Chapter 16 & 17

Question 0

amine

Answer 0

A compound that has the general formula R3N, where R may be H or a hydrocarbon group. (Section 16.7)

Question 1

acid-dissociation constant (Ka)

Answer 1

An equilibrium constant that expresses the extent to which an acid transfers a proton to solvent water. (Section 16.6)

Question 2

amphiprotic

Answer 2

Refers to the capacity of a substance to either add or lose a proton (H+). (Section 16.2)

Question 3

amphoteric oxides and hydroxides

Answer 3

Oxides and hydroxides that are only slightly soluble in water but that dissolve in either acidic or basic solutions. (Section 17.5)

Question 4

autoionization

Answer 4

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)

Question 5

base-dissociation constant (Kb)

Answer 5

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)

Question 6

Brønsted–Lowry acid

Answer 6

A substance (molecule or ion) that acts as a proton donor. (Section 16.2)

Question 7

Brønsted–Lowry base

Answer 7

A substance (molecule or ion) that acts as a proton acceptor. (Section 16.2)

Question 8

buffer capacity

Answer 8

The amount of acid or base a buffer can neutralize before the pH begins to change appreciably. (Section 17.2)

Question 9

buffered solution (buffer)

Answer 9

A solution that undergoes a limited change in pH upon addition of a small amount of acid or base. (Section 17.2)

Question 10

carboxylic acid

Answer 10

A compound that contains the —COOH functional group. (Sections 16.10 and 24.4)

Question 11

common-ion effect

Answer 11

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)

Question 12

complex ion (complex)

Answer 12

An assembly of a metal ion and the Lewis bases (ligands) bonded to it. (Section 17.5)

Question 13

conjugate acid

Answer 13

A substance formed by addition of a proton to a Brønsted–Lowry base. (Section 16.2)

Question 14

conjugate acid–base pair

Answer 14

An acid and a base, such as H2O and OH–, that differ only in the presence or absence of a proton. (Section 16.2)

Question 15

conjugate base

Answer 15

A substance formed by the loss of a proton from a Brønsted–Lowry acid. (Section 16.2)

Question 16

formation constant

Answer 16

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)

Question 17

hydronium ion (H3O+)

Answer 17

The predominant form of the proton in aqueous solution. (Section 16.2)

Question 18

ion-product constant

Answer 18

For water, Kw is the product of the aquated hydrogen ion and hydroxide ion concentrations: [H+][OH–].

Question 19

Lewis acid

Answer 19

An electron-pair acceptor. (Section 16.11)

Question 20

Lewis base

Answer 20

An electron-pair donor. (Section 16.11)

Question 21

oxyacid

Answer 21

A compound in which one or more OH groups, and possibly additional oxygen atoms, are bonded to a central atom. (Section 16.10)

Question 22

percent ionization

Answer 22

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)

Question 23

pH

Answer 23

The negative log in base 10 of the aquated hydrogen ion concentration: pH

Question 24

pH titration curve

Answer 24

A graph of pH as a function of added titrant. (Section 17.3)

Question 25

polyprotic acid

Answer 25

A substance capable of dissociating more than one proton in water; H2SO4 is an example. (Section 16.6)

Question 26

solubility-product constant (solubility product) (Ksp)

Answer 26

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)