Name: ____________________________________________ Period: __________ Date: __________________
Learning Target:
I can understand precipitation reactions.
Criteria for Success:
I can predict whether a precipitate will form when solutions of soluble ionic compounds are combined.
I can write net ionic equations for precipitation reactions.
Precipitation Reactions
A. A _____________________ reaction is a reaction in which _______________ ions in separate solutions are mixed
together to form an __________________ compound that settles out of solution as a ________________.
1. The insoluble compound that settles out is called a _____________________.
2. Use a reference chart of ___________________ rules to determine which compounds will form
_______________________.
Which product will form a precipitate?
(NH4)2S(aq) + Cd(NO3)2(aq) → NH4NO3(?) + CdS(?)
Net Ionic Equations
A. A _________ ______________ ____________________ includes only those compounds and ions that undergo a
___________________ change in a reaction in an aqueous solution.
1. Ions that do __________ take part in a chemical reaction and are found in solution both before and after the
reaction are ___________________ __________.
Circle the spectator ions
Zn(NO3)2(aq) + (NH4)2S(aq) → ZnS(s) + 2NH4NO3(aq)
Zn2+(aq) + 2NO31-(aq) + 2NH41+(aq) + S2-(aq) → ZnS(s) + 2NH41+(aq) + 2NO31-(aq)
B. Use the following steps to ________________ net ionic equations.
1. First, convert the chemical equation into an overall ionic equation. All _____________ ionic compounds are
shown as _________________________ ions in solution. The _____________________ are shown as solids.
2. Second, _________________ the _____________________ ions on both sides of the equation.
3. Third, write final net ionic equation without _____________________ ions.
Example
Write the net ionic equation for the following reaction:
(NH4)2S(aq) + Cd(NO3)2(aq) → 2NH4NO3(aq) + CdS(s)
1.
2.
3.
Guided/Independent Practice
Part 1: Using Solubility Rules
Directions: Predict the products in the following double displacement reactions. Use a reference chart with the
solubility rules to determine which of the products will form a precipitate. If no precipitate forms, write “none.”
1. mercury(II) chloride (aq) + potassium sulfide (aq) →
2. sodum carbonate (aq) + calcium chloride (aq) →
3. copper(II) chloride (aq) + ammonium phosphate (aq) →
4. lithium hydroxide (aq) + iron (III) nitrate (aq) →
Part 2: Writing Net Ionic Equations
Directions: Determine if a precipitate will form by mixing the aqueous solutions provided in each question. If so, write
the net ionic equation for the reaction. If no precipitate forms, write “none.”
5. Will a precipitate form if solutions of potassium sulfate and barium nitrate are combined? If so, write the net ionic
equation for the reaction.
6. Will a precipitate form if solutions of potassium nitrate and magnesium sulfate are combined? If so, write the net
ionic equation for the reaction.
7. Will a precipitate form if solutions of barium chloride and sodium sulfate are combined? If so, write the net ionic
equation for the reaction.
8. Will a precipitate form if solutions of strontium chloride and potassium sulfate are combined? If so, write the net
ionic equation for the reaction.