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Chemistry - Chemical Systems and Equilibrium > 8.1 & 8.2 Nature of Acids and Bases > Flashcards

8.1 & 8.2 Nature of Acids and Bases Flashcards

1
Q

Acid - Taste

A

Sour

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2
Q

Base - Taste

A

Bitter

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3
Q

Acid - Texture of Solution

A

No characteristic feel

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4
Q

Base - Texture of Solution

A

Slippery

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5
Q

Acid - Aqueous Property of Oxides

A

Non metallic oxides

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6
Q

Base - Aqueous Property of Oxides

A

Metallic oxides

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7
Q

Acid - Reaction with Phenolphthalein

A

Colourless

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8
Q

Base - Reaction with Phenolphthalein

A

Pink

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9
Q

Acid - Reaction with Litmus

A

Blue –> Red

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10
Q

Base - Reaction with Litmus

A

Red –> Blue

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11
Q

Acid - Reaction with Metals

A

Release H2 gas

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12
Q

Base - Reaction with Metals

A

No reaction

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13
Q

Acid - Reaction with CO3^2-

A

Produce CO2 (g)

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14
Q

Base - Reaction with CO3^2-

A

No Reaction

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15
Q

Acid - Reaction with NH4Cl

A

No Reaction

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16
Q

Base - Reaction with NH4Cl

A

Produce NH3 (g)

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17
Q

Acid - Reaction with Fatty Acids

A

No Reaction

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18
Q

Base - Reaction with Fatty Acids

A

Produce soaps

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19
Q

Acid - Neutralization Reactions

A

Neutralize bases

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20
Q

Base - Neutralization Reactions

A

Neutralize acids

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21
Q

What are the two main acid-base theories?

A
  • Arrhenius Theory
  • Bronsted-Lowry Theory
22
Q

What is the Arrhenius Theory?

A

Based on the ions produced when they dissociate in water

23
Q

Arrhenius Theory - Acids

A
  • Produce hydrogen ions (H+)
  • Ex: HBr –> H+ + Br-
24
Q

Arrhenius Theory - Bases

A
  • Produce hydroxide ions (OH-)
  • Ex: NaOH –> Na+ + OH-
25
Q

Arrhenius Theory - Limitations

A
  • Unable to explain role of H2O
  • Limited to H2O as the only solvent
  • Unable to explain basic behaviour of NH3
26
Q

What is the Bronsted-Lowry Theory?

A

It defines acids/bases regarding protons (H+)

27
Q

Bronsted-Lowry Theory - Acids

A
  • Proton (H+) donor
  • Produce H3O+ ions
  • Ex: HBr + H2O –> H3O+ + Br-
28
Q

Bronsted-Lowry Theory - Bases

A
  • Proton (H+) acceptors
  • Ex: NH3 + H2O –> NH4 + OH-
29
Q

Bronsted-Lowry Theory - Limitations

A

Amphiprotic nature of the theory

30
Q

What does amphiprotic mean?

A

Any chemical that can act as both an acid or a base

31
Q

Conjugate Acid

A

Forms when a base accepts a hydrogen ion (proton)

32
Q

Conjugate base

A

From when an acid loses a hydrogen ion (proton)

33
Q

What are conjugate acid/base pairs?

A
  • Same overall chemical structure, but different ionic charges
34
Q

What happens when weak acids ionize and dissociate in water?

A

They form a dynamic equilibrium

35
Q

Binary Acids

A
  • 2 elements
  • Hydrogen and a non-metal
  • Ex: HCl, HBr, H2S
36
Q

Oxygen Acids

A
  • 3 elements
  • Hydrogen, oxygen and a polyatomic ion
  • Ex: H2SO4, H2CO3
37
Q

Organic Acids

A
  • Have functional groups
  • Ex: acetic acid (vingear), CH3COOH
38
Q

Strong Acids

A
  • Ionize completely in water
  • Ka is very large
39
Q

Weak Acids

A
  • Ionize partially in water
  • In equilibrium
  • Smaller Ka values
40
Q

Position of the ionization equilibrium - strong acid

A
  • Far to the right
  • Favours products
41
Q

Position of the ionization equilibrium - weak acid

A
  • Far to the left
  • Favours reactants
42
Q

Eq concentration of H+ (aq) compared to the original concentration of HA - Strong Acid

A

[H+] = [HA]

43
Q

Eq concentration of H+ (aq) compared to the original concentration of HA - Weak Acid

A

[H+] < [HA]

44
Q

When the acid is stronger what happens to the conjugate base?

A

It’s weaker

45
Q

When the acid is weaker what happens to the conjugate base?

A

It’s stronger

46
Q

Weak bases

A
  • CO3^2-
  • HCO3-
  • NH3
  • All derivatives of ammonia
47
Q

Strong bases

A

All OH-

48
Q

Auto ionization of water

A
  • Water can behave as both an acid and a base
  • 2H2O(l) ↔ H3O+(aq) + OH-(aq)
49
Q

What does Kw represent?

A

The equilibrium constant for the auto ionzation of water

50
Q

The big 6 acids

A
  1. HClO4
  2. HNO3
  3. N2SO4
  4. HBr
  5. HCl
  6. HI

Chemistry - Chemical Systems and Equilibrium (12 decks)

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