I understand most of what I am supposed to be doing, but there are a few things that stand out. I will post the whole problem, just so I don't accidentally leave something critical out.
A 1.00 liter solution is made up of .23M ammonia and .25M Ammonium Chloride. If .12 moles of HBr is added to the system...(and it goes on to name T/F questions.)
Chemical Equation: NH
3+H
2O
NH
4+ + OH
-I need help understanding a few concepts as to why certain parts be as they are.
In one explanation, the homework states "The equilibrium H3O will increase, because [OH] = Kb[NH3] / [NH4+]. Since the concentration of NH3 decreased and the concentration of [NH4+] increased, the concentration [OH-] at equilibrium is lower.[/b]
Why is it that they have written the equation as [Reactants] / [Products] instead of vice versa? I have yet to go over this in class, it is on my online homework. But, I have no idea where this came about.
Can anyone lend me some of your insight on this subject, It would be greatly appreciated.
-Thank you, Vicktor.