solubility and precipitation

Question

Consider each of the following aqueous solutions being mixed. Based on solubility rules, determine whether a reaction will occur or not. If a reaction will occur:

a. Write a complete balanced chemical equation AND net ionic equation with appropriate state symbols.

If NO precipitate is formed, write NO REACTION. You do not need to write a complete balanced equation or net ionic equation.

1. Sodium sulfate and lithium nitrate
2. Silver nitrate and sodium sulfate
3. Potassium phosphate and cobalt (ll) nitrate

Answer 1

A couple of things you must know:

1). know the charges of the polyatomic ions

2). know the general formula for a double displacement

a. AB + CD ---> AD + CB

3). know the solubility rules

1. sodium sulfate and lithium nitrate

Na₂SO₄(aq) + 2 LiNO₃(aq) ---> 2 NaNO₃(aq) + Li₂SO₄(aq) since everything is in aqueous form, no precipitate is formed and therefore, NO REACTION

1. silver nitrate and sodium sulfate

2 AgNO₃(aq) + Na₂SO₄(aq) ---> Ag₂SO₄(s) + 2 NaNO₃

complete ionic

2 Ag(aq) + 2 NO₃(aq) + 2 Na(aq) + SO₄(aq) ---> Ag₂SO₄(s) + 2 Na(aq) + 2 NO₃(aq)

now remove spectator ions by putting a line through compounds that are the exact same on the reactants and products side. Then what is left will be you net ionic equation.

net ionic

2 Ag(aq) + SO₄(aq) ---> Ag₂SO₄(s)

By now you should be able to do the last one. You can easily look up the charges for polyatomic ions and the solubility rules on the internet. Thanks!