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acid ionization
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reaction involving the transfer of a proton from an acid to water, yielding hydronium ions and the conjugate base of the acid
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acid ionization constant (
K
a
)
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equilibrium constant for an acid ionization reaction
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acid-base indicator
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weak acid or base whose conjugate partner imparts a different solution color; used in visual assessments of solution pH
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acidic
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a solution in which [H
3
O
+
] > [OH
−
]
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amphiprotic
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species that may either donate or accept a proton in a Bronsted-Lowry acid-base reaction
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amphoteric
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species that can act as either an acid or a base
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autoionization
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reaction between identical species yielding ionic products; for water, this reaction involves transfer of protons to yield hydronium and hydroxide ions
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base ionization
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reaction involving the transfer of a proton from water to a base, yielding hydroxide ions and the conjugate acid of the base
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base ionization constant (
K
b
)
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equilibrium constant for a base ionization reaction
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basic
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a solution in which [H
3
O
+
] < [OH
−
]
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Brønsted-Lowry acid
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proton donor
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Brønsted-Lowry base
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proton acceptor
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buffer
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mixture of appreciable amounts of a weak acid-base pair the pH of a buffer resists change when small amounts of acid or base are added
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buffer capacity
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amount of an acid or base that can be added to a volume of a buffer solution before its pH changes significantly (usually by one pH unit)
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color-change interval
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range in pH over which the color change of an indicator is observed
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conjugate acid
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substance formed when a base gains a proton
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conjugate base
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substance formed when an acid loses a proton
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diprotic acid
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acid containing two ionizable hydrogen atoms per molecule
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diprotic base
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base capable of accepting two protons
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Henderson-Hasselbalch equation
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logarithmic version of the acid ionization constant expression, conveniently formatted for calculating the pH of buffer solutions
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ion-product constant for water (
K
w
)
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equilibrium constant for the autoionization of water
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leveling effect
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observation that acid-base strength of solutes in a given solvent is limited to that of the solvent’s characteristic acid and base species (in water, hydronium and hydroxide ions, respectively)
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monoprotic acid
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acid containing one ionizable hydrogen atom per molecule
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neutral
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describes a solution in which [H
3
O
+
] = [OH
−
]
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oxyacid
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ternary compound with acidic properties, molecules of which contain a central nonmetallic atom bonded to one or more O atoms, at least one of which is bonded to an ionizable H atom
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percent ionization
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ratio of the concentration of ionized acid to initial acid concentration expressed as a percentage
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pH
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logarithmic measure of the concentration of hydronium ions in a solution
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pOH
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logarithmic measure of the concentration of hydroxide ions in a solution
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stepwise ionization
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process in which a polyprotic acid is ionized by losing protons sequentially
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titration curve
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plot of some sample property (such as pH) versus volume of added titrant
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triprotic acid
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acid that contains three ionizable hydrogen atoms per molecule
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