Using Equilibrium Constants

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Reversible Reaction Noun

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[ri-vur-suh-buhl ree-ak-shuhn]

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Reversible Reaction

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A chemical reaction that can proceed in both the forward and reverse directions, allowing products to reform into reactants.

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Example: Reactants A and B combine to form products C and D, while products C and D also react to re-form A and B, as shown by the double arrow.

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Chemical Equilibrium Noun

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[kem-i-kuhl ee-kwuh-lib-ree-uhm]

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Chemical Equilibrium

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The state in a reversible reaction where the rate of the forward reaction equals the rate of the reverse reaction.

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Example: This graph shows that in a chemical reaction, reactants decrease and products increase until their concentrations stop changing, reaching a state of chemical equilibrium.

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Equilibrium Constant (Keq) Noun

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[ee-kwuh-lib-ree-uhm kon-stuhnt]

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Equilibrium Constant (Keq)

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A value representing the ratio of product concentrations to reactant concentrations at equilibrium for a specific temperature.

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Example: This image shows the formula for the equilibrium constant (Kc), which compares the amount of products to reactants in a chemical reaction at equilibrium.

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Homogeneous Equilibrium Noun

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[hoh-muh-jee-nee-uhs ee-kwuh-lib-ree-uhm]

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Homogeneous Equilibrium

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An equilibrium state in which all participating reactants and products exist in the same single physical state or phase.

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Example: This graph shows that as a reaction proceeds over time, the amount of reactants decreases while the amount of products increases, until they both become constant at equilibrium.

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Heterogeneous Equilibrium Noun

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[het-er-uh-jee-nee-uhs ee-kwuh-lib-ree-uhm]

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Heterogeneous Equilibrium

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An equilibrium state where the reactants and products are present in more than one physical state or phase.

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Example: Heating solid iodine crystals causes them to turn into a gas (sublimation), which then cools and turns back into solid crystals, showing an equilibrium between different phases.

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Le Châtelier's Principle Noun

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[luh shah-tuh-lyeyz prin-suh-puhl]

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Le Châtelier's Principle

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A principle stating that if a stress is applied to a system at equilibrium, the system shifts to counteract it.

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Example: This flowchart shows that when a stress disturbs a chemical equilibrium, the reaction shifts forward (if QK) to counteract the stress.

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Acclimatization Noun

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[uh-klahy-muh-tahy-zey-shuhn]

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Acclimatization

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The physiological process of an organism adjusting to a gradual change in its environment, such as a change in altitude.

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Example: This image compares three different spellings of a word—Acclimate, Acclimatize, and Acclimatise—rather than explaining the scientific process of acclimatization.

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Sparingly Soluble Adjective

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[spair-ing-lee sol-yuh-buhl]

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Sparingly Soluble

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A term describing an ionic compound that dissolves only to a very small extent in a given solvent.

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Example: An ionic solid (lattice of cations and anions) dissolves only slightly in water, with most of the solid remaining undissolved at equilibrium.

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Saturated Solution Noun

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[sach-uh-rey-tid suh-loo-shuhn]

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Saturated Solution

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A solution containing the maximum amount of a solute that can be dissolved at a specific temperature and pressure.

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Example: The middle beaker shows a saturated solution, where the liquid has dissolved the maximum amount of sugar, and any extra sugar remains undissolved at the bottom.

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Solubility Product Constant (Ksp) Noun

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[sol-yuh-bil-i-tee prod-uhkt kon-stuhnt]

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Solubility Product Constant (Ksp)

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The equilibrium constant for a solid substance dissolving in a solvent, representing the product of dissolved ion concentrations.

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Example: This image shows the general chemical equation for how a solid (MxNy) dissolves into ions (M and N) and the formula for its Ksp.