Use the solubility guidelines below to determine whether a precipitation reaction will occur in the following cases. If so write a net ionic equation for the reaction

Question

1. AgNO3(aq) + NH4CI(aq)
2. Na2SO4(aq)+ MgBr2(qq)

Answer 1

1. AgNO3(aq) + NH4CI(aq)

Looking at the solubility guidelines, we see that all nitrates (NO3-) are soluble, so AgNO3 is soluble. Similarly, all chlorides (Cl-) are soluble, so NH4CI is also soluble. This means that both AgNO3 and NH4CI will dissociate in water and remain in their ionic form.

Therefore, no precipitation reaction will occur in this case.

Net ionic equation: No reaction occurs.

2. Na2SO4(aq) + MgBr2(aq)

Using the solubility guidelines, we see that sulfates (SO42-) are usually soluble, so Na2SO4 is soluble. However, magnesium bromide (MgBr2) falls under the category of Group 2 (alkaline earth metals) halides, and most group 2 halides are slightly soluble.

This means that when Na2SO4 and MgBr2 are mixed, a precipitation reaction will occur, resulting in the formation of an insoluble compound, magnesium sulfate (MgSO4).

Net ionic equation: Mg2+(aq) + SO42-(aq) -> MgSO4(s)

Answer 2

Incorrect.
Yes, both AgNO3 and NH4Cl are soluble BUT not all chlorides are soluble; i.e. AgCl is not soluble;therefore AgCl will ppt and the reaction is
AgNO3(aq) + NH4Cl(aq) ==> AgCl(s) + NH4NO3(aq)
There is no reaction for the other one BECAUSE MgSO4 and NaBr are soluble.

Answer 3

You are correct, I apologize for the mistake in my previous response.

1. AgNO3(aq) + NH4Cl(aq)

AgNO3 is soluble, but NH4Cl contains the chloride ion, which is not soluble with silver. Therefore, a precipitation reaction will occur. The insoluble compound formed is silver chloride (AgCl).

Net ionic equation: Ag+(aq) + Cl-(aq) → AgCl(s)

2. Na2SO4(aq) + MgBr2(aq)

Both Na2SO4 and MgBr2 are soluble according to the solubility guidelines. Therefore, no precipitation reaction will occur.

Net ionic equation: No reaction occurs.