Comparison of Oxalate, Citrate and Tartrate Ions Adsorption in the Hydroxyapatite/Aqueous Electrolyte Solution System

The kinetics of adsorption/desorption of oxalate, citrate and tartrate anions was investigated using hydroxyapatite from solutions at the initial concentrations of 0.000001 and 0.001 mol/dm3 anions. The adsorption process from a solution with a concentration of 0.001 mol/dm3 takes place in three stages and is well described by the multiexponential equation of adsorption kinetics. The process of tartrate and citrate ion desorption after increasing the pH to 10 is irreversible, while the oxalate ions undergo significant desorption with the increasing pH. The adsorption of oxalate ions decreases with the increasing pH. This effect is weaker in the adsorption of citrate and tartrate ions. Ion adsorption studies were supplemented with the measurements of zeta potential, FTIR and particle distribution of hydroxyapatite particles.


Introduction
Due to its properties, hydroxyapatite [Ca 10 (OH) 2 (PO 4 ) 6 ] (HAp) can be classified as a biocompatible and bioactive material, but due to its natural microporous structure, it is also well known as a good adsorbent, particularly for immobilization cations. HAp is capable of reversible exchange of hydroxyl ions by anions like F, Cl or I ions [1]. HAp also adsorbs/exchanges some larger ions like carbonate, oxalate, citrate or tartrate. As HAp is a mineral compound of human bones and teeth and, on the other hand, the organic acids naturally occur in our diet, the interactions of both compounds can lead in our organism to, e.g., subsequent processes of adsorption, dissolution, precipitation and aggregation. Solutions that contain oxalate, citrate or tartrate salts can cause dissolution of hydroxyapatite but the mechanism of teeth surface etching by salts containing citrate ions is still not fully understood [2]. Hydroxyapatite, brushite and amorphous calcium phosphate play an important role in the heterogeneous nucleation of calcium oxalate monohydrate and the formation of "kidney stones" accumulated in the kidneys [3,4]. However, studies of the heterogeneous nucleation of calcium oxalate monohydrate were carried out in supersaturated solutions of calcium and oxalate ions to ensure crystal nucleation and growth of calcium oxalate [3].
In this paper, the comparison of the kinetic and static adsorption of oxalate, citrate and tartrate ions on hydroxyapatite was investigated using the 14 C radiolabeled acids from acid solutions of initial concentrations of 0.000001 and 0.001 mol/dm 3 and pH range from 6 to 11. The adsorption measurements were complemented by the spectrometric, potentiometric titration of HAp suspensions and electrophoretic measurements.
Studies of ion adsorption in the hydroxyapatite/aqueous electrolyte system due to the solubility of the hydroxyapatite are confined to the pH range of 6 to 11. The speciation of ionic forms created as a result of oxalic acid dissociation as a function of pH indicates that mainly C 2 O 4 2− ions are present in the pH range 6-11 [5]. The dominant forms of citrate ions below the range of pH 6-6.4 are the hydrogen citrate ions (HCit 2− ) and above the range are the citrate anions (Cit 3− ). However, in the pH range of 6 to 11, tartaric acid occurs in the form of tartrate anions [6].

Kinetics of Oxalate Ion Adsorption at the Hydroxyapatite/0.001 mol/dm 3 NaCl Aqueous Solution Interface
The rate of the ion adsorption in the hydroxyapatite/aqueous solution of electrolytes is described by the same equations as the rate of ion adsorption at the metal oxide/electrolyte.
The pseudo-first order equation depending on adsorption (a): After integration the nonlinear form the above equation is: where: a eq -the equilibrium adsorption density, a-the adsorption density, k 1 -the kinetics coefficient, t-the time.
The pseudo -second order nonlinear equation: a = a 2 eq k 2 t 1 + a eq k 2 t where: a eq -the equilibrium adsorption density, a-the adsorption density, k 2 -the kinetics coefficient, t-the time.
Multiexponential equation where: a-the adsorption density, a eq -the equilibrium adsorption, A 0 -the relative equilibrium concentration, A i -describes the part of the i-th process characterized by the coefficient k i . However, due to the specific structure of hydroxyapatite crystal (presence of natural channels) [1] and the solubility of hydroxyapatite, the long-term study of adsorption reveals that slow adsorption proceeds after the fast adsorption stage [7]. If the kinetics of ion adsorption from solutions with an initial concentration of 0.000001 mol/dm 3 for 3 h was investigated, the pseudo-first or pseudo-second-order equations would fit the experimental data [8,9].
The kinetics of the oxalate ion adsorption of the initial concentrations 0.000001 and 0.001 mol/dm 3 at the hydroxyapatite/0.001 mol/dm 3 NaCl solution is depicted in Figures 1 and 2, respectively. As it can be seen from Figure 1, the adsorption of oxalate, citrate and tartrate ions after the 5 min hydroxyapatite contact with the electrolyte solution, as well as the pH of the suspension, are stable. The fitting adsorption data of oxalic and citric ions the using pseudo-first-order and the pseudo-second-order equations show that the latter gives almost the best fit [10]. However, the kinetics of the tartrate ion adsorption on hydroxyapatite from a solution with an initial concentration of 0.000001 mol/dm 3 is best fitted by the multiexponential equation [11]. As can be seen from Figure 1, the adsorption affinity of the anions of the tested acids for the hydroxyapatite surface is the highest for the oxalic anion (~95% of the oxalate ions are adsorbed), lower for the tartrate anion (~86% of the tartrate ions are adsorbed) and the lowest for the citrate (~50% of the citrate ions are adsorbed). The adsorption affinity of carboxylic acid ions for the hydroxyapatite surface can be compared with the solubility of calcium salts of the above mentioned acids: the less soluble salt is calcium oxalate (pK so (CaOX = 8.63) [12] the more soluble salt is calcium tartrate (pK so (CaTart = 6.11) [13] and the preferred is calcium citrate (pK so (Ca 3 Cit 2 ) = 13.15) [14].
Colloids Interfaces 2020, 4, x FOR PEER REVIEW 3 of 12 adsorption proceeds after the fast adsorption stage [7]. If the kinetics of ion adsorption from solutions with an initial concentration of 0.000001 mol/dm 3 for 3 h was investigated, the pseudo-first or pseudo-second-order equations would fit the experimental data [8,9]. The kinetics of the oxalate ion adsorption of the initial concentrations 0.000001 and 0.001 mol/dm 3 at the hydroxyapatite/0.001 mol/dm 3 NaCl solution is depicted in Figures 1 and 2, respectively. As it can be seen from Figure 1, the adsorption of oxalate, citrate and tartrate ions after the 5 min hydroxyapatite contact with the electrolyte solution, as well as the pH of the suspension, are stable. The fitting adsorption data of oxalic and citric ions the using pseudo-first-order and the pseudo-second-order equations show that the latter gives almost the best fit [10]. However, the kinetics of the tartrate ion adsorption on hydroxyapatite from a solution with an initial concentration of 0.000001 mol/dm 3 is best fitted by the multiexponential equation [11]. As can be seen from Figure  1, the adsorption affinity of the anions of the tested acids for the hydroxyapatite surface is the highest for the oxalic anion (~95% of the oxalate ions are adsorbed), lower for the tartrate anion (~86% of the tartrate ions are adsorbed) and the lowest for the citrate (~50% of the citrate ions are adsorbed). The adsorption affinity of carboxylic acid ions for the hydroxyapatite surface can be compared with the solubility of calcium salts of the above mentioned acids: the less soluble salt is calcium oxalate (pKso(CaOX = 8.63) [12] the more soluble salt is calcium tartrate (pKso(CaTart = 6.11) [13] and the preferred is calcium citrate (pKso(Ca3Cit2) = 13.15) [14].
After 120 min, the pH of the suspension was changed to 10 and the kinetics of desorption of carboxylic acid anions was studied (lower right part of Figure 1). As can be seen, the change in pH caused significant desorption of oxalate ions (23% of the ions remained on the surface), while in the case of citrate ions, this was around 43%, and for tartrate ions, around 53%. However, after a long period of conditioning (1440 min), as a result of the reaction in suspension in the presence of oxalate ions, the pH dropped to the value of 8.3, which resulted in an increase in the adsorption of oxalate ions to 71%. In the case of the tartrate and citrate ions, the decrease in pH after this conditioning period was not large and thus the increase in adsorption was of the order of 1%.  Kinetics of pH changes of suspension and carboxylic ion adsorption/desorption changes on hydroxyapatite from the carboxylic ion solution of the initial concentration 0.000001 mol/dm 3 . Grey points denote the oxalic, green points denote citric, and ruby points denote tartrate ions. The black, green, and wine colored lines represent a fit with a pseudo-second-order kinetic equation for the adsorption kinetics of oxalate and citrate anions and multiexponential equation for tartrate anions, respectively. The parameters of adsorption fitting line are presented in Tables 1 and 2. Table 1. Parameters of the pseudo-first-order and the pseudo-second-order equations fitted to the data of adsorption kinetics of oxalate, citrate and tartrate ions from the solutions of the initial concentration 0.000001 mol/dm 3 on the hydroxyapatite.

Ion
Concentration mol/dm 3    Table 3.  The experimental data points: grey-oxalic ions, green-citric ions and wine color-tartaric ions. The black, green and wine colored lines represent multiexponential equation fitting the data of adsorption kinetics of oxalate, citrate and tartrate ions. The parameters of adsorption fitting line are presented in Table 3. After 120 min, the pH of the suspension was changed to 10 and the kinetics of desorption of carboxylic acid anions was studied (lower right part of Figure 1). As can be seen, the change in pH caused significant desorption of oxalate ions (23% of the ions remained on the surface), while in the case of citrate ions, this was around 43%, and for tartrate ions, around 53%. However, after a long period of conditioning (1440 min), as a result of the reaction in suspension in the presence of oxalate ions, the pH dropped to the value of 8.3, which resulted in an increase in the adsorption of oxalate ions to 71%. In the case of the tartrate and citrate ions, the decrease in pH after this conditioning period was not large and thus the increase in adsorption was of the order of 1%.

Pseudo-First-Order Pseudo-Second-Order
For the initial concentration of oxalate, tartrate and citrate ions of 0.001 mol/dm 3 , in the course of kinetics, three stages can be distinguished. The first stage in the first 5 min shows a rapid increase in adsorption (62% oxalate, 52% tartrate and 35% citrate). In the second stage, the pH increase and the anion adsorption increase by several percent are observed within 200 min. In the third stage, up to 10,080 min, there is a greater increase in the anion adsorption again, to the value of 95% oxalate ions, 83% tartrate ions and 74% citrate ions. The experimental adsorption data depicted in Figure 2 are well fitted using also the multiexponential model. Such three-stage adsorption may be the result of a dissolution-precipitation mechanism [7] adsorption at the interface or intraparticle diffusion [15]. Taking into account the anisotropic ion radiation of Van der Waals of tartrate ions (a x = 0.3 nm, a y = 0.28, a z = 2.41 nm) and citrate ions (a x = 0.33 nm, a y = 0.29, a z = 2.81nm) [16], it can be assumed that only in the case of type II channels (0.3-0.45 nm diameter) [17] is diffusion of these ions and subsequent ion exchange possible.
To describe the mechanism of slow uptake of carboxylic acid ions, particle size analysis of hydroxyapatite in the presence and absence of carboxylic acid ions was conducted.
After 10,080 min, the pH of the suspension was changed to 10 and the kinetics of desorption of carboxylic acid anions was observed (lower right part of Figure 2). Increasing the pH of the suspension causes the absorption of oxalate anions to decrease from 59% to 27%. As time passes, the pH of the suspension decreases due to the dissolution reaction and the amount of adsorbed oxalate anions decreases by~2%. After 3000 min, the pH drops further and the adsorption of oxalate ions increases to 41%. The course of adsorption of tartrate ions after changing the pH of the suspension from 7.2 to 9.9 is similar to that of oxalate ions. However, the decrease in adsorption is smaller than for oxalate ions (adsorption reduces from 83.5% to 64%). After 2880 min, the adsorption increases to 86.6%, and after 10,080 min, the adsorption value is 91%. However, in the case of citrate ions, increasing the pH does not reduce adsorption. This is probably due to the fact that the pH of the suspension drops to 8.1 after 10 min.

Study of the Carboxylic Acid Ion Adsorption at the HAp/Aqueous Electrolyte Interface as a Function of pH
The uptake of ions from the solution due to the interactions of ions with the hydroxyapatite surface may result in the adsorption of ions on the active sites of the hydroxyapatite surface (Ca 2+ , −OH, =HPO 4 ), due to the exchange of ions from the solution with those of the hydroxyapatite crystal lattice and/or the processes of hydroxyapatite dissolution and recrystallization of the new phase [18]. The above-mentioned mechanisms, depending on the pH and ion concentration, may sometimes occur simultaneously. The dissolution and recrystallization mechanisms usually take place at high concentrations of these ions in solution.
The adsorption of oxalate, citrate and tartrate ions from the solution of the initial concentrations 0.000001 mol/dm 3 and 0.001 mol/dm 3 as a function of pH on hydroxyapatite is depicted in Figures 3 and 4, respectively. As it can be seen, the adsorption of oxalate ions from the solution of the initial concentration 0.000001 mol/dm 3 , shown in Figure 3, decreases with the increase in pH of the solution, from 95% at pH = 6.8 to 16.5% at pH = 10. This graph is similar to the one depicting the adsorption of ions at the metal oxide/electrolyte solution interface that proceeds via exchange with surface of the hydroxyl ions. The tartrate ion adsorption also decreases with the increasing pH, but to a much smaller extent, from 74% at pH = 7.2 to 48% at pH = 10.7. On the other hand, the adsorption Colloids Interfaces 2020, 4, 45 6 of 12 of citrate ions is the lowest in the tested pH range and it decreases from 33% at pH = 7 to 15% at pH = 9.85. The presented relations show that the adsorption of oxalate anions in the range of pH 6-8.3 is characterized by the highest adsorption affinity for the hydroxyapatite surface, but above this pH range, the tartrate ion is more strongly adsorbed. On the other hand, in the whole pH range, the citrate ion is the most weakly adsorbed. The presented relationships of adsorption of oxalic and citric acid anions as a function of pH are in good agreement with the studies by Wei et al. [19].
Colloids Interfaces 2020, 4, x FOR PEER REVIEW 6 of 12 in the tested pH range changes less, from 53% at pH = 6.34 to 33% at pH = 10.9. The adsorption of citrate ions also decreases as the pH increases, i.e., 29% at pH = 5.75 to 7.4% at pH 10.67. Comparing the surface concentration of different adsorption sites on the hydroxyapatite surface, i.e., NCa = 7.5 μmol/m 2 , NPO4 = 5.0 μmol/m 2 [20] and NOH = 2.5 μmol/m 2 [21], with the adsorption of the tested carboxylic acid anions, it can be seen that the adsorption of these anions was much lower than the formal monolayer of each of the above-mentioned in adsorption sites. Such adsorption is dependent on carboxylic acid ions vs. pH results from the exchange of phosphate ions from the hydroxyapatite crystal.   in the tested pH range changes less, from 53% at pH = 6.34 to 33% at pH = 10.9. The adsorption of citrate ions also decreases as the pH increases, i.e., 29% at pH = 5.75 to 7.4% at pH 10.67. Comparing the surface concentration of different adsorption sites on the hydroxyapatite surface, i.e., NCa = 7.5 μmol/m 2 , NPO4 = 5.0 μmol/m 2 [20] and NOH = 2.5 μmol/m 2 [21], with the adsorption of the tested carboxylic acid anions, it can be seen that the adsorption of these anions was much lower than the formal monolayer of each of the above-mentioned in adsorption sites. Such adsorption is dependent on carboxylic acid ions vs. pH results from the exchange of phosphate ions from the hydroxyapatite crystal.   The comparison of the adsorption of oxalate, citrate and tartrate ions from the solution of the initial concentration of 0.001 mol/dm 3 as a function of pH in the hydroxyapatite/0.001 mol/dm 3 aqueous NaCl solution is presented in Figure 4. The oxalate ion adsorption decreases significantly with the pH increase, i.e., 61% at pH = 7.2 to 9.6 at pH = 10.6, whereas the adsorption of tartrate ions in the tested pH range changes less, from 53% at pH = 6.34 to 33% at pH = 10.9. The adsorption of citrate ions also decreases as the pH increases, i.e., 29% at pH = 5.75 to 7.4% at pH 10.67. Comparing the surface concentration of different adsorption sites on the hydroxyapatite surface, i.e., N Ca = 7.5 µmol/m 2 , N PO4 = 5.0 µmol/m 2 [20] and N OH = 2.5 µmol/m 2 [21], with the adsorption of the tested carboxylic acid anions, it can be seen that the adsorption of these anions was much lower than the formal monolayer of each of the above-mentioned in adsorption sites. Such adsorption is dependent on carboxylic acid ions vs. pH results from the exchange of phosphate ions from the hydroxyapatite crystal.
The effect of the adsorption of carboxylic acid ions onto hydroxyapatite on the zeta potential is depicted in Figure 5. As follows, the presence of carboxylic acid ions at the concentration 0.001 mol/dm 3 results in a decrease in the zeta potential in the pH range of 5 to 9. The most significant effect is observed for the pH range of 6 to 7, where the adsorption of carboxylic acid ions on the hydroxyapatite is the highest. The effect of zeta potential decrease by carboxylic acid ion adsorption is caused by the decrease in the substitution of the phosphate group on the hydroxyapatite surface by the carboxylic acid ions that exhibit more acidic properties than those of phosphate.
Colloids Interfaces 2020, 4, x FOR PEER REVIEW 7 of 12 The effect of the adsorption of carboxylic acid ions onto hydroxyapatite on the zeta potential is depicted in Figure 5. As follows, the presence of carboxylic acid ions at the concentration 0.001 mol/dm 3 results in a decrease in the zeta potential in the pH range of 5 to 9. The most significant effect is observed for the pH range of 6 to 7, where the adsorption of carboxylic acid ions on the hydroxyapatite is the highest. The effect of zeta potential decrease by carboxylic acid ion adsorption is caused by the decrease in the substitution of the phosphate group on the hydroxyapatite surface by the carboxylic acid ions that exhibit more acidic properties than those of phosphate.    Figure 6 presents the FTIR transmission spectra of the hydroxyapatite sample and the samples of hydroxyapatite conditioned in 0.001 mol/dm 3 oxalic, citric or tartaric acid solutions. The analysis of the characteristic bands of the hydroxyapatite sample (HAp spectrum) indicates the presence of the OH group (characteristic bands at the wavenumber 3572 and 631 cm −1 that can be assigned to the stretching mode ν s and the vibration mode ν L , respectively, and at 1630 cm −1 to the bending mode of water molecule [22]; phosphate groups bands at the wavenumber 1093, 1033, 962 cm −1 assigned to the vibrations of these groups). Moreover, the presence of the bands characteristic of the carbonate groups at the wavenumbers of 1419 and 1453 cm −1 can be seen. Their presence may be related to the chemisorption of carbon dioxide on hydroxyapatite during synthesis, storage and experiments [23,24]. The FTIR spectrum of the samples conditioned in the 0.001 mol/dm 3 carboxylic acid solutions is richer, but a number of bands overlap with the characteristic HAp bands to show the presence of acid anions from the FTIR HAp spectrum. The FTIR spectra of hydroxyapatite samples conditioned in acid solutions were subtracted and the spectra subtracted for these samples are shown in Figure 7. As can be seen in the spectrum, there are a number of bands characteristic of calcium oxalate, citrate or tartrate [25][26][27][28][29][30]. The wavenumbers corresponding to the individual bands and the bands assigned to them, on the basis of the spectra for salts or calcium complexes, are presented in Table 3. The FTIR spectra presented in Figure 7 and the data in Table 4 indicate the chemisorption of oxalate, citrate and tartrate anions on the hydroxyapatite surface.  The FTIR spectrum of the samples conditioned in the 0.001 mol/dm 3 carboxylic acid solutions is richer, but a number of bands overlap with the characteristic HAp bands to show the presence of acid anions from the FTIR HAp spectrum. The FTIR spectra of hydroxyapatite samples conditioned in acid solutions were subtracted and the spectra subtracted for these samples are shown in Figure 7. As can be seen in the spectrum, there are a number of bands characteristic of calcium oxalate, citrate or tartrate [25][26][27][28][29][30]. The wavenumbers corresponding to the individual bands and the bands assigned to them, on the basis of the spectra for salts or calcium complexes, are presented in Table 3. The FTIR spectra presented in Figure 7 and the data in Table 4 indicate the chemisorption of oxalate, citrate and tartrate anions on the hydroxyapatite surface.  [28] ν s -the symmetric stretching, ν a -the asymmetric stretching, ν-the stretching, π-the wagging, δ-the bending.
Colloids Interfaces 2020, 4, 45 9 of 12 in acid solutions were subtracted and the spectra subtracted for these samples are shown in Figure 7.
As can be seen in the spectrum, there are a number of bands characteristic of calcium oxalate, citrate or tartrate [25][26][27][28][29][30]. The wavenumbers corresponding to the individual bands and the bands assigned to them, on the basis of the spectra for salts or calcium complexes, are presented in Table 3. The FTIR spectra presented in Figure 7 and the data in Table 4 indicate the chemisorption of oxalate, citrate and tartrate anions on the hydroxyapatite surface. Figure 7. Comparison of the subtracted FTIR spectra of tartrate, citrate and oxalate ions adsorbed on hydroxyapatite. Figure 7. Comparison of the subtracted FTIR spectra of tartrate, citrate and oxalate ions adsorbed on hydroxyapatite. Figures 8 and 9 show the volume particle distributions of the conditioned hydroxyapatite samples in solutions of the 0.001 mol/dm 3 NaCl + 0.001 mol/dm 3 of the tested carboxylic acids. For comparison, Figure 8 shows the particle size distribution of the conditioned hydroxyapatite sample in the 0.001 mol/dm 3 NaCl solution (black triangles). As can be seen, the distribution of hydroxyapatite particles in the case of its conditioning in the solution of 0.001 mol/dm 3 NaCl solution and in a solution of the 0.001 mol/dm 3 NaCl containing tartrate ions with an initial concentration of 0.001 mol/dm 3 is similar, and it has a dimodal character. Most of the particles (~95%) have diameters ranging from 0.4 to 7 µm, while the other smaller fractions range from 7 to 20 µm. In the case of hydroxyapatite conditioning in the solution containing oxalate and citric ions, after 14 days of conditioning, the decomposition is trimodal; the first fraction is in the range of 0.5 to 7 µm (~94% of particles), the second 7-20 µm (~4% of particles) and the third from 20 to 200 µm (~2% particles). The particle size distribution of hydroxyapatite conditioned for 14 days in conditioning the solution of 0.001 mol/dm 3 of citric acid is also trimodal: the first fraction ranges from 0.5 to 7 µm (~91% of particles), the second one 7-20 µm (~3% of particles) and the third from 20 to 200 µm (~6% particles). The presented HAp particle distributions in the acid solutions do not indicate the formation of a separate bulk phase (calcium carboxylates).
On the other hand, the presence of large particles may indicate the phenomenon of aggregation of smaller particles in the case of conditioning in the solution of oxalic and citric acids Figure 9; however, the errors characterizing the share of a given fraction indicate the instability of these aggregates (they are broken down and aggregated under the flow and ultrasound conditions). Measurements of the particle size distribution of hydroxyapatite in the carboxylic acid solutions do not exclude the process of surface precipitation, as a result of which, statistically, a layer with a thickness of several hundred of nanometers could be formed on the surface of the tested hydroxyapatite sample, but it is below the measurement capabilities of this method.

Conclusions
The mechanism of di-and tricarboxylic acid adsorption from the aqueous solutions on the hydroxyapatite is complicated due to the variety of reactions taking place in the system as a function of pH and interaction time. The reaction kinetics of oxalate and citrate ions from a dilute solution with the post concentration of 0.00001 mol/dm 3 is well matched with the pseudo-first-order equation. On the other hand, the kinetics of oxalate, citrate and tartrate ion reactions from the solutions with the initial concentration of 0.001 mol/dm 3 is more complex. There are three stages of adsorption at the time, and such a process is well-adjusted by the multiexponential equation.
The kinetics of desorption of carboxylic acid anions is rapid due to the pH increasing to 10. An increase in pH causes significant desorption of oxalate ions, while citrate and tartrate anions are slightly desorbed. This may indicate that the oxalate ions replace the hydroxyl groups in hydroxyapatite, while the tartrate and citrate ions are phosphate groups.
The dependence of the adsorption of carboxylic acid anions on the pH of hydroxyapatite is strong for the oxalate anions and weaker for the tartrate and citrate anions. On the other hand, below pH = 8.3, at the initial concentration of 0.000001 mol/dm 3 , the oxalate anion shows the highest adsorption affinity for hydroxyapatite and citrate the weakest. Above pH 8.3, the tartrate anion adsorbs most strongly. From the solution of the initial concentration of 0.001 mol/dm 3 , below pH = 7.5, the oxalate ions exhibit the highest adsorption affinity, but above the tartrate ions.
The studies of the effect of adsorption of carboxylic acid anions on the dependence of the zeta potential of hydroxyapatite as a function of pH indicate that the adsorption of the above-mentioned anions increases the acidic nature of the hydroxyapatite surface.
The FTIR spectra of hydroxyapatite samples with the adsorbed ions of oxalic, citrate and tartaric acids showed the presence of characteristic bands for the calcium salts of these acids and indicate the chemisorption of these anions.