Here are the essential concepts you must grasp in order to answer the question correctly.
Molar Solubility
Molar solubility is the number of moles of a solute that can dissolve in a liter of solution at equilibrium. It is a measure of how much of a substance can be dissolved in a solvent, and it is often expressed in moles per liter (M). Understanding molar solubility is crucial for predicting how much of a compound will dissolve in a given solution, especially in the context of saturated solutions.
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Common Ion Effect
The common ion effect refers to the decrease in solubility of an ionic compound when a common ion is added to the solution. This phenomenon occurs because the addition of a common ion shifts the equilibrium position of the dissolution reaction, leading to a lower concentration of dissolved ions. In the case of AgBr, the presence of AgNO3 or NaBr introduces Ag+ or Br- ions, respectively, which can significantly affect the solubility of AgBr.
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Ksp (Solubility Product Constant)
The solubility product constant (Ksp) is an equilibrium constant that applies to the solubility of sparingly soluble ionic compounds. It is defined as the product of the molar concentrations of the ions, each raised to the power of their coefficients in the balanced equation. For AgBr, Ksp can be used to calculate its molar solubility in different solutions by setting up an equilibrium expression that incorporates the concentrations of Ag+ and Br- ions.
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Solubility Product Constant