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Strong: complete dissociation of ions
Weak: partial dissociation of ions

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Two aqueous solutions mix and one of the products is insoluable

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is the delivery of a measured volume of solution of known concentration into a solution containing the substance being analyzed
- equivalence point/stoichiometric point: the stage in titration when enough titrant has been added to react exactly with the analyte

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Atoms in elemental state = 0
Monatomic ions = ion charge
Metals (in compounds) = +
Molecules and formula units = sum is 0
Polyatomic ions = sum is ion charge
Nonmetals w fixed oxidation states =
F=-1, H=+1, O=-2

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Oxidation: Increase in oxidation state
Reduction: Decrease in oxidation state
The oxidizing agent: oxidizes another substance and is itself reduced
The reducing agent: reduces another substance and is itself oxidized.

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is a chemical reaction in which one of the end products is a gas such as oxygen or carbon dioxide
- examples: carbonates & bicarbonates gas evolved is CO2, sulfites & bisulfites; SO2, ammonium; NH3

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Strong electrolytes dissociate completely into ions (strong acids and bases, soluble ionic compounds)
Weak electrolytes partially dissociate into ions (weak acids and bases)

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Electrolyte: dissolves and conducts electricity (yes ions)
ex. soluble ionic compounds, acids, bases
Nonelectrolyte: dissolves but does NOT conduct electricity (no ions)
ex. soluble molecular compounds

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Oxidation-reduction (redox) reaction: electrons are transferred from one reactant to the the other.
OIL RIG: Oxidation is loss (of electrons); Reduction is gain (of electrons)
Oxidation states: charge on an atom in the extreme limit of ionic bonding  (i.e.– if all shared electrons are assigned to the more electronegative atom).

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another term for acid-base reactions

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volume A to amount A: use molarity of substance A
mol A to mol B: use mole ratio from chemical equation
mol B to volume of B: use molarity of substance B

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Formula/Molecular: Molecules
Complete Ionic: All charged components are included (ionic molecules are written as separate parts with labeled charges)
Net Ionic: Spectator ions are removed from complete ionic equation

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- strong acids & bases completely dissociated into ions
- weak acids & bases are not dissociated in net ionic reactions

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releases hydroxide (OH-) in water
- it can be assumed that OH- reacts completely with any weak acid

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when the solvent-solute is stronger than the solute-solute

"like can dissolve like"

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sol. conc.= amount of solute/amount of solvent
molarity (M)= mol of solute/L of solution
- larger molarity= more concentrated solution
- can use molarity as a conversion factor

*during dilution, the number of moles of solute stays constant

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release protons in water

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8.2, 8.3, 8.4, 8.5 - Solubility, Molarity, Sol. Stoichiometry (Electrolytes, Acids, Bases)

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8.2, 8.3, 8.4, 8.5 - Solubility, Molarity, Sol. Stoichiometry (Electrolytes, Acids, Bases)

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8.6 and 8.7, 8.8, 8.9: Precipitation, Aqueous, Complete/Net Ionic, Acid Base Equations

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8.6 and 8.7, 8.8, 8.9: Precipitation, Aqueous, Complete/Net Ionic, Acid Base Equations