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Answer: Iodometry and iodimetry are two of the most frequent titration procedures used in analytical chemistry, as we all know. Because these titrations are based on oxidation reduction, they can be used to quantitatively quantify redox species. We also know that titrations are based on a reaction between the analyte and the titrant, a standard reagent. Because of its propensity to react quickly with a wide range of species, iodine can be employed in redox titrations.
Let’s look at the basic definitions of iodometric and iodimetric titrations, as well as the differences between them:-
Iodometric titrations are performed when an analyte (an oxidising agent) is added to excess iodide to produce iodine, and the amount of iodine produced is evaluated by titration with sodium thiosulfate solution.
Iodimetric titrations are performed when an analyte (a reducing agent) is titrated directly with a standard iodine solution.
The following are the differences between iodometric and iodimetric titration:-
When utilising iodine and iodide in iodometric reactions, keep in mind that their reversibility is an advantage. To answer these types of problems, you should also strive to comprehend all types of titrations used in inorganic, organic, and analytical chemistry.
| Iodometric Titrations | iodimetric Titrations |
| It is an indirect titration approach, unlike iodometry. | It is a method of direct titration. |
| The total number of redox reactions is two in this case. | The number of redox reactions is one in this case. |
| The iodine will be oxidised first, and subsequently reduced by the reducing agent. | Iodine will be lowered in this area. |
| It’s used to calculate the amount of oxidising agents in the environment. | It’s used to measure the amount of reducing agents in a solution. |
