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11.3
REACTIONS IN
AQUEOUS SOLUTIONS
Earth’s surface is 70% water….
We are made mostly of water
Here is a REAL-LIFE,
very important exampleof an aqueous reaction
occurring inside you even as we speak
______________________________________________________________________
REMINDER:
An aqueous physical state - (aq) means
___________________________________
An aqueous solution is a solution in
which _____________________________
Remember the demo - Spirit Day precipitate
___ KI ( ) + ___ Pb(NO3)2 ( )→
A precipitate is a ________________so this means that the
yellow precipitate is__________________ in water!
Not all ionic compounds are soluble in water.If a reaction is done in water…
Under normal conditions , an ionic compound will ALWAYS SOMETIMES NEVER be a liquid or gas.
WATER- SOLUBLE?
PHYSICAL STATE IS….
YES (aq)NO (s)
“Soda straws” in a cave
SOLUBLE COMPOUNDS
Compounds containing
IMPORTANTEXCEPTIONS
nitrate none
chloride salts of silver, mercury, lead
bromide salts of silver, mercury, lead
iodide salts of silver, mercury, lead
sulfate salts of calcium, strontium,barium, mercury, lead
SOLUBILITY CHART – mostly soluble
SOLUBILITY CHART – mostly insoluble
INSOLUBLECOMPOUNDS
Compoundscontaining
IMPORTANTEXCEPTIONS
sulfide salts of ammonium, alkali metals, calcium, strontium, barium
carbonate salts of ammonium, alkali metals,
phosphate salts of ammonium, alkali metals,
hydroxide compounds of alkali metals, calcium, strontium, barium
You don’t have to memorize these charts, butYOU SHOULD REMEMBER THESE PATTERNS….
ALL COMMON SALTS WITH
_____________________________________ and/or
________________________________________ARE SOLUBLE.
ALL COMMON COMPOUNDS of_________________
ARE SOLUBLE EXCEPT FOR _____________________
Determine whether these compounds are soluble or insoluble
EXAMPLES write (s) or (aq)
a. platinum nitrate ___ b. barium sulfide ___
c. magnesium chloride ___ d. Ammonium carbonate __________________________________________________________________NOW – YOU TRY IT!
1. iron (II) iodide ___ 2. aluminum phosphate ___
3. aluminum sulfate ___ 4. ammonium carbonate ___
5. barium sulfate ___ 6. barium sulfide ___ 7. silver nitrate ___ 8. mercury (I) chloride ___
9. calcium hydroxide ___ 10. copper (I) phosphate ___
COMPLETE IONIC EQUATIONS
_______________________________________
______________________________________
RULE #1: Solids (s), liquids (l), and gases (g),
___________________________________________
___________________________________________
2 KI (aq) + __ Pb(NO3)2 (aq) → 2 KNO3 (aq) + __ PbI2 (s)
RULE #2: Assume that all soluble aqueous compounds
______________________________________________________(Actually – not all do – but save that for another year.)
___NaCl (aq) →
__KI (aq) →
2 KI (aq) + __ Pb(NO3)2 (aq) → 2 KNO3 (aq) + __ PbI2 (s)
2K1+ (aq) + 2I1- (aq) →
PbI2 (s)
RULE #3: When writing aqueous compounds as dissociated, the
only subscripts that remain the same are those in _____________
_________________. The others become ____________________
NOW IT’S YOUR TURN! For the 2 reactants below, write the1) complete, balanced chemical equation.2) complete ionic equation.
copper (II) sulfate + sodium phosphate
Net ionic equations show you
_______________________________________
2 KI (aq) + __ Pb(NO3)2 (aq) →
2K1+ (aq) + 2K1+ (aq) + Pb2+ (aq) + 2NO31- (aq) →
2 KNO3 (aq) + __ PbI2 (s)
2K1+ (aq) + 2NO31- (aq) + PbI2 (s)
Ions that are unchanged during a chemical reaction are called…..
The DRIVING FORCE for this reaction (i.e., what made a chemical reaction occur) was the formation of a
_____________________
Now - try the equation you did before.
3Cu2+ (aq) + 3SO42- (aq) + 6Na1+ (aq) + 2PO4
3- (aq) →
6Na1+ (aq) + 3SO42- (aq) + Cu3(PO4)2 (s)
The DRIVING FORCE for this reaction was also the formation of a _____________________
The driving force isn’t always the formation ofa precipitate…Below is an acid-base reaction you will do later – using the equipment shown here.
HCl + NaOH → NaCl + HOH
Unless told otherwise – assume an acid is
_________________ and water is a _________________
HCl ( ) + NaOH ( ) → NaCl ( ) + HOH ( )
The driving force for an acid-base reaction* is the formation of ___________.
*For the type of acid-base reactions we’ll do this year.
__Al ( ) + __HCl ( ) →
Three potential DRIVING FORCES for chemical reactions are:
the formation of
____________________________
_____________________________
______________________________
The driving force for this reaction was the
formation of a _____________
NOW IT’S YOUR TURN; try these. ALL EQUATIONS MUST INCLUDE PHYSICAL STATESWrite the:1. complete, balanced chemical equation,2. complete ionic equation.3. net ionic equation4. driving force
1. ___HNO3 ( ) + ___Ca(OH)2( )→
Write the:1. complete, balanced chemical equation,2. complete ionic equation.3. net ionic equation4. driving force
2. ___(NH4)2CO3 ( ) + ___SnBr2( )→
Write the:1. complete, balanced chemical equation,2. complete ionic equation.3. net ionic equation4. driving force
3. ___ H3PO4 ( ) + ___ Mg ( )→