# What is the coefficient for H^+ when the redox equation below is balanced?

## ?Ag(s) + ?NO_3^(-)(aq) + ?H^(+)(aq) -> ?Ag^(+)(aq) + ?NO(g) + ?H_2O

Nov 14, 2016

$3 A g \left(s\right) + N {O}_{3}^{-} + 4 {H}^{+} \rightarrow 3 A {g}^{+} + N O + 2 {H}_{2} O$

#### Explanation:

As usual we write separate redox reactions:

$\text{Oxidation:}$

$A g \left(s\right) \rightarrow A {g}^{+} + {e}^{-}$ $\left(i\right)$

$\text{Reduction:}$

$N {O}_{3}^{-} + 4 {H}^{+} + 3 {e}^{-} \rightarrow N O + 2 {H}_{2} O$ $\left(i i\right)$

And so, we add $3 \times \left(i\right) + \left(i i\right) :$

$3 A g \left(s\right) + N {O}_{3}^{-} + 4 {H}^{+} \rightarrow 3 A {g}^{+} + N O + 2 {H}_{2} O$

This is balanced with respect to mass and charge, so it is reasonable.

The nitrate anion is in fact a potent oxidant; however, in aqueous solution, often its reactivity is kinetically hindered.