The dark purple colour of $KMnO_4$ disappears in the titration with oxalic acid in acidic medium. The overall change in the oxidation number of manganese in the reaction is.

What is the equivalent weight of hydrochloric acid in the given redox reaction $MnO_2 + 4HCl \to MnCl_2 + 2H_2O + Cl_2$?
If the molar mass of hydrochloric acid is $M$.

$5H_2O_2 + XClO_2 + 2OH^- \to XCl^- + YO_2 + 6H_2O$
In the above balanced reaction,the reaction is balanced when,

$KMnO_4$ acts as an oxidising agent in acidic medium. The number of moles of $KMnO_4$ that will be needed to react with one mole of sulphide ion $(S^{2-})$ in acidic solution is . . . . . . (in $/5$)?

How many electrons are involved in the following redox reaction?
$Cr_2O_7^{2-} + Fe^{2+} + C_2O_4^{2-} \to Cr^{3+} + Fe^{3+} + CO_2$ (Unbalanced)

Which compound is formed when $H_2S$ gas is passed through an acidic solution of $KMnO_4$?