The total change in the oxidation state of manganese involved in the reaction of $KMnO_4$ and potassium iodide in the acidic medium is $..........$.

In the balanced chemical equation $MnO_4^- + Br^- + H_2O \to MnO_2 + BrO_3^- + OH^-$,the coefficients of $MnO_4^-$,$BrO_3^-$,and $OH^-$ are respectively:

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$MnO_2 + 2NaCl + 2H_2SO_4 \longrightarrow MnSO_4 + Na_2SO_4 + 2H_2O + Cl_2 \uparrow$

The reaction,$3 ClO^{-} \rightarrow ClO_3^{-} + 2 Cl^{-}$ occurs in two steps:
$i.$ $2 ClO^{-} \rightarrow ClO_2^{-} + Cl^{-}$
$ii.$ $ClO_2^{-} + ClO^{-} \rightarrow ClO_3^{-} + Cl^{-}$
The reaction intermediate is:

Assuming complete ionisation,same moles of which of the following compounds will require the least amount of acidified $KMnO_4$ for complete oxidation?

Consider a titration of potassium dichromate solution with acidified Mohr's salt solution using diphenylamine as indicator. The number of moles of Mohr's salt required per mole of dichromate is