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new science > C12 experimental techniques and chemical analysis > Flashcards

C12 experimental techniques and chemical analysis Flashcards

1
Q

apparatus used to measure time

A

stop-watch

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2
Q

apparatus used to measure temperature

A

thermometer

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3
Q

apparatus used to measure mass

A

mass balance

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4
Q

apparatus used to measure volume

A
  • burette
  • volumetric pipette
  • measuring cylinder
  • gas syringe
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5
Q

define solvent

A

substance that dissolves a solute

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6
Q

define solute

A

substance that is dissolved in a solvent

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7
Q

define solution

A

mixture of one or more solutes dissolved in a solvent

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8
Q

define saturated solution

A
  • contain max concentration of solute dissolved in solvent
  • at specified temperature
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9
Q

define residue

A

solid substance that remains after
- evaporation
- distillation
- filtration
- any similar process

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10
Q

define filtrate

A

liquid or solution that has passed through a filter

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11
Q

what apparatus is used in an acid-base titration

A
  • burette
  • volumetric pipette
  • suitable indicator
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12
Q

how is the end-point of a titration identified

A

indicator

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13
Q

what is the word for a volume within +-0.10cm3

A

concordant

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14
Q

use of paper chromatography

A
  • separate mixtures of soluble coloured substances
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15
Q

describe how paper chromatography is carried out

A
  1. samples of solutes placed on reference line
  2. samples placed in beaker containing solvent up to reference line
  3. solvent moves up filter paper, carrying solute with
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16
Q

what is equation for Rf

A
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17
Q

describe and explain separation and purification by a suitable solvent

A
  • mixtures of solid substances separation using solvents
  • create suspension that can be filtered
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18
Q

describe and explain separation and purification by filtration

A
  • separate insoluble solid from liquid within suspension
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19
Q

describe and explain separation and purification by crystallisation

A
  • allow pure crystals to be obtained from solution as it cools
  • works best when large difference between solubilities at diff temp
  • as temp decreases, less space for solid particles, pushed out and grad grow as crystal
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20
Q

describe and explain separation and purification by simple distillation

A
  • diff substances have varying fixed points
  • lower bp will evaporate first
  • bp temp diff at least 50degrees
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21
Q

describe and explain separation and purification by fractional distillation

A
  • separate mixture of liquids w diff bp
22
Q

apparatus used in fractional distillation

A
  • fractionating column
  • thermometer
  • condenser
23
Q

how to assess purity

A
  • compare fixed points
24
Q

how to identify carbonate

A
  • react with dilute acid
  • effervescence
  • test for carbon dioxide gas
25
Q

how to identify chloride

A
  • acidify with dilute nitric acid
  • add aqueous silver nitrate
  • white ppt, turn purple in sunlight
26
Q

how to identify bromide

A
  • acidify with dilute nitric acid
  • add aqueous silver nitrate
  • cream ppt
27
Q

how to identify iodide

A
  • acidify with dilute nitric acid
  • add aqueous silver nitrate
  • yellow ppt
28
Q

how to identify nitrate

A
  • reduction with aluminium foil and aqueous sodium hydroxide
  • test for ammonia gas (damp litmus paper blue)
29
Q

how to identify sulfate

A
  • acidify with dilute nitric acid
  • add aqueous barium nitrate
  • white ppt
30
Q

describe test to identify ammonium

A
  • add aqueous sodium hydroxide
  • ammonia gas produced on heating (red litmus turns blue)
31
Q

describe test to identify calcium ion

A

add aqueous sodium hydroxide
- white ppt, insolube in excess

add aqueous ammonia
- no ppt, or very slightly white ppt

32
Q

describe test to identify copper(II) ion

A

add aqueous sodium hydroxide
- light blue ppt, insolube in excess

add aqueous ammonia
- light blue ppt, soluble in excess
- royal blue solution

33
Q

describe test to identify iron(II) ion

A

add aqueous sodium hydroxide
- green ppt, insoluble in excess

add aqueous ammonia
- green ppt, insoluble in excess

34
Q

describe test to identify iron(III) ion

A

add aqueous sodium hydroxide
- red/brown ppt, insoluble in excess

add aqueous ammonia
- red-brown ppt, insoluble in excess

35
Q

describe test to identify zinc ion

A

add aqueous sodium hydroxide
- white ppt, soluble in excess (colourless solution)

add aqueous ammonia
- white ppt, soluble in excess (colourless solution)

36
Q

ionic equation for test for calcium ions using NaOH

A
37
Q

ionic equation for test for copper(II) ions

A
38
Q

ionic equation for test for iron(II) ions

A
39
Q

ionic equation for test for iron(III) ions

A
40
Q

ionic equation for test for zinc ions

A
41
Q

describe test to identify ammonia

A
  • place damp red litmus paper in gas
  • turns blue
42
Q

describe test to identify carbon dioxide

A
  • bubble through limewater
  • turns milky
43
Q

describe test to identify chlorine gas

A
  • place damp litmus paper in gas
  • bleaches white
44
Q

describe test to identify hydrogen gas

A
  • place lighted splint in gas
  • ignites gas with a “pop” sound
45
Q

describe test to identify oxygen gas

A
  • place glowing splint in gas
  • relights
46
Q

why does the test tube need to be inverted over the flask when testing for hydrogen

A

hydrogen is less dense than air

47
Q

describe how to carry out a flame test

A
  • nichrome wire dipped in concentrated HCl (remove impurities)
  • then into salt wanting to test
  • wire held at outer edge of blue portion of flame, colour observed
48
Q

flame colour of lithium ion

A

red

49
Q

flame colour of sodium ion

A

yellow

50
Q

flame colour of potassium ion

A

lilac

51
Q

flame colour of copper(II) ion

A

blue-green

52
Q
A

new science (37 decks)

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