Page 799 - Chemistry--atom first

Chapter 14 | Acid-Base Equilibria 789
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 the ionization of a weak acid
acid-base indicator organic acid or base whose color changes depending on the pH of the solution it is in
acidic describes a solution in which [H3O+] > [OH−]
amphiprotic species that may either gain or lose a proton in a 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 the ionization of a weak base basic describes a solution in which [H3O+] < [OH−]
Brønsted-Lowry acid proton donor
Brønsted-Lowry base proton acceptor
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
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 takes place
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. A diprotic acid ionizes in two steps diprotic base base capable of accepting two protons. The protons are accepted in two steps Henderson-Hasselbalch equation equation used to calculate the pH of buffer solutions
ion-product constant for water (Kw) equilibrium constant for the autoionization of water
leveling effect of water any acid stronger than or any base stronger than OH− will react with water to form 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
monoprotic acid acid containing one ionizable hydrogen atom per molecule neutral describes a solution in which [H3O+] = [OH−]
oxyacid compound containing a nonmetal and one or more hydroxyl groups