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Chemistry > CAP 11 > Flashcards

CAP 11 Flashcards

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1
Q

arrhenius acids

A

produce hydrogen ions (H+) when they dissolve in water

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2
Q

Naming acids

A
  • Hydrogen + Non metals= hydro+ -ic acid
    (ex. hydrochloric acid)
  • Hydrogen and polyatomic ions:
    ate becomes -ic acid (chlorate- chloric acid)
    ite becomes -ous acid (chlorite- chlorous acid)
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3
Q

HCl

A

Hydrochloric acid

strong

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4
Q

HBr

A

Hydrobromic acid

strong

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5
Q

HI

A

Hydroiodic acid

strong

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6
Q

HCN

A

Hydrocyanic acid

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7
Q

HNO3

A

Nitric acid

strong

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8
Q

HNO2

A

Nitrous acid

weak

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9
Q

H2SO4

A

Sulfuric acid

strong

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10
Q

H2SO3

A

Sulfurous acid

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11
Q

H2CO3

A

Carbonic acid

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12
Q

HC2H302

A

Acetic acid

weak

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13
Q

H3PO4

A

Phosphoric acid

weak

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14
Q

H3PO3

A

Phosphorous acid

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15
Q

HClO3

A

Chloric acid

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16
Q

HClO2

A

Chlorous acid

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17
Q

Arrhenius bases

A

Produce hydroxide ions (OH-) in water

18
Q

Naming bases

A 
Arrhenius bases are named as hydroxides
ex.
- NaOH sodium hydroxide 
- KOH potassium hydroxide 
-Al(OH)3 aluminium hydroxide
19
Q

Why arrhenius’ theory is shacky

A
  1. cannot explain why substances lacking hydroxide ions are bases ( ex. NH3)
  2. does not take into account the role of solvent
  3. does not describe accurately the role of H+ ion state ( does not exist as such in water)
20
Q

Bronsted-Lowry acids and bases

A
  • an acid is a substance that donates H+

- a base is a substance that accepts H+

21
Q

Lewis’ acids and bases

A
  • Acids can accept an electron pair

- Lewis bases can donate an electron pair

22
Q

Conjugate acid-base pairs

A

In any acid-base reaction there are two conjugate acid-base pairs.
Each pair is related by the loss and gain of one H+

23
Q

Amphoteric substances

A

Substances that can act as both acid and bases

ex. water: donates H+ when it reacts with a stronger base, accepts H+ when it reacts with a stronger acid

24
Q

Strong and weak acids

A
  • Strong acids completely ionizes in aqueous solutions

- Weak acids dissociate only slightly in water to form a few ions in aqueous solution

25
Q

Strong acids

A

HI ( hydroiodic

26
Q

HClO4

A

Perchloric acid

Strong

27
Q

HF

A

Hydrofluoric acid

weak

28
Q

Diprotic acids

A

Some acids have 2 H+ that dissociate one at a time

28
Q

Diprotic acids

A

Some acids have 2 H+ that dissociate one at a time

29
Q

Strong bases

A
  • Dissociate completely in water
  • Are formed from metals of groups 1A and 2A
    include:
    LiOH
    NaOH
    KOH
    Ba(OH)2
    Sr(OH)2
30
Q

Weak base

A

Poor acceptors of H+
Include:
NH3 ( ammonia)
NaOCl ( bleach)

31
Q

Acid dissociation constant

A

Is used to quantitatively measure the strength of an acid.
Small: the equilibrium lies to the left
Large: the equilibrium lies to the right
When an acid is strong, it’s Ka is not reported as dissociation is considered complete

32
Q

Base dissociation constant

A

The stronger the base, the larger the Kb
Small: equilibrium to the left
Large: equilibrium to the right

33
Q

Water dissociation constant

A 
Kw= (H3O+) (OH-)
Kw= 1.0 x 10^-14
34
Q

The pH scale

A 
Used to describe the acidity of solutions 
Has values that usually range from 0 to 14 
Acidic < 7
Basic > 7
Neutral= 7
Is a logarithm of the H30+ 
pH= - log (H3O+)
pH decreases as the H3O+ increases
35
Q

Acids react with

A
  • metals to produce salt and hydrogen gas

- bases to produce a salt and water

36
Q

A salt

A

An ionic compound that does not have H+ as the cation or OH- as the anion

37
Q

Neutralization reaction

A

An acid reacts with a base to produce salt and water

The salt formed is the anion from the acid and the cation from the base

38
Q

Antiacids

A

Substances that:

  • are used to neutralize excess stomach acid
  • are made of aluminum hydroxide and magnesium hydroxide mixtures
39
Q

Acid base titration

A
  • Procedure used to determine the concentration of an acid or a base by neutralizing it with a buffer
40
Q

Indicator

A

Ex. phenolphthalein

is added to identify the endpoint

Chemistry (11 decks)

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