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The solubility of CaCO3 is pH dependent. (a) Calculate the molar solubility of CaCO3(Ks p=4.5 ×10^-9) neglecting the acid-base character of the carbonate ion. (b) Use the Kb expression for the CO3^2- ion to determine the equilibrium constant for the reaction CaCO3(s) H2 O(l) ⇌Ca^2 (a q) HCO3^-(a q) OH^-(a q) (c) If we assume that the only sources of Ca^2 , HCO3^- and OH^- ions are from the dissolution of CaCO3, what is the molar solubility of CaCO3 using the equilibrium expression from part (b)?
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SOLVED: Recall the effect of pH on the solubility of CaCO3 that we discussed in class. The equations involved are Equation (1): CaCO3 (s) ⇌ Ca2 (aq) CO3^2-(aq) Equation (2): CO2^2-(aq) H3O (aq) ⇌ HCO3^-(aq) H2O (CaCO3 has Ksp = 4.96 x 10^-9, HCO2 has Ka1 = 4.45 x 10^-7 and Ka2 = 4.7 x 10^-17)(a) Calculate the equilibrium constant (K) for Equation (2).(b) Calculate the equilibrium constant (K) for the following reaction: CaCO3 (s) H2O(aq) ⇌ Ca2 (aq) HCO3^-(aq) H2OAnswer:(c) The
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