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The concentration of sulfate did not increase much in the Cascade tests. This implies <br /> that the end-product of Cascade under these conditions is elemental sulfur, not sulfate <br /> It should be emphasized that the magnitude of the changes in secondary water quality <br /> may be different in the field due to differences between field and laboratory conditions <br /> Thus, the results presented in Table 5 ,should be used as a guide to help determine which <br /> parameters, if any, could potentially be of concern and should be monitored during field <br /> pilot- or full-scale application. <br /> 3.4 Buffering/Titration Curves <br /> The buffering and titration curves generated for site groundwater (MW-3), site tap water <br /> and soil SB-10-3 are shown in Figures 1-4 Tabulated data are given in Appendix A. <br /> 3.4.1 Acid Required to Prepare Fe(ED Solution <br /> IFe(II) solution is prepared by dissolving ferrous iron heptahydrate (FeSO4 7H2O) in <br /> acidified (pH 24)water Based on the results shown in Figure 1, the amount of <br /> concentrated (98%) sulfuric acid (H2SO4) needed to decrease the pH of site tap water to <br /> pH—3 is 3 mmoles Hk/L of tap water, which is equivalent to about 300 mL of 98% <br /> H2SO4/1000 gallons of water(0 08 gallons 98%H2SO4/1000 gallons tap water). <br /> 9 <br /> 8 —a Groundwater(MW-3) <br /> 0 Site Tap Water <br /> 7 <br /> 5 <br /> 2 <br /> 4 <br /> 3 <br /> I� 2 <br /> 1 <br />� Q <br /> 0 05 1 15 2 25 3 35 4 <br /> mmoles H;Added 1100 mL Water <br /> Figure 1. Titration of 100 mL Water using 0.1 N H2SO4. <br />' PRiMA Environntental 10 Eval of Reductants <br /> January 19,2005 ATC-Diamond Walnut <br />