How do we represent the oxidation of $"bismuth metal"$ by the action of $"nitric acid"$ to give $"bismuth nitrate"$ , and $NO(g)$ ?

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Answer 1 · 2017-08-25T06:03:35

You are oxidizing $"bismuth metal"$ to $"bismuth(III) nitrate"$ .......

Bismuth metal is oxidized to $Bi^(3+)$ :

$BirarrBi^(3+) + 3e^-$ $(i)$

Nitrate, $stackrel(+V)NO_3^-$ , is reduced to $stackrel(+II)NO$ :

$NO_3^(-) + 4H^(+) + 3e^(-) rarrNO + 2H_2O$ $(ii)$

Charge and mass are balanced in both equations, and we take $(i) + (ii)$

$Bi+ NO_3^(-) + 4H^(+) rarr Bi^(3+) + NO + 2H_2O$

Is this balanced?

Else....we add $3xxNO_3^-$ to each side to get......

$Bi + 4HNO_3 rarr3Bi(NO_3)_3 +NOuarr+2H_2O$

How do we represent the oxidation of "bismuth metal""bismuth metal" by the action of "nitric acid""nitric acid" to give "bismuth nitrate""bismuth nitrate", and NO(g)NO(g)?