The calcium phosphate precipitation in a pellet reactor can be evaluated by two main parameters: the phosphate conversion ratio and the phosphate removal efficiency. The conversion ratio depends mainly on the pH. The pellet reactor efficiency depends not only on pH but also on the hydrodynamical conditions. An efficiency model based on a thermochemical precipitation approach and an orthokinetic aggregation model is presented. In this paper, the results show that optimal conditions for pellet reactor efficiency can be obtained

Azzaro-Pantel, Catherine

Biscans, Béatrice

Cabassud, Michel

Montastruc, Ludovic

English

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  CALCIUM PHOSPHATE PRECIPITATION MODELING                                     IN A PELLET REACTOR     L. Montastruc, C. Azzaro-Pantel, M. Cabassud, B. Biscans  Laboratoire de Génie Chimique- UMR CNRS/INP/UPS 5503 ENSIACET, 118 ,Rte de Narbonne 31400 TOULOUSE, France  The calcium phosphate precipitation in a pellet reactor can be evaluated by two main parameters: the phosphate conversion ratio and the phosphate removal efficiency. The conversion ratio depends mainly on the pH. The pellet reactor efficiency depends not only on pH but also on the hydrodynamical conditions. An efficiency model based on a thermochemical precipitation approach and an orthokinetic aggregation model is presented. In this paper, the results show that optimal conditions for pellet reactor efficiency can be obtained.  1. INTRODUCTION  The need to limit phosphate emission in the environment has diverted the attention in recent years to processes which lead to the recovery of phosphate. The principal legislative tool in Europe for fighting against eutrophication is the EC Urban Waste Water Treatment Directive (271/91/EEC). This action came into force in 1991 and enabled waterbodies to be classified as Sensitive Areas if they display symptoms of eutrophication. The precipitation of phosphate salts is a way of P-recovery in effluents with a low concentration in inorganic phosphorus. In the last years, several works were devoted to calcium phosphate precipitation in the so-called pellet reactor (Seckler, 1994) (Hirasawa I. Toya Y, 1990).  This process is based on the precipitation of calcium phosphate obtained by mixing a phosphate solution with calcium ions and a base. More precisely, it involves a fluidized bed of sand continuously fed with aqueous solutions. Calcium phosphate precipitates upon the surface of sand grains. The phosphate covered grains are removed from the bottom of the bed and replaced intermittently by fresh sand grains. In most studies reported in the literature, the phosphate removal efficiency of a single pass reactor, even at industrial scale, has an order of magnitude of only 50%. The efficiency represents the phosphate removal ratio from the reactor inlet to outlet and the conversion rate is the phosphate ratio from the liquid to the solid phase. Calcium phosphate precipitation involves various parameters: calcium and phosphate ion concentrations, supersaturation, ionic strength, temperature, ion types, pH and also time. In fact, the nature of the calcium phosphate precipitate depends on the supersaturation of the various species. More precisely, the co-crystallization of Amorphous Calcium Phosphate (ACP, Ca3(PO4)2) and DiCalcium Phosphate Dyhydrated (DCPD, CaHPO4) may occur in the range (6.5-7.5) of pH. The purpose of the study presented in this paper is to develop a methodology based on modeling for optimizing the efficiency of the pellet reactor.   2. CHEMICAL EQUILIBRIUM MODEL FOR CALCIUM PHOSPHATE PRECIPITATION  2.1 Assumptions  To model the evolution of phosphate conversion rate as a function of pH with respect to ACP and DCPD precipitation, the mass and electroneutrality conservation balances as well as the supersaturation were taken into account. During this precipitation, the aqueous species considered are, on the one hand, for the phosphoric acid H3PO4, H2PO4-, HPO42-, PO43-, and on the other hand, the Ca2+ ion, and the corresponding calcium salts. The KHPO4- species is not taken into account in the electroneutrality balance due to the small quantity involved resulting the low values of the dissociation onstants. .2 Equations of the model CP precipitationc 2 A : The precipitation reaction equation  (1) d phase include : - a mass balance for calcium :   can be written as follows:  2 34 3 4 23 2 ( )Ca PO Ca PO      The different mass balances in the liqui22 4 4 4[ ] [ ] [ ] [ ] [3( )]Ca CaH PO CaHPO CaPO CaOHCa P X         (2) where X  is the conv2total total ACPACP ersion ratio defined by  Total solACPTotalPP PX          (3) - a mass balance for phosphate : ]  (4) The electroneutrality requirement gives : ]2 33 4 2 4 4 4 2 4[ ] [ ] [ ] [ ] [)ACPH PO H PO HPO PO CaH PO     4 4[ ] [ ] (1totalCaHPO CaPO P X   2 32 4 4 4 42[ ] 2[ ] 3[ ] [ ] [ ] [2 4[ ] 2[ ] [ ] [ ] [ ]H PO HPO PO CaPO Cl OH            CaH PO Ca CaOH H K      (5) The ACP surpersaturation is defined by the parameter :    24232 34[ ] [ ]1 ln5Ca POACPACPCa POKs       3      (6) he supersaturation  is taken equal to zero at equilibrium.  T  DCPD precipitation: The precipitation reaction equati  (7) A mass balance for calcium gives the following equation: ] (8) d the electroneutrality equation quation(5)] are the same as for ACP precipitation. The DCPD supersaturation is defined by equation 9: on can be expressed as: 2 24 4Ca HPO CaHPO       22 4 4 4[ ] [ ] [ ] [ ] [Ca CaH PO CaHPO CaPO CaOH     ( )total total DCPDCa P X The phosphate mass balances [equation (4)] an[e   242 24[ ] [ ]1 ln2Ca HPODCPDDCPDCa HPOKs      2    (9) eviously mentioned, equilibrium is assumed and the supersaturation is taken equal  0. equilibrium constants are given for a temperature of 25°C in molar units) (see table 1): Table 1. Equilibrium constants for the system Ca-PO4-H2O As prto The concentrations of ions and complexes are determined from chemical equilibrium relations (   i iiiBA BKA  Ki A Bi AB  value i i Ki K1 H+ H2PO-4 H3PO4 7.1285*10-3 K2 H+ HPO-4 POH2PO-4 6.2373*10-8 K3 H+ -4 HPO-4 453.942*10-15 + 4 4   + H+ OH- H O 1.004*10-14 K4 Ca2+ H2PO-4 CaH2PO4 3.908*10-2 K5 Ca2+ HPO- CaHPO 1.8239*10-3 K6 Ca2+ PO-4 CaPO4- 347.536*10-9K7 Ca2+ OH- CaOH 5.8884*10-2 Kw 2 Consequently, the system to be solved for ACP precipitation contains 12 non-linear equations (equations [2, 4, 5, 6] and equilibrium equations) with 12 variables and the system for DCPD precipitation involves to the equations [4, 5, 8, 9] with the bye-Huckel model giving the activity coefficient of each species was used in this study: corresponding equilibrium equations. The De210 1DH i DHDHLog A z CB         (10)with 22 A oDHBe NBk T  and CDH is a constant equal to 0,055 mol.L-1.  3. MODEL FOR CALCIUM PHOSPHATE AGGLOMERATION  ri and rj. Kusters (1991) proposed a theory to describe the various eddies sizes (a).   A mathematical model was developed in the case of calcium phosphate precipitation by Seckler et al. (1996) to describe the orthokinetic aggregation of the particles of fines on the sand grains in a fluidized bed. This model is based on a collision frequency Jij between particles of sizes 0.5 31.29 ; 6ij i j i j kEJ r r N N a           (12)  5/12 8/31/ 4ij i j i j k2.36 ; 6 25 kEJ r r N N a        (13)   is the Kolmogodies of a scale “a”, e calculated by using the modified  the grains in a fluidized bed is derived from the particle number balance for the fines: k0.253rov length scale defined as:  /k E         (14) The subscripts i and j refer respectively, to the fines and grains. Edsimilar to the size “r”, of the particles control aggregation process.  The energy dissipation rate E in a fluidized bed can bKozeny-Carman equation for the bed porosity value. The aggregation fines-fines is neglected so that the fines diameter can be considered as constant. The decrease in the fines concentration by aggregation withidN BJdtij         (15) ed as the part nergy dissipation rate. A simple function is proposed here to describe this influence. with the initial condition Ni=Ni,in at t=0. The collision efficiency B is definof the collisions actually resulting in aggregation between two particles. The collision efficiency B includes the process of breakage of fines from grains. The breakage is influenced mainly by the eooEEB B            (16)  obtained by Seckler et al. (1996) are spectively 1.05 10-3, –1.3 and 0.049 W/kg.  used  in posed to be the additional contribution of  the two precipitated spec where Eo is an arbitrary reference value for the energy dissipation rate. Bo and  are characteristics of the precipitating system. They are the only model parameters to be adjusted in order to obtain an agreement between the model outputs and the experimental data. The values Bo , Eore The linear dependence of the aggregation process on the supersaturationequation (15) was proposed by several authors (Nore and Mersmann, 1993). In equation (15), the supersaturation is supies supersaturation. ACP DCPD          (17) with ,ottACP ACP ine         (18) ,ottDCPD DCPD te         (19)         2 ,, ,ACP tDCPD t ACP ta KOH b KOH c KOH      (20)  upeEquation (18) represents the ACP s rsaturation decrease v rsus time (along the fluidized bed height). It was deduced from the previous work of Seckler et al. (1996). teues were 5) 16) thus describe not only the aggregation between fines and grains in fluidized bed, by integrating equat oute: o=6.85s and its value is the same for the two species. Equation (20) takes into account the DCPD decrease due to the ACP decrease. oreover, the a, b, and c values depend on the KOH concentration. These valMdetermined for different KOH concentrations by simulation of ACP precipitation at a given level. These conditions enable to obtain the DCPD value according to the ACP value.  Equation (1  and (but also breakage. The phosphate removal efficiency can be calculated ion (15) from t=0 to t=t  and by assuming that the size of the fines is constant in tim,,1agi inN          (21) 4. RESULTS  i out In figure 1, the predicted conversion obtained with a phosphate concentration equal to 1.6 mmol/L and Ca/P molar ratio equal to 3 was plotted as a function of pH value. N01020304050607080901006,5 7 7,5 8 8,5 9 9,5pHconversion/efficiency (%)predicted conversionefficiency with 200µm sand and flow rate (40L/h)efficiency with 200µm sand and flow rate (60L/h)efficiency with 200µm sand and flow rate (80L/h)efficiency with 500µm sand and flow rate (80L/h)efficiency with 500µm sand and flow rate (120L/h)  Figure 1 Efficiency and the conversion rate as functions pH for different phosphate. streams in the fluidized bed   The efficiency for different flow rate values and for two sand sizes (200 µm and 500 µm) was calculated.. The curve obtained by coupling thermodynamics and kinetics models presents an optimum. Moreover, this result confirms the observations reported by Seckler et al. (1996) : it is more interesting to work in a fluidized bed with small and particles and a weak flow rate. It is important to notice that, if only ACP ered (and not DCPD), the efficiency curve as a function of pH oes not present an optimum. kinetic aggregation model. The curve obtained presents an optimum which is ery interesting for optimizing the pellet reactor efficiency. Moreover, this point  value of about 7. This pH requires no treatment after the pellet cknowledgments  are grateful to ‘the Direction Régionale de la Recherche et de la echnologie’ of Midi-Pyrénées  for its financial support to this study. nce of turbulence of aggregation of small particles in  a fluidized bed, Thesis, ed –2. Process idized-bed process for phosphate removal by calcium hosphate crystallizationACS Symposium Series, Vol.438, pp.355-363 mann, A., 1993, Batch precipitation on barium carbonate. Chem. Eng. ci. Vol. 48, pp.3083-3088. (= 1,602177 10  C) =1,380658 10-23 J.K-1)  mol-1) nt (r*o) 854187 10-12 F.m-1) ant o = solvent density (kg.m-3) sprecipitation is considd 5. CONCLUSIONS  In this paper, the conversion and the efficiency in a pellet fluidized bed precipitation was modeled. This model takes into account, on the one hand, the thermodynamics approach represented by the co-precipitation of ACP (Amorphous Calcium Phosphate) and DCPD (DiCalcium Phosphate Dihydrated) which may occur in the range of pH and, on the other hand, the hydrodynamical conditions in the fluidized bed represented by the orthovcorresponds to a pHreactor.  AThe authorsT References  Kusters, K.A., 1991, The influeagitated vessels, Thesis, Eindhoven University of Technology Seckler, M.M., 1994, Calcium phosphate precipitation inTechnische Universiteit Delft Seckler, M.M. et al., 1996, Phosphate removal in a fluidized boptimization , Water Research, Vol. 30, N°7, pp. 1589-1596 Hirasawa I. Toya Y. 1990,FlupNore, P.H., MersS Nomenclature  -19e = electronic charge kB = Boltzmann constant (NA = Avogrado number (= 6,022136 1023T = temperature (K) zi = charge number of ion solvent dielectric constao = vacuum permitivity (= 8,r  = relative solvent dielectric const = ion activity coefficient solution ionic strength (mol/L) = kinematic viscosity (mP2P/s) 

The influe agitated vessels, Thesis,

Calcium phosphate precipitation modeling in a pellet reactor

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Calcium phosphate precipitation modeling in a pellet reactor

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