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( M. 6. Hocking' McGill University Montreal, QuebecH3A 2A7 ( I Phenyl Acetate Preparation from Phenol and Acetic Acid Reassessment of a common textbook misconception It is often stated (or implied) by authors of textbooks in organic chemistry t h a t " . . . phenols cannot he esterified directlv" , I1 . .). Discussion of direct esterification is often dismissed in this way (2) and methods using acid derivati\.es are outlined. even in the neriodical literature (31. This paper reportsAthedetermination of the approximate equilibrium concentrations for the phenol and acetic acid system, together with an effective method for the direct preparation of phenyl acetate using a combination of mass action and azeotropic one pass water removal to drive this equilibrium to the right to obtain workable ester yields. Table 1. Approximate Equlllbrlum Phenyl Acetate Concentratlons from Bolllng Mlxtures of Phenol, Acetic Acld, and &lfuric Acid ~~~~ Experimental Equilibration rates and equilibria Three experiments were run, each using 18.8 g phenol (0.20 mol) and 12.0 g glacial acetic acid (0.20 mol) in flasks fitted with reflux condensers. All three were boiled under reflux, one without catalyst, and the second and third with 23 mg and 250 rng of mnc. sulfuric acid, respectively. After 22 hr boiling, the first had no phenyl acetate (<I%). The progression of phenyl acetate content with time for the other two experiments is given in Table 1. Phenyl acetate preparation To a solution of 40 g phenol (0.425 mol) in 300 g glacial acetic acid (5.0 mol) was added 2 ml cone. sulfuricacid. This solutmn was boiled while slowly distilling at atmospheric pressure up an efficient column (100 X 3 cm) fitted with a variable reflux ratio head set at I W l , until the vapor temperature reached 118O and the distillate began to turn apale yellow (about 4 hr). The residue was cooled in an ice/salt mixtureand ice cold 50%aqueoussodium hydroxide wasadded dropwise with stirring until the pH of the aqueous phase reached about 12. The separated organic phase was promptly washed with chilled water and 2% acetic acid, and then dried (MgSOd. Removal of the solvent by distillation afforded 32 g (55%)of phenyl acetate (by NMR), h.p. 193-196' (Table 2). Results Initial experiments with phenol and acetic acid established both that the eauilibrium was reached only relatively slowly and that this c&nprised not more than about 13.5% ester (Table 1). Water removal via acetic acid azeotroping markedly raised this, so that preparations employing this technique and using a four mole excess of acetic acid, achieved 55-60% yields of ester based on phenol (Table 2 ) . With less efficient columns (short Vigreux and the like), equivalent yields were obtained if the molar excess of acetic acid employed was raised to 7-9 mol per mole of phenol. Use of benzene for continuous azeotropic water removal in a modified technique, however, only increased the reaction time fivefold, and the ternary toluene azeotrope was not amenable because it would not efficiently phase separate. Discussion Ester yields obtained by the method described approximate those obtained from aliphatic alcohols by the equilibrium method and lie only about 10%below those attainable with procedures utilizing azeotropic water removal during formation of the aliphatic esters (4). Employment of molecular sieves to dehydrate recycled acetic acid, which has been shown to be effective for dehvdration of aliphatic alcohols ( 5 ) ,did not demonstrate the Bame enhancement here. Anhydrous inorganic salts such as copper sulfate (6) or potassium car- Time hours MoI ?4 phenyl acetate contentd 250 mg HISO, 23 mg H.50, 1.7 4.6 3.0 4.5 11.6 22.0 6.3 11.6 13.5 25.0 27.1' 0.1 0.6 2.6 6.0 - 12.4' - Initially using020 molofeach ol phew1 andaceticacid. Mol %'s reported represent relative integrated 'H nmr methyl singlet areas ~alcuiatedthus: @any1 acetate X 100. phenyl acetate + acetic acid a mir aaqua at= contained 1.9% a-, and 2.4%phydroxyacetopknone. identified by d i n g experiments using expsnded spsctra. Caocenbatbtianawere determined by dividing the respective ketone methyl integral by me total methyl Integral (0-, p- ketones. phenyl acetate,and acetic aca)and multiplying by 100. ~welvegems of acetic acid were aMed a m 22 hrenux p e r i d , and W n exacll~12 g distillsd over dwing the next 3 hr Table 2. Comparison of Phenyl Acetate Yields Uslng Acetic Acid Azeotroplng and Variationsa Reaction time. hr Procedure emolaved Brought to bail and distillation directly Eight hours reflux prior to distilling Benzene azeotroping solvent wilh return of benzene phase Employing 2009 fresh Molecular Sieve 3A in a soxhlet, plus acetic acid return Yield of phenyl acetate 4 12 22-24 55 5 10-12 60 55 a l l experimentsemployed a five to one mot mtio of acetic acid to phenol, and sulfuric acid catalysis (see Experimental). bonate (7) may be effective but are less easily regenerated and hence probably less attractive than the more traditional phenol esterification methods. Acknowledgment Thanks are extended to Professor A. S. Perlin for support and to Dr. A. Granata for nmr spectra. Literature Cited I11 Packer. J., and Vawhn, J.. "A Mudern Approach to Organic Chemirtry,ll Clarendon Press. Oxbrd. 1958, p. 705. i 2 ) Nuller,C.R.,"Chemistryof 0rgaganicCumpaundr.ll W. R.Saunder~Co..London, 1965. p 552. Streilweiser,Jr..A,. Heathcock. C. H.. "lntruductiun toorganic Chemiriry.l. MacMillan Publishing Cu.. lnc.. New Yurk, 1976, p. YO5 Fiepal, L. F,and Fiessr, M.. "Advanced O ~ g a n i c C h e m i s t r ~ Reinheld, ," New Yurk. 1961.Finar. I. L.."Owanic Chemistry Vul. 1: The Fundamental Principles." Longman. Landon, 1967, p. 668. Robem,1. D., and Caseriu. M. C.. "Bade Principles of Organic Chemistry," 2nd Rd., W. A. Benjamin.lnc., 0s" Milln,Ontariu, 1977.p. 1294. (3) Heilrlrin. 6. 152: 1. 87: 11. 151; 111.595:LV.611. (41 Naff,M. %and Nef1.A. S.,d.CHBM. BDUC. 44,68U (19671. (5) Fieser. L. P.. and Ficrer, M.,"Reseonts IorOrsanicSynthosis,"Val. I..luhn Wilsy and &XIS, New Yurk, 1967, p. 705. Stern. R. L.,and B d a n , E. N., C h e m lnd. (London! 825ILY6il. Harrinm, H. R..Hayer. W. M.. Arthur. P.,snd Eisenbraun,E. J..Chrm. Ind. ILundonl 156Hl196H1. (61 Clemmenaen. E., and Heitman, A. H. C.. J. Amrr. Chem. S m 42,519 119091. (7) Thiolepape, E.. HerVhir 66, ,454 l19:181. Kenyon. J., in "Organic Syntheses, Collective Vd. I," John Wiloy and Lms. Now Yerk, 1932.p. 261. 1 Present address: Department of Chemistry,University of Victoria, Victoria, B.C. V8W 2Y2. Volume 57. Number 7,July 1980 / 527