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(D) In $NaNO_2$,the oxidation state of nitrogen $(N)$ is $+3$. Nitrogen can be oxidized to a higher oxidation state (e.g.,$+5$ in $NO_3^-$) and reduce

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$NaNO_2$

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(D) In $NaNO_2$,the oxidation state of nitrogen $(N)$ is $+3$. Nitrogen can be oxidized to a higher oxidation state (e.g.,$+5$ in $NO_3^-$) and reduced to a lower oxidation state (e.g.,$+2, +1, 0, -3$). Therefore,$NaNO_2$ can act as both an oxidizing agent and a reducing agent. In $NaNO_3$,$N$ is in its maximum oxidation state $(+5)$,so it acts only as an oxidizing agent. In $Na_2O_2$,oxygen is in $-1$ state,which can be oxidized to $0$ or reduced to $-2$,but $NaNO_2$ is the classic example of a compound showing dual behavior due to the intermediate oxidation state of $N$.

$A$. The equation of the polar of $(4, 3)$ with respect to $C$	$I$. $y + 5 = 0$
$B$. The equation of the tangent at $(9, -5)$ on $C$	$II$. $x = 1$
$C$. The equation of the normal at $(-7, -5)$ on $C$	$III$. $3x + 8y = 27$
$D$. The equation of the diameter passing through $(1, -5)$ and $(1, 3)$	$IV$. $x = 9$

Which of the following substances acts as both an oxidizing agent and a reducing agent?

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