Mercuric oxide- HgO- can be analysed by reaction with iodide and then titration with an acid- HgO-4 I - - Hg I 4 2- -2 OH -then- HgO- 2 OH - - 2 H -So- if x moles HgO requires 10 moles of a dibasic acid then what is the value x -

The correct option is D 10The balanced chemical equation is, nbsp; HgO+4 I ^ +H_2O ⟶ Hg I _ 4 ^ 2 +2 OH ^ Form the above chemical equation, it can b ...

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Byju's Answer

Standard XII

Chemistry

Oxyacids of Phosphorus

Mercuric oxid...

Question

Mercuric oxide, $H g O$ , can be analysed by reaction with iodide and then titration with an acid.
$H g O + 4 I^{-} ⟶ H g I_{4}^{2 -} + 2 {O H}^{-}$
then, $H g O \equiv 2 {O H}^{-} \equiv 2 H^{+}$
So, if $x$ moles $H g O$ requires $10$ moles of a dibasic acid then what is the value $x$ .

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Solution

The correct option is D 10
The balanced chemical equation is,
$H g O + 4 I^{-} + H_{2} O ⟶ H g I_{4}^{2 -} + 2 {O H}^{-}$
Form the above chemical equation, it can be concluded that $1 mol HgO \equiv 2 mol {O H}^{-} \equiv 2 mol H^{+} \equiv 1$ mole of dibasic acid because, 1 mole of dibasic acid $H_{2} A$ gives two moles of acidic protons.
Hence, 10 moles of dibasic acid will react with 10 moles of HgO.
Thus, $x = 10$

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Similar questions

H g O

is analysed by reaction with iodine and then titrating with an acid. The equivalent mass of

H g O

is :

H_{2} O + H g O + 4 I^{-} \to H g I_{4}^{2 -} + 2 O H^{-}

Q. Consider this equilibrium, for which

Δ H < 0

H g O (s) + 4 I^{-} (a q .) + H_{2} O (l) ⇌ {H g I_{4}}^{2 -} + 2 {O H}^{-}

Which changes will increase the equilibrium concentration

{H g I_{4}}^{2 -}

I

. Increasing the mass of

H g O (s)

present

I I

. Increasing

[I^{-}]

I I I

. Adding

1 M

H C l

Q. Consider the equilibrium:

H g O (s) + 4 I^{-} (a q) + H_{2} O (l) ⇌ H g I_{4}^{2 -} (a q) + 20 H^{-} (a q)

Which changes will decrease the equilibrium concentration of

H g I_{4}^{2 -}

Q. In which of the following electrochemical cell overall cell reaction is :

H g O (s) + H_{2} (g) \to H g (ℓ) + H_{2} O (ℓ)

Q. In which of the following electrochemical cell overall cell reaction is :

H g O (s) + H_{2} (g) \to H g (l) + H_{2} O (l)

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Mercuric oxide, HgO, can be analysed by reaction with iodide and then titration with an acid.HgO+4I−⟶HgI2−4+2OH−then, HgO≡2OH−≡2H+So, if x moles HgO requires 10 moles of a dibasic acid then what is the value x .

Mercuric oxide, $H g O$ , can be analysed by reaction with iodide and then titration with an acid.
$H g O + 4 I^{-} ⟶ H g I_{4}^{2 -} + 2 {O H}^{-}$
then, $H g O \equiv 2 {O H}^{-} \equiv 2 H^{+}$
So, if $x$ moles $H g O$ requires $10$ moles of a dibasic acid then what is the value $x$ .