Chemistry Question: Balance the following redox reaction in acidic solution: H3PO4 + HNO2 - N204 + H3PO3?

Any help with solving this will be nice :)

Balance the following redox reaction in acidic solution: H3PO4 + HNO2 - N204 + H3PO3

Answer:
Inspection tells you that P and N are changing oxidation states.
HNO2: N has a +3 oxidation state
N2O4: N has a +4 oxidation state
N is being oxidized

H3PO4: P has a +5 oxidation state
H3PO3: P has a +3 oxidation state
P is being reduced

To keep the electron loss=electron gain, 2 N must be oxidized for each P that is reduced. Lets balance the electrons first-
H3PO4 + 2 HNO2 ---> N2O4 + H3PO3
Now only the H and O are unbalanced. We need 2 H and an O on the product side. That looks like H2O.

H3PO4 + 2 HNO2 ---> N2O4 + H3PO3 + H2O

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