BALANCING NET IONIC EQUATIONS!

Question

anonymous · Answer

$$H ^{+}+MnO _{4}+Fe ^{2+} \rightarrow Mn ^{2+}+Fe ^{3+}+H _{2}O$$

anonymous · Answer

i have the right answer I just don't understand how

anonymous · Answer

@aaronq

aaronq · Answer

what exactly dont you understand?

anonymous · Answer

why the balanced equations gives you five iron ions on each side?

aaronq · Answer

the  charge on $MnO_4$ is -1. So it should actually be written: $MnO_4^-$

The reaction is actually a redox reaction, where Mn(VII) gains electrons to Mn(II)

this means it gained 5 electrons, these came from the iron atom.

$Fe^{2+}$ changes to $Fe^{3+}$, so each iron atom loses 1 electron.

Therefore you need 5 of them to balance the electron transfer.

anonymous · Answer

how do we know they came from the iron ion

aaronq · Answer

because in the equation the iron was oxidized. Look at the charges on them