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On the Inhibition of the Reaction Between Anodic Aluminum Oxide and Water

On the Inhibition of the Reaction Between Anodic Aluminum Oxide and Water 1980 Gordon and Breach Science Publishers, Inc. Printed in Great Britain ON THE INHIBITION OF THE REACTION BETWEEN ANODIC ALUMINUM OXIDE AND WATER J. M. SANZ, J. M. ALBELLA and J. M. MARTNEZ-DUART Departmento de Fisica Aplicada & Instituto de Fisica del Estado S61ido (CS.I. C ), Universidad Auton6ma de Madrid, Cantoblanco (Madrid), Spain (Received November 1, 1978; in final form April 11, 1979) The reaction between anodic aluminum oxide and several passivating solutions of citric acid and ammonium dihydrogen phosphate (ADP) is studied by capacitance measurements. In addition, the passivating effect of the above solutions has been evaluated by the reaction of the oxide with pure boiling water and subsequent anodizafion. The results show a strong passivating effect of the ADP solution which is partially diminished by the addition of citrate ions. INTRODUCTION The reaction between anodic aluminum oxide and water has been widely studied by Hunter et al., Bernard and Randall 2 and Vermilyea and Vedder. 3 It has been suggested from these investigations that the mechanism of this reaction should be very similar to that between aluminum and water since the kinetics of growth of the hydroxide is similar in both cases. Vedder and Vermilyea4 have proposed the following steps for the reaction between aluminum and water: (i) formation of an amorphous oxide, (ii) solution of the oxide, and (iii) precipitation of the aluminum hydroxide. Therefore, in the reaction between aluminum oxide and water it should be expected that only steps (ii) and (iii) will occur. Vermilyea and Vedder 3 have also studied several factors, such as kind of electrolyte, its pH, etc., which influence the reaction between aluminum oxide and water. They have found that the presence of POa4 ions, even in small concentrations, strongly inhibits the attack of the oxide by the water (step ii). This fact is attributed to the formation of a complex of phosphorus and aluminum, known as variscite, nonsoluble in water and strongly bound to the aluminum surface. In this paper some of the aspects of the inhibition caused by NH4 H2 PO4 in the reaction between anodic aluminum oxide and boiling water are examined. The 3incorporation of the PO ions on the aluminum surface has been carried out by immersing the oxidized aluminum foil in an aqueous solution of the monobasic phosphate at a temperature of 90 C. The rate of the reaction has been studied for different phosphate concentrations and also for varying amounts of citric acid added to a solution of a given phosphate concentration. The significance of the reaction between aluminum oxide and water in the presence of phosphate ions is considerable since it is well known that during the manufacture of electrolytic capacitors it is a usual practice to soak the oxidized aluminum foil in aa hot aqueous solution containing PO4 ions in order to increase the oxide’s stability, s’6 EXPERIMENTAL The aluminum foil employed in this work has been of the type used in the manufacture of the anodes of electrolytic capacitors, with a purity of 99.99%. The foil was supplied electrochemically etched, with a surface gain of about 16. Samples of 3 x 3 cm2 were cut and anodized at a constant current of 30 mA cm -: (projected area). After reaching 400 V the samples were left in the electrolytic cell until the current diminished to 1/100 of its initial value. The anodization was carried out at 90C in an aqueous solution of boric acid and ammonium pentaborate with a resistivity of 1200 ohm cm. In order to increase the rate of the voltage rise during the anodization, the aluminum foil was previously immersed in boiling deionized water (p > Mohm.cm) for five minutes. By this procedure the increase of voltage with time is approximately linear 7 with a rate of about 50 V min-1 in this case. After the first anodization, the samples were hydrated and oxidized again following exactly the same procedure. In this J. M. SANZ, J. M. ALBELLA AND J. M. MARTfNEZ-DUART way the oxide is more stable resulting in a more reproducible capacitance measurement. Previous to the study of the reaction between aluminum oxide and water, the anodized samples were soaked for five minutes in an aqueous solution of several concentrations of NH4 H2 PO4 at 90 C and also, in some cases, in a 2% solution of this electrolyte containing different amounts of citric acid. It has been verified in our laboratory that a five-minute immersion is enough to get the surface of the foil saturated with the phosphate complex, except in the case of the lowest concentration investigated (0.002%). After this treatment, the samples were made to react with deionized boiling water for about one hour. After each of the above steps of oxidations and hydrations, the capacitance and dielectric losses of the samples were measured at 100 Hz by a HewlettPackard 4261A bridge in an electrolyte of boric acid (5%) and ammonium hydroxide with a resistivity of 100 ohm cm. Although the treatment of the oxide above room temperature produces a change in its dielectric constant accompanied by a decrease in capacitance, a Bernard and Randall 2 have shown that the value of 1/C, with the proper corrections, can be used as a measure of the thickness of the oxide. RESULTS AND DISCUSSION Figure shows the fraction of oxide attacked during the 5 min immersion in the hot ADP solution as a function of the pH of the solution (curve a). Since it was observed that the dielectric constant at 90C is about 95% of its value at room temperature, the capacitance measurements were corrected accordingly. From Figure it can be noted that the amount of the oxide attacked by the ADP electrolyte is relatively small until a pH of about 5 is reached. The amount then increases abruptly. The point in Figure labelled as ’water’ corresponds to the value obtained when the sample, after anodising, is treated for 5 min in pure water at 90 C. An aqueous solution of citric acid also produces a similar decrease in the oxide’s attack in relation to water (curve b), although the effect appears at lower values of pH. It can be inferred from this result that a small amount of citric acid produces a moderating effect in the reaction between aluminum and water. In this respect, it is interesting to point out that the citric acid is well known for its inhibiting capability for the formation of bohemite during hydration of aluminum. 8 The above results are in contrast with those obtained when increasing amounts of citric acid are added to a 2% solution of NH4H2 PO4 (pH 4.3). In this case the rate of attack increases as the pH decreases (curve c). Curves (a) and (c) both show the effect of the pH in the rate of attack of the electroalyte based upon PO4 ions, showing a minimum for a value of the pH in the range between 4 and 5. A similar effect has also been observed by Vermilyea and Vedder a who attribute it to the presence of hydroxide on the surface and also to the lower solubility of aluminum compounds. x o 1.0, WATER c) pH Fraction of attacked oxide during immersion in several solutions as a function of the pH of the solution. FIGURE Curve a: ammonium dihydrogen phosphate; curve 19" citric acid; curve c" citric acid added to a solution of 2% ammonium dihydrogen phosphate in water. ANODIC ALUMINUM OXIDE AND WATER WATER FIGURE 2 pH Fraction of attacked oxide during the immersion in oure boiling water (1 hour) of samples passivated by immersion in tlae solutions specified in Figure 1, as a function ot the pH or these solutions. Figure 2 shows the fraction of oxide attacked (with reference to the state of the oxide after anodising) in the 1-hour reaction with deionized boiling water for samples which had been soaked in the ammonium phosphate and citric acid electrolytes. The passivating effect of the ADP solution can be clearly appreciated from curve (a) and it may be attributed to the presence of phosphorus on the surface. 3 Auger electron spectroscopy measurements carried out in our laboratory confirm this assumption. The presence of the citrate ion in the ADP solution in increasing amounts rapidly diminishes the passivating capability of the electrolyte as can be observed from curve (c). The citrate ion by itself does not exert any passivating effect since in this case (curve b) the percentage of oxide removed is very similar to the case in which the samples are not treated or only immersed in hot water. The above results are in agreement with those obtained from the reoxidation curves of the samples after having reacted with the boiling water. Figure 3 shows for some of the samples the variation of the voltage during the reoxidation at a constant current (8 mA cm -2 ) and in the same electrolyte of the first anodization. It can be observed that the rate of voltage increase is much faster for the samples treated in a 2% ADP solution (curve A) than for those treated in the same salt at a lower concentration (curve D), as well as for those soaked in an aqueous solution of citric acid (curves E and F) or simply in pure water (curve G). The lower oxidation rate (zone I) that occurs in a sample treated in water, for example, can be attributed to the slow diffusion of the electrolyte across the porous structure of the hydroxide and to the filling of voids in the oxide as proposed by Alwitt and Dyer. 9 Once the electrolyte has penetrated the hydroxide and the voids become filled with new layers of oxide, the rate of anodization increases (zone II) due to the direct transformation of hydroxide into oxide or to some other currentconsuming transformation in the oxide. 7 Subsequently, the rate of anodization becomes slow again (zone III), and it may be due to the formation of new layers of oxide which had been attacked in the reaction with water. 9 This interpretation is supported by the fact that the rate of voltage increase, 25 V min -1 is not too different from the value during the first anodization of aluminum. In agreement with this interpretation, the samples treated in citric acid (curves E and F) show the formation of less quantity of hydroxide and a greater oxide attack than those that were only immersed in water. The samples treated in a low ADP concentration (0.004%, curve D) still show a lesser amount of hydroxide and a smaller attack by the electrolyte, whereas those samples soaked in a 2% ADP concentration (curve A) present a very fast voltage rise which indicates that practically no hydroxide has been formed and that the oxide has not been attacked by the electrolyte. Finally, when citric acid is added to the preceding ADP solution no hydroxide seems to be formed in the reaction with water. However, the oxide is attacked more J. M. SANZ, J. M. ALBELLA AND J. M. MARTNEZ-DUART REANODIZATION TIME (min) Zone Zone= A: ADP sotution 4.30 B:Citric acid +ADP 395 C: Citric acid+ADP 295 5.40 D: ADP 3.90 E: Citric acid 2.40 F: Citric acid Zone "r G: Water FIGURE 3 60 80 REANODIZATION TIME (sec) http://www.deepdyve.com/assets/images/DeepDyve-Logo-lg.png

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