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?
There is no precipitate for the reaction; all products are soluble.
Precipitate: silver sulfate
Net lonic: 2Ag+ + SO42- --> Ag2SO4
Precipitate: sodium nitrate
Net lonic: Na2+ + 2NO3 --> Na(NO3)2
Precipitate: silver sulfate
Net lonic: Ag+ + SO42- --> AgSO4
Precipitate: sodium nitrate
Net lonic: Na+ + NO3 --> NaNO3

Precipitate is silver sulfate and the net ionic equation is

2Ag⁺(aq) + SO₄²⁻(aq) → Ag₂SO₄(s)

Explanation:

The given reaction is the reaction of sodium sulfate with silver nitrate and as the reaction goes we will get the precipitate of Silver sulfate and the balanced reaction is given as,

Na₂SO₄ + 2 AgNO₃→ Ag₂SO₄↓ +  2 NaNO₃

Here silver sulfate is obtained as a precipitate.

Net ionic equation is the equation in which the ions involved in the reaction only taken into account that is ions forming precipitate, whereas the other ions are considered as spectator ions, ions do not involved in the reaction.

Here the net ionic equation is:

2Ag⁺(aq) + SO₄²⁻(aq) → Ag₂SO₄(s)

a

explanation:

1 a

2 d

3 a

4 c

explanation: