Chapter 16 & 17 Flashcards
amine
A compound that has the general formula R3N, where R may be H or a hydrocarbon group. (Section 16.7)
acid-dissociation constant (Ka)
An equilibrium constant that expresses the extent to which an acid transfers a proton to solvent water. (Section 16.6)
amphiprotic
Refers to the capacity of a substance to either add or lose a proton (H+). (Section 16.2)
amphoteric oxides and hydroxides
Oxides and hydroxides that are only slightly soluble in water but that dissolve in either acidic or basic solutions. (Section 17.5)
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. (Section 16.3)
base-dissociation constant (Kb)
An equilibrium constant that expresses the extent to which a base reacts with solvent water, accepting a proton and forming OH– (aq). (Section 16.7)
Brønsted–Lowry acid
A substance (molecule or ion) that acts as a proton donor. (Section 16.2)
Brønsted–Lowry base
A substance (molecule or ion) that acts as a proton acceptor. (Section 16.2)
buffer capacity
The amount of acid or base a buffer can neutralize before the pH begins to change appreciably. (Section 17.2)
buffered solution (buffer)
A solution that undergoes a limited change in pH upon addition of a small amount of acid or base. (Section 17.2)
carboxylic acid
A compound that contains the —COOH functional group. (Sections 16.10 and 24.4)
common-ion effect
A shift of an equilibrium induced by an ion common to the equilibrium. For example, added Na2SO4 decreases the solubility of the slightly soluble salt BaSO4, or added NaF decreases the percent ionization of HF. (Section 17.1)
complex ion (complex)
An assembly of a metal ion and the Lewis bases (ligands) bonded to it. (Section 17.5)
conjugate acid
A substance formed by addition of a proton to a Brønsted–Lowry base. (Section 16.2)
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. (Section 16.2)
conjugate base
A substance formed by the loss of a proton from a Brønsted–Lowry acid. (Section 16.2)
formation constant
For a metal ion complex, the equilibrium constant for formation of the complex from the metal ion and base species present in solution. It is a measure of the tendency of the complex to form. (Section 17.5)
hydronium ion (H3O+)
The predominant form of the proton in aqueous solution. (Section 16.2)
ion-product constant
For water, Kw is the product of the aquated hydrogen ion and hydroxide ion concentrations: [H+][OH–].
Lewis acid
An electron-pair acceptor. (Section 16.11)
Lewis base
An electron-pair donor. (Section 16.11)
oxyacid
A compound in which one or more OH groups, and possibly additional oxygen atoms, are bonded to a central atom. (Section 16.10)
percent ionization
The percent of a substance that undergoes ionization on dissolution in water. The term applies to solutions of weak acids and bases. (Section 16.6)
pH
The negative log in base 10 of the aquated hydrogen ion concentration: pH
pH titration curve
A graph of pH as a function of added titrant. (Section 17.3)
polyprotic acid
A substance capable of dissociating more than one proton in water; H2SO4 is an example. (Section 16.6)
solubility-product constant (solubility product) (Ksp)
An equilibrium constant related to the equilibrium between a solid salt and its ions in solution. It provides a quantitative measure of the solubility of a slightly soluble salt. (Section 17.4)
