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GCSE Chem > Topic 3a > Flashcards

Topic 3a Flashcards

Done except for a few specpoints

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1
Q

3.1
What ion do acids produce an excess of when dissolved in water?

A

Hydrogen ions
H+

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2
Q

3.1
What ion do alkalis produce an excess of when dissolved in water?

A

Hydroxide ions
OH-

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3
Q

Define an ion

A

An atom that has lost or gained electrons

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4
Q

Define a poly-atomic ion

A

Groups of atoms held by covalent bonds lose/gain electrons

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5
Q

3.1
Explain why the pH of hydrogen bromide becomes acidic when dissolved in water?

A

H+ ions form making it acidic

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6
Q

3.2
a) A neutral solution has a pH of…?

b) Acidic solutions have a pH of…?

c) Alkali solutions have a pH of…?

A

a) 7

b)1-6

c) 8-14

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7
Q

What is an advantage to having internationally agreed hazard symbols?

A

Anyone can understand them and stay safe

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8
Q

What is the main advantage to using a pH probe?

A

Measurements are accurate

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9
Q

3.4
The most acidic rain recorded in Britain had a pH of 2. How much more acidic is this than normal rainwater with a pH of 5. [2 marks]

A

10 × 10 × 10 =

×1000 more H+ ions

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10
Q

3.5
Describe the relationship between the pH and the concentration of hydrogen ions

A

As the pH decreases by 1, the concentration of H+ ions increases by a factor of 10

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11
Q

3.5
Describe the relationship between the pH and the concentration of hydroxide ions

A

As the pH increases by 1, the concentration of OH- ions increases by a factor of 10

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12
Q

3.7
Explain the term dilute

A

Contains relatively small v of dissolved solute

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13
Q

3.7
Define the term concentrated

A

Contains relatively large amount of dissolved solute

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14
Q

3.8
What is a strong acid?

A

-Completely dissociates to form H+ ions in solution
-High concentration of H+ ions

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15
Q

3.8
What is a weak acid?

A

-Partially dissociates to form H+ ions in solution
-Low conc H+ ions

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16
Q

3.10
What are alkalis?

A

-Soluble bases
-pH greater than 7

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17
Q

3.9
What is a base?

A

Neutralise acids to form salt + water

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18
Q

I find an unmarked bottle and want to work out if the liquid inside is acidic or not. How could I do this?

A

Universal indicator
If it’s red/orange/yellow it’s an acid

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19
Q

Why are metal oxides bases?

A

They neutralise acids

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20
Q

3.11
State 4 reaction equations of aqueous solutions of acids that produce salts

A

Metal + Acid –> Salt + Hydrogen

Metal oxide + Acid –> Salt + Water

Metal hydroxide * + Acid –> Salt + Water

Metal carbonate + Acid –> Salt + Carbon dioxide + Water

Acid + Alkali –> Salt + Water

Typically alkalis *

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21
Q

3.11
What salt will hydrochloric acid form?

A

Chloride

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22
Q

3.11
Which salt will sulfuric acid form?

A

Sulfate

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23
Q

3.11
Which salt will nitric acid form?

A

Nitrate

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24
Q

3.11
Finish the equations:
a) Zinc oxide + Sulfuric acid –>

b) Sodium oxide + Hydrochloric acid—>

A

Zinc sulfate + Water

Sodium chloride + Water

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25
Q

3.11
What happens to the ions from acids and alkali during a neutralisation reaction?

A

H+ ion from acid combines with OH- ion from alkali to form water

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26
Q

Name 3 common acids

A

Hydrochloric acid - HCl
Sulfuric acid - H₂SO₄
Nitric acid - HNO₃

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27
Q

Name 3 common alkalis

A

Sodium hydroxide - NaOH
Potassium hydroxide - KOH
Calcium hydroxide - Ca(OH)₂

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28
Q

Name 3 polyatomic ions

A

Hydroxide - OH^-
Carbonate - CO₃²^-
Nitrate - NO₃^-

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29
Q

What is the ionic formula for sodium?

A

Na(+)

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30
Q

What is the ionic formula for lithium?

A

Li(+)

31
Q

What is the ionic formula for potassium?

A

K(+)

32
Q

What is the ionic formula for magnesium?

A

Mg(2+)

33
Q

What is the ionic formula for calcium?

A

Ca(2+)

34
Q

What is the ionic formula for aluminium?

A

Al(3+)

35
Q

What is the ionic formula for fluoride?

A

F(-)

36
Q

What is the ionic formula for chloride?

A

Cl(-)

37
Q

What is the ionic formula for bromide?

A

Br(-)

38
Q

What is the ionic formula for oxygen?

A

O(2-)

39
Q

What is the ionic formula for sulfide?

A

S(2-)

40
Q

What is the ionic formula for nitrate?

A

NO₃(-)

41
Q

What is the ionic formula for sulfate?

A

SO₄(2-)

42
Q

What is the ionic formula for carbonate?

A

CO₃(2-)

43
Q

What is an independent variable?

A

One you change

44
Q

What is a dependent variable?

A

One that you measure

45
Q

What is a control variable?

A

One that stays the same

46
Q

3.6
What are the independent, dependent and control variables in neutralisation?

A

Independent - calcium hydroxide m in solution

Dependent - pH of reaction mixture

Control
- v of HCl added each t
-Conc of HCl

47
Q

3.6
Neutralisation
How can you increase the accuracy of your results?

A

-Measure calcium hydroxide m w/ balance
-Measure pH w/ pH probe rather than estimate w/ universal indicator

48
Q

3.6
Neutralisation
Describe what happens to the pH of the solution as the mass of calcium hydroxide added increases?

A

pH increases (directly proportional)

49
Q

3.6
What is the ionic equation for neutralisation?

A

H+(aq) + OH-(aq) –> H₂O(l)

50
Q

3.6
Describe 3 risks that could take place in a neutralisation reaction and how they can be managed

A

-Calcium hydroxide = irritant (goggles)
-HCl = irritant (goggles)
-Solution spill (wipe)

51
Q

What is a salt?

A

Reaction between acid + base (in neutralisation reaction)

52
Q

3.12
Describe the chemical test for hydrogen

A

-Place lit splint into test tube
-Burns to produce squeaky pop

53
Q

3.12
Describe the chemical test for carbon dioxide

A

-Pass/bubble the gas through lime water
-Lime water turns milky/cloudy

54
Q

3.12
Describe the chemical test for chlorine gas

A

-Damp blue litmus paper
-Turns red
-Then bleached

55
Q

3.13
What is a neutralisation reaction?

A

Between acid & base

56
Q

3.14
Describe what happens in a neutralisation reaction

A

H^+ ions from acid react w/ OH^- ions from alkali to form water

57
Q

~3.17
Describe how to prepare an insoluble salt

A

-Mix soluble salts in water
-Filter -> remove precipitate
-Rinse precipitate w/ distilled water -> remove traces of solution
-Dry by heating in oven

58
Q

3.19
Recall the general solubility rules of common substances in water

A

SOLUBLE
-Sodium, potassium, ammonium carbonates, hydroxides and salts
-All nitrates
-Most chlorides
-Most sulfates

INSOLUBLE
-Most carbonates & hydroxides
-Silver & lead chloride
-Lead, barium & calcium sulfate

59
Q

3.19
Using the solubility rules identify whether each of these substance are soluble or insoluble
a) Sodium chloride
b) Silver chloride
c) Silver nitrate
d) Calcium carbonate

A

a) Soluble
b) Not soluble
c) Soluble
d) Not soluble

60
Q

3.20
What happens during a precipitation reaction?

A

Soluble substance in solution forms insoluble precipitate

61
Q

3.20
Name the precipitate formed when solutions of the following compounds are mixed together
a) Sodium hydroxide & barium chloride
b) Silver nitrate & potassium chloride

A

a) Sodium chloride (aq) + BARIUM HYDROXIDE (s)
b) SILVER CHLORIDE (s) + Potassium nitrate (aq)

(Note: precipitate is in capitals bc I put all the products & precipitate is insoluble one)

62
Q

~3.21
Describe how to prepare a soluble salt

A

-Add excess base to ensure all acid used up
-Heat mixture in water bath (speed reaction)
-Filter to ensure prepared salt = pure
-Heat -> crystallise salt solution
-Leave to slowly evaporate -> bigger crystals

63
Q

3.17
Explain how to prepare a pure dry sample of copper sulfate

A

-Fixed v dilute sulfuric acid
-Warm acid in water bath
-Small amounts of copper oxide to acid (stir)
-Copper oxide reacts -> dissolves
-Continue adding until powder = excess (no longer reacts)
-Filter mixture
-Transfer solution -> evaporating basin
-Heat (evaporating basin over beaker of water heated w/ Bb until crystals start to form)
-Pour solution in watch glass for copper sulfate crystals to form (for a few days)
-Pat dry

64
Q

3.18
Describe the process of titration

A

-Clean pipette w/ water, rinse w/ sodium hydroxide solution
-Clean burette w/ water, rinse w/ dilute HCl
-Use pipette to transfer 25cm^3 sodium hydroxide solution into conical flask
-Few drops of acid-base indicator
-Fill burette w/ dilute HCl & take reading
-Add HCl from burette to alkali in conical flask, swirling contents at all times
-Add acid drop-by-drop near end-point until colour changes
-Take final burette reading

65
Q

3.18
Suggest why universal indicator is not used in titration

A

-No sharp colour change
-Methyl orange/phenolphthalein used instead
-Bc have only 2 colour change

66
Q

3.18
Titration
Why should you clean the pipette and burette with water before carrying out titration?

A

Reduce contamination to not interfere with results

67
Q

3.18
Titration
What is the purpose of using a pipette to transfer the sodium hydroxide?

A

To accurately measure solution

68
Q

3.18
Titration
Why do we only add a few drops of acid-base indicator to the alkali solution in the conical flask?

A

-Indicator=slightly acidic
-If add too much, will interfere with results

69
Q

3.18
Titration
Why is a conical flask used to contain the alkali?

A

Allows swirling w/o spilling

70
Q

3.18
Titration
Why should you continuously swirl the contents?

A

-To mix thoroughly
-For reaction to occur

71
Q

3.18
Titration
Why is the acid added drop-by-drop near the end-point?

A

To not overshoot endpoint

72
Q

3.18
Titration
Why is a white tile used?

A

Enables indicator colour change to be seen more clearly

73
Q

Describe how to prepare a pure, dry salt from an acid and an alkali

A

-Acid + alkali -> salt + water
-Crystallise salt by heating to evaporate water
-Pat salt dry

GCSE Chem (13 decks)

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