Long story short, iodine in the solution made earlier through a reducing agent is weakly soluble and prone to loss to the air. Therefore, let's say you are using the titration to determine concentration of the titrant, the concentration would be off from the "true" concentration because you've lost some reactants.
When an analyte that is a reducing agent is titrated directly with a standard iodine solution, the method is called "iodimetry". When an analyte that is an oxidizing agent is added to excess iodide to produce iodine, and the iodine produced is determined by titration with sodium thiosulfate, the method is called "iodometry".
Not usually. Potassium iodide is usually present in a large excess. It is usually the potassium iodate that is the limiting ingredient.
THE PROCESS IS CALLED STANDARDIZATION OR CALIBRATION. It's called titration
This is far to be a rule for this titration.
The easiest way is to add back some of the solution you were titrating. If phenolphthalein remains, it will react with the solution and change back to purple. Incidentally, phenolphthalein will always remain in the solution of the titration reaction - it changes color depending upon the pH of the solution, but the indicator itself is not affected by the titration reaction.
hypo solution used in iodometric titration is sodiumthiosulphate. Its N\10 normality of Na2S2O3.
Because the iodine is liberated, hence it is called as iodometric titration.
The end-point of the titration is more sharper if NH4CNS exist in the solution;
A thiosulfate titration is mostly carried out to determine the amount of iodine present in the solution. In these reactions, thiosulfate ion acts as the reducing agent. This types titrations are often called as 'iodometric titrations'.
It is used as indicator for the endpoint of a Iodometric (redox) titration: it gives a bluish grey to black color with very minute excess of Iodine-iodide ions (I3-)
Because starch forms a dark blue colored soluble product with free iodine, so that the appearance of color in the solution from this reaction effectively shows when all the substances in the solution that react more strongly with iodine than does starch have been consumed and the titration is finished.
· In analytical chemistry, sodium thiosulphate is used for the determination of the strength of a given solution of iodine. · Sodium thiosulphate is preferred in iodometric analysis due to the fact that sodium thiosulphate is oxidized by iodine. It is also used to determine the strength of many oxidizing agents.
Sulphuric acid helps in maintaining pH around 3-4 which further helps in liberation of iodine upon adding KI solution.
When an analyte that is a reducing agent is titrated directly with a standard iodine solution, the method is called "iodimetry". When an analyte that is an oxidizing agent is added to excess iodide to produce iodine, and the iodine produced is determined by titration with sodium thiosulfate, the method is called "iodometry".
Not usually. Potassium iodide is usually present in a large excess. It is usually the potassium iodate that is the limiting ingredient.
A Hypo Solution is used in iodometric titrations, its is basically sodiumthiosulphate (Na2S2O3)
coz the oxidation state of manganese ion changes from +7 to +4. as a result Mno2 is formed which is brown in colour hence titration colour change cannot be detected