Write an equation for the acid–base reaction between ammonium ion and sulfate ion.
a. why does the equillibrium favor the reactants?
This was my answer
NH3+H2O--><--(NH4)2SO4
NH3 is ammonia.
NH4+ is the ammonium ion.
Note that your equation has no S on the reactant side; therefore, you can't produce S on the right.
The question is sparse on details. Is this aqueous solution, gas phase reaction, or what? And what makes it an acid/base reaction?
2NH4^+(aq) + SO4^2-(aq) ==> (NH4)2SO4(aq)
The equation you provided, NH3 + H2O <--> (NH4)2SO4, is incorrect because it does not represent an acid-base reaction between ammonium ion (NH4+) and sulfate ion (SO42-).
To accurately write the equation, we need to understand the acid-base properties of ammonium ion and sulfate ion.
1. Ammonium ion (NH4+) is an acid because it can donate a proton (H+ ion).
2. Sulfate ion (SO42-) is a base because it can accept a proton (H+ ion).
So the correct equation for the acid-base reaction between ammonium ion and sulfate ion is:
NH4+ + SO42- --> H2SO4 + NH3
In this equation, ammonium ion (NH4+) donates a proton (H+) to sulfate ion (SO42-), resulting in the formation of sulfuric acid (H2SO4) and ammonia (NH3).
Now, let's address the second part of your question: Why does the equilibrium favor the reactants?
Acid-base reactions can reach a state of equilibrium, meaning that the forward and reverse reactions occur at equal rates. In this case, the equilibrium between ammonium ion and sulfate ion lies predominantly on the side of the reactants (NH4+ and SO42-).
The reason for this is related to the relative strength of the acids and bases involved. Ammonium ion (NH4+) is a weak acid, while sulfate ion (SO42-) is a strong base. Weak acids tend to have weaker tendencies to donate a proton compared to strong acids, and strong bases have a stronger tendency to accept protons. So, in this reaction, the weak acid (NH4+) and strong base (SO42-) tend to favor the formation of the weak acid and strong base species rather than the formation of the strong acid (H2SO4) and weak base (NH3).
Therefore, the equilibrium position of the reaction lies more towards the reactants, resulting in a higher concentration of ammonium ion (NH4+) and sulfate ion (SO42-).