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4.6: Key Terms

Last updated

Aug 26, 2023
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- 4.5: Quantitative Chemical Analysis
- 4.7: Key Equations

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Example and Directions
Words (or words that have the same definition)	The definition is case sensitive	(Optional) Image to display with the definition [Not displayed in Glossary, only in pop-up on pages]	(Optional) Caption for Image	(Optional) External or Internal Link	(Optional) Source for Definition
(Eg. "Genetic, Hereditary, DNA ...")	(Eg. "Relating to genes or heredity")		The infamous double helix	https://bio.libretexts.org/	CC-BY-SA; Delmar Larsen

Glossary Entries
Word(s)	Definition	Image	Caption	Link	Source
acid	substance that produces H₃O⁺ when dissolved in water
acid-base reaction	reaction involving the transfer of a hydrogen ion between reactant species
actual yield	amount of product formed in a reaction
analyte	chemical species of interest
balanced equation	chemical equation with equal numbers of atoms for each element in the reactant and product
base	substance that produces OH⁻ when dissolved in water
buret	device used for the precise delivery of variable liquid volumes, such as in a titration analysis
chemical equation	symbolic representation of a chemical reaction
coefficient	number placed in front of symbols or formulas in a chemical equation to indicate their relative amount
combustion analysis	gravimetric technique used to determine the elemental composition of a compound via the collection and weighing of its gaseous combustion products
combustion reaction	vigorous redox reaction producing significant amounts of energy in the form of heat and, sometimes, light
complete ionic equation	chemical equation in which all dissolved ionic reactants and products, including spectator ions, are explicitly represented by formulas for their dissociated ions
end point	measured volume of titrant solution that yields the change in sample solution appearance or other property expected for stoichiometric equivalence (see equivalence point)
equivalence point	volume of titrant solution required to react completely with the analyte in a titration analysis; provides a stoichiometric amount of titrant for the sample’s analyte according to the titration reaction
excess reactant	reactant present in an amount greater than required by the reaction stoichiometry
gravimetric analysis	quantitative chemical analysis method involving the separation of an analyte from a sample by a physical or chemical process and subsequent mass measurements of the analyte, reaction product, and/or sample
half-reaction	an equation that shows whether each reactant loses or gains electrons in a reaction.
indicator	substance added to the sample in a titration analysis to permit visual detection of the end point
insoluble	of relatively low solubility; dissolving only to a slight extent
limiting reactant	reactant present in an amount lower than required by the reaction stoichiometry, thus limiting the amount of product generated
molecular equation	chemical equation in which all reactants and products are represented as neutral substances
net ionic equation	chemical equation in which only those dissolved ionic reactants and products that undergo a chemical or physical change are represented (excludes spectator ions)
neutralization reaction	reaction between an acid and a base to produce salt and water
oxidation	process in which an element’s oxidation number is increased by loss of electrons
oxidation number	(also, oxidation state) the charge each atom of an element would have in a compound if the compound were ionic
oxidation-reduction reaction	(also, redox reaction) reaction involving a change in oxidation number for one or more reactant elements
oxidizing agent	(also, oxidant) substance that brings about the oxidation of another substance, and in the process becomes reduced
percent yield	measure of the efficiency of a reaction, expressed as a percentage of the theoretical yield
precipitate	insoluble product that forms from reaction of soluble reactants
precipitation reaction	reaction that produces one or more insoluble products; when reactants are ionic compounds, sometimes called double-displacement or metathesis
product	substance formed by a chemical or physical change; shown on the right side of the arrow in a chemical equation
quantitative analysis	the determination of the amount or concentration of a substance in a sample
reactant	substance undergoing a chemical or physical change; shown on the left side of the arrow in a chemical equation
reducing agent	(also, reductant) substance that brings about the reduction of another substance, and in the process becomes oxidized
reduction	process in which an element’s oxidation number is decreased by gain of electrons
salt	ionic compound that can be formed by the reaction of an acid with a base that contains a cation and an anion other than hydroxide or oxide
single-displacement reaction	(also, replacement) redox reaction involving the oxidation of an elemental substance by an ionic species
solubility	the extent to which a substance may be dissolved in water, or any solvent
soluble	of relatively high solubility; dissolving to a relatively large extent
spectator ion	ion that does not undergo a chemical or physical change during a reaction, but its presence is required to maintain charge neutrality
stoichiometric factor	ratio of coefficients in a balanced chemical equation, used in computations relating amounts of reactants and products
stoichiometry	relationships between the amounts of reactants and products of a chemical reaction
strong acid	acid that reacts completely when dissolved in water to yield hydronium ions
strong base	base that reacts completely when dissolved in water to yield hydroxide ions
theoretical yield	amount of product that may be produced from a given amount of reactant(s) according to the reaction stoichiometry
titrant	solution containing a known concentration of substance that will react with the analyte in a titration analysis
titration analysis	quantitative chemical analysis method that involves measuring the volume of a reactant solution required to completely react with the analyte in a sample
weak acid	acid that reacts only to a slight extent when dissolved in water to yield hydronium ions
weak base	base that reacts only to a slight extent when dissolved in water to yield hydroxide ions

acid | substance that produces H₃O⁺ when dissolved in water

acid-base reaction | reaction involving the transfer of a hydrogen ion between reactant species

actual yield | amount of product formed in a reaction

analyte | chemical species of interest

balanced equation | chemical equation with equal numbers of atoms for each element in the reactant and product

base | substance that produces OH⁻ when dissolved in water

buret | device used for the precise delivery of variable liquid volumes, such as in a titration analysis

chemical equation | symbolic representation of a chemical reaction

coefficient | number placed in front of symbols or formulas in a chemical equation to indicate their relative amount

combustion analysis | gravimetric technique used to determine the elemental composition of a compound via the collection and weighing of its gaseous combustion products

combustion reaction | vigorous redox reaction producing significant amounts of energy in the form of heat and, sometimes, light

complete ionic equation | chemical equation in which all dissolved ionic reactants and products, including spectator ions, are explicitly represented by formulas for their dissociated ions

end point | measured volume of titrant solution that yields the change in sample solution appearance or other property expected for stoichiometric equivalence (see equivalence point)

equivalence point | volume of titrant solution required to react completely with the analyte in a titration analysis; provides a stoichiometric amount of titrant for the sample’s analyte according to the titration reaction

excess reactant | reactant present in an amount greater than required by the reaction stoichiometry

gravimetric analysis | quantitative chemical analysis method involving the separation of an analyte from a sample by a physical or chemical process and subsequent mass measurements of the analyte, reaction product, and/or sample

half-reaction | an equation that shows whether each reactant loses or gains electrons in a reaction.

indicator | substance added to the sample in a titration analysis to permit visual detection of the end point

insoluble | of relatively low solubility; dissolving only to a slight extent

limiting reactant | reactant present in an amount lower than required by the reaction stoichiometry, thus limiting the amount of product generated

molecular equation | chemical equation in which all reactants and products are represented as neutral substances

net ionic equation | chemical equation in which only those dissolved ionic reactants and products that undergo a chemical or physical change are represented (excludes spectator ions)

neutralization reaction | reaction between an acid and a base to produce salt and water

oxidation | process in which an element’s oxidation number is increased by loss of electrons

oxidation number | (also, oxidation state) the charge each atom of an element would have in a compound if the compound were ionic

oxidation-reduction reaction | (also, redox reaction) reaction involving a change in oxidation number for one or more reactant elements

oxidizing agent | (also, oxidant) substance that brings about the oxidation of another substance, and in the process becomes reduced

percent yield | measure of the efficiency of a reaction, expressed as a percentage of the theoretical yield

precipitate | insoluble product that forms from reaction of soluble reactants

precipitation reaction | reaction that produces one or more insoluble products; when reactants are ionic compounds, sometimes called double-displacement or metathesis

product | substance formed by a chemical or physical change; shown on the right side of the arrow in a chemical equation

quantitative analysis | the determination of the amount or concentration of a substance in a sample

reactant | substance undergoing a chemical or physical change; shown on the left side of the arrow in a chemical equation

reducing agent | (also, reductant) substance that brings about the reduction of another substance, and in the process becomes oxidized

reduction | process in which an element’s oxidation number is decreased by gain of electrons

salt | ionic compound that can be formed by the reaction of an acid with a base that contains a cation and an anion other than hydroxide or oxide

single-displacement reaction | (also, replacement) redox reaction involving the oxidation of an elemental substance by an ionic species

solubility | the extent to which a substance may be dissolved in water, or any solvent

soluble | of relatively high solubility; dissolving to a relatively large extent

spectator ion | ion that does not undergo a chemical or physical change during a reaction, but its presence is required to maintain charge neutrality

stoichiometric factor | ratio of coefficients in a balanced chemical equation, used in computations relating amounts of reactants and products

stoichiometry | relationships between the amounts of reactants and products of a chemical reaction

strong acid | acid that reacts completely when dissolved in water to yield hydronium ions

strong base | base that reacts completely when dissolved in water to yield hydroxide ions

theoretical yield | amount of product that may be produced from a given amount of reactant(s) according to the reaction stoichiometry

titrant | solution containing a known concentration of substance that will react with the analyte in a titration analysis

titration analysis | quantitative chemical analysis method that involves measuring the volume of a reactant solution required to completely react with the analyte in a sample

weak acid | acid that reacts only to a slight extent when dissolved in water to yield hydronium ions

weak base | base that reacts only to a slight extent when dissolved in water to yield hydroxide ions

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