Cezar Augusto
Bizzi
a,
Érico
Marlon de Moraes Flores
a,
Rochele
Sogari Picoloto
a,
Juliano
Smanioto Barin
b and
Joaquim
Araújo Nóbrega
*cd
aDepartamento de Química, Universidade Federal de Santa Maria, Instituto Nacional de Ciência e Tecnologia de Bioanalítica, 97105-900, Santa Maria, RS, BrazilCampinas, SP, Brazil
bDepartamento de Tecnologia e Ciência dos Alimentos, Universidade Federal de Santa Maria, 97105-900Santa Maria, RS, Brazil
cDepartamento de Química, Universidade Federal de São Carlos, 13565-905, São Carlos, SP, Brazil
dInstituto Nacional de Ciências e Tecnologias Analíticas Avançadas, Campinas, SP, Brazil. E-mail: djan@terra.com.br; Fax: +55-16-3351-8088; Tel: +55-16-3351-8088
First published on 7th April 2010
The efficiency of diluted nitric acid solutions under oxygen pressure for decomposition of bovine liver was evaluated using microwave-assisted wet digestion. Calcium, Cu, Fe, Mg, Mn and Zn were determined by inductively coupled plasma optical emission spectrometry (ICP OES). Efficiency was evaluated by determining the residual carbon content (RCC) by ICP OES and residual acidity in digests. Samples (up to 500 mg) were digested using nitric acid solutions (0.1, 0.5, 1, 2, 3, 7, and 14 mol L−1 HNO3) and the effect of oxygen pressure was evaluated using pressures of 0.5, 1, 1.5 and 2 MPa. It was demonstrated that 2 and 0.5 mol L−1 nitric acid solutions may be used for efficient digestion of 500 and 100 mg of bovine liver, respectively, with oxygen pressures ranging from 0.5 to 2 MPa. Using these conditions, less than 0.86 and 0.21 mL of concentrated nitric acid were necessary to digest 500 and 100 mg of sample, respectively. Similar digestion efficiencies for both conditions were obtained under pressures of O2 ranging from 0.5 to 2 MPa. The residual acidities in final digests were lower than 24% when compared to the initial amount of acid used for digestion. The accuracy of the proposed procedure was evaluated using certified reference materials of bovine liver and bovine muscle. Using a solution of 2 mol L−1 with oxygen pressure of 0.5 MPa for 500 mg of sample, the agreement with certified values ranged from 96 to 105% (n = 5). Using the proposed procedure with diluted nitric acid it was possible to obtain RCC values lower than 15% that is important for minimizing the generation of laboratory residues and improving limits of detection.
The possibility of working at high pressures causes an increase of the boiling point of the reagents and this aspect has important thermodynamic and kinetic implications. For instance, the oxidant properties of nitric acid are improved at high temperatures and due to this condition the digestion of samples containing high content of organics can be carried out without addition of auxiliary reagents, such as sulfuric or perchloric acids.1 The use of concentrated acids may be necessary when looking for drastic reaction conditions. However, the use of concentrated reagents is hazardous, requires dilution of the digests before analytes determination, and generates high volumes of concentrated acids as effluents.7,8
Performing reactions at high pressure and temperature may allow a reduction of the acid concentration without decreasing the efficiency of digestion. This hypothesis has been investigated in recent studies and the feasibility of using diluted solutions containing as low as 2 mol L−1 of nitric acid has been evaluated.9–12 It was experimentally demonstrated that the efficiency of using diluted acids for digestion derived from the temperature gradient inside the reaction vessel during the initial steps of sample digestion and due to the presence of oxygen in the closed-vessel atmosphere. The former aspect is related to the non-absorption of microwave radiation by the gas phase and the latter one implies that oxygen in gas phase can improve the oxidation processes. The combination of both aspects results in that reaction products can be oxidized also at the upper atmosphere of the reaction vessel and further reabsorbed in the liquid phase. The temperature gradient causes a less pronounced pressure increment in the initial digestion steps and consequently this avoids a too fast increase of temperature of the liquid phase. Again, it implies that the absorption of formed gaseous products will be more effective during these steps. It was experimentally demonstrated that the simultaneous occurrence of these processes led to a regeneration of nitric acid according to the following reactions:12
(CH2)n + HNO3(aq) → CO2(g) + NO(g) + H2O(l) | (Eq. 1) |
2 NO(g) + O2(g) → 2 NO2(g) | (Eq. 2) |
2 NO2(g) + H2O(l) → HNO3(aq) + HNO2(aq) | (Eq. 3) |
2 HNO2(aq) → H2O(aq) + NO2(g) + NO(g) | (Eq. 4) |
The occurrence of processes described in eqn (1–4) allows the regeneration of nitric acid and the reaction cycle remains effective when two conditions are simultaneously obeyed:13i) there are organic compounds in the sample being decomposed and generating NO (eqn (1)), and ii) there is oxygen in the gas phase to increase NO2 regeneration (eqn (2)). In a subsequent step, water reacts with NO2 generating HNO3 and HNO2 (eqn (3)). Furthermore, HNO2 decomposes to NO2 and NO which follows the sequence described by eqn (2) in the gaseous phase. This means that the availability of oxygen as a reagent causes an important effect on the efficiency of digestion process.
Based on these processes, it can be supposed that the pressurization of the digestion vessel with oxygen could improve the efficiency of digestion when using diluted nitric acid as reagent. This hypothesis was systematically investigated in the present work. In addition, the reduction as much as possible of the amount of nitric acid needed for the digestion process, in order to minimize the blank values, and also the decrease of the consumption of reagents and generation of laboratory residues was tried.
Analytes were determined by ICP OES using an axial view configuration spectrometer (Spectro Ciros CCD, Spectro Analytical Instruments, Kleve, Germany). Nebulization was performed through a cross-flow nebulizer coupled to a Scott double path type nebulization chamber. Plasma operating conditions and selected wavelengths used for analytes determination are listed in Table 1, and they were used as recommended by the instrument manufacturer.14 For the determination of residual carbon content (RCC),15 digested solutions were sonicated with a ultrasonic probe16 (VCX 130 PB, 130 W, 20 kHz, Sonics and Materials Inc., Newton, CT, USA) before the determination by ICP OES in order to remove the volatile carbon compounds.17 Argon 99.996% (White Martins-Praxair, São Paulo, SP, Brazil) was used in ICP OES determinations for plasma generation, nebulization and also as auxiliary gas.
Parameter | ICP OES |
---|---|
Radio-frequency power (W) | 1600 |
Plasma gas flow rate (L min−1) | 14.0 |
Auxiliary gas flow rate (L min−1) | 1.0 |
Nebulizer gas flow rate (L min−1) | 0.85 |
Spray chamber | double path, Scott type |
Nebulizer | crossflow |
Observation view | axial |
Emission line (nm) | |
C (I) | 193.091 |
Ca (II) | 393.366 |
Cu (I) | 324.752 |
Fe (I) | 238.204 |
Mg (I) | 285.213 |
Mn (II) | 257.610 |
Zn (I) | 213.857 |
Results for residual acidity were obtained using a titration system (Titrando 836, Metrohm, Herisau, Switzerland) equipped with a magnetic stirrer (module 803 Ti Stand), 20 mL burette (Dosino 800) and pH electrode (LL Electrode plus, model 6.0262.100).
Distilled-deionized water (Milli-Q, 18.2 MΩ cm, Millipore. Bedford, MA, USA) and analytical-grade nitric acid (Merck, Darmstadt, Germany) were used to prepare samples and standards. Reference solutions containing 25 to 500 mg L−1 of C were prepared by dissolution of citric acid for RCC determinations (Merck) in water. A 0.1 mol L−1 of KOH (Merck) solution was used to residual acidity determination. Glass and quartz material were soaked in 1.4 mol L−1 HNO3 for 24 h and thoroughly washed with water before use.
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Fig. 1 Effect of nitric acid concentration on digestion of 500 mg of sample mass; effectiveness of organic matter digestion performed under oxygen pressure (gray bars) and without oxygen pressure (white bars). Lines represent the residual acidity obtained from digestion performed under oxygen pressure (-■-) and without oxygen pressure (-△-). |
When using 2 MPa of oxygen and concentrated nitric acid or 7 mol L−1 (500 mg of sample), no significant difference was observed in RCC values when compared with results without using O2. In this case, the presence of O2 has no detectable effect and these results may be explained by the high oxidant environment even without O2. However, a more effective digestion was obtained with 2 MPa oxygen pressure and nitric acid solutions containing 2 and 3 mol L−1 (RCC = 13.8 and 11.7, respectively) could be used resulting in a colourless digests. Therefore, it was possible to reduce the nitric acid concentration about 3.5 times but still obtaining a similar digestion efficiency (2 mol L−1 HNO3, RCC = 13.8%). The effect of O2 was less pronounced when using lower HNO3 concentrations and this effect may be explained by the low oxidation power of a solution containing 1 mol L−1 HNO3 even associated with 2 MPa oxygen. Similar behaviour was observed when working with 100 mg of sample. However, for 100 mg of sample, even a nitric acid solution as diluted as 0.5 mol L−1 led to RCC values (7.5%) similar to those obtained using more concentrated nitric acid solutions but without oxygen pressure.
As reported in previous studies,9,10,12 the oxidant action of nitric acid may be improved if a regenerating process occurs, which is mainly dependent on the amount of oxygen available in gas phase during the oxidation of the organic matter. This reaction could be effective with diluted nitric acid if digestion vessels were pressurized with oxygen. This hypothesis was reinforced by the results obtained for residual acidity shown in Fig. 1. It may be seem that residual acidity in the same reaction conditions was higher with oxygen pressure and may be explained due to a regeneration process. In addition, after digestion it was possible to observe final digests with colourless fumes inside the reaction vessel when digestion was performed under oxygen pressure. This may be due to the absence of NO2 in the gas phase, probably owing to the regeneration process of nitric acid promoted by oxygen. The opposite behaviour was observed in final digests obtained from experiments performed without oxygen pressure, where brown fumes of NO2 were observed inside the reaction vessels.
In order to confirm if this process was related to oxygen or it was only caused by a pressure effect, digestion was performed with diluted nitric acid under an inert gas pressure. In this way, a mass of 500 mg of bovine liver was digested under 2 MPa of argon using a 2 mol L−1 HNO3 solution. It was possible to observe a yellowish colour in digests with solid residues remaining as suspended particles (RCC values were higher than 45%). These values are higher than those obtained when using the same pressure but with oxygen (colourless digests without solids in suspension, RCC = 13.8%) which confirms the effect of oxygen on digestion efficiency.
As it can be seen in Fig. 2, using sample masses of 500 mg the efficiency of digestion was not too dependent on the oxygen pressure from 0.5 to 2 MPa (for 2 or 7 mol L−1 HNO3). Using a solution of 2 mol L−1 HNO3 (Fig. 2, white bars) a suitable efficiency of digestion (RCC < 15%) was observed only when adding oxygen at pressures of 0.5, 1, 1.5, and 2 MPa. Without oxygen pressurization, the RCC of final digests was higher than 40% and solution presented a yellow aspect with solid residues. Digestions performed with 100 mg of sample presented a similar behaviour. During digestion using a solution of 0.5 mol L−1 HNO3 values of RCC were below 14% when digestion vessel was pressurized with oxygen (RCC = 12.8, 12.6, 13.8 and 7.5% for pressures of 0.5, 1, 1.5 and 2 MPa of oxygen, respectively). However, when this experiment was performed without adding oxygen the digestion presented a poor efficiency, resulting in yellowish colour solutions with solid residues and RCC higher than 32%.
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Fig. 2 Effect of oxygen pressure on digestion of 500 mg of bovine liver. Digestions performed using 7 mol L−1 HNO3 (gray bars) or 2 mol L−1 HNO3 (white bars). Lines represent the residual acidity obtained from digestion performed with 7 mol L−1 HNO3 (-■-) and 2 mol L−1 HNO3 (-△-). |
The residual acidity after digestion carried out under different oxygen pressures was also determined when the digestion was performed with 7 mol L−1 HNO3 for sample mass of 500 mg. It was possible to observe a decrease in acidity correspondent to the decrease of HNO3 concentration (Fig. 2). The residual acidity was lower than 24% when using 2 mol L−1 HNO3 under oxygen pressure ranging from 0 to 2 MPa. However, without oxygen pressure the digestion efficiency was lower and a yellowish final solution was observed. During digestions with sample masses of 100 mg, a decrease in residual acidity was observed only with lower concentrations of nitric acid. Using a solution of 7 mol L−1 HNO3, values of residual acidity were higher than 93% for both conditions of pressure (residual acidity of 93.3, 98, 98.9, 97 and 97.4% from digestions under pressures of 0, 0.5, 1, 1.5 and 2 MPa). Using a solution of 2 mol L−1 HNO3 for digestion under 2 MPa O2, the residual acidity was higher than 90%. However, for oxygen pressure of 0.5, 1 and 1.5 MPa, values of residual acidity were lower than 43%. In spite of a relatively low residual acidity obtained for digestion without oxygen (20.8%) the digestion efficiency was only 35% and a yellowish final solution was observed. Therefore, in the range of oxygen pressure evaluated in this work, no significant changes were observed and 0.5 MPa was selected for subsequent experiments.
Analyte | SRM NIST 1577a | SRM NIST 8414b | ||
---|---|---|---|---|
certified | found | certified | found | |
a Bovine liver. b Bovine muscle. | ||||
Ca | 124 ± 6 | 129 ± 6 | 145 ± 20 | 143 ± 8 |
Cu | 193 ± 10 | 185 ± 2 | 2.84 ± 0.45 | 2.75 ± 0.11 |
Fe | 268 ± 8 | 260 ± 7 | 71.2 ± 9.2 | 70.8 ± 1.8 |
Mg | 604 ± 9 | 592 ± 3 | 960 ± 95 | 944 ± 23 |
Mn | 10.3 ± 1.0 | 9.90 ± 0.52 | 0.37 ± 0.09 | 0.377 ± 0.013 |
Zn | 130 ± 13 | 137 ± 2 | 142 ± 14 | 139 ± 1 |
This journal is © The Royal Society of Chemistry 2010 |