Explain why BaCO3 is soluble in aqueous HCl, but BaSO4, which is used to make the intestines vis

step 1 In this problem, we're asked to explain why barium carbonate is soluble in aqueous hydrochloric

Explain why BaCO3 is soluble in aqueous HCl, but BaSO4,...

Explain why $\mathrm{BaCO}_{3}$ is soluble in aqueous $\mathrm{HCl}$, but $\mathrm{BaSO}_{4}$, which is used to make the intestines visible in X-ray photographs, remains sufficiently insoluble in the $\mathrm{HCl}$ in a human stomach so that poisonous barium ions do not get into the bloodstream.

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Key Concepts

Acid-Base Reaction and Equilibrium Shift

When BaCO? is added to aqueous HCl, it undergoes an acid-base reaction where the carbonate ion (CO?²?) reacts with hydrogen ions (H?) to form carbonic acid (H?CO?), which then breaks down into CO? and H?O. The production and subsequent escape of CO? gas from the reaction mixture drives the reaction forward by Le Chatelier’s principle, thereby enhancing the dissolution of BaCO?. BaSO?, however, does not react with HCl because the sulfate ion (SO?²?) does not undergo a similar reaction, so its solubility remains negligibly low.

Solubility Product and Lattice Energy

The solubility of ionic compounds is critically determined by their solubility product (Ksp), which reflects the balance between the lattice energy (the energy holding the ionic solid together) and the hydration energy (the energy released when the ions interact with water). BaSO? has a very low Ksp because its lattice energy is high relative to its hydration energy, making it extremely insoluble in water—even in the presence of acids. In contrast, BaCO? has a higher solubility product, meaning it is more readily able to dissolve under the right conditions.

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