AP CHEM UNIT 8 REVIEW

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17 Terms

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pH
A measure of the acidity or basicity of a solution, calculated as pH = -log[H+].
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Strong Acids
Acids that dissociate completely in water, with no equilibrium, including HCl, HBr, HI, HNO3, HClO4, and H2SO4.
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Weak Acids
Acids that do not fully dissociate in water, only a small fraction contributes to hydrogen ion concentration.
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pKa
The negative logarithm of the acid dissociation constant (Ka), indicating the strength of an acid.
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Common Ion Effect
The decrease in solubility of a salt when another source of one of its ions is added to the solution.
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Equilibrium Constant of Water (Kw)
Kw = [H+][OH-] = 1x10^-14 at 25 degrees Celsius, indicating the product of the concentrations of hydrogen and hydroxide ions in water.
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Neutralization Reaction
A reaction between an acid and a base that results in the formation of water and salts.
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Buffer
A solution that resists changes in pH upon the addition of small amounts of acid or base.
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Henderson-Hasselbach equation
An equation used to calculate the pH of a buffer solution: pH = pKa + log([A-]/[HA]).
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Percent Dissociation
The ratio of the concentration of dissociated acid to the initial concentration of the acid, expressed as a percentage.
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Polyprotic Acids
Acids that can donate more than one proton per molecule, such as H2SO4 and H3PO4.
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Conjugate Base
The species that remains after an acid donates a proton.
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Ka (Acid Dissociation Constant)
A constant that measures the strength of an acid in solution; higher Ka indicates a stronger acid.
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Kb (Base Dissociation Constant)
A constant that measures the strength of a base in solution; higher Kb indicates a stronger base.
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Indicators
Weak acids that undergo a color change at specific pH levels, used to indicate the acidity or alkalinity of a solution.
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Titration
A laboratory method of quantitative chemical analysis used to determine the concentration of an identified analyte.
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Half-Equivalence Point
The point in a titration where half of the acid has been converted to its conjugate base.