The key difference between iodometry and iodimetry is that we can use Iodometry to quantify oxidizing agents , whereas we can use iodimetry to quantify reducing agents. Iodometry and iodimetry are two common titration methods useful in analytical chemistry. The basis of these two types of titrations is oxidation-reduction, and we can use it to determine redox species quantitatively. The basis of titration is a reaction between the analyte and a standard reagent known as the titrant. Moreover, we can use iodine for this redox titrations due to its capability of reacting fast with many species.
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The key difference between iodometry and iodimetry is that we can use Iodometry to quantify oxidizing agents , whereas we can use iodimetry to quantify reducing agents.
Iodometry and iodimetry are two common titration methods useful in analytical chemistry. The basis of these two types of titrations is oxidation-reduction, and we can use it to determine redox species quantitatively. The basis of titration is a reaction between the analyte and a standard reagent known as the titrant. Moreover, we can use iodine for this redox titrations due to its capability of reacting fast with many species. Overview and Key Difference 2.
What is Iodometry 3. What is Iodimetry 4. In iodometry, iodides react with another oxidizing agent in an acidic medium or neutral medium. When this reaction takes place, iodide we add iodide in the form of KI oxidizes to iodine and the other species will undergo reduction by iodide. Then we can titrate the released iodine with another species. This titrating species is a standard solution of a reducing agent, which is capable of reducing iodine back to iodide form.
Usually, we use a standard thiosulphate solution for this. For example, if we want to quantify the amount of chlorine dissolved in a mixture, the following is the method to carry out an iodometric titration. First, we should take a known amount of volume from the mixture in which chlorine is dissolved into a titration flask. Then we can titrate it with a known solution of KI, and we can find the volume consumed.
Then we should carry out another titration with the same mixture to determine the released amount of iodine.
For this, we can titrate the mixture with a standard thiosulphate solution. We need to add starch as an indicator, to determine the end point of this reaction. With iodine and starch in the mixture, it will appear in dark-blue colour, but at the end point when all the iodine is finished, the dark colour will disappear. In iodimetry, it uses free iodine to undergo titration with a reducing agent.
Therefore, iodine reduces to iodide, and iodine will oxidize other species. Since we cannot easily prepare a free iodine solution, we have to mix iodine with potassium iodide and KI 3 solution to prepare the required solution.
And a standard solution of this is used for the iodometric titrations. Following reaction takes place when titrating. We can use starch as an indicator for iodometric titrations too. Iodometry is the quantitative analysis of a solution of an oxidizing agent by adding an iodide that reacts to form iodine, which is then titrated whereas iodimetry is a volumetric analysis involving either titration with a standardized solution of iodine, or the release by a substance under examination of iodine in soluble form, so that we can determine its concentration by titration.
This is one difference between iodometry and iodimetry. Furthermore, another difference between iodometry and iodimetry is that, in iodometry, iodides react with another oxidizing agent in an acidic medium or neutral medium while in iodimetry, it uses free iodine to undergo titration with a reducing agent.
Although the two terms iodometry and iodimetry sound similar, they are two different techniques we use in analytical chemistry. The key difference between iodometry and iodimetry is that we can use Iodometry to quantify oxidizing agents, whereas we can use iodimetry to quantify reducing agents.
Naviglio, Daniele. Available here. With a mind rooted firmly to basic principals of chemistry and passion for ever evolving field of industrial chemistry, she is keenly interested to be a true companion for those who seek knowledge in the subject of chemistry. Figure The Color Change in Iodometry. Figure Performing a Titration. Comments Helpful. Thank you. Leave a Reply Cancel reply.
Difference Between Iodometry and Iodimetry
As the names Iodometry and Iodimetry suggest, they relate to a process where Iodine is involved. In fact, both these terms refer to different methods of using Iodine in titrations to determine the concentration of an analyte under investigation. They differ in their approach. Iodometry is an indirect titration method whereas iodimetry is a direct titration method. This is the main difference between Iodometry and Iodimetry.
Iodometry vs. Iodimetry
Iodometry is used to determine the concentration of oxidising agents through an indirect process involving iodine as the intermediary. In the presence of iodine, the thiosulphate ions oxidise quantitatively to the tetrathionate ions. To determine the concentration of the oxidising agents, an unknown excess of potassium iodide solution is added to the weakly acid solution. The iodine, which is stoichiometrically released after reduction of the analyte, is then titrated with a standard sodium thiosulphate solution Na 2 S 2 O 3. Titration involving iodine commonly uses a starch suspension as indicator.
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Iodometry, known as iodometric titration, is a method of volumetric chemical analysis, a redox titration where the appearance or disappearance of elementary iodine indicates the end point. Note that iodometry involves indirect titration of iodine liberated by reaction with the analyte, whereas iodimetry involves direct titration using iodine as the titrant. Iodometric titration is used to find cl2 conc. Redox titration using sodium thiosulfate, Na2S2O3 usually as a reducing agent is known as iodometric titration since it is used specifically to titrate iodine. The iodometric titration is a general method to determine the concentration of an oxidising agent in solution. In an iodometric titration, a starch solution is used as an indicator since it can absorb the I2 that is released.