a) Assume a water sample is saturated in CO2 in equilibrium with an atmosphere containing 410 ppm (volume) of CO2 at 1 atm. The dissolved CO2 concentration is 1.4x10M. Express the CO2 (aq) concentration as a mole fraction and the CO2(g) concentration as a partial pressure (atm), and calculate the Henry's Law constant, K. (in atm units). CO2 (aq) mole fraction: CO2(g): atm : atm b) The water sample contains the following ions (only): H+, OH, HCO3, CO3-, SO4?, Ca2+. The pH is 7.4, the dissolved CO2 concentration is 1.4x10-M, and the sulfate (SO2) concentration is 4x10 5 M. Calculate the concentrations (M) of all ions (except SO42- which is given) using the following equilibria. H20 - H+ + OH pKw = 14 H2CO3 H+ + HCO3 pK 1 = 6.35 HCO3+ + CO32- PK 2 = 10.33 M M M H: OH: HCO3 CO32: Cat: c) Is any CaCO3 precipitate formed? Show by calculation using the solubility product data: CaCO3(s) Ca2+ + CO32- pKp = 8.34 M M