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”. involve the potentiometric titration of aqueous iodine with sodium thiosulfate the analyte (a reducing agent) reacts with iodine to produce iodide: iodimetry. Titrations Fajans Preciptation Complexometric. Fact File 1: Introduction to iodometric and iodimetric titrations. Quantitative Classical Chemical Analysis. Titrations.

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Difference Between Iodometry and Iodimetry

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

When iodide is added to a solution of hexacyanoferrate IIIthe following equilibrium exists:. Important considerations Iodometric titration needs to be done in a weak acid environment which is why we need to remember that: The most important thing in this presentation is for you to understand the differences between iodometric and iodimetric titrations.

The reaction is illustrated as the sum of the two half-reactions in fig.

Introduction to iodometric and iodimetric titrations Analytical applications: This page was last edited on 9 Septemberat Introduction to iodometric and iodimetric titrations Examples Acid-base Quantification of acetic acid in vinegar Complexometric Precipitation Redox Slide 4: 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. This is the second redox reaction and it is the reaction used for the titration.


iodimetrric In Iodimetryonly one redox reaction process takes place. In doing so, it becomes oxidized, and is therefore the electron donor in the redox. Optical methods of analysis Moreover, we can use iodine for this redox titrations due to its capability of reacting fast with many species. We can use starch as an indicator for iodometric titrations too. The key difference between iodometry and iodimetry is that we can use Iodometry to quantify oxidizing agentswhereas we can use iodimetry to quantify reducing agents.

As the names Iodometry and Iodimetry suggest, they relate to a process where Iodine is involved. Now, we are going to look at the redox titrations involving iodine.

Iodometry – Wikipedia

The analytical chemistry laboratory 3. This is the main difference between Iodometry iodimetriic Iodimetry. 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.

In Iodimetric titrations, an Iodine solution is directly titrated with a reducing solution. Iodometry is commonly employed to determine the active amount of hypochlorite in bleach responsible for the bleaching action. Does anybody remember the four types of reactions that we call fundamental analytical reactions? In acid environments the iodide is oxidised to iodine as in the reaction below: They differ in their approach. The reaction between the analyte and the titrant generates a product.

Iodine I2 Iodometric titrations: The excess arsenic trioxide is then determined by titrating against standard iodine solution using starch indicator. Introduction to iodometric and iodimetric titrations When a reducing analyte is titrated with iodine the titrantthe method is called iodimetry. Pre-treatment of the sample.


Carrying out the titration 1 Erlenmeyer flask, source: 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.

Once sulphur dioxide is added to wine it does not remain free but oxidates in part and in part combines with other molecues:.


Sodium thiosulphate needs a neutral or weak acid environment to oxidise with tetrathionate in an alkaline solution we would get sulphate oxidation. Combined sulphur dioxide is in equilibrium with the free form. Now, in order to be able to quantify the analyte, we need the analyte to react with a substance of a known concentration.

The reducing agent used does not necessarily need to be thiosulfate; stannous chloridesulfitessulfidesarsenic IIIand antimony III salts are commonly used alternatives. Introduction to iodometric and iodimetric titrations.

Note that iodometry involves indirect titration of iodine liberated by reaction with the analyte, whereas iodimetry involves direct titration using iodine as the titrant. A titration is a procedure in which volume increments of the known reagent solution-which is called the titrant- are added to the analyte until the reaction is complete.

Wikipedia ; erlenmeyer flask source: The volatility of iodine is also a source of error for the titration, this can be effectively prevented by ensuring an excess iodide is present and cooling the titration mixture. In the food industry, iodometry is widely used to determine the concentration of hydroperoxides in any given lipid matrix oils and fats for human consumption.


Some reactions involving certain reductants are reversible at certain pH, thus the pH of the sample solution should be carefully adjusted before the performing the analysis. Titratjons by Juliana Lynch Modified over 3 years ago. A definition of the word titration is: