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Understanding Precipitation Reactions and Net Ionic Equations

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imelda-compton
9 diapositives · 235 Views · Nov 05, 2014

This overview addresses the principles of precipitation reactions, focusing on solubility rules that dictate the formation of insoluble compounds when two aqueous solutions are mixed. Key rules include that most salts containing sodium, potassium, and ammonium ions are soluble, while many sulfides, carbonates, and phosphates are usually not. A practical example illustrates how silver nitrate reacts with sodium chloride, resulting in the formation of insoluble silver chloride. The section emphasizes the importance of identifying spectator ions and determining net ionic equations for precipitates.

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  1. And Net Ionic Equations Precipitation

  2. Precipitation • When two solutions are mixed, a combination of ions may occur and the resulting compound may be only slightly soluble (insoluble) • General rules of solubility may be given (but be aware these are GENERAL)

  3. Solubility Rules (Water) • Most solutions with sodium, potassium or ammonium ions are soluble • Most nitrates, acetates and chlorates are soluble • Most chlorides are soluble (except silver, mercury (I) and lead). Lead (II) chloride soluble in hot water • Most sulfates soluble (except barium, strontium and lead)

  4. Solubility Rules Continued • Most carbonates, phosphates and silicates are insoluble (except sodium, potassium or ammonium) • Most sulfides are insoluble (except calcium, strontium, sodium, potassium or ammonium)

  5. Precipitation • Use solubility rules to predict what happens when two solutions are mixed • Example: silver nitrate solution mixed with sodium chloride solution • AgNO3 → Ag+ + NO3- • NaCl → Na+ + Cl- • New compounds would be AgCl and NaNO3 • AgCl is insoluble, NaNO3 is soluble

  6. Net Ionic Equation • Net ionic equation involves ONLY those ions that form the insoluble precipitate • First write the overall reaction • Determine which substance (if any) is precipitate • Ions that do not form precipitate are spectator ions and are not included in net ionic equation • Net ionic equation includes only non-spectator ions and preciptated compounds

  7. Sample Problem 14-2 • What precipitate forms when aqueous solutions of zinc nitrate and ammonium sulfide are mixed. • Zn(NO3)2(aq) + (NH4)2S(aq) → 2NH4NO3(?) + ZnS(?) • Ammonium nitrate is soluble • Spectator ions are ammonium and nitrate • Zinc sulfide is not soluble • Ions that form precipitate are zinc and sulfide

  8. Sample problem 14-2 continued • Zn(NO3)2(aq) + (NH4)2S(aq) → 2NH4NO3(aq) + ZnS(s) • Net ionic equation: Zn+2(aq) + S-2(aq) → ZnS(s)

  9. Now you do it! • Read pages 427-430 • Do practice problems 1-4 page 430