Question

How do I balance the following redox reaction in acidic solution: Au + NO3^(-1) --> NO2 + Au^(+2)

Answer 1

\[Au+(NO_{3})^{ (-1)}---> NO _{2}+Au^{+2}\] now first of all balance hydrogen and to balance hydrogen add H+ ions on both the sides or the lagging side then balance Oxygen by adding H2O on the lagging side

Answer 2

new equation would be \[Au+NO _{3}^{-1}-->NO _{2}+Au^{+2}+H _{2}O\] now as we can see that on the product side there are two extra oxygen , you have to add 2H+ ion on reactant side and rest of the elements are balanced

Answer 3

adding two H+ ion \[2H^{+}+Au+NO _{3}^{-1}-->NO _{2}+Au^{+2}+H _{2}O\] now you can see that everything is balanced , you have to balance charge, next

Answer 4

on the left side total charge is +1 and on the right side total charge is +2 but we cant add +ve ion so to balance charge we will add electron on the right side to make it equal to +1 and after that you can do it :)

Answer 5

thank you! you helped a lot! :D

Answer 6

:)