Iodometry is an indirect titration method whereas iodimetry is a direct titration method. This is the main difference between Iodometry and. Iodometry and iodimetry are two common titration methods useful in analytical chemistry. Iodometry is the quantitative analysis of a solution of. IODIMETRIC TITRATIONS When an analyte that is a reducing agent (like hypo) is titrated directly with a standard iodine solution, the method is called “iodimetry”.

Author: Goltizil Fenrizahn
Country: Sri Lanka
Language: English (Spanish)
Genre: Travel
Published (Last): 17 August 2007
Pages: 104
PDF File Size: 14.45 Mb
ePub File Size: 4.69 Mb
ISBN: 711-7-31915-277-4
Downloads: 17565
Price: Free* [*Free Regsitration Required]
Uploader: Dizahn

Then the produced Iodine is titrated with a reducing agent such as sodium thiosulfate solution. Carrying out the titration 1 Erlenmeyer flask, source: The half-reaction is as follows: In Iodimetryonly one redox reaction process takes place. Usually, we use a standard thiosulphate iodimetrc for this. Remember, we classify titrations according to the type of reaction between the titrant and the analyte.

For this, we can titrate the mixture with a standard thiosulphate solution. Therefore, by determining the end point of the reaction, equations can be derived to obtain information of the stoichiometry and other necessary relationships between ioeimetric reducing agent and Iodine which acts as the oxidizing agent in this case.

Introduction to iodometric and iodimetric titrations When a reducing analyte is titrated with iodine the titrantthe method is called iodimetry.

Colour of the starch solution in the presence of I2.

Oxidated sulphur dioxide appears in the form of sulphur trioxide SO 3sulphuric acid or potassium bisulphate. We need to add starch as an indicator, to ipdometric the end point of this reaction.

Difference Between Iodometry and Iodimetry

The analysis that we will perform in the laboratory is the iodometric titration of cooper, which is a classical quantitative chemical analysis, a redox titration involving iodine.


And a standard titrtaion of this is used for the iodometric titrations.

Carrying out the titration 2. In Iodometric titrations, the Iodine which has been produced as a result of a previous redox reaction is been titrated with a reducing agent such as thiosulfate ions. Awarded from the Generalitat de Catalunya, Slide 1: Performing the titration Scales, source: As mentioned above, Iodometry is an indirect method.

Oxidation is uodometric chemical process which is catalysed by various factors presence of oxygen, levels of unsaturation in the oil, presence of metals, temperature and leads to the formation of hydroperoxides. Moreover, we can use iodine for this redox titrations due to its iodometrc of reacting fast with many species.

Difference Between Iodometry and Iodimetry l Iodometry vs Iodimetry

This is one difference between iodometry and iodimetry. Safety in the laboratory 4. About project SlidePlayer Terms of Service. Performing the titration cont.

Wikipedia ; erlenmeyer flask source: Introduction to iodometric and iodimetric titrations An 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: Iodine forms a deep-blue colour complex with starch and as the Iodine breaks down to Iodide ions, the colour disappears.

To make this website work, we log user data and share it with processors.

Sulphur dioxide has several important functions: GEASS ; erlenmeyer flask, source: Then we can titrate the released iodine with anx species. A direct titration with only 1 reaction: Do you remember in which titrations the titrant is in the Erlenmeyer flask? Le lezioni del Corso 1. The volatility of iodine is also a source of error iodomwtric the titration, this can be effectively prevented by ensuring an excess iodide is present and cooling the titration mixture.

Iodometric titration needs to be done in a weak acid environment which is why we need to remember that:. The titration reaction can be represented as:. Introduction This lecture is an introduction to iodometric and iodimetric titrations.



Firstly, acid-base titrations, secondly complexometric titrations, thirdly precipitation titrations and fourthly redox titrations. The triiodide ion solution is then titrated against standard thiosulfate solution to give iodide again using starch indicator:.

Thi is another of the advantages of using sulphur dioxide because it guarantees the stability of the product over time. Tiitration, it is more common to use Iodometric methods for analysis rather than Iodimetric methods.

Introduction to iodometric and iodimetric titrations Examples Acid-base Quantification of acetic acid in vinegar Complexometric Precipitation Redox Slide 4: This is performed in the presence of a starch indicator to make it easier to recognize the end point. Introduction to iodometric and iodimetric titrations There are a lot of redox titrations classified according to the titrant used.

With red wines it is difficult to see the equivalence point because their oodimetric red colour makes it difficult to perceive the colour change in the indicator. A definition of the word titration ioodometric The iodometric titration is a general method to determine the concentration of an oxidising agent in solution. Strong light, nitrite and iodometroc ions catalyzes the conversion of iodide to iodine, so these should be removed prior to the addition of iodide to the sample.

Titrations are one of the two types of Classical Quantitative Analysis.