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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Acid and Ioddimetry Anhydrides These are compounds that themselves are not acids or base, but when dissolved in water produce an acid or base by reacting with. Examples include the determination of copper IIchlorateHydrogen peroxideand dissolved oxygen:. About project SlidePlayer Terms of Service.

Difference Between Iodometry and Iodimetry

Then we have dichromatometric redox titrations where the titrant is K2Cr2O7 Potassium dichromate. Application of Iodometry In the food industry, iodometry is widely used to determine the concentration of hydroperoxides iodkmetry any given lipid matrix oils and fats for human consumption.

Types of Chemical Reactions. To summarise the main information about iodimetric and iodometric titrations: The reducing agent used does not necessarily need to be thiosulfate; stannous chloridesulfitessulfidesarsenic IIIand antimony III salts are commonly used alternatives. Published by Juliana Lynch Modified over 3 years ago. Iodometry is commonly used to analyze the concentration of oxidizing agents in water samples, such as oxygen saturation in ecological studies or active chlorine in swimming pool water analysis.


Difference Between Iodometry and Iodimetry l Iodometry vs Iodimetry

When iodide is added to a solution of hexacyanoferrate IIIthe following equilibrium exists:. Oxidation is a chemical process which is catalysed by various iodoketry presence of oxygen, levels of unsaturation in the oil, presence of metals, temperature and leads to the formation of hydroperoxides. Under strongly acidic solution, the above equilibrium lies far to the right hand side, but is reversed in almost neutral solution.

Important considerations Iodometric titration needs to be done in a weak acid environment which is why we need to remember that: Pre-treatment of the sample.

Safety in the laboratory 4. However, it is more common to use Iodometric methods for analysis rather than Iodimetric methods. We divide these titrations into two types. Oxidation reduction titration The turning point indicates that all the iodine released has been titrated.

A direct titration with only 1 reaction: Iodine I2 Iodometric titrations: In the presence of iodine, the thiosulphate ions oxidise quantitatively to the iodmetry ions. This is the main difference between Iodometry and Iodimetry.

Istituto comprensivo di Tubirgo. Usually, we use a standard thiosulphate solution for this.



Neutralisation titration – part two Due to the oxidizing agents present in the water body, the Iodide ions get oxidized to Iodine, while the oxidizing agents get reduced. Introduction to iodometric and iodimetric titrations There are a lot of redox titrations classified according to the titrant used.

In the presence of I- ions the starch solution is colourless. The total sulphur dioxide in the wine sample is determined through direct iodimetric titration using starch as the indicator. The most important thing in this presentation is for you to understand the differences between iodometric and iodimetric titrations. GEASS ; erlenmeyer flask, source: This makes analysis of hexacyanoferrate III troublesome as the iodide and thiosulfate decomposes in strongly acidic medium.

Iodimetry The term iodimetry, on the other hand, refers to titration using an iodine solution and is useful for determining substances that have reducing properties. Sulfites and hydrogensulfites reduce iodine readily in acidic medium to iodide.