Titration Calculator

A titration is an analytical technique in which a solution of known concentration (the titrant) is added to a solution of unknown concentration (the analyte) until the reaction is complete (the equivalence point). The amount of titrant required reveals the amount (and concentration) of analyte. Common examples: acid-base neutralization, redox titrations, precipitation titrations.

The equivalence point is the point at which moles of titrant added exactly equals the moles of analyte (adjusted for stoichiometry). For a strong acid-strong base titration, the equivalence point is pH 7. For a weak acid-strong base, it is above 7. For a weak base-strong acid, it is below 7. The equivalence point can be detected with an indicator, a pH meter, or a conductivity meter.

From stoichiometry: moles of analyte = (n_analyte/n_titrant) * M_titrant * V_titrant. Then concentration C_analyte = moles / V_analyte. For a 1:1 reaction (like NaOH + HCl): M1V1 = M2V2. For a 1:2 reaction (like H2SO4 + 2NaOH): moles H2SO4 = moles NaOH / 2.

A primary standard is a highly pure substance of known composition that can be used to prepare a solution of exactly known concentration or to standardize another solution. Properties: high purity (greater than 99.9%), non-hygroscopic, stable in air, high molar mass (to reduce weighing error). Examples: potassium hydrogen phthalate (KHP) for base standardization, sodium carbonate for acid standardization.

A back titration is used when the analyte reacts too slowly, is insoluble, or no suitable direct indicator exists. An excess of a known reagent is added to react completely with the analyte. The excess is then titrated with a second standard solution. Moles of analyte = moles of reagent added - moles of excess reagent titrated.