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Aqueous Reactions and Solution Stoichiometry (Oxidation-Reduction…
Aqueous Reactions and Solution Stoichiometry
General Properties
Compounds in Water
Ionic
Ions dissociate completely
Molecular
limited number of ions formed
Does a substance form ions?
yes
does solution conduct electricty well?
yes
Strong electrolyte
no
Weak electrolyte
no
nonelectrolyte
Precipitation reactions
Ions that are always soluble
Nitrate (NO3-)
Ammonium (NH4+)
Group 1 ions
Ionic Equations
molecular
Complete chemical forms (normal)
complete ionic
separate all aqueous compounds
net ionic
all ions that change
Acid-Base Reactions
Does it increase or decrease H+ concentration
increases
Acids
decreases
Bases
Reactions with
salt
acid + base -> water + salt
gas
Carbonates + acid -> CO2
NH4+OH -> H2O + NH3
sulfide+ acid -> H2S
Acids/Bases That are
Weak
are weak electrolytes
#
partially ionized
are reversible
Strong
are strong electrolytes
#
completely ionized
Identifying them
Acids
The chloric twins (HClO3, HClO4)
The other two (H2SO4, HNO3)
The Halogen Trio (HCl, HBr, HI)
Bases
Metal (OH)n
Oxidation-Reduction Reactions
Substance
gains electons
reduction
loses electrons
oxidation
Oxidation numbers
elements(by itself)
0
monatomic ion
equal to charge
nonmetals
oxygen
-2
-1 in peroxides
hydrogen
+1 when bonded to nonmetals
-1 when bonded to metals
halogens
-1
Oxidation by Acids/Salts
General pattern: A +BX -> AX + B
metal + acid-> H2
Activity Series
top metals
active metals
bottom metals
noble metals
metal below oxidized metal above
Concentrations of Solutions
Molarity
moles solute/
liters of solution
M = (mol/L)
Dilution
M(initial)
V(initial) = M(final)
V(final)
Solution Stoichiometry and Chemical anaylisis
types of units
lab units (measurable)
grams->moles: molar mass
volume/molarity ->moles: M = mol/L
chem units (moles)
moles->grams: molar mass
moles -> volume/molarity: M = mol/L
Titrations