The Starch-Iodide complex is not very soluble in water, so the starch is added near the endpoint of an Iodine titration, when the Iodine concentration is low. This eliminates errors due to the fact that some Iodine may remain adsorbed on the complex and go undetected.
so if you add the starch indicator only right near the end point when the solution is a light yellow colour the starch shouldn't complex and go lumpy.
Too early addition might block the iodine molecules in the internal structure of the alpha-starch helix.
First this doesn't give good and sharp color change from blue to colourless, secondly some iodine may not react at all giving a wrong outcome.
Just some drops of added titrant before end point, when the solution is turning from brown to yellow, the added starch indicator will give a full purple-blue iodine-starch-complex color (should not be black!: still too much I2).
Because the blue complex formed with high concentrations of iodine is insoluble and does not re-dissolve as more thiosulfate is added.
This is far to be a rule for this titration.
An indicator shows when we have added just enough of the second reagent to react with the first. If you mean why do we add only a small amount of indicator, it is to keep the answer accurate. Some of the reagent is used changing the indicator so the answer is always slightly bigger than perfection, and the more indicator you add, the larger the error.
No, at least if it doesn't contain something he's titrating. Too much can influence the sudden change at the end point, so no indicator will 'see' it.
during the complexometric titration using edta it is very necessary to maintain the ph of the solution near about 10 so we use ammonium chloride buffer if we will not use this buffer dring the titration ph of sol. will ho lower side
An indicator reaction is always pH dependent because it involves hydrogen. During the reaction, hydrogen ions are either released or captured during the process.
Starch
It's the colour indicator you watch for during the titration.
to acidify the solution
the reason why a indicator is important in some titration is to show a change in the solution. for example as a solution runs from acidic to basic the indicator may turn a different color. but this is the reason why it is important inmost experiments.
To see where the equivalent point is
The indicator will change color as the pH changes.
Phenolphthalein indicates red for acids and blue for bases.
A double indicator is used to find the alkalinity of the water sample to prevent errors.
Usually there is no indicator needed in potassium permanganate titrations as there will be an excess of manganate ions in the conical flask, turning the solution from colourless to pale pink.
During an experiment for chemistry, if an indicator will not work due to the lack of a reactant, the reactant can be added. You must then compensate for the added amount by creating a solution of the indicator and the the same amount of the reactant. The volume required in the blank titration must then be subtracted from the other results to obtain quality results. This is an indicator blank and how it is used.
during a titration when a titrant completely furnished the sample then this is the end point of titration.
This is far to be a rule for this titration.