title: Removal of phosphate from solution by adsorption and precipitation of calcium phosphate onto monohydrocalcite.
abstract: The sorption behavior and mechanism of phosphate on monohydrocalcite (CaCO(3)·H(2)O: MHC) were examined using batch sorption experiments as a function of phosphate concentrations, ionic strengths, temperatures, and reaction times. The mode of PO(4) sorption is divisible into three processes depending on the phosphate loading. At low phosphate concentrations, phosphate is removed by coprecipitation of phosphate during the transformation of MHC to calcite. The sorption mode at the low-to-moderate phosphate concentrations is most likely an adsorption process because the sorption isotherm at the conditions can be fitted reasonably with the Langmuir equation. The rapid sorption kinetics at the conditions is also consistent with the adsorption reaction. The adsorption of phosphate on MHC depends strongly on ionic strength, but slightly on temperature. The maximum adsorption capacities of MHC obtained from the regression of the experimental data to the Langmuir equation are higher than those reported for stable calcium carbonate (calcite or aragonite) in any conditions. At high phosphate concentrations, the amount of sorption deviates from the Langmuir isotherm, which can fit the low-to-moderate phosphate concentrations. Speciation-saturation analyses of the reacted solutions at the conditions indicated that the solution compositions which deviate from the Langmuir equation are supersaturated with respect to a certain calcium phosphate. The obtained calcium phosphate is most likely amorphous calcium phosphate (Ca(3)(PO(4))(2)·xH(2)O). The formation of the calcium phosphate depends strongly on ionic strength, temperature, and reaction times. The solubility of MHC is higher than calcite and aragonite because of its metastability. Therefore, the higher solubility of MHC facilitates the formation of the calcium phosphates more than with calcite and aragonite.
authors: Division of Earth and Environmental Sciences, Graduate School of Natural Science and Technology, Kanazawa University, Kanazawa, Ishikawa, Japan.
authors: Shintaro
authors: S
authors: Yagi
authors: Keisuke
authors: K
authors: Fukushi
mesh_terms: D000327:Adsorption; D002119:Calcium Carbonate / Q000737:chemistry*; D002130:Calcium Phosphates / Q000302:isolation & purification*; D005618:Fresh Water / Q000737:chemistry*; D007700:Kinetics; D009994:Osmolar Concentration; D012995:Solubility; D012996:Solutions; D013696:Temperature; D013816:Thermodynamics; D014874:Water Pollutants, Chemical / Q000302:isolation & purification*; D018508:Water Purification; D014961:X-Ray Diffraction
chemical_list: D002130:Calcium Phosphates; D012996:Solutions; D014874:Water Pollutants, Chemical; C020243:calcium phosphate; D002119:Calcium Carbonate