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of water. These ion exchange reactions are <br />2NaA/SiZ06 HSUB20+CaZ =Ca(AISiZ06)Z•HZO+2Na <br />2NaA1Si~06•HZO+Mg'- =Mg(A(SiZ06)•HZO+2Na' <br />MgZ~+Na-Clay=2NaZ +Mg-Clay <br />CaZ +Na -clay =2Na ' +Ca -clay <br />The statement is made that the Edwards Portal spring water could not be "in-mine fault water" <br />because no plausible mechanism exists for reducing the Na content of water between the in-mine <br />faults and the Edwards Portal spring because the loss in Na would require reverse ion exchange. <br />That ignores the equilibrium constant of the reaction, mathematically described by the Gibbs <br />Free Energy G in the following equation: <br />OG =-RTInK <br />rin ¢ <br />where the (G) is a function of temperature and the equilibrium constant Ka of the reaction. <br />Using the 4th mineral reaction listed above, in which Mg is exchanged for Na in a clay, <br />MgZ +Na-clay=2Na'+Mg-clay <br />the equilibrium constant is the activity of the reaction products divided by that of the reactants. <br />Symbolically, <br />Ka =(a Na)Z(aAfgclay)!(aMg)(aNacluy) <br />The activity (a) is essentially the concentration of each of those reaction constituents (Na, Mg, <br />Na-clay and Mg-clay). The K• term is a constant for the temperature, so the proportions of <br />each participant in the reaction adjusts itself to maintain equilibrium concentrations at the <br />