[Bryby]

Hi. I just started an internship at a wastewater treatment plant. They treat the water with mono-chloramine (NH₂Cl to kill organisms. Then they have to remove that to meet EPA discharge standards. They use sodium bisulfite (NaHSO₃. I get the following two equations.
NH₂Cl + H₂O <-> NH₃ + HOCL
NaHSO₃ + HOCL <->NaHSO₄ + HCL

HCl + NH₃ -> NH₄Cl

But what happens with the NaHSO₄ and the NH₄Cl? My understanding is that HSO₄- is amphiprotic while NH₄Cl is acidic. HSO₄- would therefor act like a base. HSO₄ + NH₃Cl.... but this doesnt seem to get me any closer to the answer, or maybe it does. How far does this reaction go? Am i doing it right? I want to know the final products of this reaction and understand it in the entirety. Please help.

Thanks,
Bryby

[Borek]

This is an equilibrium question - to solve that you need all Ka values and all concentrations. You will find outline of the general approach that should be used here:

http://www.chembuddy.com/?left=pH-calculation&right=general-pH-calculation

You may also try pH calculator built in Buffer Maker, this will give you final answer much faster.

[Bryby]

Borek, i just want to find out if this equation boils down to harmless molecules. I think it would be easier for me to understand things in a chemical equation without amounts and Ka values. I just want to get to the end result of the basic equation. Unfortunately i am stuck with NH₄Cl and NaHSO₄. Do they react with anything that i am missing, or with each other or not at all? 

[Borek]

Do they react with anything that i am missing, or with each other or not at all?

There will be no other reaction between these molecules than the acid/base equilibrium.