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The Free Energy of Formation of Datolite

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The Free Energy of Formation of Datolite American Mineralogist, Volume 80, pages 576-584, 1995 The free energy of formation of datolite WEN YANG, * PHILIP E. ROSENBERG Department of Geology, Washington State University, Pullman, Washington 99164-2812, U.S.A. ABSTRACT The solubility of datolite, CaBSi04(OH), has been determined experimentally at tem- peratures from 100 to 250°C and Pv = PH20,Activity products (Q) were calculated for the dissolution reaction after 8-10 time intervals in experiments of up to four months' du- ration in order to determine Koo..A linear relationship between log Koo.and reciprocal temperature [log Keq = 4.405 + 637.01T (K); R = 0.97] suggests the attainment of equi- librium. The IlG? extrapolated to 25°C, -2318 :t 2 kl/mol, is the same as a calculated calorimetric value (Semenov et aI., 1988) and close to the value of - 2317 kl/mol esti- mated with the use of the polyhedral model of Chermak and Rimstidt (1989). However, at elevated temperatures f1G? values determined from solubility data diverge from the other two estimations, suggesting that the latter may be more accurate. The IlG? values calculated from the data of Semenov et ai. (1988) have been used to d~termine the temperature dependence of datolite-danburite stability relations and activity diagrams for the system CaO-B203-Si02-H20 at 250°C in an effort to place limits on solution compositions in equilibrium with mineral assemblages in the quaternary system. Higher activities of H3B03.aq and Si02.aq and lower pH are required for the formation of danburite than for datolite, whereas high a Ca2+favors the crystallization of datolite. INTRODUCI'ION When these data are available, the calculation of the sta- Although calcium borosilicates are not rare minerals bility relationships of the calcium borosilicates in solu- few mineralogical, field, or laboratory studies have sough~ tions of varying composition will be possible over a wide to account for their genesis. Thus, qualitative statements temperature range. A knowledge of these phase relations concerning the chemistry of fluids responsible for the would be of interest in studies ofwater/rock interactions crystallization of datolite or danburite are the rule (e.g. in B-bearing systems. Eugster and Wise, 1963). For example, the higher CaOI The stability relations of danburite and datolite were B203 ratio in datolite than danburite must reflect the determined experimentally by Eugster and Wise (1963) compositions of the fluids that coexisted with these min- and more recently by Kurshakova (1982), but thermo- erals, but what are these compositions and how do they dynamic data was not retrieved. The enthalpy of forma- vary with temperature and pressure? While some exper- tion (Illf?) of danburite was determined calorimetrically by Semenov et ai. (1988); earlier entropy, and specific imental and calorimetric data are available (Kurshakova, 1982; Semenov et aI., 1988), much more are necessary to heat measurements for datolite and danburite (Zhdanov define the stability relations of calcium borosilicates in et aI., 1977; Agoshkov et aI., 1977) were also tabulated. the system CaO-B203-Si02-H20. The present investiga- The standard enthalpy of formation of datolite was then tion is a contribution to this effort. calculated using P-T data for the reaction B-bearing minerals have not, as yet, been included in 2CaBSi04(OH) + Si02 = CaB2Si20s + CaSi03 + H20 (1) internally consistent, thermodynamic data sets (e.g., Ber- man, 1988; Holland and Powell, 1990) largely because of (Eugster and Wise, 1963) and thermodynamic data from the paucity of data currently available for these minerals. the literature; the free energy of formation of datolite cal- Few reactions involving borosilicates have been studied culated from the data published by Semenov et ai. (1988) experimentally and published calorimetric studies are in- is - 2318 :t 2 kl/moi. complete. However, efforts are now underway to fill this More recently, heat capacity data for danburite and information gap, particularly for the calcium borosili- datolite have become available (Mazdab et aI., 1992), but cates, danburite, CaB2Si20s, and datolite, CaBSi04(OH), the enthalpy of formation of datolite and, thus, its free energy offormation have never been determined directly. which occur in a wide variety of geologic environments. The standard entropy aI)d heat capacity of danburite quoted by Semenov et ai. (1988),154.8 :t 2.1 J/(mol'K) and 185.1 :t 0.9 J/(mol. K), respectively, are in close * Present address: California Environmental Protection Agen- cy, 10 1 Centre Plaza Drive, Monterey Park, California 91754, agreement with the values determined by Mazdab et ai. U.S.A. (1992) [SO= 155.4 J/(mol. K), 0 = 185.0 J/(mol. K); the 0003-004X/9 5/0506-057 6$02.00 576 YANG AND ROSENBERG: FREE ENERGY OF FORMA nON OF DA TOLITE 577 Sg98value given for danburite by Mazdab et a1. (1992) is TABLE 1. Analytical data (EPMA *) for datolite and its ideal com- actually their value for C~.298;L. M. Anovitz, personal position (in weight percent) communication]. Measured values of H373.15for danbur- Datolite ite are also nearly identical (186.1 kllmol: Semenov et Oxide EPMA Ideal aI., 1988; 185.2 kllmol: L. M. Anovitz, personal com- munication). These studies provide a reliable database Na20 0.02 0.00 FeO 0.03 0.00 for danburite, but the thermochemical parameters of da- K20 0.00 0.00 tolite are less well known. In order to provide direct mea- Si02 36.56 37.56 CaO 34.39 35.05 surements for datolite, a solubility study was undertaken AI2O, 0.01 0.00 in the temperature range 100-250°C. Ti02 0.03 0.00 Datolite is stable with respect to danburite in the sys- MgO 0.01 0.00 MnO 0.02 0.00 tem CaO-B203-Si02-H20 at low temperatures and H3B03 B2O, 21.76 activities. At low temperatures «200°C) datolite reacts H2O 5.63 to form CaB609(OH)2' H20 + quartz (Kurshakova, 1982). Total 71.01 100.00 Although the lower thermal stability limit has not been . Average of six point analyses. firmly established, extrapolation ofthe experimental data of Kurshakova (1982) suggests that, at the extremely low activities of H3B03 anticipated in solubility studies, da- After quenching, solutions were filtered through 0.1 ~m tolite may be stable above about 125°C. Preliminary ex- filters in < 5 min; pH was measured immediately after periments in this laboratory show, however, that datolite filtration. Solutions were diluted for analysis immediately persists up to four months at 100°C; reaction products after filtration to prevent precipitation due to decreasing were not detected by X-ray diffractometry or by optical temperature. Si02 and B concentrations in the solutions and electron microscopy. Alteration products (calcium were determined within 5 h, whereas Ca was analyzed borates) have been recently observed under the electron within 24 h after the termination of an experiment. Solid microscope in the products of long-term experiments at materials were washed in a centrifuge using distilled wa- lower temperatures (Yang, 1990). Thus, datolite appears ter and dried at 60°C for examination by X-ray diffrac- to be suitable for solubility studies above 100°C but not tometry and optical microscopy. below this temperature. Analytical methods SoLUBILITY STUDIES Solid products were characterized by X-ray powder Starting materials diffractometry and optical microscopy. The chemical Datolite from Summit, New Jersey (Wards research- composition of the datolite samples was determined by grade), occurs in fine-grained «0.2 mm diameter) aggre- electron microprobe analysis (Table 1). Inasmuch as in- gates with calcite and minor amounts of quartz. The bulk significant amounts of nonessential elements were ob- sample was ground to <50 ~m. To remove the carbonate, served, the ideal formula has been used throughout this the sample was washed with a dilute sodium acetate so- study; elements present in datolite at low concentrations lution following the procedures of Kittrick and Hope (eg., Fe, Ti) were not determined in the dissolution ex- (1963). Quartz was not separated because it does not sig- periments. nificantly affect the solubility of datolite under the exper- The colorimetric, azomethine-H method (John et aI., imental conditions of this study (silica concentrations in 1975) was used to determine B concentrations in solution the experiments were higher than those for quartz equi- with an error of < 3%. Aqueous silica was analyzed using librium). Preliminary experiments suggested that some the molybdosilicate method (Skougstad et al., 1979) with amorphous silica may be present in the sample; it was an estimated precision of ::t5%. Ca concentrations were removed by washing with O.5N NaOH solution (Foster, determined to within 10% by atomic absorption spectro- 1953) followed by rinsing with double distilled water. The photometry (AA). The pH values were measured at room size fraction <0.2 ~m was discarded and the remaining temperature with a precision of ::to.05 pH units using a mineral powder was dried at 60°C. Double distilled water combination glass electrode and a Beckman 71 pH meter was used as the starting solution in all experiments. standardized with two buffers. The overall error in the free energy of formation of datolite, owing to analytical Laboratory procedures uncertainties, is estimated to be <2 kllmo1. All experiments were carried out in Teflon(PTFE)-lined, Al or stainless steel pressure vessels. The 20 mL Teflon Calculations liners contained 12-15 mL H20 and 0.5-2 g of mineral Activity coefficients and pH at elevated temperatures powder. These vessels were heated in ovens for up to four were calculated from concentrations and pH measured at months and then quenched to room temperature in 5-15 25°C and with the use of the program SOL VEQ (Reed, min in cold water (Sass et aI., 1987; Aja, 1989).
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