precipitation reactions
DESCRIPTION
Precipitation Reactions. Precipitation. When two aqueous solutions combine to form an insoluble or only slightly soluble salt. Solubility Rules. Memorize: sodium, potassium, ammonium and nitrate always soluble. Is Each Soluble?. AgNO 3 KCl K 2 CrO 4 AgCl Ba(OH) 2 CaS NaOH. - PowerPoint PPT PresentationTRANSCRIPT
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Precipitation Reactions
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Precipitation
When two aqueous solutions combine to form an insoluble or only slightly soluble salt
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Solubility Rules
Memorize: sodium, potassium, ammonium and nitrate always soluble
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Is Each Soluble?
AgNO3
KClK2CrO4
AgClBa(OH)2
CaSNaOH
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Double Replacement Reactions
Ions trade placesAX + BY AY + BX
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What Will Occur In Each?If a precipitate forms underline KNO3 + BaCl2
Na2SO4 + Pb(NO3)2
KOH + Fe(NO3)3
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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
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For each below write the molecular equation, complete ionic equation, and net ionic
equationAqueous potassium chloride is added to
aqueous silver nitrate
Aqueous potassium hydroxide is mixed with aqueous iron (III) nitrate
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Net Ionic also applies to Single Replacement
Sodium metal is dropped into cold water
Lithium metal is dropped into a solution of zinc nitrate
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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
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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