Precipitation Reactions

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Precipitation Reactions Graphic: Wikimedia Commons User Tubifex

Double Replacement Reactions The ions of two compounds exchange places in an aqueous solution to form two new compounds. AX + BY  AY + BX One of the compounds formed is usually a precipitate (an insoluble solid), an insoluble gas that bubbles out of solution, or a molecular compound, usually water.

Double replacement forming a precipitate… Lead(II) nitrate + potassium iodide  lead(II) iodide + potassium nitrate Double replacement (ionic) equation Pb(NO3)2(aq) + 2KI(aq)  PbI2(s) + 2KNO3(aq) Complete ionic equation shows compounds as aqueous ions Pb2+(aq) + 2 NO3-(aq) + 2 K+(aq) +2 I-(aq)  PbI2(s) + 2K+(aq) + 2 NO3-(aq) Net ionic equation eliminates the spectator ions Pb2+(aq) + 2 I-(aq)  PbI2(s)

Solubility Rules – AP Chemistry All sodium, potassium, ammonium, and nitrate salts are soluble in water. Memorization of other “solubility rules” is beyond the scope of this course and the AP Exam. Therefore, the following slides are only for your amusement, and will not be tested 

Solubility Rules – Mostly Soluble Ion Solubility Exceptions NO3- Soluble None ClO4- Na+ K+ NH4+ Cl-, I- Pb2+, Ag+, Hg22+ SO42- Ca2+, Ba2+, Sr2+, Pb2+, Ag+, Hg2+

Solubility Rules – Mostly Insoluble Ion Solubility Exceptions CO32- Insoluble Group IA and NH4+ PO43- OH- Group IA and Ca2+, Ba2+, Sr2+ S2- Groups IA, IIA, and NH4+

Solubility Chart: Common salts at 25C S = Soluble I = Insoluble P = Partially Soluble X = Other