In the following reaction, species which has been reduced is :

$Z n + 2 {O H}^{-} + 2 H_{2} O ⟶ Z n {(O H)}_{4}^{2 -} + H_{2}$

Z n

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{O H}^{-}

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H_{2} O

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none of these

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Solution

The correct option is C ${O H}^{-}$
$Z n + 2 {O H}^{-} + 2 H_{2} O ⟶ Z n {(O H)}_{4}^{2 -} + H_{2}$
0 -2+1 +1-1 +2 -2+1 0
So here, Zn oxidises and hydrogen ion reduces to hydrogen gas.

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Similar questions

Q. In the following reaction

Z n + 2 O H^{-} + 2 H_{2} O ⟶ Z n (O H)_{4}^{2 -} + H_{2}

The species which has been reduced is:

Q. The salt

Z n (O H)_{2}

is involved in the following two equilibria:

Z n (O H)_{2} (s) ⇌ Z n^{2 +} (a q) + 2 O H^{-} (a q); K_{s p} = 1.3 \times 10^{- 17}

Z n (O H)_{2} (s) + 2 O H^{-} (a q) ⇌ [Z n (O H)_{4}]^{2 -} (a q); K_{c} = 0.13

Calculate the pH of the solution at which solubility is minimum.

Q. Which of the following species are oxidised and reduced in the following (unbalanced) reaction?

C + Z n O ⟶ Z n + C O

The standard reduction potential at $25^{o} C$ of the reaction $H_{2} O + 2 e^{-} \to H_{2} + 2 O H^{-}$ is $- 0 .8277 V$ . Calculate the equilibrium constant for the reaction $2 H_{2} O \to H_{3} O^{+} + O H^{-}$ at $25^{o} C$ .

Q. At what concentration of

[O H^{-}]

does the following half reaction has a potential of

0 V

when other species are at

1 M

N O_{3}^{-} + H_{2} O + 2 e^{-} \to N O_{2}^{-} + 2 O H^{-}; E^{0} c e l l = - 0.06 V

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In the following reaction, species which has been reduced is :Zn+2OH−+2H2O⟶Zn(OH)2−4+H2

The correct option is C OH−Zn+2OH−+2H2O⟶Zn(OH)2−4+H2 0 -2+1 +1-1 +2 -2+1 0So here, Zn oxidises and hydrogen ion reduces to hydrogen gas.

In the following reaction, species which has been reduced is :

$Z n + 2 {O H}^{-} + 2 H_{2} O ⟶ Z n {(O H)}_{4}^{2 -} + H_{2}$

The correct option is C ${O H}^{-}$
$Z n + 2 {O H}^{-} + 2 H_{2} O ⟶ Z n {(O H)}_{4}^{2 -} + H_{2}$
0 -2+1 +1-1 +2 -2+1 0
So here, Zn oxidises and hydrogen ion reduces to hydrogen gas.