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?

AgNO3

KClK2CrO4

AgClBa(OH)2

CaSNaOH

Double Replacement Reactions

Ions trade placesAX + BY AY + BX

What Will Occur In Each?If a precipitate forms underline KNO3 + BaCl2

Na2SO4 + Pb(NO3)2

KOH + Fe(NO3)3

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

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

Net Ionic also applies to Single Replacement

Sodium metal is dropped into cold water

Lithium metal is dropped into a solution of zinc nitrate

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

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