A) \[{{K}_{2}}[Cu{{(CN)}_{4}}]\]
B) \[[{{K}_{2}}{{[CuCn)}_{4}}]\]
C) \[CuC{{N}_{2}}\]
D) \[Cu[K\,\,Cu{{(CN)}_{4}}]\]
Correct Answer: B
Solution :
\[CuS{{O}_{4}}\]reacts with \[KCN\] gives a white precipitate of cuprous cyanide and cyanogen gas. The cuprous cyanide dissolves in excess of \[KCN\] forming\[{{K}_{3}}[Cu{{(CN)}_{4}}]\]. \[CuS{{O}_{4}}+2KCN\xrightarrow{{}}{{K}_{2}}S{{O}_{4}}+Cu{{(CN)}_{2}}\] \[2Cu{{(CN)}_{2}}\xrightarrow{{}}\underset{\text{insoluble}}{\mathop{2CuCN}}\,+\underset{\text{cyanogen}}{\mathop{CN-CN}}\,\] \[CuCN+3KCN\xrightarrow{{}}{{K}_{3}}\underset{\text{soluble}}{\mathop{[Cu{{(CN)}_{4}}]}}\,\]
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