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Chemistry > Acids And Bases - Lecture 15 > Flashcards

Acids And Bases - Lecture 15 Flashcards

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1
Q

What is an Arrhenius acid?

A

Substances that contain hydrogen and dissociates in water to form a hydrogen ion

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2
Q

What is an Arrhenius base?

A

Substances that contain the hydroxyl group (OH) and dissociates in water to form a hydroxide ion and a cation

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3
Q

What does an Acid produce according to the theory of Arrhenius in water

A

H+ ion (proton)

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4
Q

What does a base produce according to the theory of Arrhenius in Water?

A

OH- ion (hydroxide ion)

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5
Q

What is a strong acid according to Arrhenius?

A

Completely dissociates/fully ionised in solution and produces a lot of Hydrogen ions (H+)

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6
Q

What is a weak acid according to Arrhenius?

A

Is one that is only partially ionised/slightly dissociates in water and produces only a few H+ Ions (hydrogen ions)

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7
Q

Examples of strong acids according to Arrhenius?

A

Hydrochloric acid , Sulphuric acid, hydrobromic acid, hydroiodic (hydriodic) acid, nitric acid and perchloric acid

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8
Q

Examples of weak acids according to Arrhenius

A

Hydrofluoric acid, hydrosulfuric acid, hydrocyanic acid, acetic acid (ethanoic acid)

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9
Q

Monoprotic Acids

A

Acids that produce only one proton (H+) when dissolved in water

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10
Q

Polyprotic Acids

A

Acids that produce more than one H+ ion in water

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11
Q

Strong base according to Arrhenius

A

Strong electrolyte, which is completely ionised/completely dissociates in water (aqueous solution) to produce hydroxide ions (OH-)

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12
Q

Weak base according to Arrhenius

A

Only partially ionise/slightly dissociate in water to produce OH- ions (hydroxide ions)

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13
Q

Acid + Base =

A

Salt + Water

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14
Q

Base that dissolves in Water is called an

A

Alkali

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15
Q

Acid + Metal =

A

Salt + Hydrogen

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16
Q

Acids + Metal Carbonate =

A

Salt + Water and CO2 gas given off

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17
Q

Acids and Bases are

A

Electrolytes

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18
Q

Neutralisation

A

Reaction between an acid and a base to form a salt and water

19
Q

Why does Neutralisation Occur?

A

Hydrogen ions (H+) and hydroxide ions (OH-) react to produce water

20
Q

State 3 limitations of the Arrhenius theory of acids and bases

A
  1. Limited to acid-base reactions that place in water
  2. Restricts acids to hydrogen containing species and bases to hydroxide containing species
  3. Does not explain how certain substances can be amphoteric
21
Q

Amphoteric

A

Substance that can act as both an acid and a base

22
Q

Bronsted Lowry acid

A

Proton donor (H+)

23
Q

Bronsted Lowry Base

A

Proton (H+) acceptor (must contain lone pair of electrons)

24
Q

Conjugate pair

A

A pair of substances, an acid and a base, that differ by one H+

25
Q

Conjugate Acid

A

Base + Hydrogen ion (H+)

26
Q

Conjugate Base

A

Acid - Hydrogen ion (H+)

27
Q

According to BL theory, acids may be

A

Cations, neutral molecules or anions

28
Q

According to BL theory, bases may be

A

Anions or neutral molecules

29
Q

Is water an amphoteric substance

A

Yes

30
Q

Protophilic solvents

A

Act as proton acceptors (bases)

31
Q

Protogenic solvent

A

Proton donors (acids)

32
Q

Amphiprotic Solvents

A

Act as an acid or base (water, alcohol)

33
Q

Aprotic Solvents

A

Solvents which will neither donate nor accept protons
Eg.// benzene, carbon tetrachloride

34
Q

Lewis Acid

A

Electron pair acceptor

35
Q

Lewis Base

A

Electron pair donor

36
Q

Acid according to Lewis

A

Substance that can accept a pair of electrons from another atom to form a new bond

37
Q

Base according to Lewis

A

Substances that can donate an electron pair to another atom to form a new bond

38
Q

Lewis definition includes

A

Metal ions and other electron pairs as acids

39
Q

Lewis acid …..

A

Has an empty atomic orbital of low energy that can accommodate a pair of electrons

40
Q

The process of neutralisation of a Lewis Base forms

A

Coordinate Covalent bond between an acid and base

41
Q

The product of Lewis Acid-Base reaction is referred to as

A

Adduct

42
Q

Example of Lewis acid-base adducts

A

Complex ions

43
Q

Advantages of Lewis Theory

A
  1. Expands acid base reactions to include ,any substances without H in the formula
  2. Used to explain the effect of compounds which act as an acid in nonaqueous organic solvents
44
Q

Limitation of Lewis Theory

A
  1. Includes all the coordination reactions and coordination compounds which may not always be true
  2. Cannot explain the behaviour of well known protonic acids which do not form coordination bonds with bases
  3. Relative strengths of acids and bases cannot be explained by this theory

Chemistry (4 decks)

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