Three different solutions of oxidising agents, i.e. K2Cr2O7,I2 and KMnO4 is titrated separately with 0.19 g of K2S2O3. The molarity of each oxidising agent is 0.1M and the reactions are as follows: i. Cr2O2−7+S2O2−3→Cr3++SO2−4 ii. I2+S2O2−3→I⊝+S4O2−6 iii. MnO⊝4+S2O2−3→MnO2+SO2−4 (Molecular weight of K2S2O3=190,K2Cr2O7=294,KMnO4=158, and I2=254gmol−1 Which of the following statements is/are correct?
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Q3
In the reaction: Mn2++S2O2−8→SO2−4+MnO−4 (acid medium), the number of moles of S2O2−8 required to oxidize 2 moles of Mn2+ is :
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Q4
The oxidation of iodide ion by perdisulphate ion is described as follows :
I⊝+S2O2−8→I⊝3+SO2−4
If the rate disappearance of S2O2−8 ions is 1.5×10−3Ms−1, the rate of formation of SO2−4ions is: