ch 16 vocab
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| hydronium ion (H3O+) | the predominant form of the proton in aqueous solution
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| Bronsted-Lowry acid | a substance (molecule or ion) that acts as a proton donor
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| Bronsted-Lowry base | A substance (molecule or ion) that acts as a proton acceptor
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| amphiprotic | refers to the capacity of a substance to act as either an acid or a base
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| conjugate base | a substance formed by the loss of a proton fro a Bronsted-Lowry acid
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| conjugate acid | a substance formed by the addition of a proton to a Bronsted-Lowry base
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| conjugate acid-base pair | An acid and a base, such as H2O and OH-, that differ only in the presence or absence of a proton
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| autoionization | the process whereby water spontaneously forms low concentrations of H+(aq) and OH-(aq) ions by proton transfer from one water molecule to another
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| ion-product constant | for water, K sub w is the product of the aquated hydrogen ion and hydroxide ion concentrations
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| pH | the negative log in base 10 of the aquated hydrogen ion concentration : pH= -log[H+]
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| acid-dissociation constant (K sub a) | an equilibrium constant that expresses the extent to which an acid transfers a proton to solvent water
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| polyprotic acid | a substance capable of dissociating more than one proton in water
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| base-dissociation constant (K sub b) | an equilibrium constant that expresses the extent to which a base reacts with solvent water, accepting a proton and forming OH-(aq)
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| hydrolysis | a reaction with water. when a cation or an anion reacts with water, it changes the pH
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| oxyacid | a compound in which one or more OH groups, and possibly additional oxygen atoms are bonded to a central atom
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| carboxylic acid | a compound that contains the -- COOH functional group
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| Lewis acid | an electron-pair acceptor
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| Lewis base | an electron-pair donor
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