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BS REPORTS
EDTMP is also one of the most
commonly used scale and corrosion
inhibitors in circulating cooling water
systems. It forms stable complexes with
many ions, Ca(II), Mg(II), Fe(II), Zn(II),
Al(III), Fe(III) etc., and the chelators are
often multi-ring.
STUDIES ON APPLICATION OF ANION EXCHANGERS IN REMOVAL OF METAL COMPLEXES WITH EDTMP
Dorota KOŁODYŃSKA, Marzena GĘCA, Zbigniew HUBICKI
DEPARTMENT OF INORGANIC CHEMISTRY
For many years complexing agents have received increasing attention among
researchers. They are widely used in many industries, moreover, they have also
become an integral part of everyday human life. These compounds are capable of
chelating with metal ions to create connections in the form of complexes. Besides
the positive aspects of the use of complexing agents in our lives, there are some
negative ones – the complexing agents affect the bioavailability of the metal ions,
disturbing their natural speciation, which may cause their release from sewage
sludge. However, the largest concern is connected with the lack of their
biodegradability and persistence in the environment [1].
In the group of complexing agents, aminopolycarboxylic acids (APCA),
aminopolyphosphonic acids (APPA) and hydroxoacids (HA) should be mentioned.
They are characterized by good pH, temperature and pressure stability, high water
solubility, high density of functional groups, good compatibility with other
ingredients of formulations.
Phosphonates belong to the group of complexing agents which contain one or
more phosphonic acid groups –PO(OH)2 [2]. The most important in industry and
analytical chemistry are aminopolyphosphonic complexones, which are regarded as
analogues of commonly used chelating agents such as EDTA
(ethylenediaminetetracetic acid) or NTA (nitrilotriacetic acid). In this group
EDTMP (1,2-diaminoethanetetrakis(methylenephosphonic acid)) should be
mentioned.
The main tasks of the presented paper were (1) to test the commercially
available anion exchangers towards such species as Cu(II), Zn(II), Pb(II) and Cd(II)
complexes with EDTMP and (2) to select the anion exchanger that showed the best
performance towards the above-mentioned species and (3) characterize their
structure and physicochemical properties as far as the anionic species sorption is
concerned.
1,2-diaminoethanetetrakis(methylenephosphonic acid) EDTMP (other
abbreviations EDTP, EDTPH, ENTMP, EDTMPO, EDTMPA) is formed by
ethylenediamine, formaldehyde and phosphorus trichloride. Its structure can be
presented as:
EDTMP is effective in inhibiting calcium carbonate scale formation, iron
oxide and hydrated calcium sulfate scale, and the largest extent in the stable
supersaturated solution of calcium sulfate. The loose scale does not decompose at
473 K, therefore, EDTMP is more applicable for the treatment of low pressure
boiler furnace.
Investigations were carried out using the static and dynamic methods, based on
which adsorption parameters were calculated. The exemplary breakthroughs as well
as the mass (Dg) and volume (Dv) distribution coefficients as well as the working
(Cw) and total (Ct) ion exchange capacities (mg/cm3) for Cu(II), Zn(II), Pb(II) and
Cd(II) in the presence of EDTMP on Lewatit MonoPlus M 500 in the M(II)-
EDTMP=1:2 system at pH 9.0 are presented below:
During research it was found that phase contact time, pH, temperature and
initial metal concentration influence the effectiveness of heavy metal complexes
sorption in the presence of EDTMP on Lewatit MonoPlus M 500 and Lewatit MP
62. Batch equilibrium was relatively fast and it reached equilibrium after about 60
min of contact. The ion exchange process, which is pH dependent showed
maximum removal of Cu(II) at pH 9.0 (initial concentration of 1× 10-3
M) only for
the strongly basic anion exchanger. It was shown that temperature slightly affects
sorption efficiency. The pH dependence of ion exchange may suggest that the metal
ions are adsorbed according to an ion exchange mechanism.
References:
[1] A.T. Stone, M.A. Knight, B. Nowack, Speciation and chemical reactions of phosphonates chelating agents in aqueous media, in: Chemicals in the
Environment, R.L. Lipnick, R.P. Mason, M.L.Phillips, Ch.U. Pittman, Jr, (eds),
ACS Symposium Series 806, American Chemical Society, Washington,
[2] B. Nowack, J.M. VanBriesen, Chelating agents in environment, in: Biogeochemistry of chelating agents, B. Nowack, J.M. VanBriesen(eds.), ACS
Symposium series 910, pp. 1-18.
System
/Ion exchanger
D
g
D
v
C
w
C
t
Lewatit MonoPlus M 500
Cu(II)-
EDTMP=1:2
2
16.7
7
2.0
0
.002
0
.004
Zn(II)-
EDTMP=1:2
2
4.2
8
.0
0
.003
0
.005
Pb(II)-
EDTMP=1:2
1
90.6
6
3.3
0
.007
0
.013
Cd(II)-
EDTMP=1:2
4
98.4
1
65.6
0
.014
0
.018
INVESTIGATION OF REDUCTION MECHANISM OF CHROMIUM
(VI) IONS IN QUATERNARY AMMONIUM SALT EXTRACTION
PROCESS
Zbigniew HUBICKI and Grzegorz WÓJCIK
DEPARTMENT OF INORGANIC CHEMISTRY
Chromium(VI) is more toxic than chromium(III) due to its toxic effects on
biological systems: nasal septum, asthma, bronchitis, pneumonia, inflamation of the
larynx and liver, skin allergies, dermatitis which can occur after inhalation or skin
contacts with chromium(VI) compounds. For this reason large amounts of
chromium(VI) must be reduced to the safe level. The elimination of toxic and
hazardous chemical substances such as chromium (VI) from waste effluents is a
major concern worldwide. Among all heavy metals, copper, chromium and zinc
ingestion beyond permissible quantities causes various chronic disorders in human
beings [1].The aim of these studies was to investigate of extraction mechanism of
chromium(VI) ions from water solution in the pH range from 1 to 7 by using
Aliquat 128 in toluene. Aliquate 128 is methyltrioctylammonium chloride and was
supplied by Aldrich.
Fig. 1. Molecular structure of Aliquat 128
All experiments were carried out at ambient temperature. Aqueous solution
containing a known amount of Cr (VI) (100ppm) was mixed with 0.1% of Aliquat
128 diluted with toluene at an organic/aqueous (O/A) ratio of 1:1 in a separatory
funnel. The aqueous layer was analyzed for remaining Cr by AAS and Cr(VI)
spectrophotometrically with diphenylcarbazide.
Experimental result (Fig. 2.) showed that the extraction equilibrium takes place at
about 5min.
In acidic medium (pH < 1) Cr (VI) ion exists partly as H2CrO4. At pH between 2
and 6 there is an equilibrium between Cr2O72−
and HCrO4- ionic species and under
alkaline conditions (pH > 8) it exists predominantly as chromate anion[2]. Aliquat
128 shows the maximum extraction efficiency (100%) for the uptake of Cr (VI) at
pH of 1.5. With increase in pH to 3.5, and 7 the extraction efficiency decreases to
90 and 50%, respectively.
The extraction equilibrium of Cr(VI) by Aliquat 128 can be represented
stoichiometrically by the following equations:
R1(R2)3N+Cl
- + HCrO4
- ⇌ R1(R2)3N
+HCrO4
- + Cl
-
2R1(R2)3N+Cl
- + Cr2O7
2- ⇌ (R1(R2)3N
+)2 Cr2O7
2- + 2Cl
-
2R1(R2)3N+Cl
- + CrO4
2- ⇌ (R1(R2)3N
+)2CrO4
2- + 2Cl
-
Fig. 2. Effect of phase contact time on values of extraction factor for Cr(VI) ions on
Aliquat 128 in pH range 1.5-7.
The investigations of chromium(III) and(VI) speciation allowed to notice that
chromium(VI) is reduced to chromium(III) ions at pH 1.5. The reduced
chromium(III) ions are not retained by Aliquate 128 organic phase but are
transferred from internal to aqueous solution. Similar observation during sorption of
chromium (VI) ions on strongly basic anion exchanger were reported[3,4].
The metal loaded solvent was stripped with alkaline solution of 1M NaOH
+1M NaCl to recover the extracted Cr (VI) by mixing for 5 min.
References:
[1] R.S. Prakasham, J.S. Merrie, R. Sheela, N. Saswathi, S.V. Ramakrisha,
Environmental Pollution 104 (1999) 421–427.
[2] R. Ansari, Acta Chimica Slovenica 53 (2006) 88–94.
[3] G. Wójcik, Z. Hubicki, P. Rusek, Przemysł Chemiczny, 90 (2011) 2153.
[4] G. Wójcik, Z. Hubicki, P. Rusek, Przemysł Chemiczny, 92 (2013) 82.
EVALUATION OF EFFECTIVNESS OF INTERMEDIATE AND
STRONGLY BASIC ANION EXCHANGERS IN REMOVAL OF
DIRECT AND REACTIVE DYES FROM AQUEOUS SOLUTIONS
AND WASTEWATERS
Monika WAWRZKIEWICZ, Zbigniew HUBICKI
DEPARTMENT OF INORGANIC CHEMISTRY
INTRODUCTION
Dyeing is a fundamental operation during the textile fiber processing. This
operation causes the production of more or less coloured wastewaters, depending on
the degree of fixation of the dyes on the substrates, which varies with the nature of
the substances, the desired intensity of coloration, and the application method.1 The
dye bearing effluents are considered to be a very complex and inconsistent mixture
of many pollutants ranging from organic-chlorine based pesticides, alkalis, oils,
detergents, salts of organic and inorganic acids to heavy metals [1-4]. Ion exchange
is a very versatile and effective tool for the treatment of aqueous hazardous wastes.
The role of ion exchange in dye effluents treatment is to reduce the magnitude of
hazardous load by converting them into a form in which they can be reused, leaving
behind a less toxic substance in its place or to facilitate ultimate disposal by
reducing the hydraulic flow of the stream bearing the toxic substance. Another
significant feature of the ion exchange process is that it has the ability to separate as
well as to concentrate pollutants.
The adsorption of the dye C.I. Reactive Black 5 (RB5) and C.I. Direct Blue 71
(DB71) from aqueous solution on the intermediate and strongly basic anion
exchangers (Lewatit MonoPlus MP64, Lewatit MonoPlus MP500 and Lewatit
MonoPlus M500) was investigated in order to identify the ability of these materials
to remove textile dyes from wastewaters. For this purpose a series of batch tests
were carried out as a function of contact time (1 min-24 h), dye concentration (100,
500, 1000 mg/L) and auxiliaries presence (NaCl, Na2SO4, surfactant).
RESULTS AND DISSCUSSION
The most famous adsorption models in linearized form for single-solute
systems are the Langmuir and Freundlich. The experimental data obtained in the
present work were tested with these equations. The Langmuir constants Q0 and b
were calculated from the slope and intercept of the plot Ce/qe vs Ce. The plot log qe
versus log Ce should produce a straight line with the slope 1/n and the intercept of
kF. The applicability of isotherm equations was compared by judging the correlation
coefficients (R2). It was found that the dyes sorption on the intermediate and
strongly basic anion exchange resins were well described by the Langmuir
isotherm. For RB5 dye, the values of the monolayer sorption capacities on Lewatit
MonoPlus MP500, Lewatit MonoPlus MP64 and Lewatit MonoPlus M500 were
found to be 1170.5 mg/g (R2=0.997), 592.8 mg/g (R
2=0.989) and 5.2 mg/g
(R2=0.992), respectively. The intermediate and strongly basic anion exchangers
were characterized by lower affinity for the direct dye. The Q0 values obtained from
the Langmuir model of adsorption were found to be 523.64 mg/g, 420.4 mg/g and
2.02 mg/g for Lewatit MonoPlus MP500, Lewatit MonoPlus MP64 and Lewatit
MonoPlus M500, respectively. Taking the above into account, it can be stated that
not only anion exchangers basicity but also the type of dye play an important role in
sorption processess.
The presence of inorganic salts and surfactant such as NaCl, Na2SO4 and SDS
in the solution during the dye adsorption on the anion exchangers was examined
because these substances are typically present in real wastewaters. The following
systems were studied: 100 mg/L of RB5 or DB71 in 25-100 g/L NaCl or Na2SO4 as
well as 100 mg/L of RB5 or DB71 in 0.1-1.0 g/L SDS. The sorption of the dyes on
Lewatit MonoPlus MP500 was slightly reduced in the presence of both electrolytes.
The amounts of RB5 retained by the strongly basic resin MP500 at equilibrium
dropped from 10 mg/g to 9.3 mg/g and from 10 mg/g to 9.2 mg/g with the
increasing amount of NaCl and Na2SO4, respectively. It is due to a competition
between Cl- and SO4
2- anions and the anionic dye. Direct Blue 71 sorption on the
anion exchangers was not influenced by the presence of NaCl and Na2CO3. No
influence of SDS on the dyes sorption by the anion exchangers was observed.
The strongly basic anion exchanger MP500 proves to be capable of color
removal of reactive dye wastewater providing 89% color removal after only 15 min
of adsorption process and reaching 99.9% color removal after 3 h. This percentage
of color removal attained for the model textile wastewater is very high and suggests
that Lewatit MonoPlus MP500 with very good sorption characteristics could be a
promising adsorbent for real textile wastewaters containing reactive dyes.
The adsorption of the dyes on the anion exchangers followed the pseudo-
second order kinetics.
Dye desorption from Lewatit MonoPlus MP500 was effective using 1 M HCl
in 90% CH3OH.
CONCLUSION
The above results indicate that the anion exchange sorption is promising
treatment for the removal of RB5 dye from aqueous solutions and real textile
streams.
References:
[1] N. Ouazene, A. Lounis, Color. Technol. 127 (2011) 1.
[2] S.T. Ong, Ch.K. Lee, Z. Zainal, Aust. J. Basic& Appl. Sci. 3 (2009) 3408.
[3] C.H. Liu, J.S. Wu, H.C. Chiu, S.Y. Suen, K.H. Chu, Water Res. 41 (2007) 1491.
[4] Z.P. Sandić, A.B. Nastasović, N.P. Jivić-Jovičić, A.D. Milutinović-Nikolić,
D.M. Jovanović, J. Appl. Polym. Sci. 121 (2011) 234.
STUDIES OF SEPARATION AND SORPTION OF METAL IONS ON
THE CHELATING RESIN WITH PARTICULAR CONSIDERATION
OF NOBLE METAL IONS
Anna WOŁOWICZ, Zbigniew HUBICKI,
DEPARTMENT OF INORGANIC CHEMISTRY
The preparation of functionalized polymers containing ion-selective ligands
allows to use sorption technology for the separation and recovery of valuable metals
e.g. noble metal ions, for removal of toxic and base metal ions from environmental
sources, waste materials, metallurgical etc. Nowadays strong efforts are directed on
the development and broader application of the chelating resin of polyacrylate
matrix in water treatment, food processing, purification of drugs, antibiotics and
vitamins, wastewaters treatment, dye removal as well as in recovery, removal,
preconcentration and separation of selected noble metal ions [1-9]
.
The aim of research was to study the possibility of applied the chelating resin
for metal ions separation and sorption from chloride and chloride-nitrate solutions
with particular consideration of noble metal ions. The properties of chelating resin
used in this studies is presented in Table 1. Moreover, the working ion-exchange
capacities as well as the weight and bed distribution coefficients were determined
from the metal ions breakthrough curves. The kinetics, equilibrium and desorption
of loaded metal ions were performed.
Table 1. Characteristics of the ion exchanger.
Description Purolite S-984
Structure Macroporous
Type Weak Base / Chelating
Functional groups polyamine - mixed primary, secondary and
tertiary amines
Ionic form as shipped Free base
Matrix Polyacrylate
Moisture Retention 45 - 55 % Cl- form
Temp. Limit 373 K Cl- form
Total exchange
capacity [eq/cm3]
2.7
Sorption recovery of palladium(II), platinum(IV) and gold(III) from the
chloride and chloride-nitrate(V) solutions on the polyacrylate Purolite S-984 resin
was investigated. The studies showed that Purolite S-984 possesses high affinity for
noble metal ions in both single and tertiary component solutions. Purolite S-984
was found to be the most effective one for the sorption of gold(III) as its
breakthrough capacity and sorption capacity were found to be 0.2125 g/cm3 and
0.3248 g/cm3 respectively in 0.1 M HCl. Decrease of the working ion exchange
capacities with the hydrochloric acid concentration increase can be easily observed.
97.7 % reduction of this capacity was observed for Au(III) and for Pd(II) whereas
for Pt(IV) of 90.6 %. As follows from the kinetic studies, the sorption process is
fast and the time required to reach the system equilibrium is short. The time
required to reached equilibrium by the system is equal to 15 min - 0.1 M HCl; 120
min – 1.0 M HCl; 240 min – 3.0 M HCl, whereas for the HCl-HNO3 solutions this
time is in the range 120-240 min. The increasing effect of competitive sorption with
the increasing chloride ions concentration is observed which results in longer time
required to reach equilibrium in the solutions of higher HCl acid concentration.
The pseudo-second order kinetic equation fits well the experimental results.
Moreover, the changes of experimental conditions contribute to the highest metal
ions removal. The agitation speed effect is observed only at the beginning of the
sorption process until the equilibrium is reached. At 120 гpm agitation speed the
kinetics of Pd(II) sorption is slower, the time required to reach equilibrium is longer
than for 150 and 180 гpm speed of agitation and is equal to 180 min (120 гpm), 60
min (150 гpm) and 30 min (180 гpm), respectively. Then the values of the sorption
capacities are as high as possible and equal to 50 mg/g for all cases. The ion
exchange resin beads size also affect the sorption efficiency of Pd(II) but only at the
beginning of the sorption. With the decrease of the ion exchange resin beads size
the qt values reach higher values. The amount of sorbed Pd(II) increased slightly
with the temperature changes from ambient to higher with the 0-15 min phases
contact time but 313 and 333 K temperatures gave similar results in the whole
phases contact time. The anion exchange resin capacity is high enough - all Pd(II)
ions to be removed quantitatively from the 0.1 M HCl – x mg Pd(II)/L (where x =
100, 500 or 1000) solution. The sorption capacity was as follows: 10 mg/g, 49.99
mg/g and 99.98 mg/g, respectively. The initial Pd(II) concentration affects the time
required to reach the system equilibrium. The Langmuir maximum sorption
capacity for Purolite is equal to 504.3 mg/g. Purolite S-984 can be regenerated
using different experimental conditions with different efficiency and after the
desorption process the capacity of resin remains high. The separation of noble metal
ions from the tertiary component solutions is difficult and was not achieved by the
applied eluting agents. Purolite S-984 sorbed all noble metal ions from the tertiary
component Pd(II)-Pt(IV)-Au(III) solutions without preference for any of them.
References:
[1] F. Helfferich, Ion Exchange, McGraw Hill, New York 1962.
[2] C. E. Harland, Ion Exchange: Theory and Practice, Second Ed., The Royal
Society of Chemistry, Cambridge 1994.
[3] H. Hubicka, D. Kołodyńska, Hydrometallurgy, 62 (2001) 107.
[4] Z. Hubicki, G. Wójcik, Desalination, 197 (2006) 82.
[5] Z. Hubicki, M. Leszczyńska, Desalination, 175 (2005) 289.
[6] O.N.Kononova, N.G. Goryaeva, O.V.Dychko, Natural Sci., 1 (2009) 166.
[7] I. Matsubara, Y. Takeda, K. Ishida, Fresenius' J. Anal. Chem., 366 (2000) 213.
[8] A.A. Blokhin, N.D. Abovskii, Y.V. Murashkin, Russ. J. App. Chem., 80
(2007) 1058.
[9] A. Da browski, Z. Hubicki, P. Podkościelny, E. Robens, Chemosphere, 56 (2004) 91.
http://rd.springer.com/search?facet-author=%22A.+A.+Blokhin%22http://rd.springer.com/search?facet-author=%22N.+D.+Abovskii%22http://rd.springer.com/search?facet-author=%22Yu.+V.+Murashkin%22http://www.sciencedirect.com/science?_ob=RedirectURL&_method=outwardLink&_partnerName=27983&_origin=article&_zone=art_page&_linkType=scopusAuthorDocuments&_targetURL=http%3A%2F%2Fwww.scopus.com%2Fscopus%2Finward%2Fauthor.url%3FpartnerID%3D10%26rel%3D3.0.0%26sortField%3Dcited%26sortOrder%3Dasc%26author%3DDa%25CC%25A7browski,%2520A.%26authorID%3D7101722036%26md5%3D2a6e2ee03b132a460e8310a31ddd47aa&_acct=C000059500&_version=1&_userid=4479552&md5=3f244e28a29c5b3de5c30c69ecbd7ad1http://www.sciencedirect.com/science?_ob=RedirectURL&_method=outwardLink&_partnerName=27983&_origin=article&_zone=art_page&_linkType=scopusAuthorDocuments&_targetURL=http%3A%2F%2Fwww.scopus.com%2Fscopus%2Finward%2Fauthor.url%3FpartnerID%3D10%26rel%3D3.0.0%26sortField%3Dcited%26sortOrder%3Dasc%26author%3DHubicki,%2520Z.%26authorID%3D7003490656%26md5%3Dc062b9a689197d06d7f88196cf0aaac1&_acct=C000059500&_version=1&_userid=4479552&md5=f589433b3c84de28995753b80d683df2http://www.sciencedirect.com/science?_ob=RedirectURL&_method=outwardLink&_partnerName=27983&_origin=article&_zone=art_page&_linkType=scopusAuthorDocuments&_targetURL=http%3A%2F%2Fwww.scopus.com%2Fscopus%2Finward%2Fauthor.url%3FpartnerID%3D10%26rel%3D3.0.0%26sortField%3Dcited%26sortOrder%3Dasc%26author%3DPodko%25C5%259Bcielny,%2520P.%26authorID%3D6603159248%26md5%3D6a67249beb4640a639fa2dc6a96a1b60&_acct=C000059500&_version=1&_userid=4479552&md5=0d5df093e54cada16810b1bd535ddbechttp://www.sciencedirect.com/science?_ob=RedirectURL&_method=outwardLink&_partnerName=27983&_origin=article&_zone=art_page&_linkType=scopusAuthorDocuments&_targetURL=http%3A%2F%2Fwww.scopus.com%2Fscopus%2Finward%2Fauthor.url%3FpartnerID%3D10%26rel%3D3.0.0%26sortField%3Dcited%26sortOrder%3Dasc%26author%3DRobens,%2520E.%26authorID%3D7005748372%26md5%3D94fde200b7f3aaed0c2d18ffe045ee2c&_acct=C000059500&_version=1&_userid=4479552&md5=5d29fd053574565ceaf8c6b290d51043http://www.sciencedirect.com/science/journal/00456535
FLUORESCENCE QUENCHING PROCESS OF PORPHYRIN
SYSTEMS AS A RESULT OF INTERACTIONS WITH
BIOLOGICALLY ACTIVE COMPOUNDS
Magdalena MAKARSKA-BIAŁOKOZ
DEPARTMENT OF INORGANIC CHEMISTRY
The porphyrin systems are characterized as the substances showing high
intensity of absorption and emission and ability to electron transfer, as well as
sensibility for the subtle changes proceeding in the reaction environment.
Spectroscopic properties of this class of compounds, primarily their fluorescence
intensity, are subject to limitation as a result of the change of their structure during
interactions with different aromatic compounds, such as xanthine and its
derivatives.
One of the examples of such compounds is caffeine (1,3,7-trimethylxanthine),
applied as the component of many drugs and medicaments. The association
processes occurring between chosen water-soluble porphyrins (4,4’,4’’,4’’’-
(21H,23H-porphine-5,10,15,20-tetrayl)tetrakis-(benzoic acid) (H2TCPP),
5,10,15,20-tetrakis(4-sulfonato phenyl)-21H,23H-porphine (H2TPPS4), 5,10,15,20-
tetrakis[4-(trimethylammonio) phenyl]-21H,23H-porphine tetra-p-tosylate
(H2TTMePP), 5,10,15,20-tetrakis(1-methyl-4-pyridyl)-21H,23H-porphine tetra-p-
tosylate (H2TMePyP) and the Cu(II) complexes of H2TTMePP and H2TMePyP) and
aromatic compounds (caffeine, nucleic bases, nucleosides and nucleotides) were
monitored before with use of UV-VIS and emission spectroscopy techniques [1, 2].
The spectroscopic data obtained during these studies became the base for the
determining both association (KAC of the order of magnitude of 103-10
5 mol
-1) and
fluorescence quenching constants (KSV of the order of magnitude of 103 mol
-1) in
the systems examined. Taking into consideration the 1:1 model of complex
formation, the calculations of the association constants were done applying the
equation based on Bjerrum function modified by Beck,
][][1
][
1
110 PLK
LKA
where A is the absorbance; 0, the molar absorbance index for starting porphyrin; 1
and K1 are the molar absorbance index and the gradual binding constant,
respectively, when [L] and [P] stand for the analytical concentration of ligand
(caffeine) and porphyrin. Whereas the fluorescence quenching constants were
determined using Stern-Volmer equation,
][10
QKF
FSV
where F0 and F are the fluorescence intensities in the absence and presence of
quencher, respectively; [Q] is the concentration of quencher, KSV is the Stern-
Volmer quenching constant. For all calculations the non-linear curve-fitting
procedure based on Marquardt–Levenberg algorithm from Sigma Plot (version 9.0,
Jandel Corp.) database program, modified for the particular systems, was employed.
639.5-642.5 nm
H2TTMePP 3.27*10-7 mol dm-3 + caffeine
CM porph. * 10-7
2.0 2.2 2.4 2.6 2.8 3.0 3.2
flu
ore
scen
ce (
a.u
.)
6
8
10
12
14
16
18
exc.412 nm
em.642.5nmem.max
em.639.5nm
[nm]
550 600 650 700 750
flu
ore
scen
ce (
a.u
.)
0.00
5.00
10.00
15.00
20.00
Fig. 1 The process of fluorescence quenching during interactions between H2TTMePP and
caffeine: the dependence of fluorescence intensity vs. porphyrin molar concentration (left
plot) and the decrease of fluorescence intensity (emission spectra, right plot).
The obtained results show that caffeine can interact with water-soluble
porphyrins and through formation of stacking complexes is able to quench their
ability to emission. The bathochromic effect and hypochromicity of the Soret
maximum in the absorption spectra of the particular porphyrins, as well as the
fluorescence quenching in emission spectra point at the decrease of luminescence
properties of water-soluble porphyrins examined and can be predominantly
attributed to the process of static quenching. The magnitude of calculated KAC and
KSV constants depends strongly on the spatial structure both the particular porphyrin
and the aromatic compound. The studies described in this report are indispensable
for investigating of the processes related to porphyrin chemistry (especially the
phenomenon of fluorescence quenching), in the development of new classes of
modified porphyrins of special properties or artificial receptors, as well as in
monitoring of the porphyrin-toxic substances interactions or environmental and
sanitary parameters, where there is a great demand for different kinds of chemical
sensors.
References:
[1] M. Makarska-Bialokoz, J. Fluoresc., 22 (2012) 1521.
[2] M. Makarska-Bialokoz, Cent. Eur. J. Chem., 11 (2013) 1360.
ADSORPTION OF PHOSPHATE(V) ON BENTONITE
Agnieszka GŁADYSZ-PŁASKA, Marek MAJDAN DEPARTMENT OF INORGANIC CHEMISTRY
Among the numerous contaminants present in wastewater, phosphorus is
particularly dangerous. After a treatment process, it is still found in sewage sludge.
If the element enters the environment, it may cause eutrophication, which is a
serious threat to the water environment. The environmental effects, however, are
dependent on the chemical form of phosphorus. By using a speciation analysis, it is
possible to determine a selected chemical form of phosphorus and predict its effects
on the environment. Phosphorus is found in the form of phosphates in wastewater,
which includes organic phosphate, inorganic phosphate (orthophosphate) and
polyphosphate (particulate phosphorus). Sources of phosphorus are found in
excessive use of synthetic fertilisers, animal-based fertilisers, detergents, pigments,
water treatment and mineral processing. Phosphorus is also used in consumer
products and industrial processes that involve particles of colloidal nature [1, 2].
Several methods are available for removing phosphate from aqueous solution,
such as chemical precipitation, solvent extraction, and adsorption. Among these,
adsorption is an attractive method due to its high efficiency, ease of handling, and
availability of different adsorbents. Various kinds of new adsorbents for removing
and recovering phosphate have been reported, among which natural clays and their
composites are considered as particularly effective, low-cost, and chemical stability
[3].
The aim of the investigation was to determine the suitability of the bentonite
for removal of phosphate from aqueous solutions. Various parameters, including
initial phosphate(V) concentration, operating temperature, and solution pH, have
been investigated in batch kinetic experiments and desorption studies. All the
experimental results have been analysed by applying adsorption isotherms and
batch kinetic models. The bentonite saturated by hexadecyltrimethylammonium
bromide was used as an organoclay. The initial and the equilibrium concentrations
of phosphate ions in the aqueous phase were determined by spectrophotometric
phosphormolybdic method [4].
The bentonite is an effective sorbent for removing phosphate(V) from aqueous
solution. The kinetics of adsorption follows the pseudo-second-order model,
indicating that the adsorption was controlled by chemisorption process chich was
found to be endothermic and spontaneous. During studying the pH influence on the
adsorption process the amount of phosphate adsorbed onto HDTMA-bentonite at
pH 6.7 was the greatest (Fig. 2).
Fig. 1. The effect of time on the phosphate(V) adsorption at 293 K, pH = 6.1 (cin =0.0005M)
on HDTMA-bentonite.
Fig. 2. The effect of pH on the phosphate(V) adsorption at 293 K, (cin =0.0005M) on
HDTMA-bentonite.
References:
[1] Ch. Hinz, Geoderma 99 (3–4) (2001) 225–243.
[2] W. Jiang, S. Zhang, X. Shan, M. Feng, Y.G. Zhu, R.G. McLaren, Environ.
Pollut. 138 (2005) 278–284.
[3] T.K. Naiya, A.K. Bhattacharya, S. Mandal, J. Hazard. Mater. 163 (2009) 1254-
1264.
[4] Z. Marzenko, M. Balcerzak, Spektrofotometryczne metody w analizie
nieorganicznej, Wydawnictwo Naukowe PWN SA, Warszawa, 1998.
2 3 4 5 6 7 8 910
15
20
25
30
35
40
45
pHeq
adso
rpti
on P
( %
)
t (h)0 2 4 6 8 10
ad
sorp
tio
n P
(%
)
20
40
60
80
100
LUMINESCENCE SPECTRA OF URANIUM ON CLAY
Agnieszka GŁADYSZ-PŁASKA, Marek MAJDAN DEPARTMENT OF INORGANIC CHEMISTRY
The time-resolved laser-induced fluorescence spectroscopy (TRLFS), applied
as the method to study the kind of U(VI) surface complexes on clays, provides the
information about both lifetime and spectral characteristics of the adsorbed species,
which allows to point out the number of different species and their spectral identity.
The TRLFS technique can supply new insight into the actinide surface
complexation and, therefore, it can contribute to developed knowledge of actinide
behaviour in the environment. Figure 1 shows the typical fluorescence emission
spectrum of the free uranyl ion ([U(VI)] = 5·10-6
mol/dm3) at pH = 6.5 and
adsorbed on the clay (Fig. 1). The lifetimes of U(VI) fluorescence species were
determined from the bi-exponential fit analysis of the obtained data indicating at
least two surface species. As follows from this analysis, one point on the decay
curve represents the value of fluorescence intensity integrated for all wavelengths at
a given delay time. The fluorescence lifetimes of two U(VI) surface species were
calculated from Eq. (1):
y=y0 + A1e-(x-x0)/t1
+ A2e-(x-x0)/t2
(1)
The TRLFS measurements of uranium(VI) species yield two kinds of information:
the position of the fluorescence emission bands and the fluorescence lifetime. The
fluorescence lifetime varies depending on the number of neighbouring water
molecules surrounding the uranium(VI) atom. The TRLFS spectra of the sorbed
U(VI) surface species on sepiolite at pH 6.5 indicate at least two surface species
with two different fluorescence lifetimes, i.e., one short- and one long- lived
species. The calculated average fluorescence lifetimes of the short- (τ1) and long-
lived (τ2) species are summarized in Table 1. The shorter fluorescence lifetimes
indicate more water molecules in the coordination environment of the respective
adsorbed U(VI) surface species because water molecules quench the fluorescence
[1]. On this basis, it can be assumed that U(VI) forms two surface species on clay
(sepiolite, bentonite and red clay) which differ in the amount of water molecules in
their coordination environment.
Comparison of the mean values of the respective fluorescence lifetimes obtained in
the presence and absence of ODTMA (octadecyltrimethylammonium) allows to
conclude that in the presence of ODTMA, the fluorescence lifetimes of both species
are significantly longer. The shorter fluorescence lifetimes of U-sepiolite indicate
more water molecules in the coordination environment of the respective adsorbed
U(VI) surface species. Baumann et al. [1] attributed the surface species with the
shorter fluorescence lifetime to the bidentate mononuclear inner-sphere surface
complex in which U(VI) is bound to two reactive hydroxyl groups at the broken
edge linked to one Al. Arnold et al. [2] ascribed the surface species with the shorter
fluorescence lifetime to an inner-sphere bidentate surface complex, in which U(VI)
binds to the aluminol groups of edge-surfaces of muscovite. Both researchers
interpreted the surface species with the significantly longer fluorescence lifetimes
as an amorphous U(VI) condensate or nanosized clusters of polynuclear uranyl
surface species.
450 500 550 600 650 7000
500000
1000000
1500000
450 500 550 600 6500
500000
1000000
1500000
450 500 550 600 650 7000
500000
1000000
1500000U-ODTMA-sepiolite
U-sepiolite([U(VI)] = 5·10
-6 mol/dm
3)
at pH = 6.5.
Wavelength (nm)
Flu
ores
cenc
e in
tens
ity
(a.u
.)
A) B)
Fig. 1. Fluorescence emission spectrum of U(VI) adsorbed on the sepiolite (A) and an
aqueous solutions ([U(VI)] = 5∙10-6
mol/dm3) at pH 6.5 (B).
Table 1. Comparison of fluorescence lifetimes (τ1 and τ2 ) of uranium species.
System τ1 , ns τ2, ns
U(VI) (acetale) 2200±320 7320±450
U-sepiolite 2420±430 37950±5710
U-ODTMA-sepiolite 3523±160 45400±1830
U-bentonite Volclay 1090±102 67400
U-PO4-bentonite Volclay 1290 70100
U-red clay 1060 26400
U-PO4-red clay 6530 27550
U-gibbsite 322±25 [1] 5180±400 [1]
U-silica gel 138400±52900 [4] 361800±103200 [4]
U-kaolinite 5900±700 [3] 42500±1700 [3]
U-HA-kaolinite (HA-
humic acid)
4400±600 [3] 30900±3600 [3]
References:
[1] N. Baumann, V. Brendler, T. Arnold, G. Geipel, G. Bernhard, J. Colloid. Interf.
Sci. 290 (2005) 318-324.
[2] T. Arnold, T. Zorn, H. Zanker, G. Bernhard, H. Nitsche, J. Contam. Hydrol. 47
(2001) 219–231.
[3] A. Křepelovǎ, Influence of humic acid on the sorption of uranium(VI) and
americium(III), Disseration, University of Technology, Dresden, 2007.
[4] P. Trepte, Sorption von Radionukliden an Tongestein: Spektroskopische
Referenzdaten. Diploma thesis, University of Applied Science, Dresden (2006).
THE APPLICATION OF MICRO- AND MESOPOROUS
ADSORBENTS FOR ENRICHEMNT AND DETERMINATION OF
CHOSEN ELEMNTS BY USING ATOMIC ABSORPTION
SPECTROMETRY METHODS
Ryszard DOBROWOLSKI
DEPARTAMENT OF ANALYTICAL CHEMISTRY
AND INSTRUMENTAL ANALYSIS
The simplicity of the sol-gel method allows to synthesize wide range of hybrid
porous materials based on silica, which are widely exploited in membranes,
adsorption and catalysis. The sol-gel method provide the opportunity of the
incorporation of different organic groups into the materials structure by co-
condensation of tetraethoxysilane (TEOS) with different functionalized silanes. The
functionalization of the surface layer can affect the sorption characteristics of
obtained materials.
The hydrolysis of TEOS followed by its co-condensation with appropriate
organosilicas monomers leads to the formation of functionalized amorphous
polysiloxane xerogels (APX). The sol-gel method give a possibility to design and
keep control over chemical and physical properties of synthesized micro- and
mesoporous materials.
For the first time ordered mesoporous silicas (OMSs) called M41S were
synthesized in 1990. In 1998 hexagonally arranged and highly ordered mesoporous
silicas (OMSs) were produced at the University of California, Santa Barbara. OMSs
are characterized by tuneable pores size, thick pore walls, high specific surface area,
and good textural properties.
The possibility of functionalization and easy one-step synthesis of the OMSs
and APX makes them promising candidates for environmental applications and for
catalytic and adsorption processes. Functionalized silicas have found applications as
adsorbents of many species including biomolecules, pharmaceuticals and heavy
metal ions. However, the amount of information regarding the application of
mesoporous organosilica materials for removal of noble metals is poor.
Platinum is the most relevant noble metal and due to is high cost and limited
world reserves the recovery of its from waste waters and used converters is a very
important issue. The solution of the problem may be functionalized organosilicas
exhibiting substantial adsorption affinity towards noble metal ions.
In this work the amine-functionalized APX and OMS were synthesized,
characterized and compared as sorbents for Pt(II) ions adsorption.
Synthesis of modified SBA-15 and APX materials were carried out using sol-
gel method. In order to synthesize ordered mesoporous organosilicas (OMOs) 2g of
Pluronic 123 was dissolved in 60 mL of 2M HCl and 11 mL of deionized water.
After 8h of stirring at 40°C tetraethoxysilane (TEOS) was added into solution. After
15 minutes the silane coupling agent was added. The mixture was next stirred for
24h at 40°C and aged for 48h at 100°C. The obtained materials were washed by
using deionized water, filtered and dried at 70°C. Removal of template was done by
tree-time extraction with EtOH at 70°C.
In order to synthesize APX the NH4F was dropped the solution of TEOS
which was dissolved in 15 mL of EtOH. After 15 minutes silane coupling agent was
added into mixture. After two days resulting gel was pounded and dried in vacuum.
The initial molar ratios of monomers used for the one-step synthesis were as
follows: a) (TEOS/ATES=19/1), b) (TEOS/ATES=18/2), c) (TEOS/TMPD=19/1),
d) (TEOS/TMPD=18/2) both for OMOs and APX.
The values of specific surface areas obtained for OMOs were in the range
740–840 m2/g, whereas for APX the corresponding values were lower (280–520
m2/g). It was found that in the case of APX the efficiency of amine groups
incorporation into the final material structure is higher (70-80%) than for OMOs.
The adsorption of Pt(II) ions is strongly pH-dependent. In the case of ATES-
functionalized samples, the highest adsorption capacity is obtained for the
equilibrium pH of 2.5 and 3.3 for OMOs and APX, respectively. The maximum
uptake for TMPED- functionalized SBA-15 is achieved at pH around 2.5, and for
TMPED- functionalized APX the plateau is observed in the range of pH 0.8–5.5.
The kinetic of Pt(II) adsorption onto studied APX is generally slower than in the
case of amine-functionalized SBA-15. In Fig. 1 the effect of chlorides on the
adsorption of Pt(II) is presented. In the case of OMOs and APX modified by ATES
the presence of chlorides concentration higher than 0.01 mol/L causes drastic
decrease of the adsorption by about 80–90 %. Only in the case of TMPD-
functionalized APX chlorides do not cause such drastic decrease of adsorption. The
adsorption isotherms of Pt(II) ions are presented in Fig. 2. The high values of
adsorption capacity makes these materials promising candidates for Pt(IV) removal
and preconcentration.
Fig.1. Impact of chlorides on the Pt(IV)
adsorption onto APX and SBA-15
(TEOS/functionalizing monomer=18/2); m
= 0.05 g, V = 50 ml, T = 25ºC.
Fig.2. Adsorption isotherms of Pt(IV) on
functionalized SBA-15 and APX in respect
to thiourea concentration; (TEOS/
functionalizing monomer=18/2); m = 0.05
g, V = 50 ml, T = 25ºC.
SYNTHESIS, CHARACTERIZATION AND APPLICATION OF SBA-
15 MATERIALS FOR ENRICHMENT AND DETERMINATION OF
CHOSEN METALS USING ATOMIC ABSORPTION
SPECTROMETRY METOD
Joanna DOBRZYŃSKA
DEPARTAMENT OF ANALYTICAL CHEMISTRY
AND INSTRUMENTAL ANALYSIS
Since the discovering in 1998 mesoporous SBA-15 materials, due to their
tunable pores size, thick pore walls, high surface area and good textural properties
are in the spotlight of many researchers all over the world. Due to the hydrothermal
and mechanical stability SBA-15 can find the applications for adsorption of
different substances from diluted aqueous solutions. The simplicity of SBA-15
modification, via sol-gel synthesis, allows to create sorbents exhibiting high
adsorption capacities towards chosen inorganic or organic molecules including:
heavy metal ions, biomolecules or pharmaceutics. The previous data concerning
adsorption of Pt(IV) [1] ions onto functionalized SBA-15 led me to study of Pd(II)
ions adsorption onto modified SBA-15 containing sulfur and nitrogen atoms.
Palladium is widely used in catalytic converters and telecommunication
industry; it also is applied for manufacture of watches and special mirrors. The
increasing use of palladium causes that everlasting control of its content in waters,
soils, food and also in human tissues is necessary. In order to determine palladium
in drinking water and plant samples where it occurs in ultra trace amounts,
enrichment stage has to be introduced to the analytical procedure.
The aim of this study was the synthesis, characteristic and application of
amino- and thiol-functionalized mesoporous organosilicas for Pd(II) ions
adsorption.
Synthesis of modified SBA-15 materials was carried out using sol-gel method.
2g of Pluronic 123 was dissolved in 60 mL of 2M HCl and 11 mL of deionized
water. After 8h of stirring at 40°C tetraethoxysilane (TEOS) was added into
solution. After 15 minutes the silane coupling agent was added, (3-mercaptopropyl)
trimethoxysilane (MPTMS), 3-aminopropyltriethoxysilane (ATES) and N-[3-
(trimethoxysilyl)propyl]-ethylenediamine TMPED. The mixture was stirred for 24h
at 40°C and aged for 48h at 100°C. The obtained materials were washed by using
deionized water, filtred and dried at 70°C. Removal of template was done by tree-
time extraction with EtOH at 70°C.
The object of this work was the synthesis, characteristic and application of
amino-functionalized mesoporous organosilicas for Pd(II) ions adsorption.
The initial molar ratios of monomers used for the one-step synthesis were as
follows: a) (TEOS/ATES=19/1), b) (TEOS/ATES=18/2), c) (TEOS/TMPD=19/1),
d) (TEOS/TMPD=18/2), e) (TEOS/MPTMS=19/1), f) (TEOS/MPTMS=18/2), g)
(TEOS/MPTMS=15/5).
The effect of pH on the Pd(II) adsorption onto modified SBA-15 and the
adsorption kinetic were studied. In the case of the thiol-functionalized SBA-15
materials high adsorption capacities were reached for equilibrium pH lower than 6,
whereas for TMPD and ATES functionalized silicas the optimal adsorption pH
range is from 1.2 to 2.2 and from 4 to 6.4, respectively. The obtained material
exhibit high adsorption capacities, which were assigned by setting the runs of Pd(II)
adsorption isotherms. The maximum static adsorption capacities (MSSCs) are 22,
24, 33, 66, 125, 190 and 280 mg/g for samples a, b, c, d, e, f and g, respectively.
The influence of nitrates and chlorides (Fig.1.) on the Pd(II) ions adsorption and
palladium removing from functionalized SBA-15 using thiourea and inorganic acids
were studied (Fig. 2). Due to incomplete Pd species desorption using inorganic
acids and the possibility of full dilution/digestion of sorbent by using HF solution
the slurry sampling GF AAS was proposed and applied as the most promising
technique for Pd determination in environmental samples after enrichment.
The functionalized SBA-15 exhibit high adsorption capacities, reaching 280
mg/g for organosilica synthesized of TEOS/MPTMS in the molar ratio 15/5. In the
case of the thiourea application 80-100% desorption of Pd species from amine-
functionalized silicas was observed. For thiol-functionalized silicas the desorption
reached maximally 80%. The high adsorption capacities and really fast kinetics
makes the materials promising for Pd(II) recycling from converters.
Fig.1. Impact of nitrates and chlorides on
the Pd(II) adsorption onto
(TEOS/MPTMS=18/2); m = 0.05 g, V = 50
ml, pH=1.2, t = 48h, T = 25ºC
Fig.2. Desorption of Pd(II) from
functionalized SBA-15 by using different
concentrations of thiourea; m = 0.005 g, V
= 2ml, t = 24h, T = 25ºC, a(TEOS/ATES=18/2) =
9.5 mg/g, a(TEOS/TMPD=18/2) = 9.8 mg/g
References:
[1] R. Dobrowolski, M. Oszust-Cieniuch, J. Dobrzyńska , M. Barczak, Colloid.
Surface. A., 435 (2013) 63-70.
THE MODIFIED CARBON NANOTUBES IN ANALYTICAL
APPLICATIONS OF PRECONCENTRATION AND DETERMINATION OF SOME ELEMENTS BY ATOMIC
SPECTROMETRY
Agnieszka MRÓZ DEPARTAMENT OF ANALYTICAL CHEMISTRY
AND INSTRUMENTAL ANALYSIS
Palladium has been used in different areas of science and technology including
agents, brazing alloys, petroleum, electrical industries and catalytic chemical
reactions, especially the usage as an effective catalyte for the fuel control of
automobiles. Environmental or industrial pollutions by palladium have so far been
hardly reported as compared with toxic heavy metals such as cadmium, mercury,
and lead. Exposure to certain level of palladium compounds can cause asthma,
allergy and other serious health problems [1]. So, it is of special interest in
environmental analysis and very important for public health to develop new
separation and preconcentration method for detection of palladium in real samples.
Nowadays, carbon nanotubes (CNTs) have attracted much interest that was
directed toward exploiting unique thermal, mechanical, electronic, and chemical
properties since they were first discovered. The extremely large surface area and the
unique tubular structure make CNTs a promising adsorbent material. The modified
carbon nanotubes can be potentially employed both in the industry for recycling of
precious metals from industrial waste, and – in analytical chemistry – as adsorbents
used for enrichment of trace precious metals [2].
The goal of this work was the synthesis and characteristic of modified
multiwalled carbon nanotubes (MWCNTs). Moreover, the performances of
modified multiwalled carbon nanotubes were tested as a new sorbent for the
preconcentration of trace Pd(II). Adsorption of Pd(II) were carried out in a static
system, and Pd(II) were determined by GF AAS technique.
MWCNTs were modified by compounds with different groups:
- 3-aminopropyltriethoxysilane (APTES)
- ethylenediamine (EDA)
- 3-mercaptopropyltrimethoxysilane (MPTMS)
- 2-cyanoethyltriethoxysilane (CETES)
- 3-thiocyanatopropyltriethoxysilane (TCTES)
- diethylphosphatoethyltriethoxysilane (DPTES)
- 1-(2-pyridylazo)- 2-naphthol (PAN)
Prior to modification, MWCNTs were oxidized with concentrated nitric acid,
in order to open the MWCNT ends and generate carboxyl groups. The treatment
was carried out by dispersing 50 mL of concentrated HNO3 to 1.0 g of MWCNTs,
and then heating for 4 h at 100oC. Afterward, the oxidized MWCNTs were washed
with distilled water until removing any excess of nitric acid (neutral pH of
solution). Then, about 1.5 g of oxidized MWCNTs were dispersed in 80 mL of
toluene and 0.01 mol of the modifying agent were added and kept under reflux at
65°C for 3 h. After cooling to room temperature, the MWCNTs were washed with
toluene and ethanol and dried at 60 °C for 12 h. Modification of nanotubes surfaces
as a result of chemical functionalization was confirmed through the presence of
characteristic groups examined by X-ray photoelectron spectroscopy (XPS).
The basic parameters affecting the adsorption capacity of Pd(II) ions on
modified carbon nanotubes were studied and the effect of MWCNTs modification
has been determined by studying the initial runs of adsorption isotherms (Fig.1).
The value of the Pd(II) adsorption is depended on both the carbon nanotubes
modification and the pH of solution. The maximum Pd(II) adsorption onto modified
MWCNTs occurs in the equilibrium pH ranges of 2.0-4.0. In order to evaluate the
potential of modified MWCNTs for the analytical application, the effect of Cl- and
NO3- was studied under optimized adsorption conditions (Fig. 2). Obtained results
have shown that NO3- ions do not interfere in the adsorption of Pd(II). In turn, in the
case of high concentration of Cl- ions (more than 0.1 mol/L), the decrease of Pt(IV)
adsorption onto modified CNTs is observed.
The modified MWCNTs exhibit satisfying adsorption kinetics and high
adsorption capacities. The maximum adsorption capacity was found to be as high as
55 mg/g, what together with favorable adsorption kinetics makes these materials
promising candidates for Pd(II) removal and preconcentration.
Fig. 1. Initial runs of adsorption
isotherms of Pd(II) onto modified
MWCNTs; m=0.01 g, V=5 mL, pH=2.5,
t=24 h, T=25ºC.
Fig. 2. The influence of NO3
- on the
Pd(II) adsorption onto modified
MWCNTs; m=0.01 g, V=5 mL,
C=80 mg/L, pH=2.5, t=24 h, T=25ºC.
References:
[1] C. Yuan, Y. Zhang, S. Wang, A. Chang, Microchimica Acta, 173 (2011) 361.
[2] X. Ren, C. Chen, M. Nagatsu, X. Wang, Chemical Engineering Journal, 170
(2011) 395.
ELIMINATION OF INTERFERENCES IN VOLTAMMETRIC
STRIPPING DETERMINATION OF LEAD USING AMBERLITE
XAD RESIN
Mieczysław KOROLCZUK, Małgorzata GRABARCZYK, Iwona RUTYNA
DEPARTMENT OF ANALYTICAL CHEMISTRY
AND INSTRUMENTAL ANALYSIS
Lead is one of the most toxic heavy metals with major interest in
environmental safety. Even small amounts of lead that enter the environment should
be controlled as they result in a cumulative effect. Electrochemical stripping
analysis is generally recognized as one of the most suitable methods for trace metal
determination. The analytical advantages of the stripping voltammetric techniques
include excellent sensitivity with a large useful linear concentration, rapid analysis
times and low cost. These methods have also a weakness - the measurement can be
disturbed by the organic compounds, particularly surface active substances, which
can foul and passive the electrode causing a decrease or total decay of the
analytical signal. It is a special disadvantage during the analysis of environmental
water samples which generally contain organic compounds in different
concentrations.
In the proposed procedure of lead determination an anodic stripping
voltammetry method is exploited and interferences from dissolved organic matter
are drastically reduced by adding to voltammetric cell Amberlite XAD. In such
measurements lead is accumulated on the electrode by its reduction to the metallic
form and, as was proved, it doesn`t adsorb on the resin. While the negative
influence of organic matter is eliminated by adsorption of these substances onto the
surface of Amberlite XAD-7 resin. The purpose of the work was the selection of the
optimal conditions for ultra trace determination of lead in the environmental water
samples containing high concentrations of surface active substances.
The course of the procedures
In order to eliminate interferences caused by surfactants the addition of
Amberlite XAD-7 resin to the voltammetric cell with the analysed sample was
studied. At first the stability of the Pb(II) signal value in the presence of resin was
examined. The experiments were performed for the samples containing 5 × 10-8
mol
L-1
Pb(II) and 0.5, 1 or 1.5 g XAD-7 resin added to 10 mL of the solution. For each
sample the signal of Pb(II) after accumulation on a mercury drop for 30 s at -0.55 V
was recorded and compared with the signal of Pb(II) obtained in the absence of
XAD-7 resin. It was found that in each case the addition of resin to the samples did
not affect the Pb(II) analytical signal value, which confirms that lead does not
adsorb on the surface of the resin. For further measurements the amount of resin
equal to 0.5 g was chosen and it was tested that in the presence of such an amount
of resin the signal of lead was stable for at least 15 min. In standard measurements
the time of mixing the sample with resin for 5 min. was used because, as was
proved in previous papers, further lengthening of the sample contact time with resin
did not maximise the efficiency of organic substance removal.
Voltammetric measurements were made using anodic stripping voltammetry
(ASV) according to the following procedure: A mercury drop was formed and the
preconcentration of lead was carried out for 30 s at -0.55 V whilst stirring the
solution with a magnetic stirring bar. At the end of the preconcentration time, the
stirrer was switched off, and after a 5 s equilibration time, a differential pulse
stripping voltammogram was recorded, while the potential was scanned from -0.55
V to -0.2 V at a scan rate 20 mV s-1
and a pulse height 50 mV.
Analytical parameters
The dependence of the Pb(II) peak current on its concentration was found to be
linear in the range from 2 × 10-9
to 2 × 10-6
mol L-1
for an accumulation time 30 s
and obeyed the equation y = 598x – 1 (y and x are the peak current (nA) and Pb(II)
concentration (µmol L-1
), respectively), with a correlation coefficient of r = 0.998.
The relative standard deviation for 10 replicate measurements of 1 × 10-8
mol L-1
Pb(II) was equal to 3.4 %. The detection limit estimated from three times the
standard deviation for a low Pb(II) concentration and accumulation time of 30 s was
equal to 8.6 × 10-10
mol L-1
.
Achievement
The effect of the chosen surfactants, that is cationic CTAB, anionic SDS and
nonionic Triton X-100, on the lead analytical signal was tested. The obtained results
indicate that the addition of resin drastically eliminates the unwanted negative
influence of the nonionic, anionic and cationic surfactants on lead peak height. In
the presence of Amberlite XAD-7 resin inherency of even 20 mg L-1
of SDS and
CTAB and 15 mg L-1
of Triton X-100 does not affect the lead signal at all. The 20
mg L-1
of Triton X-100 causes a decrease of the lead signal to 80 % of its original
value. It is a very satisfactory result, considering that in the absence of resin even 1
mg L-1
of SDS, CTAB or Triton X-100 causes total decay of lead peak signal.
Other important components of natural organic matter, inevitably present in
natural samples, are humic substances. Out of the total amount of humic substances
in surface waters, fulvic acids typically account for the majority of the dissolved
organic carbon (80 %), with humic acids accounting for the remaining 20 %. In the
presented communication the effect of fulvic acids (FA) and humic aicds (HA) as
representative humic substances was investigated and it was found that when using
the proposed procedure with the addition of Amberlite XAD-7 resin, 20 mg L-1
of
FA and 5 mg L-1
of HA do not disturb the Pb(II) analytical signal, whereas 10 mg L-
1 of HA decreases it to 40 % of the initial value. The typical range of dissolved
organic carbon in natural waters is from 2 - 10 mg L-1
.
RESEARCHES ON ION SELECTIVE ELECTRODE FOR
INDOMETHACIN DETERMINATION
Joanna LENIK DEPARTMENT OF ANALYTICAL CHEMISTRY
AND INSTRUMENTAL ANALYSIS
One of medicines belonging to NSAID-s group is indomethacin (1-(p-
chlorobenzoyl)-5-methoxy -2-methyl-3-indolylacetic acid) (Fig 1). It is commonly
used to reduce fever, pain, stiffness, and swelling. It works by inhibiting the
production of prostaglandins. Indomethacin is a potent drug with many serious side
effects and should not be considered an analgesic for minor aches and pains or
fever. The drug is best used as an anti-inflammatory, rather than an analgesic.
Indomethacin membrane sensors based on different plasticizers and quaternary
ammonium salt tetraoctylammonium 1-(p-chlorobenzoyl)5-methoxy-2-methyl-3-
indolylacetate (INDO–TOA) were prepared.
The electrode’s basic parameters, such as the slope of characteristics, selectivity
(Table 2), response time lifetime, the influence of pH on the electrode’s potential,
were established (Table 1).
The calibration curves were determined in the main ion and interfering ions solution
at pH 8.8 in the range of concentration 10-2
– 10-6
mol L-1
.
The electrode (with PVC membrane plasticized with dibutylphthalate) response to
indomethacin has the sensitivity near Nernstian (-59.8±1.5 mV decade-1
) over the
linear range of 1x10-5
- 1x10-2
mol L-1
and limit of detection 3.16x10-6
mol L-1
. The
present electrodes show clear discrimination of indomethacin ions from several
inorganic, organic and some common drug excipients. This electrode has a response
time 12 s and can be used in the pH range 6.0 - 10.0. The notably property and
attractive quality of the indomethacin sensor is low cost, comfortable application.
The best values of selectivity coefficient in respect of inorganic ions NO3-
> Br-
>Cl- > H2PO4
2-, organic ions: acetate > propionate > formate > citrate > tartrate >
oxalate and amino acids: glutamic acid > glicine > aspartic acid were obtained for
the DBP electrode.
The influence of 1.0x10-5
to 1.0x10-2
mol L-1
of (2-hydroxypropyl)--cyclodextrin on the calibration curve, response time and selectivity of the electrode was
investigated. The concentration of HPCD higher than 1.0x10-2 mol L-1 causes the contraction of the range of linearity (to 1.0x10
-3 – 1.0x10
-2 mol L
-1), an increase of
detection limit (3.16x10-4
mol L-1
) and increase of potential. The response time to a
sudden concentration change of the main ion in the presence of HPCD is not changed.
Table 1. Analytical parameters of Table 2. Selectivity coefficients
indomethacin electrode
Fig. 1. Structure of (1-(p-chlorobenzoyl)-5-methoxy -2-methyl-3-indolylacetic acid) INDO
The analytical usefulness of indomethacin electrode was examined by determining
indomethacin inpharmaceutical preparations containing (1-(p-chlorobenzoyl)-5-
methoxy-2-methyl-3-indolylacetic acid in “Metindol Retard” – ICN Polfa Rzeszów
SA, Poland. The determination was performed by the calibration curve method and
the method of standard addition. Statistical parameters prove to be typical of
analytical methods using ion-selective electrodes: the accuracy (0.8 -2.5 % and the
precision (RSD 0.8 - 5.5 % ).The proposed technique for indomethacin
determination using ion-selective electrode is characterized by good sensitivity,
selectivity, precision, and accuracy and may be successfully applied for fast and
simply determination of indomethacin in pharmaceuticals.
Selectivity coefficients K
Cl-
Br-
NO3-
SO42-
H2PO4-
propionate
citrate
formate
acetate
oxalate
tartrate
glutamic acid
aspartic acid
glycine
malonate
D-mannitol
glucose
lactose
1,17x10-3
8,88x10-3
5,13x10-2
6,64x10-5
1,14x10-4
1,87x10-3
1,78x10-4
1,21x10-3
2,08x10-3
9,38x10-5
1,15x10-4
6,33x10-4
5,6x 10-4
5,19x10-4
3.47x10-3
9.12x10-4
6,16x10-4
6,20x10-4
Parameter Electrode (DPB)
Characteristic slope S
[mV decade-1
]
-59.8 ±
1.5
Linearity range,
[mol L-1
]
Correlation coefficient (r)
Intercept E0 [mV]
10-5
÷ 10-2
0.9980
10.4
Potential drift mV/day
pH range
Response time [s]
Life time, months
7
6.0 ÷ 10.0
12
2
H3CO
N
C O
Cl
CH2COOH
CH3
ADSORPTION OF SODIUM OCTANESULFONATE AND N-
OCTANE-N-METHYLGLUCAMIDE ON MERCURY ELECTRODE
Jolanta NIESZPOREK, Dorota GUGAŁA-FEKNER, Dorota SIEŃKO
DEPARTMENT OF ANALYTICAL CHEMISTRY AND
INSTRUMENTAL ANALYSIS
For the purpose of this study an anionic surfactant, sodium octanesulfonate
and nonionic surfactant, N-octane-N-methylglucamide were choosen. The chosen
surfactant’s concentrations were lower than their critical micellar point. A 1M
NaClO4 solution was used as the base electrolyte. The systems were characterized
by the measurement of differential capacity, zero charge potential (Ez), and surface
tension at this potential. Fig. 1 presents differential capacity-potential curves of the
double layer Hg / 1M NaClO4.
0 -0.4 -0.8 -1.2 -1.6
E / V
10
20
30
C /
F
. cm
-2
1 M NaClO4 pH 3
1.10-5 M
5.10-5 M
1.10-4 M
3.10-4 M
4.10-4 M
5.10-4 M
6.10-4 M
1.10-3 M
(a)
0 -0.4 -0.8 -1.2 -1.6
E / V
10
20
30
C /
F
. cm
-2
1M NaClO4 pH 3
2.10-6 M
1.10-5 M
2.10-5 M
3.10-5 M
4.10-5 M
5.10-5 M
1.10-4 M
5.10-4 M
(b)
Fig. 1 Differential capacity curves of the double layer Hg/1M NaClO4 pH 3 in the presence
of various concentrations of sodium octanesulfonate (a) and N-octane-N-methylglucamide
(b).
The highest changes of EZ appeared in solutions with addition of N-octane-N-
glucamide concentration higher than 10-4
M. (Table 1).
Table 1. The values of zero charge potential, Ez vs. Ag/AgCl electrode and surface
tension, z at Ez for the system Hg/1M NaClO4 pH 3 in the presence of various
concentrations of sodium octanesulfonate (a) and N-octane-N-methylglucamide (b).
(a) (b)
c [M] -Ez [mV] γz [mN∙m-1
] c [M] -Ez [mV] γz [mN∙m-1
]
0 471.2 425.5 0 471.2 425.5
1∙10-5
470.8 416.2 2∙10-6
471.0 417.9
5·10-5
469.3 413.7 1·10-5
470.3 412.5
1·10-4
468.7 412.0 2·10-5
469.8 411.2
3·10-4
467.2 407.8 4·10-5
468.7 407.0
4·10-4
466.2 407.0 5·10-5
468.1 404.5
5·10-4
465.9 404.5 1·10-4
466.1 394.9
6·10-4
465.3 402.8 3·10-4
459.0 392.7
1·10-3
462.3 394.4 5·10-4
442.0 388.5
Stronger changes of Ez as well as a significant decrese of differential capacity
curves for nonionic surfactant confirmed a stronger adsorption of N-octane-N-
methylglucamide in comparison with the sodium octanesulfonate. Additionally the
Ez value changes show a mechanism in which both surfactants adsorb with their
hydrocarbon chain on the electrode surface.
ELECTROCHEMICAL AND THERMODYNAMIC STUDY OF THE
ELECTROREDUCTION OF Bi(III) IONS IN THE PRESENCE OF CYSTINE IN SOLUTIONS OF DIFFERENT WATER ACTIVITY
Agnieszka NOSAL - WIERCIŃSKA
DEPARTMENT OF ANALYTICAL CHEMISTRY AND INSTRUMENTAL ANALYSIS
Cystine (RSSR) is available as an individual supplement or as part of protein
supplements. This amino acid participates in a variety of physiological functions,
including the synthesis of insulin and blood plasma proteins. Cystine is a
constituent of hair and nail keratin. It may also prevent the toxic effects of metals
and of the particularly harmful free radicals that are produced in the bodies of
cigarette smokers and alcohol abusers [1,2].
Cystine is electrochemically active and in aqueous solutions it reacts with
mercury forming cysteine mercuric thiolate Hg(SR)2 and cysteine mercurous
thiolate Hg2(SR)2 , which are both strongly adsorbed at the electrode [1].
Furthermore, a considerable influence of water on the surface properties of the
Hg/chlorate(VII) phase boundary in the presence of cystine [2] was observed.
Research methodology is mostly based on electrochemical techniques
(voltammetry, Faradaic impedance), which allow for elucidating the mechanism of
Bi(III) ion electroreduction and determining kinetic parameters, as well as for
correlating these parameters with water activity.
It has been found that cystine catalyzes the process of Bi(III) ion
electroreduction in chlorates(VII), thus meeting the requirements of the “cap-pair”
rule [2]. The obtained results show cystine to have catalytic activity in multistep
Bi(III) electroreduction in chlorate(VII) solutions. This catalytic activity clearly
depends on water activity. In solutions with high water activity, the catalytic
activity of cystine is considerably higher than in solutions with low water activity.
In highly concentrated electrolytes (6–8 mol·dm-3
), the catalytic activity of cystine
is small. It has been shown that the process of Bi(III) ion electroreduction in the
presence of cystine is controlled for all the chlorate(VII) concentrations studied (1 –
8 mol·dm-3
) by the reaction kinetics of the formation of active Bi-Hg(SR)2
complexes preceding electron transfer.
References:
[1] M. Heyrovsky, P. Mader, S. Vavřička, V. Veselá, M. Fedurco, J. Electroanal. Chem, 430(1997)103.
[2] A. Nosal – Wiercińska, Electrochim. Acta, 92, (2013)397.
APPLICATION OF LEAD FILM ELECTRODE MODYFIED WITH
POLIMER FILM TO DETERMINATION OF TRACE CONCENTRATIONS OF BIOLOGICALLY ACTIVE COMPOUNDS
BY ADSORPTIVE STRIPPING VOLTAMMETRY
Katarzyna TYSZCZUK-ROTKO
DEPARTMENT OF ANALYTICAL CHEMISTRY
AND INSTRUMENTAL ANALYSIS
Caffeine (3,7-dihydro-1,3,7-trimethyl-1H-purine-2,6-dione) is an alkaloid from
xanthine group that is widely distributed in various kinds of beverages and food,
such as coffee, tea, coca-cola, cola nuts and chocolate. It can also be purchased
in capsules and tablets for the treatment of asthma, nasal congestion, and headache
or to improve athletic endurance and facilitate weight lost [1]. The popularity of
caffeine containing products is connected with her physiological effects, such as
stimulation of the central nervous system, diuresis and gastric secretion [2].
However, it can cause adverse mutation effects when excessively consumed, such
as inhibition of DNA repair and cyclic AMP phosphodiesterase activity.
Furthermore, it can be a cause of cancer, heart diseases and complications
in pregnant women and aging [3]. For these reasons, it is very importent to control
the concentration of caffeine in its different sources.
The main aim of the study was to optimize and develop a sensitive, fast and
accurate adsorptive striping voltammetric method with the use of Nafion covered
lead film electrode (Nafion/PbFE) for the determination of caffeine in
pharmaceutical formulations and food samples.
In the course of caffeine determination at the Nafion/PbFE the potential of the
electrode was changed in the following sequence: 1 V for 30 s and -1.55 V for 120
s. The first step was applied to clean the electrode from the caffeine remaining after
the preceding measurement. During the second step caffeine was accumulated at the
Nafion/PbFE. Then, after 5 s equilibration time, the anodic differential pulse
voltammograms were registered in the range from 0.65 to 1.6 V, with amplitude of
50 mV, modulation time of 4 ms and scan rate 50 mV s-1
.
Under the optimal analytical conditions, the determination of caffeine with
different concentrations was performed. The calibration graphs for the
accumulation time of 120 s were linear from 5 × 10-8
to 5 × 10-6
mol L-1
for the peak
1 and from 5 × 10-7
to 1 × 10-5
mol L-1
for the peak 2, and obeyed the equations y =
93.01 x + 3.45 and y = 25.71 x – 0.29, respectively, where y is the peak current (nA)
and x is a caffeine concentration (µmol L-1
). The correlation coefficients (R2) for
peaks 1 and 2 were 0.9997 and 0.9999, respectively. The detection limits for peaks
1 and 2 estimated from 3 times the standard deviation for the lowest determined
concentration of caffeine were about 1.5 × 10-8
and 2 × 10-7
mol L-1
, respectively.
The advantage of using the Nafion modified lead film electrode consists in lower
detection limit of caffeine with respect to those reported for the bare and Nafion
covered electrodes [4].
The method was successfully applied to the determination of caffeine in tea,
coffee, soft and energy drinks samples as well as pharmaceutical formulation and
average the contents were in close agreement with those quoted by the
manufacturer and with those obtained by the reported spectrophotometric method
[5].
The Nafion covered lead film electrode was also applied to the determination
of acetaminophen (paracetamol) by adsorptive stripping voltammetry. In the course
of paracetamol determination the accumulation step was carried out at -1.45 V for
60 s. The square-wave voltammograms were recorded at a frequency of 200 Hz,
while the potential was scanned from -0.45 to 1.0 V. The amplitude was 50 mV.
The calibration graph for the accumulation time of 60 s was linear from
5 × 10-7
to 1 × 10-2
mol L-1
and obeyed the equation y = 12.56 x + 0.297, where y
and x are the peak current (µA) and paracetamol concentration (mmol L-1
),
respectively. The correlation coefficient (R2) was 0.9997. The relative standard
deviation for a paracetamol concentration of 1 × 10-5
mol L-1
was 3.8 % (n = 5). The
detection limits for the accumulation time of 30 s estimated from 3 times the
standard deviation for the lowest determined concentration of paracetamol was
about 1.9 × 10-7
mol L-1
.
The method was successfully applied to the determination of paracetamol in
pharmaceutical tablets and average the contents were in close agreement with those
quoted by the manufacturer.
References:
[1] O. Cauli and M. Morelli, Behavioural Pharmacology, 16 (2005) 63.
[2] N. Spătaru, B.V. Sarada, D. Tryk and A. Fuijshima, Electroanalysis, 14 (2002)
721.
[3] J.Y. Sun, K.J. Huang, S.Y. Wei, Z.W. Wu and F.P. Ren, Colloids and Surfaces
B: Biointerfaces, 84 (2011) 421.
[4] L. Švorc, International Journal of Electrochemical Science, 8 (2013) 5755.
[5] A. Belay, K. Ture, M. Redi and A. Asfaw, Food Chemistry, 108 (2008) 310.
APPLICATION OF IONIC LIQUID TO THE CONSTRUCTION OF
COPPER ION-SELECTIVE ELECTRODE WITH SOLID CONTACT
Cecylia WARDAK
DEPARTAMENT OF ANALYTICAL CHEMISTRY
AND INSTRUMENTAL ANALYSIS
The new generation of ion-selective electrodes with internal solid contact has
attracted much attention for the past few years. These electrodes will have certain
advantages over conventional ones, such as the small size, lower cost of production,
and ability to operate in high pressure environments where conventional ISEs might
be damaged. Furthermore, this type of electrode allows for low detection limit,
which was attributed to the absence of transmembrane ion fluxes [1].
The aim of this work was developed of solid contact Cu2+
- ISE using chloride
ionic liquid as transducer media. ILs act as very promising solid contact of ISE with
polymeric membrane because they connect two functions in one membrane
component. On the one hand ILs keep constant concentration of chloride ions in the
membrane phase what guarantee the stability of potential of internal Ag/AgCl
reference electrode. On the other hand they lower the membrane resistance and
reduce anion interference, altogether improving the analytical parameters of the
electrode such as detection limit, measuring range, working pH range and
selectivity [2-4]. In this work the membrane containing three ionic liquid: 1-ethyl-3-
methyl imidazolium chloride (EMImCl), 1-butyl-3-methyl imidazolium chloride
(BMImCl), 1-hexyl-3-methyl imidazolium chloride (HMImCl), as well as the
commonly used potassium tetrakis(p-chlorophenyl) borate KTpClB were
investigated. The 2- nitrophenyl octyl ether (NPOE) was used as membrane
plasticizer and N,N,N′,N′-Tetracyclohexyl-2,2′-thiodiacetamide was used as
ionophore.
An internal Ag/AgCl electrode was prepared as follows: a clean silver wire
was anodized electrochemically for 5 min in 4 M HCl using a constant voltage of 5
V from a power source. Then the electrode was rinsed with water, dried with tissue-
paper and covered by the inner membrane phase.
The electrode membrane phase consists of two layers placed in a Teflon
holder. The inner layer contains plasticizer, PVC and lipophilic additive (ionic
liquid or KTpClB) in which the Ag/AgCl electrode is placed. The outer layer
contains the same components and an ionophore. The outer layer is placed on the
inner layer and it is contacted with the tested solution. In order to prepare the inner
layer the membrane components were weighed, mixed thoroughly and the mixture
was deaerated by means of a vacuum oil pump. The Teflon holder was filled with
the mixture so that the silver-silver chloride electrode was immersed in it. Then the
mixture was gelated at 80 ◦C for 30 min. In order to prepare the outer layer the
ionophore was dissolved in a plasticizer and then mixed with other components.
The mixture was deaerated, placed on the inner layer and gelated at 80 ◦C for 10
min. After cooling to room temperature the sensor was mounted in the electrode
body and conditioned for at least 24 hours in 1x10-3
mol L-1 Cu(NO3)2 to saturate
PVC membrane in the primary ions and then for at least 24 hours in the appropriate
conditioning solution before potentiometric measurements. Concentrations of
conditioning solutions were as follows: 1x10-3
mol L-1
, 1x10-5
mol L-1
, 1x10-7
mol
L-1
and 1x10-9
mol L-1
.
In order to evaluate the effect of ionic additive to the membrane, basic
analytical parameters of studied copper electrodes were determined. The best results
were obtained for electrode having membrane doped with 1-ethyl-3-methyl
imidazolium chloride. The electrode shows a Nernstian response for copper ions
over a wide concentration range (1x10-7
-1x10-1
mol L-1
) and the slope of 28.9
mV/decade. The limit of detection is 3.2x10-8
mol L-1
. It has a fast response time of
5-10 s and can be used for more than 4 months without any divergence in potential.
The proposed sensor is not pH sensitive in the range 2.5-6.0 and shows a very good
discriminating ability towards Cu2+
ion in comparison with some alkali, alkaline
earth, transition and heavy metal ions.
The big potential drift and poor reproducibility is a serious problem of solid
contact electrodes. It is connected with the lack of thermodynamically well-defined
electrochemical interface between the membrane and the electronic conductor. So
the stability and reproducibility of the electrode potential in time were studied. The
results obtained show that the addition of ionic liquid to the membrane stabilize the
electrode potential. For the electrode based on EMImCl the determined drift of
potential was -0.1 mV per day and reproducibility of EMF values for three the same
electrodes was very good (SD≤5.8 mV).
References:
[1] J. Sutter, A. Radu, S. Peper, E. Bakker and E. Pretsch, Anal. Chim. Acta.,
523(2004)53.
[2] C. Wardak , Int.. J. Environ. Anal. Chem., 89(2009)735.
[3] C. Wardak, J. Hazar. Mater., 186(2011)1131.
[4] C. Wardak, Electroanalysis, 24(2012)85.
INFLUENCE OF THE FLUOROCARBON SURFACTANT FILM ON
THE POLYTERAFLUOROETHYLENE AND POLYMETHYL
METHACRYLATE SURFACE TENSION
Katarzyna SZYMCZYK and Bronisław JAŃCZUK
DEPARTMENT OF INTERFACIAL PHENOMENA
Surface tensions, especially of solid-vapour and solid-liquid interfaces, are
important thermodynamic parameters to predict the wetting and adhesion properties
of polymer materials including also their biocompatibility [1]. In the literature it is
suggested that liquid should wet the solid if its surface tension value is equal or
lower than that of a solid [2]. It means that decrease of the water surface tension to
that of solid by the addition of the surface active agent to water fulfils the condition
for spontaneous spreading of aqueous solution of such compounds over the solid
surface. On the other hand, such condition is fulfilled if the solid-solution interface
tension is equal to zero when the surface tension of solution and solid is the same
[2]. However, as follows from the literature in the case of aqueous solutions of
surfactants, the so-called critical surface tension of solid wetting [2] is somewhat
higher or considerably lower than the solid surface tension and in many cases it
depends on the kind of surfactant added to water [3,4]. Such behaviour of aqueous
solution of surfactants in the wetting process is caused, on one hand, by the changes
of the solid-solution interface tension, which strongly depends on the orientation of
surfactant molecules in the surface layer at the solid-solution interface different
from that at the solution-air interface. Thus, the changes of the solid-solution
interface tension can occur in a different direction from that of water surface
tension. On the other hand, this process is caused by the changes of the solid surface
tension as a function of surface active agents concentration. In the literature it is
possible to find different opinions about this problem [3,4].
In the earlier studies on the basis of the contact angle of water, formamide and
diiodomethane, it was proved that the surface tension of polymers, PTFE and
PMMA, SV , is changed under the influence of the fluorocarbon surfactants, the Zonyl FSN-100 (FSN100) and Zonyl FSO-100 (FSO100) film, on their surfaces at
different concentrations in the bulk phase and depends on the time of solution
contact with the polymer surface [5]. From this point of view, it was interesting to
determine the influence of these fluorocarbon surfactants in the solvent composed
of water and contestant concentrations of p-(1,1,3,3-tetramethylbutyl)phenoxypoly
(ethyleneglycols), Triton X-100 (TX100) and Triton X-165 (TX165) on the surface
tension components of PTFE and PMMA surface. From the measurements and
calculations it results that at the concentrations of FSN100 and FSO100 in the range
corresponding to their unsaturated monolayer at the water-air interface [46], the
components and parameters of SV practically do not depend on the fluorocarbon surfactant concentration. In this range of concentration, the surface tension of PTFE
covered with the mixed layers is somewhat higher than for "pure" PTFE and there
are only slight differences between its total surface tension and the Lifshitz-van der
Waals component of this tension. However, if the concentrations of FSN100 and
FSO100 are close to the CMC of a given mixture [6], a moderate decrease of the
surface tension of the PTFE/mixed layer is observed. At the surfactant
concentrations close or higher than their CMC, there is a considerable increase of
the total surface tension of PTFE/mixed layer as well as its Lifshitz van der Walls
component and electron-donor parameter [7].
In the case of PMMA, in the range of concentration lower than CMC, the
density of the adsorbed mixed layer is lower than in the case of PTFE because the
surface tension of the PMMA/mixed layer is close to that of the PMMA in the
absence of any surfactant layer. However, for the lowest concentration of the
hydrocarbon surfactants, if the concentration of fluorocarbon surfactant is close to
that corresponding to the saturated layer at the water-air interface, the surface
tension and particularly its Lifshitz van der Waals component decrease, having a
minimum near its CMC. It should be stressed, in contrast to PTFE, that the work of
adhesion to PMMA for water is higher than for any other of the components of the
mixture of surfactants used for the layer formation. The reason is the lower
tendency that the surfactants have to adsorb at the PMMA-solution interface rather
than at the PTFE-solution one. Therefore, the effect of the presence of an adsorbed
layer on the surface becomes evident for PMMA at higher concentration of the
surfactants mixture than for PTFE. On the other hand, PMMA is a monopolar solid
which has a considerable electron-donor parameter, then there are repulsive forces
between the PMMA surface and the surfactants head. The maximal value of the
surface tension of the PMMA/mixed layer is higher than the surface tension of all
the components of the mixture of surfactants and the maximal total surface tension
of the PTFE/mixed layer. It means that water molecules are present in the mixed
layer of the surfactant and they influence the surface tension of the polymer covered
with a surfactant layer [7].
References:
[1] J.M. Rosen, Surfactants and Interfacial Phenomena, Wiley-Interscience, New
York, 2004.
[2] W.A. Zisman, Contact Angle, Wettability and Adhesion, Advances in Chemistry
Series, vol. 43, Amer. Chem. Soc., Washington, DC, 1964.
[3] T.D. Blake, Wetting, In: T.H. Tadros (Ed.), Surfactants, Academic Press,
Orlando, 1984.
[4] Y. Kitazaki and T. Hata, J. Adhes., 4 (1972) 155.
[5] K. Szymczyk and B. Jańczuk, Ind. Eng. Chem. Res., 51 (2012) 14076.
[6] K. Szymczyk, J. Colloid Interface Sci., 363 (2011) 223.
[7] K. Szymczyk, M. L. González-Martín, J. M. Bruque and B. Jańczuk, J. Colloid
Interface Sci., 417 (2014) 180.
ADSORPTION OF FLUOROCARBON SURFACTANTS AT THE
POLYMER-SOLUTION AND SOLUTION-AIR INTERFACES AND
THE POLYMERS WETTABILITY
Katarzyna SZYMCZYK
DEPARTMENT OF INTERFACIAL PHENOMENA
The important ability of surfactants to promote wetting of solids has been
studied extensively and technologically for decades [1]. The wettability of the
surface of solids d