Private: Chapter Fourteen (83/78) -- Chemistry 110

Private: Chapter Fourteen Key Terms, Key Equations, Summaries, and Exercises (Chapter 14) Key Terms - acid ionization - reaction involving the transfer of a proton from an acid to water, yielding hydronium ions and the conjugate base of the acid - acid ionization constant (Ka) - equilibrium constant for an acid ionization reaction - acid-base indicator - weak acid or base whose conjugate partner imparts a different solution color; used in visual assessments of solution pH - acidic - a solution in which [H3O+] > [OH−] - amphiprotic - species that may either donate or accept a proton in a Bronsted-Lowry acid-base reaction - amphoteric - species that can act as either an acid or a base - autoionization - reaction between identical species yielding ionic products; for water, this reaction involves transfer of protons to yield hydronium and hydroxide ions - base ionization - reaction involving the transfer of a proton from water to a base, yielding hydroxide ions and the conjugate acid of the base - base ionization constant (Kb) - equilibrium constant for a base ionization reaction - basic - a solution in which [H3O+] < [OH−] - Brønsted-Lowry acid - proton donor - Brønsted-Lowry base - proton acceptor - buffer - 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 - 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) - color-change interval - range in pH over which the color change of an indicator is observed - conjugate acid - substance formed when a base gains a proton - conjugate base - substance formed when an acid loses a proton - diprotic acid - acid containing two ionizable hydrogen atoms per molecule - diprotic base - base capable of accepting two protons - Henderson-Hasselbalch equation - logarithmic version of the acid ionization constant expression, conveniently formatted for calculating the pH of buffer solutions - ion-product constant for water (Kw) - equilibrium constant for the autoionization of water - leveling effect - 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) - monoprotic acid - acid containing one ionizable hydrogen atom per molecule - neutral - describes a solution in which [H3O+] = [OH−] - oxyacid - 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 - percent ionization - ratio of the concentration of ionized acid to initial acid concentration expressed as a percentage - pH - logarithmic measure of the concentration of hydronium ions in a solution - pOH - logarithmic measure of the concentration of hydroxide ions in a solution - stepwise ionization - process in which a po