A new spectrophotometric method for the determination of ferrous iron in the presence of ferric iron

2007 ◽  
Vol 44 (3) ◽  
pp. 171-181 ◽  
Author(s):  
Leandro Herrera ◽  
Pauline Ruiz ◽  
Juan C. Aguillon ◽  
Alexis Fehrmann
Keyword(s):  
Spectrophotometric Method ◽  
Ferrous Iron ◽  
Ferric Iron

A new and simple spectrophotometric method for the determination of selenium in the presence of copper and tellurium

1993 ◽  
Vol 71 (6) ◽  
pp. 834-835 ◽  
Author(s):  
Güler Somer ◽  
Nuray Kutay
Keyword(s):  
Spectrophotometric Method ◽  
Ferrous Iron ◽  
Indirect Method ◽  
Ferric Iron

Selenium in anodic slime is determined by using an indirect method. Selenite is reduced by ferrous iron, the ferric iron formed is complexed with KSCN, and the absorbance at 480 nm is measured. In this way selenium (10−3–10−2 M) can be determined in the presence of copper and tellurium without any separation.

scholarly journals Iron as a disturbing factor in the determination of phosphate by the molybdenum blue method

1954 ◽  
Vol 26 (1) ◽  
pp. 159-168
Author(s):  
Armi Kaila
Keyword(s):  
Hydrochloric Acid ◽  
Sulphuric Acid ◽  
Ferrous Iron ◽  
Ferric Iron ◽  
Stannous Chloride ◽  
Phosphorus Concentration ◽  
Colour Intensity ◽  
Molybdenum Blue ◽  
Fading Effect

The interference of ferric and ferrous iron in the determination of phosphate by the molybdenum blue method has been studied. It was found that the presence of ferric iron in the solutions could cause either an increase or a decrease in the colour intensity depending on the amount of stannous chloride applied and on the acid and molybdate concentrations in the reagent. Also the phosphorus concentration exerted its effect upon the course of the errors. If the original modification of Truog and Meyer was employed, generally, the most convenient way for the elimination of the interference of ferric iron was to dilute the solution. An increase in the amount of stannous chloride largely helped to prevent the fading effect of ferric iron, provided the phosphorus concentration was not lower than 0.25 ppm. When the effect of ferric iron upon the development of molybdenum blue at various concentrations of sulphuric acid and ammonium molybdate was studied, the observation was made that at each acidity there could be found a concentration of molybdate in which the effect of even fairly high amounts of ferric iron was almost negligible. In lower molybdate concentrations the presence of ferric iron caused an increase in the colour intensity, in higher molybdate concentrations the fading effect of ferric iron was marked. This most suitable level of the molybdate concentration depended to a certain degree on the phosphorus concentration of the solution and on the amount of stannous chloride applied. Fairly good results could be obtained, if the ratio of molybdate (expressed as mg/ml) to acid (expressed as normality) in the solution to be reduced was five times as high as the acidity of the solution to be reduced (expressed as its normality), e.g. 4 in 0.8 N acid, 3.5 in 0.7 N acid, 3 in 0.6 N acid etc. Although it seemed to be fairly possible to avoid the interference of ferric iron by a proper choice of the concentrations of acid and molybdate and of the amount of stannous chloride applied, the fading effect of ferrous iron could not be prevented, if only sulphuric acid was used in the reagents. But the substitution of sulphuric acid by hydrochloric acid totally prevented the fading effect of ferrous iron. On the contrary, a slight increase in the colour intensity was demonstrated. This was true also when only one half of the acid present was hydrochloric acid. It was found that this mixture of sulphuric acid and hydrochloric acid in the molybdate reagent offers an available way for the elimination of the disturbing effect of iron.

A new spectrophotometric method for the determination of total and ferric iron in rain water at the ppb level

2001 ◽  
Vol 369 (6) ◽  
pp. 530-534 ◽  
Author(s):  
K. S. Patel ◽  
A. Shukla ◽  
A. Goswami ◽  
S. K. Chandavanshi ◽  
P. Hoffmann
Keyword(s):  
Spectrophotometric Method ◽  
Ferric Iron ◽  
Rain Water

scholarly journals Spectrophotometric method for the determination of ferric iron with acetylacetone

1959 ◽  
Vol 8 (11) ◽  
pp. 710-714 ◽  
Author(s):  
Tsunenobu SHIGEMATSU ◽  
Masayuki TABUSHI
Keyword(s):  
Spectrophotometric Method ◽  
Ferric Iron

Centrifugal Analyzer Determination of Ascorbate in Serum or Urine with Fe3+/Ferrozine

1975 ◽  
Vol 21 (10) ◽  
pp. 1493-1497 ◽  
Author(s):  
William C Butts ◽  
Harold J Mulvihill
Keyword(s):  
Ferrous Iron ◽  
Ferric Iron ◽  
Population Studies ◽  
Physiological Factors ◽  
Specific Data ◽  
Automated Method ◽  
The Stability ◽  
Serum And Urine

Abstract Measurement of serum ascorbate may be useful in long-term population studies because of the possible influence of ascorbate on numerous physiological factors. We describe an automated method for determining ascorbate in serum and urine by using the reduction of ferric iron by ascorbate and the formation of a color between the resulting ferrous iron and Ferrozine [3-(2-pyridyl)-5,6-bis(4-phenylsulfonic acid)-1,2,4-triazine]. A centrifugal analyzer is used to rapidly and simultaneously measure ascorbate in the samples and standards and minimize interference from slower reacting substances in the sample. The method is highly precise and specific. Data are also presented on the stability of ascorbate in serum, urine, and aqueous solutions.

Reductive Action of Activated Carbon on Ferric Iron Interferes on the Determination of the Oxidative Activity of Acidithiobacillus Ferrooxidans on Ferrous Iron

2009 ◽  
Vol 71-73 ◽  
pp. 291-294
Author(s):  
T. Vargas ◽  
P. Diáz ◽  
B. Escobar
Keyword(s):  
Activated Carbon ◽  
Acidithiobacillus Ferrooxidans ◽  
Ferrous Iron ◽  
Bacterial Population ◽  
Ferric Iron ◽  
Ferrous Ion ◽  
Ferric Ion ◽  
Bacterial Oxidation ◽  
Chemical Action

Ferrous iron oxidation studies in the presence of activated carbon were conducted at 30 °C in basal medium at pH 1.6 with a pure strain of Acidithiobacillus ferrooxidans. Two-chamber modified shake flasks were used in these experiments, which prevented direct contact between the microorganisms and the carbon contained in the flasks. This design permitted an accurate determination of bacterial population during the experiment and enabled the involvement of ferric iron reduction with carbon to be evidenced. Notably, iron was initially added as ferric iron in a concentration of 3 g/L. It could be observed that bacteria could grow in this condition evidencing that bacteria was in fact oxidizing ferrous ion produced from reduction of ferric by carbon. From complementary experiments in which activated carbon was contacted with abiotic solutions containing ferric ion in the concentration range 0.1 – 1.2 g/l, the chemical reductive action of carbon of ferric iron was confirmed and a kinetic expression for this reaction was determined. A mathematical model was developed which incorporated expressions for the kinetic of bacterial oxidation of ferrous ion and the chemical reduction of ferric ion. This model enabled the prediction of the rate of bacterial growth and ferrous ion oxidation in a bioreactor as a function of the initial concentrations of iron, activated carbon and bacterial population. Results in this work imply that the observed variations in activity observed by other authors during bacterial oxidation of ferrous iron with A. ferrooxidans adsorbed on carbon can be in fact related to bacterial utilization of supplementary ferrous iron produced by the chemical action of carbon, phenomenon which is not explicitly accounted for.

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