Unit 4: Questions Flashcards by Aaliyah Williams

Acid formula begins with:

H+

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

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Base formulas are usually _ compounds that contain _.

ionic, hydroxide

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

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

lose H+

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

metal + OH- ions

H+

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Constants for acids Ka:

[H2PO4-] [H3O+]/

[H3PO4]

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Constants for bases Kb:

[NH2OH]/

[NH3]

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Ionization definition

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

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

strongly acidic, high % ionization

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

weakly acidic, low % ionization

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(high/low) Kb= strong base?

high

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(high/low) Kb= weak base?

low

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

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

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

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

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If the first atom is (_ color) = acid

yellow

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Naming Binary acids

“hydro-(anion)-ic acid”

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Naming Polyatomic acids
“ite” =
“ate” =

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

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

Binary = Hydrosulfuric acid
"ite" = sulfurous acid
"ate" = sulfuric acid

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

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

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Acids ALWAYS react with water to produce _

hydronium ion (H3O+)

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Hydronium ion

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H3O+

What ion makes and acid an acid

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Hydronium (H3O+)

What ion makes MOST bases a base

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hydroxide (OH)

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

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Soluble

When bases are added to water it _

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Dissociates

Some bases react with water to PRODUCE _

(an) ionic compound(s)

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

100% (>95%)

Weak species ionize _% remains and

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

``` Strong Acids (7) Weak acids= ```

1. HNO3 2. H2SO4 3. HCLO4 4. HCLO3 5. HCL 6. HBr 7. HI Weak acids= all other acids

``` Strong Bases (5) Weak bases= ```

1. LiOH 2. NaOH 3. KOH 4. RbOH 5. CsOH Weak bases= NH3, and all other bases

The only soluble metal hydroxides (3)

1. Ca(OH)2 2. Sr(OH)2 3. Ba(OH)2

Strength (does/does not) refer to concentration

Does not

"amphoteric" = "amphiprotic" =

acts as both acidic and a basic

Symbols: H+ =

H3O+

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

"proton" or "hydrogen ion" | "hydronium ion"

Autoionization

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

What is Kw

ion product constant of water/in any aqueous solution

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

decreases | decreases

Kw: Acids and Bases For acids, [H3O+] ( >> or << ) [OH-] For bases, [H3O+] ( >> or << ) [OH-]

For acids, [H3O+] >> [OH-] | For bases, [H3O+] << [OH-]

``` Kw= ? (relationship) Kw= ? (number) (at what temp) ```

``` Kw = [H3O+][OH-] Kw = 1.0x10^-14 at 25 degrees C ```

pH expresses... | pOH expresses...

an acid solutions strength | base strength

[H3O+][OH-]= | pH+OH=

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

pH= (calc) _ or _

pH= -log[H3O+] | or [H3O+] = 10^-pH

pOH= (calc) _ or _

pOH= -log[OH-] | or [OH-] = 10^-pOH

"strongly basic" = pH < ~_ | "weakly basic" = _ < pH < ~_

"strongly basic" = pH < ~13 | "weakly basic" = 7 < pH < ~13

"strongly acidic" = pH < ~_ | "weakly acidic" = ~_ < pH < _

"strongly acidic" = pH < ~1 | "weakly acidic" = ~1 < pH < 7

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

naked proton | give off protons

Monoprotic Acids:

HCl, HCN, HF, HBr, HNO3

Diprotic Acids:

H2S, H2SO4, H2CO3

Polyprotic acids:

H3PO4, H4AsO3, H3As, etc.

Unit 4: Questions Flashcards

(49 cards)