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Balancing Redox Equations

The equivalen...

Question

The equivalent weight of $Z n {(O H)}_{2}$ in the following reaction is equal to its :
$[Z n {(O H)}_{2} + H N O_{3} \to Z n (O H) (N O_{3}) + H_{2} O]$

A

\frac{f o r m u l a w t .}{2}

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B

\frac{f o r m u l a w t .}{1}

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C

3 \times f o r m u l a w t .

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D

2 \times f o r m u l a w t .

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Solution

The correct option is B $\frac{f o r m u l a w t .}{1}$
Equivalent weight = $\frac{F o r m u l a w e i g h t}{n - f a c t o r}$ .

Now we have chemical equation as follows:

$Z n (O H)_{2} + H N O_{3} ⟶ Z n (O H) (N O_{3}) + H_{2} O$ .

Here the $Z n (O H)_{2}$ releases only one $O H^{-}$ ion in the reaction so n-factor is 1.

So, equivalent weight of $Z n (O H)_{2} = \frac{F o r m u l a w e i g h t}{n - f a c t o r} = \frac{F o r m u l a w e i g h t}{1} .$

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Similar questions

Complete the following reaction:

H N O_{3} + Z n (O H)_{2} \to

Q. Which two sets of reactants best represent the amphoteric character of

Z n {(O H)}_{2}

Z n {(O H)}_{2} (s)

{O H}^{-} (a q)

Z n {(O H)}_{2} (s)

H_{2} O (l)

Z n {(O H)}_{2} (s)

H^{+} (a q)

Z n {(O H)}_{2} (s)

{N H}_{3} (a q)

Q. The equivalent weight of

H N O_{3}

(molecular weight =

63

) in the following reaction is:

3 C u + 8 H N O_{3} \to 3 C u (N O_{3})_{2} + 2 N O + 4 H_{2} O

Q. Name the following compounds:
CaO, KNO₃, HgS, H₂O, PbSO₄, NaOH, CaCl₂, MgCO₃, CO₂, Zn(OH)₂

Z n {(O H)}_{2}

is an amphoteric hydroxide which is involved in the following two equilibria existing simultaneously in aqueous solution.

Z n {(O H)}_{2} (s) ⇌ {Z n}^{2 +} (a q) + 2 {O H}^{-} (a q)

K_{s p} = 1.2 \times 10^{- 17}

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

K_{c} = 0.12

p H

the solubility of

Z n (O H)_{2}

will be minimum?

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