The solubility of CaCO3 is pH dependent. (a) Calculate themolar solubility of CaCO3 (Ksp = 4.5 x 10-9) neglectingthe acid–base character of the carbonate ion. (b) Use the Kbexpression for the CO32 - ion to determine the equilibriumconstant for the reactionCaCO3(s) + H2O(l)  ⇌ Ca2 + (aq) + HCO3-1 (aq) + OH-1 (a q)(c) If we assume that the only sources of Ca2 + , HCO3-,and OH- ions are from the dissolution of CaCO3, what is the molar solubility of CaCO3 using the equilibrium expressionfrom part (b)? (d) What is the molar solubility ofCaCO3 at the pH of the ocean (8.3)? (e) If the pH is bufferedat 7.5, what is the molar solubility of CaCO3?

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