Final answer:
To calculate the molar solubility of calcium carbonate (CaCO3) while ignoring the acid-base nature of carbonate, use the solubility product constant (Ksp = 4.5 × 10^-9) and an ICE table set-up to find the solubility 's'. The equation becomes Ksp = s^2, and solving for 's' gives the molar solubility. This method ignores reactions in acidic solutions that can alter the solubility.
Step-by-step explanation:
The solubility of calcium carbonate (CaCO3) is influenced by the pH level of the solution, which can change the solubility by affecting the carbonate ion. To calculate the molar solubility of CaCO3, ignoring its acid-base nature, an ICE (Initial, Change, Equilibrium) table can be used along with its solubility product constant (Ksp): 4.5 × 10−9.
Setting up the dissolution equation:
CaCO3(s) ⇒ Ca2+ (aq) + CO32−(aq)
With Ksp = [Ca2+][CO32−], assuming equal molar solubility 's' for Ca2+ and CO32−, the Ksp expression becomes:
4.5 × 10−9 = s × s = s2
Solving for 's' gives the molar solubility of CaCO3. However, this calculation does not account for any additional reactions such as the dissolution in acidic conditions or the formation of carbonic acid in the presence of dissolved CO2, which may increase the actual solubility.