medium · MCAT chem-phys
A 1.0 L saturated solution of AgBr (K_sp = 5.0 × 10^-13) is prepared.
If 0.01 moles of solid NaBr are added, which statement accurately describes the change in molar solubility of AgBr?
- The molar solubility remains unchanged because K_sp is a fixed thermodynamic constant at any given temperature.
- The molar solubility decreases because the increased [Br^-] drives the dissolution equilibrium toward the solid phase.
- The molar solubility increases because the added Na^+ ions help stabilize the dissolved Ag^+ ions in solution, per ionic theory.
- The molar solubility increases because the reaction quotient Q becomes less than K_sp, favoring further net dissolution overall.
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