Solubility Equilibrium
Solubility Equilibrium - Related Videos
04:02
Solubility - Concepts
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2020
Solubility Solubility describes how much of a solute can dissolve in a given volume of a specific solvent. Solubility is usually reported in terms of solute mass per solvent volume or solute mass per solvent mass. For example, the solubility of sodium chloride in water at room temperature is reported as 36 g per 100 mL of water. If solubility is reported in solute mass per solvent mass, the solvent mass will need to be converted to volume for further calculations. Solubility changes with...
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Solubility Equilibria
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2020
Solubility equilibria are established when the dissolution and precipitation of a solute species occur at equal rates. These equilibria underlie many natural and technological processes, ranging from tooth decay to water purification. An understanding of the factors affecting compound solubility is, therefore, essential to the effective management of these processes. This section applies previously introduced equilibrium concepts and tools to systems involving dissolution and precipitation. The...
04:01
Factors Affecting Solubility
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2020
Compared with pure water, the solubility of an ionic compound is less in aqueous solutions containing a common ion (one also produced by dissolution of the ionic compound). This is an example of a phenomenon known as the common ion effect, which is a consequence of the law of mass action that may be explained using Le Chȃtelier’s principle. Consider the dissolution of silver iodide: This solubility equilibrium may be shifted left by the addition of either silver or iodide ions, resulting in...
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Solubility of Ionic Compounds
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2020
Solubility is the measure of the maximum amount of solute that can be dissolved in a given quantity of solvent at a given temperature and pressure. Solubility is usually measured in molarity (M) or moles per liter (mol/L). A compound is termed soluble if it dissolves in water. When soluble salts dissolve in water, the ions in the solid separate and disperse uniformly throughout the solution; this process represents a physical change known as dissociation. Potassium chloride (KCl) is an example...
02:20
Dynamic Equilibrium
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2020
A reversible chemical reaction represents a chemical process that proceeds in both forward (left to right) and reverse (right to left) directions. When the rates of the forward and reverse reactions are equal, the concentrations of the reactant and product species remain constant over time and the system is at equilibrium. A special double arrow is used to emphasize the reversible nature of the reaction. The relative concentrations of reactants and products in equilibrium systems vary greatly;...
FAQs
A common ion shifts the balance toward the solid phase, reducing the amount of sparingly soluble material that remains dissolved. This effect changes the apparent solubility without changing the identity of the solid. Chemists use the response to control precipitation, especially when separating ions that form solids with different solubility behavior.
The solubility product constant applies at a particular temperature, so temperature changes can alter the equilibrium relationship between the solid and its dissolved ions. A comparison made using a Ksp from another temperature may misrepresent whether precipitation or dissolution is favored. Controlling temperature therefore improves predictions and makes solubility measurements comparable.
Complex formation removes some dissolved ions by binding them into chemical complexes. Lowering the concentration of free ions can favor additional dissolution of the solid, making the compound appear more soluble than it would be without complex formation. This interaction is important when interpreting precipitation behavior in chemically complicated solutions.
A selective precipitation approach compares the ion product for possible solids with each substance’s Ksp. Conditions are adjusted so that one solid reaches its precipitation threshold before others, allowing dissolved species to be separated. Monitoring which solid forms under the chosen conditions helps researchers use equilibrium differences rather than treating all ions as equally soluble.
In qualitative inorganic analysis, precipitation behavior provides evidence about which ions may be present. By examining whether combinations of dissolved ions produce solids under selected conditions, chemists can distinguish species with different solubility relationships. The resulting observations support identification schemes and show how equilibrium constants connect visible precipitates with ionic composition.
Water treatment applications use precipitation to remove selected dissolved substances, while mineral formation studies use the same equilibrium principles to understand when solids can develop from solution. In both settings, ion concentrations, temperature, common ions, and complex formation influence the outcome. These variables help explain and manage solid formation in natural or engineered systems.