Introduction to Acid-Base Titration

Vocabulary flashcards covering the fundamentals of acid-base titration, primary standards, and standardization procedures based on the Analytical Chemistry for Engineers Laboratory lecture.

Titration

A technique where a solution of a known concentration (usually the titrant) is used to determine the concentration of the analyte in a sample.

Analytical Signal

The volume of the titrant required to completely react with the analyte in a titration process.

Titrant

The solution that is placed in a burette during titration.

Indicator

A colored substance whose change in color signals the end of the titration process (end point).

Equivalence point

The theoretical point in a titration where $mol_{titrant} = mol_{analyte}$.

End point

The point in titration where the indicator has changed color, signaling the end of the titration process, which usually requires the addition of a small excess of the titrant.

Primary Standard

A highly purified compound that serves as a reference material in volumetric and mass titrimetric methods.

Standard solution

A solution with a known concentration used in titrimetric analysis.

Standardization

The process of establishing accurately the concentration of the titrant, usually expressed in molarity ($M = \frac{mol}{V(L)}$).

Potassium hydrogen phthalate (KHP)

A primary standard ($HKC_8H_4O_4$) with a molecular weight of $204.22\,g/mol$ used to standardize bases like $NaOH$.

Sodium carbonate ($Na_2CO_3$)

The primary standard used for titrating acids such as $HCl$.

Ideal standard solution

A solution that is stable, reacts rapidly and completely with the analyte, and undergoes a selective reaction described by a balanced equation.

Vinegar

A sour liquid made by fermenting substances containing sugar (like fruit or wine), which serves as a dilute solution of acetic acid in water.

Phenolphthalein

An indicator used in the experiment whose end point is signified by the tinge of lightest pink color.

Stoichiometric Relationship

The quantitative relationship between reactants and products in a balanced chemical equation, such as $1\,mol$ of $NaOH$ reacting with $1\,mol$ of $HCl$.