Quiz 2

Question 1

What is an acid (Arrhenius theory)?

Answer 1

a substance containing H+ and whose aqueous solution contains more H+ ions than OH- ions. Disolves “HA” in water

Question 2

Acid equation (Arrhenius theory)

Answer 2

HA (aq) = H+ (aq) + A- (aq)

Question 3

What is a base? (Arrhenius theory)

Answer 3

a substance containing OH- and whose aqueous solution contains more OH- ions than H+ ions. Dissolves “BOH” in water

Question 4

Base equation (Arrhenius theory)

Answer 4

BOH (aq) = B+ (aq) + OH- (aq)

Question 5

Neutralization (Arrhenius theory)

Answer 5

Produces water and an aqueous salt

Question 6

Acid (Bronsted-Lowry Theory)

Answer 6

Proton-donor (H+ ion donor)

Question 7

Base (Bronsted-Lowry Theory)

Answer 7

Proton-acceptor (H+ ion acceptor)

Question 8

When does water act as a base?

Answer 8

When an acid gives its proton to water

Question 9

Acid (Lewis Acids)

Answer 9

Electron pair acceptor

Question 10

Base (Lewis Acids)

Answer 10

Electron pair donator

Question 11

What is the driving force in all three acid/base schemes?

Answer 11

The formation of covalent bonds

Question 12

What happens when we put an acid in water?

Answer 12

Acid donates a proton to water

Question 13

What happens when we put a base in water?

Answer 13

The base grabs a proton from water

Question 14

Conjugate acid

Answer 14

Formed when a proton is transferred to the base

Question 15

Conjugate base

Answer 15

Everything that remains of the acid molecule after a proton is lost

Question 16

Conjugate acid-base pair

Answer 16

Consists of two substances related to each other by donating and accepting a single proton

Question 17

Are small K values weak or strong acids?

Answer 17

Weak

Question 18

Are large K values weak or strong acids?

Answer 18

Strong

Question 19

What is the magnitude of Ka?

Answer 19

A measure of how likely the acid is to dissociate in water

Question 20

Do strong acids dissociate completely in water?

Answer 20

Yes

Question 21

Do weak acids dissociate in water?

Answer 21

No

Question 22

What approaches 0 in a dilute solution of a strong acid?

Answer 22

[HA]

Question 23

What approaches 0 in a dilute solution of a weak acid?

Answer 23

[H3O+]

Question 24

Stronger the acid, the higher the _______ at equilibrium

Answer 24

[H3O+]

Question 25

The weaker an acid, the stronger its _____________

Answer 25

Conjugate base

Question 26

Strong acids

Answer 26

HCl, HBr, HI, HNO3, H2SO4, HClO3, HClO4

Question 27

Are large Kb values strong or weak bases?

Answer 27

Strong

Question 28

Are small Kb values strong or weak bases?

Answer 28

Weak

Question 29

Do strong or weak bases completely dissociate in water?

Answer 29

Strong bases

Question 30

Strong bases

Answer 30

M2O or MOH (M= group 1A metals) and MO or M(OH)2 (M=group 2A metals)

Question 31

What are most weak bases similar to?

Answer 31

NH3

Question 32

Amphoteric

Answer 32

Can be an acid or base (water)

Question 33

What is Kw and what does it equal?

Answer 33

The equilibrium constant for the autoionization of water and equals 1.0 x 10^ -14

Question 34

Equation for Kw

Answer 34

Ka x Kb = Kw (conjugate acid/base pair)

Question 35

pH of [H3O+] in pure water

Answer 35

1 x 10^ -4

Question 36

Equation for pH

Answer 36

pH = -log[H3O+]

Question 37

Equation for [H3O+]

Answer 37

[H3O+] = 10^ -pH

Question 38

Find pH directly (acid)

Answer 38

[H3O+] = [HA]o

Question 39

Find pH directly (base)

Answer 39

[OH-] = [XOH]o

Question 40

Equation for power of hydroxide

Answer 40

pOH = -log[OH-]

Question 41

Power of hydroxide in aqueous solution at 25 degrees C

Answer 41

pH + pOH = 14.00

Question 42

In a dilute solution of a weak acid ______

Answer 42

[HA]initial = [HA]eq

Question 43

Which compound will be the dominant producer of H+ in a solution?

Answer 43

The compound that has the greatest Ka value

Question 44

Is an ionic compound (salt) dissolved in water neutral, acidic, or basic?

Answer 44

Neutral

Question 45

What do salts consist of?

Answer 45

Cations of strong bases and the anions of strong acids

Question 46

Do salts have an effect on pH when dissolved in water?

Answer 46

No

Question 47

A salt whose cation alone has neutral properties and anion is the conjugate base of a weak acid produces a ________

Answer 47

Basic solution in water

Question 48

A salt whose anion alone has neutral properties and cation is the conjugate acid of a weak base or a small, highly charged metal will produce _________

Answer 48

Acidic solution in water

Question 49

Metals

Answer 49

Small, highly charged cations produce acidic solution in water

Question 50

What do you pair metals with?

Answer 50

H2O

Question 51

Equivalence Point

Answer 51

Point at which the amounts of titrant and sample are stoichiometrically equal.

Question 52

Stoichiometry titration

Answer 52

Add a strong base to a weak acid and determine extent of neutralization

Question 53

Equilibrium titration

Answer 53

Concentration of all species are determined and equilibrium expression evaluated

Question 54

Common ion effect

Answer 54

A shift in the equilibrium position that occurs because of the addition of an ion already involved in the equilibrium rxn

Question 55

Buffer

Answer 55

Solution of a weak acid and its conjugate base or weak base and conjugate acid

Question 56

What do buffers prevent?

Answer 56

Large changes in pH when strong acid or base is added

Question 57

Buffer capacity

Answer 57

Amount of strong acid or base a buffer can absorb without a significant change in pH

Question 58

What determines a greater buffer capacity?

Answer 58

Solution with larger concentrations of acid

Question 59

Ratio of the pH of a buffered solution

Answer 59

[A-]/[HA]

Question 60

Higher concentration of buffer components=

Answer 60

Larger buffering capacity

Question 61

Titration curve

Answer 61

A plot of pH as a function of NaOH

Question 62

What is the pH at equivalence for titrations between strong acids and bases?

Answer 62

7

Question 63

What's present at equivalence (strong acid/base)?

Answer 63

Water and spectator ions

Question 64

What are the 4 parts of a titration curve?

Answer 64

Initial, midpoint, equivalence, and after equivalence

Question 65

Saturated solution

Answer 65

Max amount of dissolved solute

Question 66

Ksp

Answer 66

Solubility product constant - equilibrium constant of a dissolution process

Question 67

Molar solubility

Answer 67

x value in ICE table

Question 68

Large Ksp

Answer 68

Mostly products

Question 69

Small Ksp

Answer 69

Mostly reactant

Question 70

Do strong acid anions react with H3O+?

Answer 70

No

Question 71

Do weak acid anions react with H3O+?

Answer 71

Yes

Question 72

Qsp=Ksp

Answer 72

Solution is saturated and at equilibrium

Question 73

Qsp>Ksp

Answer 73

Precipitate will form until solution becomes saturated (to the right)

Question 74

Qsp

Answer 74

Solution is unsaturated and no precipitate will form (to the left)

Question 75

Ka to pKa

Answer 75

-log(Ka) = pKa

Question 76

Henderson Hasselbalch Equation

Answer 76

pH = pKa + log([base]/[acid])

Question 77

pKa to Ka

Answer 77

Ka = 10^-pKa