ABSTRACT

Livestock wastewater is mainly treated with activated sludge, but ions such as phosphorus, potassium, ammonium, nitrate and sulfate remain in the effluent. In this study, the effects of residual ions on phosphorus recovery using the magnesium potassium phosphate crystallization method were investigated when magnesium was added to increase the pH. If co-existing ions affect the products, the phosphorus to potassium molar ratio (K/P ratio) of the precipitate will deviate from being equimolar. Artificial wastewater test solutions containing 5.6 - 20.3 mM ammonium, 25.6 mM potassium, 6.5 mM phosphorus, 0 - 7.35 mM nitrate, and 0 - 3.06 mM sulfate were used. First, the optimum operating pH and amount of magnesium added to give a high phosphorus removal rate and recovery rate were determined. The experimental setup was a 10 L aerated and stirred reactor, and a 5 L settling tank. The K/P ratio in precipitate was approximately 1 using the optimum conditions. Continuous 2 h treatment allowed a white precipitate containing about 30 g of needle-like crystals to be obtained. Next, the effects of varying the ammonium, nitrate, and sulfate ion concentrations in the artificial effluent were investigated. Ammonium and sulfate ion concentrations of 8 mM or more and 3 mM or more, respectively, caused the K/P ratio to decrease to about 0.7 and 0.5, respectively. Varying the nitrate concentration did not affect the K/P ratio, even at a nitrate concentration of 7.35 mM.

Keywords:

Magnesium Potassium Phosphate, Ammonium, Sulfate, Nitrate, K/P Ratio, pH, hComponent, Formatting, Style, Styling

1. Introduction

Modern agricultural systems require phosphorus compounds to be applied in fertilizers, but the raw materials required (phosphorus ores) are likely to be exhausted at current rates of use. According to Kuroda et al., The 80% of the phosphorus ore that is extracted is currently used in fertilizers [1] . Consumption is currently increasing at 3% each year. If consumption continues to increase at this rate, consumption in the 2060s will be about five times current consumption. This will result in economically minable phosphorus ore reserves being depleted. A realistic scenario is that 50% of currently minable ore reserves will still be available in the 2060s. Japan relies on imported phosphorus ore [1] . It is therefore desirable for techniques for recovering P from waste to be developed to decrease the risk of ore reserves being depleted and decrease the reliance of Japan on imported phosphate ore. Techniques for recovering phosphorus currently discharged into the environment are required to prevent environmental degradation. Livestock wastewater contains high concentrations of phosphorus, so it is easy to study phosphorus recovery methods using livestock wastewater. A traditional livestock wastewater treatment process is shown in Figure 1. First, solids, such as feces, in the wastewater are separated from the liquid. The liquid is then treated with activated sludge, which decomposes the organic substances and nitrifies the ammonium, turning some into nitrate. Even after these treatments the liquid will contain a high concentration of phosphorus.

The ammonia concentration is high at the start of the biological treatment process, so phosphorus can be recovered as magnesium ammonium phosphate (MAP; MgNH₄PO₄) using coexisting Mg. The crystallization of MAP is caused by a reaction among ${\text{PO}}_4^{3-}$ , ${\text{NH}}_4^{+}$ , and Mg²⁺ in aqueous solution. The reaction is shown in formula (1).

${\text{Mg}}^{\text{2}+}+{\text{NH}}_4^{+}+{\text{PO}}_4^{3-}\to {\text{MgNH}}_{\text{4}}{\text{PO}}_{\text{4}}$ (1)

The MAP precipitation method is used for liquids containing P and ammonium. Mg²⁺ is added to generate MAP in weak alkaline solutions. The MAP method gives a high crystal formation rate, so crystallization occurs without seeding. This MAP method can be used at pH 8.5 to pH 9. The MAP method is of-

ten used for solutions containing relatively high P or ammonium concentrations, such as livestock wastewater and side stream wastewater produced during activated sludge treatments [2] - [7] .

The ammonium concentration will decrease and MAP treatment will be difficult when a long treatment time is used and the nitrification efficiency is high. In this study, we investigated the recovery of phosphorus as magnesium potassium phosphate (MPP) through the reaction shown in formula (2) using a high potassium concentration.

${\text{Mg}}^{\text{2}+}+{\text{K}}^{+}+{\text{PO}}_4^{3-}\to {\text{MgKPO}}_{\text{4}}$ (2)

The MPP crystallization method has been used for wastewater with a high phosphorous concentration (30 mM or more, e.g., in urine) and a high potassium concentration [8] . Wastewater treated using activated sludge contains a low ammonium concentration, so it is difficult to use the MAP method to remove phosphorous from treated water. However, the relatively high K concentrations in wastewater treated using activated sludge can be appropriate for MPP treatment. The MPP treatment method has been used to remove relatively low phosphorus concentrations from wastewater treated using activated sludge in very few studies. The optimum pH for MPP treatment depends on the target phosphorous concentration because hydroxy ions are involved in the solubilities of the products. The optimum pH for treating wastewater containing 30 mM P in synthetic urine to give an equimolar precipitate of P, Mg, and K is pH 8 [8] [9] , and the optimum pH for treating synthetic wastewater containing 7.6 mM P is pH 10 [10] . In the study described here, a P concentration of 6.5 mM was used to approximate the typical concentration in livestock wastewater, and the effects of the pH, Mg dosage, and coexisting substances on the formation of MPP were investigated using an experimental system that consisted of a reactor and a settling tank. The synthetic wastewater was designed to simulate effluent from piggery wastewater treated with activated sludge [11] .

2. Methods

2.1. Apparatus and Standard Experimental Conditions

The experimental setup is shown in Figure 2. The system consisted of a 5 L raw water storage tank, a 10 L reaction tank, and a 5 L sedimentation tank. The synthetic livestock wastewater (containing potassium chloride, sodium dihydrogenphosphate, and ammonium chloride) in the raw water tank was fed into the reaction tank at a flow rate of 7.7 L/h. A dosage Mg/P as phosphate (PO₄-P) molar concentration ratio of 1 was maintained in the reactor tank by feeding a solution containing 50 mM magnesium chloride into the reaction tank at a rate of 1.5 L/h throughout the 2 h treatment process. The mixture was stirred and aerated using an air pump supplying air at a rate of 30 L/h throughout the treatment process. The basic synthetic wastewater contained K, PO₄-P, and ${\text{NH}}_4^{+}$ at concentrations of 25.6 mM, 6.5 mM, and 5.6 mM, respectively, and the pH was 7.5.

2.2. Effects of Varying the pH and Mg Dosage on the Formation of MPP

The pH of the solution in the reactor was varied between pH 8 and pH 12 using a pH controller. The dosage Mg/P ratio was changed from 1 to 2 by changing the rate at which magnesium chloride solution was added.

2.3. Effects of Coexisting Substances

Tests were performed using ammonium concentrations of 8.36 mM, 11.4 mM, and 22.3 mM at the standard conditions. Tests were also performed at nitrate concentrations of 0 mM, 4.02 mM, and 8.04 mM, and at sulfate concentrations of 1.02 mM, 2.04 mM, and 3.06 mM.

2.4. Precipitate

The white precipitate that formed in the reaction tank was moved to the settling tank in the overflowing solution and settled in the cone of the sedimentation tank. After a reaction, the mixture was allowed to stand for a specified time, then the reaction solution in the settling tank was passed through a filter. The white precipitate adhering to the filter paper was dried for 24 h in flowing air at 60˚C. The filtrate was passed through a 0.45 μm membrane filter.

2.5. Analysis

The Magnesium concentrations in the samples were determined using an AA- 6300 atomic absorption spectrometer (Shimadzu, Kyoto, Japan). The potassium and sodium concentrations were measured by flame photometry using the same atomic absorption spectrometer. The phosphate and ammonium concentrations were measured using the molybdenum blue and ascorbic acid method and using the indophenol method, respectively, and a V-530 ultraviolet-visible spectrophotometer (JASCO, Halifax, Canada) [12] . The precipitates were inspected using an ECLIPSE E-600 optical microscope (Nikon, Tokyo, Japan) and a JSM- 6510 A scanning electron microscope (JEOL, Tokyo, Japan). The crystals were analyzed using energy dispersive X-ray spectrometry (EDS) using an EDX-LE instrument (Shimadzu, Kyoto, Japan).

3. Results and Discussion

3.1. Optimum pH

The MPP crystallization method can be used as a post-treatment for effluent treated with activated sludge, so we assessed the effects of the presence of nitrate, ammonium, and sulfate ions on the MPP production process. Table 1 and Figure 3 shows the Effects of pH control in component of precipitate, and Electron microscopy images of crystals produced. These components Mg, P, K of the crystals were almost equimolar at pH 11. Needle-like crystals peculiar to MAP and MPP were found at pH 9 or higher, but at pH 12 the components of the crystals stopped being equimolar because too much sodium hydroxide was present.

Needle-like crystals not seen at pH 8 became visible at pH 9, and the needle length increased and more needle-like crystals were present at higher pH values. The decreases in the P and K concentrations in the liquid increased as the pH increased from pH 8 and reached a maximum at pH 11, but then decreased when the pH was increased to pH 12. Figure 4 shows the decreases in the concentrations of the components of the solution at different pH.

The amount by which the Mg concentration decreased did not decrease between pH 11 and pH 12, and the ammonium concentration remained almost constant.

At pH 11, the decreases in the phosphorous potassium, and magnesium Concentrations in the liquid were almost equimolar. The molar ratios of the precipitates, determined by EDS, were 0.84 and 0.95, and the ammonium and sodium contents were 4% and 8%, respectively. It therefore seems that the contents of the components of the precipitate reflected the decreases in the concentrations of the components of the solution. We will examine this using the removal rate and recovery rate using the equations below [13] .

$\text{Recovery}\text{rate}\text{of}{\text{PO}}_4\text{-P}=\frac{{\text{PO}}_{\text{4}}\text{-P}\text{in}\text{white}\text{precipitate}}{{\text{PO}}_{\text{4}}\text{-P}\text{decrement}}$ (3)

$\text{Recovery}\text{rate}\text{of}{\text{PO}}_4\text{-P}=\frac{{\text{PO}}_{\text{4}}{\text{-P}}_{\text{initial}}-{\text{PO}}_{\text{4}}{\text{-P}}_{\text{equilibrium}}}{{\text{PO}}_{\text{4}}{\text{-P}}_{\text{initial}}}$ (4)

The results are shown in Table 2. The removal rate and recovery rate at pH 10 and pH 11 were 90% or higher. Finer crystals were produced at pH 11 than at pH 10, and this may have caused the recovery rates at pH 10 and pH 11 to be different. However, the difference was slight, so we conducted further tests at pH 11.

3.2. Optimum Dosage Magnesium

The effects of the magnesium dosage on the three components are shown in Table 3. The magnesium content of the precipitate was higher at a dosage Mg/P ratio of 1.3 than at lower ratios because magnesium hydroxide was precipitated. It appeared that the optimum magnesium concentration was the same as the phosphorus concentration.

3.3. Results of Operating the System

Further tests were performed at pH 11 using an Mg/P molar concentration ratio of 1. The results obtained when the water quality was varied are shown in Table 4, and the results of the EDS analyses and the molar ratios found when acid dissolution was performed are shown in Figure 5.

An electron microscopy photograph of the precipitate is shown in Figure 6. Both the numbers of atoms (determined by EDS) and the results of the acid dissolution analyses also indicated that the K/P molar ratios were almost 1 and that some ammonium and sodium were included in the precipitates.

3.4. Effects of Ammonium on the Formation of MPP

In our simple batch tests, ammonium concentrations up to about 5 mM did not affect the formation of MPP, and the K/P molar concentration ratios in the crystals were close to 1 [14] . The effects of varying the initial ammonium concentration on the formation of MPP were examined. The effects of varying the

initial ammonium concentration on the K/P ratio are shown in Figure 7.

Electron microscopy photographs of the crystals produced at initial ammonium concentrations of between 0 mM and 22.4 mM are shown in Figure 8. In our simple batch tests, ammonium concentrations up to about 5 mM did not affect the formation of MPP, but higher concentrations caused the K/P molar concentration ratios of the crystals to be <1. Initial ammonium concentrations of 8.36 mM and 11.4 mM gave crystals with K/P ratios of 0.75 - 0.82, but the differences between the ratios found when the tests were performed at room temperature and 30˚C were small.

An initial ammonium concentration of 22.3 mM gave crystals with a K/P ratio of 0.73, but the ratio was only 0.52 when the test was performed at room temperature. It is therefore possible to decrease the effects of the presence of ammonium even at high ammonium concentrations by aerating and stirring the solution and controlling the temperature of the system. Even though the production of MPP was affected by the higher ammonium concentrations, needle-like crystals were found in the precipitate formed at each ammonium concentration that was tested.

3.5. Effects of Sulfate on the Formation of MPP

The effects of sulfate on the components of the solutions and precipitate and an electron micrograph of the precipitate are shown in Figure 9 and Figure 10. We added nitrate to the wastewater with the compositions shown in Figure 2 to investigate the effect of the presence of nitrate on the system. The tests were performed at nitrate concentrations of 0mM, 4.02mM and 8.06 mM. The decrease in the concentration of nitrate ion in the liquid is almost unchanged at 0.1 mM. The ratio of K to P in the crystal is also almost unchanged at 1: 1, and no difference in shape can be seen in the SEM photograph. From these points, it is considered that nitrate is no effect on MPP production.

The effects of sulfate on the components of the solutions and precipitate and an electron micrograph of the precipitate are shown in Figure 11 and Figure 12. We added sulfate to the wastewater with the compositions shown in Figure 2 to investigate the effect of the presence of sulfate on the system. The tests were performed at sulfate concentrations of 0 mM, 1.02 mM, 2.04 mM, and 3.06 mM. The white precipitate that was produced when the initial ${\text{SO}}_4^{2-}$ concentration in the wastewater was 3.06 mM was analyzed by EDS and was found to contain 36.0% PO₄-P, 18.4% K, and 45.6% Mg. Little evidence of a sulfur component peak was found. Needle-like crystals were found at all of the sulfate ion concentrations that were tested. We therefore concluded that sulfate is not incorporated as a sulfur-containing compound in the crystals but inhibits MPP crystallization. No previous studies of the effects of ${\text{SO}}_4^{2-}$ on MPP crystallization have been described,

but MAP production has been found to be affected by the presence of ${\text{SO}}_4^{2-}$ at a concentration of 1300 mg/L (13.54 mM) [13] . It appears that the production of MPP is affected by the presence of ${\text{SO}}_4^{2-}$ in the same way.

4. Conclusion

The aim of the study was to further improve livestock wastewater treatment and the recycling of phosphorous resources. The MPP crystallization process was applied to model wastewater containing 25.6 mM potassium, 6.5 mM phosphorus, and 5.6 mM ammonium at pH 11 using a Mg dosage equimolar with the P concentration. Crystals containing equimolar K/P ratios were obtained after 2 h of continuous treatment. Small amounts of ammonium and sodium were found in the crystals. Nitrate did not affect the K/P ratio, but ammonia and sulfate did affect the ratio, 1 mM sulfate in particular decreasing the K/P ratio to 0.7.

Acknowledgements

This work was supported by JSPS KAKENHI (grant no. 15K00605).

Cite this paper

Harada, H., Katayama, Y., Afriliana, A., Inoue, M., Teranaka, R. and Mitoma, Y. (2017) Effects of Co-Existing Ions on the Phosphorus Potassium Ratio of the Precipitate Formed in the Potassium Phosphate Crystallization Process. Journal of Environmental Protection, 8, 1424-1434. https://doi.org/10.4236/jep.2017.811086

References