Use the three criteria for double displacement reactions, and the solubility tab

Question

Use the three criteria for double displacement reactions, and the solubility table, predict whether a double displacement reaction will occur for each of the following. If the reaction will occur, balance the reaction write conventional, total ionic and net ionic equations. Box the net ionic equation. Be sure to include the proper phase labels. If no reaction will occur, write "no reaction". All reactants are aqueous solutions. Potassium sulfide and copper (II) sulfate rightarrow Aqueous ammonia and oxalic acid rightarrow Potassium hydroxide and ammonium chloride rightarrow

Explanation / Answer

a)
NH3 + H2O --> NH4OH
this is aqueous ammonia

(COOH)2 + 2NH4OH ---> (COONH4)2 + 2H2O


Ionic
H+ + OH- --> H2O

note, any acid being neutralised by a base simplifies to this same ionic equation.

b)

Balanced equation

CuSO4(Aq) + K2S(Aq) ------> CuS(S) + K2SO4(Aq)

Balanced net ionic equation below!

Cu2+(Aq) + SO42(Aq) + K+(Aq) + S2(Aq) ----------> CuS + K+(Aq) + S2(Aq)

Cu2+(Aq) + S2-(Aq) -----------> CuS(S)

c)
NH4Cl(aq) + KOH(aq) --> NH4OH(aq) + KCl(aq)

It would be more accurate to write the equation as ...
NH4Cl(aq) + KOH(aq) --> NH3(aq) + H2O(l) + KCl(aq)

That's because there are no molecules of NH4OH in aqueous solution. For instance, in a bottle labeled "ammonium hydroxide" there are no molecules of ammonium hydroxide. Instead there are lots of ammonia molecules dissolved in water and a very few ammonium ions and hydroxide ions.
NH3(aq) + HOH(l) <==> NH4+ + OH- ........ Kb = 1.8x10^-5
As you can see from the value of Kb, the equilibrium lies far to the left, meaning that there will be very few NH4+ ions and OH- ion.

The net ionic equation is
NH4+ + OH- --> NH3 + HOH(l)

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