IEG 환경지질연구정보센터

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(1)]æ~>Æ·~ã²æ. òY. Vol. 9, No. 1, pp. 54~62, 2004. ÏbR J"* ÆWª FÆ~ ÿ*8 ;z ßWö ^¿B ~º 'Ë. B>â ÁB÷¢ *ÁRçÒ ÁB;~ 1. 1. 1. 2. ·&v ÆÏ~ã" 7&v ÆÏ". 1. 2. The Effect of Flushing Solutions on ElectroKinetic/ Remediation of Ferrous Soil Contaminated by Lead. Á. Á. Á. Soo-Sam Kim1 Byung-Il Kim1 Sang-Jae Han1 Jung-Hwan Kim2 1. Hanyang University, 2Chungang University. ABSTRACT In order to enhance the efficiency of removal a series of ElectroKinetic Remediation (EKR) tests on ferrous soil contaminated by lead are carried out using acids, chelates and surfactant as flushing agents. The test results indicate that pH in the electrolyte rapidly reached at steady state as the introduce of flushing solution of the lower pH, the type of flushing solution have no effect the distribution of electrical voltage within the sample but the increasing of solution concentration increases it at x/L=0.9. In the distribution of the residual lead in the sample SDS is the highest. Also, the removal efficiency for acetic acid concentration of 1mM is the highest but the concentration of acetic acid significantly have no effect. Key words : Ferrous, Electrokinetic remediation, Acis, Chclate, Surfactant. º £ ^. öBº Ïb J"B FV>" ÆWª ï FB ÆWª FÆö & ;z ÎNj ËçÊV * ^¿B Ö, Ò.ÞB 5 êWB¢ ÒÏ~ ÿ*V ;z þj ~& . þÖ" "«>º ^¿B~ pH & Ôj> ·(,z)&>~ pHº z V *ö ;çç 8ö ê~&b, *{ ª

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(3) ¢ & . ^¿B ³ê~ ãÖ 1 mM~ Acetic acidöB &Ë ·^ ;zÎNj &æò, j^ÞÖ~ ³ê æzº Æ Wª FÆ(Ferrous soil)~ ÿ*V ;z ÎNö 'Ëj ~æ Fº ©b ¾æÒ . *Ú : Æ9ª FÆ, ÿ*8 ;z, Ö, Ò.ÞB, ê9B 1.. * V. &¦ª~ þf EK ÎN ·^ RÒ¾Þ j &ç ò þ ãÖ`, ¢¢Þf ?f ¶ Æö z &rÚ òö & \º ç&'b ' . RÒ¾Þ~ ãÖ &æ*~%>(Variable charge mineral) ·N L~Ë(CEC) pHö ~'`, ¢¢Þ~. &R>W~

(4) z æ>ö Ôf >&~ ç~ *VËj ' Ï~º ÿ*V(~ EK) ;z VF 7.³ $º FV > J"* æ>ö ç Î¢ ® . ¾,. 1). *Corresponding author : [email protected] : 2003. 11. 13 : 2003. 12. 12 : 2004. 6. 30. ö%>¢ î~ # Æ~. ²Òß¢ Hæ. 54.

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(6) ~ ®º êWB Ò ;Öj ÒÏ~&j ãÖ ~ WWª 7 ¢¦& ÏF > ® º ^B , Ò.Þf ?f ãÖ ÒÏ ê ¾Ò>~ ² > ^B BV>Vê ~&V H^ö , ö & ' . ~& jº~ . öBº FVb" ÆWª ï FB ¶Æ ö & ÿ*V ËçV»~ 'Ï" ËçV» ê ;zßW j «~¶ Ú ¶Æö &~ ¢N~ ÿ*V ^ ¿ þj ~& . ^¿Bº Ö(j^ÞÖ, "Ö), Ò .ÞB(Ö, EDTA) 5 rNW êWB(SDS)¢ F;~&, ³ê ~ ãÖ j^ÞÖj F;~ 0, 1, 10, 50, 100 mM ³ê æzö 8 ÿ*V ;z ßWj «~¶ ~& . 1). 2). 1). 3~4). 55. ö ~ B> , Ö ;> 7.³~ BNf ËçB . ¾, Steele and Pichtel(1998) ö 8 Ï ºÂÎNf Ö~ ³êö j~'ª BB : ® . H+). 6). 7). 8). 2.2 Acetic acid. º ; ¶W~ êî& ¾º Zï~ Ú, ª¶ï 60.05, º6 16.6 C, pº6 117.8 C, j7 1.0492 . £Ö, 1 mol >ÏöBº 0.4%;ê Ò~ j^ÞÖN" >²N B . ï '~ Ö;z>V Öæ ÎÞÆöº Ö;ç& >º ©j .Ö¢ . Cline and Reed(1993) ~ ã Ö Æîö Acetic acid¢ ^¿B ÒÏ þj Û BNf ÆîF;" ^¿B~ ³êö 'Ëj Aæ p~ B~& . Ëã>(2003) ~ ãÖ Ëçbî ÏB .Öj "«bB .ç>º >wf (1) " (2)f ? ~& . (1)öBf ? .Ö~ Ôf pH 6ÆRö O* 7.³ Nz>Ú îO Ï~² B . $ (2)ö BB :f ? r ¦"ö ;WB >Öz *>j ÏB .Öj "« bB Ï >ö Ï>² B . Acetic acid(CH3COOH). o. o. 9). 10). Pb2+ (clay)2− + 2CH3COO− + 2H+. 2H. +. (clay)2− + Pb2+ + 2CH3COO−. (1). 2CH3COO− + 2H+ + Pb(OH)2. 2CH COO. −. 3. + Pb2+ + 2H2O. (2). 5). 2.. ^¿*~ ßW # J"> *` zî¾. Ö(HCl; Hydrochloric acid) "Ö~ j7f 1.190, ª¶ïf 36.46 g . Û Zï ³ê 35% ç~ ©j ê "Ö¢ ~, ê "Öf ¶' êî& ¾º Ï . HCl~ ãÖ Ïf Ôf pHöB~ ËçB îO 5 Nv~(Pb ö & 2.1. 2+. 2.3 SDS(Sodium Dodecyl Sulfate). º rNW êWB CMCº 8 mM;ê . z' Wf(H C-(CH ) -CH OSO -Na ), ª¶ïf 288 gb ÛJW ± . SDSf ? Ö" Nj

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(8) ~º Æ·~ 'Ïö º ê& ® B~& . SDS¢ "«~&j ãÖ Æ·R" BF 7.³~ îO >wj â 1ö B~& . 1êöBº Æ· R ö îf O~, 2êöB Æ· Rö OB .³"~ ç^·Ïj Û êWBf .³ îO>² B (3ê). V¢B 4êöBº Æ· Rb¦V ÎÚ 11). SDS. 3. 2 10. 2. 3. 2. 3). Journal of KoSSGE Vol. 9, No. 1, pp. 54~62, 2004.

(9) B>âÁB÷¢ÁçÒÁB;~. 56. Fig. 3. Schematic illustration of the citric acid and Pb2+ reaction.. Fig. 1. Desorption mechanism of heavy metals by anionic surfactants (Modified from Mulligan et al., 1999).. .³ FVb Ob(Metal-organic complex) ; £² îOÚÚ 7.³ ¶FN(Free metal ion)ö ~ ëW ^B¢ 6²Ò > ®, îOê V Ú Ob ; B Æ· Ú R"ö ^B& ìº ©b rJ^ ® . .³" ç&'b n; Obj ;W~º citric acid f ?f FVÖf formic¾ lactic acidf ? n; Obj ;W~æ pº © ö j Æ·b¦V .³j Fÿz Êº potentialj <º . ö~, & ª¶ï FV rN(organic anions) FV Ò*(Ligand) ·Ï~V r^, r 7.³~ Fÿz¢ Ã& Êº 3&æ ãº Ñ Ò* v~(ligand-exchange) >wj Û Æ· Rö OB .³j ~~ö ~, ~ .³j O .³-Özb Rj Ïö ~, q Ï ÚöB .³j Obzö ~B . $ º ¾ÒB 7.³~ Ï Ú ;º FVÖ ³ê 10 mM çb ¾Ò ãÖ &¦ª .³-FVb Ob~ ; ¢ &ææ .³ ¶FNö ~ ëW^Bº ìº © b , FVÖ~ ;º 7.³" Obj ¾ ¶FN ç(Cit ) _f organic-H~ ;(HCit , H Cit , H Cit) Ò~æ 7.³ ¾Òê FÂ>ö Ò~º F VÖj ç¦ª ²>~ ÒÒÏ > ® ~& . Citric acid "«ö ~ R" Ï~ .ç>º ÿ f j¾f ? ( (3), â 3). 12). 13). Fig. 2. Schematic of anionic surfactant micelle containing solubilized organic and bound counterions (Modified from Somasundaran and Krishnakumar, 1997).. ^ ¾N .³" êWB& ÿ~B, Ö .³ O >j ;W~² B (5ê). â 2º â 1öB ;WB êWB-.³ O> 1 & $º 2& ·NW .³ >& &*B îf~ R ö Ö(Bind)>Ú îf Wj r > ®V r^ö ÿ*V ;z &N *j Ë~ ÿ > ® º © j B © . \Ö) Öf &ª¶ FVÖb bö ¾ º ;Ö, ; K Ò.ÞB . ª¶ïf 210.14 g, ª¶f HOOCCH (COH)(COOH)CH COOHÁ2H O $º C H (OH) (COOH) R*B . FVÖ 7.³" ; OzË K(Complexing ability)j &^ Æ· Ú J"B 7.³j 2.4 Citric acid(. 2. 2. 2. 3. Journal of KoSSGE Vol. 9, No. 1, pp. 54~62, 2004. 3. 3. 3−. 2−. 2. −. 3. Soil − Pb + HOOCCH2 (COH) (COOH) CH2COO− + H+. Soil − H + Pb +. 2+. +. HOOCCH2 (COH) (COOH)CH2COO−. (3). 2.5 EDTA(Ethylenediaminetetraacetic acid). º &¦ª~ .³" ; >ÏW Ò.Þ¢ ; W~º ËKj &æ ®V r^ö 7.³b J"B b¦V 7.³j ºÂ~V *B ÒÏB . bö & Ïêº 22 CöB 100 ml~ bö 0.2 g º . ª ¶ïf 404.47 g . EDTA4-Nf C 6B~ ÒÞö EDTA. 2). o.

(10) ÏbR J"* Æ9ª FÆ~ ÿ*8 ;z ß9ö ^¿B ~º Ë. 57. pö Ò~º b, Gnb 6ê~&j r ¯f j j ®î . 1" 2öº ò~ V bW 5 æ >~ã' ßWj B~& . XF ;7ªC(XRF) Ö" 3" ?f Ö"¢ áj > ®î . SiO f Al O & "Wªb ¾æÒb`, Fe O & 7.67% ç® ¸f 8j ® . 2. 2. 3. 2. 3. ÿ*8 ;z þ 3.2.1 EK ;z þ Ë~ EK ;z þ Ë~º f Ú 5 Ö¦ W>Ú ®. . f Úº C 5&æ þ ÿö >¯F > ®ê '' ªÒ >Ú ®Ú *{ 5 ^¿Ï~ F« 5 ¾Ò> ~ FÂ '' ëã'b Úê (â 5). ¦öB ~ ÿ>ãÒ ;Wj Oæ~V * f~ ·¦öº ^¿ Ï Ú ®º îÒJ :æ(Mariotte bottle)j J~~& b`, r¦öº ¶F² ú~(Overflow)& &Ë~ê ~& . $, ¦³ Ë~º ''~ *~öB *{j G; > ®º *{G;Ï ö" ò¢ ªÒ~V * ò .Ï Æ6, ê² * 5 Porous stone ® . 3.2. Fig. 4. EDTA complex of Pb2+ : [Pb(EDTA)]2−.. B .³" 7 > ® (6¶Ò Ò*). ¯, 4B~ Acetate " 2B~ î² ö¶& FÖj ;W~V * Ò ÏF > ®º ¶F*¶3(jF *¶3)j &æ ® ( â 4). &¦ª~ .³-EDTA Ò.Þº rb &*>Ú ®V r^ö, EOf EMö ~ ·b Ë~ ÿ > ® . 2). 3.. þ. ò ß9 öB ÒÏ òº .V pH& 4.9 ¢> Ö Æ ·&v nÖÆ¢Ê~ " Ö~ æöB 50 cm. þ öBº 4~ 5f ? ² ^¿B «~ê þ" ^¿B ³êê þj ~& . ^¿B «~~ ãÖ HCl, Acetic acidº ÏB, Citric acidf EDTAº Ò.ÞB Ò SDSº êWB ÒÏ>îb, ^¿B ³ê öBº Acetic acid¢ Ò 3.2.2. 3.1. Table 1. Sample properties Specific gravity 2.604. Liquid limit (%) 37.1. Plastic index 8.88. Activity. USCS. 4.1. ML. Table 2. Geoenvironmental properties of the sample Initial pH 4.9. CEC (=meq/100 g dry soil) 6.68. Organic content (%) 9.85. Carbonate content (%) 1.23. Specific area (m2/g) 30.4. Fig. 5. Schematic diagram of EK test cell. Table 3. XRF Result SiO2 (Wt%) 58.84. Al2O3 (Wt%) 20.63. TiO2 (Wt%) 0.86. Fe2O3 (Wt%) 7.67. MgO (Wt%) 0.78. CaO (Wt%) 0.10. Na2O (Wt%) 0.12. K2O (Wt%) 2.29. MnO (Wt%) 0.03. P2O5 (Wt%) 0.07. L.O.I. (Wt%) 9.04. total (Wt%) 100.43. Journal of KoSSGE Vol. 9, No. 1, pp. 54~62, 2004.

(11) B>âÁB÷¢ÁRçÒÁB;~. 58 Table 4. Test conditions (Flushing solution) Pb C0 (mg/kg). Fixed factors Duration (days). Variable factors Volt. (V/cm). Agents. 1000. 15. 1.0. Initial Conc. (mM) Initial pH. HCl. Acetic. Citric. EDTA. SDS. 50. 50. 50. 50. 50. 1.79. 3.07. 2.54. 3.13. 4.67. Table 5. Test condition (Concentration) Pb C0 (mg/kg). Fixed factors Duration (days). Variable factors Volt. (V/cm). 1000. 20. 1.0. Flushing agents(Acetic acid) Initial Conc. (mM) Initial pH. Ï~& . º j^ÞÖ ÒÏ>z¢ê ~ *V*ê ê¢ ² Ã&Êæ p, ~ã'b n*~ ª F > ®V r^, $ j^rÞNf r ¦" öB jÏW "~ ;Wj Oæ~ Ôf *V*êê ' ~ B* 5 r ¦"öB~ "ê ö.æ ²Öj ï j > ® º Ë6j &æ ®V r^ . v þ Îv *{ãÒº ÿ¢~² 'Ï>î . 14). ;z þ O» b& *ËöB v¦B ç jB ò¢ 110Û5 C ~ öB 24* ç ê No. 40Ú¢ Ï~ «¶¢ B~& . No. 40Ú¢ Û" ò¢ W ê ç~ >j& >ê îÖÏ(Pb(NO ) )" jN >¢ b~ BB .V Ï ³ê& 1000 mg/kg b >¢ Î&~ ÛJò¢ B~& . BB ò¢ EK f~ ' _~ö FÒ ·b R« r f~ Ú¢ ¾Z~ £~² £ 50² ;ê æÏ ê ò~ öb ~ BB n *ö bB ò¢ R«~ ¾Z~ æÏ~& . ¢; ¸ ~ ò& ^æ æ pj r ræ f ?f ";j >~& . « ' _~ö R«B ò~ ·öº N& ìrj .j þ j Û { > ®îb, þ Ö"öº 'Ëj ~æ pj ©b 6~ þj ê¯~& . 3.2.3 EK. o. 3 2. 7.³~ ³ê G; O» Ïö & ³ê ï&º Æ·J";þ»ö &~ >¯~& . ¯, ³ò 10 gö 0.1N HCl Ï 50 mL ¢ I 1* êû ê ª«(Whatman No. 42) "~ j ICP¢ Ï~ ªC~& . 3.2.4. Journal of KoSSGE Vol. 9, No. 1, pp. 54~62, 2004. 0. 1. 10. 50. 100. 6.36. 3.74. 3.28. 3.01. 2.85. 4.. þ Ö # ª+. 4.1 ·(,z)&>ö*~ pH æz >~ *Vª >wj Û (+)öB W>º >² N (−)öB W>º >ÖzNö ~ (+)öB~ pHº £ 3~ræ 6²~`, (−)öBº £ 11çræ Ã& . f ?f Ö& \~ ÿ*V ;z þ öBê ¾æÒ (â 6). ^¿B «~fº ~ çì (−)öB~ pHº j" *ö ;çç 8ö ê ~&b`, (+)~ ãÖ HCl &Ë *ö ;çç 8ö ê~& . º HCl~ .V pH& 1.79 &Ë ÔV H^ . (+)öB~ pH 8f SDS, Citric acid, Acetic acid Ò EDTA Bb ¸² ¾æÒb`, ;ç çö ê~º *ê z ¶Ò² ¾æÒ . EDTA~ ã Ö (+)öB~ pHº ~ * ;zV*ö ö ¸f 8j &b`, jL' æz ©b ¾æÒ . f ? f Ö ~ EDTA~ ãÖ òÚ¦~ Ö*F~ ÿ ² ÚJj ©b $B . ^¿Ïj Acetic acid ;Ê ³ê¢ Ò þöBº (+)öB pH& 1 mM¢ B~ Îv FÒ Ö¢ & .. òÚ *{ãÒ~ æz (+)öB ;WB >²N (−)öB ;WB >Öz N ò¾B b ;W>¾, pH 6* 'öB *b~ B b ~ N. B>, ¦ V &Ã& *V*êê~ 6²f *{N~ Ã& & \öBê x/L=0.9æ6öB BB ©b ¾æÒ. . â 7f þ jò ç* ò Ú¦öB~ *{ ª

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(13) ÏbR J"* Æ9ª FÆ~ ÿ*8 ;z ß9ö ^¿B ~º Ë. Fig. 6. Changes in pH of the electrolyte with elapsed time.. 59. Fig. 8. Changes in electrical potential with elapsed time (at x/ L=0.9).. ¾æ p~b`, ³ê ~ ãÖ ³ê& Ã&ö V¢ (+)b¦V ;z* Ò 0.9æ6öB~ *{f z ² ¾æ¾º ãËj & . º ^¿ÏöB~ j^ ÞÖ~ ³ê Ã&ö V *>öB~ N Ã& 5 ö V *V*êê~ Ã& r^¢ $* . *ö V 0.9æ6öB~ *{~ æz ·çj ¾æÞ â 8~ ãÖ SDS& &Ë ·f *{j & . EDTA~ ãÖ *{~ æz V* z ^² ²º>î . * ;zV *ö ö ^¿B «~ê jv , SDS<HCl< Acetic ~ Citric<EDTABb ¾æÒ . ^¿B ³ê~ ã Ö 0<10 ~ 50<1<100 mM Bb *{~ æz·çj & b, &Ú ³ê& Ã&ö V¢ 0.9æ6öB~ N ³ê 5 *V *êê~ Ã& ~ *{f Ã&~º ãËj & . þê >j ª

(14) þ ê >j ª

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(16) 60. B>âÁB÷¢ÁRçÒÁB;~. Fig. 9. Distribution of normalized water content within the test sample.. Fig. 10. pH Distribution within the test sample after tests.. >j £* ² ¾æÂ ©b $B . (−) ¦ "~ ãÖ *î Ï~ (−)b~ FÂ ~ . V >j £* 6² ©b $>, SDS~ ãÖ 0.7æ6öB &Ë >j æz& ©f â 7ö BB *{ ª

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(18) ÆWª FÆö & ÿ*V Ëç þ ê ò Ú¦ öB~ pH¢ â 10ö B~& . âö BB :f ? ~ * º*ö ö pHº .V~f jv~ æz¢ æ p~ . º öB ÒÏB ò& ¸f FVbï" ÆÖzb ïj &rV r^ö 4.4. Journal of KoSSGE Vol. 9, No. 1, pp. 54~62, 2004. þ ê ³ê ª

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(24) ÏbR J"* Æ9ª FÆ~ ÿ*8 ;z ß9ö ^¿B ~º Ë. Fig. 11. Distribution of the residual lead within the test sample.. ·(+)b ÿ~æò >&OË(-)b~ *VN ÿ(EM)ö ~ O¢ AV H^ö ò~ 7¦ö » ' * ©b $* . ^¿B ³ê~ ãÖ Ï~ ª

(25) ·çöBº ^¿B~ F Zö 8¢ ÿ ·ç ² ¾æÒ . ¯, ^¿B& ÒÏ>æ pf BlankþöBº r ¦"öB &Ë ³ê~ 6²& &æò, ^¿B& ÒÏB ãÖ (+) ¦ "öBê ³ê~ *' B~& . (+) ¦"öB~ ³ ê *'f 1<100<10 ~ 50 mMBb ¾æÒb`, r ¦ "öBº Î ³ê& 6²¢ & . *Ú' ãË j "H 1 mM~ Acetic acidöB &Ë ·^ ;zÎNj &b, Wong et al.(1997) Acar and Alshawebkeh (1993) & B :f ? j^ÞÖ~ ³ê æzº Æ Wª FÆ~ ÿ*V ;z ÎNö 'Ëj ~æ p º ©b $B . 4). 15). 5.. Ö V. ^¿B Ö, Ò.ÞB 5 êWB¢ ÒÏ~ F. 61. Vb ÆWª ï FB ÆWª FÆ(Ferrous soil) ö &~ ËçB ÿ*V ;z ßW þ Ö. r ?f Öj áj > ®î . 1. "«>º ^¿B~ pH& Ôj> ·(,z)&> ~ pHº z *ö ;çç 8ö ê~& . 2. þ jò ç* ò Ú¦öB~ *{ ª

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(29) ¢ & . SDS& &Ë ¸f º~ Ï³ê¢ Fº .V pH& 4.67 &Ë ¸j Ï~ îO Ï~æ p~V H^ ©b $B . 5. ^¿B ³ê~ ãÖ 1 mM~ Acetic acidöB &Ë · ^ ;zÎNj &æò, j^ÞÖ~ ³ê æzº ÆW ª FÆ~ ÿ*V ;z ÎNö 'Ëj ~æ pº ©b ¾æÒ .. ^^ò 1. Li, R.S.O., “A study of the efficiency and enhancement of electro-kinetic extraction of a heavy metal from contaminated soils”, Ph.D thesis, McGill University, Montreal, Canada, p. 224 (1997). 2. Yeung, A.T., Hsu, C.N., and Menon, R.M., “EDTAenhanced electrokinetic extraction of lead”, J. of Geotechnical Engineering, 122(8), pp. 666-673 (1996). Column 3. ,“. Òö Æ·^¿j *R êRWB~ F;V»" j ÏR

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