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🥼🧪 > 3.4 chemistry > Flashcards

3.4 chemistry Flashcards

1
Q

pH < 7

A

acidic

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2
Q

pH = 7

A

neutral

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3
Q

pH > 7

A

alkaline

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4
Q

methyl orange: acidic, neutral and alkaline colours:

A

red, yellow and yellow

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5
Q

phenolphthalein: acidic, neutral and alkaline colours:

A

colourless, colourless and pink

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6
Q

red litmus paper: acidic, neutral and alkaline colours:

A

red, red and blue

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7
Q

blue litmus paper: acidic, neutral and alkaline colours:

A

red, blue and blue

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8
Q

what is an indicator

A

it is a substance that changes colour to tell you about the pH of a solutuon

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9
Q

the universal indicator is special because

A

the range of colours tells you the approximate pH

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10
Q

effervescence is

A

the escape of gas from an aqueous solution (salt CARBONATE)

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11
Q

nitrogen % in air

A

N2 = 78%

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12
Q

oxygen % in air

A

O2 = 21%

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13
Q

argon % in air

A

Ar = 0.96%

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14
Q

carbon dioxide % in air

A

CO2 = 0.04%

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15
Q

what is element combustion

A

it’s when an element reacts with oxygen to produce an oxide

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16
Q

sulphur + oxygen -> sulphur dioxide

A

S(s) + O2(g) -> SO2(g) v

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17
Q

sulphur dioxide observation is

A

a blue flame

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18
Q

metal ion of iron(II)

A

Fe2+ ^

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19
Q

metal ion of silver

A

Ag+ ^

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20
Q

metal ion of iron(III)

A

Fe3+ ^

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21
Q

metal ion of zinc

A

Zn2+ ^

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22
Q

metal ion of copper

A

Cu2+ ^

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23
Q

metal ion of lead

A

Pb2+ ^

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24
Q

acid definition

A

H+ donor ^

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25
Q

base definition

A

H+ acceptor ^

26
Q

alkali definition

A

OH- donor ^

27
Q

sodium hydroxide + sulphuric acid ->

A

sodium sulphate + water

28
Q

what is titration

A

it is a method for making a soluble salt from a soluble base and an acid

29
Q

titration method is used to make salts that contain which ions

A

sodium Na+
potassium K+
ammonium NH4+

30
Q

why do you use titration method when making salts that contain potassium, sodium or ammonium ions?

A

because their bases are all soluble so you wouldn’t be able to filter out the excess if you use the insoluble base method

31
Q

what are 3 usual acids

A

hydrochloric acid • HCl
sulphuric acid • H2SO4
nitric acid • HNO3

32
Q

what are 3 usual alkalis

A

sodium hydroxide • NaOH
potassium hydroxide • KOH
ammonium hydroxide • NH4OH

33
Q

insoluble base method

A
  1. HEAT sulphuric acid in a beaker
  2. whilst stirring with a glass rod ADD copper oxide until NO MORE dissolves
  3. let the mixture COOL before FILTERING to remove the excess base (insoluble)
  4. let the salt solution COOL DOWN
  5. HEAT the salt solution until some crystals start to form
  6. allow the solution to COOL in an evaporating basin
  7. FILTER out the crystals
  8. DRY the crystals by dabbing them with filter paper
34
Q

crystallisation method

A
  1. HEAT the salt solution until some crystals start to form
  2. allow the solution to COOL in an evaporating basin
  3. FILTER out the crystals
  4. DRY the crystals by dabbing them with filter paper
35
Q

short insoluble base words

A

HEAT
ADD
NO MORE
COOL
FILTER
COOL DOWN

HEAT
COOL
FILTER
DRY

36
Q

short filtering words

A

HEAT
COOL
FILTER
DRY

37
Q

acid + base (oxide)

A

insoluble base method

38
Q

acid + alkali (hydroxide)

39
Q

titration method

A
  1. place a known volume of *acid (hydrochloric acid)
  2. add a few drops of indicator
  3. using a burette start adding *alkali solution (potassium hydroxide) until the colour starts to change
  4. stop adding the alkali and measure how much has been added to change the colour
  5. repeat the titration but without using the indicator and using a burette to add exactly the right volume to the acid for neutralisation

crystallisation!!

40
Q

ammonium ion

41
Q

hydroxide ion

42
Q

nitrate ion

43
Q

sulphate ion

44
Q

carbonate ion

45
Q

hydrocarbonte ion

46
Q

nitric acid

A

Acid formula: HNO3
Ion formula: NO3-
Ion name: Nitrate

47
Q

sulphuric acid

A

Acid formula: H2SO4
Ion formula: SO42-
Ion name: Sulphate

48
Q

phosphoric acid

A

Acid formula: H3PO4
Ion formula: PO43-
Ion name: Phosphate

49
Q

carbonic acid

A

Acid formula: H2CO3
Ion formula: CO32-
Ion name: Carbonate

50
Q

knowing bases

A

have O or CO
(oxides or carbonates)

51
Q

knowing salts

A

SO4, CL, NO3, PO4, ethanoates + citrates
(common acids)

52
Q

knowing alkalis

A

OH
(hydroxide)

53
Q

knowing acids

A

H2SO4 (sulphuric)
HCL (hydrochloric)
HNO3 (nitric)
H3PO4 (phosphoric)
CH3COOOH (ethanoic)

54
Q

what is the formula of strontium chloride

55
Q

what is the formula for potassium nitride

56
Q

what is the formula for copper (II) oxide

57
Q

what is the formula for silver (I) chloride

58
Q

what’s the formula for chromium (III) oxide

59
Q

list the properties of ionic compounds and list the reasons for those properties

A

• they have high m + b points
• strong electrostatic forces
• a giant lattice structure
• forces act in all directions
• require a lot of energy to break
________________________________________

• they are soluble in polar substances
(like water)
• poor conductors when solid
(ions in fixed position)
• conduct electricity in liquid
(ions are free to move)

60
Q

% of oxygen in the atmosphere

A

burning phosphorus in an evaporating basin in a bell jar which is immersed in a trough of water

61
Q

what are the following four acids:
• H2So4
• HNO3
• HCl
• H3PO4

A

sulphuric acid
nitric acid
hydrochloric acid
phosphoric acid

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