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A LEVEL CHEMISTRY > ACIDS, BASES AND SALTS 2B > Flashcards

ACIDS, BASES AND SALTS 2B Flashcards

1
Q

Definition of an acid

A

Proton donor - releases H+ ions when in aqueous solution

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2
Q

Definition of a strong and weak acid

A

Strong is fully dissociated in solution

Weak is partially dissociated in solution

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3
Q

What is the link between strength of acids and the concentration of H+ ions?

A

The weaker the acid is, the lower proportion of the acid is dissociated, and so there is a lower concentration of H+ ions in the solution.

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4
Q

How is a strong acid generally written?

A

HA(aq) -> H(aq)+ + A(aq)-

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5
Q

How is a weak acid generally written?

A

HA(aq) EQUILIBRIUM ARROWS H(aq)+ + A(aq)-

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6
Q

Definition of a base

A

Proton acceptor

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7
Q

Name the types of bases and how they are bases

A

Metal hydroxides - accepts H+ to become water
Metal oxides - accepts H+ to become OH- (soluble oxide)
- accepts 2H+ to become water
Ammonia/amino compounds - N forms a dative bond with H+ ion

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8
Q

How can water act as a base?

A

H+ +H2O -> H3O+ (hydronium ion)

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9
Q

How can water act as an acid?

A

H2O -> OH- + H+

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10
Q

Definition of an alkali

A

Soluble base that releases OH- ions in water

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11
Q

Definition of a salt

A

Ionic compounds formed when the H+ ions in acids are replaced by metal ions or ammonium ions

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12
Q

Acid + Metal hydroxide

A

Salt + Water

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13
Q

Acid + Metal oxide

A

Salt + Water

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14
Q

Acid + Metal carbonate

A

Salt + Water + Carbon dioxide

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15
Q

Acid + reactive metal

A

Salt + Hydrogen

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16
Q

Why do ionic compounds have high melting and boiling points?

A

A lot of energy is needed to break the strong electrostatic forces of attraction between oppositely charged ions.

17
Q

Why do ionic compounds conduct electricity when molten or in aqueous solution?

A

When molten, ions are free to move as mobile charge carriers.

18
Q

Why do ionic compounds dissolve in polar solvents?

A

Polar molecules break down the lattice structure and surround the ions in solution. If the compound has larger charges, they are less soluble.

19
Q

Why are ionic compounds hard crystalline substances?

A

Made up of ions that are strongly attracted to each other by electrostatic forces

20
Q

Soluble or insoluble - K

A

Soluble

21
Q

Soluble or insoluble - Na

A

Soluble

22
Q

Soluble or insoluble - NH4+

A

Soluble

23
Q

Soluble or insoluble - Halides

A

Soluble except when combined with Ag+,Pb2+,Hg+

24
Q

Soluble or insoluble - Nitrates

A

Soluble

25
Q

Soluble or insoluble - Sulfates

A

Soluble except when combined with Ag+,Pb2+,Ca2+,Sr2+,Ba2+

26
Q

Soluble or insoluble - Carbonates

A

Insoluble except when combined with Na, K, NH4+

27
Q

Soluble or insoluble - Oxides

A

Insoluble except when combined with Group 1 or NH4+

28
Q

Soluble or insoluble - Phosphates

A

Insoluble except when combined with Group 1 or NH4+

29
Q

Soluble or insoluble - Hydroxides

A

Insoluble except when combined with Group 1 or NH4+, Ca2+, Mg2+, Sr2+, Ba2+

30
Q

Soluble or insoluble - Sulfides

A

Insoluble except when combined with Group 1 or NH4+

31
Q

Soluble or insoluble - Chromates

A

Insoluble except when combined with Group 1 or NH4+, Ca2+, Mg2+

32
Q

Acid + Metal hydrogen carbonate

A

Salt + Water + Carbon dioxide

33
Q

Acid + Alkali

A

Salt + Water

34
Q

Test for halides (including in isolation)

A

Add silver nitrate to unknown substance
Cl ion = white precipitate
Br ion = cream precipitate
I ion = yellow precipitate
In isolation add dilute ammonia solution -> precipitate dissolves then it’s Cl ions
Add conc. ammonia solution -> dissolves then it’s Br ions
Doesn’t dissolve in either then it’s I ions

35
Q

What are the ions that don’t change in a reaction called?

A

Spectator ions

36
Q

What must ionic equations balance for?

A

Atoms and charge

37
Q

Test for sulfates

A

Add Barium chloride and if a white precipitate forms then it’s a sulfate

38
Q

Test for carbonates

A

Add dilute nitric acid and there should be effervescence.

To prove this is CO2, bubble it through limewater and it will turn cloudy

39
Q

Test for ammonium ions

A

Add sodium hydroxide solution and heat. Hold damp red litmus paper over it and it will turn blue if ammonium ions are present

A LEVEL CHEMISTRY (6 decks)

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