Ap Chem 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. Potassium sulfide and barium chloride
2. Lead (lll) nitrate and ammonium chromate
3. Sodium sulfate and lithium nitrate
4. Silver sulfate and lithium nitrate
5. Silver nitrate and sodium sulfate
6. Potassium phosphate and cobalt (ll) nitrate

Answer 1

1. Potassium sulfide and barium chloride

K₂S(aq) + BaCl₂(aq) => 2KCl(aq) + BaS(s)

net ionic: Ba²⁺(aq) + S^2-(aq) => BaS(s)

1. Lead (lll) nitrate and ammonium chromate

2Pb(NO₃)₃(aq) + 3(NH₄)₂CrO₄(aq) => Pb₂(CrO₄)₃(s) + 6NH₄NO₃(aq)

net ionic: 2Pb³⁺(aq) + 3CrO₄^2-(aq) ==> Pb₂(CrO₄)₃(s)

You should try to do the rest. If you have problems, re-submit and we'll try to help you

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