International Journal of Analytical Chemistry

International Journal of Analytical Chemistry / 2012 / Article
Special Issue

Fundamentals and Applications of Analytical Chemistry in Natural Products

View this Special Issue

Research Article | Open Access

Volume 2012 |Article ID 981758 |

V. S. Anusuya Devi, V. Krishna Reddy, "Spectrophotometric Determination of Iron(II) and Cobalt(II) by Direct, Derivative, and Simultaneous Methods Using 2-Hydroxy-1-Naphthaldehyde-p-Hydroxybenzoichydrazone", International Journal of Analytical Chemistry, vol. 2012, Article ID 981758, 12 pages, 2012.

Spectrophotometric Determination of Iron(II) and Cobalt(II) by Direct, Derivative, and Simultaneous Methods Using 2-Hydroxy-1-Naphthaldehyde-p-Hydroxybenzoichydrazone

Academic Editor: Ricardo Vessecchi
Received05 Sep 2011
Revised24 Oct 2011
Accepted03 Nov 2011
Published27 Feb 2012


Optimized and validated spectrophotometric methods have been proposed for the determination of iron and cobalt individually and simultaneously. 2-hydroxy-1-naphthaldehyde-p-hydroxybenzoichydrazone (HNAHBH) reacts with iron(II) and cobalt(II) to form reddish-brown and yellow-coloured [Fe(II)-HNAHBH] and [Co(II)-HNAHBH] complexes, respectively. The maximum absorbance of these complexes was found at 405 nm and 425 nm, respectively. For [Fe(II)-HNAHBH], Beer’s law is obeyed over the concentration range of 0.055–1.373 μg mL−1 with a detection limit of 0.095 μg mL−1 and molar absorptivity ɛ, 5.6 × 104 L mol−1 cm−1. [Co(II)-HNAHBH] complex obeys Beer’s law in 0.118–3.534 μg mL−1 range with a detection limit of 0.04 μg mL−1 and molar absorptivity, ɛ of 2.3 × 104 L mol−1 cm−1. Highly sensitive and selective first-, second- and third-order derivative methods are described for the determination of iron and cobalt. A simultaneous second-order derivative spectrophotometric method is proposed for the determination of these metals. All the proposed methods are successfully employed in the analysis of various biological, water, and alloy samples for the determination of iron and cobalt content.

1. Introduction

Iron and cobalt salts are widely used in industrial materials [1, 2], paint products [3], fertilizers, feeds, and disinfectants. They are important building components in biological systems [4]. Special cobalt-chromium-molybdenum alloys are used for prosthetic parts such as hip and knee replacements [5]. Iron-cobalt alloys are used for dental prosthetics [6]. There has been growing concern about the role of iron and cobalt in biochemical and environmental systems. Normally small amounts of iron and cobalt are essential for oxygen transport and enzymatic activation, respectively, in all mammals. But excessive intake of iron causes siderosis and damage to organs [7]. A high dosage of cobalt is very toxic to plants and moderately toxic to mammals when injected intravenously. Hence, quantification of various biological samples for iron and cobalt is very important to know their influence on these systems.

A good number of reviews have been made on the use of large number of chromogenic reagents for the spectrophotometric determination of iron and cobalt. Some of the recently proposed spectrophotometric methods for the determination of iron [815] and cobalt [1622] are less sensitive and less selective. We are now proposing simple, sensitive and selective direct and derivative spectrophotometric methods for the determination of iron(II) and cobalt(II) in various complex materials using 2-hydroxy-1-naphthaldehyde-p-hydroxybenzoichydrazone as chromogenic agent. We are also reporting a highly selective second-order derivative method for the simultaneous determination of iron and cobalt in different samples.

2. Experimental

2.1. Preparation of Reagents

0.01 M iron(II) and cobalt(II) solutions were prepared by dissolving appropriate amounts of ferrous ammonium sulphate (Sd. Fine) in 2 M sulphuric acid and cobaltous nitrate (Qualigens) in 100 mL distilled water. The stock solutions were diluted appropriately as required. Other metal ion solutions were prepared from their nitrates or chlorides in distilled water. 1% solution of cetyltrimethylammonium bromide (CTAB), a cationic surfactant in distilled water is used. Buffer solutions of pH 1–10 are prepared using appropriate mixtures of 1 M HCl–1 M CH3COONa (pH 1–3.0), 0.2 M CH3COOH, 0.2 M CH3COONa (pH 3.5–7.0), and 1 M NH4OH and 1 M NH4Cl (pH 7.5–10.0). HNAHBH was prepared by mixing equal amounts of 2-hydroxy-1-naphthaldehyde in methanol and p-hydroxybenzoichydrazide in hot aqueous ethanol in equal amounts and refluxing for three hours on water bath. A reddish brown coloured solid was obtained on cooling. The product was filtered and dried. It was recrystallized from aqueous ethanol in the presence of norit. The product showed melting point 272–274°C.

The structure of the synthesized HNAHBH was determined from infrared and NMR spectral analysis.  M solution of the reagent was prepared by dissolving 0.306 g in 100 mL of dimethylformamide (DMF). Working solutions were prepared by diluting the stock solution with DMF (see Scheme 1).

2.2. Preparation of Sample Solutions
2.2.1. Soil Samples

The soil sample (5.0 g) was weighed into a 250 mL Teflon high-pressure microwave acid digestion bomb and 50 mL aquaregia were added. The bomb was sealed tightly and then positioned in the carousel of a microwave oven. The system was operated at full power for 30 minutes. The digested material was evaporated to incipient dryness. Then, 50 mL of 5% hydrochloric acid was added and heated close to boiling to leach the residue. After cooling, the residue was filtered and washed two times with a small volume of 5% hydrochloric acid. The filtrates were quantitatively collected in a 250 mL volumetric flask and diluted to the mark with distilled water.

2.2.2. Alloy Steel Sample Solution

A 0.1–0.5 g of the alloy sample was dissolved in a mixture of 2 mL HCl and 10 mL HNO3. The resulting solution was evaporated to a small volume. To this, 5 mL of 1 : 1 H2O and H2SO4 mixture was added and evaporated to dryness. The residue was dissolved in 15 mL of distilled water and filtered through Whatman filter paper no. 40. The filtrate was collected in a 100 mL volumetric flask and made upto the mark with distilled water. The solution was further diluted as required.

2.2.3. Food and Biological Samples

A wet ash method was employed in the preparation of the sample solution. 0.5 g of the sample was dissolved in a 1 : 1 mixture of nitric acid and perchloric acid. The solution was evaporated to dryness, and the residue was ashed at 300°C. The ash was dissolved in 2 mL of 1 M sulphuric acid and made up to the volume in a 25 mL standard flask with distilled water.

2.2.4. Blood and Urine Samples

Blood and urine samples of the normal adult and patient (male) were collected from Government General Hospital, Kurnool, India. 50 mL of sample was taken into 100 mL Kjeldal flask. 5 mL concentrated HNO3 was added and gently heated. When the initial brief reaction was over, the solution was removed and cooled. 1 mL con. H2SO4 and 1 mL of 70% HClO4 were added. The solution was again heated to dense white fumes, repeating HNO3 addition. The heating was continued for 30 minutes and then cooled. The contents were filtered and neutralized with dil. NH4OH in the presence of 1-2 mL of 0.01% tartrate solution. The solution was transferred into a 10 mL volumetric flask and diluted to the volume with distilled water.

2.2.5. Water Samples

Different water samples were collected from different parts of Anantapur district, A. P, India and filtered using Whatman filter paper.

2.2.6. Pharmaceutical Samples

A known quantity of the sample was taken in a beaker and dissolved in minimum volume of alcohol. Then added 3 mL of 0.01 M nitric acid and evaporated to dryness. The dried mass was again dissolved in alcohol. This was filtered through Whatman filter paper, and the filtrate was diluted to 100 mL with distilled water. The lower concentrations were prepared by the appropriate dilution of the stock solution.

2.3. Apparatus

A Perkin Elmer (LAMBDA25) spectrophotometer controlled by a computer and equipped with a 1 cm path length quartz cell was used for UV-Vis spectra acquisition. Spectra were acquired between 350–600 nm (1 nm resolution). ELICO model LI-120 pH-meter furnished with a combined glass electrode was used to measure pH of buffer solutions.

3. Results and Discussions

Iron(II) and cobalt(II) react with HNAHBH forming reddish brown and yellow coloured complexes. The colour of the complexes was stable for more than two days.

3.1. Direct Method of Determination of Iron(II)

The absorption spectrum of [Fe(II)-HNAHBH] shows maximum absorbance at 405 nm. The preliminary investigations indicate that the absorbance of the complex is maximum and stable in pH range of 4.5–5.5. Hence pH 5.0 was chosen for further studies. A considerable increase in the colour intensity in the presence of 0.1% CTAB was observed. Studies on reagent (HNAHBH) concentration effect revealed that a maximum of 15-fold excess reagent is required to get maximum and stable absorbance for the complex. From the absorption spectra of [Fe(II)-HNAHBH] the molar absorptivity, coefficient is calculated as  L mol−1 cm−1. Variable amounts of Fe(II) were treated with suitable amounts of reagent, surfactant, and buffer and the validity of Beer’s law was tested by plotting the measured absorbance values of the prepared solutions against concentration of Fe(II). The calibration curve was linear over the range 0.055–1.373 μg mL−1. The composition of the complex [Fe(II) : HNAHBH] was determined as 2 : 3 by Job’s continuous variation method and the stability constant of the complex was calculated as . Other analytical results are presented in Table 5.

3.1.1. Effect of Diverse Ions in the Determination of Iron by Direct Method

Numerous cations and anions were added individually to the experimental solution containing 0.558 μg mL−1 of iron and the influence was examined (Table 1). All the anions and many cations were tolerable in more than 100 fold excess. The tolerance limits of some ions were in the range of 5–50 folds. Some of the metal ions, which strongly interfered, could be masked using appropriate masking agents.

Foreign ionTolerance limit (μg mL−1)Foreign ionTolerance limit (μg mL−1)Foreign ionTolerance limit (μg mL−1)


In the presence of μg of tartrate, μg of thiocyanate.
3.1.2. Determination of Iron in Surface Soil and Alloy Steels by Direct Spectrophotometric Method

The applicability of the developed direct method was evaluated by applying the method for the analysis of some surface soil and alloy steel samples for their iron content. Different aliquots of sample solutions containing suitable amounts of iron were treated with known and required volume of HNAHBH at pH 5.0 and 0.1% CTAB and diluted to 10 mL with distilled water. The absorbance of the resultant solutions was measured at 405 nm, and the amount of iron present was computed from the predetermined calibration plot. The results were compared with the certified values and presented in Tables 2 and 3.

SampleSource of the sampleAmount of iron (mg Kg−1) ± SD*

S1Groundnut cultivation soil
Akuthotapalli, Anantapur
40.98 ± 0.45
S2Cotton cultivation soil,
Singanamala, Anantapur district,
27.48 ± 0.36
S3Sweet lemon cultivation soil,
Garladinne, Anantapur distrcct
44.88 ± 0.24
S4Paddycultivation soil
Garladinne, Anantapur district
20.86 ± 0.37

*Average of five determinations.

Alloy steel composition (%)Amount of iron (%)
Certified valuePresent Relative error (%)

High tensile steel
(42.98 Zn, 19.89 Si, 0.351 Pb, 0.06 Sn, 0.04 Cd, 0.024 As, 0.14 Cu, and 4.13 Fe)
4.13 0.17
(34.26 Zn, 0.38 Si, 1.2 Cd, 48.57 Sb, 0.95 S, and 0.32 F)
34.26 0.01
(9.29 Al, 1.04 Ca, 9.53 Fe)9.53 0.08

*Average of five determinations.
3.2. Determination of Iron(II) by Derivative Method

Different amounts of Fe(II) (0.027–1.375 μg mL−1) were treated with suitable amounts of HNAHBH in buffer solutions of pH 5.0 along with 0.1% CTAB and made upto 10 mL with distilled water. 1st, 2nd, and 3rd order derivative spectra were recorded in the wavelength region 350–600 nm. The first-order derivative spectra showed maximum derivative amplitude at 427 nm (Figure 1). The second-order derivative spectra gave one large trough at 421 nm and a large crust at 435 nm with zero cross at 428 nm (Figure 2). A large crust at 415 nm and a large trough at 426 nm with zero cross at 421 nm were observed for the third-derivative spectra (Figure 3). Hence Fe(II) was determined by measuring the derivative amplitudes at 427 nm for 1st order, at 421 nm and 435 nm for 2nd order, and at 415 nm and 426 nm for 3rd order spectra.

3.2.1. Determination of Iron(II)

The derivative amplitudes measured at the analytical wavelengths as mentioned above for different derivative spectra were plotted against the amount of Fe(II). The calibration plots are linear in the range 0.027–1.375 μg mL−1. All the derivative methods are found to be more sensitive with a wider Beer’s law range than the zero order method (Table 5)

3.2.2. Effect of Foreign Ions in Derivative Method of Determination of Iron

The influence of some of the cations, which showed serious interference in zero order method, on the derivative amplitudes was studied by the reported methods and the results obtained are shown in Table 4. It can be observed from the table that large number of ions showed significantly high-tolerance limits in some of the derivative methods.

Foreign ionTolerance limit (in folds)
Direct methodFirst derivativeSecond derivativeThird derivative


ParameterDirect methodFirst derivativeSecond derivativeThird derivative
405 nm427 nm421 nm435 nm415 nm426 nm

Beer’s law range (μg mL−1)0.055–1.3730.027–1.3760.027–1.3760.027–1.3760.027–1.3760.027–1.376
Molar absorptivity, (L mol−1 cm−1)
Sandell’s sensitivity, (μg cm−2)0.0012
Angular coefficient (m)0.9740.0720.0060.0930.0020.085
Y-intercept (b)0.0047−0.0045
Correlation coefficient0.99970.99990.99990.99990.99990.9999
RSD (%)2.190.850.760.891.311
Detection limit (μg mL−1)0.0650.10.0220.02680.0360.304
Determination limit, (μg mL−1)0.1970.30.0680.80.110.914
Composition (M : L)2 : 3
Stability constant

3.2.3. Determination of Iron in Food and Biological Samples by First Order Derivative Method

Known aliquots of the prepared food and biological sample solutions were treated with suitable volumes of HNAHBH, buffer solution, and CTAB surfactant and diluted to the volume in 10 mL volumetric flasks. The first-order derivative spectra were recorded, and the derivative amplitudes were measured at analytical wave lengths. The amounts of Fe(II) in the samples were computed from predetermined calibration plots and presented in Table 6. The food and biological samples were further analyzed by Atomic Absorbance Spectrophotometric method, and the results obtained were compared with those of the present method.

Samples Amount of iron(μg mL−1) ± SD ( )
presentAASAddedpresentAAS% recovery

Wheat 5 97.6
Rice 5 102
Tomato 5 104
Orange 5 96
Banana 5 98.3
Prostate gland 6.5 103
Benign (enlarged prostate gland 6.5 95.12

3.3. Direct Method of Determination of Cobalt(II)

[Co(II)-HNAHBH] complex shows maximum absorbance at 425 nm. Maximum and stable absorbance of the complex is achieved in the pH range of 5.0–7.0. Hence pH 6.0 was chosen for further studies. A marginal increase in the absorbance was observed in presence of 0.15% of CTAB. 10-folds excess of HNAHBH is sufficient to get maximum absorbance. Molar absorptivity of the complex was calculated as  L mol−1 cm−1. Beer’s law is tested taking the different amounts of Co(II) in presence of suitable buffer, surfactant, and HNAHBH, linearity of the calibration curve is found between 0.118–3.534 μg mL−1 with a detection limit of 0.04 μg mL−1 and determination limit 0.124 μg mL−1 (Table 11), which shows the sensitivity of the present method. The stoichiometry of the complex was found to be 2 : 3 (Metal : Ligand) by Job’s method. The stability constant is calculated as .

3.3.1. Effect of Foreign Ions in the Determination of Cobalt by Direct Method

The effect of various anions and cations normally associated with Co(II) on the absorbance of the experimental solution was studied. The tolerance limits of the tested foreign ions, which bring about a change in the absorbance by ±2% were calculated and presented in Table 7.

Foreign ionTolerance limit (μg mL−1)Foreign ionTole limit (μg mL−1)Foreign ionToler limit (μg mL−1)


In the presence of μg of tartrate, μg of oxalate and μg of thiourea.

Among anions, except EDTA and citrate, all other tested ions were tolerable in more than 200-fold excess. EDTA and citrate were tolerable in 144- and 150-fold excess, respectively. Of the tested cations, some of them did not interfere even when present in more than 500 fold excess, many cations were tolerable between 10–80-folds. Cations which interfere seriously are masked with suitable anions.

3.3.2. Determination of Cobalt in Surface Soil, Blood and Urine Samples by Direct Method

Suitable aliquots of the soil, blood, and urine sample solutions were taken and analyzed for cobalt content by the proposed method, and the results are presented in Tables 8 and 9. The soil solutions were further analyzed by a reference method [23], and biological samples were analyzed by flame atomic absorption spectrophotometer, and the results obtained were compared with those of present method, which indicate the acceptability of the present method.

Sample and sourceCobalt (μg mL−1)
Present method*Reference method

S1Agricultural land
(red soil Anantapur.)
S2Agricultural land (black soil, Tadipatri.)
S3Riverbed soil (Tungabhadra river, Kurnool)
S4Industrial soil (electroplating industry, Anantapur)

*Average of four determinations.

Sample source SampleCobalt (μg mL−1)
Present ( )AAS ( )

Normal adult (male)Blood
Anemia patient (female)Blood
Paralysis patientBlood
Pulmonary patientBlood

3.4. Determination of Cobalt by Derivative Method

Variable amounts (0.059–4.712 μg mL−1) of Co(II), taken in different 10 mL volumetric flasks, were treated with optimal amounts of reagent HNAHBH at pH 6.0 in presence of 0.15% CTAB, and the derivative spectra were recorded in the wavelength region 350–600 nm against reagent blank. The second-derivative curves (Figure 4) gave a trough at 431 nm and a crust at 443 nm with a zero cross at 437 nm. In the third-derivative spectra (Figure 5), maximum amplitude was observed at 424 nm, 437 nm, 449 nm, and at 462 nm with zero crossings at 431 nm, 443 nm, and 456 nm.

3.4.1. Determination of Cobalt

The derivative amplitudes measured for different concentrations of Co(II) at appropriate wavelengths for 2nd and 3rd order derivative spectra were plotted against the amount of Co(II) which gave linear plots in the specified concentration regions. All the parameters like detection limit, correlation coefficient, and relative standard deviation values are presented in Table 11.

3.4.2. Effect of Foreign Ions

The selectivity of the derivative methods was evaluated by studying the effect of metal ions closely associated with cobalt on its derivative amplitudes under experimental conditions. The results are presented in Table 10. The results show that the tolerance limits of Th(IV), U(VI), Mn(II), Cu(II), Ni(II), Zn(II), Sn(II), In(II), Ga(III) and V(V) which interfere seriously in zero order method were greatly enhanced in the derivative methods indicating the greater selectivity of derivative methods over the direct method.

Diverse ionZero orderSecond derivativeThird derivative


ParameterDirect methodSecond derivativeThird derivative
425 nm431 nm443 nm437 nm449 nm

Beer’s law range (μg mL−1)0.118–3.5340.059–4.7120.059–4.7120.059–1.3800.056–1.380
Molar absorptivity, (L mol−1 cm−1)
Sandell’s sensitivity, μg cm−20.003
Angular coefficient (m)0.3750.00030.0930.00020.009
Y-intercept (b)0.0197
Correlation coefficient0.99990.9990.99990.99990.9999
RSD (%)1.371.844.31.157.6
Detection limit (μg mL−1)
Determination limit, (μg mL−1)0.1240.180.390.1140.65
Composition (M : L)2 : 3
Stability constant

3.4.3. Determination of Cobalt in Water and Pharmaceutical Samples by Second-Order Derivative Method

Suitable aliquots of water and pharmaceutical samples were taken and analysed for cobalt by second-order derivative method. The results obtained in the analysis of water samples by the proposed method are presented in Table 12 and the validity of the results was evaluated by adding known amounts of Co(II) and calculating their recovery percentage. The results obtained with pharmaceutical samples were compared with those obtained by AAS method and presented in Table 13.

Samplecobalt (μg mL−1)
AddedFoundRecovery (%)RSD (%)

Tap water (municipality water supply, Anantapur)0.00.322.5

River water (Penna, Tadipatri.)0.01.523.0

Drain water (vanaspati industry, Tadipatri.0.03.601.7

Sample (mg/tablet)Amount of cobalt (μg mL−1)
ReportedFound*Relative error (%)

Neurobion forte
(cyanocobalamine-15 mg)
Basiton forte
(cyanocobalamine-15 mg)

*Average of four determinations.
3.5. Simultaneous Second-Order Derivative Spectrophotometric Determination of Iron(II) and Cobalt(II)

Iron and cobalt occur together in many real samples like alloy steels, biological fluids, and environmental samples. In most cases, the characterizations of these samples include the determination of their metal ion content. The need for the determination of iron and cobalt in environmental and biochemical materials has increased after reports on different roles of these metals in human health and diseases. We are now reporting a simple, sensitive, and selective second-order derivative spectrophotometric method for the simultaneous determination of Fe(II) and Co(II) using HNAHBH without the need to solve the simultaneous equations.

3.5.1. Derivative Spectra

The 2nd order derivative spectra recorded for [Fe(II)-HNAHBH] and [Co(II)-HNAHBH] at pH 5.5 showed sufficiently large derivative amplitude for cobalt at 426 nm while the Fe(II) species exhibit zero amplitude (Figure 6). At 436 nm, maximum derivative amplitude was noticed for Fe(II) where there was no amplitude for Co(II). This facilitates the determination of Fe(II) and Co(II) simultaneously by measuring the second-derivative amplitudes of binary mixtures containing Fe(II) and Co(II)at 436 nm and 426 nm, respectively.

3.5.2. Determination of Fe(II) and Co(II)

Aliquots of solutions containing 0.055–1.650 μg mL−1 of Fe(II) or 0.117–4.719 μg mL−1 of Co(II) were transferred into a series of 10 mL calibrated volumetric flasks. HNAHBH (  M, 0.3 mL), CTAB (1%, 1.5 mL), and buffer solution (pH 5.5, 4 mL) were added to each of these flasks and diluted to the mark with distilled water. The zero-crossing points of [Fe(II)-HNAHBH] and [Co(II)-HNAHBH] species were determined by recording the second-order derivative spectra of both the systems with reference to the reagent blank. Calibration plots for the determination of Fe(II) and Co(II) were constructed by measuring the second-derivative amplitudes at zero crossing points of [Co(II)-HNAHBH] (436 nm) and [Fe(II)-HNAHBH] (426 nm), respectively, and plotting against the respective analyte concentrations. Fe(II) and Co(II) obeyed Beer’s law in the range 0.055–1.650 μg mL−1 and 0.117–4.719 μg mL−1 at 436 nm and 426 nm, respectively. Calibration plots were constructed for the standard solutions containing Fe(II) alone and in the presence of 0.589 μg mL−1 of Co(II). Similarly, the calibration graphs were constructed for standards containing Co(II) alone and in the presence of 0.330 μg mL−1 of Fe(II). The slopes, intercepts, and correlation coefficients of the prepared calibration plots were calculated and given in Table 14. The derivative amplitudes measured at 436 nm and 426 nm were found to be independent of the concentration of Co(II) and Fe(II), respectively. This allows the determination of Fe(II) and Co(II) in their mixtures without any significant error and without the need for their prior separation.

Metal ion determined Wave length (nm)Other metal present (μg mL−1) Slope Intercept Correlation coefficient

Fe(II)436 0.9994
0.589 0.9995
Co(II)426 0.9999
0.33 0.9998

3.5.3. Simultaneous Determination of Co(II) and Fe(II) in Binary Mixtures

Fe(II) and Co(II) were mixed in different proportions and then treated with required amount of HNAHBH in the presence of buffer solution (pH 5.5) and 0.15% of CTAB and diluted to the volume in 10 mL volumetric flasks. The second-order derivative spectra for these solutions were recorded (350–600 nm) and the derivative amplitudes were measured at 436 nm and 426 nm. The amounts of Fe(II) and Co(II) in the mixtures taken were calculated from the measured derivative amplitudes using the respective predetermined calibration plots. The results obtained along with the recovery percentage and relative errors are presented in Table 15, which indicate the usefulness of the proposed method for the simultaneous determination of Fe(II) and Co(II) in admixtures.

Amount taken (μg mL−1)Amount found* (μg mL−1)Relative error (%)

0.060.590.053 (96.3)0.572 (98.8)−3.6−2.8
0.120.590.120 (103.4)0.592 (100.5)3.440.5
0.230.590.230 (99.1)0.586 (99.4)−0.86−0.5
0.330.590.334 (101.2)0.572 (98.8)1.21−2.8
0.440.590.441 (100.2)0.590 (100.1)0.220.2
0.550.590.542 (98.5)0.586 (99.3)−1.45−0.5
0.330.590.328 (99.3)1.120 (94.9)−0.60−0.7
0.331.180.326 (89.6)2.280 (96.6)−1.21−5.0
0.332.360.324 (98.1)3.600 (101.7)−1.81−3.3
0.333.540.336 (101.8)4.670 (98.9)1.811.6
0.334.720.332 (100.6)4.670 (98.9)0.60−1.0

* Average of four determinations.
3.5.4. Simultaneous Determination of Iron and Cobalt in Alloy Samples

The developed second-order derivative spectrophotometric method was employed for the simultaneous determination of iron and cobalt in some alloy samples. Appropriate volumes of the alloy samples were treated with required amount of HNAHBH at pH 5.5 in the presence of 0.15% CTAB and diluted to 10 mL in standard flasks. The second-derivative curves for the resultant solutions were recorded, and the derivative amplitudes were measured at 426 nm and 436 nm. The amounts of iron and cobalt in the samples were evaluated with the help of predetermined calibration plots and presented in Table 16.

Sample (composition)Amount (%) Relative error (%)
CertifiedFound ( ) ± SD

(20 Cr; 15 Ni; 0.15 C; 2 Mn; 7 Mo;.05 Be)
1540 1.331.52
Rim alloy
(17 Mo; 3Mn)
6812 1.880.66
Sofcomag 25
(Fe and Co)
7525 1.483.92
Sofcomag 49
(Fe and Co)
5149 2.180.36

4. Conclusions

A comparison of the analytical results of the proposed methods was made with those of some of the recently reported spectrophotometric methods and presented in Table 17. The data in the above table reveals that the proposed method of determination of iron is more sensitive than those reported by Malik and Rao [27], Patil and Dhuley [28], Nagabhushana et al. [29], Wang et al. [30], Zhang et al. [31], and Martins et al. [36]. The methods proposed by Katmal and Hoyakava [24], Morales and Toral [25], and Reddy et al. [26] are more sensitive than the present method. However they are less selective than the proposed method as they suffer interference from W(VI), Pd(II), Cr(III), Tl(I), Pb(II), Bi(III), Hg(II), Mo(VI), EDTA, CN-. Regarding the determination of cobalt, the present method is more sensitive than those reported by Malik et al [16], Patil and Sawant [32], Adinarayana Reddy et al. [33], and Prabhulkar et al. [22]. However, the preset method is less sensitive than the methods reported by Guzor and Jin [21] and Qiufen et al. [34], but these methods are less selective due to the interference of many cations and anions. The results obtained in the simultaneous determination of Fe(II) and Co(II) are well comparable with the reported methods. Above all most of the reported methods involve extraction into spurious organic solvents where as the present methods are simple, nonextractive, and reasonably accurate.

Metal ionReagent (nm)pH/mediumAqueous/extractionBeer’s law μg mL−1 L mol−1 cm−1InterferenceReference

Fe(II)2-[2-(3,5-Dibromopyridyl-azo]-5-dimethyl amino-benzoic acid6152.0–7.0Extraction0–5.59.36Tl(I), Zn(II), Cr(III), W(VI), Co(II), Cu(II), Ni(II), and Pd(II)[24]
Fe(II)1,10-Phenanthroline and picrate5102.0–9.0Extraction0.1–3.613EDTA, CN-[25]
Fe(II)4-(2-Pyridylazo)resorcinol5056.0–7.5Extraction0–2.06Ni(II), Co(II), Pb(II), and EDTA[26]
Fe(II)1,3-Diphenyl-4-carboethoxy pyrazole-5-one5253.5–4.0Aqueous0.5–101.156Cu(II), Co(II), Zn(II), Mo(VI), EDTA[28]
Fe(II)Dyformyl hydrazine4707.3–9.3Aqueous0.25–130.3258[29]
Fe(II)4,7-Diphenyl-1,10-phenanthroline and tetraphenylborate534Extraction0–20.02[30]
Fe(II)Thiocyanate-acetone480HClO4Aqueous2.1Cu(II), , and [31]
Fe(II)2-Hydroxy-1-naphthaldehyde-p-hydroxybenzoic hydrazone4055Aqueous0.05–1.375.6Sn(II), Co(II) Ni(II) Zn(II) Al(III) Cu(II)Present method
Co(II)Sodium isoamyl xanthate4004.5–9.0Aqueous3.0–351.92[16]
Co(II)2-Pyridine carboxalde hydeisonicotinyl-hydrazine3469Aqueous0.01–2.77.1Au(III), Ag(I), Pt(III)[18]
Co(II)2-Hydroxy-1-naphthalidene salicyloyl hydrazone4308.0–9.0Extraction0–100.16[22]
Co(II)Pyridine-2-acetaldehyde salicyloyl hydrazone4151.0–6.0Extraction0.5–7.01.04[32]
Co(II)2-Hydroxy-l-naphthalidene-salicyloylhydrazone4308.0–9.0Extraction0–101.6 × 103[22]
Co(II)2-(2-Quinolynylazo)-5-dimethylamino aniline6255.5Extraction0.01–0.64.3Many cations and anions[34]
Co(II)2-Hydroxy-3-methoxy benzaldehyde thiosemicarbazone3906Aqueous0.06–2.352.74[35]
Co(II)2-Hydroxy-1-naphthaldehyde-p-hydroxybenzoic hydrazone4255Aqueous0.12–3.542.3Ni(II), Zn(II), Sn(II), In(III), and Ga(IIII)Present method


  1. E. Wildermuth, H. Stark, G. Friedrich et al., “Iron compounds,” in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, 2000. View at: Google Scholar
  2. F. C. Campbell, “Cobalt and cobalt alloys,” in Elements of Metallurgy and Engineering Alloys, pp. 557–558, ASM International, 2008. View at: Google Scholar
  3. M. L. C. Adolfsson, A. K. Saloranta, and M. K. Silander, “Colourant composition for paint products,” US Patent, Patent number: 5985987, 1999. View at: Google Scholar
  4. M. W. Hentze and L. C. Kühn, “Molecular control of vertebrate iron metabolism: mRNA-based regulatory circuits operated by iron, nitric oxide, and oxidative stress,” Proceedings of the National Academy of Sciences of the United States of America, vol. 93, no. 16, pp. 8175–8182, 1996. View at: Publisher Site | Google Scholar
  5. R. Michel, M. Nolte, M. Reich, and F. Loer, “Systemic effects of implanted prostheses made of cobalt-chromium alloys,” Archives of Orthopaedic and Trauma Surgery, vol. 110, no. 2, pp. 61–74, 1991. View at: Google Scholar
  6. J. A. Disegi, R. L. Kennedy, and R. Pillia, Cobalt-Base Alloys for Biomedical Applications, ASTM International Standards, 1999.
  7. J. T. Ellis, I. Schulman, and C. H. Smith, “Generalized siderosis with fibrosis of liver AND pancreas in cooley's (Mediterranean) anemia with observations on the pathogenesis of the siderosis AND fibrosis,” American Journal of Pathology, vol. 30, no. 2, pp. 287–309, 1954. View at: Google Scholar
  8. Wu, Li-Xiang, Guo, and J. Cun, Metallurgical Analysis, vol. 24, no. 3, pp. 66–68, 2004.
  9. L. Zaijun, F. You, L. Zhongyun, and T. Jian, “Spectrophotometric determination of iron(III)-dimethyldithiocarbamate (ferbam) using 9-(4-carboxyphenyl)-2,3,7-trihydroxyl-6-fluorone,” Talanta, vol. 63, no. 3, pp. 647–651, 2004. View at: Publisher Site | Google Scholar
  10. Qi-Kai Zhang, Ling-Zhao Kong, and Li Wang, “Spectrophotometric determination of micro amount of iron in oils with thiocyanate-phenanthroline-OP,” Fenxi Shiyanshi (Analytical Laboratory), vol. 24, no. 1, pp. 77–79, 2005. View at: Google Scholar
  11. P. K. Tarafder and R. Thakur, “Surfactant-mediated extraction of iron and its spectrophotometric determination in rocks, minerals, soils, stream sediments and water samples,” Microchemical Journal, vol. 80, no. 1, pp. 39–43, 2005. View at: Publisher Site | Google Scholar
  12. F. G. Martins, J. F. Andrade, A. C. Pimenta, L. M. Lourenco, J. R. M. Casto, and V. R. Balbo, “Spectrophotometric study of iron oxidation in the iron(II)/thiocyanate/acetone system and some analytical applications,” Eclética Química, vol. 30, no. 3, pp. 63–71, 2005. View at: Google Scholar
  13. A. K. Sharma and I. Singh, “Spectrophotometric trace determination of iron in food, milk, and tea samples using a new bis-azo dye as analytical reagent,” Food Analytical Methods, vol. 2, no. 3, pp. 221–225, 2009. View at: Publisher Site | Google Scholar
  14. L. I. Cheng-hong, G. E. Chang-hua, L. Hua-ding, and P. Fu-you, “Spectrophotometric determination of iron with 2-(5-carboxy-1,3,4-triazolylazo)-5-diethylamino aniline,” Science Technology and Engineering, vol. 21, pp. 5780–5782, 2008. View at: Google Scholar
  15. Q. Z. Zhai, “Catalytic kinetic spectrophotometric determination of trace copper with copper(II)-p-acetylchlorophosphonazo-hydrogen peroxide system,” Bulletin of the Chemical Society of Ethiopia, vol. 23, no. 3, pp. 327–335, 2009. View at: Google Scholar
  16. A. K. Malik, K. N. Kaul, B. S. Lark, W. Faubel, and A. L. J. Rao, “Spectrophotometric determination of cobalt, nickel palladium, copper, ruthenium and molybdenum using sodium isoamylxanthate in presence of surfactants,” Turkish Journal of Chemistry, vol. 25, no. 1, pp. 99–105, 2001. View at: Google Scholar
  17. B. R. Reddy, P. Radhika, J. R. Kumar, D. N. Priya, and K. Rajgopal, “Extractive spectrophotometric determination of cobalt(II) in synthetic and pharmaceutical samples using cyanex 923,” Analytical Sciences, vol. 20, no. 2, pp. 345–349, 2004. View at: Publisher Site | Google Scholar
  18. G. A. Shar and G. A. Soomro, “Spectrophotometric determination of cobalt(II), nickel(II) and copper (II) with 1-(2 pyridylazo)-2-naphthol in micellar medium,” The Nucleus, vol. 41, pp. 77–82, 2004. View at: Google Scholar
  19. N. Veerachalee, P. Taweema, and A. Songsasen, “Complexation and spectrophotometric determination of cobalt(II) ion with 3-(2′-thiazolylazo)-2,6-diaminopyridine,” Kasetsart Journal—Natural Science, vol. 41, no. 4, pp. 675–680, 2007. View at: Google Scholar
  20. Y. Haoyi, Z. Guoxiu, and Y. Gaohua, “Determination of cobalt in terephthalic acid by picramazochrom spectrophotometry,” Chemical Analysis and Meterage, vol. 1, 2009. View at: Google Scholar
  21. S. H. Guzar and Q. H. Jin, “Simple, selective, and sensitive spectrophotometric method for determination of trace amounts of nickel(II), copper (II), cobalt (II), and iron (III) with a novel reagent 2-pyridine carboxaldehyde isonicotinyl hydrazone,” Chemical Research in Chinese Universities, vol. 24, no. 2, pp. 143–147, 2008. View at: Publisher Site | Google Scholar
  22. S. G. Prabhulkar and R. M. Patil, “2-Hydroxy-1-naphthalidine salicylohydrazone as an analytical reagent for extractive spectrophotometric determination of a biologically and industrially important metal Cobalt(II),” International Journal of Chemical Sciences, vol. 6, no. 3, pp. 1480–1485, 2008. View at: Google Scholar
  23. J. E. Huheey, E. A. Keiter, and R. L. Keiter, Inorganic Chemistry, Harper Collins, New York, NY, USA, 4th edition, 1993.
  24. T. Katami, T. Hayakawa, M. Furukawa, and S. Shibata, “Extraction—spectrophotometric determination of iron with 2-[2-(3,5-Dibromopyridyl)azo]-5-dimethylaminobenzoic acid,” The Analyst, vol. 109, no. 2, pp. 159–162, 1984. View at: Google Scholar
  25. A. Morales and M. I. Toral, “Extraction—spectrophotometric determination of iron as the ternary tris(1,10-phenanthroline)-iron(II)-picrate complex,” The Analyst, vol. 110, no. 12, pp. 1445–1449, 1985. View at: Google Scholar
  26. M. R. P. Reddy, P. V. S. Kumar, J. P. Shyamsundar, and J. S. Anjaneyulu, “Extractive spectrophotometric method for the determination of iron in titanium base alloys using 4- (2-Pyridylazo) resorcinol and a long chain quaternary ammonium salt,” Journal of the Indian Chemical Society, vol. 66, pp. 437–439, 1989. View at: Google Scholar
  27. A. K. Malik and A. L. J. Rao, “Spectrophotometric determination of iron(III) dimethyldithiocarbamate (ferbam),” Talanta, vol. 44, no. 2, pp. 177–183, 1997. View at: Publisher Site | Google Scholar
  28. R. K. Patil and D. G. Dhuley, “Solvent extraction and spectrophotometric determination of Fe(II) with 1,3-diphenyl-4-carboethoxy pyrazole-5-one,” Indian Journal of Chemistry, vol. 39, no. 10, pp. 1105–1106, 2000. View at: Google Scholar
  29. B. M. Nagabhushana, G. T. Chandrappa, B. Nagappa, and N. H. Nagaraj, “Diformylhydrazine as analytical reagent for spectrophotometric determination of iron(II) and iron(III),” Analytical and Bioanalytical Chemistry, vol. 373, no. 4-5, pp. 299–303, 2002. View at: Publisher Site | Google Scholar
  30. L. M. Wang, C. Song, and J. Jin, “Spectrophotometric determination of iron by extraction of its ternary complex with 4,7-diphenyl-1,10-phenanthroline and tetraphenylborate into molten naphthalene,” Fenxi Shiyanshi (Analytical Laboratory), vol. 23, no. 9, pp. 48–50, 2004. View at: Google Scholar
  31. F. G. Martins, J. F. Andrade, A. C. Pimenta, L. M. Lourenco, J. R. M. Casto, and V. R. Balbo, “Spectrophotometric study of iron oxidation in the iron(II) thiocyanateacetone system and some analytical application,” Electica Quimica, vol. 30, no. 3, pp. 63–71, 2005. View at: Google Scholar
  32. S. S. Patil and A. D. Sawant, “Pyridine-2-acetaldehyde salicyloylhydrazone as reagent for extractive and spectrophotometric determination of cobalt(II) at trace level,” Indian Journal of Chemical Technology, vol. 8, no. 2, pp. 88–91, 2001. View at: Google Scholar
  33. S. Adinarayana Reddy, K. Janardhan Reddy, S. Lakshmi Narayana, Y. Sarala, and A. Varada Reddy, “Synthesis of new reagent 2,6-diacetylpyridine bis-4-phenyl-3- thiosemicarbazone (2,6-DAPBPTSC): Selective, sensitive and extractive spectrophotometric determination of Co(II) in vegetable, soil, pharmaceutical and alloy samples,” Journal of the Chinese Chemical Society, vol. 55, no. 2, pp. 326–334, 2008. View at: Google Scholar
  34. Q. Qiufen, G. Yang, X. Dong, and J. Yin, “Study on the solid phase extraction and spectrophotometric determination of cobalt with 2-(2-quinolylazo)-5-diethylaminoaniline,” Turkish Journal of Chemistry, vol. 28, no. 5, pp. 611–619, 2004. View at: Google Scholar
  35. A. P. Kumar, P. R. Reddy, and V. K. Reddy, “Direct and derivative spectrophotometric determination of cobalt (II) in microgram quantities with 2-hydroxy-3-methoxy benzaldehyde thiosemicarbazone,” Journal of the Korean Chemical Society, vol. 51, no. 4, pp. 331–338, 2007. View at: Google Scholar
  36. F. G. Martins, J. F. Andrade, A. C. Pimenta, L. M. Lourenço, J. R. M. Castro, and V. R. Balbo, “Spectrophotometric study of iron oxidation in the iron(II)/thiocyanate/ acetone system and some analytical applications,” Ecletica Quimica, vol. 30, no. 3, pp. 63–71, 2005. View at: Publisher Site | Google Scholar

Copyright © 2012 V. S. Anusuya Devi and V. Krishna Reddy. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

More related articles

 PDF Download Citation Citation
 Download other formatsMore
 Order printed copiesOrder

Related articles

Article of the Year Award: Outstanding research contributions of 2020, as selected by our Chief Editors. Read the winning articles.