A) \[{{K}_{3}}[Fe{{(OH)}_{6}}]\]
B) \[{{K}_{2}}[Fe{{O}_{4}}]\]
C) \[FeS{{O}_{4}}{{(N{{H}_{4}})}_{2}}S{{O}_{4}}\cdot 6{{H}_{2}}O\]
D) \[{{[Fe{{(CN)}_{6}}]}^{3-}}\]
Correct Answer: C
Solution :
The oxidation state of \[Fe\]in\[{{K}_{3}}[Fe)OH{{)}_{6}})\]is \[3(+1)+x+6(-1)=0\] \[3+x-6=0\] \[x-3=0\] \[x=+3\] The oxidation state of Fe in \[{{K}_{2}}[Fe{{O}_{4}})\] is \[2(+1)+x+4(-2)=0\] \[2+x-8=0\] \[x=+2\] The oxidation state of \[Fe\] in\[FeS{{O}_{4}}\cdot {{(N{{H}_{4}})}_{2}}S{{O}_{4}}\cdot 6{{H}_{2}}O\]is \[x+(-2)+2(+1)+(-2)=0\] \[x-2+2-2=0\] \[x=+2\] The oxidation state of \[Fe\] in\[{{[Fe{{(CN)}_{6}}]}^{3-}}\]is \[x+6(-1)=-3\] \[x=-3+6\] \[x=+3\] Thus \[FeS{{O}_{4}}\cdot {{(N{{H}_{4}})}_{2}}S{{O}_{4}}\cdot 6{{H}_{2}}O\] has least oxidation state of\[Fe\].
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