11.3 Solubility
2 min read•june 25, 2024
is a key concept in chemistry, influenced by various factors. Temperature and pressure play crucial roles, affecting how substances dissolve in different ways. Understanding these effects helps predict and control in various applications.
explains gas solubility in liquids, relating it to pressure. Liquid-liquid solubility ranges from fully to , depending on molecular properties. These principles are essential for understanding behavior and chemical processes.
Factors Affecting Solubility
Temperature and pressure effects on solubility
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- Temperature effects on solubility
- Solids in liquids
- Generally increases solubility as temperature rises (sugar, salt)
- Endothermic process absorbs heat favored by higher temperatures
- Gases in liquids
- Decreases solubility as temperature rises (carbonated beverages, oxygen in water)
- Exothermic dissolution process releases heat favored by lower temperatures
- Solids in liquids
- Pressure effects on solubility
- Solids and liquids
- Minimal effect on solubility due to incompressible nature of substances
- Gases in liquids
- Increases solubility as pressure rises following Henry's law
- Gas solubility directly proportional to partial pressure of gas above solution
- Solids and liquids
Henry's law for gas solubility
- Henry's law:
- : solubility of gas (mol/L or M)
- : Henry's law constant (mol/L·atm or M/atm) specific to gas-liquid pair at given temperature
- : partial pressure of gas above solution (atm)
- Calculating gas solubility
- Determine Henry's law constant for specific gas-liquid pair at given temperature
- This constant is related to the process of the gas in the liquid
- Identify partial pressure of gas above solution
- Multiply Henry's law constant by partial pressure to find solubility
Liquid-Liquid Solubility
Spectrum of liquid-liquid solubility
- : ability of liquids to mix forming homogeneous solution
- Fully miscible liquids
- Completely soluble in each other forming single phase (ethanol and water, acetone and water)
- liquids
- Soluble in each other to limited extent forming two phases with different compositions (ether and water)
- Immiscible liquids
- Insoluble in each other forming two distinct phases with no mixing (oil and water, hexane and water)
- Factors affecting miscibility
- : similar polarity promotes miscibility
- Hydrogen bonding: liquids capable of hydrogen bonding more likely to be miscible
- Temperature: higher temperatures may increase miscibility
Solubility Dynamics
- : the point at which a solution contains the maximum amount of dissolved at a given temperature and pressure
- Dissolution: the process by which a dissolves in a to form a solution
- : the formation of a solid from a solution when it becomes
Key Terms to Review (26)
Dissolution: Dissolution is the process by which a solute (a substance that is dissolved) disperses and incorporates into a solvent (the dissolving medium) to form a homogeneous solution. This term is central to understanding the fundamental concepts of solubility and precipitation in chemistry.
Henry’s law: Henry's law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid. This relationship is typically expressed as $C = kP$, where $C$ is the concentration of the gas, $k$ is Henry's law constant, and $P$ is the partial pressure.
Henry's Law: Henry's Law is a fundamental principle in chemistry that describes the relationship between the concentration of a gas dissolved in a liquid and the partial pressure of that gas above the liquid. It states that the amount of a gas that dissolves in a liquid is directly proportional to the partial pressure of that gas in contact with the liquid.
Immiscible: Immiscible describes liquids that do not mix together to form a homogeneous solution. When combined, immiscible liquids separate into distinct layers.
Le Chatelier's Principle: Le Chatelier's Principle states that when a system at equilibrium is subjected to a change in one of the conditions (concentration, temperature, or pressure) affecting that equilibrium, the system will shift to counteract the change and re-establish equilibrium.
Miscibility: Miscibility refers to the ability of two or more liquids to mix in any proportion without separating into two phases. This property is crucial in understanding how different substances interact, particularly in terms of solubility and the formation of solutions. When liquids are miscible, they can form a homogeneous mixture, while immiscible liquids do not mix and instead separate into distinct layers.
Miscible: Miscible substances are those that can be mixed together in any proportion to form a homogeneous solution. Typically, this term is used to describe liquids.
Partially miscible: Partially miscible liquids are those that can dissolve in each other but only to a limited extent. Beyond a certain concentration, two distinct liquid layers will form.
Polarity: Polarity refers to the unequal distribution of electrons within a molecule, resulting in the creation of partially positive and partially negative regions. This concept is fundamental in understanding the properties and behavior of ionic, molecular, and organic compounds.
Precipitation: Precipitation is the process by which a solid or liquid substance separates from a solution or suspension and forms a distinct phase. This phenomenon is commonly observed in the context of chemical reactions and the solubility of substances in various media.
Precipitation reaction: A precipitation reaction occurs when two aqueous solutions react to form an insoluble solid, known as the precipitate. This type of reaction is a double displacement reaction where the ions in solution exchange partners.
Recrystallization: Recrystallization is a purification technique used to isolate a solid compound from a mixture by taking advantage of differences in solubility. It involves dissolving the impure solid in a suitable solvent, followed by controlled cooling or evaporation to induce the formation of pure crystals.
Saturated: A solution is saturated when it contains the maximum amount of solute that can dissolve at a given temperature and pressure. Any additional solute will remain undissolved.
Saturation: Saturation refers to the maximum amount of a substance that can be dissolved in a given volume of a solvent at a specific temperature. It is a key concept in understanding the solubility of substances and the equilibrium that exists between dissolved and undissolved components in a solution.
Solubility: Solubility is the maximum amount of a substance that can dissolve in a solvent at a given temperature and pressure. It determines how substances interact in solutions.
Solubility: Solubility is a measure of the ability of a substance to dissolve in a solvent, forming a homogeneous solution. It is a fundamental concept in chemistry that describes the maximum amount of a substance that can be dissolved in a given volume of a solvent under specific conditions of temperature and pressure.
Solubility Product: The solubility product, denoted as $K_{sp}$, is an equilibrium constant that describes the solubility of a slightly soluble ionic compound in water. It represents the product of the concentrations of the ions in a saturated solution of the compound, each raised to the power of their stoichiometric coefficients.
Solute: A solute is a substance that is dissolved in a solvent to form a solution. It can be in any phase: solid, liquid, or gas.
Solute: A solute is the substance that is dissolved in a solution, typically in smaller quantities compared to the solvent. It is the component of a solution that is present in a lesser amount and is dispersed throughout the solvent.
Solution: A solution is a homogeneous mixture composed of two or more substances. In a solution, a solute is dissolved in a solvent, resulting in a single phase with a uniform composition and properties throughout.
Solvation: Solvation is the process of surrounding solute particles with solvent molecules to form a solution. It involves interactions between the solute and solvent molecules.
Solvation: Solvation is the process by which solute particles or ions become surrounded by solvent molecules, forming a solvated species. This interaction between the solute and solvent is a critical aspect of the dissolution process, the behavior of electrolytes, and the solubility of substances.
Solvent: A solvent is a substance, typically a liquid, that dissolves a solute to form a solution. The solvent is usually present in greater amount compared to the solute.
Solvent: A solvent is a liquid, solid, or gas that can dissolve other substances, known as solutes, to form a solution. Solvents play a crucial role in various chemical processes, including chemical reactions, extraction, and purification.
Supersaturated: A supersaturated solution is a solution that contains more dissolved solute than the solvent can normally hold at a given temperature. This state is unstable and the excess solute will typically precipitate out of the solution if given the chance.
Unsaturated: An unsaturated solution is one that contains less solute than the maximum amount that can be dissolved at a given temperature. Additional solute can still be added and dissolved in an unsaturated solution.