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17 Nov 2019
The reactions for the dissolution of limestone (CaCO_3(s)) and for the dissociation of bicarbonate ion (HCO_3^-) are as follows. CaCO_3(s) Ca^2+ + CO_3^2- K_eq = 10^-8.3 HCO_3^- H^+ + CO_3^2- K_eq = 10^-10-33 These reactions have reached equilibrium in a solution at pH 9.33 that contains 10^-2 mol/L CaCO_3(.s) and 10^-3 3 mol/L Ca^2+. What is the HCO_3^- concentration in the solution, assuming that activity coefficients for all species are 1.0? Would you expect the Ca^2+ concentration to increase, decrease, or not change if the system changed in the following ways? (For this part of the problem, do not assume that activity coefficients are 1.0.). Explain your reasoning briefly (1-2 sentences). The concentration of CaCO_3(.s) is doubled.
The reactions for the dissolution of limestone (CaCO_3(s)) and for the dissociation of bicarbonate ion (HCO_3^-) are as follows. CaCO_3(s) Ca^2+ + CO_3^2- K_eq = 10^-8.3 HCO_3^- H^+ + CO_3^2- K_eq = 10^-10-33 These reactions have reached equilibrium in a solution at pH 9.33 that contains 10^-2 mol/L CaCO_3(.s) and 10^-3 3 mol/L Ca^2+. What is the HCO_3^- concentration in the solution, assuming that activity coefficients for all species are 1.0? Would you expect the Ca^2+ concentration to increase, decrease, or not change if the system changed in the following ways? (For this part of the problem, do not assume that activity coefficients are 1.0.). Explain your reasoning briefly (1-2 sentences). The concentration of CaCO_3(.s) is doubled.
Reid WolffLv2
24 Sep 2019