Acid-Base Titrations

Question 1

pH meter measures the _______ produced in the solution

Answer 1

voltage

Question 2

blue paper turns red at pH?

Answer 2

<5

Question 3

They defined acid-base reactions as processes that involve the transfer of proton (H+) from one substance to another. The one which donates the proton is the acid while the one that accepts the proton is the base.

Answer 3

Johannes Brønsted and Thomas Lowry

Question 4

red paper turns blue at pH?

Answer 4

8

Question 5

These are aqueous systems that tend to resist changes in pH when small amounts of acid (H⁺) or base (OH⁻) are added

Answer 5

Buffers

Question 6

are important because it tells you the pH of the solution at the equivalence point

Answer 6

Titration Curves

Question 7

CH3COOH has a conjugate base pair

Answer 7

CH3COO-

Question 8

If [H3O+] is higher, then it is

Answer 8

acidic

Question 9

Weak acid and a Conjugate base in a sol’n will give you

Answer 9

Buffer Solution

Question 10

For less accurate method, one can use this to measure the pH of a solution

Answer 10

litmus papers

Question 11

For more accurate measurements, a ___________ is used which measures the voltage produced in the solution.

Answer 11

pH meter

Question 12

The one that accepts the proton is the

Answer 12

Base

Question 13

What happens to pH at equivalence point?

Answer 13

changes drastically so the curve is somewhat vertical at equivalence point

Question 14

have two ionizable protons

Answer 14

Diprotic acids

Question 15

Since strong acids and bases completely dissociates in solution, the equilibrium concentrations of H3O+ (for acids) and OH- (for bases) are?

Answer 15

equal to their initial concentrations

Question 16

pH range where the buffer is most effective in resisting pH change

Answer 16

Buffer Range

Question 17

The only difference between conjugate pairs is the transfer of

Answer 17

H+

Question 18

The one which donates the proton is the

Answer 18

Acid

Question 19

One common example of amphiprotic substances

Answer 19

water

Question 20

A solution in which [H3O+] is equal to [OH-] is called

Answer 20

Neutral

Question 21

encompass all acids containing more than one ionizable H

Answer 21

polyprotic acids

Question 22

This property of water where it can act as either a Bronsted-Lowry acid or a Bronsted-Lowry base is called

Answer 22

autoionization

Question 23

He defined acids as substances that, when dissolved in pure water, increase the concentration of H+ ions, and bases are those that increase the concentration of OH− ions.

Answer 23

Svante Arrhenius

Question 24

It completely dissociates in solution

Answer 24

strong acids and strong bases

Question 25

plots the pH of the solution against the volume of titrant added

Answer 25

Titration Curves

Question 26

acids as substances, when dissolved in pure water, increase the concentration of H+ ions, and bases are those that increase the concentration of OH− ions.

Answer 26

Arrhenius Definition

Question 27

They proposed a more general description for acids and bases.

Answer 27

Johannes Brønsted and Thomas Lowry

Question 28

indicates the end point of the titration

Answer 28

Acid-Base Indicators

Question 29

The equilibrium constant of the weak base is therefore called the

Answer 29

base-dissociation constant, Kb

Question 30

A proton donor and its corresponding proton acceptor make up a

Answer 30

conjugate acid-base pair

Question 31

The buffering power at midpoint is

Answer 31

maximal

Question 32

acts in the cytoplasm of all cells

Answer 32

Phosphate buffer system

Question 33

at half equivalence point, you will have

Answer 33

Buffer Solution

Question 34

There are substances that are capable of donating and accepting protons called

Answer 34

Amphiprotic substances

Question 35

This equilibrium constant of weak acid is called the

Answer 35

acid-dissociation constant, Ka

Question 36

higher [OH-] is considered

Answer 36

basic

Question 37

NH3 has a conjugate acid pair

Answer 37

NH4+

Question 38

These are mixtures of weak acids and their conjugate bases

Answer 38

Buffer systems

Question 39

In all acid-base reactions, the products will always be the ________________ of the other

Answer 39

conjugate pair

Question 40

The pH range of your indicator must be near the _____________________

Answer 40

Equivalence Point

Question 41

The higher the value of Ka

Answer 41

the stronger the acid

Question 42

This property of water where it can act as either a

Answer 42

Bronsted-Lowry acid or a Bronsted-Lowry base

Question 43

solutions containing a weak acid and its conjugate base, or a weak base and its conjugate acid

Answer 43

Acid-Base Indicators

Question 44

pH of an acidic solution

Answer 44

< 7.00

Question 45

pH of a neutral solution

Answer 45

= 7.00

Question 46

pH of a basic solution

Answer 46

> 7.00

Question 47

[H+][(M) of an acidic solution

Answer 47

> 1.0 x 10^-7

Question 48

[H+][(M) of a neutral solution

Answer 48

= 1.0 x 10^-7

Question 49

[H+][(M) of a basic solution

Answer 49

< 1.0 x 10^-7

Question 49

[OH-][(M) of an acidic solution

Answer 49

< 1.0 x 10^-7

Question 50

[OH-][(M) of a basic solution

Answer 50

> 1.0 x 10^-7

Question 51

[OH-][(M) of a neutral solution

Answer 51

= 1.0 x 10^-7

Question 52

pH + pOH = pKw= ?

Answer 52

14

Question 53

the equilibrium concentrations of H3O+ (for acids) and OH- (for bases) are equal to their

Answer 53

initial concentrations

Question 54

The higher the value of Ka, the __________ the acid.

Answer 54

stronger

Question 55

where HA is a weak acid and its conjugate base is A-, the equilibrium constant is called the?

Answer 55

acid-dissociation constant, Ka

Question 56

where HB is the conjugate acid of the base, the equilibrium constant expression is called the

Answer 56

base-dissociation constant, Kb

Question 57

the higher the value of Kb, the __________ the base

Answer 57

stronger

Question 58

have two ionizable protons

Answer 58

diprotic acids

Question 59

encompass all acids containing more than one ionizable H

Answer 59

polyprotic acids

Question 60

The stronger the acid, the __________ its pKa

Answer 60

lower

Question 61

the stronger the base, the ___________ its pKa

Answer 61

higher

Question 62

examples of strong acids

Answer 62

Perchloric acid Chloric acid Hydrobromic acid Hydrochloric acid Hydroiodic acid

Question 63

examples of strong bases

Answer 63

Potassium hydroxide Lithium hydroxide Rubidium hydroxide Sodium hydroxide Strontium hydroxide

Question 64

These are aqueous systems that tend to resist changes in pH when small amounts of acid (H⁺) or base (OH⁻) are added

Answer 64

Buffers

Question 65

where the buffer is most effective in resisting pH change

Answer 65

Buffer range - pH range

Question 65

These are mixtures of weak acids and their conjugate bases.

Answer 65

Buffer systems

Question 66

The buffering power at midpoint is

Answer 66

maximal

Question 67

A proton donor and its corresponding proton acceptor make up a

Answer 67

conjugate acid-base pair

Question 68

The only difference between conjugate pairs is the transfer of

Answer 68

H+

Question 68

In all acid-base reactions, the products will always be the ____________________ of the other.

Answer 68

conjugate pair

Question 69

expression that relates pH, pKa, and buffer concentration

Answer 69

Henderson-Hasselbalch Equation

Question 69

these are equal at midpoint

Answer 69

pH and pKa

Question 69

Henderson-Hasselbalch equation also allows us to calculate ________, given pH and the molar ratio of proton donor and acceptor

Answer 69

pKa

Question 70

Henderson-Hasselbalch equation also allows us to calculate ________, given pKa and the molar ratio of proton donor and acceptor

Answer 70

pH

Question 70

Henderson-Hasselbalch equation also allows us to calculate the __________________________, given pH and pKa

Answer 70

molar ratio of proton donor and acceptor

Question 71

__[buffer], ↓ΔpH, ↑ buffer capacity

Answer 71

↑

Question 71

factors affecting buffer capacity

Answer 71

1. concentration of the two buffer components 2. pH

Question 72

↑[buffer], __ΔpH, ↑ buffer capacity

Answer 72

↓

Question 73

↑[buffer], ↓ΔpH, __buffer capacity

Answer 73

↑

Question 74

buffer is most effective (ΔpH) when the acid is ________ since it gives greater capacity to neutralize the added base

Answer 74

higher

Question 75

buffer is most effective (ΔpH) when the acid is higher since it gives ___________________ to neutralize the added base

Answer 75

greater capacity

Question 76

acts in the cytoplasm of all cells, consists of H2PO4⁻ as proton donor and HPO42−as proton acceptor:

Answer 76

phosphate buffer system

Question 76

Blood plasma is buffered in part by the bicarbonate system, consisting of carbonic acid (H2CO3) as proton donor and bicarbonate (HCO3⁻) as proton acceptor

Answer 76

bicarbonate system

Question 76

these are two especially important biological buffers

Answer 76

1. Phosphate buffer system 2. Bicarbonate system

Question 77

proton donor in phosphate buffer system

Answer 77

H2PO4-

Question 78

proton acceptor in phosphate buffer system

Answer 78

HPO4^2-

Question 79

proton donor in bicarbonate system

Answer 79

H2CO3

Question 80

proton acceptor in bicarbonate system

Answer 80

HCO3-

Question 81

Titration curves are important because it tells you the pH of the solution at the?

Answer 81

equivalence point

Question 82

solutions containing a weak acid and its conjugate base, or a weak base and its conjugate acid

Answer 82

acid-base indicators

Question 83

The pH range of your indicator must be near the?

Answer 83

equivalence point