Term
| Acid Dissociation Constant (Ka) |
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Definition
| The ratio of the concentration of the dissociated form of an acid to the undissociated form; stronger acids have larger Ka values than weaker acids |
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Term
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Definition
| Any solution in which the hydrogen-ion concentration is greater than the hydroxide-ion concentration |
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Definition
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Definition
| A substance that can act as both an acid and a base |
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Term
| Base Dissociation Constant (Kb) |
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Definition
| The ratio of the concentration of the conjugate acid times the concentration of the hydroxide ion to the concentration of the base |
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Definition
| Any solution in which the hydroxide-ion concentration is greater than the hydro-ion concentration |
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Term
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Definition
| A solution in which the pH remains relatively constant when small amounts of acid or base are added; a buffer can be either a solution of a weak acid and the salt of a weak acid, or a solution of a weak base with the salt of a weak base |
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Definition
| A measure of the amount of acid or base that may be added to a buffer solution before a significant change in pH occurs |
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Definition
| The particle formed when a base gains a hydrogen ion; NH4+ is the conjugate acid of the base NH3 |
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Definition
| Two substances that are related by the loss or gain of a single hydrogen ion; ammonia (NH3) and the ammonium ion (NH4+) are a conjugate acid-base pair |
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Definition
| The particle that remains when an acid has donated a hydrogen ion; OH- is the conjugate base of the acid water |
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Definition
| Any acid that contains two ionizable protons (hydrogen atoms); sulfuric acid (H2SO4) is a diprotic acid |
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Definition
| The point in a titration at which the indicator changes color |
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Term
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Definition
| The point in a titration where the number of moles of hydrogen ions equals the number of moles of hydroxide ions |
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Definition
| The positive ion formed when a water molecule gains a hydrogen ion |
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Term
| Ion-product constant for water (Kw) |
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Definition
| The product of the concentrations of hydrogen ions and hydroxide ions in water; it is 1 x 10-14 at 25○C |
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Definition
| Any substance that can accept a pair of electrons to form a covalent bond |
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Definition
| Any substance that can donate a pair of electrons to form a covalent bond |
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Definition
| Any acid that contains on ionizable proton (hydrogen ion); nitric acid (HNO3) is a monoprotic acid |
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Term
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Definition
| An aqueous solution in which the concentrations of hydrogen and hydroxide ions are equal; it has a pH of 7.0 |
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Term
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Definition
| A reaction in which an acid and a base react in an aqueous solution to produce a salt and water |
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Term
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Definition
| A number used to denote the hydrogen-ion concentration, or acidity, of a solution; it is the negative logarithm of the hydrogen-ion concentration of a solution |
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Term
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Definition
| A process in which the cations or anions of a dissoviated salt accept hydrogen ions from water or donate hydrogen ions to water |
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Term
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Definition
| A term describing the reaction in which two water molecules react to produce ions |
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Term
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Definition
| A solution of known concentration used in carrying out a titration |
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Definition
| An acid that is completely (or almost completely) ionized in an aqueous solution |
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Definition
| A base that completely dissociates into metal ions and hydroxide ions in aqueous solution |
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Term
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Definition
| Process used to determine the concentration of a solution (often an acid or base) in which a solution of known concentration (the standard) is added to a measured amount of the solution of unknown concentration until an indicator signals the end point |
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Term
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Definition
| Any acid that contains three ionizable protons (hydrogen ions); phosphoric acid (H3PO4) is a triprotic acid |
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Term
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Definition
| An acid that is only slightly ionized in aqueous solution |
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Term
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Definition
| A base that reacts with water to form the hydroxide ion and the conjugate acid of the base |
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