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29 Cards in this Set
- Front
- Back
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Acidic Solution
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Contains more Hydrogen Ions than Hydroxide Ions
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Basic Solution
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Contains more Hydroxide Ions than Hydrogen Ions
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Arrhenius Model
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A model of acids and bases; states that an acid is a substance that contains hydrogen and ionizes to produce hydrogen ions in aqueous solution and a base is a substance that contains a hydroxide group and dissociates to produce a hydroxide ion in aqueous solution; Used for Strong Acids
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Bronsted-Lowry Model
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A model that focuses on the hydrogen ion (H+); an acid is a hydrogen-ion donor and a base is a hydrogen-ion acceptor; Used for Weak Acids
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Conjugate Acid
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The species produced when a base accepts a hydrogen ion from an acid
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Conjugate Base
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The species that results when an acid donates a hydrogen ion to a base
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Conjugate Acid-Base Pair
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Consists of two substances related to each other by the donating and accepting of a single hydrogen ion
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Amphoteric
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Water and other substances that can act as either an acid or base
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Monoprotic Acid
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An acid that can donate only one hydrogen ion
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Polyprotic Acid
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Any acid that has more than one ionizable hydrogen atom
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Anhydrides
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Oxides that can become acids or bases by adding the elements contained in water
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Strong Acid
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An acid that ionizes completely in aqueous solution
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Weak Acid
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An acid that ionizes only partially in dilute aqueous solution
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Acid Ionization Constant (Ka)
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The value of the equilibrium constant expression for the ionization of a weak acid
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Strong Base
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A base that dissociates entirely into metal ions and hydroxide ions in aqueous solution
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Weak Base
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Ionizes only partially in dilute aqueous solution to form the conjugate acid of the base and hydroxide ion
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Base Ionization Constant (Ka)
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The value of the equilibrium constant expression for the ionization of a base
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Ion Product Constnat for Water (Kw)
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The value of the equilibrium constant expression for the self-ionization of water; H2O is Kw = 1.0 x 10 E-14
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pH
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The negative logarithm of the hydrogen ion concentration
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pOH
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The negative logarithm of the hydroxide ion concentration
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Neutralization Reaction
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A reaction in which an acid and a base react in aqueous solution to produce a salt and water
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Salt
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An ionic compound made up a cation from a base and an anion from an acid
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Titration
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A method for determining the concentration of a solution by reacting a known volume of the solution with a solution of known concentration
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Equivalence Point
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The stoichiometric point of a titration
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Acid-Base Indicators
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Chemical dyes whose colors are affected by acidic and basic solutions
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End Point
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The point at which the indicator used in a titration changes color
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Salt Hydrolysis
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The process in which anions of the dissociated salt accept hydrogen ions from water or the cations of the dissociated salt donate hydrogen ions to water
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Buffer
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Solutions that resist changes in pH when limited amounts of acid or base are added
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Buffer Capacity
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The amount of acid or base a buffer solution can absorb without a significant change in pH
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