8.1 & 8.2 Nature of Acids and Bases

Question 1

Acid - Taste

Answer 1

Sour

Question 2

Base - Taste

Answer 2

Bitter

Question 3

Acid - Texture of Solution

Answer 3

No characteristic feel

Question 4

Base - Texture of Solution

Answer 4

Slippery

Question 5

Acid - Aqueous Property of Oxides

Answer 5

Non metallic oxides

Question 6

Base - Aqueous Property of Oxides

Answer 6

Metallic oxides

Question 7

Acid - Reaction with Phenolphthalein

Answer 7

Colourless

Question 8

Base - Reaction with Phenolphthalein

Answer 8

Pink

Question 9

Acid - Reaction with Litmus

Answer 9

Blue –> Red

Question 10

Base - Reaction with Litmus

Answer 10

Red –> Blue

Question 11

Acid - Reaction with Metals

Answer 11

Release H2 gas

Question 12

Base - Reaction with Metals

Answer 12

No reaction

Question 13

Acid - Reaction with CO3^2-

Answer 13

Produce CO2 (g)

Question 14

Base - Reaction with CO3^2-

Answer 14

No Reaction

Question 15

Acid - Reaction with NH4Cl

Answer 15

No Reaction

Question 16

Base - Reaction with NH4Cl

Answer 16

Produce NH3 (g)

Question 17

Acid - Reaction with Fatty Acids

Answer 17

No Reaction

Question 18

Base - Reaction with Fatty Acids

Answer 18

Produce soaps

Question 19

Acid - Neutralization Reactions

Answer 19

Neutralize bases

Question 20

Base - Neutralization Reactions

Answer 20

Neutralize acids

Question 21

What are the two main acid-base theories?

Answer 21

• Arrhenius Theory
• Bronsted-Lowry Theory

Question 22

What is the Arrhenius Theory?

Answer 22

Based on the ions produced when they dissociate in water

Question 23

Arrhenius Theory - Acids

Answer 23

• Produce hydrogen ions (H+)
• Ex: HBr –> H+ + Br-

Question 24

Arrhenius Theory - Bases

Answer 24

• Produce hydroxide ions (OH-)
• Ex: NaOH –> Na+ + OH-

Question 25

Arrhenius Theory - Limitations

Answer 25

- Unable to explain role of H2O - Limited to H2O as the only solvent - Unable to explain basic behaviour of NH3

Question 26

What is the Bronsted-Lowry Theory?

Answer 26

It defines acids/bases regarding protons (H+)

Question 27

Bronsted-Lowry Theory - Acids

Answer 27

- Proton (H+) donor - Produce H3O+ ions - Ex: HBr + H2O --> H3O+ + Br-

Question 28

Bronsted-Lowry Theory - Bases

Answer 28

- Proton (H+) acceptors - Ex: NH3 + H2O --> NH4 + OH-

Question 29

Bronsted-Lowry Theory - Limitations

Answer 29

Amphiprotic nature of the theory

Question 30

What does amphiprotic mean?

Answer 30

Any chemical that can act as both an acid or a base

Question 31

Conjugate Acid

Answer 31

Forms when a base accepts a hydrogen ion (proton)

Question 32

Conjugate base

Answer 32

From when an acid loses a hydrogen ion (proton)

Question 33

What are conjugate acid/base pairs?

Answer 33

- Same overall chemical structure, but different ionic charges

Question 34

What happens when weak acids ionize and dissociate in water?

Answer 34

They form a dynamic equilibrium

Question 35

Binary Acids

Answer 35

- 2 elements - Hydrogen and a non-metal - Ex: HCl, HBr, H2S

Question 36

Oxygen Acids

Answer 36

- 3 elements - Hydrogen, oxygen and a polyatomic ion - Ex: H2SO4, H2CO3

Question 37

Organic Acids

Answer 37

- Have functional groups - Ex: acetic acid (vingear), CH3COOH

Question 38

Strong Acids

Answer 38

- Ionize completely in water - Ka is very large

Question 39

Weak Acids

Answer 39

- Ionize partially in water - In equilibrium - Smaller Ka values

Question 40

Position of the ionization equilibrium - strong acid

Answer 40

- Far to the right - Favours products

Question 41

Position of the ionization equilibrium - weak acid

Answer 41

- Far to the left - Favours reactants

Question 42

Eq concentration of H+ (aq) compared to the original concentration of HA - Strong Acid

Answer 42

[H+] = [HA]

Question 43

Eq concentration of H+ (aq) compared to the original concentration of HA - Weak Acid

Answer 43

[H+] < [HA]

Question 44

When the acid is stronger what happens to the conjugate base?

Answer 44

It's weaker

Question 45

When the acid is weaker what happens to the conjugate base?

Answer 45

It's stronger

Question 46

Weak bases

Answer 46

- CO3^2- - HCO3- - NH3 - All derivatives of ammonia

Question 47

Strong bases

Answer 47

All OH-

Question 48

Auto ionization of water

Answer 48

- Water can behave as both an acid and a base - 2H2O(l) ↔ H3O+(aq) + OH-(aq)

Question 49

What does Kw represent?

Answer 49

The equilibrium constant for the auto ionzation of water

Question 50

The big 6 acids

Answer 50

1. HClO4 2. HNO3 3. N2SO4 4. HBr 5. HCl 6. HI