RELATIONSHIP BTN Ksp AND PRECIPITATION CONTINUED

The relationship between Ksp (solubility product constant) and precipitation is fundamental in understanding how solids dissolve and come out of solution. Here's the key concept:

* **Ksp is a constant value for a specific ionic compound.** It represents the equilibrium point at which the dissolved ions (from the compound) and the undissolved solid are in balance within a solution.

* **Precipitation occurs when the concentration of dissolved ions exceeds the Ksp value.** This means there are more ions floating around in the solution than the system can stably hold at equilibrium. To re-establish equilibrium, the excess ions come together and form a solid precipitate.

Here's a breakdown of the relationship:

* **Ksp > Qsp (ionic product):** Solution is unsaturated. No precipitation occurs.
* **Ksp = Qsp:** Solution is saturated. Ions are at equilibrium and neither dissolving nor precipitating.
* **Ksp < Qsp:** Solution is supersaturated. Precipitation will occur to reduce the ion concentration and reach equilibrium.

In essence, Ksp acts as a threshold. If you push the system past this point (by adding more solute or changing conditions), precipitation will happen to restore equilibrium.