Opening the book…
- Acids: Substances that increase the concentration of hydrogen ions (H⁺) or hydronium ions (H₃O⁺) in aqueous solution.
- Bases: Substances that increase the concentration of hydroxide ions (OH⁻) or accept hydrogen ions (H⁺) in aqueous solution.
- Litmus: a water-soluble mixture of different dyes extracted from lichens. It is often absorbed onto filter paper to produce one of the oldest forms of pH indicator, used to test materials for acidity
- Salts: Ionic compounds formed from the neutralization reaction between an acid and a base.
- Binary Acids: Acids composed of hydrogen and one other nonmetal element, such as HCl or HF.
- Oxyanion: A negatively charged polyatomic ion that contains oxygen and another element, often a nonmetal.
- Neutralize: To react an acid and a base to produce water and a salt, typically bringing the solution closer to a neutral pH.
- Proton: A positively charged subatomic particle found in the nucleus of an atom, and often used to refer to a hydrogen ion (H⁺) in acid-base chemistry.
- Ionizable: Describes a substance that can dissociate in solution to produce ions.
- Hydronium ion: The H₃O⁺ ion formed when a hydrogen ion (H⁺) associates with a water molecule in solution.
- Solvents: The component of a solution that is present in the greatest amount and dissolves the solute.
- Mono-protic: An acid that can donate only one proton (H⁺) per molecule.
- Di-protic: An acid that can donate two protons (H⁺) per molecule.
- Tri-protic: An acid that can donate three protons (H⁺) per molecule.
- Conjugate Acid: The species formed when a base gains a hydrogen ion (H⁺).
- Conjugate Base: The species formed when an acid loses a hydrogen ion (H⁺).
- Conjugate acid-base pair: Two species that differ by one proton, such as H₂O and OH⁻ or NH₄⁺ and NH₃.
- Amphoteric: A substance that can act as either an acid or a base depending on the chemical environment.
- Amphiprotic: A substance that can both donate and accept a proton (H⁺), a type of amphoteric behavior.
- Autoionization of Water: The process by which water molecules spontaneously produce equal concentrations of H₃O⁺ and OH⁻ ions.
- Acid Strength: A measure of how completely an acid dissociates into ions in solution.
- Strong Acid: An acid that completely dissociates into hydrogen ions and its conjugate base in aqueous solution.
- Strong Base: A base that completely dissociates into hydroxide ions and its cation in aqueous solution.
- Weak Acid: An acid that only partially dissociates in solution, existing in equilibrium with its conjugate base.
- Weak Base: A base that only partially accepts protons or produces hydroxide ions in solution.
- Chemical Equilibrium: A state in which the forward and reverse reactions occur at equal rates, and the concentrations of reactants and products remain constant.
- Dynamic Equilibrium: A condition where reactions continue to occur in both directions, but with no net change in concentrations.
- Acid Dissociation Constant: A value that quantifies the extent to which an acid dissociates in solution.
- Base Dissociation Constant: A value that quantifies the extent to which a base accepts protons or generates OH⁻ in solution.
- pH Scale: A logarithmic scale used to express the acidity or basicity of a solution, ranging from 0 (very acidic) to 14 (very basic), with 7 being neutral.
- Acid-Base Titration: A laboratory technique used to determine the concentration of an acid or base by reacting it with a base or acid of known concentration.
- Analyte: The unknown solution in a titration whose concentration is being determined.
- Standard: A solution of known concentration used in titration to react with the analyte.
- Equivalence Point: The point in a titration at which the number of moles of acid equals the number of moles of base.
- End Point: The observable point in a titration, often indicated by a color change, that signals the equivalence point has been reached or passed.
- Buffers: Solutions that resist significant changes in pH when small amounts of acid or base are added, typically made from a weak acid and its conjugate base.
- Buffer Capacity: The amount of acid or base a buffer can neutralize before a significant change in pH occurs.
This page titled 11.9: Key Terms was last modified on Wed, 03 Sep 2025 08:15:58 GMT and is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by Burçak Artun, Gorkem Ermut, and Semere Bairu.
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