Given below are two statements:
Statement-$I$ : Heating $NaCl$ with concentrated $H_2SO_4$ and $MnO_2$ results in oxidation of $Mn$.
Statement-$II$ : Heating $NaI$ with concentrated $H_2SO_4$ and $MnO_2$ results in reduction of $Mn$.
In light of the above statements, choose the most appropriate answer from the options given below:
Statement-$I$ : Heating $NaCl$ with concentrated $H_2SO_4$ and $MnO_2$ results in oxidation of $Mn$.
Statement-$II$ : Heating $NaI$ with concentrated $H_2SO_4$ and $MnO_2$ results in reduction of $Mn$.
In light of the above statements, choose the most appropriate answer from the options given below:
- ABoth Statement-$I$ and Statement-$II$ are correct.
- BBoth Statement-$I$ and Statement-$II$ are incorrect.
- CStatement-$I$ is correct but Statement-$II$ is incorrect.
- DStatement-$I$ is incorrect but Statement-$II$ is correct.
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Similar Questions
To an acidified dichromate solution,a pinch of $Na_2O_2$ is added and shaken. What is observed?
Difficult
View SolutionIf stoichiometric quantities of a $KMnO_4$ and $K_2Cr_2O_7$ mixture are added for the oxidation of $Fe^{2+}$ to $Fe^{3+}$ in an acidic medium,then $Fe^{2+}$ will be oxidized:
Match the chemical reactions given in List-$I$ with their types given in List-$II$:
List-$I$ List-$II$ $A$. $TiCl_{4(l)} + 2Mg_{(s)} \xrightarrow{\Delta} Ti_{(s)} + 2MgCl_{2(s)}$ $I$. Disproportionation reaction $B$. $2H_2O_{2(aq)} \rightarrow 2H_2O_{(l)} + O_{2(g)}$ $II$. Metal displacement reaction $C$. $C_{(s)} + O_{2(g)} \xrightarrow{\Delta} CO_{2(g)}$ $III$. Decomposition reaction $D$. $2NaH_{(s)} \xrightarrow{\Delta} 2Na_{(s)} + H_{2(g)}$ $IV$. Combination reaction
| List-$I$ | List-$II$ |
| $A$. $TiCl_{4(l)} + 2Mg_{(s)} \xrightarrow{\Delta} Ti_{(s)} + 2MgCl_{2(s)}$ | $I$. Disproportionation reaction |
| $B$. $2H_2O_{2(aq)} \rightarrow 2H_2O_{(l)} + O_{2(g)}$ | $II$. Metal displacement reaction |
| $C$. $C_{(s)} + O_{2(g)} \xrightarrow{\Delta} CO_{2(g)}$ | $III$. Decomposition reaction |
| $D$. $2NaH_{(s)} \xrightarrow{\Delta} 2Na_{(s)} + H_{2(g)}$ | $IV$. Combination reaction |
$500$ mL of $0.2$ $M$ $MnO_4^-$ solution in basic medium when mixed with $500$ mL of $1.5$ $M$ $KI$ solution, oxidises iodide ions to liberate molecular iodine. This liberated iodine is then titrated with a standard $x$ $M$ thiosulphate solution in presence of starch. If $300$ mL of thiosulphate was consumed, then the value of $x$ is . . . . . . .
DifficultJEE MAIN 2026
View SolutionIn neutral or faintly alkaline medium,$MnO_4^{-}$ oxidizes $I^{-}$ to iodate. What is the volume (in $L$) of $0.02 \ M \ KMnO_4$ required to completely convert $1 \ L$ of $0.5 \ M \ KI$ solution to iodate in neutral or faintly alkaline medium?
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