unit 10 - acids, bases, & salts

Question 1

electrolytes

Answer 1

Substances that can conduct electric current, because they dissociate into ions (charged
particles that can carry a current) in the liquid state.

• ALL acids, bases, and salts are electrolytes

Question 2

Acids

Answer 2

Release Hydrogen Ions (H+) or form Hydronium Ions (H3O+) ions in solution.

• Watch out for “COOH” endings
  they are organic acids (CH3COOH)
• Watch out for CO2 (aq); carbon dioxide in
  water becomes H2CO3

Question 3

COOH endings are

Answer 3

organic acids (CH3COOH)

Question 4

acids generally begin with

Answer 4

H or end in COOH

Question 5

reading table k (acids)

Answer 5

as you go down, weaker the acid

HCl - strong
CH3COOH - weak

Question 6

bases

Answer 6

Release Hydroxide Ions (OH-) in solution.

*Watch out for NH3 (aq); ammonia in water becomes NH4OH

Question 7

bases end in

Answer 7

OH generally

Question 8

salts

Answer 8

Substances that are not acids or
bases BUT ! dissociate into ions in
solution that are not H+ and OH-.

Question 9

nonelectrolytes

Answer 9

Substances that are bad conductors of electricity because they do NOT dissociate into ions in solution.

Ex. Molecular Substances or Covalent
- C6H12O6, C12H22O11 (sugars)
- C2H5OH (alcohol) * Watch out for this* alcohols have C’s & H’s followed by OH thus they are not a base.

Question 10

alcohols have…

Answer 10

C’s and H’s followed by OH thus they are not a base

Question 11

characteristics of acids

Answer 11

• Acids have a sour taste.
  Ex. Lemon contain Citric Acid.
• Acids are electrolytes & conduct electric currents.
  All Acids release H+ Ions/H3O+
  (hydrogen)/(hydronium)

Question 12

arhenius definition of an Acid

Answer 12

Acids are electrolytes & conduct electric currents. All Acids release H+ Ions/H3O+
(hydrogen)/(hydronium)

Question 13

strong acids easily…

Answer 13

ionize
- release high [H+]

Question 14

weak acids dont easily

Answer 14

ionize
- release low [H+]

Question 15

characteristics of bases

Answer 15

• Bases have a Bitter taste.
• Bases are slippery to the touch.
• Bases are electrolytes & conduct Electric Currents. All Bases release
  [OH-] Ions

Question 16

arrhenius definition of Bases

Answer 16

• Bases are electrolytes & conduct Electric Currents. All Bases release
  [OH-] Ions

Question 17

strong bases release

Answer 17

high [OH-]

Question 18

weak bases release

Answer 18

low [OH-]

Question 19

What are the two major reaction that involve acids &/or bases?

Answer 19

1) Neutralization Reactions
- Acids + Bases
2) Special Single Replacement Rxns
- Acids + Strong!! Metals

Question 20

Neutralization Reaction

Answer 20

** special double replacement

acid + base => salt + water

Question 21

what is the reverse reaction of neutralization

Answer 21

• reverse reaction (opposite) is hydrolysis
• salt + water => acid + base

Question 22

acids react with _______ metals to produce what

Answer 22

STRONG metals to produce hydrogen gas

**not all metals will do this because of their reactivity

Question 23

acids reacting with metals

Answer 23

• Look it up on Table J
• ONLY!! metals listed above Hydrogen (H2) Are reactive enough that will react with acids to produce Hydrogen gas + a salt.

Question 24

acids and bases affect the color of indicators based on the specific

Answer 24

pH

Question 25

EX: Will Cu react with HCl? Why or why not?

Answer 25

No, Cu is not active enough

Question 26

pH is based on the

Answer 26

• concentration of an acid
• pH scale expresses [H+] concentration as a # from 0-14

Question 27

pH of 0

Answer 27

strong acid

Question 28

pH of 7

Answer 28

neutral

Question 29

pH of 14

Answer 29

strong base

Question 30

DO NOT discuss pH range

Answer 30

• USE ONLY!!! The numbers to the right or left of \the range. Even for part 2 answers
• Never use number in the range because the indicator is just changing color.

Question 31

the lower the pH the…

Answer 31

more acidic the substance is (the less basic it is)

Question 32

more acidic = _____ H+ ions released

Answer 32

more H+ ions released
ex: pH of 3 more acidic than 4

Question 33

the higher the pH the…

Answer 33

less acidic the substance is (the more basic it is)

Question 34

less acidic = _____ H+ ions released

Answer 34

fewer H+ ions released
ex: pH of 9 is less acidic (more basic) than 7

Question 35

water can dissociate

Answer 35

when pH 7 or pure water at 25°C
[H+] = 1 x 10^-7 & [OH-] = 1x 10^-7

Question 36

concentration in acids

Answer 36

[H+] is Greater than [OH-]

Question 37

concentration in bases

Answer 37

[OH-] is Greater than [H+]

Question 38

concentration when neutral

Answer 38

[H+] is equal to [OH-]

Question 39

pH formula

Answer 39

pH = -log [H+]

• to find the pH, you need H+ concentration

Question 40

pH change

Answer 40

• each change in a single pH unit is a TEN fold change in the [H+]
• ex: [H+] is 10x greater in a solution with a pH of 5 as a solution with a pH of 6

Question 41

if [H+] = 1x10^-9, pH is

Answer 41

9

Question 42

pOH formula

Answer 42

pOH = -log [OH-]

Question 43

other than neutral

Answer 43

[H+] X [OH-] = 1 X 10^-14 M

Question 44

pH + pOH

Answer 44

= 14

Question 45

titrations

Answer 45

The process of adding measured volumes of an Acid or Base of known concentration TO an Acid or Base of unknown concentration until neutralization occurs

Question 46

when the NEUTRALIZATION point is reached it means the

Answer 46

[H+ ] = [OH- ]; pH is 7

• moles of H+ = moles of OH-

Question 47

titration formula

Answer 47

Ma x Va = Mb x Vb
- look at this for sigfigs

Question 48

when data table says “volume used”

Answer 48

use that in MaVa = MbVb

Question 49

when data table says “initial or final volume”

Answer 49

subtract to find volume used

Question 50

Bronsted/Lowry:”Alternate Theory”: Acids

Answer 50

acids lose protons (proton donors)

Question 51

Bronsted/Lowry:”Alternate Theory”: Bases

Answer 51

bases gain protons (proton acceptors)