Acid-Base Equilibria

Question 1

Bronsted-Lowry Acid

Answer 1

Proton donor

Question 2

Bronsted-Lowry Base

Answer 2

Proton acceptor

Question 3

Conjugate Base

Answer 3

Substance formed when an acid loses a proton

Question 4

Conjugate Acid

Answer 4

Substance formed when a base gains a proton

Question 5

Acid Ionization

Answer 5

Reaction involving the transfer of a proton from an acid to water, yielding hydronium ions and the conjugate base of the acid

Question 6

Base Ionization

Answer 6

Reaction involving the transfer of a proton from water to a base, yielding hydroxide ions and the conjugate acid of the base

Question 7

Amphiprotic

Answer 7

Species that may either donate or accept a proton in a Bronsted-Lowry acid-base reaction

Question 8

Amphoteric

Answer 8

Species that can act as either an acid or a base

Question 9

Autoionization

Answer 9

Reaction between identical species yielding ionic products; for water, this reaction involves the transfer of protons to yield hydronium and hydroxide ions

Question 10

Ion-Product Constant for Water (Kw)

Answer 10

Equilibrium constant for the autoionization of water

Question 11

Neutral

Answer 11

Describes a solution in which [H3O+]=[OH-]

Question 12

Acidic

Answer 12

A solution in which [H3O+]>[OH-]

Question 13

Basic

Answer 13

A solution in which [H3O+]<[OH-]

Question 14

pH

Answer 14

Logarithmic measure of the concentration of hydronium ions in a solution

Question 15

pOH

Answer 15

Logarithmic measure of the concentration of hydroxide ions in a solution

Question 16

Acid-Ionization Constant (Ka)

Answer 16

Equilibrium constant for an acid ionization reaction

Question 17

Percent Ionization

Answer 17

Ratio of the concentration of ionized acid to initial acid concentration expressed as a percentage

Question 18

Base-Ionization Constant (Kb)

Answer 18

Equilibrium constant for a base ionization reaction

Question 19

Leveling Effect

Answer 19

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)

Question 20

Oxyacids

Answer 20

Ternary compound with acidic properties, molecules of which contain an central nonmetallic atom bonded to one or more O atoms, at least one of which is bonded to an ionizable H atom

Question 21

Monoprotic Acids

Answer 21

Acid containing one ionizable hydrogen atom per molecule

Question 22

Diprotic Acids

Answer 22

Acid containing two ionizable hydrogen atoms per molecule

Question 23

Stepwise Ionization

Answer 23

Process in which a polyprotic acid is ionized by losing protons sequentially

Question 24

Tripotic Acid

Answer 24

Acid that contains three ionizable hydrogen atoms per molecule

Question 25

Diprotic Base

Answer 25

Base capable of accepting two protons

Question 26

Buffer

Answer 26

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

Question 27

Buffer Capacity

Answer 27

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)

Question 28

Henderson-Hasselbalch Equation

Answer 28

Logarithmic version of the acid ionization constant expression, conveniently formatted for calculating the pH of buffer solutions

Question 29

Titration Curve

Answer 29

Plot of some sample property (such as pH) versus volume of added titrant

Question 30

Acid-Base Indicators

Answer 30

Weak acid or base whose conjugate partner imparts a different solution color; used in visual assessments of solution pH

Question 31

Color Change Interval

Answer 31

Range in pH over which the color change of an indicator is observed