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| acid ionization | 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 (Ka) | equilibrium constant for the ionization of a weak acid
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| acid-base indicator | organic acid or base whose color changes depending on the pH of the solution it is in
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| acidic | describes a solution in which [H3O+] > [OH−]
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| amphiprotic | species that may either gain or lose a proton in a reaction
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| amphoteric | species that can act as either an acid or a base
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| autoionization | 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 | 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 (Kb) | equilibrium constant for the ionization of a weak base
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| basic | describes a solution in which [H3O+] < [OH−]
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| Brønsted-Lowry acid | proton donor
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| Brønsted-Lowry base | proton acceptor
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| buffer | mixture of a weak acid or a weak base and the salt of its conjugate; the pH of a buffer resists change when small amounts of acid or base are added
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| buffer capacity | 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 | range in pH over which the color change of an indicator takes place
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| conjugate acid | substance formed when a base gains a proton
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| conjugate base | substance formed when an acid loses a proton
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| diprotic acid | acid containing two ionizable hydrogen atoms per molecule. A diprotic acid ionizes in two steps
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| diprotic base | base capable of accepting two protons. The protons are accepted in two steps
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| Henderson-Hasselbalch equation | equation used to calculate the pH of buffer solutions
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| ion-product constant for water (Kw) | equilibrium constant for the autoionization of water
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| leveling effect of water | any acid >H3O+, or any base > OH− will react with water to form H3O+, or OH−, respectively; water acts as a base to make all strong acids appear equally strong, and it acts as an acid to make all strong bases appear equally strong
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| monoprotic acid | acid containing one ionizable hydrogen atom per molecule
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| neutral | describes a solution in which [H3O+] = [OH−]
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| oxyacid | compound containing a nonmetal and one or more hydroxyl groups
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| percent ionization | ratio of the concentration of the ionized acid to the initial acid concentration, times 100
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| pH | logarithmic measure of the concentration of hydronium ions in a solution
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| pOH | logarithmic measure of the concentration of hydroxide ions in a solution
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| stepwise ionization | process in which an acid is ionized by losing protons sequentially
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| titration curve | plot of the pH of a solution of acid or base versus the volume of base or acid added during a
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| titration | triprotic acid acid that contains three ionizable hydrogen atoms per molecule; ionization of triprotic acids occurs in three steps
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