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Precipitation Reactions

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Presentation on theme: "Precipitation Reactions"— Presentation transcript:

1 Precipitation Reactions
& Solubility Rules

2 Precipitation Reactions
Precipitation Rxn: A reaction that produces an insoluble product, a.k.a… a precipitate Insoluble: Does NOT dissolve in water (not aqueous!) these substances are labeled (s) for solid Important to remember: (s) = SOLID = NOT SOLUBLE IN WATER!!! (aq) = AQUEOUS = SOLUBLE IN WATER!!!

3 Find the Precipitate… AgNO3(aq) + KCl(aq)  AgCl(s) + KNO3(aq)
Silver Chloride is a solid, (s). It does NOT dissolve in water—it’s a PRECIPITATE! Review From Yesterday: Can you write total and net ionic equations for this reaction?

4 Precipitation of Silver Chloride
Molecular Equation: AgNO3(aq) KCl(aq)  AgCl(s) KNO3(aq) Total Ionic Equation: Ag+(aq) + NO3-(aq) + K+(aq) + Cl-(aq)  AgCl(s) + K+(aq) + NO3-(aq) Net Ionic Equation: Ag+(aq) + Cl-(aq)  AgCl(s) Spectator Ions: NO3- & K+

5 Precipitation of Silver Chloride
Precipitate: AgCl Spectator Ions: NO3- & K+ K+ K+ NO3‾ Ag+ Cl‾ NO3‾ AgCl

6 Predicting Precipitation Reactions
How do we know whether a certain compound is aqueous or solid? (How do we know whether it is SOLUBLE or not?) We need SOLUBILITY RULES in order to: Determine if a precipitate is formed in a reaction Write correct Total and Net Ionic equations

7 Solubility Rules (Describe solubility of substances in WATER)
Notice the ions that are soluble NO MATTER WHAT they form compounds with! These ions will ALWAYS be SPECTATOR IONS!!!

8 Predicting Precipitation Reactions
Will a precipitate (s) form when solutions of Calcium Chloride and Sodium Carbonate are mixed? This is a double replacement reaction (don’t forget to balance!) CaCl2(?) + Na2CO3(?)  CaCO3(?) + 2NaCl(?)

9 Predicting Precipitation Reactions
Will a precipitate (s) form when solutions of Calcium Chloride and Sodium Carbonate are mixed? CaCl2(aq) + Na2CO3(aq)  CaCO3(s) + 2NaCl(aq) Yes! ppt = CaCO3 (Calcium Carbonate = chalk!)

10 Total Ionic and Net Ionic Equations
Now that we have labeled each substance using the SOLUBILITY RULES, we should be able to write Total Ionic and Net Ionic Equations CaCl2(aq) + Na2CO3(aq)  CaCO3(s) + 2NaCl(aq) Total Ionic: Ca+2(aq) + 2Cl- (aq) + 2Na+(aq) + CO3-2(aq)  CaCO3(s) + 2Na+(aq) + 2Cl-(aq) Net Ionic: Ca+2(aq) + CO3-2(aq)  CaCO3(s) Cl‾ Na+ Ca+2 Na+ CO3‾2 Cl‾ CaCO3

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