Question

Solutions of sodium sulfate and silver nitrate are mixed together.

On a piece of scratch paper write a fully balanced double-replacement equation for this reaction.

Using the chemical equation you wrote; which answer correctly identifies the precipitate (if there is one) and the net ionic equation for the reaction that formed the precipitate?

a
Precipitate: silver sulfate

Net Ionic: 2Ag+ + SO42- --> Ag2SO4

b
There is no precipitate for the reaction; all products are soluble.

c
Precipitate: sodium nitrate

Net Ionic: Na+ + NO3- --> NaNO3

d
Precipitate: sodium nitrate

Net Ionic: Na2+ + 2NO3- --> Na(NO3)2

e
Precipitate: silver sulfate

Net Ionic: Ag+ + SO42- --> AgSO4

Answer 1

The correct option is a) Precipitate: silver sulfate

Net Ionic: 2Ag+ + SO42 →Ag2SO4

Step-by-step explanation:

When sodium sulfate reacts with silver nitrate, the following reaction occurs:

2AgNO3 + Na2SO4 → Ag2SO4 + 2NaNO3

The NaNO3 is easily soluble in water. However, silver ions form an insoluble solid with SO4. The Ag+ in this compound will be a cation having a positive charge. The SO4- will be an anion having an negative charge.

The table with solubility rules show that the sulfates of Ag+, Ca+, Sr2+, Ba2+, Hg22+ and Pb2+ are insoluble.