Here are the essential concepts you must grasp in order to answer the question correctly.
Molar Solubility
Molar solubility refers to the maximum amount of a solute that can dissolve in a given volume of solvent at a specific temperature, expressed in moles per liter (M). It is a crucial concept in understanding how ionic compounds dissociate in solution and is often determined through equilibrium expressions.
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Common Ion Effect
The common ion effect describes the decrease in solubility of an ionic compound when a common ion is added to the solution. In this case, the presence of Ba<sup>2+</sup> ions from Ba(NO<sub>3</sub>)<sub>2</sub> will shift the equilibrium of barium fluoride dissolution, reducing its molar solubility due to Le Chatelier's principle.
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Equilibrium Constant (Ksp)
The solubility product constant (Ksp) is an equilibrium constant that applies to the dissolution of sparingly soluble ionic compounds. It quantifies the product of the molar concentrations of the ions in a saturated solution, raised to the power of their coefficients in the balanced dissolution equation, and is essential for calculating molar solubility in different solutions.
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