How Do You Balance Zinc and Nitrate in a Basic Solution?

[KingNothing]

I don't understand this question in my chemistry book. It's not homework, I'm just studying, but I would really like to know.

What are the coefficients in front of nitrate ion and zinc when the following equation is balanced in a basic solution:

___ NO3-(aq) + ___ Zn(s) --> ___ Zn2+(aq) + ___ NO(g)?

1) 2, 5
2) 2, 3
3) 3, 4
4) 3, 2

That's the nitrate ion, zinc, zinc with a 2+ charge, and NO. Can someone explain how to do this? Also, what is the answer, so I can work backwards?

So far, it looks to me like both reactants are being oxidised, so I'm left with a big half-reaction with electrons.

 

[KingNothing]

Alright, I finally got it! As it turns out, my error the whole time was labeling H as a negative ion in my reduction reaction.