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chemistry > unit 10 - acids, bases, & salts > Flashcards

unit 10 - acids, bases, & salts Flashcards

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1
Q

electrolytes

A

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
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2
Q

Acids

A

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
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3
Q

COOH endings are

A

organic acids (CH3COOH)

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4
Q

acids generally begin with

A

H or end in COOH

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5
Q

reading table k (acids)

A

as you go down, weaker the acid

HCl - strong
CH3COOH - weak

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6
Q

bases

A

Release Hydroxide Ions (OH-) in solution.

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

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7
Q

bases end in

A

OH generally

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8
Q

salts

A

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

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9
Q

nonelectrolytes

A

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.

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10
Q

alcohols have…

A

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

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11
Q

characteristics of acids

A
  • Acids have a sour taste.
    Ex. Lemon contain Citric Acid.
  • Acids are electrolytes & conduct electric currents.
    All Acids release H+ Ions/H3O+
    (hydrogen)/(hydronium)
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12
Q

arhenius definition of an Acid

A

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

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13
Q

strong acids easily…

A

ionize
- release high [H+]

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14
Q

weak acids dont easily

A

ionize
- release low [H+]

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15
Q

characteristics of bases

A
  • Bases have a Bitter taste.
  • Bases are slippery to the touch.
  • Bases are electrolytes & conduct Electric Currents. All Bases release
    [OH-] Ions
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16
Q

arrhenius definition of Bases

A
  • Bases are electrolytes & conduct Electric Currents. All Bases release
    [OH-] Ions
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17
Q

strong bases release

A

high [OH-]

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18
Q

weak bases release

A

low [OH-]

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19
Q

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

A

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

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20
Q

Neutralization Reaction

A

** special double replacement

acid + base => salt + water

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21
Q

what is the reverse reaction of neutralization

A
  • reverse reaction (opposite) is hydrolysis
  • salt + water => acid + base
22
Q

acids react with _______ metals to produce what

A

STRONG metals to produce hydrogen gas

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

23
Q

acids reacting with metals

A
  • 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.
24
Q

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

A

pH

25
Q

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

A

No, Cu is not active enough

26
Q

pH is based on the

A
  • concentration of an acid
  • pH scale expresses [H+] concentration as a # from 0-14
27
Q

pH of 0

A

strong acid

28
Q

pH of 7

A

neutral

29
Q

pH of 14

A

strong base

30
Q

DO NOT discuss pH range

A
  • 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.
31
Q

the lower the pH the…

A

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

32
Q

more acidic = _____ H+ ions released

A

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

33
Q

the higher the pH the…

A

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

34
Q

less acidic = _____ H+ ions released

A

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

35
Q

water can dissociate

A

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

36
Q

concentration in acids

A

[H+] is Greater than [OH-]

37
Q

concentration in bases

A

[OH-] is Greater than [H+]

38
Q

concentration when neutral

A

[H+] is equal to [OH-]

39
Q

pH formula

A

pH = -log [H+]

  • to find the pH, you need H+ concentration
40
Q

pH change

A
  • 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
41
Q

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

A

9

42
Q

pOH formula

A

pOH = -log [OH-]

43
Q

other than neutral

A

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

44
Q

pH + pOH

A

= 14

45
Q

titrations

A

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

46
Q

when the NEUTRALIZATION point is reached it means the

A

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

  • moles of H+ = moles of OH-
47
Q

titration formula

A

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

48
Q

when data table says “volume used”

A

use that in MaVa = MbVb

49
Q

when data table says “initial or final volume”

A

subtract to find volume used

50
Q

Bronsted/Lowry:”Alternate Theory”: Acids

A

acids lose protons (proton donors)

51
Q

Bronsted/Lowry:”Alternate Theory”: Bases

A

bases gain protons (proton acceptors)

chemistry (11 decks)

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