What is the result of the reaction between $KMnO_4$ and $HCl$?
- AOxidation of $Mn$ in $KMnO_4$ and production of $Cl_2$
- BReduction of $Mn$ in $KMnO_4$ and production of $H_2$
- COxidation of $Mn$ in $KMnO_4$ and production of $H_2$
- DReduction of $Mn$ in $KMnO_4$ and production of $Cl_2$
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For the reaction $I^{-} + ClO_3^{-} + H_2SO_4 \to Cl^{-} + HSO_4^{-} + I_2$ (no free $H^{+}$ is present),select the correct statement for the balanced equation (coefficients in smallest whole number ratio).
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View Solution$MnO_4^-$ on reduction in acidic medium forms
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View Solution$A_2O_x$ is oxidised to $AO_3^-$ by $MnO_4^-$ in acidic medium. If $1.5 \times 10^{-3} \text{ mole of } A_2O_x$ requires $40 \text{ mL}$ of $0.03 \text{ M } KMnO_4$ solution in acidic medium,which of the following statement$(s)$ is/are correct?
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View SolutionDiscuss the types of redox reactions in detail.
In the balanced chemical reaction
$IO_3^- + aI^- + bH^+ \to cH_2O + dI_2$
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$IO_3^- + aI^- + bH^+ \to cH_2O + dI_2$
$a, b, c, d$ respectively correspond to
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