Acids and Bases

Question 1

Arrhenius Acid

Answer 1

Produces H+

Question 2

Arrhenius Base

Answer 2

Produces OH-

Question 3

Bronsted-Lowry Acid

Answer 3

Donates H+

Question 4

Bronsted-Lowry Base

Answer 4

Accepts H+

Question 5

Lewis Acid

Answer 5

Accepts electron pair

Question 6

Lewis Base

Answer 6

Donates electron pair

Question 7

Amphoteric Species

Answer 7

Species that can behave as an acid or a base.

Question 8

Amphiprotic

Answer 8

amphoteric species that specifically can behave as a Bronsted-Lowry acid/base.

Question 9

Polyprotic Acid

Answer 9

An acid with multiple ionizable H atoms

Question 10

Equivalent

Answer 10

1 mole of the species of interest

Question 11

Normality

Answer 11

Concentration of equivalents in solution

Question 12

Polyvalent

Answer 12

Can donate or accept multiple equivalents

Question 13

Half-Equivalence Point (midpoint)

Answer 13

The midpoint of the buffering region, in which half the titrant has been protonated or deprotonated. [HA] = [A-] and pH = pKa and a buffer is formed.

Question 14

Equivalence Point

Answer 14

The point at which equivalent amounts of acid and base have reacted. N1V1 = N2V2

Question 15

pH with strong acid + strong base

Answer 15

pH = 7

Question 16

pH with weak acid + strong base

Answer 16

pH > 7

Question 17

pH with weak base + strong acid

Answer 17

pH < 7

Question 18

pH with weak acid + weak base

Answer 18

pH > or < 7 depending on the relative strength of the acid and base

Question 19

Indicators

Answer 19

Weak acids or bases that display different colors in the protonated and deprotonated forms. The indicators pKa should be close to the pH of the equivalence point.

Question 20

Water dissociation constant

Answer 20

Kw = 10^-14 at 298 K
Kw = Ka x Kb

Question 21

pH and pOH

Answer 21

pH = -log[H+]
pOH = -log[OH-]
pH + pOH = 14
[H+] = 10^-pH

Question 22

p scale value approximation

Answer 22

-log(A x 10^-B)

p value is approximately -(B + 0.A)

Question 23

Litmus Test

Answer 23

Acid = red, Base = blue, Neutral = purple

Question 24

Phenolphthalein Test

Answer 24

pH < 8.2 = colorless, pH > 8.2 = purple

Question 25

Methyl Orange Test

Answer 25

pH < 3.1 = red, pH > 4.4 = yellow

Question 26

Bromophenol Blue Test

Answer 26

pH < 6 = yellow, pH > 8 = blue

Question 27

Endpoint

Answer 27

When indicator reaches full color

Question 28

Polyvalent Acid/Base Titrations

Answer 28

Multiple buffering regions and equivalence points

Question 29

Strong Acids/Bases

Answer 29

Dissociate completely

Question 30

Weak Acids/Bases

Answer 30

Do not completely dissociate

Question 31

Acid Dissociation Constant

Answer 31

Ka = [H2O+][A-] / [HA]
pKa = -log(Ka)

Question 32

Base Dissociation Constant

Answer 32

Kb = [B+][OH-] / [BOH]
pKb = -log(Kb)

Question 33

pKw

Answer 33

pKa + pKb = 14

Question 34

Conjugate Acid/Base Pairs

Answer 34

Strong acids and bases / weak conjugate

Weak acids and bases / weak conjugate

Question 35

Neutralization Reactions

Answer 35

From salts and (sometimes) H2O

Question 36

Buffer

Answer 36

Weak acid + conjugate salt

Weak base + conjugate salt

Question 37

Buffering Capacity

Answer 37

The ability of a buffer to resist changes in pH. Maximum buffering capacity is within 1 pH point of the pKa.

Question 38

Henderson-Hasselbalch Equation

Answer 38

pH = pKa + log[A-]/[HA]
pOH = pKb + log[B+]/[HOH]