Direct titration of `I_(2)` with a reducing agent is called iodimetry. If `I_(2)` is leberated by the oxidation of `I_(ɵ)` ion by a strong oxidising agent in neutral or acidic medium, the liberated `I_(2)` is then titrated with reducing agent. Iodometry is used to estimate the strngth of the oxidising agent. For example, in the estimation of `Cu^(2+)` with `S_(2)O_(3)^(2-)`
`Cu^(2+)+I^(ɵ)toCuI_(2)+I_(2)` (iodometry)
`I_(2)+S_(2)O_(3)^(2-)toS_(4)O_(6)^(2-)+I^(ɵ)` (iodimetry)
Strach is used as an indicator at the end point, which forms bluecoloured complex with `I_(3)^(ɵ)` Disappearance of blue colourindicates the end point whe free `I_(2)` in not present.
Q. In the reaction
`2CuSO_(4)+4KItoCu_(2)I_(2)+2K_(2)SO_(4)+I_(2)`
The equivalent weight of `CuSO_(4)` is
`(Mw=159.5g mol^(-1))`

Direct titration of I_(2) with a reducing agent is called iodimetry. If I_(2) is leberated by the oxidation of I_(ɵ) ion by a strong oxidising agent in neutral or acidic medium, the liberated I_(2) is then titrated with reducing agent. Iodometry is used to estimate the strngth of the oxidising agent. For example, in the estimation of Cu^(2+) with S_(2)O_(3)^(2-) Cu^(2+)+I^(ɵ)toCuI_(2)+I_(2) (iodometry) I_(2)+S_(2)O_(3)^(2-)toS_(4)O_(6)^(2-)+I^(ɵ) (iodimetry) Strach is used as an indicator at the end point, which forms bluecoloured complex with I_(3)^(ɵ) Disappearance of blue colourindicates the end point whe free I_(2) in not present. Q. The volume of KI solution used for CuSO_(4) is:

Direct titration of I_(2) with a reducing agent is called iodimetry. If I_(2) is leberated by the oxidation of I_(ɵ) ion by a strong oxidising agent in neutral or acidic medium, the liberated I_(2) is then titrated with reducing agent. Iodometry is used to estimate the strngth of the oxidising agent. For example, in the estimation of Cu^(2+) with S_(2)O_(3)^(2-) Cu^(2+)+I^(ɵ)toCuI_(2)+I_(2) (iodometry) I_(2)+S_(2)O_(3)^(2-)toS_(4)O_(6)^(2-)+I^(ɵ) (iodimetry) Strach is used as an indicator at the end point, which forms bluecoloured complex with I_(3)^(ɵ) Disappearance of blue colourindicates the end point whe free I_(2) in not present. Q. The volume of KI solution used for CuSO_(4) is:

I_(2)+S_(2)O_(3)^(2-) to I^(-)+S_(4)O_(6)^(2-)

I_(2)+S_(2)O_(3)^(2-) to I^(-)+S_(4)O_(6)^(2-)

I_(2)+S_(2)O_(3)^(2-) to I^(-)+S_(4)O_(6)^(2-)

All titration which involves the direct titration of Iodine with a reducing agent are grouped under lodimetry. Iodimetry is employed to determine the strength of reducing agent such as sodium thio sulphate I_(2) + 2Na_(2)S_(2)O_(3) rarr 2I^(-)+S_(4)O_(6)^(-) If iodine is liberated as a result of chemical reaction involving oxidation of an idodide ion by a strong oxidizing agent in neutral or acidic medium the liberated iodine is then titrated with reducing agent. This titration is called lodometry. Todometry is used to estimate the strength of oxidizing agent. For example the estimation of Cu^(++) with thiosulphate. Cu^(+ +) +I^(-) Cu_(2)I_(2)+I_(2) , I_(2) +S_(2)O_(3)^(-) rarrS_(4)O_(6)^(-) +I^(-) Starch used as indicator near the end point which form blue colour complex with I_(3)^(-) . The blue colour disappears when In the reaction, 2CuSO_(4) +4KI rarr Cu_(2)I_(2) + 2K_(2)SO_(4)+I_2 the ratio of equivalent weight of CuSO_4 to its molecular weight is:

All titration which involves the direct titration of Iodine with a reducing agent are grouped under lodimetry. Iodimetry is employed to determine the strength of reducing agent such as sodium thio sulphate I_(2) + 2Na_(2)S_(2)O_(3) rarr 2I^(-)+S_(4)O_(6)^(-) If iodine is liberated as a result of chemical reaction involving oxidation of an idodide ion by a strong oxidizing agent in neutral or acidic medium the liberated iodine is then titrated with reducing agent. This titration is called lodometry. Todometry is used to estimate the strength of oxidizing agent. For example the estimation of Cu^(++) with thiosulphate. Cu^(+ +) +I^(-) Cu_(2)I_(2)+I_(2) , I_(2) +S_(2)O_(3)^(-) rarrS_(4)O_(6)^(-) +I^(-) Starch used as indicator near the end point which form blue colour complex with I_(3)^(-) . The blue colour disappears when 10 mL of H_2O_2 solution on treatment with KI and titration of liberated I_2 required 10 mL of 1 N hypo . Thus H_2O_2 is :