Ionic Equations and Acid-Base Reactions

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Presentation transcript:

Ionic Equations and Acid-Base Reactions

The complete ionic equation A complete ionic equation shows all aqueous ionic compounds separated into their ions Molec. eq’n: Pb(NO3)2(aq) + 2KI(aq)  PbI2(s) + 2KNO3(aq) Comp. ionic eq’n: Net ionic eq’n:

The net ionic equation A net ionic equations shows only the compounds directly participating in the reaction Comp. ionic: Pb2+(aq) + 2NO3-(aq) + 2K+(aq) + 2I-(aq)  PbI2(s) + 2K+(aq) + 2NO3-(aq) Net ionic:

One more together Write the net ionic equation for the following reaction: BaCl2(aq) + Na2SO4(aq)  BaSO4 + 2NaCl(aq)

Try this one on your own What is the net ionic equation for the following reaction? (NH4)2SO4(aq) + CaCl2(aq)  2NH4Cl(aq) + CaSO4(s)

Acids and bases Acids produce ___ ions when dissolved in water Bases produce ___ ions when dissolved in water H+ Cl- H+ Cl- H+ Cl- Na+ Na+ OH- Na+ OH- OH-

Strong Acids and Strong Bases dissolve completely into their ions in water ______ is created when a strong acid reacts with a strong base

Chemical Reactions Double Displacement Precipitation Acid-Base Form solid Form water

Determine the net ionic equation HNO3(aq) + KOH(aq)  H2O(l) + KNO3(aq) hydrochloric acid plus sodium hydroxide 

Determine the molecular and net ionic equations

Most salts of Na+, K+, and NH4+ Soluble Slightly Soluble Insoluble Most NO3- Salts Most salts of Na+, K+, and NH4+ Most chloride salts (Cl-) and iodide and bromide salts AgCl, PbCl2, Hg2Cl2,Those containing Ag+, Hg22+, Pb2+ Most sulfate (SO42-) salts BaSO4, PbSO4, CaSO4 NaOH and KOH Most hydroxide (OH-) compounds. Ba(OH)2 and Ca(OH)2 moderately soluble Most sulfide (S2-) carbonate (CO32-) and phosphate (PO43-) salts  Note: the terms insoluble and slightly soluble really mean the same thing, since such a tiny amount dissolves that it is not possible to detect it with the naked eye.