See discussions, stats, and author profiles for this publication at: https://www.researchgate.

net/publication/305461449

Determination of Trace Amount of Cu (II) Using UV-Vis. Spectrophotometric

Method

Article · January 2013

CITATIONS READS

6 7,796

2 authors, including:

Khokan Chandra Sarker

Bangladesh University of Engineering and Technology
5 PUBLICATIONS 37 CITATIONS

SEE PROFILE

All content following this page was uploaded by Khokan Chandra Sarker on 20 July 2016.

The user has requested enhancement of the downloaded file.

 ISSN: 2321-4902
Volume 1 Issue 1
Online Available at www.chemijournal.com

International Journal of Chemical Studies

Determination of Trace Amount of Cu (II) Using UV-Vis.
Spectrophotometric Method
Khokan Chandra Sarker*1, Dr. Md. Rafique Ullaha 2

1. Ph.D. researcher, Department of Chemistry, Faculty of Engineering, Bangladesh University of Engineering

and Technology, Dhaka-1000, Bangladesh. [E-mail:khokanchem@yahoo.com]

2. Professor, Department of Chemistry, Faculty of Engineering, Bangladesh University of Engineering and

Technology, Dhaka-1000, Bangladesh. [E-mail:rafique@chem.buet.ac.bd]

Abstract: Trace amount of Copper(II) has determined by spectrophotometric technique using 1-(2-pyridylazo)-
2-naphthal (PAN), as a new spectrophotometric reagent which is insoluble in water. PAN reacts in highly acidic
solution at pH 2.40 to 2.50 with Cu(II) to give a pink chelate which has an absorption maximum (λmax.) at 550nm.
The reaction is instantaneous and absorbance remains stable for over 48hrs. The average molar absorption co-
efficient (ε) was found to be 2.05×104 L mol-1cm-1 and Sandell sensitivity is 3.23×10−4 μg cm−2. Linear
calibration graphs were obtained for 0.1-4.0 μgL-1 of Cu(II) and RSD (%) is 1.16. The stoichiometric composition
of the chelate is 1:2 (Cu:PAN). Large excess of over 50 cations, anions, and some common complexing agents (e.g.
oxalate, phosphate, tartarate, thio-urea) do not interfere in the determination. The method was successfully used in the
determination of Cu(II) in Several Standard Reference Materials as well as in some environmental and industrial
waste water. The method has high precision and accuracy.

Keyword: UV-VIS. Spectrophotometry, Absorption spectrum (λmax fixation), 1-(2-pyridylazo)-2-naphthal (PAN),

Calibration using Beer’s law, Environmental and waste water samples.

1.Introduction: and the risk of skin cancer[6]. It also caused

Different types of ligand were used with about 30 generalized cancers in laboratory animals and has
toxic metal ions to obtain colour chelate through been linked epidemiologically with certain
the novel reaction techniques. Finally Trace human cancers[6]. The most serious situations
amount of toxic element Cu(II) was determined being the disease called cirrhosis, Wilson’s,
by spectrophotometric method using PAN as a Alzheimer’s diseases and skin cancer which
new spectrophotometric reagent in acidic water. causes gradual weakening of the bone structure,
Copper in trace amounts is important diminution of stature and ultimately the total
industrially[1], as a toxicant[2] and biological non- collapse of the entire skeletal system[7]. Its
essential[2], as an environmental pollutant[3] and extreme toxicity towards marine and fresh water
as an occupational hazard [4]. It is a toxic metal, organisms is also well known [7]. Copper is a
has been responsible for a number of diseases [5]. potential health hazard due to its presence in
The symptoms of copper poisoning are drinking water, food cooked in copper utensil[7].
instantaneous hypertension, shortening of life- The permissible limit of copper in drinking water
span; Kidney damage, bronchitis, retardation of is 2.0mgL-1 according to EPA[8]. Increasing
growth, cirrhosis, Wilson’s, Alzheimer’s copper pollution of the environment resulting
diseases, gross abnormalities of the vital organs from the growth of copper based industries and

Vol. 1 No. 1 2013 www.chemijournal.com Page | 5

International Journal of Chemical Studies

the use of fossil fuels makes the development of polypropylene bottles containing 1mL of
method for the trace and ultra-trace analysis of concentrated HNO3. More rigorous
this toxic metal essential. Spectrophotometry is contamination control was used when the copper
essentially a trace analysis technique and is one levels in the specimens were low.
of the most powerful tools in chemical analysis.
PAN has been reported as a spectrophotometric 2.3 PAN Solution (4.01x 10-4 M):
reagent for Co, Ni, Zn, Mn, Ca[9] but has not Prepared by dissolving the requisite amount of
previously been used for spectrophotometric PAN (BDH chemicals) in a known volume of
determination of Cu(II) in acidic aqueous media. highly acidified (HCl) de-ionized water. More
This paper reports its use in a very sensitive, dilute solutions of the reagent were prepared as
highly specific spectrophotometric method for the required. PAN is insoluble in water and soluble in
trace determination of Cu(II). The method organic solvent, but we have used acid and water
possesses distinct advantages over existing to soluble PAN.
methods[10-18] with respect to sensitivity,
selectivity, range of determination, simplicity, 2.4 Cu(II) Standard Solutions:
speed, pH range, thermal stability, accuracy, A 100mL of stock solution of divalent copper
precision and ease of operation. The method is was prepared by dissolving 0.03929mg of AR
based on the reaction of non-absorbent PAN in crystallize copper sulfate (Cu SO4; 5H2O)
highly acidic solution with copper to produce a (Merck) in doubly distilled de-ionized water.
highly absorbent deep pink chelate product, Aliquots of this solution were standardized by
followed by direct measurement of the EDTA titration using Sulfon black-T as indictor.
absorbance in aqueous solution. With suitable More dilute standard solutions were prepared by
masking, the reaction can be made highly appropriate dilution of aliquots from the stock
selective solution with de-ionized water and when
required.
2. Experimental:
2.1 Apparatus: 2.5 EDTA Solution:
A shimadzu (Kyoto, Japan) (Model-1601PC) 100mL stock solution of EDTA (0.01% w/v) was
double beam UV-VIS. recording prepared by dissolving 10mg of A.C.S. grade
spectrophotometer and Jenway (England, U.K.) (≥99%) of disodium dihydrogen ethylenediamine
(Model-3010) pH meter were used for the tetraacetate dihydrate in (100mL) de-ionized
measurement of absorbance and pH, respectively. water.
A Shimadzu (Model-AA 6200) atomic absorption
spectrophotometer equipped with a micro 2.6 Potassium Permanganate Solution:
computer-controlled nitrous oxide-acetylene A 1% potassium permanganate Solution (Merck)
flame was used for comparison of the results. was prepared by dissolving in de-ionized water.
Aliquots of this solution were standardized with
2.2 Reagents and Solutions: oxalic acid. Sodium azide solution (2.5% w/v)
All the chemicals used, were of analytical-reagent (purity >99%) was also used.
grade of the highest purity available. Doubly
distilled de-ionized water, which is non-absorbent 2.7 Tartarate Solution:
under ultraviolet radiation, was used throughout. A 100mL stock solution of tartarate (0.01% w/v)
Glass vessels were cleaned by soaking in was prepared by dissolving 10mg of A.C.S grade
acidified solutions of KMnO4 or K2Cr2O7 (99%) potassium sodium tartarate tetrahydrate in
followed by washing with nitric acid (1+1) and (100mL) de-ionized water.
rinsed several times with high-purity de-ionized
water. Stock solutions and environmental water
samples (1000mL each) were kept in

Vol. 1 No. 1 2013 www.chemijournal.com Page | 6

International Journal of Chemical Studies

2.8 Aqueous Ammonia Solution:

A 100mL solution of aqueous ammonia was
prepared by diluting 10mL concentrated NH4OH
(28–30%, A.C.S grade) to 100mL with deionized
water. The solution was stored in polypropylene
bottle.

2.9 Other Solutions:

Solutions of a large number of inorganic ions and
complexing agents were prepared from their
analar grade or equivalent grade water soluble
salts (or the oxides and carbonates in
hydrochloric acid); those of niobium, titanium,
zirconium and hafnium were specially prepared
from their corresponding oxides (Specpure,
Johnson Matthey) according to the recommended Fig.1: Absorption spectrum of Cu (II)-PAN against the
reagent blank (at pH=2.50, λMax=550 nm) in aqueous
procedures of Mukharjee[19]. In the case of solution.
insoluble substances, special dissolution methods
were adopted [20].

2.10 Procedure:
To 0.1–1.0mL of a neutral aqueous (pH=4)
solution containing 1–10µg of copper in a 10mL
calibrated flask was mixed with 1:5-1:10 fold
molar excess of PAN reagent solution preferably
4.01×10 -4M followed by the addition of 0.5M
hydrochloric acid (HCl) and NH4OH to control
pH of solution at around 2.50. The mixture was
diluted to the mark with de-ionized water. The
absorbance was measured at λ max=550nm against
a corresponding reagent blank. The copper
content in an unknown sample was determined (Fig.1.a): Absorption spectrum of PAN and Cu (II)-PAN
using concurrently prepared calibration graph. against the reagent blank at pH=2.50 in aqueous solution.

3. Results and discussion: 3.2 Effect of Acid and pH:

To see the effect of different pH we have taken
3.1 Absorption spectrum:
0.5ppm Cu(II) solution. Of the various acids
The absorption spectrum o f t h e Cu (II)-PAN
(nitric, sulfuric, hydrochloric and phosphoric)
solution system in 1(M) HCl medium was
recorded using the UV-Vis. Spectrophotometer. studied hydrochloric acid was found to be the
The absorption spectrum of the Cu(II)-PAN are a best acid for the system. The absorbance was
maximum when the pH of the solution is 2.5 at
symmetric curve with the maximum absorbance
co-efficient is shown in (Fig-1) and Absorption room temperature (25±5)0C. We have controlled
spectrum of PAN and Cu(II)-PAN against the the pH of the solution using hydrochloric acid
reagent blank at pH=2.50 in aqueous solution is and ammonium hydroxide as a base and double
shown in Fig.-1.a. In all instances measurements distilled water. Outside this range of acidity, the
were made at 550nm against a reagent blank. The absorbance decreased (Fig.-2). At λMax=550nm
reaction mechanism of the present method is as the absorbance values of Cu(II)-PAN complex
reported earlier[21]. are as follows. At higher concentration of PAN

Vol. 1 No. 1 2013 www.chemijournal.com Page | 7

 International Journal of Chemical Studies

solution starts to form ppt. at pH 2.00. So we

1.5
have used the lower concentrated solution
(4.0×10-4M) of PAN.
1.0

a bsorbance
0.18

0.16

0.14 0.5

0.12
absorbance

0.10

0.08
0.0
0.06 1 2 3 4 5 10 24 48

0.04 Time (hours)

0.02 (b)
0.00
0.5 1.0 1.5 2.0 2.5 3.0 3.5

pH of Cu-PAN solution Fig.-3. b: Effect of the time on the absorbance of Cu(II)-

PAN (1:10) system.
Fig.-2: Effect of pH on the absorbance of Cu(II)-PAN
(1:10) complex. 3.4 Effect of Temperature:
The Cu(II)-PAN system obtained maximum and
3.3 Effect of Time: constant absorbance at room temperature
The reaction is instantaneous. Constant maximum (25±5)0C. Outside this range of temperature, the
absorbance was obtained just after diluting to absorbance decrease gradually (Fig.-4).
volume and remained strictly unaltered for 48
hours (Fig.-3 a, b). At pH over 3.00 Cu(II)-PAN 0.166

complexes and PAN itself start to form ppt in 0.164

0.162

solution. When the solution forms ppt it goes out 0.160

0.158

of the measurement of spctrophotomatric

Absorbance

0.156

0.154

analysis. We have fixed the pH at 2.50; (or 2.00 0.152

to 2.50) in this pH the complex will not form ppt 0.150

0.148

for the long time. We have observed sample of 0.146

0.144
10 15 20 25 30 35 40 45 50

complex for 48 hours and constant maximum Temperature ( 0 C)

absorbance was obtained just after diluting to

Fig-4: Effect of temperature on absorbance of Cu(II)-PAN
volume and remained strictly unaltered form
solution.
beginning to end.
3.5 Effect of Reagent Concentration:
1.5 Different molar excesses of PAN were added to
fixed metal ion concentration and absorbances
1.0 were measured according to the standard
absorbance

procedure. It was observed that at the 1ppm

0.5
Cu(II) metal the reagent molar ratios of 1:2-1:20
produce a constant absorbance of the Cu(II)-PAN
0.0
complex (Fig.-5). For all subsequent
0.0 05 10 15
60
20 25 30
measurements different amount (mL) of 4.01×10 -
Time (min.) 4
(a) M, PAN reagent was added.
Fig.-3.a: Effect of the time on the absorbance of Cu(II)- PAN
(1:10) system.

Vol. 1 No. 1 2013 www.chemijournal.com Page | 8

 International Journal of Chemical Studies

0 .3 5

0 .3 0

0 .2 5
Absorbance

0 .2 0

0 .1 5

0 .1 0

0 .0 5

0 .0 0
0 1 2 3 4 5 6
C o n c e n t ra ti o n o f P A N

Fig.-5: Effect of reagent (PAN) molar concentration ratio

on the absorbance of Cu(II)-PAN system. (Fig-6.a): The overlay of absorption spectrum of Cu(II)-PAN for 0.1–
5.0µg mL-1 of Copper at pH= 2.50, λ ma x=550nm.

3.6 Calibration Graph (Beer’s law): 3.7 Effect of foreign ions:

The well-known equation (A=εcl) for The effect of over 50 ions and complexing agents
spectrophotometric analysis in very dilute solution on the determination of only 1µg mL-1 of Cu(II)
was derived from Beer’s law. The effect of metal was studied. The criterion for interference [23] was
concentration was studied over 0.1-5.0µgL-1. The an absorbance value varying by more than ±5%
absorbance was linear for 0.1–4.0µgL-1 of Cu(‫ )׀׀‬at from the expected value for copper alone. The
λmax=550nm. The molar absorption co-efficient, (ε) most serious interferences were from Ni(II), Co(II)
[22]
was found to be 2.052×104 L mol-1cm-1. Of the and Fe(III) ions. Interference from these ions is
calibration graph which that showing the limit of probably due to complex formation with PAN. The
linearity range is given in (Fig.-6) and overlay of greater tolerance limits for these ions can be
spectrum layout is shown in (Fig-6.a). achieved by using several masking agents. In order
to eliminate the interference if Ni and Co are
present in the sample they are eliminated by
extraction from the sample using 15ml of 10×10-
3
mole/L DMG solution in 1,2-dichloroethane. If
1.8
the aqueous phase contains mercury and iron, 1gm
1.6

1.4
of KI was added masking agent for Hg and 10gm
1.2
of KF dissolved in 4mole/L HNO3 solution was
used to preclude the interference of iron [24].
Absorbance

1.0

0.8 Interference from these metal ions Ni(II), Co(II)

0.6 and Fe(III) have been effectively removed by a
0.4
short single step ion-exchange separation process,
0.2
using an Amberlite XAD-8 resin (100-200 mesh)
0.0
0 1 2 3 4 5 6 ion exchanger [25].
Concentration of Cu(II)
* [Coefficients: b[0]= 0, b[1]=0.3235095023]
3.8 Composition of the absorbent Complex:
(Fig.-6):Calibration graph of absorbance of Cu(II)–PAN Job’s method[26] of continuous variation and the
complex against the different concentration of Cu
0.1 to 5.0 ppm. molar-ratio method [27] were applied to ascertain
the stoichiometric composition of the complex. A
Cu(‫–)׀׀‬PAN (1:2) complex was indicated by both
methods.

Vol. 1 No. 1 2013 www.chemijournal.com Page | 9

 International Journal of Chemical Studies

HO relative standard deviation (n=5) was 0–1.16%

for 0.1–4.0µgL-1 of Cu(II) in 10mL, indicating
N
that this method is highly precise and
N
N reproducible (Table-1). The detection limit is 0.1-
Cu 4.0µgL-1. Added copper was accurately recovered
N
from the other metals. The reliability of our
N
Cu(II)-PAN procedure was tested by recovery
N studies. The average percentage recovery
OH obtained for addition of Cu(II) to some
environmental water and industrial waste water
Structure of the Cu(II)-PAN complex (proposed) samples was quantitative as shown in (Table-2).
The results of water samples analysis by the
3.9 Precision and accuracy: spectrophotometric method were in excellent
The precision of the present method was agreement with those obtained by AAS. Hence
evaluated by determining different concentrations the precision and accuracy of the method were
of Cu(II) (each analyzed at least five times). The found to be excellent.

3.10 Selected analytical parameters obtained with the optimization experiments:

Parameter Studied range Selected Value

Wavelength, λmax (nm) 200 - 800 550
pH 1.0 – 3.5 2.40 – 2.50
Time/h 0 - 72 24
Temperature, °C 1 - 50 25 ±5
Reagent (fold molar excess, M: R) 1 : 2 – 1: 20 1 : 5 – 1: 10
Linear range, µgL-1 0.01 - 20 0.1 – 5.0
Detection limit, µgL-1 0.1 - 20 0.1 – 4.0
Reproducibility (% RSD) 0-5 0 – 1.16

4. Applications: 4.1 Determination of Cu(II) in Environmental

The present method was successfully applied to and Industrial Water:
the determination of Cu(II) in various industrial Each filtered (with whatman No.-40)
waste water samples of various compositions environmental water sample (1000mL) was
(Table-2) and also in number of real samples, e.g. evaporated nearly to dryness with a mixture of
several Certified Reference Materials (CRM). 5mL of concentrated H2SO4 and 10mL of
The method was also extended to the concentrated HNO3 in a fume cupboard following
determination of copper in a number of a method recommended by Greenberg et al.[28],
environmental samples. In view of the unknown and was then cooled to room temperature. The
composition of environmental water samples, the residue was then heated with 10mL of de-ionized
same equivalent portions of each such sample water in order to dissolve the salts. The solution
was analyzed for Cu(II) content, recoveries in was then cooled and neutralized with dilute
both the ‘spiked` (added to the samples before the NH4OH in the presence of 1–2mL of 0.01 %
mineralization or dissolution) and the ‘unspiked` (w/v) tartarate solution. The resulting
samples are in good agreement (Table-2). The solution was then filtered and quantitatively
results o f industrial w a s t e w a t e r a n a l y s i s transferred into a 25mL calibrated flask and
b y spectrophotometric method were found to be made up to the mark with de-ionized water. An
in excellent agreement with those obtained by aliquot (1–2mL) of this pre-concentrated water
AAS. The precision and accuracy of the method sample was pipette into a 1 0 mL C a lib r at ed
were excellent. f l a s k a n d the Cu(II) content was

Vol. 1 No. 1 2013 www.chemijournal.com Page | 10

 International Journal of Chemical Studies

Determined as described under procedure using The suggested safe level of copper in drinking
KF as a masking agent. The analysis of water for humans varies depending on the source,
environmental water samples from various but tends to be pegged at 2.0mg/L [28]. The results
sources for Cu (II) are shown in (Table-3). Most of water samples analysis by spectrophotometric
spectrophotometric method for the determination method were found to be in excellent agreement
of Cu (II) in natural and sea water require pre- with those obtained by AAS, results are shown in
concentration of Cu (II)[29]. The concentration of Cu table-2.
(II) in natural and sea water is a few µgL -1.

Table-1: Standard deviation and relative Standard deviation of Cu (II) - PAN system:

Mean
   Standard Relative
Cu(II) taken Cu(II) Found
Sample No.
µgL -1 X1 µgL -1
X X1 - X (X1 - X )2 deviation standard
µgL - 1 (±S) deviation (S r)%

1 100.0 98.5 1.64 2.67

2 100.0 99 1.14 1.29

3 100.0 101 0.86 0.75

4 100.0 100.5 0.36 0.13

5 100.0 99.5 0.64 0.41

6 100.0 101.5 1.36 1.85

100.14  1.16 1.16

7 100.0 101 0.86 0.74

8 100.0 99.5 0.64 0.41

9 100.0 98.5 1.64 2.69

10 100.0 101.5 1.36 1.85

11 100.0 101 0.86 0.74

 
2
∑X1- X = ∑ (X1 - X ) =
N = 11 ∑X1 = 1101.5
11.364 13.53

Vol. 1 No. 1 2013 www.chemijournal.com Page | 11

 International Journal of Chemical Studies

Table-2: Determination of Copper in some environmental water and industrial waste water samples (*Average of five
replicate determinations.):

Copper/ µg L-1
Sample
Added Found a
Recovery
±S (%) srb (%)
0 2.5 ±0.2 0.25
Tap water
100 102.0 99±0.6 0.58
0 1.5
Waste Water of UFFL 100.2±0.4 0.39
100 101.0
0 1.0
Waste Water of PUFFL 100.4±0.6 0.59
100 102.0
0 1.0
Waste Water of CUFL 100.2±0.8 0.79
100 101.5
0 1.5
Waste Water of JFCL 100.0±0.3 0.29
100 102.0
0 1.5
Waste Water of AFCL 100.0±0.4 0.39
100 102.0
0 2.5
Waste Water of TSP 100.2±0.3 0.29
100 103.5
0 5.0
River water

Buriganga (upper)
100 107.0 100.9±0.4 0.24
0 5.5
Buriganga (lower) 99.4±0.3 0.37
100 105.5

0 12.0
Bay of Bengal (upper) 99±0.2 0.29
Sea water

100 120.0

0 13.5
Bay of Bengal (lower) 100.1±0.3 0.21
100 114.8
0 15.0
Berger Paints, Dhaka 99±0.5 0.43
Drain
water

100 113.0
0 12.0
Asian Paints, Dhaka 100.9±0.3 0.26
100 114.0

Table-3: Determination of Copper in some environmental water and industrial waste water samples (a, average of five replicate
determinations, b, the measure precision is the relative standard deviation S r.):

Serial Copper/µgL-1 Sample source

No Sample Proposed
AAS
method
01 Waste Water 0.9 1.5±0.5 UFFL, Ghorashal, Narshingdi.
02 Waste Water 1.6 1.0±0.6 PUFFL Ghorashal, Narshingdi.
03 Waste Water 1.7 1.0±0.8 CUFL, Chittagong.
04 Waste Water 2.0 1.5±0.4 JFCL, Jamalpur.
05 Waste Water 1.8 1.5±0.3 AFCL, Ashogong.
06 Waste Water 2.9 2.5±0.3 TSP, Chittagong.
07 River water 5.4 5.0±0.4 Buriganga
08 Sea water 12.3 12.0±0.3 Bay of Bengal
09 Drain Water 15.6 15.0±0.6 Berger Paints, Dhaka
10 Drain Water 12.4 12.0±0.3 Asian Paints, Dhaka

4.2 D e t e r m i n a t i o n o f C u (II) i n a l l o y s Was accurately weighed into a 50mL flask

a n d Steels: 0.1g amount of an alloy or steel following a method recommended by Parker [30].
sample

Vol. 1 No. 1 2013 www.chemijournal.com Page | 12

International Journal of Chemical Studies

To it, 10mL of 20% (V/V) sulfuric acid was Solution. The resulting solution was filtered, if
added, carefully covering with a watch-glass until necessary, through a whatman No. 40 filter paper
the brisk reaction subsided. The s o lu tio n w as into a 50mL calibrated flask. The residue was
heated and simmered gently after addition of 5ml washed with a small volume of hot water and the
of concentrated H N O 3 until all car b id es volume was made up with de-ionized water. A
w er e decomposed. Then 2mL of 1:1 (V/V) suitable aliquot (0.1–1.0mL) of the above
H2SO4 was added and the solution was solution was taken into a 10mL calibrated flask
evaporated carefully to dense white fumes to and the Cu(II) content was determined as
drive off the oxides of nitrogen and then cooled described under procedure using fluoride as a
to room temperature (25± 5)0C. After suitable masking agent. The results are shown in (Table-
dilution with de-ionized water, the contents of the 4). Added copper was recovered accurately from
flask were warmed to dissolve the soluble salts. the other metals.
The solution was then cooled and neutralized
with dilute NH4OH in the presence of 1–2mL of
0.01% ( W/V) tar tr ate
Table-4: Determination of copper in alloys and Steels samples (a. Value given represents the average of triplicate
determination, b. The measure of precision is the standard deviation (S).):

Cu spiked
Sample Certified Reference Recovery
No. Material (Composition, %) Added (µgL -1) Founda (µgL -1) ± Sb(%)
BAS032a, Al-Bronze Allo y
0.10 86.01 100 ± 0.2
1. Cu=85.9, Zn=0.94 Mn=0.27
0.50 85.95 99 ± 0.5
Fe=2.67, Ni=1.16,Al = 8.8
BAS-646, High speed steel, Te=0.90,
0.10 0.102 100 ± 0.2
2. Cr = 4.55,Mo=4.95, V= 1.99
0.50 0.50 100 ± 0.0

5. Conclusions: 6. Acknowledgement:
In this Thesis a new simple, sensitive, selective We are grateful to the authorities of different
and inexpensive technique with Cu(II)-PAN industries for their generous help in supplying
complex was developed for the determination of industrial waste water samples. We are especially
Cu(II) in environmental and industrial waste indebted to DAERS, BUET, Dhaka and the
water samples for continuous monitoring. authorities of analytical Research Division of
Although many sophisticated techniques such as BCSIR Laboratories, Dhaka for analyzing the
pulse polarography, HPLC, AAS, ICP-AES, and samples by AAS.
ICP-MS, are available for the determination of
Cu(II) at trace level in numerous complex 7. References
materials, factors such as the low cost of the
1. G. D. Clayton and F. A. Clayton (Eds.), Patty’s
instrument, easy handling, lack of requirement for Industrial Hygene and Toxicology, Vol. 2A, 3rd edn.,
consumables etc. have caused spectrophotometry John Wiley and Sons, New York, 1981, P.1563.
to remain a popular techniques particularly in 2. P. B. Hammond and Robert P. Beliles, Metals in
laboratories of developing countries with limited “Casarett and Doull’s Toxicology”, C.D. Klassen, M.O.
budget. The sensitivity in terms of relative Amdur and J. Doull (Eds.) 3rd end. Macmillan, New
York, 1986, P. 428.
standard deviation of the present method are very 3. L. Friberg, M. Piscator, G. F. Nordberg and T.
reliable for the determination of Cu(II) in real Kjellstrom (Eds.) “Cadmium in the Environment”,
samples down to µgL-1 levels in aqueous medium 2nd Edn., CRC Press, InC., Cleveland. 1974.
at room temperature (25± 5)0C.

Vol. 1 No. 1 2013 www.chemijournal.com Page | 13

 International Journal of Chemical Studies

4. D.M. Taylor and D.R. Williams, Trace Elemint 25. I. Nukatsuka, A. Nashimura and O. Kunio, Anal.
Medicine and Chelation Therapy, The Royal Society Chim. Acta., 304 (1995) 243.
of Chemistry, Cambridge, 1995, p. 22. 26. P. Job. Ann. Chim. (Paris) 9(1928) 113.
5. M. M. Key, A.F. Henschel, J. Butter, R. N. Ligo and I.R. 27. J.A. Yoe, A. L. Jones, Ind. Eng. Chem. Anal. Ed. 16
Tabershaed (Eds.), “Occuptional Diseases-A Guide (1944) 11.
to Their Recognition”, U. S. Department of health, 28. E.A. Greenberg. S.L. Vlesceri and D.A. Eaton (Eds.)
Education ande Welfare, US Government Printing, “Standard Methods for the Examination of water
Washington, DC, June, 1977,p 265. and wastewater”, 18th ed. American Public Health
6. J.E. Fergusson, The toxicity of heavy element to Association, Washington, D.C., p. 382.
human beings in : “The Heavy Elements : Chemistry, 29. Ch. S.S.S. Murthy and Y. Anjaneyaula, “Heavy Metals
Environmental Impact and Health Effects”, and Organochlorine Level in Kakindada Bay In:
Pergamon Press, Oxford, 1989, p.548. Proceedings of the International Conference on
7. B. Venugopal and T.D. Luckey, “Metal Toxicity in Industrial Pollution and Control Technologies” Y.
Mammals-2”, Plemum Press, New York, 1979,p.76. Anjaneyulu (Ed.), Allied Publishers Limited,
8. Second Annual Report of Carcinogens, Hyderabad, 1997, pp. 747-753.
Environmental Protection agency, NTP, 81-43, Dec., 30. G.A. Parker, “Analytical Chemistry of Molybdmum”,
1981. Springer-Verlag, Berlin, 1983.
9. M. Jamaluddin Ahmed and M. Jobaer Hassan,
Research Journal of Chemistry and Environment.
3(3) (1999) 9.
10. F. Shaohua, Z. Yishan, N. Qidao, and J. Lihua, Fence
Huaxue, 35(2) (1999) 79, (Chem. Abstr., 131 (1999)
37304U.)
11. G. Jiang, W. Xiaoju, T. Yanhong, and L. Zhetl. Guang
puxue Yu Guangpu Fenxi, 19(3) (1999) 474[Chem.
Abstr, 131 (1999) 96547f].
12. M. Yang, C. Gong. G Li, and C. Jin, Fenxi Shiyanshi,
18(3) (1999) 52-54[Chem. Abstr. 131 (1999)
129614w].
13. L. Shutin, and Z. Shulin, Jezin Fenxi, 19(3) (1999)
21[Chem. Abstr, 131(1999) 237200b].
14. S. Kattikeyan, T. P. Rao, C. S. P. lyer and A. D.
Damodaran, Talants., 40(1993) 771.
15. T.P. Rao and T.V. Ramakrishna, Analyst, 107 (1982)
704.
16. J. Hu. W.B. Qi and B. Y. Pu, Mikrochim. Acta., 109
(1992) 295.
17. Jose Anchieta Gomes Neto, H. Bergamin Fo, Elias
Ayres, G. Zagotto and Francisco J. Krug, Anal. Chim.
Acta., 308 (1995) 439.
18. Dr. Md. Rafiqullah and Md. Enamul Haque,
Analytical Sciences, (communicated-2007).
19. A.K. Mukharjee, Analytical Chemistry of Zirconium
and Hafnium, 1st Ed; Pergamon Press, New York,
1970, p. 12.
20. B.K. Pal and B. Chowdhuary, Mikrochim. Acta.,
11(1994) 121.
21. A. L Busev, V.G. Tiptsova and V.M. lvanov, Analytical
Chemistry of Rare Elements, (Eds) Mir Publishers.
Moscow, 1981. p. 385.
22. E.B. Sandell, “Colorimetric Determination of Traces
of Metals”, Interscience, New York. 1965, p. 269.
23. C Bosch Ojeda, A. Garcia de Torres, F. Sanchez Rojas
and J. M. Cano Pavon, Analyst, 112 (1987) 1499.
24. B.K. Pal, K. A. Singh and K. Dutta, Talanta, 39, (1992)
971.

Vol. 1 No. 1 2013 www.chemijournal.com Page | 14

View publication stats