Solubility and Equilibria

These flashcards cover key vocabulary and concepts related to solubility, equilibria, and relevant chemical reactions.

Ksp

The solubility product constant, representing the equilibrium constant for a sparingly soluble salt's dissociation into its ions.

Solubility Equilibria

Equilibria that involve the dissolution and precipitation processes in saturated solutions of ionic compounds.

Molar solubility

The number of moles of solute that can be dissolved in one liter of saturated solution.

Common ion effect

The decrease in solubility of an ionic compound due to the presence of a common ion.

Fractional precipitation

The process of selectively precipitating one compound while keeping others in solution.

Lewis acids

Substances that accept electron pairs to form bonds.

Lewis bases

Substances that donate electron pairs to form bonds.

Complex ion

A species formed from a central metal ion bonded to one or more molecules or ions.

Saturated solution

A solution in which the maximum amount of solute has dissolved at a given temperature.

Q (reaction quotient)

A measure of the concentration of reactants and products at a given state of the reaction, used to predict the direction of the equilibrium.

Ksp (AgCl)

The equilibrium constant for the dissolution of silver chloride, indicating its solubility.

Dilution

The process of reducing the concentration of a solute in solution, typically by mixing with a solvent.

Precipitate

An insoluble solid that forms and separates from a liquid solution.

Molarity (M)

A measure of concentration, defined as moles of solute per liter of solution.

Kf

The formation constant, indicating the strength of a complex ion formation in solution.

Precipitation reactions

Chemical reactions in which a solid forms and separates from a solution.

Ag+(aq) + 2NH3(aq)

The reaction forming the complex ion [Ag(NH3)2]+, where silver ion combines with ammonia.