Polarographic Determination of Parabanic Acid.

Struck, William A.; Elving, Philip J.

doi:10.1021/ac60213a055

Cited by 7 publications

(6 citation statements)

References 9 publications

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“…pH 4.6 (Table I; Figure 4). As the electrolysis proceeds, wave I, while unmistakably clear, shows some irregularities, very likely owing to the low product concentration and the high buffer phosphate concentration (Struck and Elving, 1964a); however, it is fairly well defined by the end of the electrolysis. The material accounting for wave I was identified polarographically as parabanic acid by comparing the two in acetate medium where well-defined waves are obtained, e.g., identity of both and wave slope (Table II).…”

Section: Resultsmentioning

confidence: 99%

Electrolytic Oxidation of Uric Acid: Products and Mechanism^*

Struck¹,

Elving²

1965

Biochemistry

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Section: Resultsmentioning

confidence: 99%

Electrolytic Oxidation of Uric Acid: Products and Mechanism^*

Struck¹,

Elving²

1965

Biochemistry

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“…The cathodic peak (peak IIc) observed for both guanine and uric acid is probably due to reduction of a product of partial further oxidation of III, namely, parabanic acid (V, Fig. 3) (25). Authentic parabanic acid shows a similar pH dependence to peak IIc although the peak potential for its reduction generally occurred at somewhat more negative potential.…”

Section: Mechanismmentioning

confidence: 92%

“…Manuscript submitted Nov. 25,1969; revised manuscript received May 20, 1970. Any discussion of this paper will appear in a Discussion Section to be published in the June 1971 JOURNAL.…”

mentioning

confidence: 99%

Electrochemical Oxidation of Guanine at the Pyrolytic Graphite Electrode

Dryhurst¹,

Pace

1970

J. Electrochem. Soc.

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The electrochemical oxidation of guanine at the pyrolytic graphite electrode was investigated by linear and cyclic scan voltammetry between pH 0–12.5 and by controlled electrode potential electrolysis in aqueous 1M acetic acid solution. Guanine is oxidized by an initial 2normale/2H+ potential determining attack at the −Nfalse(7false)=Cfalse(8false)− double bond followed by a further 2normale/2H+ oxidation of the −Cfalse(4false)‒Cfalse(5false)− double bond to give 2‐amino‐6,8‐dioxypurine ‐4,5‐diol which, being unstable, undergoes further reaction by two routes: (a) further electrochemical oxidation to parabanic acid, guanidine, and carbon dioxide; and (b) hydrolysis to oxalyl guanidine and carbon dioxide. The exact nature of intermediate species in the electro‐oxidation of guanine and uric acid were more thoroughly established by extensive use of fast sweep cyclic voltammetry. In particular it appears that in ammonia buffers at moderately high pH, the intermediate is a 4,5‐diamine rather than a 4,5‐diol.

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“…Indeed, Dryhurst has clearly shown that such latter decomposition follows a minority path which increases in yield with acidity of the media. 24,29 Moreover, the yield of this secondary path strongly depends on the electrode material as reported by Struck et al 30 who detected parabanic acid reduction using polarography following UA oxidation at a spectroscopic graphite electrode in place of pyrolitic graphite. In such a way, according to the local pH decrease at the vicinity of the electrode owing to UA oxidation and to the acidic comportment and the nature of hydrogenated diamond electrodes, parabanic acid may be produced with a yield of around 6% (obtained from ratio of the plateau limiting currents that involve both two electrons and two protons).…”

Section: ■ Results and Discussionmentioning

confidence: 88%

Quasi-Real Time Quantification of Uric Acid in Urine Using Boron Doped Diamond Microelectrode with in Situ Cleaning

et al. 2012

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We report herein an innovative electrochemical (EC) technique based on boron doped diamond (BDD) microelectrodes which enable the fast determination of uric acid (UA) concentrations in urine. On the basis of fast cyclic voltammetry (CV), the technique was assessed in human urine samples and compared successfully using routine spectrophotometric diagnosis. The approach relies on the use of BDD's superior properties such as low background current, low adsorption of species, long-term stability, and antifouling capabilities using electrochemical reactivation. Moreover, the article also describes an in situ activation technique, where the electrodes were reactivated within human urine, thereby opening the way toward automatic quantification of UA with in situ cleaning. The time taken to quantify UA concentration and cleaning remains below 0.5 s. Two analytic models were derived, based on different concentrations of ascorbic acid (AA) and uric acid, consisting of 2 s order calibration curves. Solving the second order equation enables the direct estimation of UA concentration, and values demonstrated good accuracy when compared with spectrophotometric measurements.

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Polarographic Determination of Parabanic Acid.

Cited by 7 publications

References 9 publications

Electrolytic Oxidation of Uric Acid: Products and Mechanism^*

Electrolytic Oxidation of Uric Acid: Products and Mechanism^*

Electrochemical Oxidation of Guanine at the Pyrolytic Graphite Electrode

Quasi-Real Time Quantification of Uric Acid in Urine Using Boron Doped Diamond Microelectrode with in Situ Cleaning

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Polarographic Determination of Parabanic Acid.

Cited by 7 publications

References 9 publications

Electrolytic Oxidation of Uric Acid: Products and Mechanism*

Electrolytic Oxidation of Uric Acid: Products and Mechanism*

Electrochemical Oxidation of Guanine at the Pyrolytic Graphite Electrode

Quasi-Real Time Quantification of Uric Acid in Urine Using Boron Doped Diamond Microelectrode with in Situ Cleaning

Contact Info

Product

Resources

About

Electrolytic Oxidation of Uric Acid: Products and Mechanism^*

Electrolytic Oxidation of Uric Acid: Products and Mechanism^*