In neutral or faintly alkaline medium,$KMnO_4$ being a powerful oxidant can oxidize thiosulphate almost quantitatively to sulphate. In this reaction,the overall change in the oxidation state of manganese will be:
- A$5$
- B$1$
- C$0$
- D$3$
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Explain why the colour of $KMnO_4$ disappears when oxalic acid is added to its solution in acidic medium.
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View SolutionThe following reaction occurs in acidic medium: $KMnO_4 + 8 H^{+} + 5 e^{-} \longrightarrow K^{+} + Mn^{2+} + 4 H_2O$. What is the equivalent weight of $KMnO_4$? (Molecular weight of $KMnO_4 = 158$)
The oxidation state of chromium in the final product formed in the reaction between $KI$ and acidified $K_{2}Cr_{2}O_{7}$ solution is:
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View SolutionThe values of coefficients to balance the following reaction are
$Cr(OH)_3 + ClO^{-} + OH^{-} \to CrO_4^{2-} + Cl^{-} + H_2O$
Find the coefficients for $Cr(OH)_3$,$ClO^{-}$,$CrO_4^{2-}$,and $Cl^{-}$ respectively.
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Find the coefficients for $Cr(OH)_3$,$ClO^{-}$,$CrO_4^{2-}$,and $Cl^{-}$ respectively.
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View SolutionThe equivalent weight of $MnSO_4$ is half of its molecular weight when it is converted to
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