Observations on the Interaction of Ion Exchange Resins with Some Cupric Compounds Citation Ferington, Thomas Edwin (1952) Observations on the Interaction of Ion Exchange Resins with Some Cupric Compounds. Master's thesis, California Institute of Technology. doi:10.7907/CMRX-8587. https://resolver.caltech.edu/CaltechTHESIS:10162017-102130831 Abstract The interaction of the Sulfonic Acid Resin, Nalcite HCR, with Cu II halide solutions was studied in hope of obtaining dissociation constants for the complex ions CuX + . The fact that CuX + is absorbed by the resin to an appreciable extent prevented the attainmnet of this goal. It was found in the case of CuF + that the complex ion is absorbed even more strongly than Cu ++ . The presence of a Cu ++ -F - complex was indicated by spectrophotometric observations. The action of the carboxylic acid resin, IRC - 50 was studied in a column. It was found that the volume of the resin in the Cu ++ salt form depended on the salt with which the resin was treated. In the case of solutions of Cu(OAc) 2 it was found that Cu(OAc) + was taken into the resin as well as Cu ++ . A titration curve for IRC - 50 with NaOH in solutions of ionic strength one is given. Item Type: Thesis (Master's thesis) Subject Keywords: Chemistry Degree Grantor: California Institute of Technology Division: Chemistry and Chemical Engineering Major Option: Chemistry Thesis Availability: Public (worldwide access) Research Advisor(s): Davidson, Norman R. Thesis Committee: Unknown, Unknown Defense Date: 1951 Record Number: CaltechTHESIS:10162017-102130831 Persistent URL: https://resolver.caltech.edu/CaltechTHESIS:10162017-102130831 DOI: 10.7907/CMRX-8587 Default Usage Policy: No commercial reproduction, distribution, display or performance rights in this work are provided. ID Code: 10518 Collection: CaltechTHESIS Deposited By: Benjamin Perez Deposited On: 16 Oct 2017 19:34 Last Modified: 02 May 2023 16:30 Thesis Files Preview PDF - Final Version See Usage Policy. 4MB Repository Staff Only: item control page

Obs ervati ons on the Intera ction of Ion Excha ng e Resins with s ome Cu·oric Comuounds Thesis by Thomas Edwin Ferington In Parti a l Fulfillment of the Re quirements for the Degree of Ma ster of Science Ca liforni a Institute of Technology Pas a dena , Ca liforni a 1951 AcknoviTl e dgement The a uthor wishes to exnress his sincere apnrecia tion a nd gr atitude to Dr. Norman Davidson , who suggested this work a nd under whose guidance it was ca rried out. Abstract The intera ction of the Sulfonic Acid Resin, Nalcite HCR, with Curr helide solutions was studied in hope of obt a ining dissociation const a nts for the complex ions Cux+ . The f a ct tha t CuX ~ is absorbed by the resin to an appreciable extent prevented the att a inment of this goa l. It was found in the cas e of CuF + that the complex ion is abs orbed even more strongly tha n cu+"' . The nresence of a Cu........- F - complex was indica ted by spectrophotometric observations. The action of the carboxylic acid resin, IRC50 was studied in a colwnn. It vras found that the volume of the resin in the cu+• salt form de ue nded on the s a lt with which the resin was treated. In the cas e of solutions of CU.(0Ac) 2 it was found that Cu(OAc)+ was taken into the resin as well as Cu.,..+ . A titration curve for IRC - 50 with NaOH in solutions of ionic strength one is given. ~able of Contents Psrt I Pag e Interaction of a stron~ a ci d resin 1 with solutions containing ions of ,.._ the ty ~ e CuX : II Introduction ~xDe rimental 3 Results 4 Con clusion 10 'i1he Inter ac t ion of various Cu+...,.. solutions with Colmnns of Resin i!:xnerimental 12 l?. esults 13 III Batch Study of IRC - 50 Resin 17 IV Hef erences 20 - 1 - Part I Inter a ctions of a strong acid Resin 1Nith solutions containing ions of the type CuX -tIntroduction McConnell a n d Davidson (1) have determined the const a nts for the re a ctions Cu+++ Cl CuCl+ to be: -- ..f- Cl- - cuci,.. k1 CuC1 2 k2 k1 -- 1.30 .=I= .03 k2 -- 25.2° c .23 :l:: .15 by s pectrophotometric mea ns, at~ = 1. N!!.sl!nsen (2), however, g ives k 1 =.34 under the same conditions. Schubert (3), Schubert and Richter (4} and Schubert, Russell and Myers (5) have studied the dissoci ation constants of several complex ions, which are neutral or have a negative charge, by means o:f ca tion exchange resins using tracer amounts of cation in solution. It was hoped that by using a similar method we could determine the constant for CuCl + with sufficient accuracy to warrant a decision between the two values mentioned above. Since it has been observed (6,7) that divalent ions are much more strongly t aken up by a n ion exchanger than monova lent ones, we made the a ssumption that the absorption of CuCl +- by the resin would be ne gli g ible. In such a case the situation in the - 2 s olution vvhi ch is in cont a ct with the resin is as follows. 'I'here a re t wo e q uilibria competing for Cu -r-1( 1) Cu +..f- + 2NaR CuR2 + + Cl- + Cu-"+ (2 ) where NaR refers to~he CuCl 2Na+ . k' ~ k.l sodium s a lt form of the resin a nd CuR 2 to the co pper s a lt form. but the amounts of Cu++-and CuR 2 which are involved 2 a re so small tha t the ratio (Na ~ / (NaR ) 2 is con- st a nt a nd we ma y write Let: c0 - - the initia l amount of Cu ~r 1Jresent in the solution in a ny form. cf = the fin a l amount of Cut-+ in solution in a ny form. c 0 - cf = A c = amount of Cu-r+-tak en u p by the resin. then kR 0 (CuR ~ (cu+ F)11 +-ki (c1-)) = L f-koaki(Cl-) where kR refers to the c as e in which (Cl-) so k. l -- 0 - 3 - v, the volume of the solution a nd w, the weight of the resin were kept const a nt in a ll experiments. Experimental The experiments were carried out a t unit ionic strengt h , using sodium perchlorate made by neutra lizing perchloric acid with ca rbonate free NaOH to maint a in this strength. The sulfonic acid resin used was Nalcite HCR distributed by the. National AluJninate Corporation l a lso available as Dowex 50 (8) ). It was converte d to the s odium form for use in these experiments by washing with a satura te d solution of NaCl until the effluent liq_uid was neutra l a nd t he n ·washing with dis tilled water until chloride free, The resin was dri ed in a ir at room t emper ature to cons t a nt weight a nd used in tha t state. 'I'he c apacity of the res in for Cu;--+ 11\TB.S determined by s a tur ating a small column of it with a solution of 0 .5F Cu(Cl04) 2 • The cu++- was washed out wit h NaCl solution a nd det ermine d . As a che ck the col- umn was then s s.tur ate d with o. 5F CuC1 2 solution a nd the Cu++- again determi ned. 'rhe capa city of both the H1' and Na -t-forms was 3. 75 me q . of Cu t-+-per gr aro. of air dried resin . 'rhe method of a na lysis for Cu+.-r was that of Moeller ( 9) , which uses th e yellow complex formed by Cu-t-+- with 8- hydroxyq_uinoline so l utions in chloroform. Optical density re adings were t aken on a Beckman Model DU Spectronhotometer. The chemic c ls used were a ll re agent gr a de. The solutions to be studied were pl s.ce d in ti ghtly stoppered test tubes with the resin a nd f a stened to a slowly rot ating shaft so that they were thoroughly mixed for 24 hours. It was found that the a ir in the mixing appar atus var ied from 26° to 28° during this period. It has been pointed out in a recent a rticle (10) that the dry resin when ula ced in solution t a kes up some water in swelling a nd thus changes the concentra ti on of the fin a l solution even before e ny exchange takes pl a ce. This effect makes the finsl observed concentra tion l a r ger than it would be if a ll of the ;,~rater were still in the solution . When 2 g . of my air dried resin were ulaced on a V\ratch gl ass in a desicc a tor with a be aker of lF NaC10 4 aqueous solution (vapor pres s ure about 17mm at 30°) it was found that it ha d gained 0.653 g . in wei ght a fter 16 days when equilibrium was nearly at t a ined. I have used this va lue in comnut;.. ing Cf (corr.) in the t a bles. Results The precision of the method may be jud ~ ed from the de termina tion of A c 0 /c~ as given in TRble I. -5 Ta ble I co ( F) c ~ (F ) 0 c~(corr.)(F) A c 0 (F ) A c0 CV- 5.06)(10-5 2.53 x10-5 2 .49x 10 -5 2 .57x 10-5 1.03 2. ooX1 o- 1+ i.02 .(10-4 i. oo ><Lo-4 l.00" 10-4 1. 00 5.06 )(10-5 2. 5o x10-5 2.46~10-5 2.60 ,u o-5 1.05 5 .06 "10-5 2.64x 10-5 2.6o xi o-5 2.46 ~10-5 0. 95 5o06" lo-5 2 .61 X"l0-5 2.56x 10-5 2.66 rj_o-5 1.0~- Aver age value of A c0 /c~ = 1.01;:!:: .03 The results of the study of the Cu-++ - Cl- solutions a re shovm in Ta ble II. In the first colunn of the t able the first m.unber in e a ch groun refers to the cu-+1- concentra tion , ~ the second to t he NaClOL1- concentra tion a nd the third to the chloride ion (Na Cl) concentra tion. All other fi gures refer to concentra tion of Cu -J+. Ta ble I I c 0 ( :E' ) cf (F) 5.28 ~10-5 .75 . 25 2. 87 (1.o-5 2. s2 x10-5 2.46'(10-5 . 873 .65 J.61~10-5 3.54"'1 o-5 2 .04x10-5 .576 i.oo cf (corr. ) A c(F) .. -· A C . Cf ki 5.66x 10-5 .50 .50 5. 5sx 10-5 .25 .75 5.301<. l0-5 .06 .94 - 6 Ta ble II (cont.) ~ c(F) k·1 .A c cf l.10 ~10-4 2.00( 10-4 l.os <i.o-4 .92~ 10-4 . 852 .74 .61",10-4 .521 l.oo .75 .25 2.021(10-4 .50 .50 1. 99( 10-4 .25 .75 l.80x:l0-4 .06 .94 Averag e va lue of ki .87;:1:: .12 In these experiments as in all those that follow 2 g . of resin were used in 40 ml. of solution. rhe value of ki is f a irly const a nt, but unfor- 1 tuna tely it is a lmost exa ctly h a lfway between the t wo v a lues mentioned a bove so it doe s not hel u to decide between them. It seems that the a bsorption of CuCl+ by the resin is great enough to interfere with a ny qua ntitative result in this ca se. cu++ - Br- and cu++ - F- solutions vvere a lso studied in t he hope of obt a ining at lea st a series which would g ive the relative complexing nower of Br-,c1- a nd Ir'for Cu '*"_,. in aqueous solution at unit ionic strength. The experiment s.I methods were the same a s those us ed above in the case of c1-. The results of the study of Br- a re g iven in Table III. In the first column the arra ng ement is the s ame a s in Ta ble II. - 7 Ta ble III c (F) 0 5~16 )(10-5 cf (F) cf (corr.) A c (F) k·l. il cf' 2 064 (10-5 2.59 ~10-5 2.57(10-5 .992 .07 5.63 (lo-5 .50 050 2. 95 >'1 0-5 2 .9ox-10-5 2.73)(10-5 .942 .J.4 50061'10-5 025 075 2.89)(10-5 2 .. 84 ~10- 5 2 .22 JC10-5 .782 .39 5 .19J<10-5 . .06 094 2.841'10-5 2 o. 791'}.o-5 2.40,c10-5 .825 .. 18 lo93Xlo-4 .75 . 25 i.211'10-4 1.191':10"'"4 . 74 ~10-4 .621 (2 o5 2.04"-10-4 .50 .50 1.341'10-4 l.32 iq o-4 • 72 ~10-4 .545 (1.7 } 1.94)(10-4 .25 .75 1.241<10-4 l . 22-1a o-4 .72~ 10-4 .590 { 5.05ic10-5 .75 . 25 2.611'10-5 2.56~ 10-5 2.49 ~10-5 .973 .16 5.27x10-5 .50 .50 3.861'10-5 3 79"10-5 l.48 ~10-5 ,390 ( 3 .18) 4.94x10-5 025 075 2.66 )(10-5 2.62 1<10-5 2.321'10-5 .886 .19 4-.98Klo-5 .06 .94 3 .OO ?'lQ-5 2o95 J<l0-5 2.03 1'].o-5 .689 ,50 l.85,c10-4 .75 .25 l.02 xi o-4 l.oo ,c10-4 ,85.~n o-4 .85 { . 76) .75 .25 0 } .95) - 8 - Table III (cont.) cf (F) cf (corr.) ~ c (F) ~ cf' ki 1. 8D(lo-4 .50 ; 50 lo02 Xlo-4 l.00K10-4 .81}<10-4 081 .50 1. 75 ·•,n o-4 .25 .75 1.011'10-4 • 99 .xio-4 .767(10-4 .769 .42 c 0 (F) Average value of ki -- .28;:\::i ,15 The values in parentheses were left out in calculating the average value because they were so far away from the others. Three of them were done at the same time and under the s ame experimental conditions so apparently something interfered with that batch. Again there is some constancy indicated, but the value does not compare well with that of 2.l::P.25 obtained by P. Farrington (11) by spectrophotometric means. The case of cu +i' - F- solutions which was studied last vvas interesting because the results were so unexpected. It was impossible to prepare lF solutions of NaF due to the limited solubility of the salt. Table IV gives the experimental results for this case 0 In the first column of the table, the first number in each group refers to the Cu -t + concentration, the second number to the NaF and the third to the Nac10 . 4 All other figures refer to the concent:ra:t ion of cu"'"+. - 9 Ta ble IV cf (F ) cr(corr.) 4 c (F) fj. c cf 4.7tJ<.10 -5 .90 o87lCl o- 5 o86 XJ.o-5 3. 9C»C lo-5 4 . 54 5.05 .xJ..o-5 018 2'. 321'10- 5 2 . 28,c.10- 5 2 . 77 x10- 5 1 . 21 5.5o x10- 5 .54 l o94 Kl0 - 5 .Bo 1.88 040 5 .29 "10- 5 l o52Xlo-5 1 .. 49 )(1.0-5 2.54 .90 *This value is a little sma ll due to difficulties in the a nalysis . The expectation in each of the above ca ses ha d been that the ad dition of a complexing a gent to the solution would decrea se the A.mount of co pper t aken up by the resin o Th i s expect a tion was re a lized in the c Bs e of c1- e.nd Br- , but when F- was added to the solution the amount of copper which was t a ken u p was increased (compA re Table I). to the presence of a This effect may be due copper fluoride positively char ge d complex which i s more strongly a bsorbed in the resin than Cu+-t-" If CuF+ ha s a smaller ionic radius thc:in hydrat ed Cu ... ..,_ t his expl a na tion is proba bly true, since it has been found that the a ffinity of a resin for a cati on increa ses a s the hydra ted r a dius of the ion decre a ses (6 ) . Another possible expl a nation for the ef- feet would be tha t the F- ion has some sort of unusua l - 10 - influence on the resin and alters the e quilibrium. This does not seem too likely. A spectrophotometric st·udy wa s made of the Cu+t- - Fsystem to see if a complex was present . presented on Graph I. The result is Curve 1 is obtained from a 0.01215 F Cu(d10 4 )2 solution; curve 2 from a 0.9 F NaF solution; curve 3 was obt a ined by a dding curves 1 and 2, and · curve 4 was obt s ined frorri a solution which was 0.01215 Fin Cu~.,_ and 0 . 9 Fin NaF. It an ne ars from the difference in a bsor ption bet ween curves 3 a nd 4 in the re g ion 230 ~ to 260 1.7""" that R comnlex may be rhis favors the ide a th~t CuF + is more strongly . . ... + held by the resin than Cu o formed. 1 Conclusion for Part I This procedure is not usable for the determination of dissocia tion constants of complex c ations due to the a ffinity of the resin for the complex iori itself. The procedure could be used, hovvever, to determine whether or not a comrilex is nresent if the sy~ te m is such that s pectrophotometric means will not detect it Q GRAPH I - 11 - 2 1.0 .8 .6 .4 .08 .06 .04 .03 .01 230 250 270 ~Cmµ> 290 310 330 - 12 - Part II The Intera ction of Va rious Gu ++ Solutions with Columns of Resin Experimental The ca rboxylic a cid resin I RC - 50 (12 , 13) manufa ctured by the Rohm a nd Haas Com.-pany was studied in a s mall column cont a ining 3.54 g . of the a ir dried H+ form of the resin. In preliminary exneriments it was found that no detectable exchange took pla ce between r the H ~~ form of the resin a nd Cu , solutions so the resin in the column was changed to the Na ..r form before e a ch new expe riment .' by washing it thoroughly with 1 N sodium hydroxide solution. The resin was rinsed with NaCl solution to remove the excess base, wh ile pre venting hydrolysis of the s a lt of the wea.k:l y a cidic resin. Most of the chloride ion was t he n washe d away with small nortions of distilled water. A solution of the s a lt to be tested WFJ..S then allowed to flow slowly throuf,h the col1unn from the top until the blue color of the resin indicated thRt it ·was completely s a turated with cu-t ....-. After a n ex ce ss of the solution was pr:i.ss ed through the column it was washed free of Cu ..-.,.. solution with five 10 ml o portions of water a nd then slowly with 1 F HC104 until the Cu +~ ha d been entirely removed . The resulting solution was diluted until it was less tha n 0 .1 F in Cu ++- to prevent loss of iodine from the solu- -13tion during titration and a n a liQuot a na lyzed for Cu ........ by adding 3 g. KI a nd titrating with O.l N Na.28203 in a n atmosphere of co2 to a starch iodine end uoint (14). Since it was also desired to obt a in a rough measure of the de gree of swelling which the resin underwent in the various solutions, the column was 1Nashed u pward with water before each experiment so that the resin was loosened and was then allowed to settle before the liq_uid wss drawn off a nd the experiment st a rted •. At the end of the ex-periment "bhe column was t apped sharply to help the resin to settle together and the height of the column was me a sured. to 0.3 The results were re produci ble Cffio Results The results of tre ating the resin with various solutions ar e shown in Table v. Table V Solution passed through column Height of column meq absorbe d in resin 1 F NaOH 16.8 cm. 32.2 1 F HCl 10.3 cm. 29.5* 1 F CuS04 14 .2 cm. 31.8 .5 F Cu(OA..c} 2 13.5 cm. 36.4 .. 5 F Cu(Cl04)2 14 o0 cm. 31.5 *The meq_ of HCl used up were determined by evaporating the solution and weighing the residue of NaCl. Some of the NaCl, however, was lost in the process on two attemnts. - 14 In view of the agreement of the other r esults I did not feel that it was worth while to re peat this determina tion. A solution ·wh ich was 0. 5 F in CuCl2 was a lso tried, but a preci pit ate formed in the column so it coul d not be used. The preci pit ate may ha ve be en a ba sic cupric chloride formed by the hydrolysis of the sodium s a lt of the wea kly a cidic resin. It was not possible to prevent the formation of this precipit ate even by the a ddition of a O.lF a cet ate buffer mixture to the solu ti on, The height of the column, which i s a me a sure· of the de gree of s well i ng of the resin, va ries from a l a r ge va lue for the Na + form of the resin to a muc h sma ller one for the resin in the H +- formp The degree of s welling of the r es in is determined by t~e osmotic pressure ins ide the resin particles. In the Na T- form of the resin the a ctive groups a re completely ioniz e d like a s a lt a nd consequently there a re a l a r ge number of Na+ ions to contribute to r a i s ing the osmotic :ore s sure. In the c a se of the cu++- s a lt form of the resin the number of ions is a bout half of that in the first c ~ se so the osmotic pre s sure is lower a nd the s welling less. Fi na l ly , the .H.f- f orm of the res in has few i ons becaus e the weak l y a ci dic gr oups a re only sli sht ly i on iz ed . Th e above exnlai ns t he r esults vvit h CuS04 and Cu ( Cl04 )2 , - 15 but Gu( 0Ac ) 2 i s out of lj_n e in b ot h co J u.rms of the t a ble. '..!..'h e r e sin in cont a ct wit h its s ol ut :i..on d o e s not s wel l. as much as :Lt J oe s in the c e:1s e of ot hc-o r 1 +.- Cu solut i ons a n d more meq of co nner are a bs or b e d from it th a n from the ot he rs. to the f a ct th a t This e f f e ct may be due Cu -t-T- forms conrol exes vvit b c a r b oxv l i c ac i d s ( 1 5 ) and the active groups in the resin a re c a rboxylic a ci r.:' cTouus . ~.'he CuOAc 't- g rou n \\'f) ich ls p resent in t l1e s oluti on n a y mi g r a te into the r es i n as a uni t a n d t ~1 ere u nite wit h s n a ci d [~ rou:o to form a comri lex suc L as Cu ( CA c) ( RCO O) ·wh ic h wou l d be f aj r 1y st a ble. Th e effect of such a cti on would be to re duce the numbe r of i ons or r)articl e s in soli..;_tion insi de the r e~ in a n d thus reduce t h e osmotic press ure s nd s we l ling . The number of mi llie q ui v a lents of co r' n er wh i ch cou ld be t a ken up wou : ct be g re at er due to the f a ct t hat in some c <:1.ses one ac :L(l ic gr oun wou l d suff ice to h old on e Cu -t-t inside t h e resin, wher e a s two s u c h groups. or rl ina r j ly it r e nuires 'i.'he results of the e xr.ie ri.ments :::i re a cc ount ed f or by t he Above. In ord er to in v esti ga t e tb e ef f ec t t ha t comn l ~ xi n~ . a g ent s mi ght have o n th e a b ~:3 orntion of Cu+.,.. by a s trong acid r e sin a s ma ll col umn of Jowex 50 cont a i n i ng 6 . 87 g of th e a ir dried so clitun f orm of t he re si n wB s rir enar e d a n d t reate d •·, i th solutions of cupric s 2 lts a s foJ. J ows - 16 'L' able VI Sol ution Form of resin ... meq cu+-t- absorbed .5F Cu(Cl0 )2 4 25.6 Na+ .5F Cu(C10 4 ) 2 25.4 Na + .5F CuC1 2 25.4 H As wa s e x necte d t he resin has the s ame c a nacity for CO p )) er in both t he so rJ ium ::rnd hydro g e n forms. Th e same amount of cu ++ V'JaS abs orbe d by t h e resi n from t he Cu(Cl04) 2 soluti o n i n 1ivh ich it is pres u mably un-comnlexed about a nd from the CuCl2 solution in which +-t- 50% of t h e Cu i s nresent as CuCl ~ • Th e strongly ioniz e d sulfonic a ci d groups do not e xert any comnlexing effect on t h e c uc1+ . - 17 Part III Batc h Study of IRC - 50 A titration curve of IHC - 50 resiE wi;:is run by p l a cing .2 g samples of the H+ form of t he resin in test tubes and e quilibr a ting for several days with solutions cont a ining v a rious amounts of NaOH in 1 F Nac10 • 4 The nH of the resultiw)~ on a Beckman Hodel G nH Lileter. on Graph II. solutlons was resd The r e sults are shown The curve is sir11il -, r to t :riose nublished for neutr a lization wit h KOH ( 13) , but dis-0 l :=i ced someWha.t si nce t h e re n ct :Lon is not sim-oly the neutrali z- ation of a n a cid by a base , but r 2ther: HCOOH .f. Na• I·{,.. -t o:r.r = RCOO~a+ ~ H -t = ;'.:CJH 'l'he a bility of the c a ti on t o reD l r' ce H+ in the r e sin is t he i rrrr:i ort a nt f ac t or in ciet errn. i ning the n2_t1 n 'e of the titrat i on curve. 'l'h e titr a ti on curve vv:::s use J to neenare some of t he r bs i n · h i ch vris buffered e t nH = 5 . 2 b :1r eC'ui l i+ br a t in~ t he II forYi\ with t he co c'I'(:': Ct ::n1 onnt of' J.·'aOH in 1 F N2 C10 • 4 rL'es ts -.,:._ erE~ run on til e c oDne r p m 1er of t his buf'fered resin e n d i t found 'V 8 S ++ t=~ bs orbing ti1~1t .1 g of the resin woulj remo ve 90~ of · '~0 1 F Cu f.1"-solution. Jince .1 g of resin ?snrcse nts f the Cu about 1 11rn c1 , the res in vms 5 ': ~ sa t urated . from 50 ml -·-~ ·or the exn - 2 3 4 5 6 7 8 9 10 11 ~ 2 6 8 12 14 16 . 18 20 22 24 ml O.lN NaOH added per 0 . 2 g dry Resin 10 26 28 Base NaOH Vol - 30 ml }La I (NaCL04 ) 30 32 34 pH r--~~- TITRATION OF IRC-50 RESIN I co I-' - 19 eri1ac~nts v1ith CO TJT) :c hO'lj_ cJo s 1:1e ,'les:i_red a system in v:hich the ernount of exclwn7e v·ou l '' no:r.'Iflnlly be about 50!') a n d t he resin i"'On ld be very dilute in Cu++ . this reas o n t hA u~rn not uursued fu r ther . }!,or of THC - 50 in t:·,js c r' nnecti ('l1. 1.y;.:1 s - 20 - Hef'ere nces 1. i.~ cConnell and Dav i dson, J. ii..m . Chem • .3 oc., ( 1950) 2. ~Asgnsen , Acta Ch em . d cand., (1950) 4, 140 3. Schubert, J. Phys . & Co JJ.o id Chem., (1 9 48) _g, 340 Li,. :jchubert & Richter, J. Am . Chem • .-3o c., (1 948) ?O, 4295 5. -:khubert, Russe ll & L·Iyers , J. Biol. Chern.., (l c.; 50) l fi 5, 387 6 . Boyd, Schubert & Adarnson, J. Arn. Chem . 3oc., (l OLi-7) 69, 2818 7. './alton , J. Phys. Chem., (1943) 47, 371 \lc:i lton, ibid 8. Bauman & Eichorn, J. Am. CJ:-iem. Soc . , ( 1 9 4 7) _, 69 2830 9 . Moeller, Ind. Eng. Chem., An a l. Ed ., (1 943) 12., 3Li-6 10 . .l ·0"/,'en' Stoenner, Ar g ersin ~e r, J. P...m. Chem.• Soc ., JJnvid_s on, & _·.ume, F (1c)51) 73, 2838 11. Farri n.o:ton, Ph. D. Thesis, Ca lifornia Institute of ~e chnolo gy , (1 9 50) 12. Ku nin & Ba rry, Incl. Eng . Chen ., (1 9 1+9) Li-1, 12 6 9 13. Kun in, Ana l. Chem . , ( l c 1+9) 21, P.7 14. Swift, " A System of Chemical An 2 lysis", (l C:Li,6 ) Prentice - HR ll, Pew York - 21 1 5 . J i dg-wick , (1 950 ) 1 1 n l he Oxford . Cl1emi_c ::-·J :::l ements s.nd 'l1he ir CorrFiounds" ,