Ferrometric determination of vanadium in VN1−x using visible and potentiometric equivalence point detection

1985 ◽  
Vol 322 (1) ◽  
pp. 23-25 ◽  
Author(s):  
Walter Lengauer
Keyword(s):  
Equivalence Point ◽  
Point Detection

The determination of phosphorus in organic compounds with potentiometric end-point detection

1970 ◽  
Vol 58 (1) ◽  
pp. 52-57 ◽  
Author(s):  
J. Slanina ◽  
P. C. M. Frintrop ◽  
J. F. Mansveld ◽  
B. Griepink
Keyword(s):  
Organic Compounds ◽  
End Point ◽  
End Point Detection ◽  
Point Detection

Determination of titratable acidity of wines and total acidity of vinegars by discontinuous flow analysis using photometric end-point detection

The Analyst ◽  
1991 ◽  
Vol 116 (10) ◽  
pp. 1051 ◽  
Author(s):  
Terence J. Cardwell ◽  
Robert W. Cattrall ◽  
Graeme J. Cross ◽  
Gregory R. O'Connell ◽  
John D. Petty ◽  
...  
Keyword(s):  
Flow Analysis ◽  
Titratable Acidity ◽  
Total Acidity ◽  
Discontinuous Flow ◽  
End Point ◽  
End Point Detection ◽  
Point Detection

scholarly journals Microtitrimetric determination of a drug content of pharmaceuticals containing olanzapine in non-aqueous medium

2009 ◽  
Vol 15 (2) ◽  
pp. 77-81 ◽  
Author(s):  
Kanakapura Basavaiah ◽  
Nagaraju Rajendraprasad ◽  
Basavaiah Vinay
Keyword(s):  
Standard Deviation ◽  
Aqueous Medium ◽  
Reference Method ◽  
Standard Addition ◽  
Cost Effective ◽  
Pharmaceutical Products ◽  
Relative Standard ◽  
Bulk Drug ◽  
Point Detection

Two simple, rapid, reliable and cost-effective methods based on titrimetry in non-aqueous medium are described for the determination of olanzapine in pharmaceuticals. In these methods, the drug dissolved in the glacial acetic acid was titrated with the acetous perchloric acid with visual and potentiometric end point detection, crystal violet being used as the indicator for visual titration. The methods are applicable over 1-15 mg range of olanzapine. The procedures were applied to determine olanzapine in pharmaceutical products and the results were found to be in a good agreement with those obtained by the reference method. Associated pharmaceutical materials did not interfere. The precision results, expressed by inter-day and intra-day relative standard deviation values, were satisfactory, higher than 2%. The accuracy was satisfactory as well. The methods proved to be suitable for the analysis of olanzapine in bulk drug and in tablets. The accuracy and reliability of the methods were further ascertained by recovery studies via a standard addition technique with percent recoveries in the range 97.51-103.7% with a standard deviation of less than 2%.

scholarly journals Coulometric titrations of bases in propylene carbonate and γ-butyrolactone using hydroquinone as the depolarizer and a quinhydrone indicator electrode

2000 ◽  
Vol 65 (8) ◽  
pp. 587-593 ◽  
Author(s):  
Lj.N. Jaksic ◽  
R.M. Dzudovic ◽  
R.P. Mihajlovic ◽  
Z.D. Stanic
Keyword(s):  
Propylene Carbonate ◽  
Platinum Electrode ◽  
Indicator Electrode ◽  
Hydrogen Ions ◽  
Organic Bases ◽  
Oxidation Potentials ◽  
End Point Detection ◽  
Point Detection ◽  
Current Potential

The application of hydroquinone for the coulometric generation of hydrogen ions in propylene carbonate (PC) and ?-butyrolactone (GBL) is described. The current-potential curves recorded for this depolarizer, titrated bases, indicator and the solvents used showed that the investigated depolarizer is oxidized at lower potentials than the oxidation potentials of other components in the solution. The hydrogen ions generated by the oxidation of hydroquinone were used for the titration of organic bases (triethylamine, n-butylamine, pyridine, quinoline, aniline, N,N'-diphenylguanidine, piperidine, and 2,2?-bi?pyridine) in PC and GBL with with visual (Crystal Violet as indicator) and potentiometric end-point detection using a quinhydrone electrode as the indicator electrode. The quinhydrone added to the to be analyzed solution served both as a source of hydrogen ions and, together with the immersed platinum electrode, as a quinhydrone electrode. The relative error of the determination of the bases was about 1%.

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