For the dissolution of BaSO4(s) ⇌ Ba^2+(aq) + SO4^2−(aq), if the solubility is s, which expression gives Ksp?

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Multiple Choice

For the dissolution of BaSO4(s) ⇌ Ba^2+(aq) + SO4^2−(aq), if the solubility is s, which expression gives Ksp?

Explanation:
Ksp is the product of the molar concentrations of the ions formed when a sparingly soluble salt dissolves. For BaSO4, the dissolution yields Ba2+ and SO4^2− in a 1:1 ratio. If the solubility is s, then [Ba2+] = s and [SO4^2−] = s, so Ksp = [Ba2+][SO4^−] = s × s = s^2. The other powers would imply different stoichiometry or additional species are involved, which isn’t the case here.

Ksp is the product of the molar concentrations of the ions formed when a sparingly soluble salt dissolves. For BaSO4, the dissolution yields Ba2+ and SO4^2− in a 1:1 ratio. If the solubility is s, then [Ba2+] = s and [SO4^2−] = s, so Ksp = [Ba2+][SO4^−] = s × s = s^2. The other powers would imply different stoichiometry or additional species are involved, which isn’t the case here.

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