Indirect Electrochemical Determination of Chlorpropamide Through Its Interaction with Valsartan Using Square Wave Voltammetry

2021 ◽  
pp. 6541-6544
Author(s):  
Amer Th. Al-Taee ◽  
Aws Z. Al-Hafidh
Keyword(s):  
Limit Of Detection ◽  
Silver Chloride ◽  
Detection System ◽  
Reference Electrode ◽  
Electrochemical Determination ◽  
Square Wave ◽  
The Stability ◽  
Silver Silver ◽  
Silver Silver Chloride

A square wave voltammetric technique coupled with three electrode detection system consist of hanging mercury drop electrode (HMDE) as working electrode, 1mm platinum wire as an auxiliary electrode (Pt-wire) and silver/silver chloride saturated potassium chloride (Ag/AgCl.sat.KCl) as reference electrode was used to determine the chlorpropamide indirectly through its interaction with valsartan, chlorpropamide gives no reduction peaks in the studied range. The effect of pH and the stability of the measurement were examined calibrations curve of chlorpropamide was constructed and the relation between current and concentration of chlorpropamide was linear with R2 value = 0.9944. The limit of detection for chlorpropamide was 4.89 x 10-9 M through its interaction with valsartan.

ELECTRODE POTENTIALS OF THORIUM TETRACHLORIDE IN ALKALI CHLORIDE MELTS

1964 ◽  
Vol 42 (6) ◽  
pp. 1315-1322 ◽  
Author(s):  
R. Srinivasan ◽  
S. N. Flengas
Keyword(s):  
Silver Chloride ◽  
Gravimetric Method ◽  
Reference Electrode ◽  
The Other ◽  
Alkali Chloride ◽  
Electrode Potentials ◽  
Silver Chloride Reference Electrode ◽  
Chloride Melts ◽  
Silver Silver ◽  
Silver Silver Chloride

The electrode potentials of the system Th, ThCl4 (KCl, NaCl) were measured at various concentrations of thorium chloride, and at temperatures between 670 °C and 850 °C, using a silver – silver chloride reference electrode. It was shown by a direct gravimetric method that the reaction,Th(metal) + ThCl4(melt) = 2ThCl2(in melt),postulated by previous investigators, did not take place.The activity coefficients, and the other partial molal properties of the solutions of ThCl4, in the equimolar mixture of potassium and sodium chlorides, were calculated as a function of temperature from the e.m.f. measurements.

Thermodynamics of electrolyte solutions: activity coefficients of NaCl in the NaCl–NiCl2–H2O system at 25, 35, and 45 °C

1990 ◽  
Vol 68 (2) ◽  
pp. 294-297 ◽  
Author(s):  
Ch. Venkateswarlu ◽  
J. Ananthaswamy
Keyword(s):  
Activity Coefficients ◽  
Silver Chloride ◽  
Osmotic Coefficients ◽  
Reference Electrode ◽  
Nickel Chloride ◽  
Electrolyte Solutions ◽  
Pitzer Formalism ◽  
Harned Coefficients ◽  
Silver Silver ◽  
Silver Silver Chloride

The activity coefficients of NaCl in the NaCl–NiCl2–H2O system were estimated at 25, 35, and 45 °C and total ionic strengths of 0.5, 1.0, 2.0, and 3.0 m by an EMF method using a Na-ion selective electrode and a silver–silver chloride reference electrode. The Harned coefficients were calculated at all the temperatures studied. At 25 °C the data were analysed using the Pitzer formalism. The osmotic coefficients and the excess free energies of mixing were also calculated at 25 °C. Keywords: activity coefficients, sodium chloride, nickel chloride, Pitzer equations, thermodynamics.

The preparation in situ of a silver-silver chloride reference electrode

1994 ◽  
Vol 6 (11-12) ◽  
pp. 945-952 ◽  
Author(s):  
Juozas Kulys ◽  
Jens A Munk ◽  
Thomas Buch-Rasmussen ◽  
Henrik E. Hansen
Keyword(s):  
Silver Chloride ◽  
Reference Electrode ◽  
Silver Chloride Reference Electrode ◽  
Silver Silver ◽  
Silver Silver Chloride

VOLTAIC CELLS IN FUSED SALTS: PART II. THE SYSTEMS: (a) SILVER – SILVER CHLORIDE, LEAD – LEAD CHLORIDE; (b) SILVER – SILVER CHLORIDE, ZINC – ZINC CHLORIDE; AND (c) SILVER – SILVER CHLORIDE, NICKEL – NICKELOUS CHLORIDE

1957 ◽  
Vol 35 (11) ◽  
pp. 1254-1259 ◽  
Author(s):  
S. N. Flengas ◽  
T. R. Ingraham
Keyword(s):  
Zinc Chloride ◽  
Dissociation Constants ◽  
Silver Chloride ◽  
Reference Electrode ◽  
Lead Chloride ◽  
Effect Of Temperature ◽  
Fused Salts ◽  
Electrode Potentials ◽  
Silver Silver ◽  
Silver Silver Chloride

Using a reversible silver – silver chloride reference electrode, described in the first paper of this series, standard electrode potentials have been established for the systems lead – lead chloride, zinc – zinc chloride, and nickel – nickelous chloride, in melts containing equimolar quantities of KCl and NaCl. Deviations from ideality were observed, and these were attributed to the formation of complexes. Dissociation constants for the complexes were calculated. The effect of temperature on the electromotive forces of the voltaic cells was also measured, and the heats of the cell reactions were calculated from the data.

Collaborative Study on a Potentiometric Titration of Soluble Chlorides in Feeds

1969 ◽  
Vol 52 (3) ◽  
pp. 607-609
Author(s):  
D L Sharpe
Keyword(s):  
Nitric Acid ◽  
Silver Chloride ◽  
Collaborative Study ◽  
Reference Electrode ◽  
Arithmetic Mean ◽  
Official Method ◽  
Silver Chloride Reference Electrode ◽  
Coefficients Of Variations ◽  
Silver Silver ◽  
Silver Silver Chloride

Abstract In the method described, a weighed feed sample is placed in 200 ml water, 1 ml nitric acid is added, and the chlorides present are titrated with silver nitrate. The titration is performed with a potentiometer equipped with a silver-silver chloride reference electrode a nd a silver indicating electrode. Collaborative s tudy showed that the method is more precise than the official method. An arithmetic mean for the coefficients of variations was 8.0 and 4.1, respectively, for the official and the potentiometric method.

Electrochemical sensor for continuous transcutaneous PCO2 measurement

1976 ◽  
Vol 41 (3) ◽  
pp. 442-447 ◽  
Author(s):  
A. V. Beran ◽  
R. F. Huxtable ◽  
D. R. Sperling
Keyword(s):  
Silver Chloride ◽  
Reference Electrode ◽  
Antimony Oxide ◽  
Oxidation Reduction ◽  
Oxidation Reduction Potential ◽  
Teflon Membrane ◽  
Human Volunteers ◽  
Pco2 Measurement ◽  
Silver Silver ◽  
Silver Silver Chloride

A sensor suitable for continuous transcutaneous PCO2 measurements is described. The sensor consists of an antimony-antimony oxide electrode in combination with a silver-silver chloride reference electrode, bathed in an electrolyte and covered by a Teflon membrane. A servo-controlled heater unit was used to maintain the sensor's temperature and to produce local hyperemia. The resulting oxidation-reduction potential under constant temperature isa linear function of the logarithm PCO2. Response time (95%) to stepchanges in PCO2 from 27 to 70 mmHg was 2.7 +/- 0.3 min. Following a 12-h “aging”time, the electrode exhibited a minimal drift of 5.2 +/-2.2 mV for 16 h, representing an average PCO2 drift of 0.5 mmHg/h. This sensor was applied onthree rabbits and on five human volunteers, and found satisfactory under normal physiological conditions.

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