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Chemistry IGCSE > Chapter 7 > Flashcards

Chapter 7 Flashcards

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1
Q

Indicators: universal indicator

A

Changes colour to match pH scale (depending on pH of solution)

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2
Q

Indicators: litmus indicator

A
  • red in acidic solutions
  • purple in neutral solutions
  • blue in alkaline solutions
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3
Q

Indicators: litmus paper

A
  • Red litmus paper -> turns blue in alkaline solutioms
  • Blue litmus paper -> turns red in acidic solutions
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4
Q

Indicators: methyl orange

A
  • Red in acidic solutions
  • Yellow in alkaline solutions
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5
Q

Indicators: thymolphthalein

A
  • Colourless in acidic soloutions
  • Blue in alkaline solutions
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6
Q

Acid

A

H+ donor/proton donor

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7
Q

Base

A

H+ receiver/ proton acceptor

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8
Q

Alkali

A

Base that is soluble in water

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9
Q

Neutralisation

A

Reaction between an acid and a base/alkali -> products are neutral

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10
Q

Aqueous solutions of acids (neutralisation)

A

Contain H+ ions -> this is because acids ionise (split up) in solution to produce a hydrogen ion, H+, and another ion
Eg: HCl -> H+ + Cl -

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11
Q

Aqueous solutions of alkalis (neutralisation)

A

Contain OH- ions -> this is because acids ionise (split up) in solution to produce a hydroxide ion, OH- and another ion
Eg: NaOH -> Na+ + OH-

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12
Q

Acid + base

A

Acid + base (metal oxide or hydroxides) -> salt (sulfates, nitrates or chlorides) + water

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13
Q

Acid + ammonia

A

Acid + ammonia -> ammonium salt

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14
Q

Acid + metal

A

Acid + metal -> salt + hydrogen

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15
Q

Acid + metal carbonate

A

Acid + metal carbonate -> salt + water + carbon dioxide

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16
Q

Base + ammonium salt

A

Base + ammonium salt -> salt + water + ammonia

17
Q

Types of oxides: acidic

A
  • react with bases
  • are non-metal oxides
    -> on right side of periodic table
    Eg: SO2 and CO2
18
Q

Types of oxides: basic

A
  • react with acids
  • are metal oxides
    -> on left side of periodic table
    Eg: CaO and CuO
19
Q

Types of oxides: amphoteric

A
  • reacts with bothe acids and bases to form salt and water
  • only zin oxide (ZnO) and aluminium oxide (Al2O3)
  • experiment: to prove amphoteric add ZnO to acid and base
    -> should dissolve in both
20
Q

Strong acids

A

Acid that is completely ionised (dissociated) in aqueous solution -> releasing lots of H+ ions

21
Q

Weak acid

A

Acid that is partially ionised (dissociated) in aqueous solution -> releasing fewer H+ ions

22
Q

Soluble or inssoluble salts: sodium, potassium and ammonium

A

Soluble: ALL
Insoluble: NONE

23
Q

Soluble or inssoluble salts: nitrates

A

Soluble: ALL
Insoluble: NONE

24
Q

Soluble or inssoluble salts: Ethanoates

A

Soluble: ALL
Insoluble: NONE

25
Q

Soluble or inssoluble salts: chlorides

A

Soluble: MOST ARE
Insoluble: SILVER AND LEAD (II)

26
Q

Soluble or inssoluble salts: sulphates

A

Soluble: MOST ARE
Insoluble: BARIUM, CALCIUM AND LEAD (II)

27
Q

Soluble or inssoluble salts: carbonates

A

Soluble: CARBONATES OF SODIUM, POTASSIUM AND AMMONIUM
Insoulble: MOST ARE

28
Q

Soluble or inssoluble salts: hydroxides

A

Soluble: HYDROXIDES OF SODIUM, POTASSIUM AND CALCIUM (calcium is slightly soluble)
Insoluble: MOST ARE

29
Q

Preperation of salts: soluble salt from acid and soluble base -> alkali

A

1) Titration using methyl orange to find end point of reaction
2) repeat titration without methyl orange
3) heat until point of crystallisation
4) leave to dry between filter paper

30
Q

Preperation of salts: soluble salt from acid and insoluble base

A

1) Heat the acid
2) Add an excess of insoluble base
3) Filtration to remove unreleased base
4) Heat until point of crystallisation
5) Leave to dry between filter paper

31
Q

Preperation of salts: Insoluble salt from two soluble salts

A

1) mix two solutions
2) filter to remove insoluble salt
3) wash to remove impurities
4) leave to dry on filter paper

32
Q

Preperation of salts: soluble salt from acid and soluble base/alkali -> recognising reactants

A

Sodium hydroxide
Potassium hydroxide
Ammonium hydroxide

33
Q

Preperation of salts: soluble salt from acid and soluble base/alkali: how is endpoint determined? -> how much base is needed to neutralise

A
  • Acids are aqueous
  • Soluble bases are aquaeous
  • Use titration to find point of neutralisation
34
Q

Preperation of salts: soluble salt from acid and soluble alkali/bass -> common example

A

Potassium hydroxide + hydrochloric acid -> potassium chloride + water

35
Q

Preperation of salts: soluble salt from acid and insoluble base: recognising reactants

A

Insoluble bases
Eg: metal oxides
-> copper oxide, calcium oxide OR copper carbonate

36
Q

Preperation of salts: soluble salt from acid and insoluble base: how is endpoint determined? -> how much base is needed to neutralise

A
  • Acids are aquaeous
  • Insoluble bases are solid
  • Add an excess of the solid -> add until no more solid dissolve in acid
37
Q

Preperation of salts: soluble salt from acid and insoluble base:common example

A

Sulfuric acid + copper oxide -> copper sulfate + water

38
Q

Preperation of salts: Insoluble salt from two soluble salts -> recognising reactants

A

NO MENTION OF AN ACID REACTANT
- All reactants are salts:
-> metal sulfate, metal nitrate, metal chloride, metal hydroxide, metal carbonate

39
Q

Preperation of salts: Insoluble salt from two soluble salts -> common example

A

Barium nitrate + sodium sulfate -> sodium nitrate +barium sulfate
- Insoluble substance -> salt wanted

Chemistry IGCSE (11 decks)

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