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• W2056325089 abstract "Abstract A monobasic and a dibasic phosphate salt are usually added to water to form a standard phosphate buffer solution. The solution pH depends primarily on the concentration ratio R of the two salts, and secondarily on their concentrations and on the concentrations of the supporting electrolytes such as NaCl or KCl. Various ideal and non-ideal solution thermodynamic models are presented. The ideal solution model predicts that the pH should depend only on R , and underestimates the pH at physiological osmolarities by 0.3–0.5 pH units at both 298 K and 310 K, depending on the phosphate, NaCl, and KCl concentrations. Model predictions using the non-ideal extended Debye–Huckel (D–H) equation agree with the data up to ca. ±0.1 pH units at 298 K and 310 K. The pH predictions for the standard isotonic phosphate buffer saline, containing 2 mM of monobasic and 8 M of dibasic sodium phosphate, 137 mM of NaCl, and 2.7 mM of KCl agree well with the data. When CaCl 2 is added, up to 3 mM, a phosphate salt often precipitates, affecting the free Ca 2+ ion concentration, the phosphate ion concentrations, and the pH. The conditions for the formation at equilibrium of hydroxyapatite (Ca 5 (PO 4 ) 3 (OH)), or dicalcium phosphate dehydrate (CaHPO 4 ·2H 2 O), or tricalcium phosphate (Ca 3 (PO 4 ) 2 ), are predicted. The results are important in determining and predicting electrolyte concentrations for achieving desirable pH values while avoiding precipitation for various biological or biomedical applications." @default.
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• W2056325089 date "2009-04-01" @default.
• W2056325089 modified "2023-10-14" @default.
• W2056325089 title "Effect of phosphate salts concentrations, supporting electrolytes, and calcium phosphate salt precipitation on the pH of phosphate buffer solutions" @default.
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• W2056325089 doi "https://doi.org/10.1016/j.fluid.2009.01.005" @default.
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