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

Chemistry
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\[Au+(NO_{3})^{ (-1)}---> NO _{2}+Au^{+2}\] 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
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
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

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Other answers:

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 :)
thank you! you helped a lot! :D
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