Analytical Chemistry - Titration and Titrimetric Methods

A complete set of vocabulary flashcards covering key definitions, titration methods, standards, indicators, apparatus setups, and historical context from the Analytical Chemistry lecture notes.

Titration

The overall analytical procedure for determining the stoichiometric or equivalence point of a reaction between an analyte and a standard reagent.

Titrant

The solution added or reagent generated in a titration, which has a known concentration and reproducible stoichiometry.

Titrand

The solution to which the titrant is added, containing the analyte of unknown concentration.

Equivalence point

The point in a titration when the amount of added standard reagent is chemically equivalent to the amount of analyte in the sample.

End point

A point in the progress of a reaction precisely located by an observable physical change, such as a color change, signaling that the titration is complete.

Indicator

A reagent or device added to the analyte solution to produce an observable physical change at or near the equivalence point.

Primary standard

An ultrapure compound that serves as the reference material for a titration or for another type of quantitative analysis.

Secondary standard

A compound whose purity has been determined by chemical analysis, serving as the working standard material for titrations.

Standard solution

A reagent of known concentration used in titrations and many other chemical analyses.

Volumetric titration

A titration method that involves measuring the volume of a solution of known concentration needed to react completely with the analyte.

Gravimetric titration

A titration method in which the mass of the reagent is measured instead of its volume.

Coulometric titration

A titration method in which the reagent is a constant direct electrical current of known magnitude that consumes the analyte.

Back-titration

A process in which an excess of a standard solution used to consume an analyte is determined by titrating with a second standard solution, often used when the reaction rate is slow or the standard solution lacks stability.

Quantitative analysis

Chemical analysis aimed at determining the amount or concentration of a specific substance present in a sample.

Titrimetry

A group of quantitative analytical procedures based on measuring the amount of a reagent of known concentration consumed by an analyte in a chemical or electrochemical reaction.

18th-Century Vinegar Analysis

A historical quantitative method where vinegar concentration was determined by measuring the amount of potassium carbonate ($K_2CO_3$) added until bubbling of acetic acid ceased.

Phenolphthalein pH Behavior

An acid-base indicator that appears orange at $pH < 0$, colorless in acidic/neutral solutions ($0 < pH < 8$), light pink in slightly basic solutions ($8 < pH < 12$), and fades to colorless in strongly basic solutions ($pH > 12$).

Titration Apparatus Setup

A standard laboratory assembly for titration consisting of a burette, burette clamp and stand, stopcock, and Erlenmeyer flask containing the solution of analyte with indicator.

Equivalence Point vs Endpoint Comparison

A direct comparison where equivalence point is the theoretical end of the reaction, whereas endpoint is the experimental point signaled by a color change.

pH Indicator Transition Ranges

A chart displaying the specific pH ranges and associated color changes for common chemical indicators used in titrations.