Chapter 4

Question 1

What is the name of the theory that says acids release H= ions and bases release OH- ions, and the cation from the base and anion from the acid make a salt?

Answer 1

Arrhenius theory

Question 2

What does the Bronsted-Lowry theory say about acids?

Answer 2

An acid donates an H+ ion

Question 3

What does the Bronsted-Lowry theory say about bases?

Answer 3

A base accepts an H+ ion.

Question 4

In a Bronsted-Lowry equilibrium, acids and bases can be found on which sides of the formula?

Answer 4

Both

Question 5

What do you call the H3O+ ion?

Answer 5

Hydronium

Question 6

What is a conjugate acid/base pair?

Answer 6

Two substances on opposite sides of the formula that differ by an H+ ion.

Question 7

What do you call a chemical species that can act as both an acid and a base?

Answer 7

Amphiprotic

Question 8

Are uncharged substances usually amphiprotic?

Answer 8

No.

Question 9

What charge are amphiprotic species usually?

Answer 9

negative

Question 10

Does the strength of an acid or base depend on concentration?

Answer 10

No.

Question 11

What is the strength of an acid/base?

Answer 11

The ability to produce ions in solution (dissociate)

Question 12

What do you call an acid that completely ionizes in solution?

Answer 12

Strong acid.

Question 13

What do you call an acid that only partially ionizes in solution?

Answer 13

Weak acid.

Question 14

Is an equilibrium an indicator of a strong or weak acid/base?

Answer 14

WEAK

Question 15

What do you call a base that completely dissociates in solution?

Answer 15

Strong base

Question 16

What do you call a base that partially dissociates in solution?

Answer 16

Weak base.

Question 17

What does the acid/base ionization constant not include?

Answer 17

Water

Question 18

What is the acid ionization constant equation? (Ka)

Answer 18

Ka = [product] [H3O] / [reactant]

Question 19

What is the base ionization constant equation? (Kb)

Answer 19

Kb = [product] [OH-] / [reactant]

Question 20

If Keq > 1 then the reaction favours the

Answer 20

reactants

Question 21

If Keq < 1 then the reaction favours the

Answer 21

products

Question 22

What levels the strength of strong acid/bases?

Answer 22

Water

Question 23

What do you call it when two water molecules automatically exchange an H+ ion between them?

Answer 23

The autoionization of water

Question 24

What is the ionization constant for water? (Kw)

Answer 24

Kw = [H3O+] [OH-] = 1.00x10^-14 = 25 degrees

Question 25

What happens when you add strong acids and bases to each other?

Answer 25

They neutralize each other

Question 26

What do you get when you multiply Kb and Ka?

Answer 26

Kw

Question 27

How to find the Kb value?

Answer 27

divide Kw (10^-14) by the Ka of the conjugate acid

Question 28

What is the equation to determine pH?

Answer 28

pH= -log [H3O+]

Question 29

What is the pH of acidic solutions?

Answer 29

less than 7

Question 30

What is the pH of basic solutions?

Answer 30

more than 7

Question 31

Every unit decrease in pH represents a decrease in how much [H3O+]?

Answer 31

a factor of 10

Question 32

What is the equation to calculate [H3O+] from pH?

Answer 32

[H3O+] = 10^-pH

Question 33

what does the lowercase “p” represent?

Answer 33

-log10 (10 is subscript)

Question 34

What do you get when you add pH and pOH?

Answer 34

pH + pOH = pKw

Question 35

For metal oxides we do not include what in our ionization equation?

Answer 35

Equilibrium arrows

Question 36

What are the steps for calculating whether a solution is acidic or basic when a strong acid is mixed with a strong base?

Answer 36

1: net reaction equation (neutralization)
2: calculate # of mol present before and after reaction
3: From excess reactant, calculate pH

Question 37

How do you determine the pH of weak acids?

Answer 37

Use the Ka expression, as well as an ice table.

Question 38

How do you determine the pH of weak bases?

Answer 38

Use an ice table and Kb expression

Question 39

How do you calculate the [weak base] necessary to produce a certain pH?

Answer 39

1: equilibrium equation + ice table
2: calculate [OH-]
3: compute Kb
4: solve