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Question: Which of the following will give \((F{e^{3 + }})\) ions in the solution? A. \({[Fe{(CN)_6}]^{3 - }...

Which of the following will give (Fe3+)(F{e^{3 + }}) ions in the solution?
A. [Fe(CN)6]3−{[Fe{(CN)_6}]^{3 - }}
B. [Fe(CN)6]4−{[Fe{(CN)_6}]^{4 - }}
C. NH4(SO4)2.FeSO4.6H2ON{H_4}{(S{O_4})_2}.FeS{O_4}.6{H_2}O
D. Fe2(SO4)3F{e_2}{(S{O_4})_3}

Explanation

Solution

[Fe(CN)6]3−{[Fe{(CN)_6}]^{3 - }} and [Fe(CN)6]4−{[Fe{(CN)_6}]^{4 - }} are the complex ions. NH4(SO4)2.FeSO4.6H2ON{H_4}{(S{O_4})_2}.FeS{O_4}.6{H_2}O is a double salt. Fe2(SO4)3F{e_2}{(S{O_4})_3} also breaks into individual ions and will give Fe3+F{e^{3 + }} ions in the solution.

Complete step by step answer:
[Fe(CN)6]3−{[Fe{(CN)_6}]^{3 - }}, also called ferricyanide is an anion and Ferrocyanide, [Fe(CN)6]4−{[Fe{(CN)_6}]^{4 - }} are complex ions. They retain their identity in the solution. Hence, they will not give Fe3+F{e^{3 + }} ions in the solution.
Fe2++[Fe(CN)6]3−→Fe3++[Fe(CN)6]4−F{e^{2 + }} + {[Fe{(CN)_6}]^{3 - }} \to F{e^{3 + }} + {[Fe{(CN)_6}]^{4 - }}
In this reaction ferricyanide ions [Fe(CN)6]3−{[Fe{(CN)_6}]^{3 - }} oxidise iron (II) to iron (III) forming ferrocyanide ions, [Fe(CN)6]4−{[Fe{(CN)_6}]^{4 - }}
The third compound, NH4(SO4)2.FeSO4.6H2ON{H_4}{(S{O_4})_2}.FeS{O_4}.6{H_2}O or Mohr salt is a double salt. It contains only ferrous ions
In the solution, it breaks into individual ions, but it will give Fe2+F{e^{2 + }} ions in the solution.
Similarly, Fe2(SO4)3F{e_2}{(S{O_4})_3}, Ferric sulphate is a chemical compound which is a yellow coloured salt and is soluble in water. Iron (III) sulphate is most often generated as a solution rather than being isolated as a solid. It is an extremely strong acidic compound. It also breaks into individual ions. Hence, they will give Fe3+F{e^{3 + }} ions in the solution.
Hence, only Fe2(SO4)3F{e_2}{(S{O_4})_3} will give
Fe3+F{e^{3 + }} ions in the solution.

Therefore, the correct answer is option (D).

Note: Ferrocyanide, [Fe(CN)6]4−{[Fe{(CN)_6}]^{4 - }} is a diamagnetic species. Although many salts of cyanides are toxic but ferrocyanide [Fe(CN)6]4−{[Fe{(CN)_6}]^{4 - }} and ferricyanide [Fe(CN)6]3−{[Fe{(CN)_6}]^{3 - }} are less toxic because they do not release free cyanide. The treatment of ferrocyanide [Fe(CN)6]4−{[Fe{(CN)_6}]^{4 - }} and ferricyanide [Fe(CN)6]3−{[Fe{(CN)_6}]^{3 - }} salts will give an intense coloured pigment Prussian blue which is sometimes called ferric ferrocyanide [Fe(CN)6]4−{[Fe{(CN)_6}]^{4 - }} and ferrous ferricyanide [Fe(CN)6]3−{[Fe{(CN)_6}]^{3 - }}. They both cannot pass through plasma membranes.