Chp 10

Question 1

What is a Bronsted acid?

Answer 1

A Bronsted acid is a proton donor.

Question 2

What is a Bronsted base?

Answer 2

A Bronsted base is a proton acceptor.

Question 3

What is a Lewis acid?

Answer 3

A Lewis acid is an electron acceptor.

Question 4

What is a Lewis base?

Answer 4

A Lewis base is an electron donor.

Question 5

What is the difference between strong acids and weak acids?

Answer 5

Strong acids dissociate easily, while weak acids dissociate incompletely.

Question 6

What is the pH range for strong acids?

Answer 6

The pH for strong acids is less than 2.

Question 7

What is the pH range for weak acids?

Answer 7

The pH for weak acids is between 2 and 8.

Question 8

What is the pKb range for weak bases?

Answer 8

The pKb for weak bases is between 2 and 8.

Question 9

What does pH measure?

Answer 9

pH measures the acidity of a solution.

Question 10

What is the significance of a high pH?

Answer 10

A high pH indicates a basic solution.

Question 11

What is the significance of a low pH?

Answer 11

A low pH indicates an acidic solution.

Question 12

What does pOH measure?

Answer 12

pOH measures the basicity of a solution.

Question 13

What is the formula for calculating pOH?

Answer 13

pOH = -log[OH-]

Question 14

What is the significance of a high pOH?

Answer 14

A high pOH indicates an acidic solution.

Question 15

What is the significance of a low pOH?

Answer 15

A low pOH indicates a basic solution.

Question 16

What are strong acids and bases?

Answer 16

Strong acids and bases completely dissociate in solution.

Question 17

What are weak acids and bases?

Answer 17

Weak acids and bases partially dissociate in solution.

Question 18

What does Ka represent?

Answer 18

Ka (acid dissociation constant) measures the strength of an acid in solution.

Question 19

What does a higher Ka value indicate?

Answer 19

A higher Ka indicates a stronger acid that dissociates more into ions in solution.

Question 20

What does KB represent?

Answer 20

KB (base dissociation constant) measures how completely a base dissociates into its components in water.

Question 21

What does a higher KB value indicate?

Answer 21

A higher KB indicates a stronger base that dissociates more completely and produces more hydroxide ions.

Question 22

What is the relationship between pKa and acid strength?

Answer 22

Lower pKa indicates a stronger acid (more H+), while higher pKa indicates a weaker acid.

Question 23

How is pKa calculated?

Answer 23

pKa = -log(Ka).

Question 24

What is the relationship between pKb and base strength?

Answer 24

Lower pKb indicates a stronger base (more OH-), while higher pKb indicates a weaker base.

Question 25

What is the relationship between pKa and pKb for a conjugate acid-base pair?

Answer 25

pKa + pKb = 14 at 25°C.

Question 26

How do stronger acids relate to their conjugate bases?

Answer 26

A stronger acid has a very weak conjugate base.

Question 27

How do weaker acids relate to their conjugate bases?

Answer 27

A weak acid has a stronger conjugate base.

Question 29

What is the equilibrium constant (K) for a reaction?

Answer 29

The equilibrium constant (K) is a number that expresses the ratio of the concentrations of products to the concentrations of reactants at equilibrium, raised to the power of their coefficients in the balanced equation.

Question 30

True or False: The value of K changes with temperature.

Answer 30

True

Question 31

What is the relationship between pH and pOH?

Answer 31

pH + pOH = 14

Question 32

Which has a higher pH: a strong acid or a weak base?

Answer 32

A weak base

Question 33

Define a strong acid.

Answer 33

A strong acid is an acid that completely dissociates in solution, resulting in a high concentration of H+ ions.

Question 34

Give an example of a weak base.

Answer 34

Ammonia (NH3)

Question 35

What does a lower pH indicate about the strength of an acid?

Answer 35

A lower pH indicates a stronger acid.

Question 36

True or False: A buffer solution resists changes in pH upon the addition of small amounts of acid or base.

Answer 36

True

Question 37

What is the relationship between acid strength and the dissociation constant (Ka)?

Answer 37

The larger the Ka, the stronger the acid.

Question 38

Identify the term: The measure of how much a base can dissociate to produce OH- ions.

Answer 38

Base strength

Question 39

What happens to the pH of a solution when an acid is added?

Answer 39

The pH decreases.

Question 40

Define pOH.

Answer 40

pOH is a measure of the concentration of hydroxide ions (OH-) in a solution.

Question 41

Fill in the blank: A solution with a pH of 3 is ____ compared to a solution with a pH of 5.

Answer 41

more acidic

Question 42

True or False: The concentration of H+ and OH- ions in pure water at 25°C is equal.

Answer 42

True

Question 43

What does a pKa value indicate?

Answer 43

pKa indicates the strength of an acid; lower pKa values signify stronger acids.

Question 44

What is an aqueous solution?

Answer 44

An aqueous solution is a solution in which water is the solvent.

Question 45

If 2 1.0M solutions are made, one of a strong acid and one of a weak acid, the pH of the strong acid solution will be:

Answer 45

lower

Question 46

A 1.0M solution of a strong base will have what pH compared to a 1.0M solution of a weak base?

Answer 46

Higher pH

Question 47

Which solution has a higher pH: strong base solution, weak base solution, should be the same

Answer 47

Strong base solution

Question 48

Which base has a larger Kb: strong base or weak base

Answer 48

Strong base

Question 49

Which base has a more positive pkg: Strong base or weak base

Answer 49

Weak base

Question 50

Which solution has a larger concentration of the bases conjugated acid: strong base solution, weak base solution, should be the same

Answer 50

Weak base solution