, being 2.4 for green mature, 2.7 for half-ripe, and 3.44 for ripe fruits [7].Averrhoa carambola is a very good source of oxalic acid, with oxalic acid contents that can be as high as 1 wt% of wet mass (representing about 74% of the total acid content depending on the level of maturity of the fruits) [7, 14, 15].The high concentration of oxalic acid in this fruit is responsible for its toxicity. Star fruit and other plants containing high amounts of oxalates can cause neurotoxic and nephrotoxic effects in humans and animals [16–19]. It will therefore be very useful to develop an approach that can reduce the amount of acid in the fruit prior to its consumption. We here explore the feasibility of using this naturally available and sustainable resource (Averrhoa carambola L.) rather than the commercial sources for the synthesis of metal oxalates. The use of these natural renewable resources is of environmental significance and in the case of free oxalic acid rich fruits (e.g.,Averrhoa carambola L.) could result in a significant reduction in the level of the free acid, thus adding value to the elimination of toxic components through reaction with metal ions of biological and technological importance. This could also open up the possibility of high value exploitation of spoiled fruits.In order to render the synthesis cost effective and eco-friendly, we decided to proceed with a synthetic pathway where the fruit juice is used directly without initial purification steps or prior extraction of the acid. This decision was guided by the fact that in the natural condition of the juice (pH 2.6–3.1) oxalic acid has a better chance to react preferentially with the metal ions owing to its relative high acidic strength (pKa1 (1.23) and pKa2 (4.19)). In comparison with the other carboxylic acids present in the juice, oxalic acid requires no initial alkaline deprotonation step to precipitate with the metal ions and the precipitation can therefore occur at the natural pH of the juice.The synthesis of metal (Mn, Fe, Co, Ni, Cu, Zn, and Cd) oxalates by solvothermal [4], microemulsion [2], reverse micellar route [13], solid state route [20] and by single diffusion technique in agar gel [6] has been reported. These oxalate nanorods have been used as precursors for the synthesis of oxide nanoparticles. Thermal decomposition of these precursors in the temperature range 450–500°C yielded homogeneous oxide nanoparticles. In the different synthesis methods, a reaction of the appropriate metal salts and oxalic acid from commercial sources was used.Herein we present a facile and green approach for the synthesis of metal oxalates and their subsequent thermal decomposition to the oxide nanoparticles. Our approach is based on mixing the metal ion solution and the fruit juice extract without the use of hazardous organic compounds or surfactants. In this preliminary study, five divalent 3d metal ions (Fe2+, Co2+, Ni2+, Zn2+, and Cu2+) were used for the proof of concept. The as prepared complexes and their various thermal decomposition products have been characterized by FTIR, powder XRD, and TGA.


## 2. Experimental

### 2.1. Chemicals

Fe(II), Co(II), Ni(II), Cu(II), and Zn(II) chlorides were obtained from Sigma Aldrich. The chemicals were of analytical grade and were used without further purification. HPLC grade oxalic, ascorbic, citric, lactic, malic, malonic, and succinic acids were also used.


### 2.2. Processing of the Fruit Juice

Ripe carambola fruits were harvested from the campus of CRTV Buea in the South-West Region of Cameroon. The fruits were washed under running tap water and crushed in a blender. The juice was extracted by squeezing through cheese cloth. The collected juice was centrifuged for 20 min at 3000 rpm, the supernatant was filtered, and the filtrate collected and kept in a freezer for further use.


### 2.3. Characterization of the Juice

The acid content of the juice was investigated using HPLC. The HPLC system (DEGASY DG-1210) with an autosampler was coupled to a Gynkotek UV-detector (UVD340S) set at three wavelengths (214, 230, and 254 nm). The data was collected and processed with Chromeleon software. The analyses were performed isocratically at 1.2 mL/min at room temperature with an Altima C18 column (250 × 10 mm, 5μm). The mobile phase was 0.1% W/V H3PO4 acidified distilled water. Standard solutions of several acids (oxalic, ascorbic, citric, lactic, malic, malonic, and succinic acids) were prepared and their chromatograms recorded as described above with a run time of 25 min and compared to that of the juice extract. Identification of the peaks enabled us to determine the nature of the acids contained in the juice. The amount of oxalic acid in the juice was determined by a spectrophotometric method based on the catalytic oxidation of bromophenol blue by dichromate using oxalic acid as the catalyst [21].


### 2.4. Synthesis of the Metal Oxalates

Prior to the synthesis, the pH of the juice was measured with Fisherdrand Hydrus 500 pH meter.Solutions (0.1 M) of the various metal ions (Fe2+, Co2+, Ni2+, Zn2+, and Cu2+) were prepared by dissolving the appropriate amount of the metal chloride in 100 mL distilled water. 30 mL of the juice extract was poured into a 250 mL round bottom flask immersed into a water bath maintained at 80°C. The appropriate metal ion solution (40 mL) was added slowly into the juice while stirring, and the mixture was stirred for a given period of time, as summarized in Table 1. The mixture was allowed to cool to room temperature and the precipitates obtained were filtered, washed several times with distilled water (to remove any undesired ions), allowed to air-dry overnight, and finally dried in a desiccator over calcium chloride.Table 1
Summary of sample codes, synthesis time, and colour of precipitates.
Sample (code)
Synthesis time (min)
Colour of precipitate formed
Fe2+ (P1)
45
Yellow
Co2+ (P2)
30
Pink
Ni2+ (P3)
60
Light green
Cu2+ (P5)
60
Light blue
Zn2+ (P4)
60
WhiteIn order to study the effect of temperature on the synthesis product, we synthesized Co2+ complexes at various temperatures (room temperature, 45°C, 60°C, and 80°C) and compared their XRD patterns. Based on our observations 80°C was chosen as synthesis temperature for the precursors.


### 2.5. Thermal Decomposition of the Complexes

A sample of the dry precursor (0.5 g) was ground, placed in a ceramic crucible and the crucible was placed in the furnace that had been heated to the desired calcination temperature of 550°C and calcination in air continued for 4 h. The sample was allowed to cool down to room temperature in the furnace. The residues (Dp1, Dp2, Dp3, and Dp4, resp., from P1, P2, P3, and P4) obtained were weighed and kept for further analyses. They represent, respectively, 43.9%, 44.4%, 42.9%, and 40.9% of the precursors.


### 2.6. Characterization Techniques

FTIR spectra were recorded from 4000 to 400 cm−1 on a PerkinElmer Spectrum Two Universal Attenuated Total Reflectance Fourier Transform Infrared (UATR-FTIR) spectrometer. Thermogravimetric analysis (TGA) was obtained using a Pyris 6 PerkinElmer TGA 4000 thermal analyser. The TGA analysis was conducted between 30 and 900°C under nitrogen atmosphere at a flow rate of 20 mL/min and a temperature ramp of 10°C/min. The XRD diffractograms of the precursors and the decomposition products were recorded on a Bruker D8 advance X-ray diffractometer using a Cu Kα radiation source (λ = 0.15406 nm, 40 kV, and 40 mA). Scans were taken over the 2θ range from 10° to 100° in steps of 0.01° at room temperature in open quartz sample holders. The phase was identified with the help of the BrukerDIFFRACplus evaluation software in combination with the ICDD powder diffraction data base (International Centre for Diffraction Data).


## 2.1. Chemicals

Fe(II), Co(II), Ni(II), Cu(II), and Zn(II) chlorides were obtained from Sigma Aldrich. The chemicals were of analytical grade and were used without further purification. HPLC grade oxalic, ascorbic, citric, lactic, malic, malonic, and succinic acids were also used.


## 2.2. Processing of the Fruit Juice

Ripe carambola fruits were harvested from the campus of CRTV Buea in the South-West Region of Cameroon. The fruits were washed under running tap water and crushed in a blender. The juice was extracted by squeezing through cheese cloth. The collected juice was centrifuged for 20 min at 3000 rpm, the supernatant was filtered, and the filtrate collected and kept in a freezer for further use.


## 2.3. Characterization of the Juice

The acid content of the juice was investigated using HPLC. The HPLC system (DEGASY DG-1210) with an autosampler was coupled to a Gynkotek UV-detector (UVD340S) set at three wavelengths (214, 230, and 254 nm). The data was collected and processed with Chromeleon software. The analyses were performed isocratically at 1.2 mL/min at room temperature with an Altima C18 column (250 × 10 mm, 5μm). The mobile phase was 0.1% W/V H3PO4 acidified distilled water. Standard solutions of several acids (oxalic, ascorbic, citric, lactic, malic, malonic, and succinic acids) were prepared and their chromatograms recorded as described above with a run time of 25 min and compared to that of the juice extract. Identification of the peaks enabled us to determine the nature of the acids contained in the juice. The amount of oxalic acid in the juice was determined by a spectrophotometric method based on the catalytic oxidation of bromophenol blue by dichromate using oxalic acid as the catalyst [21].


## 2.4. Synthesis of the Metal Oxalates

Prior to the synthesis, the pH of the juice was measured with Fisherdrand Hydrus 500 pH meter.Solutions (0.1 M) of the various metal ions (Fe2+, Co2+, Ni2+, Zn2+, and Cu2+) were prepared by dissolving the appropriate amount of the metal chloride in 100 mL distilled water. 30 mL of the juice extract was poured into a 250 mL round bottom flask immersed into a water bath maintained at 80°C. The appropriate metal ion solution (40 mL) was added slowly into the juice while stirring, and the mixture was stirred for a given period of time, as summarized in Table 1. The mixture was allowed to cool to room temperature and the precipitates obtained were filtered, washed several times with distilled water (to remove any undesired ions), allowed to air-dry overnight, and finally dried in a desiccator over calcium chloride.Table 1
Summary of sample codes, synthesis time, and colour of precipitates.
Sample (code)
Synthesis time (min)
Colour of precipitate formed
Fe2+ (P1)
45
Yellow
Co2+ (P2)
30
Pink
Ni2+ (P3)
60
Light green
Cu2+ (P5)
60
Light blue
Zn2+ (P4)
60
WhiteIn order to study the effect of temperature on the synthesis product, we synthesized Co2+ complexes at various temperatures (room temperature, 45°C, 60°C, and 80°C) and compared their XRD patterns. Based on our observations 80°C was chosen as synthesis temperature for the precursors.


## 2.5. Thermal Decomposition of the Complexes

A sample of the dry precursor (0.5 g) was ground, placed in a ceramic crucible and the crucible was placed in the furnace that had been heated to the desired calcination temperature of 550°C and calcination in air continued for 4 h. The sample was allowed to cool down to room temperature in the furnace. The residues (Dp1, Dp2, Dp3, and Dp4, resp., from P1, P2, P3, and P4) obtained were weighed and kept for further analyses. They represent, respectively, 43.9%, 44.4%, 42.9%, and 40.9% of the precursors.


## 2.6. Characterization Techniques

FTIR spectra were recorded from 4000 to 400 cm−1 on a PerkinElmer Spectrum Two Universal Attenuated Total Reflectance Fourier Transform Infrared (UATR-FTIR) spectrometer. Thermogravimetric analysis (TGA) was obtained using a Pyris 6 PerkinElmer TGA 4000 thermal analyser. The TGA analysis was conducted between 30 and 900°C under nitrogen atmosphere at a flow rate of 20 mL/min and a temperature ramp of 10°C/min. The XRD diffractograms of the precursors and the decomposition products were recorded on a Bruker D8 advance X-ray diffractometer using a Cu Kα radiation source (λ = 0.15406 nm, 40 kV, and 40 mA). Scans were taken over the 2θ range from 10° to 100° in steps of 0.01° at room temperature in open quartz sample holders. The phase was identified with the help of the BrukerDIFFRACplus evaluation software in combination with the ICDD powder diffraction data base (International Centre for Diffraction Data).


## 3. Results and Discussion

Reaction of the respective metal salts with the carambola juice at 80°C generally leads to coloured complexes (except the zinc complex, P4) in high yields. The metal complexes are less intense in colour than the respective metal salts from which they were derived. The complexes are crystalline solids that are air stable and nonhygroscopic as opposed to the starting salts. Physical data for the complexes are presented in Table1.


### 3.1. HPLC Analysis of Juice Extract

Figure1 shows the HPLC chromatogram of the juice. Only two peaks appear after 22 minutes of run. These peaks are compared with those of the standard oxalic acid (RT 10.966 min) and ascorbic acid (RT 18.938 min). The absence of the peaks of other acids indicates that they are either absent or if present they are in trace proportions. This observation supports that of several authors who found that the principal acids in the mature fruits are ascorbic and oxalic acids [7, 14, 15]. It has been observed that as the fruits mature the relative content of oxalic acid increases while that of other acids decrease [7, 15]. The amount of oxalic acid in the juice as determined by spectrophotometry was found to be in the range of 7.6–11.6 gL
-
1, in agreement with the literature reports where the content is generally in the range of 6.3 to 12 gL−1 of the juice [7, 14]. The pH of the juice was found to be in the range 2.6 to 3.1. This falls within the range observed by Patil et al. [7] and Narain et al. [15]. These authors both observed an increase of pH as the fruit mature.Figure 1
HPLC chromatogram of the juice.


### 3.2. FTIR Spectral Characterisation

The formation of pure oxalate phases is indicated by FTIR analysis. Figure2((a)–(e)) shows the FTIR spectra of all the metal complexes synthesized from carambola juice. They all exhibit similar characteristics and comparable patterns, except that of P5. The bands observed are similar to those reported in the literature for metal oxalate dihydrates [22, 23]. The broad band at 3343 cm
-
1 is attributed to the stretching vibration of the O–H bond of water molecules of crystallisation. The absence of this band in the spectrum of the copper complex (P5) attests to the reduced amount of water of crystallisation in this complex. The strong band at 1614 cm
-
1 is due to the antisymmetric stretching mode of the carbonyl group C=O of the oxalate. The two bands at 1359 and 1314 cm
-
1 are those of C–O symmetric stretching mode. The difference between ν
as(COO) and ν
sym(COO) stretching frequencies is 255 cm
-
1 indicating a bidentate or a terminal monodentate coordination mode of the oxalate ligand in the complexes [24]. The bands at 822 cm
-
1 is attributed to the bending vibration of O–C–O and the band at 745 cm
-
1 (absent in the spectrum of the Cu complex) is attributed to H–O–H rocking. The fact that no other bands are present attests to the identity and purity of the samples.Figure 2
FTIR spectra of the complexes (spectra (a), (b), (c), (d), and (e) are for P1, P2, P3, P4, and P5, resp.).Figure3((a)–(d)) shows the FTIR spectra of the decomposition products (DPi) of the various complexes. The bands present on the spectrum of the precursor complexes (Figure 2) have disappeared and new bands have appeared. The disappearance of the bands is attributed to the complete decomposition of the complexes. We observed the appearance of new bands in all the spectra suggesting the formation of new products. These bands are all around 500 cm
-
1 and are attributed to the stretching vibration of the M–O bond. The spectra of Dp1 and Dp2 show two bands in this vicinity. In the case of cobalt product (Dp2) the bands are at 660 and 550 cm
-
1 which suggest the formation of spinel Co3O4 that is (Co2+)(Co3+)2(O
2
-)4 [25]. These bands have been attributed, respectively, to (Co2+)–O–(Co3+) and to (Co3+)–O–(Co3+) vibrations [16–18, 25]. The presence of two bands instead of one or three bands in the spectrum of the iron product excludes the possibility of having Fe3O4 or γ-Fe2O3 and suggests that the product is likely to be pure α-Fe2O3 [19, 26].Figure 3
FTIR spectra of the thermal decomposition products (spectra (a), (b), (c), and (d) are for Dp1, Dp2, Dp3, and Dp4, resp.).


### 3.3. X-Ray Diffraction

The XRD spectra of the cobalt complexes synthesised at different temperatures are shown in Figure4. The observed XRD patterns are similar to that of the standard prepared from commercial oxalic acid as well as to those reported in the literature [20, 24]. This indicates that cobalt oxalate dihydrate was obtained at the different synthesis temperatures. However, a close look at the XRD patterns reveals that some of the peaks such as (400) are not well resolved at lower temperatures (RT, 45 and 60°C). The spectra of the samples synthesized at lower temperatures also exhibit unidentified peaks (
*
). This suggests that despite the possibility to obtain the complexes at low temperatures, pure phases that compare to the standard are obtained at 80°C. This prompted our decision to run all of the subsequent syntheses at 80°C.Figure 4
XRD patterns of CoOX synthesised at different temperatures.The XRD patterns of the metal complexes and their corresponding decomposition products are shown in Figure5. The peaks have been indexed as shown on the spectra. The patterns of the complexes (a1, b1, c1, and d1, respectively, for P1, P2, P3, and P4) are in good agreement with the JCPDS cards reported for the various metal oxalate dihydrates (except the pattern e which is not that of a dihydrate). The XRD spectrum of sample P1 matches the JCPDS card no 72-1305 for FeC2O4
·2H2O [19]. The XRD pattern of sample P2 matches the JCPDS card no 25-0250 for β-CoC2O4
·2H2O [20, 24, 27]. The pattern of the nickel complex (P3) agrees with the JCPDS card no 14-0742 for NiC2O4·2H2O [20]. The zinc complex is identified as ZnC2O4·2H2O [28], its pattern agrees with JCPDS card no 25-1029, and the pattern of P5 is indexed in an orthorhombic cell with parameters described in JCPDS card no 21-0297 for CuC2O4·xH2O (x
<
1) [20]. All of the peaks are attributed to the corresponding M
II
C
2
O
4
·
2
H
2
O and confirm that our products are the expected metal oxalates as already suggested from FTIR results.XRD spectra for the complexes (a1–e) and of their decomposition products (a2–d2).
(a)
(b)
(c)
(d)
(e)The XRD pattern of the thermal decomposition products (Dp1, Dp2, Dp3, and Dp4) matched the patterns of the metal oxides as follows: the pattern of Dp1 compares with JCPDS card no 33-0664 for pure rhombohedral α-Fe2O3 [19, 26]. The pattern of Dp2 compares with JCPDS card no 42-1467 for the spinel Co3O4 (space group: Fd3m, lattice parameter) [27]. The pattern of Dp3 agrees with JCPDS card no 73-1519 for NiO [29] and the XRD pattern of Dp4 is indexed with respect to the parameters of JCPDS card no 36-1451 corresponding to ZnO [28, 30]. The purity of the products is evidenced by the absence of any impurity peaks.The average crystallite sizes of the complexes were estimated using the Debye-Scherrer equation:(1)
D
=
0.9
λ
β
cos
⁡
θ
,
where λ is the wavelength of the X-ray, β is the full width at half maximum (FWHM) of the diffraction peak, and θ is the Bragg diffraction angle. The FWHM and the other parameters of the peaks were determined with OriginLab7 fitting wizard by using the Amplitude version of Gaussian peak function. Calculations were done with three peaks for each of the samples and averaged. The as-determined average particle sizes for both the complexes and their decomposition products are shown in Table 2. The products are of nanometre size with average crystallite size in the range 14–25 nm.Table 2
Average crystallite sizes of the complexes and their decomposition products obtained using Debye-Scherrer equation.
Metal ion
Metal oxalate
Metal oxide
Peak
Size (nm)
Average (nm)
Peak
Size (nm)
Average (nm)
Fe2+
(202)
23.08
24.9
(012)
23.34
22.6
(224)
27.10
(104)
24.35
(022)
24.57
(024)
21.03
Co2+
(002)
21.65
22.5
(220)
21.74
20.3
(022)
24.06
(311)
21.98
(224)
21.67
(400)
17.23
Ni2+
(202)
17.42
19.7
(111)
14.80
14.5
(004)
22.54
(200)
14.50
(022)
19.17
(220)
14.05
Zn2+
(002)
24.64
23.3
(100)
20.72
19.3
(402)
22.12
(101)
19.76
(022)
23.28
(102)
17.40
Cu2+
(110)
16.25
15.0
(011)
15.99
Not available
(220)
12.78The thermograms of the complexes are shown in Figure6 and summarised in Table 3. To better elucidate the thermal behaviour of the complexes, a graph of the weight difference for consecutive rows against the temperature was plotted (Figure 7). The thermograms of four of the complexes (MC2O4·xH2O, where M = Fe2+, Co2+, Ni2+, and Zn2+) show two well defined steps of weight loss in agreement with reports in literature [24, 28, 31]. The first weight loss for FeC2O4·xH2O (20.9%) occurs in the range 170–218°C. This is attributed to the elimination of two molecules of water of crystallization according to the theoretical value (19.69%). The same is true for the first weight loss of CoC2O4·xH2O (19.34%, 170–232°C), NiC2O4·xH2O (20.61%, 210–285°C), and ZnC2O4·xH2O (17.83%, 132–198°C) according to their respective theoretical values (19.69%, 19.71%, and 19.02%). This confirms the XRD observation that the complexes are metal oxalate dihydrates (MC2O4·2H2O, where M = Fe, Co, Ni, or Zn). The dehydration reaction can be written as follows:
(2)
MC
2
O
4
·
2
H
2
O
⟶
MC
2
O
4
+
2
H
2
O
.Table 3
Thermal decomposition temperatures and weight loss.
(a)
First weight loss
Second weight loss
Temp (°C)
Obs. (%)
Calc. (%)
Temp. (°C)
Obs. (%)
Calc. (%)
PossibleMO
x formed
FeC2O4·2H2O
170–218
20.9
20.95
242–330
35.7
40.03
FeO
35.59
Fe2O3
37.07
Fe3O4
CoC2O4·2H2O
170–232
19.3
19.69
350–436
39.7
39.36
CoO
34.99
Co2O3
36.44
Co3O4
NiC2O4·2H2O
210–285
20.6
19.72
370–434
41.9
39.41
NiO
ZnC2O4·2H2O
132–198
17.8
19.02
385–445
38.9
38.02
ZnO
(b)
Sloppy weight loss
Sharp weight loss
Temp. (°C)
Obs. (%)
Calc. (%) depends onx
Temp. (°C)
Obs. (%)
Calc. (%) depends onx
MO
x
CuC2O4·xH2O
272
3.8
x = 0
0
272–360
54.4
x = 0
46.89
CuO
x = 1
21.25
x = 1
42.47
x = 0.3
3.92
x = 0.3
55.5
CuTG thermograms of the metal oxalates.
(a)
(b)
(c)
(d)
(e)Figure 7
Df-TG plots of the difference in weight in consecutive rows against temperature.On the other hand, the thermogram of CuC2O4·xH2O shows a single well-defined weight loss portion. There is a region of gradual weight loss (3.8%) between 245 and 310°C immediately followed by the sharp portion hat end at 360°C. This decomposition pattern has been observed by Jongen et al. [32]. The absence of a well-defined dehydration step suggests that there is a very little amount of water of crystallization in CuC2O4·xH2O. Using the observed weight loss, the amount of water was estimated and the following molecular formula proposed CuC2O4·0.3H2O. This agrees with its FTIR spectrum which shows no clear bands that can be assigned to water. The sharp weight loss portion on the thermogram of CuC2O4·0.3H2O corresponds to 54.4% which is very close to 55.5% expected for the loss of two molecules of CO2 and the formation of metallic copper. As shown by the TG and Df-TG graphs, there is an increase in weight that occurs around 460°C. We attribute this event to the oxidation of the metallic copper. As can be seen on Table 2 this is the process that best agrees with the observed values. This weight loss portion corresponds to the second weight loss portions of FeC2O4·xH2O (35.7%, between 242 and 330°C), CoC2O4·xH2O (39.68%, 350–436°C), NiC2O4·xH2O (41.9%, 370–434°C), and ZnC2O4·xH2O (38.9%, 385–445°C). As observed in the literature [28] some of these complexes will likely decompose in pathways which involve the decomposition of the anhydrous metal oxalate (NiC2O4 and ZnC2O4) into (NiO and ZnO, resp.) with the elimination of CO2 and CO. As for FeC2O4·2H2O and CoC2O4·2H2O this decomposition step might result in the production of a variety of products (MO, M2O3, or M3O4). The Df-TG of CoC2O4·2H2O suggests that its second weight loss proceeds in two steps. Based on this observation and on the report made by Wu (2011) [33] we suggest that CoC2O4 undergoes both decomposition and oxidation reactions to produce CO2 and Co3O4 (3):
(3)
3
CoC
2
O
4
+
2
O
2
⟶
Co
3
O
4
+
6
CO
2
.


## 3.1. HPLC Analysis of Juice Extract

Figure1 shows the HPLC chromatogram of the juice. Only two peaks appear after 22 minutes of run. These peaks are compared with those of the standard oxalic acid (RT 10.966 min) and ascorbic acid (RT 18.938 min). The absence of the peaks of other acids indicates that they are either absent or if present they are in trace proportions. This observation supports that of several authors who found that the principal acids in the mature fruits are ascorbic and oxalic acids [7, 14, 15]. It has been observed that as the fruits mature the relative content of oxalic acid increases while that of other acids decrease [7, 15]. The amount of oxalic acid in the juice as determined by spectrophotometry was found to be in the range of 7.6–11.6 gL
-
1, in agreement with the literature reports where the content is generally in the range of 6.3 to 12 gL−1 of the juice [7, 14]. The pH of the juice was found to be in the range 2.6 to 3.1. This falls within the range observed by Patil et al. [7] and Narain et al. [15]. These authors both observed an increase of pH as the fruit mature.Figure 1
HPLC chromatogram of the juice.


## 3.2. FTIR Spectral Characterisation

The formation of pure oxalate phases is indicated by FTIR analysis. Figure2((a)–(e)) shows the FTIR spectra of all the metal complexes synthesized from carambola juice. They all exhibit similar characteristics and comparable patterns, except that of P5. The bands observed are similar to those reported in the literature for metal oxalate dihydrates [22, 23]. The broad band at 3343 cm
-
1 is attributed to the stretching vibration of the O–H bond of water molecules of crystallisation. The absence of this band in the spectrum of the copper complex (P5) attests to the reduced amount of water of crystallisation in this complex. The strong band at 1614 cm
-
1 is due to the antisymmetric stretching mode of the carbonyl group C=O of the oxalate. The two bands at 1359 and 1314 cm
-
1 are those of C–O symmetric stretching mode. The difference between ν
as(COO) and ν
sym(COO) stretching frequencies is 255 cm
-
1 indicating a bidentate or a terminal monodentate coordination mode of the oxalate ligand in the complexes [24]. The bands at 822 cm
-
1 is attributed to the bending vibration of O–C–O and the band at 745 cm
-
1 (absent in the spectrum of the Cu complex) is attributed to H–O–H rocking. The fact that no other bands are present attests to the identity and purity of the samples.Figure 2
FTIR spectra of the complexes (spectra (a), (b), (c), (d), and (e) are for P1, P2, P3, P4, and P5, resp.).Figure3((a)–(d)) shows the FTIR spectra of the decomposition products (DPi) of the various complexes. The bands present on the spectrum of the precursor complexes (Figure 2) have disappeared and new bands have appeared. The disappearance of the bands is attributed to the complete decomposition of the complexes. We observed the appearance of new bands in all the spectra suggesting the formation of new products. These bands are all around 500 cm
-
1 and are attributed to the stretching vibration of the M–O bond. The spectra of Dp1 and Dp2 show two bands in this vicinity. In the case of cobalt product (Dp2) the bands are at 660 and 550 cm
-
1 which suggest the formation of spinel Co3O4 that is (Co2+)(Co3+)2(O
2
-)4 [25]. These bands have been attributed, respectively, to (Co2+)–O–(Co3+) and to (Co3+)–O–(Co3+) vibrations [16–18, 25]. The presence of two bands instead of one or three bands in the spectrum of the iron product excludes the possibility of having Fe3O4 or γ-Fe2O3 and suggests that the product is likely to be pure α-Fe2O3 [19, 26].Figure 3
FTIR spectra of the thermal decomposition products (spectra (a), (b), (c), and (d) are for Dp1, Dp2, Dp3, and Dp4, resp.).


## 3.3. X-Ray Diffraction

The XRD spectra of the cobalt complexes synthesised at different temperatures are shown in Figure4. The observed XRD patterns are similar to that of the standard prepared from commercial oxalic acid as well as to those reported in the literature [20, 24]. This indicates that cobalt oxalate dihydrate was obtained at the different synthesis temperatures. However, a close look at the XRD patterns reveals that some of the peaks such as (400) are not well resolved at lower temperatures (RT, 45 and 60°C). The spectra of the samples synthesized at lower temperatures also exhibit unidentified peaks (
*
). This suggests that despite the possibility to obtain the complexes at low temperatures, pure phases that compare to the standard are obtained at 80°C. This prompted our decision to run all of the subsequent syntheses at 80°C.Figure 4
XRD patterns of CoOX synthesised at different temperatures.The XRD patterns of the metal complexes and their corresponding decomposition products are shown in Figure5. The peaks have been indexed as shown on the spectra. The patterns of the complexes (a1, b1, c1, and d1, respectively, for P1, P2, P3, and P4) are in good agreement with the JCPDS cards reported for the various metal oxalate dihydrates (except the pattern e which is not that of a dihydrate). The XRD spectrum of sample P1 matches the JCPDS card no 72-1305 for FeC2O4
·2H2O [19]. The XRD pattern of sample P2 matches the JCPDS card no 25-0250 for β-CoC2O4
·2H2O [20, 24, 27]. The pattern of the nickel complex (P3) agrees with the JCPDS card no 14-0742 for NiC2O4·2H2O [20]. The zinc complex is identified as ZnC2O4·2H2O [28], its pattern agrees with JCPDS card no 25-1029, and the pattern of P5 is indexed in an orthorhombic cell with parameters described in JCPDS card no 21-0297 for CuC2O4·xH2O (x
<
1) [20]. All of the peaks are attributed to the corresponding M
II
C
2
O
4
·
2
H
2
O and confirm that our products are the expected metal oxalates as already suggested from FTIR results.XRD spectra for the complexes (a1–e) and of their decomposition products (a2–d2).
(a)
(b)
(c)
(d)
(e)The XRD pattern of the thermal decomposition products (Dp1, Dp2, Dp3, and Dp4) matched the patterns of the metal oxides as follows: the pattern of Dp1 compares with JCPDS card no 33-0664 for pure rhombohedral α-Fe2O3 [19, 26]. The pattern of Dp2 compares with JCPDS card no 42-1467 for the spinel Co3O4 (space group: Fd3m, lattice parameter) [27]. The pattern of Dp3 agrees with JCPDS card no 73-1519 for NiO [29] and the XRD pattern of Dp4 is indexed with respect to the parameters of JCPDS card no 36-1451 corresponding to ZnO [28, 30]. The purity of the products is evidenced by the absence of any impurity peaks.The average crystallite sizes of the complexes were estimated using the Debye-Scherrer equation:(1)
D
=
0.9
λ
β
cos
⁡
θ
,
where λ is the wavelength of the X-ray, β is the full width at half maximum (FWHM) of the diffraction peak, and θ is the Bragg diffraction angle. The FWHM and the other parameters of the peaks were determined with OriginLab7 fitting wizard by using the Amplitude version of Gaussian peak function. Calculations were done with three peaks for each of the samples and averaged. The as-determined average particle sizes for both the complexes and their decomposition products are shown in Table 2. The products are of nanometre size with average crystallite size in the range 14–25 nm.Table 2
Average crystallite sizes of the complexes and their decomposition products obtained using Debye-Scherrer equation.
Metal ion
Metal oxalate
Metal oxide
Peak
Size (nm)
Average (nm)
Peak
Size (nm)
Average (nm)
Fe2+
(202)
23.08
24.9
(012)
23.34
22.6
(224)
27.10
(104)
24.35
(022)
24.57
(024)
21.03
Co2+
(002)
21.65
22.5
(220)
21.74
20.3
(022)
24.06
(311)
21.98
(224)
21.67
(400)
17.23
Ni2+
(202)
17.42
19.7
(111)
14.80
14.5
(004)
22.54
(200)
14.50
(022)
19.17
(220)
14.05
Zn2+
(002)
24.64
23.3
(100)
20.72
19.3
(402)
22.12
(101)
19.76
(022)
23.28
(102)
17.40
Cu2+
(110)
16.25
15.0
(011)
15.99
Not available
(220)
12.78The thermograms of the complexes are shown in Figure6 and summarised in Table 3. To better elucidate the thermal behaviour of the complexes, a graph of the weight difference for consecutive rows against the temperature was plotted (Figure 7). The thermograms of four of the complexes (MC2O4·xH2O, where M = Fe2+, Co2+, Ni2+, and Zn2+) show two well defined steps of weight loss in agreement with reports in literature [24, 28, 31]. The first weight loss for FeC2O4·xH2O (20.9%) occurs in the range 170–218°C. This is attributed to the elimination of two molecules of water of crystallization according to the theoretical value (19.69%). The same is true for the first weight loss of CoC2O4·xH2O (19.34%, 170–232°C), NiC2O4·xH2O (20.61%, 210–285°C), and ZnC2O4·xH2O (17.83%, 132–198°C) according to their respective theoretical values (19.69%, 19.71%, and 19.02%). This confirms the XRD observation that the complexes are metal oxalate dihydrates (MC2O4·2H2O, where M = Fe, Co, Ni, or Zn). The dehydration reaction can be written as follows:
(2)
MC
2
O
4
·
2
H
2
O
⟶
MC
2
O
4
+
2
H
2
O
.Table 3
Thermal decomposition temperatures and weight loss.
(a)
First weight loss
Second weight loss
Temp (°C)
Obs. (%)
Calc. (%)
Temp. (°C)
Obs. (%)
Calc. (%)
PossibleMO
x formed
FeC2O4·2H2O
170–218
20.9
20.95
242–330
35.7
40.03
FeO
35.59
Fe2O3
37.07
Fe3O4
CoC2O4·2H2O
170–232
19.3
19.69
350–436
39.7
39.36
CoO
34.99
Co2O3
36.44
Co3O4
NiC2O4·2H2O
210–285
20.6
19.72
370–434
41.9
39.41
NiO
ZnC2O4·2H2O
132–198
17.8
19.02
385–445
38.9
38.02
ZnO
(b)
Sloppy weight loss
Sharp weight loss
Temp. (°C)
Obs. (%)
Calc. (%) depends onx
Temp. (°C)
Obs. (%)
Calc. (%) depends onx
MO
x
CuC2O4·xH2O
272
3.8
x = 0
0
272–360
54.4
x = 0
46.89
CuO
x = 1
21.25
x = 1
42.47
x = 0.3
3.92
x = 0.3
55.5
CuTG thermograms of the metal oxalates.
(a)
(b)
(c)
(d)
(e)Figure 7
Df-TG plots of the difference in weight in consecutive rows against temperature.On the other hand, the thermogram of CuC2O4·xH2O shows a single well-defined weight loss portion. There is a region of gradual weight loss (3.8%) between 245 and 310°C immediately followed by the sharp portion hat end at 360°C. This decomposition pattern has been observed by Jongen et al. [32]. The absence of a well-defined dehydration step suggests that there is a very little amount of water of crystallization in CuC2O4·xH2O. Using the observed weight loss, the amount of water was estimated and the following molecular formula proposed CuC2O4·0.3H2O. This agrees with its FTIR spectrum which shows no clear bands that can be assigned to water. The sharp weight loss portion on the thermogram of CuC2O4·0.3H2O corresponds to 54.4% which is very close to 55.5% expected for the loss of two molecules of CO2 and the formation of metallic copper. As shown by the TG and Df-TG graphs, there is an increase in weight that occurs around 460°C. We attribute this event to the oxidation of the metallic copper. As can be seen on Table 2 this is the process that best agrees with the observed values. This weight loss portion corresponds to the second weight loss portions of FeC2O4·xH2O (35.7%, between 242 and 330°C), CoC2O4·xH2O (39.68%, 350–436°C), NiC2O4·xH2O (41.9%, 370–434°C), and ZnC2O4·xH2O (38.9%, 385–445°C). As observed in the literature [28] some of these complexes will likely decompose in pathways which involve the decomposition of the anhydrous metal oxalate (NiC2O4 and ZnC2O4) into (NiO and ZnO, resp.) with the elimination of CO2 and CO. As for FeC2O4·2H2O and CoC2O4·2H2O this decomposition step might result in the production of a variety of products (MO, M2O3, or M3O4). The Df-TG of CoC2O4·2H2O suggests that its second weight loss proceeds in two steps. Based on this observation and on the report made by Wu (2011) [33] we suggest that CoC2O4 undergoes both decomposition and oxidation reactions to produce CO2 and Co3O4 (3):
(3)
3
CoC
2
O
4
+
2
O
2
⟶
Co
3
O
4
+
6
CO
2
.


## 4. Conclusion

We have been able to useAverrhoa carambolajuice as source of oxalic acid for the synthesis of some divalent metal oxalates. The synthesis required no special treatment of the juice as the product was obtained by directly mixing the metal ion solution and the juice. The products were all identified as the expected metal oxalates. Both the complexes and their decomposition products were found to be nanomaterials with their crystallite size ranging from 14 to 25 nm.



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*Source: 767695-2014-09-17.xml*