chem lecture ch15
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| Brønstedt-Lowry acids and bases | Arrhenius defined, that acid-base neutralizations are reactions in which an acid and a base combine forming water and a salt.views acid-base reactions as proton transfers.
An acid is a proton donor.
A base is a proton acceptor.
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| conjugate acid-base pair | Two substances that differ from each other by only one proton
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| Amphoteric substances | substances (molecules, ions) that can react as either acids or bases
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| define strength of an acid | its ability to donate a proton to a base. We measure the strength by determining the progress of this reaction towards completion. A reference base is needed to compare different acids, water is the reference of choice.
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| define a strong acid | one that is completely converted to a new acid, the hydronium ion. Accordingly, H3O+ is the strongest acid in water.
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| define a weak acid | one that produces two acidic species.
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| When two amphoteric substances are mixed...? | the stronger acid will react as an acid, the stronger base as a base.
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| Binary acids | acids that consist of hydrogen and a nonmetal.The strength of the binary acids increase from the left to the right within a period.
The strength of the binary acids increase from the top to the bottom within a group.
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| oxoacids | Acids composed of hydrogen, oxygen and some other element. All structures of oxoacids have O-H groups, which donate the protons. The acidity of the protons is determined by the polarity of the O–H bond.
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| how does electronegativity of the central atom affect the acidity of an oxoacid? | As the electronegativity of the central atom increases, the acid becomes stronger.
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| Lewis acid | any ionic or molecular species that can accept a pair of electrons in the formation of a coordinate covalent bond. have valence orbitals, that are not completely filled such as BF3 or H+.
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| Lewis base | any ionic or molecular species that can donate a pair of electrons in the formation of a coordinate covalent bond. have completely filled valence orbitals and unshared pairs of electrons
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| acidic anhydrides | Nonmetal oxides that react with water and give acidic solutions.
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| how does the oxidation number of a metal influence acid-base properties? | As the oxidation number on a metal ion increases, the metal ion becomes more acidic, it becomes a better electron pair acceptor.
Examples:
Na2O
CaO
Al2O3
CrO3
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| define Acidic and basic solutions in terms of relative concentrations of hydronium and hydroxide ions. | Neutral solution: [ H3O+ ] = [ OH- ]
Acidic solution: [ H3O+ ] > [ OH- ]
Basic solution: [ H3O+ ] < [ OH- ]
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| pH basic formulas | pH = -log [ H+ ]
[ H+ ] = 10^-pH
Ion product constant KW = [ H+ ] [ OH- ] at 25 °C
pKW = pH + pOH = 14 at 25 °C
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| Contributors to the proton concentration in an acid (formula) | [ H+ ]total = [ H+ ]solute + [ H+ ]water
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