11.3 reactions in aqueous solutions. earth’s surface is 70% water…

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 ( )→