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y chemistry paper two > required practicals > Flashcards

required practicals Flashcards

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1
Q

Describe a practical to show the effect of the concentration of a reactant on the rate of the reaction. (hint: sulfur)

A

effect of concentration on rate (sulfur):

1) 10cm3 of sodium thiosulfate into conical flask
2) place this onto a printed bold black cross
3) add 10cm3 of hydrochloric acid, swirl and start stopwatch
4) look through top of conical flask, swirl and stop when you can no longer see the cross (sodium, a product, causes cloudiness)
5) repeat with lower concentrations of sodium thiosulfate
- may not be repeatable as different eyesights

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2
Q

Describe a practical to show the effect of the concentration of a reactant on the rate of the reaction. (hint: HCl)

A

effect of concentration on rate (HCl):

1) 50cm3 of HCl into conical flask
2) attach a bung and delivery tube
3) place the delivery tube in water and an upturned measuring cylinder filled with water over the delivery tube
4) add 3cm strip of Mg to HCl and start stopwatch
5) H will be trapped in the measuring cylinder, measure every 10s until no more produced
6) repeat with different concentrations of HCl

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3
Q

Describe a practical to produce a chromatagram.

A

chromatography:

1) draw a pencil line on chromatography paper about 2cm above the bottom (pencil as not soluble)
2) mark 5 pencil spots at equal spaces (at least 1cm) across the line
3) use a capillary tube (thin glass tube) to put a small spot of each substance on the spots (must be relatively small to prevent overlap)
4) pour water into a beaker at a depth of 1cm (this is the solvent)
5) attach the paper to a glass rod using tape and lower the paper into the beaker; the bottom should just dip into the water
- not above pencil line as will wash substance off of line
- sides of paper must not touch sides of beaker as it will interfere with how the water moves
- put a lid on the beaker to reduce evaporation
6) water moves up paper and colours carried up; DO NOT MOVE THE BEAKER
7) remove paper when water is about 3/4 up paper
- use pencil to mark where water reached
8) hang paper up to dry

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4
Q

Describe the test for hydrogen gas.

A

test for hydrogen gas:

  • remove bung and insert burning splint
  • hydrogen gas burns rapidly and produces pop sound
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5
Q

Describe the test for oxygen gas.

A

test for oxygen gas:

- insert glowing splint, it will relight

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6
Q

Describe the test for carbon dioxide gas.

A

test for carbon dioxide gas:

  • use an aqueous solution of calcium hydroxide (limewater)
  • draw some gas into plastic pipette
  • bubble the gas through the limewater and repeat
  • if carbon dioxide, it will go cloudy or milky
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7
Q

Describe the test for chlorine gas.

A

test for chlorine gas:

  • insert damp litmus paper
  • it will bleach the litmus paper and turn it white
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8
Q

Describe the test for lithium.

A

test for lithium:

  • place small amount of lithium onto loop on a wire mounted on a handle and place in blue Bunsen flame
  • flame will turn crimson
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9
Q

Describe the test for sodium.

A

test for sodium:

  • place small amount of sodium onto loop on a wire mounted on a handle and place in blue Bunsen flame
  • flame will turn yellow
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10
Q

Describe the test for potassium.

A

test for potassium:

  • place small amount of potassium onto loop on a wire mounted on a handle and place in blue Bunsen flame
  • flame will turn lilac
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11
Q

Describe the test for calcium.

A

test for calcium:

  • place small amount of calcium onto loop on a wire mounted on a handle and place in blue Bunsen flame
  • flame will turn orange-red
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12
Q

Describe the test for copper.

A

test for copper:

  • place small amount of copper onto loop on a wire mounted on a handle and place in blue Bunsen flame
  • flame will turn green
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13
Q

Describe the test for carbonates.

A

test for carbonates:

  • add dilute acid
  • the acid will react with the carbonate to form CO2, and will see fizzing (effervescence), but not definitely CO2
  • bubble gas through limewater, if cloudy, it is CO2, so must have started with a carbonate
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14
Q

Describe the test for chloride ions.

A

test for chloride ions:

  • add dilute nitric acid and dilute silver nitrate
  • halide ions produce a precipitate of the silver halide
  • chloride ions produce a white precipitate of silver chloride
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15
Q

Describe the test for bromide ions.

A

test for bromide ions:

  • add dilute nitric acid and dilute silver nitrate
  • halide ions produce a precipitate of the silver halide
  • bromide ions produce a cream precipitate of silver bromide
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16
Q

Describe the test for iodide ions.

A

test for iodide ions:

  • add dilute nitric acid and dilute silver nitrate
  • halide ions produce a precipitate of the silver halide
  • iodide ions produce a yellow precipitate of silver iodide
17
Q

Describe the test for sulfates.

A

test for sulfates:

  • add dilute HCl and barium chloride
  • if sulfate ions, there will be a white precipitate
18
Q

Describe a practical to establish whether the water sample is pure.

A

pure water sample:

1) check pH by placing a small amount of water on universal indicator paper, green if pH 7
- if not green, contains dissolved acid or alkali, so impure
- if green, maybe pure… test for dissolved solids
2) use a balance to weigh and record evaporating basin
3) fill evaporating basin with water sample and place on tripod
4) use Bunsen to gently heat until evaporated
5) allow evaporating basin to cool and weigh again
- if contained dissolved solids, mass will have increased
- if mass didn’t increase, could be pure but may have contained dissolved gases

19
Q

Describe a practical to purify water by distillation.

A

purify water:

1) Bunsen under conical flask with water sample, with bung connected to delivery tube to test tube in water and ice bath
2) gently heat water so boils gently and evaporates
3) water vapour travels along delivery tube and condenses in test tube (this is distilled, pure water, pH 7)

20
Q

Describe a practical to discover the conditions needed for iron to rust.

A

rusting iron conditions:
1) one test tube with iron nail in distilled water, open to air (water and air present), nail will be covered in rust

2) iron nail in distilled, boiled water (removes dissolved air) and oil on top (prevents air from dissolving in the water) (no air, just water present), no rust
3) iron nail in anhydrous calcium chloride powder (removes water from air) and rubber bung (prevents moist air from entering) (no water, just air present), no rust
- shows air and water must be present for rusting

21
Q

Describe the test for aluminium ions in a solution.

A

test for aluminium ions:

  • add sodium hydroxide, forms white precipitate
  • add excess sodium hydroxide, and the aluminium precipitate will redissolve

aluminium nitrate + sodium hydroxide –> sodium nitrate + aluminium hydroxide
Al(NO3)2 + 3NaOH –> 3NaNO3 + Al(OH)3

22
Q

Describe the test for calcium ions in a solution.

A

test for calcium ions:

  • add sodium hydroxide, forms white precipitate
  • flame test the solution, will turn orange-red

calcium nitrate + sodium hydroxide –> sodium nitrate + calcium hydroxide
Ca(NO3)2 + 2NaOH –> 2NaNO3 + Ca(OH)2

23
Q

Describe the test for magnesium ions in a solution.

A

test for magnesium ions:

  • add sodium hydroxide, forms white precipitate
  • add excess sodium hydroxide, and the magnesium precipitate won’t redissolve

magnesium nitrate + sodium hydroxide –> sodium nitrate + magnesium hydroxide
Mg(NO3)2 + 2NaOH –> 2NaNO3 + Mg(OH)2

24
Q

Describe the test for copper(II) ions.

A

test for copper(II) ions:

  • add sodium hydroxide
  • forms a blue precipitate

copper(II) nitrate + sodium hydroxide –> sodium nitrate + copper(II) hydroxide
Cu(NO3)2 + 2NaOH –> 2NaNO3 + Cu(OH)2

25
Q

Describe the test for iron(II) ions.

A

test for iron(II) ions:

  • add sodium hydroxide
  • forms a green precipitate

iron(II) nitrate + sodium hydroxide –> sodium nitrate + iron(II) hydroxide
Fe(NO3)2 + 2NaOH –> 2NaNO3 + Fe(OH)2

26
Q

Describe the test for iron(III) ions.

A

test for iron(III) ions:

  • add sodium hydroxide
  • forms a brown precipitate

iron(III) nitrate + sodium hydroxide –> sodium nitrate + iron(III) hydroxide
Fe(NO3)2 + 3NaOH –> 3NaNO3 + Fe(OH)3

y chemistry paper two (6 decks)

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