## Redox in basic solution

Balance in basic (check my work)

NO + MnO4- ------ NO3- + MnO2

4OH- + 4H+ + NO ---- NO3- + 2H2O + 4OH-
4OH- + 4H+ + MnO4- --- MnO2 + 2H2O + 4OH-
Balanced with 5 e- on each side

2H2O + NO + MnO4- ----- NO3- + MnO2 + 8OH-

Thanks
Nautica
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 Recognitions: Gold Member Science Advisor You need help, my friend First, prepare atomic-based electron balance: $$N^{2+} \longrightarrow N^{5+} + 3e^-$$ $$Mn^{7+}+5e^- \longrightarrow Mn^{2+}$$ Then balance them. $$5N^{2+}+3Mn^{7+}\longrightarrow 5N^{5+}+3Mn^{2+}$$ You'll see that both electron counts and atom counts are balanced now. When you write the "real" ions, I mean, NO and MnO4-, you'll have to add OH- and H2O to the side with less oxygen and less hydrogen, etc.
 Cool, this is what I got 5NO + 3MNO4 = 5NO3 + 3MnO2 It appears that all are balanced. Does this look right. Thanks nautica

## Redox in basic solution

Another class mate said that the original reaction was already balanced. He said he worked through it and kept coming up with the original equation.

Could this be right??? Or does mine look fine???

Thanks
Nautica

Recognitions:
Gold Member
 Quote by nautica Cool, this is what I got 5NO + 3MNO4 = 5NO3 + 3MnO2 It appears that all are balanced. Does this look right. Thanks nautica
Well, it seems that atom counts are okay, but you've forgotten ionic counts. This is why redox reactions are hard to study.

You said that this redox should be in basic solution; so just put OH- ions to the left side. However, there is a serious error; in basic solutions, permanganate is only reduced to manganese dioxide, as you correctly wrote. So the coefficients cancel to reflect this:

$$N^{2+}+Mn^{7+}\longrightarrow N^{5+}+Mn^{4+}$$

So if we write its real forms, we'll get this one:

$$NO + KMnO_4 \longrightarrow KNO_3 + MnO_2$$