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1.2 1.0 0.8 0.6 0.4 0.2 0.0 H2CO3 HCO3- CO32- 1 2 3 4 5 6 7 8 9 10 11 12 13 14 pH Figure 1: Total Carbonate Expressed as a Function of pH By examining Figure 1, the fractional amounts of carbonate species at pH of 7.8 are αH2CO3 = 0.04, αHCO3- =- 0.96, and αCO3- = 0.0 indicating that 96 % of the carbon in the oceans is in the form of HCO3 . At pH of 4.5, it shows that 99 % of all carbonate species exist as H2CO3. CO2 dissolved in water is in equilibrium with H2CO3 as shown in equation 15 as: CO2 + H2O = H2CO3 (15) The hydration equilibrium constant is 1.70×10−3. This indicates that H2CO3 is not stable and gaseous CO2 readily dissociates at pH of 4.5, allowing CO2 to be easily removed by degassing. In order to convert HCO3- to H2CO3, the pH of seawater must be lowered. A detailed composition of seawater shows a carbon (C) concentration of 28 ppm (~100 mg/L as CO2). Assuming that C exists as HCO3-, the HCO3- concentration in seawater will be approximately 142 ppm (0.0023 M), therefore approximately 23 mL of 0.100 M hydrochloric acid (HCl) acid is required per liter of seawater where Cl- is chloride ion. HCl + HCO3- H2CO3 + Cl- (16) Johnson et al. demonstrated this concept when they showed that CO2 existed only in the dissolved gas form when the pH of seawater was decreased to 6 or less [14]. Based on these principles, Hardy et al. investigated the use of simple strong cation exchange resin systems to increase the rate and yield of carbon dioxide recovery from seawater [3]. They successfully utilized the ion exchange material to acidify the seawater below pH 6. However, the volume of water per unit weight of resin required to regenerate the resin was much larger than the volume of CO2 recovered, and potentially larger than the volume of fuel produced from the CO2. As a result the approach was deemed impractical for a sea-based application [3]. Thus as one further 3 Fractional Amount (α)PDF Image | CO2 from Seawater
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