The document discusses iodometric and iodimetric titrations, which are analytical chemistry methods used to determine concentrations of unknown solutions. Iodometry involves indirect titration to estimate oxidizing agents, while iodimetry involves direct titration to quantify reducing agents. The document also highlights various applications of these methods, particularly in determining sulfites, hydrogensulfites, sulfides, and hydrogensulfides.

1. Iodometric &
Iodimetric
Titration

2. CONTENT
• Titration
• Types of Titration
• Redox titration
• Iodometry
• Iodimetry
• Difference between
iodometric and iodimetric
titration
• Analytical applications
on Idometric and
Iodimetric titration
• Conclusion

3. Titration
A titration is technique where a solution of known concentration
is used to determine the concentration of unknown solution.
A solution whose concentration is known is called as
standard solution
The solution whose concentration is unknown is called as
sample solution

4. Types of Titration
• Acid-base titration
• Redox titration
• Gas-phase titration
• Complexometric titration
• Zeta potential titration
• Assay

5. Redox titration
A redox reaction involves an oxidation and reduction reaction between the analyte
and the titrant.
There are a lot of redox titrations classified according to the titrant used:
1) Permanganimetric: Titrant KMnO4
2) Dichromatometric: Titrant K2Cr2O7
3) Titrations involving iodine (I2)
• Iodimetry
• Iodometry

6. IODOMETRY
Iodometry: Not a direct titration because there are 2 reactions:
analyte + I- → I2
unknown
I2 + titrant (standard thiosulfate) → product
Known
The method is called iodometry when a solute (oxidizing
agent) is added to excess iodide to obtain iodine, and the
amount of iodine produced is estimated by titration with a
sodium thiosulfate solution.

7. Iodimetry
Prod
uct
A
solution .
Iodimetry: A direct titration with only 1 reaction:
analyte + titrant (iodine I2) → product
(iodide I-)
unknown known
Iodimetry is a method for titrating a compound
(reducing agent) directly with a standard iodine
solution .

8. Difference between iodometric and iodimetric
titration
Iodometric titration Iodimetric titration
Iodimetric titration is an indirect
titration method.
Iodometric titration is a direct
titration method.
Two redox reactions occur in this
titration.
One redox reaction occurs in this
titration.
It is used to quantify the oxidizing
agent.
It is used to quantify the reducing
agent.

9. Analytical applications on Idometric and Iodimetric titration
There are too many applications of iodometry and iodimetry . Some of them are:
1. Determination of Sulfites and hydrogensulfites :
Sulfites and hydrogensulfites reduce iodine readily in acidic medium to
iodide
SO3
2- + I2 + H2O= SO4
2- +2H+ +2I-
HSO3
- + I2 + H2O= SO4
2- +3H+ +2I-

10. 2.Determination of Sulfides and hydrogensulfides :
The excess arsenic trioxide is then determined by titrating against standard
iodine solution using starch indicator
As2O3 + 3H2S=As2S3 + 3H2O
Analytical applications on Idometric and Iodimetric titration

11. Conclusion
Although the names iodometry and iodimetry seem
similar, they represent two distinct analytical chemistry
methods. The main distinction between iodometry and
iodimetry is that iodometry may be used to measure oxidising
agents whereas iodimetry can be used to measure reducing
agents.

12. THANK YOU