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Solvent: a substance in a solution that is present in the largest amount
Solute: the dissolved substance in a solution
Electrolyte: a substance that dissolves in water to yield a solution that conducts electricity
Nonelectrolyte: a substance that dissolves in water to yield a solution that does not conduct
electricity
*The difference between an aqueous solution that conducts electricity and one that does not is
the presence or absence of ions
...
Strong Electrolyte: an electrolyte that ionizes or dissociates completely
• All water-soluble ionic compounds are strong electrolytes
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Instead, forward and reverse reactions both occurs,
and a state of dynamic chemical equilibrium is established
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*Soluble molecular compounds are sometimes strong electrolytes
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2: Precipitation Reactions
Precipitate: an insoluble product that separates from a solution
Precipitation Reaction: a chemical reaction in which a precipitate forms
Hydration: the process by which water molecules surround solute particles in an aqueous
solution
Solubility: the maximum amount of solute that will dissolve in a given quantity of solven at a
specific temperature
Water-Soluble Compounds
Insoluble Exceptions
+
Compounds containing an alkali metal cation (Li ,
Na+, K+, Rb+, Cs+) or the ammonium ion
Compounds containing the nitrate ion
,
acetate ion
, or chlorate ion
Compounds containing the chloride ion (Cl−),
Compounds containing Ag+,
−
−
bromide ion (Br ), or iodide ion (I )
, or Pb2+
Compounds containing Ag+,
Compounds containing the sulfate ion
, Pb2+, Ca2+, Sr2+, or Ba2+
Water-Insoluble Compounds
Compounds containing the carbonate ion
,
phosphate ion
, chromate ion
, or
2−
sulfide ion (S )
Compounds containing the hydroxide ion (OH−)
Soluble Exceptions
Compounds containing
Li+, Na+, K+, Rb+, Cs+, or
Compounds containing
Li+, Na+, K+, Rb+, Cs+, or
Ba2+
Molecular Equation: a chemical equation written with all compounds represented by their
chemical formulas
*If the compound is soluble, the phase is (aq)
...
Ionic Equation: chemical equation in which all strong electrolytes are shown as ions
• Species that are insoluble are represented with their chemical formulas
...
Net Ionic Equation: chemical equation from which spectator ions have been removed
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Brønsted Acid: a substance that donates a proton (H+)
Brønsted Base: a substance that accepts a proton (H+)
Hydronium Ion: a hydrated proton (H3O+)
Monoprotic Acid: an acid with one ionizable proton
Diprotic Acid: an acid with two ionizable protons
Triprotic Acid: an acid molecule with three ionizable protons
Polyprotic Acid: an acid with more than two ionizable protons
Neutralization Reactions: a reaction between an acid and a base
Salt: an ionic compound made up of the cation from a base and the anion from an acid
Arrhenius Acids
Arrhenius Bases
HX(aq)
Ionic compound containing: OH-, CO32-, or
HCO3HaXbOc
NH3
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For one species to gain electrons, another must lose them, and vice versa
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*Because compounds are electrically neutral, the oxidation numbers in any compound will sum
to zero
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Assigning Oxidation Numbers:
• The oxidation number of any element, in its elemental form, is zero
...
• The oxidation number of a monatomic ion is equal to its charge
...
Examples: LiH and CaH2—the oxidation
number of H is −1 in both examples
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Examples: H2O2 and
KO2—the oxidation number of O for H2O2 is −1 and for KO2
is
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Examples: ClF,
,
fluorine)
and
—the oxidation numbers of Cl, Br, and I are +1, +7,
and +5, respectively
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ß Oxidation # of element
ß Total contribution to charge by that element
Displacement Reaction: reaction in which two reactants trade components (double
displacement) or where a component of a reactant is removed (single displacement)
Activity Series: a list of metals arranged from top to bottom in order of decreasing ease of
oxidation
*An element will react with anything below it on the activity series, but will not react
with species above it
...
Metals at the bottom of
the series are called noble metals
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Separate the unbalanced reaction into half-reactions
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Balance each of the half-reactions with regard to atoms other than O and H
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Balance both half-reactions for O by adding H2O
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Balance both half-reactions for H by adding H+
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Balance both half-reactions for charge by adding electrons
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*A final check should show that the equation is balanced both for mass and charge
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Disproportional Reaction: when an element undergoes both oxidation and reduction in the
same reaction
Combustion: burning in air
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Molarity (M) =
L =
mol = M*L
*Molarity is defined in terms of the volume of solution, not volume of solvent
...
c = concentrated
dilute
d=
*Square brackets […] around a chemical species can be read as “the concentration of” that
species
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6: Aqueous Reactions and Chemical Analysis
*Experiments that measure the amount of a substance present are called quantitative analysis
...
* Highly accurate
*No two compounds that contain the same anion (or cation) have the same percent composition
by mass
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g
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Redox Titration: titration in which reactants undergo a redox reaction