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#

1 Answer
Nov 14, 2016

Answer:

#3Ag(s) +NO_3^(-) +4H^(+)rarr 3Ag^(+) +NO +2H_2O#

Explanation:

As usual we write separate redox reactions:

#"Oxidation:"#

#Ag(s) rarr Ag^(+) + e^-# #(i)#

#"Reduction:"#

#NO_3^(-) +4H^(+) + 3e^(-) rarr NO +2H_2O# #(ii)#

And so, we add #3xx(i) + (ii):#

#3Ag(s) +NO_3^(-) +4H^(+)rarr 3Ag^(+) +NO +2H_2O#

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.