Titration, often referred to as titrimetry, is a volumetric analysis used to measure the analyte concentration in a sample solution. In which the two steps performed are called standardization and titration.
Standardization is the process of calculating the exact concentration of the prepared solution. Titration is the process of calculating an unknown sample concentration. Standardization is often done in the form of titrations.
It consists of a burette filled with titrant and a pipette that is used to pour the titrand into the conical flask where the reaction takes place.
Until the reaction is complete, i.e., the chemical equivalence point or endpoint, a titrant of a known concentration is applied. To indicate the endpoint, a chemical compound called an indicator is used.
Why do we standardize a solution?
It is required to standardize the solution/reagent before starting an experiment since it allows us to obtain accurate measurements during the experiment; On the other hand, the exact concentration of the solution may differ.
You can also reduce the deviation of instrumental and random human errors by standardizing the solution.
As a result, it's necessary to standardize and measure the actual concentration right at the start of the titration.
Example of standardization in chemistry:
Standardization of sodium hydroxide (NaOH) using potassium hydrogen phthalate (C8H5KO4) or oxalic acid dihydrate (C2H2O4). In which KHP/oxalic acid solution is used as a primary standard.
If you prepare the 0.1N NaOH solution, however, its actual concentration is not actual 0.1N therefore we need to standardize it to determine its exact concentration.
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