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acid
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substance that produces H
3
O
+
when dissolved in water
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acid-base reaction
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reaction involving the transfer of a hydrogen ion between reactant species
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actual yield
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amount of product formed in a reaction
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analyte
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chemical species of interest
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balanced equation
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chemical equation with equal numbers of atoms for each element in the reactant and product
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base
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substance that produces OH
−
when dissolved in water
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buret
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device used for the precise delivery of variable liquid volumes, such as in a titration analysis
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chemical equation
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symbolic representation of a chemical reaction
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coefficient
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number placed in front of symbols or formulas in a chemical equation to indicate their relative amount
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combustion analysis
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gravimetric technique used to determine the elemental composition of a compound via the collection and weighing of its gaseous combustion products
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combustion reaction
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vigorous redox reaction producing significant amounts of energy in the form of heat and, sometimes, light
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complete ionic equation
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chemical equation in which all dissolved ionic reactants and products, including spectator ions, are explicitly represented by formulas for their dissociated ions
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end point
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measured volume of titrant solution that yields the change in sample solution appearance or other property expected for stoichiometric equivalence (see
equivalence point
)
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equivalence point
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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
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excess reactant
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reactant present in an amount greater than required by the reaction stoichiometry
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gravimetric analysis
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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
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half-reaction
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an equation that shows whether each reactant loses or gains electrons in a reaction.
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indicator
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substance added to the sample in a titration analysis to permit visual detection of the end point
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insoluble
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of relatively low solubility; dissolving only to a slight extent
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limiting reactant
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reactant present in an amount lower than required by the reaction stoichiometry, thus limiting the amount of product generated
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molecular equation
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chemical equation in which all reactants and products are represented as neutral substances
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net ionic equation
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chemical equation in which only those dissolved ionic reactants and products that undergo a chemical or physical change are represented (excludes spectator ions)
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neutralization reaction
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reaction between an acid and a base to produce salt and water
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oxidation
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process in which an element’s oxidation number is increased by loss of electrons
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oxidation number
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(also, oxidation state) the charge each atom of an element would have in a compound if the compound were ionic
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oxidation-reduction reaction
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(also, redox reaction) reaction involving a change in oxidation number for one or more reactant elements
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oxidizing agent
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(also, oxidant) substance that brings about the oxidation of another substance, and in the process becomes reduced
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percent yield
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measure of the efficiency of a reaction, expressed as a percentage of the theoretical yield
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precipitate
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insoluble product that forms from reaction of soluble reactants
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precipitation reaction
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reaction that produces one or more insoluble products; when reactants are ionic compounds, sometimes called double-displacement or metathesis
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product
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substance formed by a chemical or physical change; shown on the right side of the arrow in a chemical equation
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quantitative analysis
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the determination of the amount or concentration of a substance in a sample
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reactant
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substance undergoing a chemical or physical change; shown on the left side of the arrow in a chemical equation
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reducing agent
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(also, reductant) substance that brings about the reduction of another substance, and in the process becomes oxidized
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reduction
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process in which an element’s oxidation number is decreased by gain of electrons
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salt
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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
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single-displacement reaction
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(also, replacement) redox reaction involving the oxidation of an elemental substance by an ionic species
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solubility
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the extent to which a substance may be dissolved in water, or any solvent
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soluble
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of relatively high solubility; dissolving to a relatively large extent
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spectator ion
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ion that does not undergo a chemical or physical change during a reaction, but its presence is required to maintain charge neutrality
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stoichiometric factor
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ratio of coefficients in a balanced chemical equation, used in computations relating amounts of reactants and products
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stoichiometry
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relationships between the amounts of reactants and products of a chemical reaction
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strong acid
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acid that reacts completely when dissolved in water to yield hydronium ions
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strong base
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base that reacts completely when dissolved in water to yield hydroxide ions
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theoretical yield
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amount of product that may be produced from a given amount of reactant(s) according to the reaction stoichiometry
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titrant
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solution containing a known concentration of substance that will react with the analyte in a titration analysis
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titration analysis
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quantitative chemical analysis method that involves measuring the volume of a reactant solution required to completely react with the analyte in a sample
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weak acid
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acid that reacts only to a slight extent when dissolved in water to yield hydronium ions
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weak base
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base that reacts only to a slight extent when dissolved in water to yield hydroxide ions
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