Solubility Equilibria and Ksp Calculations Lecture Notes

Flashcards covering key concepts, definitions, and applications related to solubility equilibria and the solubility product constant (Ksp) from the lecture notes.

Solubility Equilibria

Established when the dissolution and precipitation of a solute species occur at equal rates.

Saturated Solution

A solution formed when a solute is added to a solvent in an amount exceeding its solubility, resulting in a heterogeneous mixture of the saturated solution and the excess, undissolved solute.

Sparingly Soluble Salt

An ionic solid that dissolves slightly, producing a very dilute solution of ions in equilibrium with its undissolved solid form.

Solubility Product Constant (Ksp)

The equilibrium constant for solubility equilibria, representing the product of the concentrations of the dissolved ions, each raised to the power of its stoichiometric coefficient in the dissolution equation.

Molar Solubility

The solubility of a compound, measured as moles of dissolved solute per liter of saturated solution.

Reaction Quotient for Solubility (Qsp)

A value that compares ion concentrations in a mixture to the Ksp to predict whether precipitation will occur. If Qsp < Ksp, no precipitation; if Qsp > Ksp, precipitation occurs; if Qsp = Ksp, equilibrium is established.

Selective Precipitation

An experimental strategy used to remove individual ions from a solution containing two or more ions that may form insoluble compounds with the same counter ion, by controlling the counter ion concentration.

Common Ion Effect

The phenomenon where the solubility of an ionic compound is decreased in an aqueous solution containing a common ion (an ion also produced by the dissolution of the ionic compound), explained by Le Châtelier's principle.

Hydroxylapatite (Ca5(PO4)3OH)

A compound formed from calcium and phosphate ions, often precipitated in wastewater treatment to remove phosphates.