In nitroprusside ion, the iron and `NO` exist as `Fe(II)` and `NO^(+)` rather than `Fe^(III)` and `NO`. These forms can be differentiated by

Options

A. Estimating the concentration of iron
B. Measuring the concentration of `CN^(-)`
C. Measuring the solid state magnetic moment
D. Thermally decomposing the compound

Answer

C

Explanation

The existence of `Fe^(2+)` and `NO^(+)` in Nitroprusside ion `[Fe(CN)_(5)NO]^(2-)` can be establised by measuring the magnetic moment of the solid compound which should corresponded to `(Fe^(2+)=3d^(6))` four unpaired electrons.