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Precipitation Reactions

Explore precipitation reactions, solubility rules, double replacement reactions, net ionic equations, and stoichiometry calculations in aqueous solutions. Practice predicting outcomes and determining the mass of precipitates formed.

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Precipitation Reactions

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  1. Precipitation Reactions

  2. Precipitation • When two aqueous solutions combine to form an insoluble or only slightly soluble salt

  3. Solubility Rules

  4. Is Each Soluble? • AgNO3 • KCl • K2CrO4 • AgCl • Ba(OH)2 • CaS • NaOH

  5. Double Replacement Reactions • Ions trade places • AX + BY  AY + BX

  6. What Will Occur In Each?If a precipitate forms underline • KNO3 + BaCl2 • Na2SO4 + Pb(NO3)2 • KOH + Fe(NO3)3

  7. Net Ionic Equations • Strong electrolytes are represented as ions in aqueous solution • Spectator ions (not part of the reaction) cancel out • What is left behind is called the net ionic equation

  8. For each below write the molecular equation, complete ionic equation, and net ionic equation • Aqueous potassium chloride is added to aqueous silver nitrate • Aqueous potassium hydroxide is mixed with aqueous iron (III) nitrate

  9. Stoichiometry • Calculate the mass of NaCl that must be added to 1.50L of a .100M AgNO3 solution to precipitate all of the Ag+ ions

  10. Calculate the mass of precipitate formed when 1.25L of a .0500M lead nitrate solution is mixed with 2.00L of a .0250M sodium sulfate solution

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