The answers are a) 4.3x10^-5. b) 5.2*10^-4 M =21 mg/L. c) 0.023 bar. Please show work. Thank you!
8-34. Heterogeneous equilibria and calcite solubility. If river water in Box 8-2 saturated with (CaCO), (Ca] is governed by is calcite the following equilibria: CaCO,(S) - Ca? + CO ? K, p = 4.5 X 10 CO , 0.032 CO2(g) = CO2(aq) COLaq) + HO HCO ; + H K= 4.46 X 107 K, = 4.69 x 10-1 HCO) = CO , + H (a) Combine these reactions to find the equilibrium constant for the reaction CaCO,(s) + CO2(a) + HO - Car + 2HCO, K = ? (A) (b) The mass balance for Reaction A is [HCO,] = 2[Ca]. Find [Cai (in mol/L and in mg/L) in equilibrium with atmospheric CO, if P = 4.0 X 10 " bar = 10 34 bar. Locate this point on CO2 the line in Box 8-2 2 (c) The concentration of Ca" in the Don River is 80 mg/L. What effective PCO, is in equilibrium with this much Cat? How can the river have this much CO,?
