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Preparation and Characterization of Lanthanum Carbonate Octahydrate for the Treatment of Hyperphosphatemia
We proposed a new approach to prepare lanthanum carbonate via reactions between lanthanum chloride and NaHCO3. In the reaction, small amount of NaHCO3 solution was firstly added to the acidic lanthanum chloride solution to generate lanthanum carbonate nuclei and then NaHCO3 is added to the lanthanum chloride at a constant speed. This approach makes both precipitation reaction and neutralization reaction take place simultaneously. Consequently, lanthanum carbonate is produced at low pH environment (pH below 4.0) so that the risk of generating lanthanum carbonate hydroxide is reduced. The product of the above reaction is validated by EDTA titration, elemental analysis, and XRD characterization. In addition, we established a FTIR spectroscopic method to identify La(OH)CO3 from La2(CO3)2·8H2O. Lanthanum carbonate exhibits considerable ability to bind phosphate.
Hyperphosphatemia is a complication of end stage renal failure. In healthy adults, the average daily intake of phosphate is around 1000–1500 mg, which is balanced by faecal and urinary outputs . For patients with renal failure, however, the phosphate excretion ability of kidneys is reduced significantly. Consequently, the concentration of phosphate in the blood increases, leading to hyperphosphatemia . Hyperphosphatemia causes secondary hyperparathyroidism, renal osteodystrophy, and other diseases. Moreover, high concentration of phosphate in serum results in the formation of calcium phosphate precipitates. Large amount of calcium phosphate precipitates deposited in blood vessels may lead to fetal cardiovascular and cerebrovascular problems in end stage renal failure patients .
Current treatment of hyperphosphatemia involves dietary phosphate restrictions, dialysis, and taking phosphate binder and vitamin D . Most dietary phosphate is derived from protein, and the phosphate content has an almost linear correlation with protein intake. Dialysis patients have a higher dietary protein requirement than healthy persons . It is difficult to rely on dietary restrictions to achieve control of phosphate. Moreover, dialysis provides inadequate removal of phosphate in serum. Therefore, renal failure patients have to take phosphate binders .
The use of phosphate binder began in the early 1970s  and the earliest phosphate binders are aluminum-based compounds. The drug is highly effective and cheap . However, aluminum may accumulate in bone, brain, heart, and liver, causing aluminum toxicity in long-term use [6, 7]. Later, a calcium-based phosphate binder was developed. However, the efficacy of the calcium-based drug turned out to be lower than that of the aluminum-based compound. Moreover, calcium-based phosphate binder can cause hypercalcaemia and gastrointestinal adverse effects . Therefore, ideal phosphate binders that are safe and highly effective in binding phosphate are needed .
Lanthanum carbonate is an ideal phosphate binder. It prevents the adsorption of dietary phosphate by forming insoluble lanthanum phosphate. It has been reported that lanthanum carbonate binds phosphate optimally at pH 3–5, while retaining binding activity at pH 1–7 [8, 9]. In vitro studies suggest that the efficacy of lanthanum phosphate is comparable to that of aluminium compounds in binding with phosphate . The FDA has approved that lanthanum carbonate can be utilized as a phosphate binder for renal failure patients.
Concerning the preparation of lanthanum carbonate, there are several approaches reported in the literature [10, 11]. However, these methods have unresolved problems. For example, it has been reported that lanthanum carbonate can be prepared by a reaction between Na2CO3 and LaCl3 in aqueous solutions. We notice that lanthanum ion possesses strong ability to bind hydroxide ion when the pH value of the aqueous solution is high. On the other hand, the pH value of an aqueous solution of Na2CO3 is rather high. As a result, the reaction between Na2CO3 and LaCl3 may produce undesirable La(OH)CO3 as a side product with lanthanum carbonate.
Although it has been reported that La(OH)CO3 can bind phosphate , La(OH)CO3 has not been approved by the FDA for the treatment of hyperphosphatemia. It has not been elucidated whether the La(OH)CO3 is safe in medical practice.
In this paper, we proposed a new approach to prepare lanthanum carbonate via reactions between NaHCO3 and LaCl3 in aqueous solution under low pH environment. In addition, the prepared lanthanum carbonate was characterized by using FTIR, XRD, elemental analysis, and titration methods. The ability of the lanthanum carbonate in binding phosphate was validated by spectrometric methods.
Lanthanum oxide (99.999% purity) was purchased from Jiaton technology company.
Hydrochloric acid (37 wt%, AR), sodium bicarbonate (AR), disodium salt of EDTA (AR), acetic acid (AR), and sodium acetate (AR) were purchased from Beijing Chemical Plant.
Zinc oxide (reference materials) was purchased from Beijing Institute of Chemical Reagents.
Elemental analyses (C, H, N) were performed on an Elementar Vario EL elemental analyzer.
X-ray powder diffraction (XRD) data were recorded on a Rigaku D/Max-2000 diffractometer at 40 kV, 100 mA for Cu Kα.
FTIR spectra of La2(CO3)3·8H2O and La(OH)CO3 were collected on a Thermo-Fisher Nicolet iN10 MX FTIR spectrometer equipped with an IR microscope. The spectra were recorded under transmission mode at a resolution of 8 cm−1 and 64 scans were coadded.
Other FTIR spectra were recorded on a Fourier Transform Nicolet 6700 by using KBr pellets method. The spectra were recorded under transmission mode at a resolution of 2 cm−1 and 16 scans were coadded.
Quantitative analysis of phosphate was performed by using spectrophotometry (λ = 700 nm) on a PE Lambda 35 UV-Vis spectrophotometer.
2.3.1. Preparation of Lanthanum Carbonate
Lanthanum chloride was prepared via a reaction between lanthanum oxide and HCl solution. The initial concentration of La3+ was 1 mol/L and the initial pH value of the solution was below zero. NaHCO3 was dissolved in deionized water, and the concentration of NaHCO3 of the obtained solution was 1 mol/L.
Lanthanum carbonate was prepared by adding NaHCO3 solution into an aqueous solution of lanthanum chloride under stirring. Description and discussion on the experimental conditions in detail can be found in Section 3. During the reaction, the pH values of the reactive environment were measured by using a combination electrode. The data were converted into digital signal and collected into a desktop computer via a cluster communication port (Scheme 1).
2.3.2. Preparation of Lanthanum Carbonate Hydroxide
The obtained lanthanum carbonate was suspended in deionized water and the mixture was refluxed for 15 hours. Afterwards, the product was obtained via a filtration process.
2.4. Chemical Analysis of the Samples
The La3+ content of the samples was measured by using EDTA titration. The concentration of the EDTA solution was calibrated by using zinc oxide.
3. Results and Discussion
When the sodium bicarbonate solution is added to the lanthanum chloride solution, the following two reactions cooccur in the system: Reaction (1) is a precipitation reaction between and and the products of the reaction are La2(CO3)3 precipitates and proton. Reaction (2) is a neutralization reaction between and . The precipitation reaction cannot be initiated without lanthanum carbonate nuclei being in the system while the acid-based neutralization reaction takes place as long as and cooccur in the system. If the NaHCO3 solution was slowly added to the lanthanum chloride solution, the precipitation reaction cannot be initiated since no lanthanum carbonate nuclei occur in the system. As a result, only the neutralization reaction takes place in the system. Thus, the pH value of the system increases monotonically as more NaHCO3 solution is added. As a result, lanthanum carbonate is prepared at high-pH environment and the risk of producing lanthanum carbonate hydroxide increases considerably.
Herein, we propose an alternative approach to prepare lanthanum carbonate at lower pH environment. The approach is composed of three steps: preparation of lanthanum carbonate nuclei, preparation of lanthanum carbonate, and (3) termination of the reaction.
In the first step, small amount of NaHCO3 solution was quickly added to the lanthanum chloride solution. The concentration of NaHCO3 in the local regions is high enough so that lanthanum carbonate precipitates are formed. The produced lanthanum carbonate can be used as nuclei center and hence the bottleneck of the lack of lanthanum carbonate nuclei is removed. During the reaction, the variation of pH value is monitored and shown in Figure 1. When aqueous solution of NaHCO3 was quickly added, the pH value jumped around 3. In the meantime, white precipitates of lanthanum carbonate appeared. Since was released from the precipitation reaction between La3+ and , the decrease of pH can be observed in Figure 1. If no more NaHCO3 was added, the produced lanthanum carbonate can be dissolved completely by the acid produced from the reaction. To preserve the lanthanum carbonate nuclei, NaHCO3 solution was introduced into the system by using a ZDJ-400 multifunctional titrimeter so that the injecting rate can be accurately controlled. The speed of injection of NaHCO3 solution was kept at 0.2 mL/s. During this process, more and more lanthanum carbonate precipitates were produced, while the pH value almost remained invariant. The reason for this phenomenon is that NaHCO3 plays a dual role in the system. On the one hand, NaHCO3 reacts with La3+ to produce lanthanum carbonate together with . On the other hand, NaHCO3 acts as a base that can neutralize . Since both precipitation reaction and neutralization reaction cooccur in the system, a dynamic equilibration on the concentration of is established and the pH value remains a constant during the reaction. It should be pointed out that the reaction is carried out at lower pH environment (pH is below 4.0) and the risk of producing La(OH)CO3 is significantly reduced.
When La3+ in the solution is completely consumed by the reaction, the precipitating reaction cannot be performed any more. However, the neutralization reaction can still be carried out. As a result, the pH value of the system jumped to 6 (Figure 1). To confirm that La3+ is used up at this moment, we collected small amount of supernatant from the system and added several drops of NaOH solution (1 mol/L), and no La(OH)3 precipitate was observed, confirming that La3+ is completely consumed. Therefore, the reaction was stopped and the precipitate was collected as sample I.
The sample I was characterized by using XRD and the result is shown in Figure 2. The XRD pattern of the product matches with the La2(CO3)3·8H2O. in ICDD PDF2-2004 database (card number: 25-1400) with a matching degree of 92.0%. This result indicated that the product of the above reaction is La2(CO3)3·8H2O.
The sample I was added to deionized water and the mixture was refluxed for 15 hours. Afterwards, the product was obtained after a filtration process and denoted as sample II. XRD pattern of sample II is shown in Figure 3. The XRD pattern matches with the La(OH)CO3 in ICDD PDF2-2004 database (card number: 26-0815) with a matching degree of 95.7%. Thus, the product is proved to be La(OH)CO3.
Titration and elemental analysis results provide additional experimental evidence to support that the two samples are La2(CO3)3·8H2O and La(OH)CO3, respectively. The contents of lanthanum in the two samples were measured by EDTA titration. The contents of carbon were obtained by elemental analysis. The results of the above analysis are summarized in Table 1. Good agreement is found between the theoretical content and experimental results. From the chemical formula, we find that lanthanum carbonate and lanthanum carbonate hydroxide show significant difference on the molar ratio between carbon and lanthanum (denoted by /). If the prepared sample is La2(CO3)3, the / should be 3/2 = 1.5. If the sample was La(OH)CO3, the / should be 1/1 = 1. The / values for sample I and sample II are 1.52 and 1.08 (Table 1), confirming that the products are lanthanum carbonate and lanthanum carbonate hydroxide, respectively.
Based upon the above result, we used the FTIR spectroscopic method to establish a rapid and reliable approach to identify lanthanum carbonate and lanthanum carbonate hydroxide.
FTIR spectrum of La2(CO3)3·8H2O is given in Figure 4. For comparison, FTIR spectrum of La(OH)CO3 is also shown. Significant difference between the spectrum of La2(CO3)3·8H2O and that of La(OH)CO3 can be clearly observed in the fingerprint region (1000~600 cm−1). La2(CO3)3·8H2O has sharp peaks at 850 cm−1, 747 cm−1, and 679 cm−1, while La(OH)CO3 has absorption peaks at 872 cm−1, 848 cm−1, 778 cm−1, and 707 cm−1. The above dramatically different spectral features make it possible to detect La(OH)CO3 impurity in lanthanum carbonates. Here, different amount of La(OH)CO3 was mixed with La2(CO3)3·8H2O, and FTIR spectra of the mixtures were collected by using KBr pellets method. Characteristic peak of La(OH)CO3 at 872 cm−1 can be observed when 5 wt% of La(OH)CO3 was mixed with La2(CO3)3·8H2O (Figure 5). To improve the sensitivity of the FTIR method, second derivative spectra were utilized. In this case, characteristic peak of La(OH)CO3 at 872 cm−1 can be identified even if only 1 wt% of La(OH)CO3 was mixed with La2(CO3)3·8H2O (Figure 6).
To characterize the ability of lanthanum carbonate to bind phosphate, the following experiment was conducted: 0.2 g KH2PO4 was dissolved in CH3COOH-CH3COONa solution (the concentrations of CH3COOH and CH3COONa are both 1 mol/L) so that 100.0 mL KH2PO4 solution whose pH value is around 4.7 was prepared. 0.5 g La2(CO3)3·8H2O was added to the phosphate solution. Enough stirring was applied on the suspension. During the experiment, phosphate can be adsorbed by lanthanide carbonate so that the concentration of phosphate is decreased with time. To monitor the decay of the concentration of phosphate, small amount of supernatant was collected at different time and the concentration of phosphate in the supernatant was analyzed by using the Mo-Sb antispectrophotometric method. Figure 7 shows the variation of the concentration of phosphate in the solution as a function of time. 50% phosphate is removed from the solution within 30 min and more than 95% phosphate is adsorbed by lanthanum carbonate within 120 min. Considering the fact that food stays in the stomach for 4 hours, lanthanum carbonate is enough to bind most phosphate.
We proposed a new approach to prepare lanthanum carbonate via reactions between lanthanum chloride and NaHCO3. In the reaction, small amount of NaHCO3 solution was quickly added to the acidic lanthanum chloride solution to generate lanthanum carbonate nuclei. As a result, both precipitation reaction and neutralization reaction take place simultaneously. Lanthanum carbonate is produced at low pH environment (pH below 4.0) so that the risk of generating lanthanum carbonate hydroxide is significantly reduced. EDTA titration, elemental analysis, and XRD characterization confirm that La2(CO3)2·8H2O are obtained by using the above method. In addition, we established a method to identify La(OH)CO3 from La2(CO3)2·8H2O. Small amount of La(OH)CO3 can be identified from La(OH)CO3/La2(CO3)2·8H2O mixture even if the content of La(OH)CO3 is only 1 wt%. Lanthanum carbonate exhibits a considerable ability to bind phosphate.
Conflict of Interests
The authors declare that there is no conflict of interests regarding the publication of this paper.
This work is supported by the National Natural Science Foundation of China (51373003).
- F. Albaaj and A. J. Hutchison, “Hyperphosphataemia in renal failure: causes, consequences and current management,” Drugs, vol. 63, no. 6, pp. 577–596, 2003.
- T. Plagemann, A. Prenzler, and T. Mittendorf, “Considerations about the effectiveness and cost effectiveness of therapies in the treatment of hyperphosphataemia,” Health Economics Review, vol. 1, no. 1, pp. 1–9, 2011.
- J. J. Schucker and K. E. Ward, “Hyperphosphatemia and phosphate binders,” American Journal of Health-System Pharmacy, vol. 62, no. 22, pp. 2355–2361, 2005.
- D. D. Freitas, R. L. Donne, and A. J. Hutchison, “Lanthanum carbonate—a first line phosphate binder?” Current Opinion in Nephrology & Hypertension, vol. 13, no. 6, pp. 403–409, 2004.
- J. A. Coladonato, “Control of hyperphosphatemia among patients with ESRD,” Journal of the American Society of Nephrology, vol. 16, no. 11, pp. S107–S114, 2005.
- M. Tonelli, N. Pannu, and B. Manns, “Oral phosphate binders in patients with kidney failure,” New England Journal of Medicine, vol. 362, no. 14, pp. 1212–1324, 2010.
- H. H. Malluche and H. Mawad, “Management of hyperphosphataemia of chronic kidney disease: lessons from the past and future directions,” Nephrology Dialysis Transplantation, vol. 17, no. 7, pp. 1170–1175, 2002.
- S. P. Fricker, “The therapeutic application of lanthanides,” Chemical Society Reviews, vol. 35, no. 6, pp. 524–533, 2006.
- B. A. Murrer and N. A. Powell, “Pharmaceutical composition containing selected lanthanum carbonate hydrates,” Patent US 5968976, 1999.
- B. A. Murrey and N. A. Powell, “Pharmaceutical composition containing selected lanthanum carbonate hydrates,” Patent CN 96193918.4, 1996.
- P. Jeevanandam, Y. Koltypin, O. Palchik, and A. Gedanken, “Synthesis of morphologically controlled lanthanum carbonate particles using ultrasound irradiation,” Journal of Materials Chemistry, vol. 11, no. 3, pp. 869–873, 2001.
- J. C. Ferdinando and D. Gilmour, “Method of treating hyperphosphataemia using lanthanum hydroxyl carbonate,” Patent CN 200580030985.1, 27 7 2005.
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