Quiz 4 Cards (Exam 2)

Question 1

Which definition defines an acid as “producing H+ in aqueous solutions”? (ex: HCl)

Answer 1

The Arrhenius Definition

Question 2

Which definition defines a base as “producing OH- in aqueous solutions”? (ex: NaOH)

Answer 2

The Arrhenius Definition

Question 3

Which definition describes an acid as “a proton/H+ DONOR”?

Answer 3

The Bronsted-Lowry Definition

Question 4

Which definition describes a base as “a proton/H+ ACCEPTOR”?

Answer 4

The Brønsted-Lowry Definition

Question 5

What are substances that can act as an acid AND base? (ex: H20)

Answer 5

Amphoteric

Question 6

Which definition describes an acid as “an electron pair ACCEPTOR”?

Answer 6

Lewis Acid-Base Definition

Question 7

Which definition describes a base as “an electron pair DONOR”?

Answer 7

Lewis Acid-Base Definition

Question 8

What makes strong acids and bases “strong”?

Answer 8

They are considered strong when there is COMPLETE ionization
(they are NOT at equilibrium/you CAN’T use an equilibrium expression for them)

Question 9

What are the six strong acids?

Answer 9

HCl
HNO3
HI
HBr
H2SO4
HClO4

Question 10

What are the six strong bases?
are ALL group 1 and 2 metals paired w/ OH

Answer 10

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

Question 11

Are weak acids and bases at equilibrium?

Answer 11

Yes (you can make equilibrium expressions for these)

Question 12

What does Kw= [H3O+] [OH-] equal?

Answer 12

1.0 x 10 to the -14 @ 25 degrees celcius

Question 13

When something is acidic, is [H3O+] larger or smaller than [OH-]?

Answer 13

It is bigger than [OH-]

Question 14

When something is basic, is [H3O+] larger or smaller than [OH-]?

Answer 14

It is smaller than [OH-]

Question 15

What makes something neutral?

Answer 15

When [H3O+] is equal to [OH-]

Question 16

What is the equation for pH?

Answer 16

pH= -log [H3O+]

Question 17

What is the equation for pOH?

Answer 17

pOH= -log [OH-]

Question 18

In regards to pH, what makes something acidic?

Answer 18

When the pH level is less than 7

Question 19

In regards to pH, what makes something basic?

Answer 19

When the pH level is greater than 7

Question 20

In regards to pH, what makes something neutral?

Answer 20

When the pH level is equal to 7

Question 21

What is the equation that relates pH AND pOH?

Answer 21

14=pH+pOH

Question 22

What is the equation that relates conjugate acid-base pairs?

Answer 22

Ka x Kb= Kw

Question 23

A larger Ka equals what?

Answer 23

A stronger acid

Question 24

A larger Kb equals what?

Answer 24

A stronger base

Question 25

The validity of x is ______% or *less* of the *initial concentration*

Answer 25

5%

Question 26

Neutral salts come from the *anion* of a *strong _______* and the cation of a *strong _______*

Answer 26

* Acid* *Base*

Question 27

Basic salts come from the cation of a *strong* and the anion is the * _________ of a weak acid*

Answer 27

*Base* *Conjugate base*

Question 28

In acidic salts, the cation is a _________ of a weak base/the anion is a strong ______

Answer 28

*Conjugate acid* *Acid*

Question 29

What resists pH change?

Answer 29

Buffer

Question 30

What components go into choosing a buffer?

Answer 30

*Preparation (acid and base concentrations must be large* *Buffering range* *Capacity*

Question 31

What will neutralize acid and base?

Answer 31

[Base]=[Acid]

Question 32

What will neutralize an acid?

Answer 32

[Base]>[Acid]

Question 33

What will neutralize a base?

Answer 33

[Acid]>[Base]