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.

Consider the following redox reaction taking place in acidic medium: $BH_{4}^{-}(aq) + ClO_{3}^{-}(aq) \rightarrow H_{2}BO_{3}^{-}(aq) + Cl^{-}(aq)$. If the Nernst equation for the above balanced reaction is $E_{cell} = E_{cell}^{o} - \frac{RT}{nF} \ln Q$, then the value of $n$ is . . . . . . . (Nearest integer)

Given the redox reaction:
$X Na_2HAsO_3 + Y NaBrO_3 + Z HCl \longrightarrow NaBr + H_3AsO_4 + NaCl$
The values of $X$,$Y$,and $Z$ in the balanced equation are respectively:

Assign $A$,$B$,$C$,$D$ from given type of reaction.
$Zn_{(s)} + 2HCl_{(aq)} \longrightarrow ZnCl_{2(aq)} + H_{2(g)}$

When $CrI_3$ oxidises to $Cr_2O_7^{2-}$ and $IO_4^-$,the equivalent mass of $CrI_3$ will be :-

$NaClO$ solution reacts with $H_2SO_3$ as,$NaClO + H_2SO_3 \to NaCl + H_2SO_4$. $A$ solution of $NaClO$ used in the above reaction contained $15 \ g$ of $NaClO$ per litre. The normality of the solution would be