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Standard X

Chemistry

Reaction of Non-Metallic Oxides with Bases

Light green C...

Question

Light green (Compound 'A') $Δ - \to$ White Residue (B) $H i g h - -- \to t e m p . C + D + E$
(i) 'D' and 'E' are two acidic gas.
(ii) 'D' is passed through $H g {C l}_{2}$ solution to give yellow ppt.
(iii) 'E' is passed through water first and then $H_{2} S$ is passed, white turbidity is obtained.
(iv) A is water-soluble and addition of $H g {C l}_{2}$ in it, white ppt is obtained but white ppt does not turn into grey on addition of excess solution of 'A'.

Yellow ppt in the above observation is:

mercuric oxide

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basic mercury (II) sulphite

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basic mercury (II) sulphate

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mercuric iodide

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Solution

The correct option is C basic mercury (II) sulphate
The yellow precipitate is due to formation of basic mercury (II) sulfate.
$S O_{3} D + H g C l_{2} + H_{2} O \to H g S O_{4} y e l l o w p r e c i p i t a t e, b a s i c m e r c u r y (I I) s u l p h a t e + 2 H C l$

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A white amorphous powder (A) when heated gives a colourless gas (B), which turns lime water milky and the residue (C) which is yellow when hot but white when cold. The residue (C) dissolves in dilute HCl and the resulting solution gives a white precipitate on addition of potassium ferrocyanide solution. (A) dissolves in dilute HCl with the evolution of a gas which is identical in all respects with (B). The solution of (A) as obtained above gives a white precipitate (D) on addition of excess of

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The correct option is C basic mercury (II) sulphateThe yellow precipitate is due to formation of basic mercury (II) sulfate.SO3D+HgCl2+H2O→HgSO4yellowprecipitate,basicmercury(II)sulphate+2HCl

The correct option is C basic mercury (II) sulphate
The yellow precipitate is due to formation of basic mercury (II) sulfate.
$S O_{3} D + H g C l_{2} + H_{2} O \to H g S O_{4} y e l l o w p r e c i p i t a t e, b a s i c m e r c u r y (I I) s u l p h a t e + 2 H C l$