unit 4

Question 1

What is the base equilibrium constant?

Answer 1

Kb

Question 2

What is the expression for Kb?

Answer 2

[HB+][OH-] / [B]

HB+ is the conjugate acid
B is the base

Question 3

Kb is less than 1

Answer 3

Weak base

Question 4

Kb is greater than 1

Answer 4

Strong base

Question 5

Lower Kb means

Answer 5

Weaker base

Question 6

Weak electrolyte

Answer 6

partially dissolves

Question 7

Strong electrolyte

Answer 7

completely dissolves

Question 8

If [H+] increases, then pH

Answer 8

decreases

Question 9

If [H+] decreases, then pH

Answer 9

increases

Question 10

What is the equation for pH?

Answer 10

pH= -log[H+]

Question 11

What is the equation for pOH?

Answer 11

pOH= -log[OH-]

Question 12

What is the equation for [H3O+]?

Answer 12

[H3O+] = 10^-pH

Question 13

What is the equation for [OH-]?

Answer 13

[OH-] = 10^-pOH

Question 14

When can you substitute H+ in the pH equation?

Answer 14

When you have a strong acid

Question 15

What are the strong acids?

Answer 15

HCl
HBr
HI
HNO3
HClO3
HClO4
H2SO4

Question 16

What are the weak acids?

Answer 16

HF
CH3COOH
CHOOH
H2SO3
H2CO3
H3PO4

Question 17

What are the strong bases?

Answer 17

LiOH
NaOH
BaOH
Ca(OH)2
Sr(OH)2
Ba(OH)2

Question 18

What are the weak bases?

Answer 18

NH3
F-
NO2-
C2H3O2-
CN-
HSO3
CH3NH2
C2H5NH2
C5H5N

Question 19

If you have a strong acid, the conjugate base will be

Answer 19

weak

Question 20

If you have a weak acid, the conjugate base will be

Answer 20

strong

Question 21

What is the Arrhenius definition of acids and bases

Answer 21

Bases produce OH- ions in solutions
Acids produce H+ ions in solutions

Question 22

What is the Brønsted-Lowry definition of acids and bases?

Answer 22

Acids are H+ donors
Bases are H+ acceptors

Question 23

Where do we see conjugate bases/acids present?

Answer 23

Bronstead-Lowry acids and bases

Question 24

How do you identify which substance is the conjugate acid?

Answer 24

Which ever one has the hydrogen “added” to it

Question 25

How do you identify which substance is the conjugate base?

Answer 25

Which ever one has the hydrogen going "bye bye"

Question 26

Define amphoterism

Answer 26

When a substance (which must have hydrogen) can act as both an acid and a base

Question 27

Autoionization

Answer 27

Water acting with itself

Question 28

[H3O+] is greater than [OH-]

Answer 28

Acidic solution

Question 29

[H3O+] is less than [OH-]

Answer 29

Basic solution

Question 30

[H3O+] is equal to [OH-]

Answer 30

Neutral solution

Question 31

pH < 7

Answer 31

Acidic

Question 32

pH > 7

Answer 32

Basic

Question 33

pH = 7

Answer 33

Neutral

Question 34

pOH < 7

Answer 34

Basic

Question 35

pOH > 7

Answer 35

Acidic

Question 36

pOH = 7

Answer 36

Neutral

Question 37

Kw expression

Answer 37

Kw = 1.0 x 10^-14M at 25 degrees celsius Kw = [H3O+][OH-]

Question 38

When given a picture, how do you identify the strong acid versus weak acid?

Answer 38

A strong acid dissociates completes so it will have more single ions and less molecules A weak acid dissociates partially so it will have less ions and more molecules

Question 39

pKA equation

Answer 39

pKa= -log(Ka)

Question 40

Higher Ka / Lower Ka

Answer 40

Higher Ka = stronger acid Lower Ka = weaker acid

Question 41

Higher pKa / Lower pKa

Answer 41

Higher pKa = weaker acid Lower pKa = stronger acid

Question 42

Higher pKb / Lower pKb

Answer 42

Higher pKb = weaker base Lower pKb = stronger base

Question 43

Kw expression in terms of Ka and Kb

Answer 43

(Ka)(Kb) = Kw

Question 44

If you warm water, what happens to the Kw, [H+], [OH-] pH, and pOH?

Answer 44

Kw increases [H+]/[OH-] increases pH/pOH decreases

Question 45

Define lewis acids

Answer 45

Lewis acids and electron pair acceptors

Question 46

Define lewis bases

Answer 46

Lewis bases are electron pair donors

Question 47

What happens to pH if you increase the concentration?

Answer 47

pH decreases