Final answer:
To determine which of the two compounds A₂X or A₃X₂ with the same Ksp value has a higher molar solubility, the stoichiometry of their dissolution must be considered. Direct comparison is not possible without solubility values or additional data, as Ksp values depend on the dissolution stoichiometry, which differs for each compound.
Step-by-step explanation:
The question is inquiring about the molar solubility of two compounds, A₂X and A₃X₂, both with a given Ksp of 1.5×10⁻⁵ M. To determine which compound has a higher molar solubility we need to consider their stoichiometry in the dissolution process. For A₂X, the dissolution can be represented as A₂X(s) → 2A+(aq) + X⁻²(aq), and the solubility product will be Ksp = [A+] * [X⁻²]. Similarly, for A₃X₂, the dissolution can be represented as A₃X₂(s) → 3A+(aq) + 2X⁻²(aq), and the solubility product will be Ksp = [A+] ³ * [X⁻²]². Without the actual solubility values or more information, it’s not possible to accurately compare the molar solubility of the two compounds based solely on the Ksp values because the formulas involve different stoichiometries in the balanced dissolution equations. Therefore, we need either the individual solubilities or additional data to compare them directly.