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Chemistry A level > Acids, Bases, and Salts > Flashcards

Acids, Bases, and Salts Flashcards

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1
Q

What’s Hydrochloric acids formula?

A

HCl

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2
Q

What’s sulphuric acids formula?

A

H2SO4

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3
Q

What’s Nitric acids formula?

A

HNO3

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4
Q

What’s Phosphoric acids formula?

A

H3PO4

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5
Q

What’s ethanoic acids formula?

A

CH3COOH

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6
Q

Definition of an acid?

A

Releases H+ ions in aqueous solution, it’s also a proton donor

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7
Q

What’s a strong acid?

A

An acid which fully dissociates in aqueous solution

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8
Q

What’s a weak acid?

A

An which partially dissociates in aqueous solution

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9
Q

Ethanoic acid is a weak acid, show it dissociating?

A

CH3COOH(aq) ⇌ CH3COO- (aq) + H+(aq)

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10
Q

How can water act as a weak acid?

A

H2O ⇌ OH- + H+

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11
Q

So generally what’s the difference in writing the dissociation of a weak acid, and a strong acid?

A

⇌

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12
Q

Base definition?

A

A compound which neutralises an acid to form a salt, (proton accepter)

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13
Q

Different types of bases?

A

Metal hydroxides, Metal Oxides, Ammonia (NH3)

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14
Q

Features of Sodium Hydroxide?

A

NaOH, Ionic, Metal Hydroxide

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15
Q

Features of Ammonia?

A

NH3, Covalent, Nitrogen Compound

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16
Q

Features of Potassium Oxide?

A

K20, ionic, Metal Oxide

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17
Q

Features of Calcium Hydroxide?

A

Ca(OH)2, ionic, Metal Hydroxide

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18
Q

Features of Copper (II) Oxide?

A

CuO, ionic, Metal Oxide

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19
Q

How can water act as a base?

A

When an acid dissociates, and the hydrogen ion is accepted by a water molecule, forming a hydronium ion H3O+

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20
Q

3 main alkalis?

A

Sodium Hydroxide, Potassium Hydroxide, aqueous ammonia

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21
Q

What is an alkali?

A

A soluble base, which releases OH- ions in water

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22
Q

What do you write to replace water when an alkali is dissociating, but the water doesn’t effect the products chemically?

A

Aqua

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23
Q

Formula for when ammonia dissociates in water?

A

NH3 + H2O = NH4+ + OH-

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24
Q

What is an alkali compared to a base?

A

A sub-set

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25
Q

What are salts?

A

Ionic compounds formed when the H+ ions in acids, are replaced by metal or ammonia ions (Charges must balance aka it’s neutral)

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26
Q

Charge of a silver ion?

A

Ag +

27
Q

Charge of a Copper (II) ion?

A

Cu 2+

28
Q

Charge of an ammonium ion?

A

NH4 +

29
Q

Charge of an Iron (II) ion?

A

Fe 2+

30
Q

Charge of an Iron (III) ion?

A

Fe 3+

31
Q

Charge of a zinc ion?

A

Zn 2+

32
Q

Charge of a lead (II) ion?

A

Pb 2+

33
Q

Carbonate ion and it’s acid?

A

Co3 2-, H2CO3

34
Q

Sulfate ion and it’s acid?

A

SO4 2-, H2SO4

35
Q

Nitrate ion and it’s acid?

A

NO3 -, HNO3

36
Q

Phosphate ion and it’s acid?

A

PO4 3-, H3PO4

37
Q

Hydrogen Carbonate ion and it’s acid?

A

HCO3 -, H2CO3

38
Q

Hydroxide ion and it’s acid?

A

OH-, H2O

39
Q

Products of an acid and a metal hydroxide?

A

Salt + water

40
Q

Products of an acid and a metal oxide?

A

Salt + Water

41
Q

Products of an acid and a metal carbonate?

A

Salt+ Carbon Dioxide + Water

42
Q

Products of an acid and a reactive metal?

A

Salt + Hydrogen

43
Q

What do ionic substances form if they dissolve in water?

A

Hydrated ions

44
Q

Why are ionic compounds hard crystalline substances?

A

Ionic compounds are made up of ions which are strongly attracted to each other by electrostatic forces

45
Q

Why do ionic compounds have high melting points?

A

The electrostatic forces holding the oppositely charged ions take a lot of energy to break

46
Q

Why are ionic compounds soluble in water?

A

Polar water molecules area attracted to the charged ions, and surround them pulling them away from the structure, meaning they have dissolved

47
Q

What does soluble mean?

A

Dissolves in solute, so in formula it will become aqueous

48
Q

What are the products of an acid and alkali?

A

Salt + Water

49
Q

What are the products of an acid and a metal hydrogen carbonate?

A

Carbon Dioxide + Salt + Water

50
Q

How to test for Halides?

A

Add silver Nitrate solution

51
Q

What will happen to a Chloride ion when reacted with silver Nitrate solution?

A

Silver Chloride formed, which is a white precipitate, it will be soluble in dilute and concentrated ammonia solution

52
Q

What will happen to a Bromide ion when reacted with silver Nitrate solution?

A

Silver Bromide formed, which is a Cream precipitate, it wont be soluble in dilute ammonia solution, but will be soluble in concentrated ammonia solution

53
Q

What will happen to a iodide ion when reacted with silver Nitrate solution?

A

Silver Bromide formed, which is a Yellow precipitate, it wont be soluble in dilute and concentrated ammonia solution

54
Q

What happens to silver halides when they are exposed to light?

A

They decompose, to release silver metal

55
Q

What useful about silver halides decomposing when exposed to light?

A

Used in photography, photographic plate coated in silver halides, depending how much light they were exposed to, the more or less they would decompose, creating an image

56
Q

How to write an ionic equation?

A

Write the balanced equation with state symbols
Anything which is aqueous, split up into it’s ions
Cancel out anything which stays aqueous on both sides (spectator ions)
Rewrite ionic equation

57
Q

Test for sulfate ions?

A

Product needs to be an insoluble sulfate

Add Barium Chloride or Barium Nitrate solution, if a sulfate is present a white precipitate will be formed

58
Q

Test for carbonate ions?

A

Add dilute nitric acid to test substance, if effervescence or bubbles are seen it could be CO2, then bubble the gas through limewater, if it turns cloudy then it is CO2

59
Q

Test for ammonium ions?

A

Heat, if present ammonia will be smelt, and damp red litmus paper will turn blue

60
Q

Why does ammonia turn damp red litmus paper blue?

A

Because it is an alkali

61
Q

Formula for ammonia?

A

NH3

62
Q

Formula for ammonium?

A

NH4 +

63
Q

Order in which the ions should be tested for?

A

Carbonate
Sulfate
Halides
Ammonium

Chemistry A level (16 decks)

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