| Term | Definition |
|---|---|
| concentration | The amount of solute dissolved in a given volume of solution, typically expressed in molarity or other units of amount per volume. |
| disturbance | A change or stress applied to a system at equilibrium that causes Q to differ from K and shifts the system out of equilibrium. |
| equilibrium | The state in which the forward and reverse reaction rates are equal, resulting in constant concentrations or partial pressures of reactants and products. |
| equilibrium constant | A numerical value that expresses the ratio of products to reactants at equilibrium, indicating the extent to which a reaction proceeds. |
| partial pressure | The pressure exerted by a single gas in a mixture of gases, used in equilibrium expressions for gas-phase reactions. |
| reaction quotient | A value calculated using the same expression as the equilibrium constant but using current (non-equilibrium) concentrations or partial pressures. |
| Term | Definition |
|---|---|
| absorption | The process by which a gas is taken up by a solid or liquid. |
| concentration | The amount of solute dissolved in a given volume of solution, typically expressed in molarity or other units of amount per volume. |
| condensation | The process by which a gas converts to a liquid. |
| desorption | The process by which an absorbed gas is released from a solid or liquid. |
| dissolution | The process by which a solute dissolves in a solvent to form a solution, involving the breaking of bonds or interactions in the solute and formation of new interactions with the solvent. |
| dynamic equilibrium | A state of equilibrium in which forward and reverse reactions continue to occur at equal rates, maintaining constant macroscopic properties. |
| electron transfer | The movement of one or more electrons from one chemical species to another in a redox reaction. |
| equilibrium | The state in which the forward and reverse reaction rates are equal, resulting in constant concentrations or partial pressures of reactants and products. |
| evaporation | The process by which a liquid converts to a gas. |
| partial pressure | The pressure exerted by a single gas in a mixture of gases, used in equilibrium expressions for gas-phase reactions. |
| precipitation | The process by which a dissolved solute forms a solid and separates from a solution. |
| proton transfer | The movement of a proton (H⁺) from one species to another in an acid-base reaction. |
| reversible process | A chemical or physical process that can occur in both forward and reverse directions, such as evaporation-condensation or dissolution-precipitation. |
| Term | Definition |
|---|---|
| balanced chemical equation | A chemical equation where the number of atoms of each element is equal on both the reactant and product sides. |
| dissolution | The process by which a solute dissolves in a solvent to form a solution, involving the breaking of bonds or interactions in the solute and formation of new interactions with the solvent. |
| equilibrium system | A system in which the forward and reverse reactions occur at equal rates, resulting in constant concentrations of reactants and products. |
| Ksp | The solubility product constant; the equilibrium constant for the dissolution of a sparingly soluble salt into its ions. |
| molar solubility | The solubility of a substance expressed as the number of moles of solute that dissolve per liter of solution in a saturated solution. |
| salt | An ionic compound formed from the reaction of an acid and a base. |
| saturated solution | A solution that contains the maximum amount of dissolved solute at a given temperature, in equilibrium with undissolved solute. |
| solubility | The maximum amount of a solute that can dissolve in a given amount of solvent at a specific temperature, typically expressed in moles per liter (molarity) or grams per 100 mL of solvent. |
| solubility rules | Guidelines that predict whether an ionic compound is soluble or insoluble in water based on the identity of the cation and anion. |
| soluble salts | Ionic compounds that dissolve readily in water, typically corresponding to Ksp values greater than 1. |
| stoichiometry | The quantitative relationship between reactants and products in a balanced chemical equation that determines the rates of change of their concentrations. |
| Term | Definition |
|---|---|
| common ion | An ion that is already present in a solution and is also produced by the dissolution of a salt added to that solution. |
| common-ion effect | The phenomenon in which the solubility of a salt is reduced when dissolved in a solution that already contains one of the ions present in the salt. |
| dissolution | The process by which a solute dissolves in a solvent to form a solution, involving the breaking of bonds or interactions in the solute and formation of new interactions with the solvent. |
| Ksp | The solubility product constant; the equilibrium constant for the dissolution of a sparingly soluble salt into its ions. |
| Le Châtelier's principle | A principle stating that when a system at equilibrium is disturbed, the system shifts to counteract the disturbance and re-establish equilibrium. |
| salt | An ionic compound formed from the reaction of an acid and a base. |
| solubility | The maximum amount of a solute that can dissolve in a given amount of solvent at a specific temperature, typically expressed in moles per liter (molarity) or grams per 100 mL of solvent. |
| Term | Definition |
|---|---|
| equilibrium state | The condition reached when the rate of the forward reaction equals the rate of the reverse reaction, resulting in no net change in the amounts of reactants and products. |
| forward reaction | The reaction pathway in which reactants are converted to products. |
| net conversion | The overall change in the amounts of reactants or products as a result of the forward and reverse reactions occurring simultaneously. |
| reaction rate | The speed at which reactants are converted to products per unit of time in a chemical reaction. |
| reverse reaction | The reaction that proceeds from products back to reactants, opposite to the direction written in the balanced chemical equation. |
| reversible reaction | A chemical reaction that can proceed in both the forward and reverse directions, with reactants forming products and products reforming reactants. |
| Term | Definition |
|---|---|
| equilibrium constant | A numerical value that expresses the ratio of products to reactants at equilibrium, indicating the extent to which a reaction proceeds. |
| equilibrium expression | A mathematical equation that relates the concentrations or partial pressures of reactants and products at equilibrium, expressed as Kc or Kp. |
| Kc | The equilibrium constant expressed in terms of molar concentrations of reactants and products at equilibrium. |
| Kp | The equilibrium constant expressed in terms of partial pressures of gaseous reactants and products at equilibrium. |
| law of mass action | The principle that the equilibrium expression for a reversible reaction is the ratio of the concentrations (or partial pressures) of products to reactants, each raised to the power of their stoichiometric coefficients. |
| partial pressure | The pressure exerted by a single gas in a mixture of gases, used in equilibrium expressions for gas-phase reactions. |
| reaction quotient | A value calculated using the same expression as the equilibrium constant but using current (non-equilibrium) concentrations or partial pressures. |
| reversible reaction | A chemical reaction that can proceed in both the forward and reverse directions, with reactants forming products and products reforming reactants. |
| Term | Definition |
|---|---|
| concentrations at equilibrium | The molar amounts of reactants and products per unit volume when a reversible reaction reaches equilibrium and no net change occurs. |
| equilibrium constant expression | A mathematical expression that relates the concentrations or partial pressures of products and reactants at equilibrium, with each raised to the power of its stoichiometric coefficient. |
| Kc | The equilibrium constant expressed in terms of molar concentrations of reactants and products at equilibrium. |
| Kp | The equilibrium constant expressed in terms of partial pressures of gaseous reactants and products at equilibrium. |
| partial pressures | The individual pressure exerted by each gas in a mixture of gases at equilibrium. |
| Term | Definition |
|---|---|
| chemical species | A distinct chemical entity such as an atom, molecule, or ion that participates in a chemical reaction. |
| equilibrium concentrations | The concentrations of reactants and products when a reversible reaction reaches equilibrium and no further net change occurs. |
| equilibrium constant | A numerical value that expresses the ratio of products to reactants at equilibrium, indicating the extent to which a reaction proceeds. |
| proceeds to completion | A reaction that converts essentially all reactants to products, occurring when the equilibrium constant is very large. |
| Term | Definition |
|---|---|
| equilibrium constant | A numerical value that expresses the ratio of products to reactants at equilibrium, indicating the extent to which a reaction proceeds. |
| multistep process | A reaction mechanism consisting of two or more elementary steps that combine to produce an overall reaction. |
| overall equilibrium expression | The equilibrium constant expression for the net reaction obtained by adding multiple elementary steps together. |
| reaction quotient | A value calculated using the same expression as the equilibrium constant but using current (non-equilibrium) concentrations or partial pressures. |
| stoichiometric coefficients | The numerical coefficients in a balanced chemical equation that indicate the relative proportions of reactants and products. |
| Term | Definition |
|---|---|
| balanced reaction | A chemical equation in which the number of atoms of each element is equal on both sides of the equation. |
| chemical species | A distinct chemical entity such as an atom, molecule, or ion that participates in a chemical reaction. |
| concentration | The amount of solute dissolved in a given volume of solution, typically expressed in molarity or other units of amount per volume. |
| dynamic equilibrium | A state of equilibrium in which forward and reverse reactions continue to occur at equal rates, maintaining constant macroscopic properties. |
| equilibrium | The state in which the forward and reverse reaction rates are equal, resulting in constant concentrations or partial pressures of reactants and products. |
| equilibrium constant | A numerical value that expresses the ratio of products to reactants at equilibrium, indicating the extent to which a reaction proceeds. |
| forward reaction | The reaction pathway in which reactants are converted to products. |
| initial conditions | The starting concentrations or partial pressures of reactants and products before a reaction reaches equilibrium. |
| net consumption | The overall decrease in the amount of a substance as a result of a chemical reaction. |
| partial pressures | The individual pressure exerted by each gas in a mixture of gases at equilibrium. |
| reaction quotient | A value calculated using the same expression as the equilibrium constant but using current (non-equilibrium) concentrations or partial pressures. |
| reverse reaction | The reaction that proceeds from products back to reactants, opposite to the direction written in the balanced chemical equation. |
| Term | Definition |
|---|---|
| equilibrium | The state in which the forward and reverse reaction rates are equal, resulting in constant concentrations or partial pressures of reactants and products. |
| equilibrium constant | A numerical value that expresses the ratio of products to reactants at equilibrium, indicating the extent to which a reaction proceeds. |
| particulate model | A representation of matter showing individual atoms, molecules, or ions and their interactions to describe chemical processes at the molecular level. |
| product | Substances formed as a result of a chemical reaction. |
| reactant | Substances that are consumed in a chemical reaction to form products. |
| reversible reaction | A chemical reaction that can proceed in both the forward and reverse directions, with reactants forming products and products reforming reactants. |
| Term | Definition |
|---|---|
| chemical species | A distinct chemical entity such as an atom, molecule, or ion that participates in a chemical reaction. |
| dilution | The process of decreasing the concentration of a solute in a solution by adding solvent, which can shift equilibrium position. |
| equilibrium | The state in which the forward and reverse reaction rates are equal, resulting in constant concentrations or partial pressures of reactants and products. |
| external stress | A change applied to a system at equilibrium, such as addition or removal of a chemical species, temperature change, pressure change, or dilution. |
| Le Châtelier's principle | A principle stating that when a system at equilibrium is disturbed, the system shifts to counteract the disturbance and re-establish equilibrium. |
| pH | A logarithmic scale used to express the concentration of hydronium ions in a solution, calculated as −log[H3O+]. |
| pressure | The force exerted by gas molecules; changes in pressure of a gas-phase system can shift the equilibrium position. |
| temperature | A factor that influences reaction rate by affecting the kinetic energy and collision frequency of reactant molecules. |
| volume | The space occupied by a system; changes in volume of a gas-phase system can shift equilibrium position. |