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If you are looking at a iodide to iodine redox titration, the solution would turn yellow instead of blue/black. The blue/black color of the iodine-starch complex is very intense and so the end-point is sharper. Without the starch, the endpoint, when the first yellow from the formation of iodine I2, appears, is less sharp and is harder to see.
it give sharp end point for coloured soln. even for those that are precipitate out in other volumetric titration
Iodometry, also 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.
The indicator is used to measure the end point of titration. Methyl red and phenolphthalein are frequently used indicators in acid-base titration. Potassium permanganate can used as a self indicator in redox titrations where applicable.
to determine the end point of titration
it give sharp end point for coloured soln. even for those that are precipitate out in other volumetric titration
If you are looking at a iodide to iodine redox titration, the solution would turn yellow instead of blue/black. The blue/black color of the iodine-starch complex is very intense and so the end-point is sharper. Without the starch, the endpoint, when the first yellow from the formation of iodine I2, appears, is less sharp and is harder to see.
Iodometry, also 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.
The indicator is used to measure the end point of titration. Methyl red and phenolphthalein are frequently used indicators in acid-base titration. Potassium permanganate can used as a self indicator in redox titrations where applicable.
Cu2I2 is precipitates in light pink colour due to adsorption of I2 and the precipitate releases I2 very slowly. Therefore very small amount of potassium thiocyanate is added towards the end point which helps to displace the adsorbed I2 quickly by combining with Cu2I2 to form CuSCN which has less tendency to adsorb I2.
to determine the end point of titration
during a titration when a titrant completely furnished the sample then this is the end point of titration.
neutralization of reaction or completion of titration
Titration in which the end point is marked by a color change.
indicates end of titration neutralisation of the reaction
Because the end point can easily be observed. Example: consider the titration between potassium manganate (IV) which is purple and ammonium iron (II) sulfate - colourless. At the end point the colourless standard solution will turn pale pink when the correct volume of deep purple titre is added. No indicator is required. Also this is not necessarily an acid base rxn
Titration error is simply the difference between the end point of a titration and the equivalence point of it. It can mathematically defined as Error = Vol(End Point) - Vol(Equivalence Point)