photocatalytic oxidation of cyanide under visible light by pt doped agins2 nanoparticles

Journal of Industrial and Engineering Chemistry xxx (2014) xxx–xxx

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JIEC-1834; No. of Pages 6

Photocatalytic oxidation of cyanide under visible light by Pt dopedAgInS2 nanoparticles

E.S. Aazam *

Chemistry Department, Faculty of Science, King Abdulaziz University, P.O. Box 80203, Jeddah 21589, Saudi Arabia

A R T I C L E I N F O

Article history:

Received 19 December 2013

Accepted 29 December 2013

Available online xxx

Keywords:

Pt doping

AgInS2

Visible photocatalyst

Oxidation of cyanide

A B S T R A C T

AgInS2 nanoparticles were prepared by a microwave method, while Pt was doped on the surface of

AgInS2 via photoassisted deposition method. The catalytic performances of the AgInS2 and Pt/AgInS2

samples were carried out for photocatalytic oxidation of cyanide under visible light. The UV–vis analysis

proved a red shift was detected after the loading of Pt into the AgInS2. The maximum oxidation efficiency

achieved was 100% at 1.5 wt% Pt/AgInS2 photocatalyst after 35 min reaction time. The catalyst could be

reused without any loss in activity during the first five cycles.

� 2014 The Korean Society of Industrial and Engineering Chemistry. Published by Elsevier B.V. All rights

reserved.

Contents lists available at ScienceDirect

Journal of Industrial and Engineering Chemistry

jou r n al h o mep ag e: w ww .e lsev ier . co m / loc ate / j iec

1. Introduction

Environmental problems associated with hazardous wastes andtoxic water pollutants have been attracted much attention.Cyanides are one of the major groups of problems in wastewatersproduced from various industries including metal cleaning,plating, electroplating, metal processing, automobile parts manu-facture, steel tempering, mining, photography, pharmaceuticals,coal coking, ore leaching, plastics, etc., Among various physical,chemical, and biological techniques for treatment of wastewaters,photocatalysis has been considered as a cost-effective for waterremediation [1–3]. Advanced Oxidation Processes (AOPs), such asheterogeneous photocatalysis, have gained a great deal ofattention. TiO2 is the most popular material for these processesdue to its higher photocatalytic activity, good photostability, non-toxicity, and low price. However, the large band gap of TiO2, whichis 3.2 eV, has proven to be a major drawback; wavelengths below400 nm are necessary for excitation, which limits the efficiency ofsolar light sources. Therefore, modifying the band gap of TiO2

would be useful for the improvement of the optical properties ofthis material. In the last few decades, doping with both metals andnonmetals has been successfully utilized to shift the opticalresponse of the catalytically active TiO2 from the UV to the visiblelight region. Zeolite [4,5], graphene [6], Eu [7], Bi [8], Ni [9], Pt [10],Au [11], Ag [12–15], rare earth dopants [16,17], and Co, Cr, Ag[18,19] have been used to extend the photoresponse range of the

* Tel.: +966 2 640000; fax: +966 2 6952292.

E-mail address: [email protected]

Please cite this article in press as: E.S. Aazam, J. Ind. Eng. Chem. (20

1226-086X/$ – see front matter � 2014 The Korean Society of Industrial and Engineer

http://dx.doi.org/10.1016/j.jiec.2013.12.104

TiO2 matrix. Ternary halcogenides of XYmZn (X = Cu, Ag, Zn, Cd;Y = Ga, In; Z = S, Se, Te; m, n = integer) have attracted considerableattention due to their excellent electrical and optical properties,and have been applied in the photovoltaic solar cells, linear andnonlinear optical instruments, and photocatalysis [20–25]. As oneof the most important ternary chalcogenides, AgInS2 is anintriguing functional material because of its promising applica-tions in photovoltaic, optoelectronic and photocatalytic fields [26–28]. Tsuji et al. [28] have reported that solid solutions consisting ofcombinations of CuInS2, AgInS2, and ZnS showed the highphotocatalytic activities for H2 evolution from aqueous sulfideand sulfite solutions under visible light irradiation. Additionally,we found that ternary AgInS2 has absorption of visible light. Thus,it is of great interest to investigate the photocatalytic activity ofAgInS2 for thiophene pollutant degradation. So far, many methodsfor preparing AgInS2 powder and film have been reported, such assolvothermal synthesis approach [28,29], hot press method [30],and spray pyrolysis technique [26,31]. These approaches areimportant for understanding the formation process and mecha-nism of complex AgInS2. However, these methods mentionedabove have some disadvantages. (1) Some of these methods reliedon relatively high temperature [32] and pressure [30]. (2) Certainapparatuses such as Teflon-lined stainless-steel autoclave wereindispensable [28,33]. (3) A lot of approaches made use of organicsolvents (anisole [35], ethylenediamine [29,34], and ethanol [35])as the reaction mediates. (4) Most of these methods require a longreaction time. Therefore, the challenge remains how to prepareAgInS2 nanostructure using a facile, mild, no secondary pollution,stable, and time saving method, and also how to decrease orprevent the recombination rate of photogenerated carriers to

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20 30 40 50 60 70

2.0 wt % Pt/ AgInS2

Inte

nsity

, a.u

.

2-Theta/ deg ree

1.5 wt % Pt/ AgInS2

1.0 wt % Pt/ AgInS2

0.5 wt % Pt/ AgInS2

AgInS2

Fig. 1. XRD pattern of AgInS2 and Pt/AgInS2 nanoparticles.

65 70 75 80

Inte

nsity

, a.u

.

Binding energy (eV)

Pt 4f7/2

Pt 4f5/2

Fig. 2. XPS for Pt 4f for 1.5 wt% Pt/AgInS2.

E.S. Aazam / Journal of Industrial and Engineering Chemistry xxx (2014) xxx–xxx2

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increase the photocatalytic activity of AgInS2. Herein, we presentthe synthesis of Pt doped AgInS2 photocatalyst. The effect of Ptcontent on the photocatalytic activity of AgInS2 has beeninvestigated in detail. It was found that the presence of Pt couldsignificantly improve the photocatalytic performance of AgInS2

towards cyanide photocatalytic oxidation in visible light.

2. Experimental

2.1. Synthesis of AgInS2

AgInS2 nanoparticles were prepared by a microwave method asthe following steps: silver nitrate (AgNO3), Indium (yII) chloridetetrahydrate (InCl3�4H2O), and thioacetamide (C2H5NS, TAA) as theinitial chemicals with a molar ratio of 1:1:2 were slowly dissolvedin 10 mL ethylene glycol (EG) as a solvent separately. Then, thesesolutions were mixed together. An appropriate amount of sodiumdodecyl sulfate (SDS) as a surfactant (In: SDS atomic/molecularratio of 1:5) was added to above prepared mixture to provide thehigh dilution and to prevent further accumulation of particles. Themixture was stirred for 10 min and then was placed into adomestic microwave oven with the power of 900 W for 15 min.Finally, the obtained precipitation was filtered, washed severaltimes with ethanol and distilled water and dried at 70 8C for 4 h in avacuum oven

2.2. Synthesis of Pt/AgInS2

Pt/AgInS2 catalysts (0.5, 1.0, 1.5, and 2.0 wt% of Pt metal) weresynthesized using a photoassisted deposition (PAD) route asfollows: Pt metal was deposited on AgInS2 from aqueous solutionof H2PtCl6 under UV-light irradiation. The samples were dried at378 K then followed by H2-reduction (20 ml min�1) at 673 8C foranother 2 h.

2.3. Characterization techniques

X-ray diffraction (XRD) analysis was carried out at roomtemperature with a Bruker axis D8 using Cu Ka radiation(l = 1.540 A). The specific surface area was calculated from N2-adsorption measurements, which were obtained using a Nova2000 series Chromatech apparatus at 77 K. Prior to the measure-ments, the samples were treated under vacuum at 120 8C for 2 h.The band gap of the samples was identified by UV–vis diffusereflectance spectroscopy (UV–vis-DRS), which was performed inair at room temperature in the wavelength range of 200–800 nmusing a UV/vis/NIR spectrophotometer (V-570, JASCO, Japan).Transmission electron microscopy (TEM) was conducted with aJEOL-JEM-1230 microscope, and the samples were prepared bysuspension in ethanol, followed by ultrasonication for 30 min.Subsequently, a small amount of this solution was placed onto acarbon-coated copper grid and dried before loading the sample inthe TEM. X-ray photoelectron spectroscopy (XPS) studies wereperformed using a Thermo Scientific K-ALPHA, XPS, England.Photoluminescence (Pl) emission spectra were recorded with aShimadzu RF-5301 fluorescence spectrophotometer.

2.4. Photocatalytic activity

The application of the synthesized nanoparticles for thephotodegradation of cyanide was investigated under a visible lightirradiation. Experiments were carried out using a horizontal cylinderannular batch reactor. The photocatalyst was irradiated with a bluefluorescent lamp (150 W, maximum energy at 450 nm) which isdoubly covered with a UV cut filter. The intensity data of UV light isconfirmed to be under the detection limit (0.1 mW/cm2) of a UV


radiometer. In a typical experiment, a desired weight of the catalystwas suspended into a 300 mL, 100 mg/L potassium cyanide (KCN)solution. Ammonia solution was used to set the pH of theexperiment at 10.5 to avoid evolution of HCN gas. The reactionwas carried out isothermally at 25 8C and samples of the reactionmixture were analyzed at different intervals time for a total reactiontime of one hour. The CN� concentration in samples was estimatedby a volumetric titration with AgNO3, using potassium iodide todetermine the titration end-point. The removal efficiency of CN�

was measured by applying the following equation:

% removal efficiency ¼ ðC0 � CÞC0

� 100 (1)

where C0 is the initial concentration of the uncomplexed CN� in thesolution and C is the concentration of unoxidized CN� in thesolution.

3. Results and discussion

3.1. Structural, morphological and compositional characterizations

The XRD patterns of each parent AgInS2 and Pt/AgInS2

nanoparticle samples are compared in Fig. 1. The structural



E.S. Aazam / Journal of Industrial and Engineering Chemistry xxx (2014) xxx–xxx 3

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characteristic of AgInS2 and Pt/AgInS2, are mainly composed oforthorhombic phase AgInS2 (JCPDS Card: 25–1328), whichindicated that the AgInS2 structure remained after doping ofplatinum. However, no diffraction peaks of Pt in the patterns ofPt/AgInS2 samples appeared. This is probably attributable to thelow Pt doping content. Moreover, the data may imply that the Ptis well dispersed within the AgInS2 phase. Pt played a prominentrole in the process of crystallization as can be seen from XRDpatterns showing that the orthorhombic AgInS2 phase charac-teristic diffraction peaks became broad and the diffractionpeaks’ intensity decreased with increased Pt loading. Theaverage crystallite sizes of AgInS2 were calculated by Scherer’sequation using the full width at half maximum of the X-raydiffraction peaks at u = 26.68 corresponding to the most intense

Fig. 3. TEM images of AgInS2 and Pt/AgInS2 nanoparticles, wher


orthorhombic AgInS2 peak. The crystallite size of the AgInS2,0.5 wt% Pt/AgInS2, 1.0 wt% Pt/AgInS2, 1.5 wt% Pt/AgInS2, and2.0 wt% Pt/AgInS2 were 10, 8, 6, 5, and 3 nm, respectively.Therefore, the particle size became smaller as the Pt concentra-tion increased.

To investigate the nature of the Pt introduced into thecomposite, we performed XPS measurements. Fig. 2 shows theXPS analysis for 1.5 wt% Pt/AgInS2. The presence of the peaksassigned to the Pt at about 70.4 and 74 eV indicates the formationof nanosized Pt metal.

The TEM images of AgInS2 and Pt/AgInS2 nanoparticles areshown in Fig. 3. The results reveal that Pt dispersed on the surfaceof the catalyst and diameter of the Pt increased with increases inthe wt% of Pt.

e wt% of Pt is 0.0 (A); 0.5 (B); 1.0 (C); 1.5 (D); and 2.0 (F).



Table 1BET surface area of AgInS2 and Pt/AgInS2 nanoparticles.

Samples SBET (m2/g)

AgInS2 12

0.5 wt% Pt/AgInS2 11

1.0 wt% Pt/AgInS2 9.5



Table 2Band gap energy of AgInS2 and Pt/AgInS2 nanoparticles.

Sample Band gap energy, eV

AgInS2 2.57






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3.2. Surface area analysis

Specific surface area (SBET) of parent AgInS2 and Pt/AgInS2

nanoparticles were determined. The SBET values were 12, 11, 9.5,9.0, and 8.4 m2/g for the AgInS2; 0.5 wt% Pt/AgInS2; 1.0 wt% Pt/AgInS2; 1.5 wt% Pt/AgInS2 and 2.0 wt% Pt/AgInS2, respectively. Thesurface area of parent AgInS2 and Pt/AgInS2 nanoparticles arecollected in Table 1. The surface area of AgInS2 is higher than thatPt/AgInS2 samples due to the blocking of some pores by doping ofPt.

3.3. Optical characterization

The UV–vis diffuse reflectance spectra of the AgInS2 and Pt/AgInS2 nanoparticles are displayed in Fig. 4. The loading of Pt intothe AgInS2 caused a red shift toward higher wavelengths from 492to 549 nm for different loadings of Pt compared to a wavelength ofAgInS2 at about 481 nm. The direct band gap energy for the AgInS2

and Pt/AgInS2 nanoparticles was calculated from their reflectionspectra based on a method suggested by Kumar et al. [36] and theresults are tabulated in Table 2. It is clear that the energy gapdecreased with the increase in the Pt. The band gap values were2.57, 2.52, 2.39, 2.31, and 2.26 eV for the AgInS2; 0.5 wt% Pt/AgInS2;1.0 wt% Pt/AgInS2; 1.5 wt% Pt/AgInS2 and 2.0 wt% Pt/AgInS2,respectively. This result indicates that Pt doping can narrow theband gap of catalysts, which may be beneficial for improving thephotocatalytic activity of the catalysts.

Photoluminescence (Pl) emission spectra have been used tostudy the transfer of the photogenerated electrons and holes and tounderstand the separation and recombination of photogeneratedcharge carries. In order to investigate the photoelectric propertiesof the prepared samples, the Pl spectra were detected for thedifferent samples exited at 270 nm at room temperature as shown

300 400 500 60 0 70 0 80 0 900

Abs

orba

nce,

a.u

.

Wavelength, nm

AgInS2

0.5 wt % Pt/ AgInS2

1.0 wt % Pt/ AgInS2

1.5 wt % Pt/ AgInS2

2.0 wt % Pt/ AgInS2

Fig. 4. UV–vis absorption spectra of AgInS2 and Pt/AgInS2 nanoparticles.


in Fig. 5. It is clear that the Pl intensity greatly decreased with theincrease of the Pt percent. Pt acts as a trapping site to capturephotogenerated electrons from the conduction band, thus sepa-rating the photogenerated electron-hole pairs. It is generallyaccepted that the incorporation of noble metal nanoparticles intothe semiconductor-based catalysts could enhance the lightabsorption of the catalysts in the visible-light region. This leadsto a shift of the absorption edge toward longer wavelength,indicating a decrease in the band gap energy and that morephotogenerated electrons and holes could participate in thephotocatalytic reactions. In the case of Pt, Pt seems to modifythe interface of AgInS2 in a way that altering the mechanism thatphotogenerated charge carriers undergo a recombination orsurface reactions. This would force AgInS2 to be activated morein the visible region. The shift in emission position could beattributed to the charge transfer between the Pt generated bandand the conduction band of AgInS2 as a semiconductor.

3.4. Photocatalytic activity

3.4.1. Effect of catalyst type on photocatalytic removal of cyanide

Fig. 6 shows the photocatalytic removal of cyanide by AgInS2

and Pt/AgInS2 samples under visible light and the experimentcarried out under the following conditions: 100 ppm KCN, 1000 mlvolume of KCN solution and 0.4 gm weight of catalyst. The resultsindicate that AgInS2 has small photocatalytic activity under visiblelight. In addition to, photocatalytic activity of Pt/AgInS2 increasedin the following order 0.5 wt% Pt/AgInS2 <1.0 wt% Pt/AgInS2

<1.5 wt% Pt/AgInS2 �2.0 wt% Pt/AgInS2 which in agreement withXRD, TEM and Band gap. AgInS2 is a visible light photocatalystabsorbing wavelengths shorter than 481 nm. The electrons inAgInS2 valence band are excited and transfer to conduction bandunder visible light irradiation. Then the oxidative species �OH and

500 550 60 0 650 700

Inte

nsity

/a.u

.

Wavelength /nm

AgInS2

0.5 wt % Pt/AgInS2

1.0 w t % Pt/AgInS2

1.5 wt % Pt/AgInS2

2.0 wt % Pt/ AgInS2

Fig. 5. Pl spectra of AgInS2 and Pt/AgInS2 nanoparticles.



0 5 10 15 20 25 30 35 40 45 50 55 600

10

20

30

40

50

60

70

80

90

100P

hoto

cata

lytic

rem

oval

of c

yani

de, %

Reaction time, min

Ag InS2

0.5 wt % Pt/ AgInS2

1.0 wt % Pt/ AgInS2

1.5 wt % Pt/ AgInS2

2.0 wt % Pt/ AgInS2

Fig. 6. Effect of type of catalyst on photocatalytic removal of cyanide.

1 2 3 4 5 60

20

40

60

80

100

Pho

toca

taly

tic r

emov

al o

f cya

nide

, %

No of cycles

Fig. 8. Recycle and reuse of photocatalysts for on photocatalytic removal of cyanide.

0 5 10 15 20 25 30 35 40 45 50 55 600

10

20

30

40

50

60

70

80

90

100

Pho

toca

taly

tic r

emov

al o

f cya

nide

, %

Reaction time, min

0.2 gm 0.3 gm 0.4 gm 0.6 gm 0.8 gm 1.0 gm

Fig. 7. Effect of loading of 1.5 wt% Pt/AgInS2 on photocatalytic removal of cyanide.

E.S. Aazam / Journal of Industrial and Engineering Chemistry xxx (2014) xxx–xxx 5

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photogenerated holes form and decompose the pollutant com-pounds. However, the high recombination rate of photogeneratedcarriers leads to the low photoactivity of pure AgInS2. When the Ptspecies is introduced into the AgInS2 samples, the Pt can act aselectron traps promoting the electron–hole separation andsubsequent transfer the trapped electron to the adsorbed O2

which acting as an electron acceptor on the surface of the AgInS2.The holes still remain in the AgInS2 valence band after migration ofexcited electrons. Therefore, the recombination of electron–holepairs is restrained, and the photocatalytic reaction can beenhanced greatly. It has been reported that the surface of somenoble metals and compounds on some photocatalyst can beexcited by visible light [37–40], enhancing the surface electronexcitation and electron–hole separation and therefore increasephotocatalytic activity.

3.4.2. Effect of photocatalyst amount on photocatalytic removal of

cyanide

The photocatalyst amount was another important parameter ofphotocatalytic removal of cyanide solution under visible lightirradiation. Amounts of 1.5 wt% Pt/AgInS2 ranging from 0.1 to


1.0 g L�1 in 100 mg L�1 KCN solutions were employed in this study.As shown in Fig. 7, an decrease in reaction time which required tooxidized cyanide from 60 to 35 min. was observed with theincrease in catalyst amount from 0.2 g L�1 to 0.8 g L�1, respective-ly. However, further increases of the photocatalyst amount above0.8 g L�1 increase reaction time again to 50 min. The increase in thephotocatalyst amount increased the number of active sites on thephotocatalyst [40]. Consequently, the number of cyanide mole-cules and photons absorbed increased. However, at photocatalystdosages above 0.8 g L�1, the reaction time required to oxidizedcyanide increased due to the blocking of light penetration by theexcessive amount of photocatalysts [41].

3.4.3. Recycling of photocatalyst

Recycling catalysts is one of the key steps for assessing thepractical application of photocatalysts and to develop heteroge-neous photocatalysis technology for wastewater treatment. Anexamination of the photocatalytic activity of the recycled 1.5 wt%Pt/AgInS2 catalyst was carried out. The photocatalytic removal ofcyanide was 100% during the first five cycles (Fig. 8). The resultsreveal that the separation of photocatalyst is effective and thus thephotocatalyst is basically stable and is promising for environmen-tal remediation.

4. Conclusions

In summary, the Pt/AgInS2 photocatalyst was successfullysynthesized and proven to be a promising catalyst due to its highoxidation efficiency of the pollutant under visible light. The redshift phenomenon was found to depend on the wt% of Pt doped onAgInS2, which has been observed in the UV–vis spectra of AgInS2

and Pt/AgInS2 samples. Photocatalytic measurements through thephotocatalytic oxidation of cyanide solution showed that Pt/AgInS2

nanoparticles with 1.5 wt% of Pt exhibited the highest catalyticactivities and efficient photocatalytic properties in water purifica-tion and may find potential applications in related fields.Optimization of reaction conditions led to a conclusion that1.5 wt% Pt/AgInS2 and the use of 0.8 g of the catalyst on a 1000 mL,100 mg/L KCN solution yielded 100% oxidation of the cyanidesolution within 35 min irradiation of visible light. The results ofcatalyst re-use revealed the present photocatalyst remainseffective and active after five cycles, which indicates the promisingrecyclability of the Pt/AgInS2 photocatalyst.




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photocatalytic oxidation of cyanide under visible light by pt doped agins2 nanoparticles

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