An empirical equation of quartz solubility in H
2O at elevated pressures and temperatures (up to 10 kb and 900°C) is obtained based on the published experimental results. The resultant solubility equation is as follows: lnS
water = –1.51914 + 1.99970lnρ
water – 2636.78
T–1 + 0.00387766
T + 0.0198582
PT–1, where
Swater,
Pwater,
T, and
P stand for quartz solubility (mol/kg H
2O), density (g/cm
3) of pure water, temperature (Kelvin), and pressure (bar), respectively. Densities of pure water are calculated by the equation of Haar
et al. (1984). The solubility equation is then modified for describing the solubility behavior of quartz in H
2O + CO
2 or H
2O + NaCl fluid. For the modification, this study uses the weight fraction of water in the solvent (
F), density of the aqueous fluid (ρ
aq), and an empirical constant (Θ) as the additional terms. The ratio of quartz solubility in aqueous fluid (
Saq) to that in pure water (
Swater) at the same pressure-temperature condition is then expressed as ln(
Saq/
Swater) = Θln(ρ
aqF/ρ
water). Densities of H
2O + CO
2 and H
2O + NaCl fluids are computed with the equations of Kerrick and Jacobs (1981) and Anderko and Pitzer (1993a), respectively. The empirical constant for quartz solubility in H
2O + CO
2 fluid is 1.49063. For obtaining the constant, this study considers the published experimental results done at 1.5 kb to 5 kb, 600° to 700°C, and up to 71 wt% CO
2 concentration (mole fraction of CO
2 = 0.505). The O value for quartz solubility in H
2O + NaCl fluid is 3.24740, which gives the calculated solubilities consistent with the experimental results done at 0.2 kb to 2 kb, 200° to 700°C, and up to 33.6 wt% NaCl concentration.
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