Bob Jones Chemistry - Chapter 16
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| acidic solution | A solution with more H 3 O+ ions than OH- ions, resulting in a pH less than 7.
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| acid-ionization constant | Related to the ionization constant of water, it is the value that describes the extent of the forward equilibrium reaction in the formation of the hydronium ion.
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| amphoteric | A substance that can act as either a Bronsted-Lowry acid or base.
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| Arrhenius acid | A substance that releases hydrogen ions (H+) when dissolved in water.
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| Arrhenius base | A substance that releases hydroxide ions (OH-) when dissolved in water.
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| base-ionization constant | Related to the ionization constant of water, the value that describes the extent of the forward equilibrium reaction in the formation of the hydroxide ion.
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| basic solution | A solution with fewer H 3 O+ ions than OH- ions, resulting in a pH greater than 7; also called an alkaline solution.
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| Bronsted-Lowry acid | A substance that donates protons.
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| Bronsted-Lowry base | A substance that accepts protons.
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| buffer | A solution that resists changes in pH when a moderate amount of either an acid or base is added.
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| conjugate acid | The structure formed when a base is protonated.
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| conjugate base | The structure formed when an acid has donated a proton.
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| conjugate pair | Two particles that differ from each other by only a proton (a hydrogen ion).
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| deprotonation | The process of losing a proton.
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| diprotic | An acid that can donate two protons.
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| electrolyte | A substance that releases ions and conducts electricity when it dissolves in water.
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| end point | The point in a titration at which some change in a property of the solution is detected.
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| equivalence point | The point in a titration at which an equivalent amount of titrant has been added. The number of H 3 O+ ions equals the number of OH- ions.
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| indicator | A substance that changes color when the pH of a solution changes.
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| ionization constant of water | In self-ionization, the product of the concentrations of the hydronium ion (H 3 O+) and the hydroxide ion (OH-); 1.0 x 10 -14 at 25 °C; also called the dissociation constant of water.
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| Lewis acid | Any substance that can accept a pair of electrons.
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| Lewis base | Any substance that can donate a pair of electrons.
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| monoprotic | An acid that can donate only one proton.
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| neutralization reaction | The reaction of an acid and a base to produce a neutral solution (pH=7) of water and a salt.
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| neutral solution | A solution with equal numbers of H 3 O+ and OH- ions; pH=7.
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| pH | A measure of the hydronium ion (H 3 O+) concentration. It is the negative logarithm of the molar H 3 O+ ion concentration:
pH=-log (H 3 O+).
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| pOH | A measure of the hydroxide ion (OH-) concentration. It is the negative logarithm of the molar OH- ion concentration:
pOH=-log (OH-).
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| polyprotic | An acid that can donate more than one proton per molecule.
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| protonation | The process of gaining a proton.
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| salt | An ionic compound formed from the cation of a base and the anion of an acid.
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| self-ionization of water | A process in an acid-base reaction in which one molecule donates a proton to another molecule of the same substance; also called auto-ionization or autoprotolysis.
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| strong acid | A substance that readily gives up protons and ionizes completely in an aqueous solution.
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| strong base | A substance that readily accepts protons.
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| titration | A controlled reaction (often neutralization) conducted to measure the capacity of a solution of unknown concentration to react with one of known concentration.
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| titration curve | A graph that plots the pH change of a solution versus the volume of added acids or bases.
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| transition interval | An indicator's range of pH values over which a color change occurs.
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| triprotic | An acid that can donate three protons.
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| weak acid | A substance that does not give up protons easily and does not ionize completely in an aqueous solution; a weak electrolyte.
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| week base | A substance that is a poor proton acceptor and does not ionize completely in an aqueous solution; a weak electrolyte.
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