Chemistry > Stoichiometry > 8.0 Iodimetric and Iodometric Titrations
Stoichiometry
1.0 The Mole
2.0 The Limiting Reagent
3.0 Gravimetric Analysis
4.0 Volumetric Analysis
5.0 Calculation of n-factor
6.0 Redox Reactions
7.0 Titration
7.1 Simple Titration
7.2 Double Titration
7.3 Method
7.4 Titration of the solution containing both $N{a_2}C{O_3}$ and $NaHC{O_3}$
7.5 Titration of the solution containing both $NaOH$ and $N{a_2}C{O_3}$
7.6 Back Titration
8.0 Iodimetric and Iodometric Titrations
9.0 Volume strength peroxide solution
10.0 Percentage Labeling of Oleum
11.0 Hardness of Water
8.1 Iodimetric Titrations
7.2 Double Titration
7.3 Method
7.4 Titration of the solution containing both $N{a_2}C{O_3}$ and $NaHC{O_3}$
7.5 Titration of the solution containing both $NaOH$ and $N{a_2}C{O_3}$
7.6 Back Titration
Iodimetric titrations are defined as those iodine titrations in which a standard iodine solution is used as an oxidant and iodine is directly titrated against a reducing agent. Iodimetric procedures are used for the determination of strength of reducing agent like thiosulphates, sulphites, arsenites and stannous chloride etc., by titrating them against standard solution of iodine taken in a burette. Some cases of oxidation-reduction reactions are given as under:
(i) $2N{a_2}{S_2}{O_3} + {\text{ }}{I_2} \to N{a_2}{S_4}{O_6} + {\text{ }}2NaI$
(ii) $N{a_2}S{O_3} + {\text{ }}{I_2} + {\text{ }}{H_2}O \to N{a_2}S{O_4} + {\text{ }}2HI$
(iii) $N{a_3}As{O_3} + {\text{ }}{H_2}O \to N{a_3}As{O_4} + {\text{ }}2HI$
