Transcript Precipitation Reactions - Lompoc Unified School District

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
 KCl
 K2CrO4
 AgCl
 Ba(OH)2
 CaS
 NaOH
Double Replacement
Reactions

Ions trade places
 AX + 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
equation

Aqueous 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