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CHEM 120 SUMR'DONE > Unit 4: Questions > Flashcards

Unit 4: Questions Flashcards

1
Q

Acid formula begins with:

A

H+

e.g. HCl, HF, H2S, HNO3, H3PO4, etc.

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2
Q

Base formulas are usually _ compounds that contain _.

A

ionic, hydroxide

e.g. NaOH, Ba(OH)2, NH3, etc.

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3
Q

In aqueous solutions acids (gain/lose) H+?

A

lose H+

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4
Q

In aqueous solutions bases USUALLY dissociate into _ + _ ions?
Bases ALWAYS acquire _ in rxns?

A

metal + OH- ions

H+

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5
Q

Constants for acids Ka:

A

[H2PO4-] [H3O+]/

[H3PO4]

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6
Q

Constants for bases Kb:

A

[NH2OH]/

[NH3]

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7
Q

Ionization definition

A

convert (atom, molecule, or substance) into an ion or ions typically by removing one or more electrons

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8
Q

Ka is >1: (strongly/weakly) acidic, (high/low) % ionization

A

strongly acidic, high % ionization

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9
Q

Ka is <1: (strongly/weakly) acidic, (high/low) % ionization

A

weakly acidic, low % ionization

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10
Q

(high/low) Kb= strong base?

A

high

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11
Q

(high/low) Kb= weak base?

A

low

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12
Q

Properties of acids: (1)
Touch sensation:
Litmus: turns _ paper _
Tastes:

A

Electrolytes
Sting and burn
Litmus: turns blue paper red
Sour (function of tongue)

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13
Q

Properties of bases: (1)
Touch:
Litmus: turns _ paper _
Tastes:

A

Electrolytes
Slippery (still very damaging)
Litmus: turns red paper blue
Bitter

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14
Q

If the first atom is (_ color) = acid

A

yellow

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15
Q

Naming Binary acids

A

“hydro-(anion)-ic acid”

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16
Q

Naming Polyatomic acids
“ite” =
“ate” =

A 
"ite" = "(polyatomic name)-ous acid"
"ate" = "(polyatomic name)-ic acid"
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17
Q

Naming Sulfur (exceptions)
Binary=
“ite” =
“ate” =

A 
Binary = Hydrosulfuric acid
"ite" = sulfurous acid
"ate" = sulfuric acid
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18
Q

Naming Phosphorus (exceptions)
Binary=
“ite”=
“ate”=

A

Binary = hydrophosphoric acid
“ite” =phosphorous acid
“ate” = phosphoric acid

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19
Q

Acids ALWAYS react with water to produce _

A

hydronium ion (H3O+)

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20
Q

Hydronium ion

A

H3O+

21
Q

What ion makes and acid an acid

A

Hydronium (H3O+)

22
Q

What ion makes MOST bases a base

A

hydroxide (OH)

23
Q

Most bases are ionic compounds, and MUST be (soluble/insoluble)

A

Soluble

24
Q

When bases are added to water it _

A

Dissociates

25
Q

Some bases react with water to PRODUCE _

A

(an) ionic compound(s)

26
Q

Strong species (acids/bases) ionize nearly % (>%)

A

100% (>95%)

27
Q

Weak species ionize _% remains and

A

<5%

So >95% remains and <5% is broken up

28
Q 
Strong Acids (7)
Weak acids=
A
  1. HNO3
  2. H2SO4
  3. HCLO4
  4. HCLO3
  5. HCL
  6. HBr
  7. HI
    Weak acids= all other acids
29
Q 
Strong Bases (5)
Weak bases=
A
  1. LiOH
  2. NaOH
  3. KOH
  4. RbOH
  5. CsOH
    Weak bases= NH3, and all other bases
30
Q

The only soluble metal hydroxides (3)

A
  1. Ca(OH)2
  2. Sr(OH)2
  3. Ba(OH)2
31
Q

Strength (does/does not) refer to concentration

A

Does not

32
Q

“amphoteric” = “amphiprotic” =

A

acts as both acidic and a basic

33
Q

Symbols: H+ =

A

H3O+

34
Q

Names:
H+ = _ or _
H3O+ = _ ion

A

“proton” or “hydrogen ion”

“hydronium ion”

35
Q

Autoionization

A

the reaction of a chemical with ITSELF to produce positive and negative ions by the disassociation of one molecule

36
Q

What is Kw

A

ion product constant of water/in any aqueous solution

37
Q

If [H3O+] increases, [OH-] (increases/decreases)

If [OH-] increases, [H3O+] (increases/decreases)

A

decreases

decreases

38
Q

Kw: Acids and Bases
For acids, [H3O+] (&raquo_space; or &laquo_space;) [OH-]
For bases, [H3O+] (&raquo_space; or &laquo_space;) [OH-]

A

For acids, [H3O+]&raquo_space; [OH-]

For bases, [H3O+] &laquo_space;[OH-]

39
Q 
Kw= ? (relationship)
Kw= ? (number) (at what temp)
A 
Kw = [H3O+][OH-]
Kw = 1.0x10^-14 at 25 degrees C
40
Q

pH expresses…

pOH expresses…

A

an acid solutions strength

base strength

41
Q

[H3O+][OH-]=

pH+OH=

A

= 1.0x10^-14 (for ALL aqueous solutions)

= 14

42
Q

pH= (calc) _ or _

A

pH= -log[H3O+]

or [H3O+] = 10^-pH

43
Q

pOH= (calc) _ or _

A

pOH= -log[OH-]

or [OH-] = 10^-pOH

44
Q

“strongly basic” = pH < ~_

“weakly basic” = _ < pH < ~_

A

“strongly basic” = pH < ~13

“weakly basic” = 7 < pH < ~13

45
Q

“strongly acidic” = pH < ~_

“weakly acidic” = ~_ < pH < _

A

“strongly acidic” = pH < ~1

“weakly acidic” = ~1 < pH < 7

46
Q

Polyprotic acids:
H+ is a _ proton
Acids are “protic” because they…

A

naked proton

give off protons

47
Q

Monoprotic Acids:

A

HCl, HCN, HF, HBr, HNO3

48
Q

Diprotic Acids:

A

H2S, H2SO4, H2CO3

49
Q

Polyprotic acids:

A

H3PO4, H4AsO3, H3As, etc.

CHEM 120 SUMR'DONE (9 decks)

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