Iodometry, also known as iodometric titration, is a method of volumetric chemical analysis, involves indirect titration of iodine liberated by reaction with the analyte, whereas iodimetry involves direct titration using iodine as the titrant. What is the Difference Between Iodometry and Iodimetry? In Iodometry two redox reactions occur. In Iodimetry, only one redox reaction process. Iodometry and Iodimetry – Download as Word Doc .doc /.docx), PDF File .pdf), Text File .txt) or read online.

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Exam 2 on Wed, Nov 3. Chapter 4Reactions in Aqueous Solutions. In this case the analyte is an oxidizing agent. Thi is another of the advantages of using sulphur dioxide because it guarantees the stability of the product over time. Although the sulfide content in sample can be determined straight forwardly as described for sulfites, the results are often poor and inaccurate.

Introduction to iodometric and iodimetric titrations When a reducing analyte is titrated with iodine the titrantthe method is called iodimetry. Wikipedia ; burette, source: Here, the Iodine reduces to Iodide ions while the thiosulfate ions get oxidized further.

Titration involving iodine commonly uses a starch suspension as indicator. In this method, excess iodimetru known amount of iodide is added to known volume of sample, in which only the active electrophilic can oxidize iodide to iodine. The iodine, which nad stoichiometrically released after reduction of the analyte, is then titrated with a standard sodium thiosulphate solution Na 2 S 2 O 3. In the presence of I- ions the starch solution is colourless.

For analysis of antimony V compounds, some tartaric acid is added to solubilize the antimony III product. As we saw in slide 2, we classify redox titrations according to the titrant which is being used. Acid and Base Anhydrides These are compounds that themselves are not acids or base, but when dissolved in water produce an acid or base by reacting with.



Wikipedia ; erlenmeyer flask source: Formula for the determination of sulphur dioxide. Principles of method Hydroperoxides in the presence of KI reduce as shown in the redox reaction below. Published by Juliana Lynch Modified over 3 years ago. Iodometry is commonly employed to determine the active amount of hypochlorite in bleach responsible for ane bleaching action.

Due to the oxidizing agents present in the water body, the Iodide ions get oxidized to Iodine, while the oxidizing agents get reduced. Overview and Key Difference 2. As you can see from the diagram, the titrant is usually delivered from a buret. Introduction to iodometric and iodimetric titrations Examples Acid-base Quantification of acetic acid in vinegar Complexometric Quantification of chloride Cl- in water Precipitation Water Hardness Calcium and magnesium Redox Quantification of hydrogen peroxide H2O2 Slide 4: To use this website, you must agree to our Privacy Policyincluding cookie policy.

Strong light, nitrite and copper ions catalyzes the iodomrtry of iodide to iodine, so these should be removed prior to the addition of iodide to the sample.

Therefore, by determining the end point of the reaction, equations can be derived to obtain information of the stoichiometry and other necessary relationships between the reducing agent and Iodine which acts as the oxidizing agent in this case.

To determine the concentration of the oxidising agents, an unknown excess of potassium iodide solution is added to the weakly acid solution.

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. For example, the reaction:. Feedback Privacy Policy Feedback. To a known volume of sample, an excess but known amount of iodide is added, which the oxidizing agent then oxidizes to iodine.


Difference Between Iodometry and Iodimetry l Iodometry vs Iodimetry

Introduction to iodometric and iodimetric titrations A reducing agent is the element or compound in a redox reaction that reduces another species. Sodium thiosulphate needs a neutral or weak acid environment to oxidise with tetrathionate in an alkaline solution we would get sulphate oxidation. This makes analysis of hexacyanoferrate III troublesome as the iodide and thiosulfate decomposes in strongly acidic medium. Introduction to iodometric and iodimetric titrations Examples Acid-base Quantification of acetic acid in vinegar Complexometric Precipitation Redox Slide 4: Safety in the laboratory.

When iodide is added to a solution of hexacyanoferrate IIIthe following equilibrium exists:.

Difference Between Iodometry and Iodimetry

In the presence of iodine, the thiosulphate ions oxidise quantitatively to the tetrathionate ions. Not a direct titration because there are 2 reactions: The analytical chemistry laboratory 3.

Introduction to iodometric and iodimetric titrations Example: Yes, we have done other redox titrations like the determination of the percent of hydrogen peroxide and other ones. This indicates the end point of the titration.

The disappearance of the deep blue color is due to the decomposition iidometry the iodine-starch clathrate marks the end point. Now, we are going to look at the redox titrations involving iodine.


For this, we can titrate the mixture anv a standard thiosulphate solution. The iodine released is titrated using sodium thiosulphate at a known concentration with a starch indicator blue colour. The reducing agent used does not necessarily need to be thiosulfate; stannous chloridesulfitessulfidesarsenic IIIand antimony III salts are commonly used alternatives.

What is Iodimetry 4.