Titration Procedure
Titration starts with the preparation of a titrant/titrator, which is a standard solution with a predetermined volume and concentration. This titrant is then allowed to react with the analyte until an endpoint or equivalence point is reached, at which point the analyte concentration can be estimated by measuring the amount of titrant consumed. Titration, on the other hand, is a stoichiometric technique used to determine a solution’s unknown concentration.
In terms of method steps, a highly exact amount of analyte is introduced to a beaker or Erlenmeyer flask. A little amount of the titrant (such as phenolphthalein) is placed beneath a calibrated burette or chemical pipetting syringe containing the indicator.
Small amounts of titrant are mixed into the analyte and indicator. This will continue until the indicator’s color changes in response to the titrant saturation threshold. At this moment, it will show that we have reached the end of the titration. Essentially, the amount of titrant present during the reaction balances the amount of analyte present.
Titration
Titration is the gradual addition of a known concentration solution (called a titrant) to a known volume of an unknown concentration solution until the reaction approaches equilibrium, which is sometimes shown by a color change. The titrant solution must satisfy the appropriate criteria to be used as a primary or secondary standard. Titration is a technique for determining the concentration of an unknown solution in a general way.