On-line version ISSN 1816-7950
Print version ISSN 0378-4738
Water SA vol.41 n.2 Pretoria 2015
M VogtsII; DS IkumiI; GA EkamaI, *
IWater Research Group, Dept of Civil Engineering, University of Cape Town, Rondebosch, 7701, South Africa
IIRoyal HaskoningDHV, Pietermaritzburg, South Africa
Biological nutrient removal (BNR) activated sludge (AS) systems produce a waste activated sludge (WAS) that is rich in nitrogen (N) and phosphorus (P). When this sludge is thickened to 3-6% total suspended solids (TSS) and digested (aerobic or anaerobic), a high proportion of N and P are released to the bulk liquid resulting in high concentrations of ammonia/nitrate and orthophosphate up to several hundred mg/ℓ (without denitrification or P precipitation). This research investigates P removal by P precipitation in anoxic-aerobic digestion of P-rich BNR system WAS. The experimental setup for this work was a lab-scale membrane UCT BNR system fed real settled sewage with added acetate, orthophosphate, and cations Mg and K to increase biological excess P removal. This WAS was fed to batch aerobic digesters at various TSS concentrations, and to two 20-day retention time continuous anoxic-aerobic digesters (AnAerDig) with aeration cycles of 3-h air on and 3-h air off, one fed concentrated WAS (20 g TSS/ℓ ) and the other fed diluted WAS (3 g TSS/ℓ). Nitrogen removal has been discussed in the previous paper. This paper focuses on the P removal by P precipitation observed in the batch tests and continuous systems. The rate of polyphosphate release (bGP) during batch aerobic digestion at low TSS without P precipitation was found to be 2.5 times faster than the endogenous respiration rate (bG) of phosphorus accumulating organics (PAO), i.e. bGP= 0.1/d. This rate was then applied to the high-TSS aerobic batch tests and continuous anoxic-aerobic digesters to estimate the P precipitation at various TSS concentrations, with and without additional Mg or Ca dosing. Newberyite (MgHPO4.3H2O) and amorphous tricalcium phosphate (ACP or TCP, Ca3(PO4)2.xH2O) are found to be the most common phosphate precipitates.
Keywords: biological excess phosphorus removal, waste activated sludge, anoxic-aerobic digestion, phosphate release, mineral precipitation.
The release rate of polyphosphate from nitrification-denitrifi-cation biological excess phosphorus removal (NDBEPR) waste activated sludge (WAS) in anaerobic and aerobic digesters has been studied by the Water Research Group at the University of Cape Town for the past 8 years. In anaerobic digestion, the release of polyphosphate was found to be complete within 5 days of digestion (Harding, 2009), due to the availability of acetate under anaerobic conditions, followed by a slower P release as the organics of the biomass (phosphate-accumulating organisms, PAO and ordinary heterotrophic organisms, OHO) is digested. In aerobic digestion, it was previously accepted that the PAO polyphosphate was released at the same rate as the PAO endogenous respiration rate, bG (Mebrahtu and Ekama, 2008; Mebrahtu et al., 2010). In this paper, the rate of polyphosphate release is shown to be 2.5 times faster than bG; it is completely released in about 15 days in aerobic batch digestion.
A high P removal UCT NDBEPR system was operated to provide the P-rich WAS for this study. This WAS was used to start aerobic batch digestion tests at different total suspended solids (TSS) concentrations to observe the N and P release, and the WAS was also fed to 2 continuously-fed (once daily) anoxic-aerobic digesters operated at a steady-state sludge age of 20 d at high (20 g TSS/ℓ) and low (3 g TSS/ℓ) TSS concentrations. Moreover, the anoxic-aerobic digested (effluent) sludge waste was further digested in batch aerobic digesters, to check for further P release and denitrification capabilities.
To determine and quantify which phosphate minerals precipitate, weak acid/base chemistry principles (Loewenthal et al., 1994) were applied to the actual and predicted dewatering liquor (DWL) aqueous phases. Interestingly, struvite was found not to precipitate, most likely due to the complete nitrification of ammonia released in digestion.
To observe the rate of release of polyphosphate from P-rich WAS, a lab-scale UCT system was set up with membranes for solid-liquid separation. This NDBEPR system was operated for enhanced bio-P removal with acetate (200 mg COD/ℓ influent), Mg and K added to its settled sewage feed (see Vogts and Ekama, 2012, for details). A summary of this system's operating conditions is given in Table 1.
The WAS withdrawn from the aerobic reactor of this UCT system (Ekama, 2010) was concentrated (8-10 g TSS/ℓ) due to the membranes (Ramphao et al., 2005) and high in P (0.10-0.14 mg P/mg VSS). The UCT system also effectively removed N, having an effluent (and WAS stream) with low ammonia (1-3 mg NH4-N/ℓ) and nitrate below effluent quality standards (8-15 mg NO3-N/ℓ). The effluent orthophosphate was high (15-25 mg PO4-P/ℓ) due to the P (and Mg and K) dosed to the influent. Consequently, P was not limiting and therefore maximised the P content of the WAS. The P-rich WAS was batch digested at low and high TSS to observe the rate of P release and extent of P precipitation, and also fed to 2 continuously fed (once daily) anoxic-aerobic digesters: one was fed concentrated WAS (2x) at 20 g TSS/ℓ and the other was fed dilute WAS (1/3) at 3 g TSS/ℓ as described in Vogts and Ekama (2012). The plant-wide layout of the UCT system and linked anoxic-aerobic digesters are shown in Fig. 1.
Sewage batches were collected from Mitchell's Plain wastewater treatment plant (Cape Town, South Africa) in 2 000 ℓbatches, macerated and stored in 400-ℓ stainless steel tanks in a 4°C cold room. These sewage batches were numbered sequentially, and fed in turn to the UCT system, each batch lasting a period of about 3 weeks. The results, measured on the influent, reactors and effluent of the UCT system, were averaged over a sewage batch period to give the average performance of the system for that period.
From January 2008 to October 2010, the 2 anoxic-aerobic digesters were operated over 4 time periods, each with different dosing chemicals for P precipitation and 2 different aeration patterns as shown in Table 2. This was to observe the effect of pH on nitrification and P precipitation, the effect of different cations on P precipitation and the build-up of nitrate under fully aerobic conditions at 20-days retention time to monitor the biomass digestion rate via the nitrate increase. Table 3 gives the quantities of additives dosed to the WAS feed of each digester during the 4 time periods. Alkalinity was added to maintain a pH between 7.2 and 7.5. Average results for both digesters over the 4 time periods, as well as the impact of continuous aeration on the low-TSS digester's oxygen uptake rate (OUR) and the impact of added Mg and Ca on the high-TSS digester's orthophosphate and filtered polyphosphate cations were presented in Vogts and Ekama (2012). Full results of the investigation are given in Vogts et al. (2014).
Aqueous-solid phase weak acid base chemistry
Batstone et al. (2012) discuss the importance of ionic interactions (weak acid-base chemistry) in wastewater treatment modelling. These interactions affect the alkalinity and pH of a solution. Weak acid-base chemistry involves the processes of solid-aqueous liquid (and aqueous-gas) interaction, as when at high enough aqueous cation and anion concentration, minerals precipitate to become solid. The cations and anions involved with aerobic digestion are the trivalent phosphate system, divalent carbonate (as carbon dioxide is produced, dissolves and some exits the system by air stripping), ammonia, nitrate and metal cations. This mix of weak and strong acids and bases at different concentrations is evaluated to check if phosphate precipitates with metal cations and ammonia. These processes are well described by Loewenthal et al. (1994) and Harding (2009) for determining ionic products of the different cations and anions that make up various minerals in anaerobic digester dewatering liquor. These same principles are applied to the aqueous phase aerobic and anoxic-aerobic digestion at high and low TSS concentrations.
Loewenthal et al. (1989, 1991) and Harding (2009) developed a method whereby a solution containing many dissolved species can be characterised in its weak acid base systems. This is useful for dosing (e.g. to precipitate a certain amount of phosphate by dosing lime). Here the digester aqueous phase (which becomes dewatering liquor after solid-liquid separation) is characterised to assess what phosphate minerals potentially precipitate.
The weak acid base species involved in aerobic digestion and their dissociation equations and constants (pKs) from Loewenthal et al. (1991) are given below. Trivalent orthophosphate (released from organics and polyphosphate), divalent carbonate from dissolved carbon dioxide and monovalent ammonia dissociate as follows:
Nitrate is a strong acid and so, like the metal cations (K+, Mg2+ and Ca2+), is completely dissociated. Nitrate is only in dissolved form and so can only be measured in soluble form, but the cations can be in solid or dissolved forms and were measured in filtered and unfiltered samples.
The dissociation Eqs (1) to (3) need to be corrected for activity, for example for the phosphate subsystem:
where ( ) denotes activity mol/ℓ and [ ] mass mol/ℓ. The activity is calculated as follows: with reference to the most protonated species: fm for one proton away (monovalent), fd two (divalent) and ft three protons away (trivalent), e.g., PO3-4 has lost 3 protons from its most protonated form, H3PO4. The activities of ions depend on the aqueous ionic strength, or conductivity, which is more accurately measured than TDS (total dissolved solids), viz.
ƒi is the activity coefficient for ionic species i, written as fm, fd and ft for mono-, di- and trivalent ions, respectively
μ is ionic strength = 1.68*10-4*SC where SC is the measured specific conductance (mS/m)
Zi is the charge of the ithspecies, 1 for mono-, 2 for di- and 3 for trivalent
A is a temperature-dependent constant = 1.825*10-6(78.3T)-1.5 with T in Kelvin
pH is directly measured as activity, i.e.,
where (H+) is the measured pH, i.e. pH = -log(H+)
Therefore, for example, the mass concentration of aqueous PO34-can be found from inserting the species' pKs in Eq. (4) into the total phosphate (PT) equation PT = [H3PO4] + [H2PO4] + [HPO2-4] + [PO3-4], rearranging to find [PO3-4], and inserting activities.
To judge the precipitation potential of a possible precipitant, the ionic product (multiplication of the involved ionic species) is found and compared with its solubility product. Of particular interest here is phosphate, whose ions PO43- and HPO2-4can precipitate. The measured orthophosphate (OP, in mg PO4-P/ℓ) is the total orthophosphate species (Ps or Pt mol/ℓ = mg P/ℓ divided by 31), i.e.:
Then from Eqs (4) and (5), the concentration of PO3-4 is found by:
Using Eq. (6) to calculate in terms of pH and pK':
Therefore, with a known PT and pH, the concentration of PO3-4 is found. The concentration of HPO3-4will be similarly derived.
Thus from the measured OP, pH and conductivity (a measure of the TDS related to ionic strength), and the equations in (1) above, the ionic products can be calculated in a given solution. For example, the ionic product of newberyite (MgHPO4) is:
Where pIP = -log IP, and the concentration of dissolved magnesium is measured in the solution (as described in methods) and HPO2-4is calculated in Eq. (7) above, using Eq. (4). This ionic product is then compared to the solubility product from literature (see Table 4) to judge if precipitation is likely to happen or not.
The precipitates considered in this study are struvite (magnesium ammonium phosphate, MAP, MgNH4PO4), amorphous tricalcium phosphate (ACP or TCP, Ca3(PO4)2-xH2O), potassium magnesium phosphate (KMP, MgKPO4), newberyite (MgHPO4), magnesium phosphate (bobierite, Mg3(PO4)2-8H2O), magnesite Mg2(CO3)2 and calcite CaCO3. Struvite (MgNH4PO4) was chosen because it is a common precipitant in anaerobic DWL, as is newberyite and ACP (Musvuto et al., 2000). Bobierite was considered a possibility - however, it is said to be rare. Magnesite and calcite are possibilities at well-maintained pHs and high Mg and Ca concentrations. KMP (potassium magnesium phosphate, MgKPO4) precipitates at high pH and temperature (Wilsenach et al., 2007, Schuiling and Andrade, 1999), but was considered a possibility as ammonia (NH4) that would be used for NH4- struvite (MgNH4PO4) precipitation is nitrified and potassium (K) is available in ever increasing amounts due to polyphosphate release. Table 4 shows the solubility products taken from the literature that were used in this study to find precipitants.
The UCT NDBEPR system produced a WAS rich in P, which is illustrated by its N and P content in Figs 2a and 2b. The P content of the WAS progressively increased during 2010, with a total phosphorus (TP) of about 1 200 mg P/ℓ in a WAS of 6-7 g VSS/l during sewage batches 15 to 21.
The two anoxic-aerobic digesters fed with this WAS have been described in some detail in previous papers. The steady state model for continuous and batch digestion was described in Mebrahtu et al. (2010), with initial results from the high-TSS digester. Vogts and Ekama (2012) described the operation and testing of the NDBEPR system and linked anoxic-aerobic digesters with some results from both the high- and the low-TSS digester. This paper will present further results, with a focus on orthophosphate release and precipitation. It will also present the results of further batch tests - one on NDBEPR WAS that shows the release rate of polyphosphate from NDBEPR WAS and the other on high-TSS digester effluent sludge to observe the continued release of polyphosphate, with precipitation. Further analysis of these results with the 3-phase (aqueous-gas-solid) plant-wide, integrated biological, chemical and physical processes model of Ikumi et al. (2013) will be included in a later publication.
Precipitation of orthophosphate released from NDBEPR WAS was expected in the high-TSS digester, and indeed occurred, as is seen in the plotted calculated ionic products in Fig. 3.
Magnesium phosphate (bobierite, Mg3(PO4)2.8H2O) and newberyite, MgHPO4 are represented in Fig. 3a with a pKsp of 24.36 and 5.8, respectively. Using measured concentrations and pH, the ionic product (pIP) in the high-TSS digester is consistently below the pKsp for bobierite, indicating that precipitation is/must be taking place. For newberyite, the pIP hovers around the pKsp, indicating that precipitation is likely to take place. In Fig. 3b, struvite (MgNH4PO4) is in blue with its pKsp of 12.36, and KMP (MgKPO4) is in red, with its pKsp of 10.62. The top blue line of struvite pIP, calculated from measured concentrations, shows that no precipitation of struvite occurred in the digester (which had complete nitrification-denitrification), although it came close during period 3 (SB 14 to 17) due to the added magnesium and also higher orthophosphate concentrations due to the high TP in the WAS. The bottom blue line of struvite pKsp on predicted concentrations, is well below the pKsp, showing precipitation of struvite (MgNH4PO4) if the ammonia had built up and not been nitrified (an unlikely situation also because the ammonia would lower from predicted concentrations due to precipitation, had it not been nitrified). For the red lines of KMP in Fig. 3b, both remain well above the pKsp of 10.62, showing no precipitation of potassium with orthophosphate. This is likely to be the case, as KMP precipitates at high pHs (about 10, Wilsenach et al.,2007; Taylor et al., 1963).
Another expected precipitant is calcium phosphate [Ca3(PO4)2]. However, calcium phosphate pIP never reaches its solubility product (pKsp), even with OP as high as 400 mg PO4-P/ℓ (SB 13 to 17 and 21), as seen by the orange markers in Fig. 4, well above the horizontal line of the pKsp of 26. But the filtered Ca2+ remains low, reaching a high of 62 mg Ca2+/ℓ in SB 19 even when 515 mg Ca2+/ℓ was added to the WAS feed. This low-filtered Ca shows that Ca must precipitate, after which the magnesium phosphates dominate the stability of the solution with their ionic products.
A further possible precipitant is carbonate, with either magnesium or calcium, and therefore ionic products for magnesite (Mg2(CO3)2) and calcite (CaCO3) were calculated and are shown below in Figs 5a and 5b, respectively. In Fig. 5a, the measured pIP of magnesite is above the pKsp of 7 until sewage batch 13, after which it is lower, indicating precipitation of magnesite. This can be attributed to the rise in H2CO3* alkalinity (an indicator of buffering capacity and carbonate concentration) and filtered Mg, the result of added hydroxide and cations (Mg first, then Ca) respectively, during periods 3 and 4. In Fig. 5b, the pIP of calcite is consistently above the pKsp of 6.45, indicating no precipitation. However, the filtered Ca concentration remained around 10 mg Ca2+/ℓ except when excess Ca was added to precipitate orthophosphate to low concentrations (20-50 mg PO4-P/ℓ, as seen in Vogts and Ekama, 2012).
In the low-TSS digester, fed 3 g TSS/ℓ, mineral precipitation was not expected. However, as implied by Mebrahtu et al. (2008), a third of released orthophosphate will precipitate with available cations. Thus, even at such low TSS concentrations, with WAS of such a high P content, orthophosphate was seen to precipitate. pH was also a factor as precipitates were more likely at higher pHs due to the availability of precipitating orthophosphate anions HPO42-and PO43- at high pH. This is illustrated in Table 5 with measured concentrations and calculated ionic products from 3 time periods: one at low pH, stable pH and increased unfiltered TP.
Table 5 shows that the sludge had a high P content - over 200 mg P/ℓ for a WAS feed of 3 g/ℓ, and increasing throughout the testing period to a high 380 mg P/ℓ. The low-TSS digester had an uncontrolled low pH in steady-state Period 3 that resulted in no precipitation. At controlled pHs, bobierite (Mg3(PO4)2-8H2O) precipitated, and newberyite (MgHPO4) at higher OP and filtered magnesium (150 mg PO4-P/ℓ and 48 mg Mg2+/ℓ respectively, for steady state period 20). Struvite (MgNH4PO4) is not seen to precipitate in this digester, nor magnesite (Mg2(CO3)2) and calcite (CaCO3) at an H2CO3* alkalinity range between 200 and 300 mg CaCO3/ℓ.
Since phosphate precipitation was found in this low-TSS digester, the filtered potassium (K) was used to track P release. As discussed above, K did not precipitate even in the high-TSS digester. Therefore, the measured and predicted filtered potassium are given in Fig. 6a. The filtered potassium is above that predicted by the model based on the P release at the PAO (and OHO) endogenous respiration rate (bG=0.04/d, bH=0.24/d). This indicates that P is released by the PAOs at a rate faster than their 'death rate' at their endogenous respiration rate. Similarly the measured OP in Fig. 6b also is above that predicted. Comparing Fig. 6a with Fig. 6b, a higher % of total K than P has been 'released' (measured as filtered), and therefore the P associated with the higher K release probably precipitated.
With precipitation occurring in even the low-TSS digester, the dilute aerobic batch tests were used to observe the release of polyphosphate without precipitation.
Batch Test 2 (BT2)
In BT2, the WAS from the NDBEPR system was batch digested at 3.0 g TSS/ℓ (the same as that fed to the low-TSS continuous digester) to observe the rate of release of P from polyphosphate - at such a low TSS, it was believed P precipitation would not take place. The P content of the WAS was high, at 0.148 mg P/mgVSS. This batch test was modelled based on the activated sludge model of Ekama et al. (2006), extended for BEPR by Mebrahtu et al. (2007)according to the BEPR model of Wentzel et al. (1990). The model-predicted nitrate and VSS concentrations matched the measured concentrations well (Fig. 7), which confirmed the model PAO and OHO endogenous respiration rates (bG=0.04/d and bH=0.24/d respectively). However, the predicted TSS concentration, which takes into account the changes due to polyphosphate release according to the ISS model of Ekama and Wentzel (2004), is higher and curved (Fig. 7b) compared with the linear trend observed for the measured TSS.
Figure 8 shows the predicted and measured P and Mg, Ca and K cation release. After an initial P uptake on Day 1 (continued aerobic P uptake from the NDBEPR system), the measured P and Mg release appear linear up to Day 14, after which they show a decrease. The predicted P and Mg concentrations are curved, decreasing with time as expected from the exponential behaviour of the model. The observed rate of P release is 16.4 mg PO4-P/(ℓ.d). This observed linear release is confirmed in Fig. 9a which shows a constant daily increment in P concentration between 6 and 10 mg PO4-P/(ℓ.d). Also, while the N release (as NH4+ but nitrified to NO3-) per cumulative oxygen consumed (Fig. 9b) is linear (as expected because the VSS removed, oxygen consumed and N released are proportionally related to the COD/VSS (ƒcv) and N/VSS (ƒn) mass ratios of the OHO and PAO biomass), the P release per cumulative oxygen consumed (Fig. 9b) is curved (parabolic) indicating a non-proportional P release to VSS removal. From Day 14, the measured P and cation concentrations decrease, which, though unlikely, is possibly due to dilution problems in sample analysis. More likely is that the aqueous phase had to become supersaturated to trigger nucleation of mineral seed crystals followed by mineral precipitation to saturation, even at the low initial batch VSS concentration, due to the high P content of this NDBEPR WAS.
The observed linear OP release in Fig. 8b was then used to predict TSS concentration in the batch test. The predicted TSS now fits the measured TSS much better as shown in Fig. 10 compared with that originally predicted by the model (Fig. 7b) when the polyphosphate was released at the PAOs' endogenous respiration rate (bG of 0.04/d).
The observed linear P release after initial P uptake was also applied to model the release of the polyphosphate cations using the observed uptake molar ratio observed in the NDBEPR system of 0.245:0.349:0.028:1 for K:Mg:Ca:P. The predicted and measured results are shown in Fig. 11a. Apart from K, which was not observed to be taken up during Day 1 of the batch test, the predicted and measured concentrations match well, confirming (i) the linear faster P release rate and (ii) that polyphosphate is released with the same cation ratio that it is taken up, in the NDBEPR system. Based on the observed linear P release rate, Fig. 11b shows with time (i) the predicted increase in aqueous P concentration from released polyP (PP rel), (ii) the decrease in stored PAO polyP (PP), (iii) the slow increase in aqueous P from the organically bound P in the OHO and PAO biomass due to endogenous respiration (other rel) and (iv) the polyP content of the PAOs (mg PP/mg PAOVSS, ƒXBGPP). The stored polyphosphate in the PAOs (PP) is depleted within 15 days and the PAO polyP content (ƒXBGPP) decreases parabolically because the stored polyP is decreasing faster than the PAO biomass.
To check for P precipitation, the ionic products (as pIP) were calculated from the day-to-day measured aqueous species that make up the different minerals according to the method of Loewenthal et al. (1989). The results of these calculations for the observed polyP release in the low-TSS BT2 are shown in Table 6.
From Table 6 it can be seen that even at the low TSS concentration of 3 g TSS/ℓ, OP does appear to precipitate, due to the high P content of the WAS. Newberyite (MgHPO4) and bobierite (Mg3(PO4)2.8H2O) are indicated to precipitate from around Day 8 based on measured concentrations and pH. Other points of interest are (i) struvite (MgNH4PO4) did not appear to precipitate, because in aerobic digestion the ammonia released is nitrified leaving little residual ammonia available to precipitate, (ii) potassium magnesium phosphate (KMP, MgKPO4) also did not appear to precipitate - it generally precipitates at higher pHs (Taylor et al., 1963, Wilsenach et al., 2007), and (iii) calcium phosphate (Ca3(PO4)2) did not appear to precipitate due to the low calcium content of the polyP.
Revising the P release model
Because a linear polyP release rate cannot be generalised within the endogenous respiration model framework of steady state and dynamic models, a separate first order (exponential) rate was developed for polyP release from the PAOs (bGP), while keeping the PAO and OHO endogenous respiration rates at their usual bG=0.04/d and bH=0.24/d respectively to model the P release in (anoxic) aerobic digestion of BEPR WAS in general. This approach was applied not only to BT2 but also to the other batch tests at different TSS concentrations, active fraction of PAOs (ƒav,PAO) and PAO P content (ƒXBGP). A bGP rate of 0.10/d was found, which is 2.5 times faster than the endogenous respiration rate of PAOs. The predicted and measured results for BT2 are shown in Fig. 12.
In Fig. 12a, the orthophosphate release is better predicted by the increased first-order rate of bGP=0.10/d, showing precipitation after Day 15 by a lower-than-predicted measured orthophosphate. The outliers on Days 14 and 15 can be attributed to the supersaturation required to trigger nucleation, as discussed with Fig. 8. In Fig. 12b, the potassium is well predicted without continued aerobic P uptake from the UCT system. Magnesium is over predicted initially until Days 14 and 15, after which it precipitates. Filtered calcium remains low and fluctuates.
Batch Test 3 (BT3)
Waste sludge from the high-TSS 20-d continuous anoxic-aerobic digester at 13 g VSS/ℓ was digested for a further 40 d in this aerobic BT3. To model this, the effluent concentrations predicted by the 20 d continuous steady state digester model were used as initial conditions for the 40 d batch test. Some polyP release was expected by this 20 d continuous digester waste sludge because it was fed fresh WAS from the UCT NDBEPR system daily.
The measured polyphosphate release is compared against predicted release in Fig. 13. In Fig. 13a, the digester waste (which contains a small fraction of fresh WAS, being fed daily) has a large amount of remaining stored polyphosphate, which is expected to be released, whereas in Fig. 13b, the predicted polyphosphate release is initially fast and then flattens off to lower 20 d predicted concentrations (732 mg PO4-P/ℓ and 351 mg K+/ℓ compared to 800 mg PO4-P/ℓ and 390 mg K+/ℓ in Fig. 13a). This is because, at rate bGP=0.10/d, more of the polyphosphate will have already been released in the 20-d steady-state high-TSS digester than at release rate bG=0.04/d and therefore not appear to be released in the batch test. However, in Fig. 13, the measured concentrations appear lower than predicted, even for potassium, which remains flat.
In Table 7, newberyite (MgHPO4) and bobierite (Mg3(PO4)2-8H2O) were precipitating already in the high-TSS digester waste and continued to precipitate throughout the 40-d aerobic batch test. Struvite (MgNH4PO4) remains just above the solubility product as a result of the high orthophosphate and magnesium. Calcium phosphate (Ca3(PO4)2) comes close to its Ksp by the end of the 40 days, due to a slight increase in pH and dissolved Ca.
The faster polyphosphate release rate bGP of 0.10/d is also applied to the high-TSS digester waste, the results of which are shown in Fig. 14 below. In Fig. 14a, the increased predicted release between rate bG=0.04/d and rate bGP=0.10/d is seen, with rate bGP consistently about a quarter above rate bG. The observed orthophosphate is consistently below predicted, typically half that predicted at rate bGP=0.10/d, showing the amount of P precipitation in the digester. Again, as in Fig. 4, low OP is observed in Period 4 when calcium was added to the high-TSS digester's WAS feed. In Fig. 14b, the measured filtered K follows that predicted at a polyphosphate release rate of bG=0.04/d until sewage batch 10, after which it follows the faster prediction of rate bGP=0.10/d showing the usefulness of potassium as a non-precipitating released polyphosphate cation.
Thus the high-TSS digester shows a significant amount of orthophosphate precipitation. It did show precipitation with a polyphosphate release rate bG of 0.04/d as was shown in Fig. 3 and Fig. 4. However, filtered potassium showed the faster polyphosphate release rate bGP of 0.10/d.
This 40-d batch test was also checked with weak acid-base chemistry calculations for precipitating minerals, some results of which are shown in Table 7 on the next page.
During this study of aerobic and anoxic-aerobic digestion of NDBEPR WAS, the common phosphate precipitants were newberyite (MgHPO4) and bobierite (Mg3(PO4)2.8H2O); magnesite (Mg2(CO3)2) was also found to precipitate at higher magnesium concentrations, with a pH raised from 7.2 to 7.5. Calcium phosphate (Ca3(PO4)2) was not calculated to precipitate, but it obviously did precipitate as filtered Ca remained low, even when excess Ca was added to the high-TSS digester. Struvite (MgNH4PO4) was not found to precipitate in either of the anoxic-aerobic digesters, nor in the aerobic batch tests, due to complete nitrification and that it generally precipitates above pH 8. Struvite (MgNH4PO4) was not found to precipitate in this study, even if a higher pKspis used, such as that of 13.26 observed by Musvuto et al. (2000). Potassium was not precipitated in place of ammonia in K-struvite (KMP, MgKPO4), confirmed by the fact that K-struvite (KMP) generally precipitates at higher pH values (>8) than those in the reactors of this study.
The release rate of polyphosphate from NDBEPR WAS under aerobic conditions was found to be faster than the PAO endogenous rate bG; in fact the rate was linear. For ease of modelling within the endogenous respiration model framework of steady state and dynamic models, a separate first order (exponential) rate was found for polyphosphate release, bGPof 0.10/d. This faster rate fitted the observed potassium release in dilute aerobic batch test BT 3 and also fitted the steady state high-TSS digester's filtered potassium, confirming not only the polyphosphate release rate, but also the usefulness of potassium as a non-precipitating cation released with polyphosphate.
This research was supported by the Water Research Commission, the National Research Foundation and the University of Cape Town.
The authors would like to acknowledge the publication workshop arranged by the South African Young Water Professionals, which the primary author attended. We would also like to convey our appreciation to the Department of Science and Technology, the Water Institute of Southern Africa and Stellenbosch University for covering the costs of the workshop.
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